Particle Physics

In order to find the number of neutrons in the atoms of an element, you must specify the isotope that you are interested in. Isotopes are specified according to their mass number. For example carbon-12 is the isotope of carbon that has a mass number of 12, and carbon-14 is the isotope of carbon that has a mass number of 14. All atoms of the same element, regardless of mass number, have the same number of protons, which is the element's atomic number. To determine the number of neutrons in an isotope, you subtract the atomic number from the mass number. For example, the atomic number of carbon is 6, which means that all carbon atoms contain 6 protons in their nuclei. So, to find the number of neutrons in a carbon-12 atom, subtract 6 from 12, and you get 6 neutrons in the atoms of carbon-12. To find the number of neutrons in a carbon-14 atom, subtract 6 from 14, and you get 8 neutrons in the atoms of carbon-14.

The neutron absorption cross section of an atom is the size of the target presented by that atom to an incoming neutron. Let's look at a couple of things and we'll get to it. Ready? Let's go.

There is a funny group of rules associated with the way an atomic nucleus reacts to an incoming neutron. It isn't necessarily like breaking a rack of billiard balls like in so many science shows. It's more like the neutron manages to press up against the nucleus and the nucleus captures it. Then what happens, happens.

One of the concepts to be considered is the energy of the incoming neutron. How fast is it going? Faster isn't necessarily better for increasing the probability of capture. It usually isn't. Another factor is the size of the target that a given nucleus presents to that neutron. We call that a neutron absorption cross section, and it's measured in barns. (Yes, like the broad side of a barn, as in hitting the broad side of a barn. And who said physicists weren't funny and couldn't make jokes!) There are tables to look this stuff up on because each given isotope of each given element has a given neutron capture cross section. That makes things challenging. And the actual cross section is different for different energies of neutrons. That ups the challenge for investigators even more.

Electrons have virtually no mass, are negatively electrically charged and are to be found orbiting an atoms nucleus in what are called electron shells.

Protons and Neutrons are to be found the the atoms nucleus and they have mass.

Neutrons have no electrical charge while Protons are positively charged. For every Proton to be found in an atom's nucleus, there is a matching electron in one of the electron shells so that overall the + and - electrical charges balance out. The number of protons in the nucleus of an atom determines what element that atom makes.

Neutrons stabilize the atom's nucleolus by separating the + charge protons and their number may vary in an atom - a variation in the number of neutrons in the nucleus with a given number of protons gives rise to atomic isotopes. Neutrons also have no charge.

Protons and Neutrons are located in the nucleus. Protons=Positive. Neutrons=no charge. Electron=E-=Negatively charge.

It would be incorrect and simplistic to say that electrons are in "orbits", because that implies a known path. It would be more correct to say that electrons are in "energy levels" or "orbitals", because we cannot know exactly where in the atom the electron is.

According to the Heisenberg Uncertainty Principle, it's impossible to know exactly where an electron is AND exactly what its velocity is. The more closely we measure one thing, the more uncertainty we add to the other.

ObJoke: The police officer pulls over an electron, and says "I clocked you at exactly 93 miles per hour!" The electron replies, "Oh, great! Now I'm COMPLETELY lost!"

So what keeps an electron within its "shell" or "probability level"? It doesn't have enough energy to go elsewhere. If the electron absorbs some energy (in the form of light) it can move to a higher energy level, or escape completely.

nonmetals are located in the right side of the periodic table. The Ionization energy(the amount of energy used to remove an electron) tends to increase from left to right across a period.It is difficult to remove the electrons from the right side because they are becoming stable

The arrows pointing in opposite directions in the orbital filling diagram represent the two electrons in the same orbital having opposite spins. According to the Pauli exclusion principle, no two electrons in an atom can have the same set of quantum numbers, so one electron must have a spin of +1/2 and the other -1/2.

The force between the nucleus and the outermost electron in a large atom is primarily governed by the attraction between the positively charged nucleus and the negatively charged electron. This force is known as the electrostatic force of attraction and is directly proportional to the product of the charges and inversely proportional to the square of the distance between the nucleus and the electron.

Quarks are fundamental particles inside protons. In the case of titanium, protons can contain a combination of up and down quarks which are the building blocks of protons. Scientists can study these quarks indirectly through high-energy scattering experiments.

Barium has 56 electrons.

A electron is one of the 3 things you need to complet a ATOM. getting back to the subject , so a electron is a thing in the ELECTRON CLOUD.

In simple, average Joe terms, string theory says that all the particles in the universe are really little "strings", rather then the conventional ball-shape they are normally thought of. Unlike the balls (or more accurately, points) which are zero-dimensional, strings are one-dimensional. This has some very interesting implications, but to explain them would evolve out stepping a "simple definition". String theory is known for uniting both the physical laws of the large (Einsteins general relativity- stars, planets, and people) and the small (quantum mechanics- subatomic particles), which were previously incompatible. Short for super sting theory, now known as M-theory. This answer explains only the very basics of string theory.

