Module # 9 Review Questions

Question 1

Polyatomic Ions

Answer 1

Ions that are formed when a group of atoms gains or lose electrons.

Question 2

Finding Chemical Formula

Answer 2

Locate the first element’s column number on the periodic chart. Remember what charge the polyatomic ion is. Switch the charge numbers as subscripts.

Question 3

VSEPR (acronym)

Answer 3

Valence Shell Electron Pair Repulsion

Question 4

VSEPR Theory

Answer 4

molecules will attain whatever shape keeps the valence electrons of the central atom as far apart as possible.

Question 5

Tetrahedron Shape

Answer 5

Four groups of electrons. Has four bonds (legs). 109-degree bond angle. No pairs of none-bonding electrons.

Question 6

Pyramidal Shape

Answer 6

Four groups of electrons. Three bonds (legs) 107-degree bond angle. One pair of none-bonding electrons.

Question 7

Bent Shape

Answer 7

Four groups of electrons. Two bonds (legs). 105-degree bond angle. Two pairs of none-bonding electrons.

Question 8

Trigonal Shape

Answer 8

Three groups of electrons. Three bonds (legs). 120-degree bond angle. No pairs of none-bonding electrons.

Question 9

Linear Shape

Answer 9

Either only two atoms or two groups of electrons around the central atom. 180-degree bond angle.

Question 10

Purely Covalent Bond

Answer 10

A covalent bond in which the electrons are shared equally among the atoms involved.

Question 11

Polar Covalent Bond

Answer 11

A covalent bond in which the electrons are shared unequally among the atoms involved.

Question 12

Ionic/polar covalent + polar covalent

Answer 12

Polar covalent compounds can dissolve other polar covalent or ionic compounds.

Question 13

Purely covalent + purely covalent

Answer 13

Purely covalent compounds can only dissolve other purely covalent compounds.