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) 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?
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.
Yeah, you're right. I know metals usually form ionic bonds, but I'm just not sure how to figure the electronegativity.
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.
No, option 3 is not correct. The top row of transition metals in the middle of the periodic table, such as iron (Fe), cobalt (Co), nickel (Ni), and copper (Cu), do not typically form ionic bonds with each other.
The correct answer is option 2: They are likely to form covalent bonds because their electronegativities are close together, making them likely to share electrons.
Covalent bonds occur when two atoms share electrons and are typically formed between nonmetals or between a nonmetal and a metalloid. Transition metals are located in the middle of the periodic table and have properties that are neither purely metallic nor nonmetallic. Therefore, they tend to form covalent bonds with each other due to their similar electronegativities.
It is important to determine the difference in electronegativities between the elements to predict the type of bond they are likely to form. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. Elements with larger electronegativity differences (e.g., metals and nonmetals) tend to form ionic bonds, while elements with smaller electronegativity differences (e.g., nonmetals and nonmetals) tend to form covalent bonds.
In the case of the top row of transition metals, their electronegativity values are relatively close together (ranging from 1.4 to 1.9). This indicates that the electron-attracting abilities of these atoms are similar, making it more favorable for them to share electrons and form covalent bonds rather than transfer electrons and form ionic bonds.