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 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:

(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 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

(b) If you combine two atomic orbitals on one atom to make a new orbital, is this a hybrid orbital or a molecular orbital?

Consider the H₂⁺ ion. (a) Sketch the molecular orbitals of the ion and draw its energy-level diagram.

Consider the H₂⁺ ion. (b) How many electrons are there in the H₂⁺ ion?

Consider the H₂⁺ ion. (c) Write the electron configuration of the ion in terms of its MOs. (d) What is the bond order in H₂⁺?

Consider the H₂⁺ ion. (e) Suppose that the ion is excited by light so that an electron moves from a lower-energy to a higher-energy MO. Would you expect the excited-state H₂⁺ ion to be stable or to fall apart?

Consider the H₂⁺ ion. (f) Which of the following statements about part (e) is correct: (i) The light excites an electron from a bonding orbital to an antibonding orbital, (ii) The light excites an electron from an antibonding orbital to a bonding orbital, or (iii) In the excited state there are more bonding electrons than antibonding electrons?

(c) Calculate the bond order in H2-.

Draw a picture that shows all three 2p orbitals on one atom and all three 2p orbitals on another atom. (a) Imagine the atoms coming close together to bond. How many σ bonds can the two sets of 2p orbitals make with each other?

Draw a picture that shows all three 2p orbitals on one atom and all three 2p orbitals on another atom. (b) How many p bonds can the two sets of 2p orbitals make with each other?