Next Semester we will begin with the study of chemical reactions

1

• Next Semester we will begin with the study of
  chemical reactions
• In order to study chemical reactions we need to
  be able to
• write chemical formulas for compounds involved
  in reactions
• Name chemical compounds involved in chemical
  reactions

2

• Metals with more than one charge
• Formula Stock name Classical name Formula
  Stock name Classical name
• Cu1 Copper (I) ion Cuprous ion
  Hg22 Mercury (I) ion Mercurous
  ion
• Cu2 Copper (II) ion Cupric ion
  Hg2 Mercury (II) ion Mercuric
  ion
• Fe2 Iron (II) ion Ferrous ion
  Pb2 Lead (II) ion Plumbous
  ion
• Fe3 Iron (III) ion Ferric ion
  Pb4 Lead (IV) ion
  Plumbic ion
• Sn2 Tin (II) ion Stannous ion
  Cr2 Chromium (II) ion
  Chromous ion
• Sn4 Tin (IV) ion Stannic ion
  Cr3 Chromium (III) ion Chromic
  ion
• Co2 Cobalt (II) ion Cobaltous ion
  Mn2 Manganese (II) ion Manganous
  ion
• Co3 Cobalt (III) ion Cobaltic ion
  Mn3 Manganese (III) ion Manganic
  ion

3

• Chapter 7 Chemical Names and Formulas
• Elements Symbols and the Diatomic 7
• 1. You probably know the chemical symbols for
  many elements (ex Sodium ____, Mercury ____,
  Silver ____, Gold ______ etc).
• 2. There are 7 elements that exist in nature as
  ___________ (two atoms together). They are
  called the diatomic 7. List them below
• (Note The charge of these diatomic elements is
  0)
• 4. Many elements exist in a combined state with
  other elements to make what is called a compound.
• Binary Ionic Compounds (pg. 222-223) Compounds
  composed of ___ elements. These elements will be
  a ____________ and _______________. (No prefixes
  for ionic compounds)
• 1. Compounds of a metal and non-metal are
  commonly called __________ compounds.
• 2. When ionic compounds form the metal will
  ___________ electrons to form a __ ion
• ( __________) and the non-metal will _________
  electrons to form a __ ion (____________).
• 3. The chemical formula for an ionic compound
  will have the __________ written first followed
  by the __________. The metal will be given its
  elemental name and the non-metal will have a
  modification of its elements name so that it
  includes an _________ ending.
• Ex Chemical Formula NaCl
  Name
• Chemical Formula LiBr
  Name
• Chemical Formula CaCl2
  Name
• To write the chemical formula for an ionic
  compound, the positive and negative charges must
  be ___________. In order to determine if the
  charges are equal, you must look at the oxidation
  number of each element present in the compound
  (recall the oxidation number for elements in
  group 1A is ___, for elements in group 6A is ___
  etc.)
• In order to balance the charge, ______________
  will be written below the chemical symbols.

Na
Hg
Au
Ag
diatoms
I2
Br2
F2
O2
Cl2
N2
H2
2
metal
non-metal
ionic
lose

gain
anion
-
cation
metal
non-metal
-ide
sodium
chloride
lithium
bromide
calcium
chloride
equal
1
-2
subscripts
4

• Ionic Compounds Containing Transition Metals
  (Use Roman Numerals)
• Stock Names
• Many transition metals have more than one charge
  as ions in compounds (exceptions Ag always has a
  ___ charge as an ion and Cd and Zn always have a
  ______charge as an ion.)
• Note We are not saying that metals always have
  a charge. In an uncombined state as an element
  they have no charge, but when they combine with
  non-metals to form compounds they will have a
  charge.

Ex Write the chemical formula for sodium
bromide
-1
1
Na
Br
Charges are balanced, erase oxidation s
Ex Write the chemical formula for potassium
oxide
1
-2
K
O
2
Ex Write the chemical formula for barium
fluoride
2
-1
Ba
F
2
Ex Write the chemical formula for calcium
phosphide
2
-3
Ca
P
3
2
2
1
5

• 2. When writing the name of an ionic compound
  with a transition metal it is important to
  indicate the _____________ of the transition
  metal. The charge will be indicated as a
  ______________ numeral after the transition
  metal.
• Ex Write the name of CuCl Write the name of
  CuCl2
• Classical Name (-ous or ic ending on transition
  metal)
• 1. Often the stock system is not used and the
  _____________ names are given to ionic compounds
  containing transition metals with more than one
  charge.
• 2. Here, the ion of a particular transition
  metal with the lower charge will have an
  _________ ending and the ion with the higher
  charge will have an _____ ending.
• 3. Your naming sheet has the charges and
  classical names for different transition metal
  ions.

