Notes to a video lecture on http://www.unizor.com
Strong Nuclear Force
Physical concept of a field assumes that there is a characteristic usually called a charge that participates in the creation of a field or its interaction with objects, manifested as a force.
Electricity has two types of charges that we call positive, carried by protons, and negative, carried by electrons.
Strictly speaking, these are just names, they do not imply that electric charges are positive or negative real numbers, but we can measure them using some clever devices and measuring units, resulting in positive or negative numbers, and they act as if we can add them together using the rules of arithmetic.
In particular, equal in magnitude positive and negative charges neutralize each other. For example, an atom of hydrogen has one proton (positively charged) and one electron (negatively charged) that neutralize each other and form an electrically neutral atom.
In quantum field theory the electric field activity is manifested itself in exchange of photons - particles that carry field energy.
Gravity has only one type of charge that we call mass and it's always present, wherever we have a matter. We can measure it using some devices and measuring units, and these charges can be dealt with using their positive numerical values. There is no opposite charge to neutralize gravity.
There is a theory (not yet decisively supported by experiments) that gravitational field's activity is manifested itself in exchange of gravitons - particles that carry gravitational field energy.
In both above cases, electric and gravitation fields, the quantum theory tells that the field interaction is an exchange of particles specific for this field.
Let's consider the strong nuclear forces now.
As we suggested in the previous lecture, following the Standard Model, protons and neutrons are comprised of three quarks each:
+1p = +2/3u + +2/3u + −1/3d
0n = +2/3u + −1/3d + −1/3d
where
p is a proton,
n is a neutron,
u is an UP quark,
d is a DOWN quark and
preceding numbers are the electric charges of corresponding particles.
Earlier in this course we mentioned the existence of strong nuclear forces that hold the nucleus together.
These forces hold triplets of quarks together to form a nucleon (a proton or a neutron), overcoming repelling electric forces between similarly charged quarks (two +2/3u quarks or two −1/3d quarks).
Strong nuclear forces are much stronger than electric forces and prevent protons from separating because of their mutually repelling positive electric charge.
What is the nature of these strong nuclear forces?
As in a case of electric or gravitational fields, there are charges that create the strong nuclear force field and there are particles that carry the energy of strong nuclear forces.
The charges that create a strong force field and interact by exerting the force are called color charges. Below is an explanation of the reasons for calling them using colors.
The particles that carry energy of strong nuclear forces are called gluons because quarks (material particles) are "glued" together into a proton or a neutron by exchanging gluons.
So, gluons are radiation type particles, carriers of strong nuclear forces analogously to how photons carry the force of electromagnetic field.
Color Charge
Strong nuclear forces are manifestations of a force field inside a nucleus that maintains the nucleus integrity. As with other fields, there is a charge that produces it and participates in its interaction.
While electric charges involved in electric forces are of two types (positive and negative) and gravitational charges are of only one type (mass), charges involved in strong nuclear field are of three different types.
Obviously, these three types of strong nuclear field charges have to be named. The types of charges for strong nuclear forces are called color charges. It has nothing to do with colors of visible light, it's just a name used to characterize and differentiate the types of charges participating in the interactions of strong nuclear forces.
According to Standard Model, there are three different types of color charges (or simply colors) participating in strong force field called:
red (R),
green (G) and
blue (B).
Again, these are just the names to differentiate the types of charges, totally unrelated to visible light and its colors.
In the world of electric fields a single charged particle (negatively charged electron or positively charged proton) prefers to find an oppositely charged particle to combine and to neutralize the charge, attaining electric neutrality.
For example, a proton and an electron can combine to form an electrically neutral atom of hydrogen.
Similarly, in the world of strong forces quarks, charged with any one of the main colors, look for stability in terms of combining their type of charge with other quarks of other charges to attain stability. This stability comes when all three types of quarks are together to form a stable particle, like a proton or a neutron.
The color analogy helps in this case because a combination of three lights of three main colors, red, green and blue, produces the white (colorless) light.
R + G + B = 0
In real numbers the opposite number to number X is the number −X that, combined with X, results in zero.
Similarly, in colors the opposite light color (we can call it anti-color) is the one that, combined with original, produces colorless (that is, white) light.
Therefore, the anti-colors are
anti-red R=G+B,
anti-green G=R+B,
anti-blue B=R+G.
These three anti-colors are the colors of anti-charges. Thus, an anti-proton is comprised from three anti-quarks, two anti-up quarks and one anti-down quark. Each of these quarks has a different anti-color, so all three anti-colors are present in the anti-proton particle.
While the term "color" applied to this physical characteristic is just a name, it was not chosen arbitrarily.
There is a similarity between a quantum characteristic of three types of strong nuclear field charges called "color" and three main colors of visible light, combination of which in proper proportion can produce any other color.
That's why we say that
anti-red = cyan (R=G+B),
anti-green = magenta (G=R+B),
anti-blue = yellow (B=R+G).
Analogously, a combination of all three anti-colors produces black (also, colorless, that is neutral, not charged) charge
R + G + B = 0
Quarks can have one of three possible color charges (or just colors) (R, G, B).
Anti-quarks have one of three anti-colors (R, G, B).
Three quarks of three different main colors make up a colorless (that is neutral and observable) proton or neutron.
For example,
p=u+u+d or p=u+d+u,
n=d+d+u or n=u+d+d.
Three anti-quarks of three different anti-colors make up a colorless anti-proton or anti-neutron.
For example,
p=u+u+d or p=d+u+u,
n=d+u+d or n=d+d+u.
We can obtain a colorless combination of a quark of some color and an anti-quark of a corresponding anti-color.
These two quarks, one of the main color and an anti-quark of the corresponding anti-color (like, u+d) make up a particle called meson.
Quarks are usually confined to a combination that has zero color charge, like a triplet of quarks of three main colors in a proton or a duo of quark and anti-quark of a corresponding anti-color in a meson.
Gluons
Gluons, like quarks, are color charged. A very important difference is that gluons carry two different color charges at the same time, while quarks are color charged with only one.
More precisely, gluons have one charge of the main color and another charge of an anti-color.
For example, green (G) and anti-red (R).
Let's see what happens when a quark emits a gluon.
Assume, a green quark emits green/anti-red gluon.
In simple terms, we subtract the green from green quark and subtract anti-red from the result.
Subtracting anti-red is equivalent to adding red. Therefore, a quark becomes a red one.
quark(G) → gluon(G,R) =
= quark(G − G − R) =
= quark(G − G + R) =
= quark(R)
If this gluon is subsequently absorbed by a red quark, we add to its color charge green and anti-red. Adding anti-red is equivalent to subtracting red. The original red color, therefore, disappears, but green will be added, so this quark becomes green.
qluon(G,R) → quark(R) =
quark(G + R + R) =
= quark(G − R + R) =
= quark(G)
The emitting of a green/anti-red gluon by a green quark and subsequent absorbing it by a red quark results in exchange of colors between these quarks. A green quark becomes red and red one becomes green.
So, quarks can change color by emitting or absorbing gluons.
If this happens inside a nucleon (a proton or a neutron), the color neutrality of this nucleon is preserved. This is a conservation of color during this process of emitting and absorbing of a gluon.
Quarks inside a nucleon constantly exchange gluons, thus establishing a strong force that is responsible for the integrity of a nucleon.
While quarks exchange the color charges, a nucleon as a whole always remains color neutral, stable and observable.
Residual Strong Force
As we stated above, three quarks make up a nucleon, uud for a proton or udd for a neutron.
