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This is referencing the concept of bond length that Dr. Lavelle explained during Friday's lecture using the example of the strong acids: HF > HCl > HB > HI. Bond strength decreases as atomic radius of increases because the atoms are farther apart and easier to pull apart. Thus, among CF4, CCl4, CBr4, CF4 would be the strongest because F is the smallest atom and can have a shorter bond length than the others.
In order to determine the order of weakest bonds it is important to identify which are the larger atoms (ionic radius=decrease left to right and increase top to bottom) because the larger atoms have a larger distance therefore longer bond length which is weaker and easier to break.
In order to answer this question, we need to look at atomic trends. F, Cl, and Br are all in the same group, but different periods. As you move down a group, atomic radius increases. Why is this important? Increasing atomic radius means increasing bond length. Longer bonds typically require less energy to break. So, we can infer that CF4 will have the strongest CX bond because F has the smallest atomic radius.
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