FINAL EXAM 2013 Q3C

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504410473
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Joined: Fri Sep 26, 2014 2:02 pm

FINAL EXAM 2013 Q3C

Postby 504410473 » Wed Dec 10, 2014 9:23 pm

The question asks for which compound has the least covalent character amongst these compounds: AgI, AgCl, AgF, AlCl3, BeCl2

I know you have to look at which is more ionic bond but how do u exactly do that?

Astred 1D
Posts: 15
Joined: Fri Sep 26, 2014 2:02 pm

Re: FINAL EXAM 2013 Q3C

Postby Astred 1D » Thu Dec 11, 2014 12:56 am

My best suggestion is to look at how far away the elements are from each other in the periodic table, therefore looking at the electronegativity difference. Fluorine is furthest from Ag, and you also know that Fluorine is very electronegative.

Nikolina Walas-3J
Posts: 19
Joined: Fri Sep 26, 2014 2:02 pm

Re: FINAL EXAM 2013 Q3C

Postby Nikolina Walas-3J » Thu Dec 11, 2014 2:26 pm

why wouldn't it be BeCl2 wouldn't the Be give up its two electrons for the two Cl and both would become ions?2

Grace Hubrig 4C
Posts: 4
Joined: Fri Sep 26, 2014 2:02 pm

Re: FINAL EXAM 2013 Q3C

Postby Grace Hubrig 4C » Thu Dec 11, 2014 6:35 pm

In order to determine which compound has the bonds with the least covalent character you look at which has the most ionic characteristics. A covalent bond has ionic characteristics when the electrons are not shared equally, which occurs when there is an electronegativity difference between the atoms in the compound (since electronegativity is the electron pulling power). The greater the electronegativity difference is, the more ionic the bond will be. Since electronegativity is based on the distance between the 2 elements on the periodic table you have to look at how far apart the elements in the compounds are. Fluorine and Silver are farther apart (with 3 rows and 6 columns separating them) than Beryllium and Chlorine (where only one row separates them).


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