Test 3. Question 7.

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Marina Souliman 1K
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Test 3. Question 7.

Postby Marina Souliman 1K » Sat Jun 02, 2018 4:40 pm

Why does CaCl2 have greater ionic character than MgCl2? What determines which one has greater ionic character?

sharonvivianv
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Joined: Fri Apr 06, 2018 11:05 am

Re: Test 3. Question 7.

Postby sharonvivianv » Sat Jun 02, 2018 4:59 pm

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.

Mohamad Farhat 1L
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Re: Test 3. Question 7.

Postby Mohamad Farhat 1L » Sat Jun 02, 2018 5:20 pm

cacl2 mgcl2

3.16-1.00 3.16-1.31
2.16 en. 1.85 en

cacl2 has greater ionic character

Andre-1H
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Re: Test 3. Question 7.

Postby Andre-1H » Sat Jun 02, 2018 8:54 pm

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.

Erin Li 1K
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Re: Test 3. Question 7.

Postby Erin Li 1K » Sat Jun 02, 2018 8:55 pm

Differences in electronegavity determine the ionic character. the higher the difference in electronegativity, the greater the ionic character

Avery Zuelch 1D
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Re: Test 3. Question 7.

Postby Avery Zuelch 1D » Sun Oct 28, 2018 10:12 pm

The difference in the electro negativity defines the ionic character !!

Ricardo Martin 1J
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Re: Test 3. Question 7.

Postby Ricardo Martin 1J » Thu Nov 01, 2018 10:06 pm

Difference in electronegativity defines ionic character.


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