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Do attractive forces have less hold on electrons farther from the nucleus?
Wiki User
∙ 14y ago
Yes, as electrons get farther from the atomic nucleus they are less attracted to that nucleus, which is exactly what you would expect on the basis of Coulomb's Law, F=q1q2/r2 as the radius of the orbit increases the attractive force becomes decreased.
Wiki User
∙ 14y ago
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What is the attraction and repulsion forces between subatomic particles?
attraction forces between the electrons of one atom and the nucleus of the other atom are balanced by the repulsive force caused by the two + charged nuclei as they are forced together~attractive forces have a little attraction for the atoms.
A main difference between gravitational and electric forces is that electrical forces?
electric forces can be attractive or repulsive, whereas gravitational forces are only attractive.
When an atom is stable what is happening with the attractive and repulsive forces in the nucleus?
Inside an atom's nucleus there is a neutron, which has no charge, therefore no attractive or repulsive forces. The proton carries a positive charge, though, and repels the negative charge of the electron particle which exists somewhere outside of the nucleus.I'm yet of the old technology which thinks that protons and electron attract. Of course, that doesn't explain why the electron don't crash into the proton, but that's another story.
Is the nuclear force a force of attraction or repulsion or both?
It is only attractive in nature. I am not sure which nuclear force you talk about. Electrical forces of the nucleus are repulsive to the positively charged. There are "strong forces" and the like which are attractive.
Electrical and gravitational forces follow similar equations with one main difference?
The main difference in the equations is that electrical forces can be attractive or repulsive, while gravitational forces are always attractive.
What is the attraction and repulsion forces between subatomic particles?
attraction forces between the electrons of one atom and the nucleus of the other atom are balanced by the repulsive force caused by the two + charged nuclei as they are forced together~attractive forces have a little attraction for the atoms.
In same group of elements ionization energy tends to decrease with increasing atomic number decreasing size of atom increasing forces of attraction or outer electrons being farther from the nucleus?
kolorita
What keeps electrons in the space around a nucleus?
The electrostatic forces between the protons and the electrons keep it in orbit.
Why the protons in the nucleus have less repulsion than electron?
Because they are farther away from the nucleus than protons, and they have more freedom as in where to move, because they fly around the nucleus in no particular order.
What are the properties of the strong force?
Well scientifically speaking the strong force causes protons and neutrons to be attracted to each other. Attractive forces between the protons and neutrons keeps the nucleus together. This is one of the four basic forces in nature.But when the protons and neutrons start to move farther apart the strong force gets weaker, and weaker the farther they move and will be repelled.
Why does not a heavy atom eject electrons from its shells and instead emits alpha and beta particles?
The reason a heavy atom breaks apart is, precisely, because of an instability in its nucleus. Note that the forces within the nucleus are several orders of magnitude stronger than the forces between the nucleus and the electrons.
Does the dispersion force increase down the halogens?
Yes, dipersion forces increase moving down the halogens, ie from fluorine to chlorine, then bromine, and then iodine. This is a general trend in most groups due to increasing numbers of electrons farther from the nucleus. However, it is especially evident in the halogens. Fluorine is the least polarizable element because of it's electronegativity and the proximty of the electrons to the nucleus (there is a high effective nuclear charge). In iodine, the electronegativity is lower and the electrons are father from the nucleus. Thus, it has much higher dispersion forces caused by temporary dipoles. The trend is true for the rest of the halogens as well.
What is responsible for keeping electrons in orbit around the nucleus?
The positive charge of some components in the nucleus.
What are the attractive forces of plasma?
The attractive forces are electrical forces between opposing charges.
What electron forces exist between the nucleus and the outermost electrons?
The coulomb force is the dominant force between the electrons of an atom and the nucleus. It is the standard force of attraction between positive and negative charges. (Of course, the electrons also interact with each other also through the repulsive coulomb force expected of like charges.) The forces between the nucleus and the electrons is the same basic coulomb force fo all electrons, inner electrons or outer electrons or any electrons. (Of course, the type of force is the same but the strength of the force varies with distance being weaker for more distant electrons.) Essentially all of chemistry is determined by this simple inverse square force of attraction and repulsion. Other forces such as the force of gravity or the more exotic nuclear forces and electroweak interactions are so small as to be irrelevant except in special circumstances.)
Explain what electric forces between oppositely charged electrons and protons have to do with chemical reactions?
When metals react, they lose electronsto become stable and sometimes form a compound.Now, electrons are negatively charged, and the nucleus, due to the presence of protons, is positively charged.As the atom of the metalgets bigger in size, the valency shell, which holds the valency electron, becomes farther away from the nucleus.The attraction between the valency electron (on the last shell) and the nucleus decreases, so the atom of this type of metal is considered to be reactive as the electron becomes easily lost due to weak forces pulling it towards the nucleus.
What are the attractive and repulsive forces involved in a covalent bond and how do their total strengths compare?
when a bond is formed then the forces of attraction are dominant to the forces of repulsion.for a chemical bond to be formed this is compulsory.