Inside a nucleon these quarks have different color charges (R, G and B) and exchange gluons to maintain their nucleon's color charge as a whole neutral (R+G+B = 0), exerting strong forces to assure a nucleon is stable and observable.
The question is, what keeps different nucleons together?
The answer, as we understand it today, is related to the same strong force and is the force called residual strong force.
Let's start with a process inside a proton, the particle #1 in an interaction we analyze and use a symbol p1 for it. Its three quarks uud constantly exchange gluons, which constantly exchanges their color charge.
(a) For some reason during this process a pair of quark d and anti-quark d are born as a result of these interactions.
p1(uud) → p1(uud) + d + d
(b) The next step is a replacement of one quark u inside a proton with quark d born above, which effectively changes quark set from uud (proton) to udd (neutron) and releases quark u.
This released quark u combines with anti-quark d born above making a virtual (very short lived) π-meson (short name is pion) π(ud).
p1(uud) + d + d →
→ n1(udd) + π(ud)
(c) Now a proton (particle #1) has transformed into a neutron and π-meson π(ud) that immediately contacted a neighboring particle #2 which is neutron n2(udd).
An anti-quark d of π-meson annihilates with quark d of this neutron (particle #2) leaving an empty spot in a neutron.
Quark u from π-meson takes an empty spot, effectively converting the whole particle into proton p2(uud).
π(ud) + n2(udd) → p2(uud)
Analogous transformation of a particle #1, neutron, transforming into a proton, and, subsequently, a particle #2, proton, transforming into a neutron, is possible as well:
(a)n1(udd) → n1(udd) + u + u
(b) n1(udd) + u + u →
→ p1(uud) + π(du)
(c) π(du) + p2(uud) → n2(udd)
The above process of transformation of a proton into a neutron and a neighboring neutron into a proton with corresponding exchange of quarks is the manifestation of residual strong forces that keep the nucleons (protons and neutron) together inside a nucleus.
That's why we observe neutrons inside any multiple protons nuclei, they are the results of constant transformation and interaction with protons, carriers of electric properties of an atom.
That's why the number of neutrons is equal (for lighter nuclei) or greater (for heavier nuclei) than the number of protons.
Obviously, residual strong forces on distances comparable with a radius of a proton should be stronger than electric repulsion between protons to keep the nucleus from disintegration.
Monday, February 27, 2023
Saturday, February 18, 2023
Quarks: UNIZOR.COM - Physics4Teens - Atoms - Elementary Particles
Notes to a video lecture on http://www.unizor.com
Quarks
Let's recall the steps of progress of our understanding of the structure of matter.
1. Splitting a drop of water or cutting the wire we gradually reached the smallest particle that retains the properties of an original object - molecule.
2. Then we realized that thousands of different molecules consist of different combinations of about a hundred of different atoms that have their own characteristics.
3. Later discoveries led to inner structure of every atom as consisting of a nucleus surrounded by shells filled with moving electrons.
4. Farther experiments proved that nucleus itself is a combination of protons and neutrons. So, three main particles - electrons, protons and neutrons - are the building blocks of all atoms.
5. Thousands of experiments showed the existence of other particles that differ from the main ones mentioned above. More than 200 particles have been discovered by physicists through numerous experiments. The number of these new particles made the picture of the structure of matter that we had in mind significantly less "structural" or, plainly, just messy.
It's time to go deeper into inner structure of all particles.
Are there any small number of smaller than proton or neutron particles, whose combinations make up already discovered particles inasmuch as about a hundred different atoms make up thousands of different molecules by grouping in different combinations?
The first theoretical answer was suggested in 1964 by Murray Gell-Mann and George Zweig. It was partially confirmed by experiments and, as a result, is accepted as a working model.
Their proposal was that protons and neutrons are not elementary particles, but, in turn, are composed of smaller particles called quarks.
The usefulness of such an approach can be demonstrated using an example from the previous lecture about isotopes.
Recall how isotope carbon-14 is formed.
Cosmic radiation hits the atoms in the upper layers of the atmosphere, breaking them into individual particles and producing free neutrons.
A free flying neutron hits an atom of nitrogen in our atmosphere, kicks off one proton, replacing it with itself, and frees up an electron.
Kicked off proton and an electron combine into a hydrogen causing the following reaction
714N + 01n → 614C + 11H
The process of carbon-14 decaying is rather complex, but can be described in an oversimplified form as follows.
A neutron in the nucleus of unstable carbon-14 transforms into a pair proton+electron. This does not change the electric neutrality of the atom, does not change the atomic mass, it remains 14, but atomic number increases by 1, thereby creating an atom of stable nitrogen.
This nuclear reaction can be described (in an oversimplified form) as
614C → 714N + e− + ?
where ? signifies additional participants in this transformation that we cannot discuss at this point because it requires knowledge of other elementary particles beyond the main ones (electron, proton and neutron).
While a transformation of an atom of nitrogen into an atom of carbon-14 is physically easy to understand (a neutron kicks off a proton and electron, replacing and taking place of a proton in a nucleus), the reverse transformation of a neutron to proton and electron via decay is less understandable, as it seems to happen without material physical factors.
It would be more understandable if this transformation can be expressed as replacing of something with something else, as in the transformation of nitrogen into carbon-14 by replacing a proton with a neutron.
Developing this idea, physicists came to a model of neutron and proton based on some smaller elementary particles and a transformation of one into another as a replacing of one elementary component with another.
The first obstacle to overcome is electric charge of a proton and electric neutrality of a neutron. If these main particles have smaller elementary components, the electric charge must be distributed among them.
Taking electric charge of a proton as +1, its components must have it as a fraction.
Here is one way to implement it.
Assume, a proton is a combination of two elementary particles, X with an electric charge +½ each, and a neutron is a combination of a particle X with an electric charge +½ and a particle Y with electric charge −½.
Then the total charge of a proton (X+X) is +½+½=+1 and for a neutron (X+Y) it is +½−½=0 as it should be.
Consider a different model.
Particle X has charge +2/3 and particle Y has charge −1/3. Then a proton can be composed of X+X+Y with charge +2/3+2/3−1/3=1, while a neutron can be composed of X+Y+Y with charge +2/3−1/3−1/3=0.
The next characteristic to satisfy using this type of modeling protons and neutrons as consisting of smaller components is mass of a particle.
These components must have masses, sum of which is equal to corresponding larger particles. Actually, almost equal because of mass and energy relationship E=m·c².
What's more difficult is to come up with a model that satisfies not only charges and masses of protons and neutrons, but also other particles observed in experiments (antiprotons, antineutrons, pions, barions, mesons etc.).
Mathematically, it means to solve a system of many linear equations (as many as the number of particles we consider as consisting from the components times the number of parameters we have to match, like electric charge and mass, separately) with as few unknowns as possible.
The latest solution to this problem is so called Standard Model that proposed relatively few elementary (not divisible any more) particles with certain characteristics.
According to Standard Model, six different "flavors" of elementary (not divisible) particles called quarks are the building blocks of about 200 observable particles.
These different quarks are called Up (u), Down (d), Charm (c), Strange (s), Top (t) and Bottom (b).
Each quark has an electric charge (positive, negative or zero), mass and other characteristics.
Here is an electric charge table with the unit of charge 1 being associated with proton (+1) or electron (−1):
Up: +2/3
Down: −1/3
Charm: +2/3
Strange: −1/3
Top: +2/3
Bottom: −1/3
They are combined into different combinations, producing different particles.
For example, proton is made from two Up and one Down quark:
p = uud
Electric charge of proton is +2/3+2/3−1/3=+1, as it should.
