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How do you compare the force of attraction from the nucleus to the outer level of electrons?
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Why do force of attraction between nucleus and electrons decrease in alkali metal as increase in size?
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.
Why are valence electrons easier to remove from an atom than core electrons?
the force of attraction between then nucleus and the valence electrons is less than that between the nucleus and the core electrons
What are the advantages of Rutherford's atomic model?
The electrostatic force of attraction between electrons and nucleus was likened to the gravitational force of attraction between the revolving planets and the Sun.
Why are electrons attracted to the nucleus?
Put simply, a nucleus is made up of protons and neutrons, protons have a positive charge, this attracts the negative charge of the electron.
What is the energy called that attracts the electrons to the nucleus of an atom?
binding energy The attraction force of the positively charged protons in the nucleus binds (holds secure) the negatively charged electrons near the nucleus.
What force holds electrons and protons in the atom?
Electro-static attraction between a positively charged nucleus and negatively charged electrons.
What energy relations exists within the atom as electrons revolve about the positive nucleus?
there is a force of attraction between the positive nucleus and each negative electrons, and this force is counterbalanced by one that is determined by the orbital motion of the electron.
What keeps electrons confined in the space surrounding the nucleus?
attraction to the positively charged nucleus
What makes the particles of atom orbit?
The force that keeps them in orbit is the electrostatic attraction between the atom's nucleus and the electrons.
What keeps electrons close to te nucleus?
Electrons are not shot off because the e- (which are negative) have an electromagnetic force hold with the protons (positive) in the centre. This attraction is also because of gravity and the force of attraction (as protons/neutrons are significantly heavier than electrons) it creates.
What is the force thea holds an electron to an atom?
The electromagnetic force (protons are positive and electrons are negative, so they attract), which is manifested into Coulomb's force of attraction. The reason that electrons will not fall into the nucleus is due to the electron's energy; it is moving fast enough to not collide with the nucleus.
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.)