charge
roman
copper chloride
copper chloride
( )
( )
II
I
classical
-ous
-ic
Write the chemical formula for Iron (II) Oxide
Write the chemical formula for Ferric Sulfide
-2
2
3
-2
Fe
S
O
Fe
2
3
Write the chemical formula for Mercury (I) Oxide
and Mercury (II) Oxide
2
-2
2
-2
Hg2
Hg
O
O
6

• Write the chemical formula for Plumbous Chloride
• Name the compound SnCl4 using the classical and
  stock names.

2
-1
Cl
Pb
2
Stock Name
tin chloride
( )
IV
Classical Name
stannic chloride
7

• Homework
• 1. Write the names for the following binary ionic
  compounds
• (For transition metal compounds use the Stock and
  Classical Names when applicable)
• a. KCl b. NaI c. K2O d. CuS
  e. Li2S f. Na3N g. AgI h. FeO
  i. ZnO
• 2. Write the chemical formula for the following
  binary ionic compounds
• a. Lithium Oxide b. Tin(IV) Sulfide
  c. Hydrogen Chloride d. Silver Chloride
• e. Manganese (II) Nitride f. Mercury (I) Oxide
  g. Mercury (II) Bromide h. Cadmium
  Sulfide

sulfide
lithium
a. potassium
chloride
e.
1.
i. zinc oxide
iodide
b. sodium
f.
sodium nitride
g. silver iodide
oxide
potassium
c.
sulfide
stock
copper
( )
II
d.
h.
stock
iron (II) oxide
sulfide
classical
cupric
ferrous oxide
classical
a. Li2O
2.
e. Mn3N2
b. SnS2
h. CdS
f. Hg2O
c. HCl
g. HgBr2
d. AgCl
8

• Chemical Names and Formulas II
• Ionic Compounds containing polyatomic ions (pg.
  225-227)
• The same rules apply to ionic compounds
  containing polyatomic ions as did for binary
  ionic compounds (___ prefixes) except there will
  be no ide endings added. Here, write the name
  of the metal first (use stock (roman numeral) and
  classical name if necessary), then write the name
  of the polyatomic ion (most polyatomic ions end
  in ite or ate ending except hydroxide (
  ), peroxide ( ) and cyanide (
  )).
• Examples
• 1. Write the Chemical Formula for the following
• 2. Write the chemical name for the following
  (include classical and stock names)

no
O2-2
OH-
CN-
a. Sodium Phosphate
b. hydrogen peroxide
c. ferrous hypochlorite
d. ammonium sulfate
-1
-2
Fe
2
-3
H
1
O2
ClO
PO4
( )
1
Na
1
SO4
-2
( )
NH4
2
3
2
2
e. calcium carbonate
f. copper (II) nitrate
-2
Ca
2
2
CO3
Cu
NO3
-1
( )
2
a. Fe2(SO4)3
b. Na2CrO4
c. Cr2(C4H4O6)3
stock
stock
chromium ( )
tartrate
III
sulfate
sodium
iron ( )
III
chromate
classical
chromic tartrate
ferric sulfate
classical
f. (Hg2)3(PO4)2
d. Mn(OH)2
e. NH4HCO3
stock
stock
ammonium hydrogen carbonate
ammonium bicarbonate
phosphate
mercury ( )
I
manganese (II) hydroxide
mercurous phosphate
classical
manganous hydroxide
classical
9

• Naming Covalent (molecular) compounds (pg.
  227-229)
• Covalent compounds are compounds composed of
  non-metals (or metalloid/non-metal).
• For these compounds prefixes will be used to
  indicate the numbers of that element present
  (exceptions ________ will not be used on the
  first element shown like CO is carbon monoxide).
  
