Chapter 8

Draw the Lewis structure for each molecule. \(\mathrm{PH}_{3}\)

Draw the Lewis structure for each molecule. \(\mathrm{H}_{2} \mathrm{S}\)

Draw the Lewis structure for each molecule. \(\mathrm{HCl}\)

Draw the Lewis structure for each molecule. \(\mathrm{CCl}_{4}\)

Challenge Draw a generic Lewis structure for a molecule formed between atoms of Group 1 and Group 16 elements.

A Identify the type of atom that generally forms covalent bonds

Describe how the octet rule applies to covalent bonds

Illustrate the formation of single, double, and triple covalent bonds using Lewis structure

Compare and contrast ionic bonds and covalent bonds

Contrast sigma bonds and pi bonds

Name each of the binary covalent compounds listed below. \(\mathrm{CO}_{2}\)

Name each of the binary covalent compounds listed below. \(\mathrm{SO}_{2}\)

Name each of the binary covalent compounds listed below. \(\mathrm{NF}_{3}\)

Name each of the binary covalent compounds listed below. \(\mathrm{CCl}_{4}\)

Challenge What is the formula for diarsenic trioxide?

Name the following acids. Assume each compound is dissolved in water. \(\mathrm{HClO}_{3}\)

Name the following acids. Assume each compound is dissolved in water. \(\mathrm{HClO}_{2}\)

Name the following acids. Assume each compound is dissolved in water. \(\mathrm{H}_{2} \mathrm{SO}_{4}\)

Name the following acids. Assume each compound is dissolved in water. \(\mathrm{H}_{2} \mathrm{S}\)

Give the formula for each compound. silver chloride

Give the formula for each compound. dihydrogen oxide

Give the formula for each compound. chlorine trifluoride

Give the formula for each compound. diphosphorus trioxide

Give the formula for each compound. strontium acetate

Challenge What is the formula for carbonic acid?

Summarize the rules for naming binary molecular compounds.

Define a binary molecular compound.

Describe the difference between a binary acid and an oxyacid.

Apply Using the system of rules for naming binary molecular compounds, describe how you would name the molecule \(\mathrm{N}_{2} \mathrm{O}_{4}\) .

Apply Write the molecular formula for each of these compounds: iodic acid, disuffur trioxide, dinitrogen monoxide, and hydrofluoric acid.

State the molecular formula for each compound listed below. \(\begin{array}{ll}{\text { a. dinitrogen trioxide }} & {\text { d. chloric acid }} \\ {\text { b. nitrogen monoxide }} & {\text { e. sulfuric acid }} \\\ {\text { c. hydrochloric acid }} & {\text { f. sulfurous acid }}\end{array}\)

Draw the Lewis structure for BH_ \(_{3}\)

Challenge A nitrogen trifluoride molecule contains numerous lone pairs. Draw its Lewis structure.

Draw the Lewis structure for ethylene, \(\mathrm{C}_{2} \mathrm{H}_{4}\)

Challenge A molecule of carbon disulfide contains both lone pairs and multiple-covalent bonds. Draw its Lewis structure.

Draw the Lewis structure for the \(\mathrm{NH}_{4}+\) ion.

Challenge The \(\mathrm{ClO}_{4}-\) ion contains numerous lone pairs. Draw its Lewis structure.

Draw the Lewis resonance structures for the following molecules. $$ \mathrm{NO}_{2}^{-} $$

Draw the Lewis resonance structures for the following molecules. $$ \mathrm{SO}_{2} $$

Draw the Lewis resonance structures for the following molecules. $$ \mathrm{O}_{3} $$

Challenge Draw the Lewis resonance structure for the ion \(\mathrm{SO}_{3}^{2-}\)

Draw the expanded octet Lewis structure for each molecule. $$ \mathrm{PCl}_{5} $$

Challenge Draw the Lewis structure for the molecule formed when six fluorine atoms and one sulfur atom bond covalently.

Describe the information contained in a structural formula.

State the steps used to draw Lewis structures.

Evaluate A classmate states that a binary compound having only sigma bonds displays resonance. Could the classmate's statement be true?

Draw the resonance structures for the dinitrogen oxide \(\left(\mathrm{N}_{2} \mathrm{O}\right)\) molecule.

Draw the Lewis structures for \(\mathrm{CN}^{-}, \mathrm{SiF}_{4}, \mathrm{HCO}_{3}^{-},\) and, AsF \(_{6}-\)

Determine the molecular shape, bond angle, and hybrid orbitals for each molecule. $$ \mathrm{BF}_{3} $$

Determine the molecular shape, bond angle, and hybrid orbitals for each molecule. $$ \mathrm{BeF}_{2} $$