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Which has more potential energy an electron close to an atomic nucleus or one far from an atomic nucleus?
An electron far from an atomic nucleus has more potential energy compared to one close to the nucleus. This is because the farther the electron is from the nucleus, the higher its potential energy due to the increased distance from the attraction of the positively charged nucleus.
Why do you suppose that an energy level close to the nucleus can hold fewer electrons than one farther away from the nucleus?
Energy levels close to the nucleus have lower energy, which means electrons are more tightly bound and experience stronger electrostatic attraction to the nucleus. This results in a limited capacity for electrons at lower energy levels. As electrons move to higher energy levels, they are farther from the nucleus and experience weaker attraction, allowing for higher electron capacity.
Why does ionization energy decrease down the family?
You question is not very clearly stated but I think I know what you are asking. As you go down the column of any family of elements in the periodic table, you move to increasingly heavier and larger atoms. Their outer electrons are therefore farther from the nucleus, and even though the nucleus is larger and has a larger positive charge, the increased distance is the predominant influence, making the outermost electrons less tightly bound, and therefore more easily ionized, with a lower ionization energy.
Why not electron collapse into the nucleus?
Electrons inhabit a probability cloud around the nucleus, which is related to their possible velocities. The closer the cloud is to the nucleus, the higher the kinetic energy, which allows it to overcome the electromagnetic attraction of the protons.
Is the valence electron farthest or closest to the nucleus?
No. By definition, valence electrons are the furthest electrons from the nucleus in the atom. They are the electrons most easily removed from (or added to) the atom to create ions. A loophole to this answer might be to say that hydrogen and helium only have 1 and 2 electrons respectively so their valence electrons are close. That's a matter of perspective, as no electrons are really "close" to the nucleus to begin with. A typical comparison is to imagine a grape seed in the middle of a football stadium. The grape seed represents the nucleus, and an electron would be a speck of dust on the outside of the stadium. No. By definition, valence electrons are the furthest electrons from the nucleus in the atom. They are the electrons most easily removed from (or added to) the atom to create ions. A loophole to this answer might be to say that hydrogen and helium only have 1 and 2 electrons respectively so their valence electrons are close. That's a matter of perspective, as no electrons are really "close" to the nucleus to begin with. A typical comparison is to imagine a grape seed in the middle of a football stadium. The grape seed represents the nucleus, and an electron would be a speck of dust on the outside of the stadium.
Which has more potential energy an electron close to an atomic nucleus or one far from an atomic nucleus?
An electron far from an atomic nucleus has more potential energy compared to one close to the nucleus. This is because the farther the electron is from the nucleus, the higher its potential energy due to the increased distance from the attraction of the positively charged nucleus.
Is this statement correct atoms are made up of nucleus and electrons composed of protons whose number is called the atomic number and neutrons whose numbers added together make the mass number?
It's close, but an atom is made of a nucleus and electrons. The nucleus is made of protons and neutrons. The number of protons equals the atomic number of the element, and the atomic mass is the number of protons plus neutrons.
How do you know protons are found in the nucleus?
The atomic number tells you how many protons are in the atomic nucleus. The atomic mass is the amount of protons plus the amount of neutrons in the atomic nucleus. So if you take the atomic number and subtract it from the atomic mass, it will give you the number of neutrons in the atomic nucleus.
What do you get if you add one neutron to a hydrogen nucleus?
If you add the number of protons and neutrons in an atomic nucleus, you get the number of nucleons. This is usually a good approximation to the atomic mass in amu, since both protons and neutrons have a mass that's pretty close to one amu. The number will be slightly off, because electrons contribute as well, protons and neutrons don't have exactly the same mass, and there's something called the atomic mass defect that has to do with the binding energy of the nucleus, but it should be fairly close.
In an atom an electron that is close to the nucleus is on the highest enegry level?
No. The greater distance from the nucleus the more energy an electron has.
Do electrons move slow or fast around the nucleus?
Electrons move fast around the nucleus at speeds close to the speed of light. The exact speed of an electron is determined by its energy level and its distance from the nucleus.
What holds electrons in their shells?
The electrons "orbit" the nucleus of an atom. They do so because they are attracted to the positive charge of the protons inside the nucleus. They do not usually leave the atom because of this attraction, and do not usually fall into the nucleus because they are moving.
What is closer to nucleus the stronger the attractive force?
When it is close to the nucleus because the postively charged protons attract the negatively charged electrons
Why do you suppose that an energy level close to the nucleus can hold fewer electrons than one farther away from the nucleus?
Energy levels close to the nucleus have lower energy, which means electrons are more tightly bound and experience stronger electrostatic attraction to the nucleus. This results in a limited capacity for electrons at lower energy levels. As electrons move to higher energy levels, they are farther from the nucleus and experience weaker attraction, allowing for higher electron capacity.
Do electron like to be close to each other?
As per modern atomic model, the neutrons would be packed along with protons in the nucleus because of nuclear force. The electrons are considered to be revolving around the nucleus. So electrons are not packed close to the neutrons.
Why does ionization energy decrease down the family?
You question is not very clearly stated but I think I know what you are asking. As you go down the column of any family of elements in the periodic table, you move to increasingly heavier and larger atoms. Their outer electrons are therefore farther from the nucleus, and even though the nucleus is larger and has a larger positive charge, the increased distance is the predominant influence, making the outermost electrons less tightly bound, and therefore more easily ionized, with a lower ionization energy.
Subatomic particles are closest in mass?
Proton and neutron (components of the atomic nucleus) have masses very close.
