*
*Determine how many moles are
in 435 grams of NaCl. Significant
figures matter so make sure you
have the correct amount.
*
Mr. Berlin
Luskin Academy
* Objective: I will be able to identify the difference
between ionic and covalent bonds and determine which
atoms will form these bonds.
*
LecturePLUS Timberlake 99
* Molecule: Two or more atoms bonded together to form a
compound.
* Ionic bond: when atoms are attracted to each other due to
ionic states of the atom.
* Covalent bond: when a bond is formed by sharing of electrons
between atoms.
* Single Bond: Shares one pair of electrons in a covalent bond.
* Double Bond: Shares two pairs of electrons in a covalent bond.
* Triple Bond: Shares three pairs of electrons in a covalent bond.
* Mole: The measurement of grams in a formula or atom. (same
as atomic mass. Also, 1 mole = 6.022 x 1023 atoms).
* Chemical Formula: The correct expression for the number of
atoms in a compound.
LecturePLUS Timberlake 99
*
*
Attraction between + ions (cations) and –
ions (anions)
Electrons go from metals to
nonmetals
electron transfer
metal
nonmetal
ion+
Electrons lost = Electrons gain
ion–
*
Formulas of ionic compounds are determined
from the charges on the ions
atoms
ions

Na

+

F : 

sodium fluorine
Charge balance:
–

Na+
: F :  NaF

sodium
fluoride
formula
1+
1-
= 0
*
Write the formula for the ionic compound that
will form between Ba2+ and Cl.
Solution:
1. Balance charge with + and – ions
2. Write the positive ion of metal first, and the
negative ion
Ba2+
Cl
Cl
3. Write the number of ions needed as
subscripts
BaCl2
*Naming Binary Ionic Compounds
Contain 2 different elements
Name the metal first, then the nonmetal as ide.
Use name of a metal with a fixed charge
Groups 1, 2, 3
and Ag, Zn, and Cd
Examples:
NaCl
sodium chloride
ZnI2
zinc iodide
Al2O3
aluminum oxide
*
Complete the names of the following binary
compounds:
Na3N
KBr
Al2O3
MgS
sodium nitride
potassium bromide
aluminum oxide
magnesium sulfide
Transition Metals
Many form 2 or more positive ions
1+
Ag+
2+
Cd2+
silver
ion
cadmium
ion
ion
Zn2+
zinc ion
1+ or 2+
Cu+, Cu2+
copper(I) ion
copper (II) ion
2+ or 3+
Fe2+, Fe3+
iron(II)
iron(III) ion
*
Use a roman number after the name of a metal that forms two
or more ions
Transition metals and
the metals in groups 4A and 5A
FeCl3
(Fe3+)
iron (III) chloride
CuCl
(Cu+ )
copper (I) chloride
SnF4
(Sn4+)
tin (IV) fluoride
PbCl2
(Pb2+)
lead (II) chloride
(Fe3+)
iron (III) sulfide
Fe2S3
*
Complete the names of the following binary
compounds with variable metal ions:
FeBr2
iron (_____) bromide
Cu2O
copper (_____) oxide
SnCl4
___( IV ) ________________
Fe2O3
CuS
________________________
________________________
*
Complete the names of the following binary
compounds with variable metal ions:
FeBr2
iron ( II ) bromide
Cu2O
copper ( I ) oxide
SnCl4
tin (IV) chloride
Fe2O3
CuS
iron (III) oxide
copper (II) sulfide
*Covalent Bonds
Formed between two nonmetals in 4, 5, 6, and
7
Nonmetals have high electronegativity values
Electrons are shared
single bond shares one pair electrons
double bond shares two pairs electrons
triple bond shares three pairs electrons
LecturePLUS Timberlake
14
*
Indicate whether a bond between the following
would be 1) Ionic
2) covalent
____
A.
sodium and oxygen
____
B.
nitrogen and oxygen
____
C.
phosphorus and chlorine
____
D.
calcium and sulfur
____
E.
chlorine and bromine
LecturePLUS Timberlake
15
*
Indicate whether a bond between the following
would be 1) Ionic
2) covalent
1
A.
sodium and oxygen
2
B.
nitrogen and oxygen
2
C.
phosphorus and chlorine
1
D.
calcium and sulfur
2
E.
chlorine and bromine
LecturePLUS Timberlake
16
*
*Share electrons
*Loss or gain electrons
*Held together by actual *Held together by +/sharing of the electrons
*Low boiling/melting
points
*Do not dissolve in
water
*Not brittle
*Not conductive
forces.
*High boiling/melting
points
*Dissolve in water
*Brittle compounds
*Salts
*conductive
*
Gases that exist as diatomic molecules
are H2, F2, N2, O2, Cl2, Br2, and I2. These molecules just keep
their original names.
octets


