Test 3 Q7

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Rebecca Chu 1C
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Test 3 Q7

Postby Rebecca Chu 1C » Mon Jun 11, 2018 4:56 pm

It asks to circle which compound has the highest ionic character and the compounds were KBr or NaBr. Why does KBr have a more ionic character than NaBr? I circled NaBr because I thought Na has a higher electronegativity than K so NaBr has a higher ionic character, but I got it wrong.

Chem_Mod
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Re: Test 3 Q7

Postby Chem_Mod » Mon Jun 11, 2018 5:42 pm

More ionic character is determined by greater difference in electronegativity. Br is more electronegative than all metals, so a less electronegative metal will make a more ionic bond with Br.

Andrew Evans - 1G
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Re: Test 3 Q7

Postby Andrew Evans - 1G » Mon Jun 11, 2018 6:06 pm

I thought of it as Na is smaller, so has the same charge as K, but in a smaller volume (so it has greater charge density). Since it has a greater charge density, it has greater polarizing power, which pulls on Br's electron cloud more, causing greater distortion making the bond have more covalent character. This would mean KBr would have more ionic character.

-Andrew Evans
Section 1G

Ismail 1F
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Re: Test 3 Q7

Postby Ismail 1F » Mon Jun 11, 2018 7:06 pm

It has a greater electronegativity and higher electron density which makes it more ionic.


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