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?(1 point)

Question

Responses

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

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

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

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

Answer 1

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

This is the correct response because the transition metals have similar electronegativities, which means they are more inclined to share rather than transfer electrons, leading to the formation of covalent bonds. Ionic bonds typically form between atoms with a significant difference in electronegativity, where one atom donates an electron to another.