Question

1. electron affinity is the tendency to:

a) gain an electron
b) lose an electron
c) share electrons
d) make bonds

1. electron affinity is highest for:

a) f
b) cl
c) br
d) i

1. which has the highest electronegativity in period 2?

a) be
b) b
c) c
d) f

Explanation:

Question 13

Electron affinity is defined as the energy change when an atom gains an electron to form a negative ion. So the tendency related to electron affinity is to gain an electron. Option a matches this definition, while losing electrons is related to ionization energy, sharing electrons is about covalent bonding, and making bonds is a broader concept not specific to electron affinity.

Among halogens (F, Cl, Br, I), chlorine (Cl) has the highest electron affinity. Fluorine has a smaller atomic size, so electron - electron repulsion in its valence shell is relatively high, which reduces its electron affinity compared to chlorine. As we go down the group (from Cl to Br to I), atomic size increases, and electron affinity generally decreases.

In a period, electronegativity generally increases from left to right. In Period 2, the elements are Be, B, C, F (and others). As we move from Be (Group 2) to B (Group 13), to C (Group 14), to F (Group 17), electronegativity increases. Fluorine is the right - most among these options in Period 2, so it has the highest electronegativity.

Answer:

a) Gain an electron

Question 14