Aluminium with atomic number 13 ie 13 protons has 14 neutrons within the nucleus. So its mass number is 27. Silicon too with atomic number 14 has 14 neutrons within. Why not? Even phosphorous with atomic number 15 has 14 neutrons. So it is an isotope that too radio active isotope. So it is very important to know about the number of protons to identify the element. But number of neutrons do differ leading to the formation of isotopes.

As a start:

Electrons that are not share between atoms. covalent bonds along with pie bonds require two electrons per bond. the two electrons in the bond are shared electrons or bonding electrons.

Atoms such as oxygen and nitrogen have electrons that are not part of a bond. Oxygen is in group VI so it wants to have 6 electrons around it. it gets 2 of its electrons from bonds. the other 4 come from non bonding electrons or two pair of electrons.

Nitrogen is in group V so it only wants 5 electrons. Thus, it has three bonds and one non bonding electron pair.

The three major sub-atomic particles are : - PROTONS, ELECTRONS and NEUTRONS.

Protons are positively charged (+) and found in the nucleus of an atom.

Electrons are negatively charged (-) and found around (not IN) the nucleus of an atom.

Neutrons have no charge (o) and are found in the nucleus of an atom .

The number of protons ( and electrons) is the ATOMIC NUMBER, and the atoms position in the Periodic Table .

The number of protons equals the number of electrons ( in order to keep the charges balanced).

The Sum total of the protons and neutrons is the ATOMIC MASS/WEIGHT.

The number of neutrons can vary This gives a different atomic mass for a given element and are known as ISOTOPES.

Taking hydrogen as an example It has three isotopes.

[1/1]H (Protium) ; 1 proton . ZERO(NO) neutrons, 1 electron.

[2/1]H (deuterium); 1 proton , 1 neutron , 1 electron

[3/1]H (tritium); 1 proton, 2 neutrons, 1 electron . (This isotope is radio-active)

[1/1] protium is the most common isotope of hydrogen , and what is normally thought of as hydrogen.

[2/1] deuterium is sometimes named as 'heavy hydrogen'. It is not a very common isotope.

[3/1] tritium is sometimes named as 'super-heavy hydrogen'. It is a rare isotope ,and because of its radio-activity only found in labs.

However, as mentioned above for all isotopes the protons and neutrons are in the nucleus of the atom, and collectively they are named as 'nucleons'. The electrons are found outside the nucleus.

These 'rules' apply to all elements.

Classical they will emit electromagnetic waves (light and radio waves).

Quantum effects might limit this since if the electrons are in the ground state (or all lower states are occupied) they can not emit any photons (quanta of electromagnetic waves).

The current view of the atom describes the location of electrons as existing in electron clouds or orbitals around the nucleus. Electrons do not follow a specific path but are rather found within a specific probability distribution around the nucleus. This model is known as the quantum mechanical model.

The electron, the neutron and the proton are the building blocks of the atom. And of the three, the electron is far and away the lightest. The neutron is slightly heavier than the proton, and either particle is over 1800 times more massive than our little electron.

Protons are positively charged.

Neutrons are neutrally charged.

Electrons are negatively charged.

Therefore if an atom is positively charged, it could have any amount of protons or neutrons, one does not need to be more than the other. However we can say it will definitely have more protons than electrons.

Fluorine require only one electron to fill its outer shell. Hence it has the greatest tendency to gain electrons than Al, Rb and I.

The existence of antimatter was first predicted by physicist Paul Dirac in 1928 as a consequence of his Dirac equation, which unified quantum mechanics and special relativity. The first observation of antimatter particles, specifically positrons, was made by physicist Carl D. Anderson in 1932 while studying cosmic rays.

The muon (from the letter mu (μ)--used to represent it) is an elementary particle with negative electric charge and a spin of 1/2. It has a mean lifetime of 2.2μs, longer than any other unstable lepton, meson, or baryon except for the neutron. Together with the electron, the tau, and the neutrinos, it is classified as a lepton. Like all fundamental particles, the muon has an antimatter partner of opposite charge but equal mass and spin: the antimuon, also called a positive muon. Muons are denoted by μ− and antimuons by μ+. For historical reasons, muons are sometimes referred to as mu mesons, even though they are not classified as mesons by modern particle physicists. Muons have a mass of 105.7 MeV/c2, which is 206.7 times the electron mass. Since their interactions are very similar to those of the electron, a muon can be thought of as a much heavier version of the electron. Due to their greater mass, muons do not emit as much bremsstrahlung radiation; consequently, they are highly penetrating, much more so than electrons. Muons have a life of about 2 nanoseconds.

The complete electron configuration for the chromium(III) ion is 1s22s22p63s23p64s03d3.

The proton is a positive subatomic particle, but the neutron is not. The neutron has a neutral charge or zero charge.

90 in ground state