N


+

N





:::N
N
Triple bond

Example: O2 is just oxygen
LecturePLUS Timberlake
18
*Learning Check
Use the name of the element to name
the following diatomic molecules.
H2
hydrogen
N2
nitrogen
Cl2
_______________
O2
_______________
I2
_______________
LecturePLUS Timberlake
19
*Solution
Use the name of the element to name
the following diatomic molecules.
H2
hydrogen
N2
nitrogen
Cl2
chlorine
O2
oxygen
I2
iodine
LecturePLUS Timberlake
20
*
Two nonmetals
Name each element
End the last element in -ide
Add prefixes to show more than 1 atom
Prefixes
mon
1
penta
di
2
hexa
tri
3
hepta
tetra
4
octa
LecturePLUS Timberlake
21
5
6
7
8
*
Fill in the blanks to complete the following
names of covalent compounds.
CO
carbon ______oxide
CO2
carbon _______________
PCl3
_______chloride
phosphorus
CCl4
carbon ________chloride
N2O
_____nitrogen
_____oxide
22
LecturePLUS Timberlake
*
CO
carbon monoxide
CO2
carbon dioxide
PCl3
phosphorus trichloride
CCl4
carbon tetrachloride
N 2O
dinitrogen monoxide
LecturePLUS Timberlake
23
The attraction of an atom for electrons
is called its electronegativity.
Fluorine has the greatest
electronegativity.
The metals have low
electronegativities.
*
LecturePLUS Timberlake
24
Nonpolar covalent bond
Electrons are shared between atoms
with the same electronegativity values.
Difference = 0
Examples:
N2
Br2
O2
*
LecturePLUS Timberlake
25
*
A.
P2O5
3) diphosphorus pentoxide
B.
Cl2O7
1) dichlorine heptoxide
C.
Cl2
1) chlorine
LecturePLUS Timberlake
26
Nonpolar covalent bond
Electrons are shared between atoms
with the same electronegativity values.
Difference = 0
Examples:
N2
Br2
O2
*
LecturePLUS Timberlake
27
Polar covalent bond
Electrons are shared between different
nonmetal atoms Examples:
O-Cl
O-S
N-Cl
H2 O
*
LecturePLUS Timberlake
28
Identify the type of bond between the
following atoms
A. K-N
1) nonpolar
2) polar 3) ionic
B. N-O
1) nonpolar
2) polar 3) ionic
C. Cl-Cl
1) nonpolar
2) polar
*
LecturePLUS Timberlake
29
3) ionic
A. K-N
3) ionic
B. N-O
2) polar
C. Cl-Cl
1) nonpolar
*
LecturePLUS Timberlake
30
*
Match each set with the correct name:
A.
Na2CO3
1) magnesium sulfite
MgSO3
2) magnesium sulfate
MgSO4
3) sodium carbonate
Ca(HCO3)2
1) calcium carbonate
CaCO3
2) calcium phosphate
Ca3(PO4)2
bicarbonate
3) calcium
B.
LecturePLUS Timberlake
31
*
A.
Na2CO3
3) sodium carbonate
MgSO3
1) magnesium sulfite
MgSO4
2) magnesium sulfate
Ca(HCO3)2
3) calcium bicarbonate
CaCO3
1) calcium carbonate
Ca3(PO4)2
phosphate
2) calcium
B.
LecturePLUS Timberlake
32
Chemical reactions are classified into
four general types
Combination
Decomposition
Single Replacement
Double Replacement
*
LecturePLUS Timberlake 99
Two or more elements or simple
compounds combine to form (synthesize)
one product
A + B
AB
2Mg + O2
2MgO
2Na + Cl2
2NaCl
SO3 + H2O
H2SO4
*
LecturePLUS Timberlake 99
One substance is broken down (split)
into two or more simpler substances.
AB
A + B
2HgO
2Hg + O2
2KClO3
LecturePLUS Timberlake 99
*2KCl
+ 3 O2
Classify the following reactions as
1) combination or 2) decomposition:
___A. H2 + Br2
2HBr
___B. Al2(CO3)3
Al2O3 + 3CO2
___C. 4 Al + 3C
Al4C3
*
LecturePLUS Timberlake 99
*
Classify the following reactions as
1) combination or 2) decomposition:
