Answer:
d. HI would be expected to have polar covalent bonds with a partial positive charge on the H atom.
Explanation:
Electronegativity is the power of an atom in a molecule to attract electrons. During chemical bonding, the difference in electronegativity values between bonded atoms determines the various bond types formed.
If the electronegativity difference between two atoms is 1.7 or more, the bond formed may be predominantly ionic; between values of 0.3 and 1.7, the bond inclines towards a polar covalent bond; and 0.3 or less ( mainly between atoms of same element e.g between two oxygen atoms ) tends to produce non-polar covalent bond.
Considering the electronegativities of H = 2.1 and I = 2.5, their electronegativity difference is = 2.5 – 2.1 = 0.4
So,compound HI would be expected to have polar covalent bonds.
Also, in a polar covalent bond, there exists an uneven charge distribution as the electrons are more attracted to the more electronegative atom, this makes the more electronegative atom possess a partial negative charge called a negative dipole, δ− , while the less electronegative atom possess a partial positive charge called a positive dipole, δ+ .
In HI, H being less electronegative ( 2.1 ) than I ( 2.5 ), there will be a partial positive charge on the H atom as the electrons incline towards the I atom.
Therefore, HI would be expected to have polar covalent bonds with a partial positive charge on the H atom.
