Frequent question: Why does electron attraction increase across a period?


Does electron electron repulsion increase across a period?

As you move across a period the number of electrons from one element to the next increases by one. The electron is added in the same valence shell which increases electron repulsion which slightly increases the atomic radius but this is a very small.

What happens to the attraction between protons and electrons as you move across a period?

Within a period, protons are added to the nucleus as electrons are being added to the same principal energy level. These electrons are gradually pulled closer to the nucleus because of its increased positive charge. Since the force of attraction between nuclei and electrons increases, the size of the atoms decreases.

Does attraction increase across a period?

Across a period, effective nuclear charge increases as electron shielding remains constant. A higher effective nuclear charge causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius.

How does electron repulsion increase?

ii) The repulsion between electron pairs increases with increase in electronegativity of central atom and hence the bond angle increases. … On smaller central atoms the bond pairs are closer and hence tend to move away from each other so as to minimize repulsion.

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Why the attractive forces of the nucleus on the valence electrons becomes greater as you move left to right across the table?

Therefore, electron affinity decreases. Moving from left to right across a period, atoms become smaller as the forces of attraction become stronger. This causes the electron to move closer to the nucleus, thus increasing the electron affinity from left to right across a period.

What makes a valence electron more attracted to the nucleus?

the closer an electron is to the nucleus, the more strongly it is attracted. the more protons in a nucleus, the more strongly an electron is attracted.

What is a Zeff?

eff. Effective nuclear charge, Zeff: the net positive charge attracting an electron in an atom. An approximation to this net charge is. Zeff(effective nuclear charge) = Z(actual nuclear charge) – Zcore(core electrons) The core electrons are in subshell between the electron in question and the nucleus.