_1_A. H2 + Br2
2HBr
_2_B. Al2(CO3)3
Al2O3 + 3CO2
_1_C. 4 Al + 3C
Al4C3
LecturePLUS Timberlake 99
*
One element takes the place of an
element in a reacting compound.
A + BC
AB + C
Zn + 2HCl
ZnCl2 + H2
Fe + CuSO4
FeSO4 + Cu
LecturePLUS Timberlake 99
Two elements in reactants take the place
of each other
AB + CD
AD + CB
AgNO3 + NaCl
AgCl + NaNO3
ZnS
ZnCl2 + H2S
+ 2HCl
*
LecturePLUS Timberlake 99
Classify the following reactions as
1) single replacement
2) double replacement
__A. 2Al + 3H2SO4
Al2(SO4)3 + 3H2
__B. Na2SO4 + 2AgNO3
Ag2SO4 + 2NaNO3
__C. 3C + Fe2O3
2Fe + 3CO
LecturePLUS Timberlake 99
*
Classify the following reactions as
1) single replacement
2) double replacement
1_A. 2Al + 3H2SO4
2_B. Na2SO4 + 2AgNO3
1_C. 3C + Fe2O3
LecturePLUS Timberlake 99
Al2(SO4)3 + 3H2
* Ag SO
2
4
+ 2NaNO3
2Fe + 3CO
A reaction in which a compound (often
carbon) reacts with oxygen
C + O2
CO2
CH4 + 2O2
CO2 + 2H2O
C3H8 + 5O2
3CO2 + 4H2O
C6H12O6 + 6O2
6CO2 + 6H2O
*
LecturePLUS Timberlake 99
Reactions that involve a loss or gain of electrons
Occurs in many of the 4 types of reactions and combustion
Important in food metabolism, batteries, rusting of metals
*Oxidation and
Reduction
LecturePLUS Timberlake 99
*Requirements for OxidizationReduction
Electrons are transferred
Two processes occur
Oxidation = Loss of electrons (LEO)
Zn
Zn2+ + 2e-
Reduction = Gain of electrons (GER)
Cu2+ + 2e-
LecturePLUS Timberlake 99
Cu
In organic and biological reactions
oxidation = Loss of H
reduction = Gain of H
*
LecturePLUS Timberlake 99
*
4 Fe + 3 O2
2 Fe2O3
Fe and O2 4 mole Fe and 3 mole O2
3 mole O2
4 mole Fe
Fe and Fe2O3 4 mole Fe and 2 mole Fe2O3
2 mole Fe2O3
4 mole Fe
O2 and Fe2O3 3 mole O2 and 2 mole Fe2O3
LecturePLUS Timberlake 99
2 mole Fe2O3
46
3 mole O2
3 H2(g) + N2(g)
2 NH3(g)
A. A mole factor for H2 and N2 is
1) 3 mole N2
N2
2) 1 mole N2
1 mole H2
3 mole H2
3) 1 mole
2 mole H2
B. A mole factor for NH3 and H2 is
1) 1 mole H2
2 mole NH3
LecturePLUS Timberlake 99
2) 2 mole NH3
3 mole H2
*
47
3) 3 mole N2
2 mole NH3
3 H2(g) + N2(g)
2 NH3(g)
A. A mole factor for H2 and N2 is
2) 1 mole N2
3 mole H2
B. A mole factor for NH3 and H2 is
2) 2 mole NH3
*
3 mole H2
LecturePLUS Timberlake 99
48
*Learning Check S2
4 Fe
+
3 O2
2 Fe2O3
How many moles of Fe are needed to react with
12.0 mole of O2?
1) 3.00 mole Fe
2) 9.00 mole Fe
3) 16.0 mole Fe
LecturePLUS Timberlake 99
49
4 Fe
+
3 O2
12.0 mole O2 x
Fe
2 Fe2O3
4 mole Fe = 16.0 mole
*
3 mole O2
LecturePLUS Timberlake 99
50
*
* Formula mass is the sum of the atomic mass weights of each
element in a empirical formula. To calculate, simply add up the
average atomic mass of each atom.
* Example:
* NaCl
Na
=
22.99 grams
*
Cl
=
35.45 grams
* total
58.44 grams
* Example:
* BeCl2
Be
=
*
2x
Cl =
* total
9.01 grams
70.90 grams
79.91 grams
*
The reaction between H2 and O2 produces
13.1 g of water. How many grams of O2
reacted?
Write the equation
H2 (g)
+ O2 (g)
H2O (g)
Balance the equation
2 H2 (g)
LecturePLUS Timberlake 99
+ O2 (g)
53
2 H2O (g)
*
1. Read an equation in moles
2. Convert given amount to moles
3. Use mole factor to give desired
moles
4. Convert moles to grams
grams (given)
LecturePLUS Timberlake 99
moles (given)
grams (desired)
54
moles (desired)