(a) Which geometry and central atom hybridization would you expect in the series BH₄^-, CH₄, NH₄⁺?

(b) What would you expect for the magnitude and direction of the bond dipoles in this series?

(a) Draw a picture showing how two p orbitals on two different atoms can be combined to make a σ bond. (b) Sketch a π bond that is constructed from p orbitals.

(c) Which is generally stronger, a s bond or a p bond? Explain.

(d) Can two s orbitals combine to form a p bond? Explain.

(b) Imagine that you could hold two atoms that are bonded together, twist them, and not change the bond length. Would it be easier to twist (rotate) around a single s bond or around a double 1s plus p2 bond, or would they be the same?

(a) Draw Lewis structures for chloromethane (CH₃Cl), chloroethene (C₂H₃Cl), and chloroethyne (C₂HCl).

(b) What is the hybridization of the carbon atoms in each molecule?

Propylene, C₃H₆, is a gas that is used to form the important polymer called polypropylene. Its Lewis structure is (a) What is the total number of valence electrons in the propylene molecule?

Benzaldehyde, C7H6O, is a fragrant substance responsible for the aroma of almonds. Its Lewis structure is

(a) What is the hybridization at each of the carbon atoms of the molecule?

Ethyl acetate, C₄H₈O₂, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is

(c) How many of the valence electrons are used to make s bonds in the molecule?

Ethyl acetate, C₄H₈O₂, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is

(e) How many valence electrons remain in nonbonding pairs in the molecule?

Consider the Lewis structure for acetic acid, which is known as vinegar:

(a) What are the approximate bond angles about each of the two carbon atoms, and what are the hybridizations of the orbitals on each of them?

Consider the Lewis structure for glycine, the simplest amino acid:

(b) What are the hybridizations of the orbitals on the two oxygens and the nitrogen atom, and what are the approximate bond angles at the nitrogen?

Consider the Lewis structure for acetic acid, which is known as vinegar: (b) What are the hybridizations of the orbitals on the two oxygen atoms, and what are the approximate bond angles at the oxygen that is connected to carbon and hydrogen? What are the hybridizations of the orbitals on the two oxygen atoms?

Consider the Lewis structure for glycine, the simplest amino acid:

(c) What is the total number of s bonds in the entire molecule, and what is the total number of p bonds?

(a) Write a single Lewis structure for N₂O, and determine the hybridization of the central N atom.

(c) Would you expect N₂O to exhibit delocalized p bonding?

In the sulphate ion, SO₄^2-, the sulphur atom is the central atom with the other 4 oxygen atoms attached to it. (b) What hybridization is exhibited by the S atom?

In the formate ion, HCO₂^-, the carbon atom is the central atom with the other three atoms attached to it. (c) Are there multiple equivalent resonance structures for the ion?

In the formate ion, HCO₂^-, the carbon atom is the central atom with the other three atoms attached to it. (d) How many electrons are in the p system of the ion? 

Consider the Lewis structure shown below.

(a) Does the Lewis structure depict a neutral molecule or an ion? If it is an ion, what is the charge on the ion? What is the charge on the ion

Predict the molecular geometry of each of the following molecules: (b) H O C O C O O H

What hybridization do you expect for the atom that is underlined in each of the following species? (a) IO₂^- (b) NH₄⁺ (c) SCN^- (d) BrCl₃