Neutron is made from one Up and two Down quarks:
n = udd
Electric charge of a neutron is +2/3−1/3−1/3=0, as it should.
The process of transformation of a neutron into a proton and electron can be imagined as replacing one u quark with a d quark.
Where the new d quark comes from, how electron is created and where a released u quark goes to is a separate issue, which is beyond the scope of this lecture.
But complexity of the Standard Model is, actually, higher than this.
For each quark of the above six types there is an anti-quark.
Its electric charge is opposite to the corresponding quark.
In addition, quarks have a characteristic called color with values red, green and blue. These "colors" have nothing to do with the colors observable by our eyes, they are just used to characterize particular quarks or their combination.
Electron belongs to another group of particles, it's not constructed from other particles, it's an elementary particle. So are muons and tau particles.
Yet another group of elementary particles (not quarks) is responsible for carrying forces between particles (electrostatic, strong, weak etc.) One of the particles in this group is photon that carries electromagnetic force. Gluon is a particle responsible for strong forces inside a nucleus.
In a word, the contemporary model of the structure of particles is very complex and requires deep studying to understand it completely.
This complexity is well represented by the following illustration of the Standard Model authored by Chris Quigg and taken from the Web site https://www.quantamagazine.org
(to view all the details, click the right button and open it in a new tab)
Quarks
Let's recall the steps of progress of our understanding of the structure of matter.
1. Splitting a drop of water or cutting the wire we gradually reached the smallest particle that retains the properties of an original object - molecule.
2. Then we realized that thousands of different molecules consist of different combinations of about a hundred of different atoms that have their own characteristics.
3. Later discoveries led to inner structure of every atom as consisting of a nucleus surrounded by shells filled with moving electrons.
4. Farther experiments proved that nucleus itself is a combination of protons and neutrons. So, three main particles - electrons, protons and neutrons - are the building blocks of all atoms.
5. Thousands of experiments showed the existence of other particles that differ from the main ones mentioned above. More than 200 particles have been discovered by physicists through numerous experiments. The number of these new particles made the picture of the structure of matter that we had in mind significantly less "structural" or, plainly, just messy.
It's time to go deeper into inner structure of all particles.
Are there any small number of smaller than proton or neutron particles, whose combinations make up already discovered particles inasmuch as about a hundred different atoms make up thousands of different molecules by grouping in different combinations?
The first theoretical answer was suggested in 1964 by Murray Gell-Mann and George Zweig. It was partially confirmed by experiments and, as a result, is accepted as a working model.
Their proposal was that protons and neutrons are not elementary particles, but, in turn, are composed of smaller particles called quarks.
The usefulness of such an approach can be demonstrated using an example from the previous lecture about isotopes.
Recall how isotope carbon-14 is formed.
Cosmic radiation hits the atoms in the upper layers of the atmosphere, breaking them into individual particles and producing free neutrons.
A free flying neutron hits an atom of nitrogen in our atmosphere, kicks off one proton, replacing it with itself, and frees up an electron.
Kicked off proton and an electron combine into a hydrogen causing the following reaction
714N + 01n → 614C + 11H
The process of carbon-14 decaying is rather complex, but can be described in an oversimplified form as follows.
A neutron in the nucleus of unstable carbon-14 transforms into a pair proton+electron. This does not change the electric neutrality of the atom, does not change the atomic mass, it remains 14, but atomic number increases by 1, thereby creating an atom of stable nitrogen.
This nuclear reaction can be described (in an oversimplified form) as
614C → 714N + e− + ?
where ? signifies additional participants in this transformation that we cannot discuss at this point because it requires knowledge of other elementary particles beyond the main ones (electron, proton and neutron).
While a transformation of an atom of nitrogen into an atom of carbon-14 is physically easy to understand (a neutron kicks off a proton and electron, replacing and taking place of a proton in a nucleus), the reverse transformation of a neutron to proton and electron via decay is less understandable, as it seems to happen without material physical factors.
It would be more understandable if this transformation can be expressed as replacing of something with something else, as in the transformation of nitrogen into carbon-14 by replacing a proton with a neutron.
Developing this idea, physicists came to a model of neutron and proton based on some smaller elementary particles and a transformation of one into another as a replacing of one elementary component with another.
The first obstacle to overcome is electric charge of a proton and electric neutrality of a neutron. If these main particles have smaller elementary components, the electric charge must be distributed among them.
Taking electric charge of a proton as +1, its components must have it as a fraction.
Here is one way to implement it.
Assume, a proton is a combination of two elementary particles, X with an electric charge +½ each, and a neutron is a combination of a particle X with an electric charge +½ and a particle Y with electric charge −½.
Then the total charge of a proton (X+X) is +½+½=+1 and for a neutron (X+Y) it is +½−½=0 as it should be.
Consider a different model.
Particle X has charge +2/3 and particle Y has charge −1/3. Then a proton can be composed of X+X+Y with charge +2/3+2/3−1/3=1, while a neutron can be composed of X+Y+Y with charge +2/3−1/3−1/3=0.
The next characteristic to satisfy using this type of modeling protons and neutrons as consisting of smaller components is mass of a particle.
These components must have masses, sum of which is equal to corresponding larger particles. Actually, almost equal because of mass and energy relationship E=m·c².
What's more difficult is to come up with a model that satisfies not only charges and masses of protons and neutrons, but also other particles observed in experiments (antiprotons, antineutrons, pions, barions, mesons etc.).
Mathematically, it means to solve a system of many linear equations (as many as the number of particles we consider as consisting from the components times the number of parameters we have to match, like electric charge and mass, separately) with as few unknowns as possible.
The latest solution to this problem is so called Standard Model that proposed relatively few elementary (not divisible any more) particles with certain characteristics.
According to Standard Model, six different "flavors" of elementary (not divisible) particles called quarks are the building blocks of about 200 observable particles.
These different quarks are called Up (u), Down (d), Charm (c), Strange (s), Top (t) and Bottom (b).
Each quark has an electric charge (positive, negative or zero), mass and other characteristics.
Here is an electric charge table with the unit of charge 1 being associated with proton (+1) or electron (−1):
Up: +2/3
Down: −1/3
Charm: +2/3
Strange: −1/3
Top: +2/3
Bottom: −1/3
They are combined into different combinations, producing different particles.
For example, proton is made from two Up and one Down quark:
p = uud
Electric charge of proton is +2/3+2/3−1/3=+1, as it should.
Neutron is made from one Up and two Down quarks:
n = udd
Electric charge of a neutron is +2/3−1/3−1/3=0, as it should.
The process of transformation of a neutron into a proton and electron can be imagined as replacing one u quark with a d quark.
Where the new d quark comes from, how electron is created and where a released u quark goes to is a separate issue, which is beyond the scope of this lecture.
But complexity of the Standard Model is, actually, higher than this.
For each quark of the above six types there is an anti-quark.
Its electric charge is opposite to the corresponding quark.
In addition, quarks have a characteristic called color with values red, green and blue. These "colors" have nothing to do with the colors observable by our eyes, they are just used to characterize particular quarks or their combination.
Electron belongs to another group of particles, it's not constructed from other particles, it's an elementary particle. So are muons and tau particles.
Yet another group of elementary particles (not quarks) is responsible for carrying forces between particles (electrostatic, strong, weak etc.) One of the particles in this group is photon that carries electromagnetic force. Gluon is a particle responsible for strong forces inside a nucleus.
In a word, the contemporary model of the structure of particles is very complex and requires deep studying to understand it completely.
