The top row of transition metals in the middle of the periodic table have electronegativities ranging from 1.4 to 1.9. Which kind of bond are these metals likely to form with one another, and why?

Question

1) They are likely to form covalent bonds because the higher electronegative atoms will take electrons from the atoms with lower electronegativities.

2) They are likely to form covalent bonds because their electronegativities are close together, making them likely to share electrons.

3) They are likely to form ionic bonds because the higher electronegative atoms will take electrons from the atoms with lower electronegativities.***

4) They are likely to form ionic bonds because their electronegativities are close together, making them likely to share electrons.

I think its C am I right?

Answer 1

I don't think so. You are correct that C describes how ionic bonds are formed but the difference in electronegativity needs to be about 1.8 or so in order to make that "electron movement" possible. In the case of the transition metals the max difference is 1.9-1.4 = 0.5 which isn't close to 1.8 or 1.9.

Answer 2

Yeah, you're right. I know metals usually form ionic bonds, but I'm just not sure how to figure the electronegativity.

Answer 3

You do it with the difference in electronegativity (EN)
A 50-50 polar covalent bond has a difference of about 1.8. Anything over that I call ionic and anything under that I call covalent. Technically, those between 1.0 and 1.7 or 1.8 are polar covalent. It sorta
gets fuzzy about exactly where we want to start with polar covalent etc. Again, technically, the only pure covalent bonds, in my opinion, are those such as H2, O2, Cl2, etc. and I've been told that even those have a smidgen of ionic character.

Answer 4

So is the answer C?