Given the following information about electronegativity, which binary compound would form covelant bonds with the greatest polarity?
Element Electronegativity
H 2.1
Li 1.0
S 2.5
Al 1.5
F 4.0
Cl 3.0
A. HCl
B. LiF
C. H2S
D. AlH3
The trick here is to use your electronegativeity to determine which are covalent.
LiF, or instance, is ionic
You figure the rest based on difference in electronegativity.
Hint: are any Gaseous? Those are probbbly covalent. If three are colvlent, and two are gases, one solid, look closely at the solid.
Thank doesn't help. I posted the question because I don't understand how to compare the electronegativity when there are molecules like AlH3.
To determine which binary compound would form covalent bonds with the greatest polarity, we need to calculate the difference in electronegativity between the two elements in each compound.
Polarity in a covalent bond is determined by the difference in electronegativity between the two elements. The greater the difference, the more polar the bond.
Let's calculate the electronegativity difference for each option:
A. HCl: The electronegativity of H is 2.1, and the electronegativity of Cl is 3.0. The difference is 3.0 - 2.1 = 0.9.
B. LiF: The electronegativity of Li is 1.0, and the electronegativity of F is 4.0. The difference is 4.0 - 1.0 = 3.0.
C. H2S: The electronegativity of H is 2.1, and the electronegativity of S is 2.5. The difference is 2.5 - 2.1 = 0.4.
D. AlH3: The electronegativity of Al is 1.5, and the electronegativity of H is 2.1. The difference is 2.1 - 1.5 = 0.6.
By comparing the electronegativity differences, we can see that the greatest difference is found in option B, LiF, with a difference of 3.0. Therefore, LiF would form covalent bonds with the greatest polarity.