Dipole moment (p) = charge (q) × distance (d) = (1.6 x 10^-19 C) × (1.5 x 10^-10 m) = 2.4 x 10^-29 C·m.

Dipole moment (μ) = charge (q) × distance (d). μ = 0.33 e × 1.27 × 10^-10 m = 4.2 × 10^-29 C·m = 1.1 D.

Formal charge = Valence electrons - (Non-bonding electrons + 1/2 Bonding electrons) = 5 - (0 + 1/2*6) = 0.

Formal charge = valence electrons - (non-bonding electrons + 1/2 bonding electrons). For nitrogen in NO3-, it is 5 - (0 + 1/2(6)) = 0.

In a tetrahedral geometry, the bond angles are approximately 109.5° due to the arrangement of four electron pairs.

The bond energy for a double bond (bond order = 2) is typically around 600 kJ/mol for C=C.

For a single bond (bond order = 1), the average bond energy is approximately 348 kJ/mol, but for C-C it is typically around 346 kJ/mol.

BF3 has a trigonal planar geometry with bond angles of approximately 120°.

Bond order = (Number of bonding electrons - Number of antibonding electrons) / 2 = (10 - 4) / 2 = 3.

Bond order = (12 - 4) / 2 = 4. The bond order for O2 is actually 2, but this question is hypothetical.

N2 has 10 bonding electrons and 2 antibonding electrons, so bond order = (10 - 2) / 2 = 4 / 2 = 2.

O2 has 12 total valence electrons. The bond order is calculated as (number of bonding electrons - number of antibonding electrons) / 2 = (10 - 2) / 2 = 4 / 2 = 2.

The typical bond length for a C-C single bond is approximately 1.54 Å.

The hybridization is determined by the number of sigma bonds. 4 sigma bonds correspond to sp3 hybridization.

With 2 bonding pairs and 2 lone pairs, the molecular geometry is bent due to the repulsion of lone pairs.

NH3 has three bonding pairs and one lone pair, resulting in a trigonal pyramidal geometry.

With 5 bonding pairs and 1 lone pair, the molecular shape is square pyramidal.

NaCl is formed by the transfer of an electron from Na to Cl, resulting in an ionic bond.