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You look at the differences in electronegativity. In the sixth edition textbook, figure 3.12 shows most of the values you'll need (and all for this problem). Even if you aren't looking at the exact values, you can estimate it using electronegativity trends. Electronegativity increases across a period and decreases down a group. You can use this knowledge to see which bonds are more ionic: for example: Iodine and Chlorine are both in the same group (halogens), but I is farther down the group than Cl, so it is less electronegative than Cl and thus closer in electronegativity to H. Therefore, the bond between Cl and H is more ionic.
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