ionic character

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giareyes_2B
Posts: 20
Joined: Wed Sep 21, 2016 2:58 pm

ionic character

Postby giareyes_2B » Sat Dec 03, 2016 10:50 pm

How do you determine which compound has bonds with greater ionic character? In the 2015 final Q3E, it asks between CO2 and CS2. I know that the greater the difference in electronegativity = greater ionic character, but isn't there a greater difference in CS2 instead of CO2?

Frankie Escobedo 3E
Posts: 16
Joined: Fri Sep 30, 2016 3:02 am

Re: ionic character

Postby Frankie Escobedo 3E » Sat Dec 03, 2016 11:03 pm

Oxygen is more electronegative than Sulfur since the trend increases up a period and to the right on the groups. Because Oxygen has a higher electronegativity, the difference with Carbon will be greater; therefore, CO2 has a greater ionic character.

BlakeMillar4J
Posts: 11
Joined: Wed Sep 21, 2016 2:56 pm

Re: ionic character

Postby BlakeMillar4J » Sat Dec 03, 2016 11:18 pm

As Group number increases, so does elecronegativity. For elements in the same group, as their atomic radius increases (going down further on the periodic table), their ability to attract electrons decreases. So the top-right of the periodic table are where the most electronegative elements are (Oxygen, Fluorine, etc).


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