Question

Question 1 5 pts Atoms having greatly differing electronegativities are expected to form: O covalent bonds O polar covalent bonds ionic bonds no bonds nonpolar covalent bonds

Answer 1

1. Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons.

If the difference in electronegativity is huge, the atom with lesser electronegativity will have less tendency to attract the shared pair of an electron than to the higher electronegative atom. This forms an ionic bond

2.

To find out the hybridization, first, you need to find steric number of the central atom by the formula steric no = 1/2(no. of valence electrons + no. of singly bonded species with the atom whose hybridization is to be determined - cationic charge on molecule + anionic charge on the molecule)

Thus in XeF₅⁺

steric no. = 1/2(8+5–1)=6

Hybridization is sp³d²

Shape= square pyramidal

^3.

Take a look at a table of electronegativities (such as the link below); the bigger the difference in electronegativities, the more polar the bond:

Difference in electronegativity

P-Cl: 3.16 - 2.19 = 0.97

As-Cl: 3.16 - 2.18 = 0.98

N-Cl: 3.16 - 3.04 = 0.12

N-Cl is the least polar bond.

As-Cl>P-Cl>N-Cl

4. For your question, PH₂⁺ has a total of 6 valence electrons. With the least electronegative atoms (hydrogen in this case) at the terminal positions and phosphorous in the center and its single lone pair, you would have three electron groups. . 3 electron groups correspond to sp². Therefore, the hybridization of the phosphorus atom in PH₂⁺ is sp²