How does the size of an atom affect its ability to attract additional electrons?

How do you think the size of an atom will affect its ability to attract additional electrons?

How do you think an atom’s size will affect its ability to hold on to its valence electrons? Why? The larger the atom is and it’s atomic radius is, the less the ionization energy will be.

How does atomic size affect electron affinity?

The smaller the atom is, the closer the outermost shell is; therefore, it is a stronger attraction between the nucleus and the incoming electron. That means the electron affinity is higher for smaller atoms.

Do smaller atoms have more electrons?

An orbital of any type will get smaller as the effective nuclear charge gets bigger, because the attraction to the nucleus is greater. As you go down the periodic table, usually atoms get bigger because n gets bigger (there are electrons in higher shells). … The more electrons you take off, the smaller it gets.

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What happens to the size of atoms as you go across a row from left to right?

Experiments have shown that the first case is what happens: the increase in nuclear charge overcomes the repulsion between the additional electrons in the valence level. Therefore, the size of atoms decreases as one moves across a period from left to right in the periodic table.

Why does electron affinity decrease with increase in size?

An increase in atomic size leads to a decrease in electron affinity because the incoming electron is added further away from the nucleus, i.e. on a higher energy level. … When you add more protons to the nucleus, it will attract electrons more.

How does electron affinity depend on size?

It is found that the smaller the size of an atom is, the closer the outermost shell is. And therefore, there is a stronger force of attraction found in between the electron and the nucleus. Which means that for smaller atoms the electron affinity is higher.

When the atomic radius increases the electron affinity?

Electron affinity increases from left to right within a period. This is caused by the decrease in atomic radius. Electron affinity decreases from top to bottom within a group. This is caused by the increase in atomic radius.

Do bigger atoms attract more electrons?

An atom’s electronegativity is affected by both its atomic number and the size of the atom. The higher its electronegativity, the more an element attracts electrons. … The nuclear charge is important because the more protons an atom has, the more “pull” it will have on negative electrons.

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Why does the size of the atom increases down the group?

The growth of nuclear charge pulls more intensely the electrons, pulling them closer to the nucleus. … The number of energy levels (n) increases in a group downwards, since there is a larger distance between the nucleus and the outermost orbital. This results in an atomic radius that is greater.

Which effect on atomic size is more significant?

Atomic size increases as you move down a period because the electrons are added to higher principal energy levels. This enlarging effect is greater than the shrinking effect caused by increasing nuclear charge.