This complexity is well represented by the following illustration of the Standard Model authored by Chris Quigg and taken from the Web site https://www.quantamagazine.org
(to view all the details, click the right button and open it in a new tab)
Sunday, February 12, 2023
Isotopes: UNIZOR.COM - Physics4Teens - Atoms - Nucleus and Electrons
Notes to a video lecture on http://www.unizor.com
Isotopes
Isotopes are atoms that have the same number of protons (atomic number Z) but different number of neutrons (N).
Since the number of electrons and their distribution among shells and subshells are the same for different isotopes of atoms with the same atomic number, these isotopes have practically the same chemical properties.
At the same time, since the number of neutrons of different isotopes of atoms with the same atomic number is different, certain physical properties of these atoms might be quite different.
Identification of different isotopes involves specifying their atomic mass.
For example, carbon has 6 protons and 6 electrons, but the number of neutrons can be 6, 7 or 8 in its nucleus with atomic masses of these isotopes, correspondingly,
A=Z+N=6+6=12,
A=Z+N=6+7=13 and
A=Z+N=6+8=14.
These isotopes are named, according to their atomic mass, carbon-12, carbon-13 and carbon-14.
Another example: uranium-235 (symbol 92235U) with 92 protons, 92 electrons (atomic number is Z=92) and 143 neutrons (N=143), which has atomic mass A=235, and uranium-238 (symbol 92238U) with the same number of protons, electrons and the same atomic number Z=92, but with 146 neutrons (N=146) and atomic mass A=238.
In most cases one particular isotope of an atom is sufficiently stable and can be found in nature, while other isotopes of the same atom might be more or less radioactive, that is their atoms break with time into other (smaller) atoms - a process called radioactive decay.
The role of neutrons in a nucleus is to stabilize it. Since protons are positively charged and repel each other, neutrons serve as a buffer between them and, therefore, their number is usually equal or greater than the number of protons.
Obviously, so-called strong forces inside a nucleus that bind together all particles (protons to protons, protons to neutrons, neutrons to neutrons) are the main forces that hold a nucleus as a whole.
Interestingly, most nuclei with even atomic number Z and even number of neutrons N demonstrate more stability than those with either Z or N or both are odd.
Radiocarbon Dating
As an example of the usage of isotopes, let's describe the determination of age of certain samples found by archeologists using radiocarbon dating.
The most stable and abundant isotope of carbon is the one with 6 protons and 6 neutrons in a nucleus - carbon-12 612C.
This carbon isotope plays extremely important role in organisms, as carbon is one of the main building blocks of all living beings on Earth.
Firstly, let's examine where carbon-14 comes from.
High energy cosmic rays bombard the Earth and break atoms of the upper layer of atmosphere, releasing some elementary particles, electrons, protons and neutrons.
Next, some neutrons (01n) hit the atoms of nitrogen (714N) in the air causing production of carbon-14 (614C) and hydrogen (11H) in the following nuclear reaction:
714N + 01n → 614C + 11H
The reaction above describes the process of a neutron hitting an atom of nitrogen, kicking out a proton and an electron that connect to each other in the form of an atom of hydrogen, while replacing a missed proton with itself, thereby reducing the atomic number by one, while retaining the atomic mass, which transforms it into an isotope carbon-14.
Now carbon-14 is formed in the air in some small quantity and participates in the cycle of life. Any living organism absorbs it the same way it absorbs regular carbon-12 during its life time and, therefore, it's present in some quantity inside this organism in proportion to regular carbon-12 similar to its proportion that exists in nature.
As we know, carbon-14 is not a stable element, it decays with a half-life about 5730 years.
The process of decaying is rather complex, but can be described in an oversimplified form as follows.
A neutron in the nucleus of unstable carbon-14 transforms into a pair proton+electron. This does not change the electric neutrality of the atom, does not change the atomic mass, it remains 14, but atomic number increases by 1, thereby creating an atom of stable nitrogen.
This nuclear reaction can be described (in an oversimplified form) as
614C → 714N + e− + ?
where ? signifies additional participants in this transformation that we cannot discuss at this point because it requires knowledge of other elementary particles beyond the main ones (electron, proton and neutron).
While an organism lives, the relative amount of carbon-14 in it is maintained on the same level. Whatever is decayed is replenished from the outside world as part of the organism's existence.
As soon as life stops, absorption of carbon-14 stops and, whatever is present in the organism is no longer renewed, but decays according to the laws of half life.
If the amount of carbon-14 in the dead tree is 1/2 of whatever is normal, the tree died approximately 5730·1=5730 years ago.
If the amount of carbon-14 in the dead tree is 1/4 of whatever is normal, the tree died approximately 5730·2=11460 years ago.
If the amount of carbon-14 in the dead tree is 1/8 of whatever is normal, the tree died approximately 5730·3=17190 years ago.
etc.
In general, if the amount of carbon-14 in the dead tree is 1/N of whatever is normal, the tree died approximately 5730·log2N years ago.
Isotopes
Isotopes are atoms that have the same number of protons (atomic number Z) but different number of neutrons (N).
Since the number of electrons and their distribution among shells and subshells are the same for different isotopes of atoms with the same atomic number, these isotopes have practically the same chemical properties.
At the same time, since the number of neutrons of different isotopes of atoms with the same atomic number is different, certain physical properties of these atoms might be quite different.
Identification of different isotopes involves specifying their atomic mass.
For example, carbon has 6 protons and 6 electrons, but the number of neutrons can be 6, 7 or 8 in its nucleus with atomic masses of these isotopes, correspondingly,
A=Z+N=6+6=12,
A=Z+N=6+7=13 and
A=Z+N=6+8=14.
These isotopes are named, according to their atomic mass, carbon-12, carbon-13 and carbon-14.
Another example: uranium-235 (symbol 92235U) with 92 protons, 92 electrons (atomic number is Z=92) and 143 neutrons (N=143), which has atomic mass A=235, and uranium-238 (symbol 92238U) with the same number of protons, electrons and the same atomic number Z=92, but with 146 neutrons (N=146) and atomic mass A=238.
In most cases one particular isotope of an atom is sufficiently stable and can be found in nature, while other isotopes of the same atom might be more or less radioactive, that is their atoms break with time into other (smaller) atoms - a process called radioactive decay.
The role of neutrons in a nucleus is to stabilize it. Since protons are positively charged and repel each other, neutrons serve as a buffer between them and, therefore, their number is usually equal or greater than the number of protons.
Obviously, so-called strong forces inside a nucleus that bind together all particles (protons to protons, protons to neutrons, neutrons to neutrons) are the main forces that hold a nucleus as a whole.
Interestingly, most nuclei with even atomic number Z and even number of neutrons N demonstrate more stability than those with either Z or N or both are odd.
Radiocarbon Dating
As an example of the usage of isotopes, let's describe the determination of age of certain samples found by archeologists using radiocarbon dating.
The most stable and abundant isotope of carbon is the one with 6 protons and 6 neutrons in a nucleus - carbon-12 612C.
This carbon isotope plays extremely important role in organisms, as carbon is one of the main building blocks of all living beings on Earth.
Firstly, let's examine where carbon-14 comes from.
High energy cosmic rays bombard the Earth and break atoms of the upper layer of atmosphere, releasing some elementary particles, electrons, protons and neutrons.
