Which of the following ionic compounds would be expected to have the highest lat

Question

Which of the following ionic compounds would be expected to have the highest lattice energy? A) KI B) KBr C) KCl D) KF Which compound is most likely to exist as a gas or liquid at room temperature? A) CaI_2 B) CCl_4 C) Al_4C_3 D) WC What is the general trend in ionization energy and electron affinity values? A) Both increase as one traverses a period from left to right and both increase as one descends a group. B) Both increase as one traverses a period from left to right and both decrease as one descends a group. C) Both decrease as one traverses a period from left to right and both decrease as one descends a group. D) Both decrease as one traverses a period from left to right and both increase as one descends a group.

Explanation / Answer

Q5.

highest lattice --> small metal ion, small halide

so there is a strong ionic figure, i.e. ionic = very metal +very nonmetal

note that Fluorine is pretty electrongative

so choose F

then, since K is the same for all

the strongest lattice if KF

Q6.

gas or liquid --> not ionic

so

CaI2 = ionic

CCl4 = expected to be gas/liquid

note that carbides are pretty high in melting/boiling points, so Al4C3 and WC are expected to be pretty large

so

only CCl4 will do (nonmetal + nonmetal )

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