Homework
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Chapter 2 Read pages 43-44
WS: Naming molecules
Quiz: Next Time!
Test Dates: Jan. 17, 18, 19
Acid Worksheet
1. perchloric acid
2. HI
3. phosphoric acid
4. H2CO3
5. hydrocyanic acid
6. HClO
7. HNO3
8. hydrochloric acid
9. H3PO3
10. HClO2
11. nitrous acid
12. HBr
13. HC2H3O2
14. H2CrO4
15. dichromic acid
16. permanganic acid
17. H2SO4
18. HClO4
19. H2C2O4
NH4Cl
Fe2S3
HMnO4
Hg2S
H2Cr2O7
SnO2
Al(NO2)3
RbI
(NH4)2CO3
MnCr2O7
ammonium chloride
iron(III) sulfide
permanganic acid
mercury(I) sulfide
dichromic acid
tin(IV) oxide
aluminum nitrite
rubidium iodide
ammonium carbonate
manganese(II) dichromate
Co3N2
cobalt(II) nitride
Ag2C2O4
silver oxalate
(NH4)2HPO4 ammonium hydrogen
phosphate
Cu(OH)2
copper(II) hydroxide
ferric sulfide
mercurous sulfide
stannic oxide
manganous
dichromate
cobaltous nitride
ammonium
biphosphate
cupric hydroxide
Ca(ClO4)2
CrSO3
Ag3PO3
Pb(C2H3O2)4
H2SiO3
Mn(MnO4)3
NH4C2H3O2
Cs2Cr2O7
HMnO4
calcium perchlorate
chromium(II) sulfite
silver phosphite
lead(IV) acetate
silicic acid
manganese(III)
permanganate
ammonium acetate
cesium dichromate
permanganic acid
chromous sulfite
plumbic acetate
manganic
permanganate
BINARY MOLECULAR
COMPOUNDS
 composed
of nonmetals
 electrons are shared (covalent):
NO CHARGES
 no criss-cross method
 do not reduce subscripts
 can combine in more than one way
NAMING BINARY
MOLECULES
 prefixes
used to denote multiple
atoms of one element in a molecule
1
2
3
4
5
mono- 6
di7
tri8
tetra- 9
penta- 10
hexaheptaoctanonadeca-
NAMING BINARY
MOLECULES
element in name ends in –ide
 for oxides: generally for mono, use
only one “o”
 monooxide becomes monoxide
 2nd
NAMING BINARY
MOLECULES
 if
there is ONE atom of the first
element, omit the prefix mono–
 ex: CO
carbon monoxide
NOT monocarbon monooxide
NAMING BINARY
MOLECULES
CO
carbon monoxide
CO2 carbon dioxide
N2O dinitrogen monoxide
Cl2O8 dichlorine octaoxide
WRITING NAMES
OF2
oxygen difluoride
N2O5 dinitrogen pentaoxide
P4O10 tetraphosphorus decaoxide
SO3
sulfur trioxide
WRITING FORMULAS
nitrogen trifluoride
disulfur dichloride
NF3
S2Cl2
dinitrogen tetraoxide N2O4
carbon tetrachloride CCl4
MOLECULAR FORMULA
 diatomic
molecules: molecules with
2 atoms of the same element
 there are 7 – know them!
N2 O2 H2 Cl2 I2 F2 Br2
or
Br2 I2 N2 Cl2 H2 O2 F2
Electronegativity and Polarity
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Electronegativity= ability of an atom to
attract electrons in a covalent bond.
Most electronegative element =
Least electronegative element =
Unequal sharing of electrons will produce
a polar bond.
Examples