Which of the following pairs of elements would be Least likely to form a compound by ionic bonding?

Question

Which of the following pairs of elements is least likely to form a compound through ionic bonding?

Na and S
Al and F
Mg and Br
Cs and O
C and N

Na and S are ionic because Na has an electronegativity of 0.9 and S has an electronegativity of 2.5, resulting in a difference of 1.6. Al and F, however, are both nonmetals and do not form an ionic bond. Mg and Br are also ionic, with an electronegativity difference of 1.6. Cs and O form an ionic bond, and the electronegativity difference here is 2.8. C and N are both nonmetals, meaning they do not form an ionic bond.
When the question refers to "least likely," which pair is the most unlikely to form an ionic bond? Based on my understanding, I would assume it's either Na and S or Mg and Br, but since both have an electronegativity difference of 1.6, I'm unsure how to determine the least likely pair.

Anonymous · Accepted Answer

When you continue studies in Chem you find ionic/covalent form a scale where few compounds are completely covalent (homonuclear) or 100% ionic, so most covalent is C and N as you predict they are closest in electronegativity 
Cs2O is most completely ionic with all the rest on the continuum. AlF3 is most definitely covalent in character but the bonds are polar.
http://en.wikipedia.org/wiki/Aluminium_fluoride

Anonymous · Answer

5. C and N… these are very likely to form a covalent bond, but not an ionic bond. (continue looking at electronegativities.)

PS Al Aluminum is a metal

Anonymous

Which of the following pairs of elements would be Least likely to form a compound by ionic bonding?

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