0
Add your answer:
Earn +20 pts
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?
Ionization energy tends to decrease down a group in the periodic table because the outermost electrons are further away from the nucleus, experiencing weaker attraction. This makes it easier to remove them, requiring less energy.
Why not electron collapse into the nucleus?
Electrons do not collapse into the nucleus due to the principles of quantum mechanics. Electrons occupy specific energy levels around the nucleus, and there are restrictions on how close an electron can get to the nucleus based on these energy levels. Additionally, the repulsive force between electrons and the nucleus prevents them from collapsing into it.
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?
Yes, the statement is correct. Atoms are composed of a nucleus containing protons and neutrons, with electrons orbiting around the nucleus. The atomic number is the number of protons in the nucleus, while the mass number is the sum of the protons and neutrons in the nucleus.
How do you know protons are found in the nucleus?
Protons are found in the nucleus of an atom because they carry a positive charge, which is attracted to the negatively charged electrons orbiting around the nucleus. The presence of protons in the nucleus is essential for maintaining the overall positive charge of the nucleus and the stability of the atom.
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, electrons close to the nucleus have lower energy levels. Electrons on higher energy levels are located farther away from the nucleus.
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?
Electrons are held in their energy levels, or shells, by the attractive force between the positively charged nucleus and the negatively charged electrons. This force, known as electrostatic attraction, keeps electrons in orbit around the nucleus.
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?
Electrons do not like to be close to each other because they are all negatively charged. Like charges repel each other, leading to electron-electron repulsion. This is why electrons tend to spread out in an atom rather than clumping together.
Why does ionization energy decrease down the family?
Ionization energy tends to decrease down a group in the periodic table because the outermost electrons are further away from the nucleus, experiencing weaker attraction. This makes it easier to remove them, requiring less energy.
What is the approximate effective nuclear charge for a valence electron in krypton?
The approximate effective nuclear charge for a valence electron in krypton is close to +8. This is because the atomic number of krypton is 36, and the core electrons shield some of the positive charge from the nucleus felt by the valence electrons.