• The last element will be given an _________
  ending.
• Prefixes
• mono-1 di-2 tri- 3 tetra- 4 penta- 5
  hexa- 6 hepta- 7 octa- 8 nona- 9
  deca- 10
• Examples
• 1. Name the following
• a. NO b. NO2 c. N2O d. P4O7
• 2. Write the chemical formula for the following
• a. dinitrogen pentoxide b. boron trifluoride c.
  carbon tetrachloride
• Summary
• When the first element of a compound is a metal
  then it is ionic. Dont use prefixes (if it is a
  transition metal give the classical and stock
  name labeled properly (no s or c)).

mono-
-ide
dinitrogen monoxide
nitrogen monoxide
nitrogen dioxide
tetraphosphorus heptoxide
CCl4
N2O5
BF3
10

• Naming Inorganic Acids (pg. 230-231)
• Acids are named for the Latin word acidus which
  means _______ or tart. Acids taste sour and
  substances that are bases are ________. The
  Arrhenius theory of acids state that acids
  release ____ when dissolved in water and bases
  release _____ when dissolved in water.
• Rules for Naming Acids
• General Chemical formula for acids HX (aq)- the
  (aq) means the substance is dissolved in
  ________. Dissolving an acid in water results in
  the releasing of an ____ ion.
• 1. When the X anion ends in ______ use _______
  stem ___ acid.
• Examples
• HCl (aq) HBr(aq) HCN(aq)
• HCl (g) hydrosulfuric acid
• 2. When the X anion ends in _______ use stem
  _____ acid.
• Examples
• HClO4 (aq) HNO3 (aq) H3PO4 (aq)
• carbonic acid acetic acid

sour
bitter
H
OH-
water
H
-ide
-ic
hydro-
hydrochloric acid
hydrobromic acid
hydrocyanic acid
hydrogen monochloride
1
-2
(aq)
S
H
2
-ate
-ic
perchloric acid
nitric acid
phosphoric acid
-2
1
-1
1
(aq)
C2H3O2
H
CO3
H
(aq)
2
11

• 3. When the X anion ends in ____ use stem _____
  acid.
• Examples
• H2SO3 (aq) HClO (aq)
• phosphorous acid chlorous acid
• Summary
• 1. If the first element of the compound is a
  metal (or ammonium ion) then it is ionic (NO
  PREFIXES!).
• -if the metal has more than 1 charge use
  classical and stock names
• 2. If the first element of the compound is a
  metalloid or non-metal (other than hydrogen) then
  it is
• covalent (USE PREFIXES!)
• 3. If the first element of the compound is H and
  there is an (aq) symbol, then it is an acid.
• if anion ends in ide use hydro stem ic acid

-ous
-ite
sulfurous acid
hypochlorous acid
-1
1
1
-3
(aq)
(aq)
H
PO3
H
ClO2
3
12

• Properties of Ionic and Covalent Compounds,
  Metals pg. 193-196
• Ionic compounds
• a. Tend to be ________________ at room
  temperature due to the strong electrostatic
  attractions between the oppositely charged ions.
  Solids have a definite shape and volume (fig. 6
  pg 9).
• b. The ions are in fixed positions relative to
  each other. If an ionic compound is struck, like
  charged ions a forced close to each other and the
  structure will _______________ (see fig. 17 pg.
  193).
• c. When heated to the molten state (or
  dissolved in water), the ions are free to move
  and will conduct ________________.
• d. The simplest particle that retains the
  properties of an ionic compound is called a
  _____________ unit.
• e. An ionic compound composed of metallic
  cations and an anion from some acid are called
  _______.
• Metals
• a. Tend to be solids at room temperature.
  Metallic bonding consists of metallic cations
  being surrounded by a sea of freely floating
  ______________ electrons (see fig. 18 pg. 195).
  The result of the freely floating electrons (free
  to move cation to cation) is the unique
  properties of malleability, ductility,
  conductivity of electricity and heat as well as
  the ability to reflect light well (have a
  luster).
• b. The simplest particle that retains the
  properties of a metal is an ____________ (just
  like most elements except for the diatomic 7
  which are composed of molecules).
• Covalent compounds
• Have a ________ range of boiling and melting
  points due to a broad range in strength of
  intermolecular forces. The result is that some
  covalent compounds being solids, some being
  liquids (have a definite volume but assume the
  shape of the container) and some being gases
  (assume the volume and shape of the container).
• b. The simplest particle that retains the
  properties of a sample of covalent compound is a
  ____________.
• c. Covalent compounds are brittle as solids and
  do not conduct electricity in the solid or molten
  state (they are ____________________). Variable
  solubility in water (depends upon the polarity of
  the molecule).

solids
shatter
electricity
formula
salts
valence
atom
broad
molecule
insulators
13

