Learning Module 16: Periodic Trends with Exceptions

Which of the following has the highest ionization energy?

Cl

Of the following, which would you expect to have the smallest electron affinity?

P

Rank the following from least to greatest electron affinity: silicon (Si), phosphorous (P), sulfur (S).

P < Si < S

Rank the following from least to greatest ionization energy: silicon (Si), phosphorous (P), sulfur (S).

Si < S < P

Why is it harder to remove an electron from fluorine than from carbon, or, to put it another way, why are the valence electrons of fluorine more strongly bound than those of carbon?

The valence electrons of both fluorine and carbon are found at about the same distance from their respective nuclei but the greater positive charge of the fluorine nucleus attracts its valence electrons more strongly.

The second ionization energy for an atom is always higher than the first ionization energy.

True

The energy needed to remove electrons from an atom is called -

ionization energy.

Electron affinity and ionization energy do not rigorously adhere to the periodic trends because

filled and half filled subshell stability.