HW 3.77

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Jane Burgan 1C
Posts: 73
Joined: Fri Sep 28, 2018 12:15 am

HW 3.77

Postby Jane Burgan 1C » Thu Nov 08, 2018 7:19 pm

For each pair, determine which compound has bonds with greater ionic character: (a) HCl or HI; (b) CH4 or CF4;
(c) CO2 or CS2.

How do you tell which compound has greater ionic character?

Bingcui Guo
Posts: 30
Joined: Fri Sep 28, 2018 12:19 am

Re: HW 3.77

Postby Bingcui Guo » Thu Nov 08, 2018 7:34 pm

You can decide by calculating the difference in each element's electronegativity. So the answer should be HCl, CF4, and CO2.

megansardina2G
Posts: 61
Joined: Fri Sep 28, 2018 12:23 am
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Re: HW 3.77

Postby megansardina2G » Thu Nov 08, 2018 7:45 pm

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.

John_Richey_4A
Posts: 69
Joined: Fri Sep 28, 2018 12:27 am

Re: HW 3.77

Postby John_Richey_4A » Fri Nov 09, 2018 10:11 am

Just look up which has a higher and lower electronegativity, and if they have a large difference, it's ionic.

Miriam Sheetz 2B
Posts: 64
Joined: Fri Sep 28, 2018 12:25 am

Re: HW 3.77

Postby Miriam Sheetz 2B » Fri Nov 09, 2018 2:13 pm

The greater the electronegativity difference, the greater the ionic character.


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