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.)
"Electron cloud" is the name given to the electrons which surrounds the atomic nucleus.
Nucleus exerts a force on every electron revolving around it. This force is inversely proportional to the distance between the nucleus and the electron. Therefore the electrons in outermost orbit (or shell) have the least nucleic forceacting upon them in comparison to the inner electrons. Therefore they are the most easily removable electrons.They are called valence electrons.
As alkali metals increase in size, the distance of the outermost electrons from the nucleus increases. The attraction between the electrons and the nucleus is electrostatic, and it is a fundamental property of electrostatic attractions that the attraction decreases with increasing distance between the attracting charges. Another way of describing this is that the attractive force is partially "screened" by the inner electrons between the outermost electrons and the nucleus.
Electrons that are further away from the nucleus have a greater attraction because the positive and negative charges are stronger than innermost electrons
The atomic radius decreases as electrons are added to a shell because the increasing number of electrons increases the electrostatic force of attraction between the electrons and the nucleus, pulling the electrons closer to the nucleus and reducing the atomic radius.
No. Electrons are located in the electron cloud surrounding the nucleus.
Electrons in the outermost electron shell have the most energy in an atom. The energy of an electron increases as it moves further away from the nucleus. Electrons in the innermost shell have the least energy, while electrons in the nucleus have the highest energy due to their proximity to the protons.
Electrons farthest from nucleus are valence electrons. They are present in outermost orbit.
"Electron cloud" is the name given to the electrons which surrounds the atomic nucleus.
The strength of attraction between a nucleus and the outermost electrons is determined by the electric charge of the nucleus (protons) and the distance between the nucleus and the electrons. This attraction is the basis for the force that holds atoms together and is essential for the stability of matter.
The force of attraction between the atom's nucleus and its valence electrons are the least. Hence valence electrons are lost easily.
Nucleus exerts a force on every electron revolving around it. This force is inversely proportional to the distance between the nucleus and the electron. Therefore the electrons in outermost orbit (or shell) have the least nucleic forceacting upon them in comparison to the inner electrons. Therefore they are the most easily removable electrons.They are called valence electrons.
No, the farthest electrons are at the highest energy level.No, the farthest electrons are at the highest energy level.No, the farthest electrons are at the highest energy level.No, the farthest electrons are at the highest energy level.
Valence electrons are present in outermost shell. They are at far distance from nucleus.
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.
As alkali metals increase in size, the distance of the outermost electrons from the nucleus increases. The attraction between the electrons and the nucleus is electrostatic, and it is a fundamental property of electrostatic attractions that the attraction decreases with increasing distance between the attracting charges. Another way of describing this is that the attractive force is partially "screened" by the inner electrons between the outermost electrons and the nucleus.
Electrostatic forces between the nucleus and outermost electrons exist due to the attraction between opposite charges. The nucleus carries a positive charge, while electrons carry a negative charge. This attraction keeps the electrons in orbit around the nucleus, creating stability within the atom.