Next, some neutrons (01n) hit the atoms of nitrogen (714N) in the air causing production of carbon-14 (614C) and hydrogen (11H) in the following nuclear reaction:
714N + 01n → 614C + 11H
The reaction above describes the process of a neutron hitting an atom of nitrogen, kicking out a proton and an electron that connect to each other in the form of an atom of hydrogen, while replacing a missed proton with itself, thereby reducing the atomic number by one, while retaining the atomic mass, which transforms it into an isotope carbon-14.
Now carbon-14 is formed in the air in some small quantity and participates in the cycle of life. Any living organism absorbs it the same way it absorbs regular carbon-12 during its life time and, therefore, it's present in some quantity inside this organism in proportion to regular carbon-12 similar to its proportion that exists in nature.
As we know, carbon-14 is not a stable element, it decays with a half-life about 5730 years.
The process of decaying is rather complex, but can be described in an oversimplified form as follows.
A neutron in the nucleus of unstable carbon-14 transforms into a pair proton+electron. This does not change the electric neutrality of the atom, does not change the atomic mass, it remains 14, but atomic number increases by 1, thereby creating an atom of stable nitrogen.
This nuclear reaction can be described (in an oversimplified form) as
614C → 714N + e− + ?
where ? signifies additional participants in this transformation that we cannot discuss at this point because it requires knowledge of other elementary particles beyond the main ones (electron, proton and neutron).
While an organism lives, the relative amount of carbon-14 in it is maintained on the same level. Whatever is decayed is replenished from the outside world as part of the organism's existence.
As soon as life stops, absorption of carbon-14 stops and, whatever is present in the organism is no longer renewed, but decays according to the laws of half life.
If the amount of carbon-14 in the dead tree is 1/2 of whatever is normal, the tree died approximately 5730·1=5730 years ago.
If the amount of carbon-14 in the dead tree is 1/4 of whatever is normal, the tree died approximately 5730·2=11460 years ago.
If the amount of carbon-14 in the dead tree is 1/8 of whatever is normal, the tree died approximately 5730·3=17190 years ago.
etc.
In general, if the amount of carbon-14 in the dead tree is 1/N of whatever is normal, the tree died approximately 5730·log2N years ago.
Saturday, February 11, 2023
Main particles: UNIZOR.COM - Physics4Teens - Atoms - Nucleus and Electrons
Notes to a video lecture on http://www.unizor.com
Main Particles
Three particles constitute the main building blocks of any atom:
electrons,
protons and
neutrons.
Let's examine their properties and functions in maintaining the integrity of an atom.
The basic atom model assumes that electrons are negatively charged particles flying on some orbits around an atom's nucleus that, in turn, contains certain number of positively charged protons and electrically neutral neutrons.
We discussed in details the distribution of electrons in shells (#1, #2, #3 etc.) and subshells (s, p, d etc.) around a nucleus.
These electrons (primarily, those on higher orbits) get involved in chemical reactions among atoms, facilitating creation of different molecules by either ionic or covalent bonding (see previous lectures on this topic).
The number of protons in a nucleus should be equal to the number of electrons circulating on orbits around this nucleus to maintain atom's neutrality.
This number is called an atomic number Z of an atom.
The electrostatic attraction between positive protons and negative electrons keeps the electrons on their stationary orbits.
But electrostatic forces repel from each other particles charged the same way (positive or negative). So, what keeps the protons in the nucleus and holds the atom's integrity?
Apparently, elementary particles inside a nucleus are held together by other forces, much stronger than electrostatic. They are called (not surprisingly) strong or nuclear forces.
These strong forces act only on a very small distance between particles inside a nucleus and have no noticeable influence on electrons around a nucleus.
Strong forces exist between protons, between protons and neutrons and between neutrons. Since neutrons are electrically neutral, greater number of them in the nucleus keeps the nucleus stronger, preventing electrostatic forces or external forces (like bombarding the nucleus with other particles) to break up an atom.
The total number of protons (Z) and neutrons (N) is called atomic mass of an atom (A=Z+N).
Nucleus of an atom takes a very small amount of space relatively to an atom's size.
For example, a nucleus of an atom of hydrogen, which consists of only one proton, has a diameter of the order of 10−15 meter, while a diameter of an atom of hydrogen is more than 100,000 greater (of the order of 10−10 meter).
Heavier elements that contain hundreds of particles (protons and neutrons, commonly called nucleons) in a nucleus have larger diameter of a nucleus, about 10 times larger than hydrogen, and their atoms are thousands times greater than their nuclei.
At the same time, the mass of an atom is concentrated in its nucleus. The nucleus' share in the mass of an atom is, approximately, 99.9%. The rest of mass is the mass of electrons.
These very approximate numbers do not take into consideration the effect of mass-energy relationship, according to Einstein Theory of Relativity formula E=m·c².
Since chemical properties of an element are defined by its electrons, the atomic number (that is, the number of electrons or equal to it the number of protons) defines chemical properties of an atom.
Different number of neutrons with the same number of protons in a nucleus of an element can occur, but these different compositions of a nucleus do not change the chemical properties of an element.
Atoms with the same number of protons but different number of neutrons are called isotopes.
We will address it in the next lecture.
Main Particles
Three particles constitute the main building blocks of any atom:
electrons,
protons and
neutrons.
Let's examine their properties and functions in maintaining the integrity of an atom.
The basic atom model assumes that electrons are negatively charged particles flying on some orbits around an atom's nucleus that, in turn, contains certain number of positively charged protons and electrically neutral neutrons.
We discussed in details the distribution of electrons in shells (#1, #2, #3 etc.) and subshells (s, p, d etc.) around a nucleus.
These electrons (primarily, those on higher orbits) get involved in chemical reactions among atoms, facilitating creation of different molecules by either ionic or covalent bonding (see previous lectures on this topic).
The number of protons in a nucleus should be equal to the number of electrons circulating on orbits around this nucleus to maintain atom's neutrality.
This number is called an atomic number Z of an atom.
The electrostatic attraction between positive protons and negative electrons keeps the electrons on their stationary orbits.
But electrostatic forces repel from each other particles charged the same way (positive or negative). So, what keeps the protons in the nucleus and holds the atom's integrity?
Apparently, elementary particles inside a nucleus are held together by other forces, much stronger than electrostatic. They are called (not surprisingly) strong or nuclear forces.
These strong forces act only on a very small distance between particles inside a nucleus and have no noticeable influence on electrons around a nucleus.
Strong forces exist between protons, between protons and neutrons and between neutrons. Since neutrons are electrically neutral, greater number of them in the nucleus keeps the nucleus stronger, preventing electrostatic forces or external forces (like bombarding the nucleus with other particles) to break up an atom.
The total number of protons (Z) and neutrons (N) is called atomic mass of an atom (A=Z+N).
Nucleus of an atom takes a very small amount of space relatively to an atom's size.
For example, a nucleus of an atom of hydrogen, which consists of only one proton, has a diameter of the order of 10−15 meter, while a diameter of an atom of hydrogen is more than 100,000 greater (of the order of 10−10 meter).
Heavier elements that contain hundreds of particles (protons and neutrons, commonly called nucleons) in a nucleus have larger diameter of a nucleus, about 10 times larger than hydrogen, and their atoms are thousands times greater than their nuclei.
At the same time, the mass of an atom is concentrated in its nucleus. The nucleus' share in the mass of an atom is, approximately, 99.9%. The rest of mass is the mass of electrons.
These very approximate numbers do not take into consideration the effect of mass-energy relationship, according to Einstein Theory of Relativity formula E=m·c².
Since chemical properties of an element are defined by its electrons, the atomic number (that is, the number of electrons or equal to it the number of protons) defines chemical properties of an atom.
