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In the above Lewis structure for ClO3F, chlorine has a formal charge of ____ and an oxidation number of ____.

In the following Lewis structure for phosphate, phosphorus has a formal charge of ____ and an oxidation number of ____.

In neutral molecules, how many bonds are commonly formed by nitrogen? And how many by oxygen?

Determine the shape (geometry) of PCl3 and then decide on the appropriate hybridization of phosphorus in this molecule. (Phosphorus is the central atom.)

The lattice energy of solid MgCl2 is the energy change for which one of the following processes?

Select the strongest bond in the following group

A molecule with the formula AX2 uses _________ to form its bonds.

According to valence bond theory, which orbitals on N and H overlap in the NH3 molecule?

Which of the following elements will form a cation with a +2 charge?

Using the bond energies provided below, calculate ΔH° for the reactionCH4(g) + 4Cl2(g) → CCl4(g) + 4HCl(g)Bond energies: C–H = 413 kJ/mol, Cl–Cl = 243 kJ/mol, C–Cl = 339 kJ/mol, H–Cl = 427 kJ/mol