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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: hupnosis on January 21, 2016, 08:43:22 AM

Title: Stable ionic compounds
Post by: hupnosis on January 21, 2016, 08:43:22 AM

which of the following is most likely to be a stable ionic compound?

a) Rb20
b) BaCl
c) Na2N

I did a lewis dot diagrahm and got these resuslts
a) one oxygen electron is unpaired
b) 2 of the 3 Ba electrons are unpaired
c) one N electron is unpaired

which one of these are the most stable and how did you come to that conclusion?

thanks for the help in advance :)

Title: Re: Stable ionic compounds
Post by: Hunter2 on January 21, 2016, 10:05:12 AM

The first two answers are wrong, the only existing compound is Rb₂O Rubidiumoxide. Each Rubidium give his s-electron to one p-Orbital of the Oxygen.
Barium has two s- electrons, one would be not paired. In c the nitrogen has one electron not paired, so these compounds do not exist under normal conditions.

Title: Re: Stable ionic compounds
Post by: AWK on January 21, 2016, 10:21:04 AM

Compound b and c rather do not exist. Expected printing error (BaCl₂ or Na₃N or Na₂NH)?