Different number of neutrons with the same number of protons in a nucleus of an element can occur, but these different compositions of a nucleus do not change the chemical properties of an element.
Atoms with the same number of protons but different number of neutrons are called isotopes.
We will address it in the next lecture.
Thursday, February 9, 2023
Valence Electrons: UNIZOR.COM - Physics4Teens - Atoms - Interaction of A...
Notes to a video lecture on http://www.unizor.com
Valence Electrons
Previous lecture was about chemical reaction between elements - bonding between atoms that does not affect their nuclei.
We have seen that the most important role in these reactions is played by electrons in the outer most shell of an atom.
In particular, chemical reactions are expected between elements that have incomplete outer subshells, but complementary to each other to form complete subshells by either borrowing electrons from each other, forming electrovalent or ionic bonding between positively and negatively charged ions or sharing electrons, forming a covalent bonding between atoms.
Recall the chemical bonding between atoms of sodium and chlorine.
Sodium has atomic number 11, and its electrons are arranged as
Na: 1s2 2s2 2p6 3s1
Chlorine has atomic number 17, and its electrons are arranged as
Cl: 1s2 2s2 2p6 3s2 3p5
The mechanism of bonding can be represented in such a case as follows.
1. Sodium atom releases the only electron from the subshell 3s, becoming a positive ion
Na → Na+ + e−
2. Chlorine atom captures this electron in its subshell 3p, becoming negative ion
Cl + e− → Cl−
3. Now all subshells are filled to capacity and both atoms are electrically charged with opposite charges, which makes them stick to each other, forming a molecule of salt.
That was a typical example of electrovalent or ionic bonding.
Valence electrons are those exact electrons that are capable of participating in bonding with other electrons of other atoms.
In most cases they belong to the outer electronic shell of an atom.
Elements with electron structure ending in 1 electron in the outer subshell s, like sodium (Na), have that 1 electron as the only valence electron. The valency of such elements is 1. Atoms of these elements often bond by giving away this electron to complete other atom's outer subshell, like ionic bonding with chlorine (Cl) that needs exactly one electron to complete its outer p subshell. The valency of the counterpart atom in such a case is also 1.
The structure of a molecule that results in bonding of these two atoms can be symbolically expressed as
Na−Cl
where a single bar between symbols of elements corresponds to the valency of each.
Considering this is an ionic bonding, we might as well use more precise symbolics
Na+−Cl−
Elements with electron structure ending in 2 electrons in the outer subshell s, like barium (Ba), have these 2 electrons as the only valence electrons. Atoms of these elements often bond by giving away both of these electrons to complete other atom's outer subshell, like ionic bonding with two atoms of chlorine (Cl), each of which needs one electron to complete its outer p subshell, forming a molecule BaCl2.
The structure of a molecule that results in bonding of these three atoms can be symbolically expressed as
Cl−Ba−Cl
where bars correspond to the valency of each atom, 2 for barium and 1 for chlorine.
This process can be described as follows.
1. Barium atom (atomic number 56) frees two electrons from the outer subshell 6s, becoming a positive ion
Ba → Ba2+ + 2e−
2. Two chlorine atoms capture one electron each in their outer subshell 3p, becoming negative ions
2Cl + 2e− → 2Cl−
3. Now all subshells are filled to capacity and three atoms are electrically charged. One atom of barium is positive, two atoms of chlorine are negative, which makes these two atoms of chorine stick to an atom of barium, forming a molecule of barium chloride BaCl2.
So, more precise representation of this molecule would be
Cl−−Ba+−Cl−
Let's consider a more complicated case of forming aluminum oxide - a molecule combining atoms of aluminum (Al) and oxygen (O).
The configuration of 13 electrons in the atom of aluminum is:
Al: 1s2 2s2 2p6 3s2 3p1
The configuration of 8 electrons in the atom of oxygen is:
O: 1s2 2s2 2p4
As we see, aluminum has one valence electron in subshell 3p. If it loses this electron, its 3rd subshell would still have two electrons in subshell 3s. While technically complete, it's still exposed to be captured by some other atom.
So, an atom of aluminum can lose either (only under special conditions) 1 electron, the 3p1, or (under normal conditions) 3 electrons, the 3p1 and 3s2.
The valency of aluminum is, therefore, either 1 (only under special conditions) or, typically, 3.
A possible molecular bonding between 2 atoms of aluminum and 1 atom of oxygen Al2O that can be established in special laboratory conditions would look like this:
Al−O−Al
This is a very unstable molecule because the 3rd shell of the atom of aluminum with only one remaining subshell 3s and two electrons in it still remains exposed.
Much more stable molecule is formed, when 2 atoms of aluminum contribute 6 electrons (3 electrons from each atom, emptying subshells 3s and 3p) and 3 atoms of oxygen capture them (2 electrons are captured by each oxygen atom to fill its 2p subshell). The formula of this aluminum oxide molecule is Al2O3 with the structure that can be pictured as
O=Al−O−Al=O
where bars correspond to the valency of each atom, 3 for aluminum and 2 for oxygen.
From the position of an exchange of electrons this can be represented as follows.
1. Two aluminum atoms free 3 electrons each from their outer shell #3 (1 electron from subshell 3p and 2 electrons from subshell 3s), becoming positive ions
2Al → 2Al3+ + 6e−
2. Three oxygen atoms capture 2 electrons each in their outer subshell 2p, becoming negative ions
3O + 6e− → 3O2−
3. Now all subshells are filled to capacity and all 5 atoms are electrically charged. Two atoms of aluminum are positive, three atoms of oxygen are negative, which makes these three atoms of oxygen stick to two atoms of aluminum, forming a molecule of aluminum oxide Al2O3.
The atoms in this molecule are bonded ionically, so we can represent the molecule's structure as
O2−=Al3+−O2−−Al3+=O2−
As you saw from the previous example, in some cases the valency of an atom can be different under different circumstances. While for a bonding between aluminum and oxygen only one stable configuration is observed, in other cases more than one configuration occurs under normal conditions.
The common property of the examples above is that we analyzed the molecules comprised of a metal and non-metal.
Metals have their outer electrons relatively easier departing from their nuclei, that's why in all cases above the bonding between a metal and non-metal was ionic, when metals gave their electrons to non-metals.
As a final example, consider the formation of a molecule of carbon monoxide CO.
The electron configuration of carbon (atomic number 6) is
C: 1s2 2s2 2p2
The configuration of 8 electrons in the atom of oxygen, as we already discussed, is:
O: 1s2 2s2 2p4
None of the elements in a molecule of carbon monoxide is a metal, so their electrons are not capable, ready and willing to depart from the their nuclei, as in metals. As a result, the electrons are not transferred from atom to atom forming ions, but are shared between the atoms to form a covalent bonding.
Two electrons from 2p subshell of carbon and four electrons from 2p subshell of oxygen, totaling 6 electrons (exactly the maximum number for 2p subshell), become a common property of both atoms, completing their corresponding outer subshells 2p.
The act of sharing electrons between atoms of carbon and oxygen is the glue holding the molecule together in covalent bonding.
Valence Electrons
Previous lecture was about chemical reaction between elements - bonding between atoms that does not affect their nuclei.
We have seen that the most important role in these reactions is played by electrons in the outer most shell of an atom.
In particular, chemical reactions are expected between elements that have incomplete outer subshells, but complementary to each other to form complete subshells by either borrowing electrons from each other, forming electrovalent or ionic bonding between positively and negatively charged ions or sharing electrons, forming a covalent bonding between atoms.