• Percentage Composition (pg. 242-244)
• Percentage composition is a statement that
  relates the ________ of one element in a compound
  to the sum of all the masses of all the elements
  within the compound.
• This may be determined in a couple of ways
• 1. Percentage composition from experimental data
• A chemist determines that there is 1.58 g of
  Copper present in 1.98 g of a compound that
  contains Copper and Sulfur. Determine the
  percentage composition of Sulfur and Copper in
  the compound.
• Cu g Cu 100
• g cmp
• Cu 1.58 g 100
• 1.98 g
• Cu 79.8
• 2. Percentage composition from Chemical Formula
  
• Is the compound shown in sample 1a. Copper (I)
  Sulfide or Copper (II) Sulfide?

mass
S 100 - Cu
S 100 79.798
S 20.2
Cu2S
Cu2S
CuS
Cu in Cu2S
Cu in CuS
Cu g Cu 100 g CuS
Cu g Cu 100 g Cu2S
Cu 63.546 g/mol 100 63.546 g/mol
32.06 g/mol
Cu 2(63.546 g/mol) 100 2(63.546
g/mol) 32.06 g/mol
Cu 66.47
Cu 79.86
14

• Empirical Formula (pg. 245-247)
• Empirical Formula is the simplest ratio of atoms
  present in a molecule
• The empirical formula for C6H6 is _________
• 2. Empirical Formulas may be determined from
  composition data. Here you must determine the
  simplest whole number ratio of _________ for each
  element.
• Determine the empirical formula for a compound
  that contains 0.900 g Ca and 1.60 g Cl.

CH
moles
moles Ca
0.900 g Ca
mol Ca 40.08 g Ca
0.022455 mol Ca
__________________ 0.022455 mol
1.00
mol Cl 35.453 g Cl
moles Cl 1.60 g Cl
0.045130 mol Cl
__________________ 0.022455 mol
2.01
To obtain the simplest ratio of moles, divide by
the smaller value
If values are within 0.1, round to the nearest
whole number
CaCl2
15

• Determine the empirical formula for a compound
  that contains 40.0 C, 6.71 H and 53.3 O.
  When 's are given merely assume that you have
  ______ g of the compound.

100
mol C 12.011 g C
40.0 g C
moles C
3.3302 mol C
__________________ 3.3302 mol
1.00
mol H 1.008 g H
6.71 g H
moles H
6.6567 mol H
__________________ 3.3302 mol
2.00
CH2O
53.3 g O
mol O 15.999 g O
moles O
3.3315 mol O
__________________ 3.3302 mol
1.00
Determine the empirical formula for a compound
that contains 25.9 Nitrogen and 74.1 Oxygen.
This example will show what to do when the mole
ratio is not a whole number.
mol N 14.007 g N
moles N
25.9 g N
1.8491 mol N
_______________ 1.8491 mol
x 2
2
1.00
N2O5
moles O
74.1 g O
mol O 15.999 g O
4.6315 mol O
_______________ 1.8491 mol
x 2
5
2.50
Not within 0.1, multiply each by a so that each
will be a whole
16

• Molecular Formulas from Empirical Formulas-this
  is the true chemical formula of a compound and
  can be determined from the ____________ formula
  and the ___________________ of the compound.
  Practice problem N 248

empirical
molar mass
Step 1 Determine the of empirical formula
units that fit within the molecule
This is obtained from the quotient of molar mass
of compound and the molar mass of the empirical
formula
283.89 g/mol________ 2(30.974 g/mol)
5(15.999 g/mol)
283.89 g/mol________ 141.943 g/mol
2.00
Step 2 Multiply each subscript of the empircal
formula by the calculated above.
Empirical formulaP2O5
P4O10
Pg. 246-247 sample problem L, M are good for
more practice on empirical formulas
17

• pg. 246,7
• L. mole Na 32.38 g Na . mol Na 1.4079 mol Na
  1.99 (2)
• 22.999 g Na 0.70640 mol
• mole S 22.65 g S . mol S 0.70640
  mol S 1.00 (1)
• 32.064 g S 0.70640 mol
• mole O 44.99 g O . mol O 2.8121 mol O
  3.98 (4)
• 15.999 g O 0.70640 mol
• Na2SO4
• M. mol P 4.433 g P . mol P 0.14312 mol P
  1.00 (2) 2
• 30.974 g P
  0.14312 mol
• mol O 5.717 g O . mol O 0.35733 mol O
  2.50 (2) 5
• 15.999 g O 0.14312 mol
  
• P2O5