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Test 3. Question 7.

Posted: Sat Jun 02, 2018 4:40 pm
by Marina Souliman 1K
Why does CaCl2 have greater ionic character than MgCl2? What determines which one has greater ionic character?

Re: Test 3. Question 7.

Posted: Sat Jun 02, 2018 4:59 pm
by sharonvivianv
The difference in electronegativity determines ionic character. If you remember the trend of electronegativity, it increases going up and increases going across.
With that in mind, you notice that Mg is higher in the periodic table than Ca so you can assume that Mg is more electronegative than Ca which would make the difference of electronegativity greater in CaCl2 than MgCl2. Therefore, CaCl2 has greater ionic character.

Re: Test 3. Question 7.

Posted: Sat Jun 02, 2018 5:20 pm
by Mohamad Farhat 1L
cacl2 mgcl2

3.16-1.00 3.16-1.31
2.16 en. 1.85 en

cacl2 has greater ionic character

Re: Test 3. Question 7.

Posted: Sat Jun 02, 2018 8:54 pm
by Andre-1H
I think about ionic and covalent character as how much they share electrons or how much they keep them to themselves. Bonds where elements share electrons more (less difference in electronegativity) have more covalent character, whereas a higher difference in electronegativity yields a bond with more ionic character. So for determining electronegativity differences I just use the trends we learned in class.

Re: Test 3. Question 7.

Posted: Sat Jun 02, 2018 8:55 pm
by Erin Li 1K
Differences in electronegavity determine the ionic character. the higher the difference in electronegativity, the greater the ionic character

Re: Test 3. Question 7.

Posted: Sun Oct 28, 2018 10:12 pm
by Avery Zuelch 1D
The difference in the electro negativity defines the ionic character !!

Re: Test 3. Question 7.

Posted: Thu Nov 01, 2018 10:06 pm
by Ricardo Martin 1J
Difference in electronegativity defines ionic character.