Recall the chemical bonding between atoms of sodium and chlorine.
Sodium has atomic number 11, and its electrons are arranged as
Na: 1s2 2s2 2p6 3s1
Chlorine has atomic number 17, and its electrons are arranged as
Cl: 1s2 2s2 2p6 3s2 3p5
The mechanism of bonding can be represented in such a case as follows.
1. Sodium atom releases the only electron from the subshell 3s, becoming a positive ion
Na → Na+ + e−
2. Chlorine atom captures this electron in its subshell 3p, becoming negative ion
Cl + e− → Cl−
3. Now all subshells are filled to capacity and both atoms are electrically charged with opposite charges, which makes them stick to each other, forming a molecule of salt.
That was a typical example of electrovalent or ionic bonding.
Valence electrons are those exact electrons that are capable of participating in bonding with other electrons of other atoms.
In most cases they belong to the outer electronic shell of an atom.
Elements with electron structure ending in 1 electron in the outer subshell s, like sodium (Na), have that 1 electron as the only valence electron. The valency of such elements is 1. Atoms of these elements often bond by giving away this electron to complete other atom's outer subshell, like ionic bonding with chlorine (Cl) that needs exactly one electron to complete its outer p subshell. The valency of the counterpart atom in such a case is also 1.
The structure of a molecule that results in bonding of these two atoms can be symbolically expressed as
Na−Cl
where a single bar between symbols of elements corresponds to the valency of each.
Considering this is an ionic bonding, we might as well use more precise symbolics
Na+−Cl−
Elements with electron structure ending in 2 electrons in the outer subshell s, like barium (Ba), have these 2 electrons as the only valence electrons. Atoms of these elements often bond by giving away both of these electrons to complete other atom's outer subshell, like ionic bonding with two atoms of chlorine (Cl), each of which needs one electron to complete its outer p subshell, forming a molecule BaCl2.
The structure of a molecule that results in bonding of these three atoms can be symbolically expressed as
Cl−Ba−Cl
where bars correspond to the valency of each atom, 2 for barium and 1 for chlorine.
This process can be described as follows.
1. Barium atom (atomic number 56) frees two electrons from the outer subshell 6s, becoming a positive ion
Ba → Ba2+ + 2e−
2. Two chlorine atoms capture one electron each in their outer subshell 3p, becoming negative ions
2Cl + 2e− → 2Cl−
3. Now all subshells are filled to capacity and three atoms are electrically charged. One atom of barium is positive, two atoms of chlorine are negative, which makes these two atoms of chorine stick to an atom of barium, forming a molecule of barium chloride BaCl2.
So, more precise representation of this molecule would be
Cl−−Ba+−Cl−
Let's consider a more complicated case of forming aluminum oxide - a molecule combining atoms of aluminum (Al) and oxygen (O).
The configuration of 13 electrons in the atom of aluminum is:
Al: 1s2 2s2 2p6 3s2 3p1
The configuration of 8 electrons in the atom of oxygen is:
O: 1s2 2s2 2p4
As we see, aluminum has one valence electron in subshell 3p. If it loses this electron, its 3rd subshell would still have two electrons in subshell 3s. While technically complete, it's still exposed to be captured by some other atom.
So, an atom of aluminum can lose either (only under special conditions) 1 electron, the 3p1, or (under normal conditions) 3 electrons, the 3p1 and 3s2.
The valency of aluminum is, therefore, either 1 (only under special conditions) or, typically, 3.
A possible molecular bonding between 2 atoms of aluminum and 1 atom of oxygen Al2O that can be established in special laboratory conditions would look like this:
Al−O−Al
This is a very unstable molecule because the 3rd shell of the atom of aluminum with only one remaining subshell 3s and two electrons in it still remains exposed.
Much more stable molecule is formed, when 2 atoms of aluminum contribute 6 electrons (3 electrons from each atom, emptying subshells 3s and 3p) and 3 atoms of oxygen capture them (2 electrons are captured by each oxygen atom to fill its 2p subshell). The formula of this aluminum oxide molecule is Al2O3 with the structure that can be pictured as
O=Al−O−Al=O
where bars correspond to the valency of each atom, 3 for aluminum and 2 for oxygen.
From the position of an exchange of electrons this can be represented as follows.
1. Two aluminum atoms free 3 electrons each from their outer shell #3 (1 electron from subshell 3p and 2 electrons from subshell 3s), becoming positive ions
2Al → 2Al3+ + 6e−
2. Three oxygen atoms capture 2 electrons each in their outer subshell 2p, becoming negative ions
3O + 6e− → 3O2−
3. Now all subshells are filled to capacity and all 5 atoms are electrically charged. Two atoms of aluminum are positive, three atoms of oxygen are negative, which makes these three atoms of oxygen stick to two atoms of aluminum, forming a molecule of aluminum oxide Al2O3.
The atoms in this molecule are bonded ionically, so we can represent the molecule's structure as
O2−=Al3+−O2−−Al3+=O2−
As you saw from the previous example, in some cases the valency of an atom can be different under different circumstances. While for a bonding between aluminum and oxygen only one stable configuration is observed, in other cases more than one configuration occurs under normal conditions.
The common property of the examples above is that we analyzed the molecules comprised of a metal and non-metal.
Metals have their outer electrons relatively easier departing from their nuclei, that's why in all cases above the bonding between a metal and non-metal was ionic, when metals gave their electrons to non-metals.
As a final example, consider the formation of a molecule of carbon monoxide CO.
The electron configuration of carbon (atomic number 6) is
C: 1s2 2s2 2p2
The configuration of 8 electrons in the atom of oxygen, as we already discussed, is:
O: 1s2 2s2 2p4
None of the elements in a molecule of carbon monoxide is a metal, so their electrons are not capable, ready and willing to depart from the their nuclei, as in metals. As a result, the electrons are not transferred from atom to atom forming ions, but are shared between the atoms to form a covalent bonding.
Two electrons from 2p subshell of carbon and four electrons from 2p subshell of oxygen, totaling 6 electrons (exactly the maximum number for 2p subshell), become a common property of both atoms, completing their corresponding outer subshells 2p.
The act of sharing electrons between atoms of carbon and oxygen is the glue holding the molecule together in covalent bonding.
Thursday, February 2, 2023
Chemical Bonding: UNIZOR.COM - Physics4Teens - Atoms - Interaction of Atoms
Notes to a video lecture on http://www.unizor.com
Chemical Bonding
From the atomic viewpoint, classical chemical bonding between atoms are interactions that do not change the composition of these atoms' nuclei.
Only electrons that surround nuclei interact among themselves, breaking some old connections and establishing new ones.
Chemical bonding can occur between atoms of simple elements, like a single atom of sodium Na and a single atom of chlorine Cl forming their compositions, a molecule of sodium chloride NaCl, which is a molecule of regular salt.
Scientists thought about why some elements bond with each other, if mixed in certain proportion and at some external conditions, while some others are inert, that is refuse to combine with other elements. So called noble gases, like helium, neon, argon or krypton are inert.
Let's examine the electron configuration of above mentioned noble gases.
Helium with atomic number 2 has the following electron configuration
He: 1s2
Neon with atomic number 10 has the following electron configuration
Ne: 1s2 2s2 2p6 =
= [He] + 2s2 2p6
Argon with atomic number 18 has the following electron configuration
Ar: 1s2 2s2 2p6 3s2 3p6 =
= [Ne] + 3s2 3p6
Krypton with atomic number 36 has the following electron configuration
Kr: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 =
= [Ar] + 3d10 4s2 4p6
As you see, all subshells of noble gases are filled to capacity:
max(s) = 2
max(p) = 6
max(d) = 10
and this is very important for stability of atoms.
