Unit 3 Bonding Review

CDO CP Chemistry Christman Fall 2013

Unit 3 Bonding Review

1. Name the following compounds

a. Ba(NO3)2 barium nitrate b. Ba(OH)2 barium hydroxide

c. KIO3 potassium iodate d. Fe(NO3)3 iron (III) nitrate

e. Cu3(PO4)2 copper (II) phospate f. SO3 sulfur dioxide

g. ZnSO4 zinc sulfate h. AgNO3 silver nitrate

i. N2O7 dinitrogen heptoxide

2. Give the correct formula for each of the following compounds:

a. sodium dichromate Na2Cr2O7

b. oxygen difluoride OF2

c. calcium sulfate CaSO4

d. dinitrogen tetrafluoride N2F4

e. tin (IV) bromide SnBr4

f. copper (II) chloride CuCl2

g. barium carbonate BaCO3

h. magnesium hydroxide Mg(OH)2

3. Identify each of the following as molecular or ionic

a. SeF4 Molecular b. BaO Ionic

c. LiBr Ionic d. As4O6 Molecular

e. SiF4 Molecular f. CuCl Ionic

g. Cs2O Ionic h. NH4HCO3 Ionic (2 polyatomics!)

i. NH3 Molecular



4. Define each of the following terms

a. Valence Electrons - electrons in the highest shell (energy level), is equal to the group

number and are the electrons available for bonding

b. Core Electrons - electrons in the lowest shells (included in the noble gas) and are

not available for bonding

c. Octet Rule – atoms form bonds in order to have access to 8 electrons in their valence

shell

d. Duet Rule - atoms which form bonds in order to have access to 2 electrons in their

valence shell, applies to H, Li and Be

e. Ionic Bond - a transfer of electrons due to electrostatic attraction, where one atom

gives an electron and the other atom accepts an electron

f. Covalent Bond – a sharing of 2 or more electrons to form a bond. Covalent bonds can

be for 1 pairs (single), 2 pairs (double) or 3 pairs (triple)

g. Diatomic Molecule – atoms which exsists in nature as a molecule consisting of 2

atoms of the same kind. H O F Br I N Cl

h. Polar Covalent Bond – a covalent bond in which the pair of electrons are shared

unequally

i. Non-Polar Covalent Bond - a covalent bond in which the electron pair is shared

equally, occurs between 2 of the same atom with the same electronegativity

j. Electronegativity – the ability of an atom to attract a pair of electrons in a bond.

Helps determine bond polarity



5. Give the number of valence electrons for each of the following atoms and draw their Lewis dot symbols:

a. Al b. Cs c. Si

d. Kr e. B f. Mg

g. P h. S i. Cl

j. C

6. What is the octet rule and how is it is satisfied with covalent and ionic bonds?

Octet rule is that atoms form bonds to have access to 8 electrons in their valence shell.

Covalent bonds are where electrons are shared to achieve an octet and ionic bonds are

where electrons are transferred to achieve an octet.

7. What are three ways that elements achieve octets?

Sharing, Giving or Receiving electrons

8. What is the difference between a polar bond and a nonpolar bond?

Polar bonds is where the shared electron pair is shared unequally, one atom pulls the

bond closer to it and in a non polar bond the pair is shared equally between the 2 atoms



9. Draw resonance structures for the following and explain why they are necessary Necessary to show the possible structures for the molecule, the actual exists

intermediate of the resonance structures

a. SO2

b. NO3-



10. What does the VSEPR Theory allow us to determine?

The three dimensional arrangement of a molecule

11. Why are double and triple bonds necessary in some molecules?

In order to have an octet for the atoms involved in the bond.

12. Indicate the type of bonding that would be expected for each of the following:

a. NaCl = ionic

b. H2O = covalent

c. H2= covalent

d. CoCl2= ionic

e. C6H12O6 = covalent

13. Draw the Lewis Structures for each of the Diatomic Molecules



14. Identify each of the following bonds as polar covalent or non-polar covalent

a. N-N = non polar covalent

b. N-O = polar covalent

c. H-Cl= polar covalent

d. F-F non polar covalent

e. B-F= polar covalent

15. Write the ion charge for each of the following atoms

a. Ca 2+

b. F 1-

c. Br 1-

d. K 1+

e. Ag 1+



16. Complete the following table

Chemical Formula

Lewis Electron Dot Structure

Electron Geometry

Molecular Geometry

Polar or Nonpolar

Predominant IMF

O2

H2O

CH3I



NH3

SO42-

CO

CO2



ClO4-

ClO3-

Unit 3 Bonding Review

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