Question

1. fluorine (f) is much more electronegative than hydrogen (h). in a bond between h and f, which atom will the electrons be more strongly attracted to?

fluorine, because it has more electron shells.
fluorine, because it has a higher electronegativity.
hydrogen, because it has a lower electronegativity.
hydrogen, because it has only one electron shell.

1. which of the following ions has the smallest radius? *

f -
k +
cl -
rb +

Explanation:

Question 7

Electronegativity is the ability of an atom to attract electrons in a chemical bond. Since fluorine (F) has a higher electronegativity than hydrogen (H), it will attract the bonding electrons more strongly. The first option is incorrect because F has fewer electron shells than H (F has 2, H has 1). The third and fourth options are incorrect as lower electronegativity or one electron shell do not lead to stronger electron attraction.

To determine the ion with the smallest radius, we analyze electron configurations and nuclear charge. \( \text{F}^- \) has 10 electrons (\( 1s^2 2s^2 2p^6 \)), \( \text{K}^+ \) has 18 electrons (\( 1s^2 2s^2 2p^6 3s^2 3p^6 \)), \( \text{Cl}^- \) has 18 electrons (\( 1s^2 2s^2 2p^6 3s^2 3p^6 \)), and \( \text{Rb}^+ \) has 36 electrons. For isoelectronic species (or comparing across periods), smaller ionic radius is associated with higher nuclear charge and fewer electron shells. \( \text{F}^- \) has the fewest electron shells (2) and, among the options, the smallest overall size. \( \text{K}^+ \) and \( \text{Cl}^- \) have 3 electron shells, and \( \text{Rb}^+ \) has 4, so they are larger.

Answer:

Fluorine, because it has a higher electronegativity.

Question 8