The electronegativity is 2.1 for H and 3.0 for N. Based on these electronegativities, NH4 would be expected to The electronegativity is 2.1 for H and 3.0 for N. Based on these electronegativities, NH4 would be expected to have polar covalent bonds with a partial positive charges on the H atoms. be ionic and contain H- ions. have polar covalent bonds with a partial negative charges on the H atoms. be ionic and contain H ions.

The ammonia has bee tend to be a polar molecule with a partial positive charge on the H atom. Thus, option A is correct.

The type of bond formed can be assessed by the difference in the electronegativity of the elements. The bonds with an electronegativity difference of more than 1.7 have been termed nonpolar bonds. The bonds with electronegativity differences less than 1.7 are termed polar bonds.

The difference in electronegativity = 3 – 2.1

The difference in electronegativity = 0.9

Since the electronegativity difference has been less than 1.7, the bond has been polar. The electrons are shifted towards nitrogen as it has been more electronegative. Thus, option A is correct.

For more information about polar bonds, refer to the link:

link

First statement is true:

Explanation:

Nitrogen (N) and hydrogen (H) are two nonmetals; thus, it should be a hint to assert that they form a covalent bond.

The difference in electronegativities between N and H is 3.0 - 2.1 = 0.9.

That makes that the bonds be polar. Ions are not formed because to transfer the electrons from one atom to the other (to form ionic bonds) requires an electronegativity difference greater than about 1.7.

Since N is more electronegative than H, in the molecule NH₄, each N atom will pull the electron density toward itself acquiring a partial negative charge and leaving H atoms with a partial positive charge.

Thus, each NH bond is polar covalent with a partial positive charge on the H atoms (first statement from the choices).