1. H2O A. Chemical Formula Shows: 1) elements in the compound
2) ratio of their atoms
H2O
1 oxygen atom
2 hydrogen atoms

2. B. Chemical Bond
Strong attractive force between atoms or ions in a molecule or compound.
Formed by:
transferring e- (losing or gaining)
sharing e-

3. Ne C. Stability Octet Rule
most atoms form bonds in order to have 8 valence e-
full outer energy level
like the Noble Gases! Ne
Stability is the driving force behind bond formation!

4. C. Stability
Transferring e-
Sharing e-

5. II. Kinds of Chemical Bonds Ionic Bond Covalent Bond Comparison Chart
Ch Chemical Bonds
II. Kinds of Chemical Bonds
Ionic Bond
Covalent Bond
Comparison Chart

6. A. Ionic Bond Attraction between 2 oppositely charged ions
Ions - charged atoms
formed by transferring e- from a metal to a nonmetal

7. A. Ionic Bond
ions form a 3-D crystal lattice
NaCl

8. B. Covalent Bond Attraction between neutral atoms
formed by sharing e- between two nonmetals

9. B. Covalent Bond
covalent bonds result in discrete molecules
NH3
H2O
Cl2

10. B. Covalent Bond Nonpolar Covalent Bond e- are shared equally
usually identical atoms

11. + - B. Covalent Bond Polar Covalent Bond
e- are shared unequally between 2 different atoms
results in partial opposite charges + -

12. B. Covalent Bond
Nonpolar
Polar
Ionic
View Bonding Animations.

13. C. Comparison Chart IONIC COVALENT transferred from metal to nonmetal
shared between nonmetals
Electrons
Melting
Point
high
low
Soluble in
Water
yes
usually not
yes (solution or liquid)
Conduct Electricity no
crystal lattice of ions, crystalline solids
molecules, odorous liquids & gases
Other
Properties

14. III. Naming Molecular Compounds Molecular Names Molecular Formulas
Ch Chemical Bonds
III. Naming Molecular Compounds
Molecular Names
Molecular Formulas

15. A. Molecular Names Write the names of both elements.
Change the final ending to -ide.
Add prefixes to indicate subscripts.
Only use mono- prefix with oxide.

16. A. Molecular Names PREFIX mono- di- tri- tetra- penta- hexa- SUBSCRIPT1 2 3 4 5 6

17. A. Molecular Names CCl4 N2O carbon tetrachloride SF6
dinitrogen monoxide
sulfur hexafluoride

18. B. Molecular Formulas Write the more metallic element first.
Add subscripts according to prefixes.

19. B. Molecular Formulas phosphorus trichloride dinitrogen pentoxide PCl3
dihydrogen monoxide
PCl3
N2O5
H2O

20. B. Molecular Formulas The Seven Diatomic Elements
Br2 I2 N2 Cl2 H2 O2 F2

21. IV. Naming Ionic Compounds Oxidation Number Ionic Names Ionic Formulas
Ch Chemical Bonds
IV. Naming Ionic Compounds
Oxidation Number
Ionic Names
Ionic Formulas

22. A. Oxidation Number The charge on an ion.
Indicates the # of e- gained/lost to become stable. 1+ 2+ 3+ 4+ 3- 2- 1-

23. B. Ionic Names Write the names of both elements, cation first.
Change the anion’s ending to -ide.
Write the names of polyatomic ions.
For ions with variable oxidation #’s, write the ox. # in parentheses using Roman numerals. Overall charge = 0.

24. B. Ionic Names NaBr Na2CO3 sodium bromide FeCl3 sodium carbonate
iron(III) chloride

25. C. Ionic Formulas Write each ion. Put the cation first.
Overall charge must equal zero.
If charges cancel, just write the symbols.
If not, crisscross the charges to find subscripts.
Use parentheses when more than one polyatomic ion is needed.
Roman numerals indicate the oxidation #.

26. C. Ionic Formulas potassium chloride magnesium nitrate K+ Cl-  KCl
copper(II) chloride
K+ Cl-  KCl
Mg2+ NO3-  Mg(NO3)2
Cu2+ Cl-  CuCl2

27. C. Ionic Formulas calcium oxide aluminum chlorate Ca2+ O2-  CaO
iron(III) oxide
Ca2+ O2-  CaO
Al3+ ClO3-  Al(ClO3)3
Fe3+ O2-  Fe2O3