Those elements that do not have this characteristic of its subshells will be easier to get into chemical bonding that facilitates sharing electrons to complete top most subshells of all involved components.
Let's examine the chemical process between elements using the above example of producing sodium chloride from sodium and chlorine
Na + Cl → NaCl
First of all, let's analyze the electronic structure of both substances.
Sodium has atomic number 11, and its electrons are arranged as
Na: 1s2 2s2 2p6 3s1
Chlorine has atomic number 17, and its electrons are arranged as
Cl: 1s2 2s2 2p6 3s2 3p5
As you see, the first subshell s of the shell #1 (that is, subshell 1s), which can hold up to 2 electrons, is completely filled for both elements, and there can be no more subshells within this shell #1.
The first subshell s of the shell #2 (that is, subshell 2s) is also completely filled for both elements, but shell #2 can have two subshells, s and p, and subshell p has capacity for 6 electrons. As we see, both 2p subshells are filled to capacity in both elements.
The first subshell s of the shell #3 (that is, subshell 3s) has only 1 electron in an atom of sodium.
The atom of chlorine, on the other hand, has this subshell filled to capacity of 2 electrons, but the next subshell 3p has only 5 electrons out of maximum 6.
Now the sharing of electrons comes to play.
The top subshell of sodium 3s contains 1 electron out of maximum 2. If it loses this electron, all its subshells will be complete, but losing electron means becoming positively charged.
The top subshell of chlorine 3p contains 5 electrons out of maximum 6. If it captures one electron, all its subshells will be complete, but capturing an electron means becoming negatively charged.
The mechanism of bonding can be represented in such a case as follows.
1. Sodium atom frees the only electron from the subshell 3s, becoming a positive ion
Na → Na+ + e−
2. Chlorine atom captures this electron in its subshell 3p, becoming negative ion
Cl + e− → Cl−
3. Now all subshells are filled to capacity and both atoms are electrically charged with opposite charges, which makes them stick to each other, forming a molecule of salt.
Let's make a few conclusive statements about this process of forming molecules.
I. Atoms like their subshells to be completely filled up to a maximum of 4m−2, where m is the subshell number (subshell #1 is labeled s, subshell #2 is labeled p etc.)
II. Some atoms are ready to accept electrons to fill up their top subshell from other atoms that are willing to give up their electrons.
III. Some other atoms are ready to give up electrons from their incomplete top subshell, leaving with themselves only complete subshells, if there is a recipient atom of these extra electrons that needs them to complete its top subshell.
IV. The necessity for an atom to have its shells filled up is very strong. Atoms with incomplete top subshells are looking for partners to get into chemical combination. If there is a fit between two atoms to transfer electrons from an incomplete top subshell of one of them to incomplete top subshell of another that completes both, electrons are transferred.
V. After the transfer of electrons that completes both atoms, they become oppositely charged ions that are attracted to each other, which establishes a stable combination.
VI. The complex combinations of more than 2 atoms can also be created based on the same principle. The mechanism is a little more complex, but follows the same idea to complete top subshells of all participants.
Chemical Bonding
From the atomic viewpoint, classical chemical bonding between atoms are interactions that do not change the composition of these atoms' nuclei.
Only electrons that surround nuclei interact among themselves, breaking some old connections and establishing new ones.
Chemical bonding can occur between atoms of simple elements, like a single atom of sodium Na and a single atom of chlorine Cl forming their compositions, a molecule of sodium chloride NaCl, which is a molecule of regular salt.
Scientists thought about why some elements bond with each other, if mixed in certain proportion and at some external conditions, while some others are inert, that is refuse to combine with other elements. So called noble gases, like helium, neon, argon or krypton are inert.
Let's examine the electron configuration of above mentioned noble gases.
Helium with atomic number 2 has the following electron configuration
He: 1s2
Neon with atomic number 10 has the following electron configuration
Ne: 1s2 2s2 2p6 =
= [He] + 2s2 2p6
Argon with atomic number 18 has the following electron configuration
Ar: 1s2 2s2 2p6 3s2 3p6 =
= [Ne] + 3s2 3p6
Krypton with atomic number 36 has the following electron configuration
Kr: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 =
= [Ar] + 3d10 4s2 4p6
As you see, all subshells of noble gases are filled to capacity:
max(s) = 2
max(p) = 6
max(d) = 10
and this is very important for stability of atoms.
Those elements that do not have this characteristic of its subshells will be easier to get into chemical bonding that facilitates sharing electrons to complete top most subshells of all involved components.
Let's examine the chemical process between elements using the above example of producing sodium chloride from sodium and chlorine
Na + Cl → NaCl
First of all, let's analyze the electronic structure of both substances.
Sodium has atomic number 11, and its electrons are arranged as
Na: 1s2 2s2 2p6 3s1
Chlorine has atomic number 17, and its electrons are arranged as
Cl: 1s2 2s2 2p6 3s2 3p5
As you see, the first subshell s of the shell #1 (that is, subshell 1s), which can hold up to 2 electrons, is completely filled for both elements, and there can be no more subshells within this shell #1.
The first subshell s of the shell #2 (that is, subshell 2s) is also completely filled for both elements, but shell #2 can have two subshells, s and p, and subshell p has capacity for 6 electrons. As we see, both 2p subshells are filled to capacity in both elements.
The first subshell s of the shell #3 (that is, subshell 3s) has only 1 electron in an atom of sodium.
The atom of chlorine, on the other hand, has this subshell filled to capacity of 2 electrons, but the next subshell 3p has only 5 electrons out of maximum 6.
Now the sharing of electrons comes to play.
The top subshell of sodium 3s contains 1 electron out of maximum 2. If it loses this electron, all its subshells will be complete, but losing electron means becoming positively charged.
The top subshell of chlorine 3p contains 5 electrons out of maximum 6. If it captures one electron, all its subshells will be complete, but capturing an electron means becoming negatively charged.
The mechanism of bonding can be represented in such a case as follows.
1. Sodium atom frees the only electron from the subshell 3s, becoming a positive ion
Na → Na+ + e−
2. Chlorine atom captures this electron in its subshell 3p, becoming negative ion
Cl + e− → Cl−
3. Now all subshells are filled to capacity and both atoms are electrically charged with opposite charges, which makes them stick to each other, forming a molecule of salt.
Let's make a few conclusive statements about this process of forming molecules.
I. Atoms like their subshells to be completely filled up to a maximum of 4m−2, where m is the subshell number (subshell #1 is labeled s, subshell #2 is labeled p etc.)
II. Some atoms are ready to accept electrons to fill up their top subshell from other atoms that are willing to give up their electrons.
III. Some other atoms are ready to give up electrons from their incomplete top subshell, leaving with themselves only complete subshells, if there is a recipient atom of these extra electrons that needs them to complete its top subshell.
IV. The necessity for an atom to have its shells filled up is very strong. Atoms with incomplete top subshells are looking for partners to get into chemical combination. If there is a fit between two atoms to transfer electrons from an incomplete top subshell of one of them to incomplete top subshell of another that completes both, electrons are transferred.
V. After the transfer of electrons that completes both atoms, they become oppositely charged ions that are attracted to each other, which establishes a stable combination.
VI. The complex combinations of more than 2 atoms can also be created based on the same principle. The mechanism is a little more complex, but follows the same idea to complete top subshells of all participants.
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