Name:
Unit 2
Outline —Chemistry
Chapter 4
Unit 1
2
KEY TERMS
OUTLINE
Day
Exam
Assignment: Read p. xxxii-xxv
p. 552 (safety in the lab)
p. 168-173 (4.1 text)
Do_reading_checks_p._171_&_174
4.1 Notes (slides 1-6)
Assignment: Subatomic Particles Wksht
p. 183 #1, 5, 9, 10
1.
2.
3.
4.
5.
6.
7.
Atom
Atomic number
Subatomic particles
Compound
Element
Ion
Molecule
3
4.1 Notes (slides 7-8)
Bohr & Lewis Diagrams Practice
Bohr Diagram Activity
Assignment: Bohr Diagram Wksht (atoms & ions)
4
4.1 Notes (slides 9-12)
Assignment: Bohr Models & Lewis Structures Wksht
p. 183 #11, 13, 14
Ch. 4.1 QUIZ
4.2 Notes (slides 1-4)
Assignment: 4.2 Names & Formulas of Simple Ionic
Compound Wksht
4.2 Notes (slides 5-8)
Dice activity
Assignment: 4.2 Names & Formulas of Ionic Compound Wksht
8. Valence electrons
9. Covalent bonding
10. Ionic bonding
7
4.2 Notes (slides 9-1 1)
Assignment: Practice Problems P. 197 #1
p. 201 #3,4,5,9,10 (copy out question for #9 &10)
Covalent Naming Assignment Wksht
14. Prefixes
15. Subscripts
8
4.3 Notes (slides 1-6)
Assignment: 4.2 Mixed Chemical Naming Wksht
Subscripts and Coefficients Wksht
p. 215 #1
16.
17.
18.
19.
20.
9
Ch. 4.2 QUIZ
Notes 4.3 (slides 7-1 1)
Balancing Chemical Equations Wksht (start as a class)
Assignment: Balancing Equations Race Wksht
p.2l5#3
5
6
1 1. Chemical formula
12. Multivalent
13. Polyatomic
Chemical equation
Reactants
Products
Coefficients
Law of Conservation
of_Mass
14. Prefixes
15. Subscripts
16.
17.
18.
19.
4.2 Notes (slides 9-11)
Assignment: Practice ProbJems P. 197 #1
p. 201 #3,4,5,9,10 (copy out question for #9 &10)
Covalent Naming Assignment Wksht
4.3 Notes (slides 1-6)
Assignment: 4.2 Mixed Chemical Naming Wksht
Subscripts and Coefficients Wksht
p. 215 #1
Cli. 4.2 QUIZ
Notes 4.3 (slides 7-Il)
Balancing Chemical Equations Wksht (start as a class)
Assignment: Balancing Equations Race Wksht
p. 2l5#3
8
9
of Mass
20. Law of Conservation
Coefficients
Products
Chemical equation
Reactants
11. Chemical formula
12. Multivalent
13. Polyatomic
7
6
5
4.1 Notes (slides 9-12)
Assignment: Bohr Models & Lewis Structures Wksht
p. 183 #11, 13,14
Ch. 4.1 QUIZ
4.2 Notes (slides 1-4)
Assignment: 4.2 Names & Formulas of Simple Ionic
Compound_Wksht
4.2 Notes (slides 5-8)
Dice activity
Assignment: 4.2 Names & Formulas of Ionic Compound Wksht
4
8. Valence electrons
9. Covalent bonding
10. Ionic bonding
4.1 Notes (slides 7-8)
Bohr & Lewis Diagrams Practice
Bohr Diagram Activity
Assignment: Bohr Diagram Wksht (atoms & ions)
Atom
Atomic number
Subatomic particles
Compound
5. Element
6. Ion
7. Molecule
1.
2.
3.
4.
KEY TERMS
12
13
11
Unit 1 Exam
Assignment: Read p. xxxii-xxv
p. 552 (safety in the lab)
p. 168-173 (4.1 text)
Do_reading checks_p._171_&_174
4.1 Notes (slides 1 -6)
Assignment: Subatomic Particles Wksht
p. 183 #1,5,9, 10
-
Chapter 4
OUTLINE
3
2
jy
10
Unit 2 Outline —Chemistry
Name:
Ch. 4. Homework Due
Ch. 4 Test
Assignment: 4.3 Writing and Balancing Equations Wksht
p. 215 #4 (copy out on I line & write formula
underneath;_balance_in_separate_color)
Assignment: Assessment 4.1, 4.2, 4.3
Ch. 4_Review p._216 # 2-8,_ti,_14-21
Review Game
Chapter 4: Atomic Theory Key Terms
Key Term
1. Atom
2. Atomic number
3. Subatomic particles
4. Compound
5.Element
6. Ion
7. Molecule
Definition
Example/Graphic
8. Valence electrons
9. Covalent bonding
10. Ionic bonding
11. Chemical formula
12. Multivalent
13. Polyatomic
14. Prefixes
15. Subscripts
16. ChemicaD equation
17. Reactants
18. Products
19. Coefficients
20. Law of conservation
of mass
4.1 Atomic Theory & Bonding Note Outline
has a neutral charge.
ATOM:
PEN
+
+
(eg.oxygen 0)
ELEMENT:
(eg. oxygen is 02*)
IONS:
MOLECULES: groups of_________________(eg. oxygen molecules are 02)
COMPOUNDS: are made up of at
-Eg. Hydrogen and oxygen are atoms/elements and 1120 is a compound
Structure of an Atom:
slame
Symbol Charge
ocation
nucleus
nucleus
area surrounding
the nucleus
Proton
N.Teutron
lectron
nudus
tomic Mass
I
eI.ctroii
1 AMU
1 AIvIU
1/1836 (0)
neutron
proton
Numbers to Remember:
Protons =
Neutrons
(Mass# proton #).
=
-
Electrons in an atom =
Electrons in an ion =
—
—
(also proton #)
ion charge
Families of the Periodic Table:
Columns of elements are called groups, or families
-similar properties
-All elements in a family have...
bond with other elements in similar ways
have the same number of valence electrons
Family names (on the periodic table!):
(1k, highly reactive)
Group 1 =
(2, reactive)
Group 2=
(1, very reactive)
Group 17 =
(0, unreactive)
Group 18 =
Periods are horizontal rows on the periodic table.
Periodic Table & Ion Formation:
Ions: Atoms that
1.
Cations:
metals
that
EMultivalent: Some metals can have
E2. Anions: Non-metals
to become stable (full valence shells).
& form positive ions (Na)
(Fe 2+ orFe 3+ ).
& form negative ions (0.2)
Periodic Ithie of the Elements
T
•
0.
Es
.97
0
C
—
4.
B
0>40
0.0
11
02
2.
10
3-4
..
—
2+20
.
‘71
.‘,
8
4
88
0,
8
±__
.
.
2+03
Sc
0.
47
72
4,
78
0.
74
9.
70
4,
70
2.
4,
77
0,
78
4-.
ir
‘
Ps
2*
78
3.
0+
00
2+
01
‘!!_
2+.
I.
3.
4
Ge
—
0
P
*14-
*14+
L_
144
P.
4+23 5,24 04232020 3+27 2+05
2*28 2+20
2+21
30
0. V
Cr 0. Mn
F. 0- Co 2- 92 0- Cii I’ Zn
Ga
1..*t
—
00*
—
—
2*
804
Ofl
—
—m
—
—
45.0
478
52.0
54.8
55.0
00.9
087
8L5
55.4
54.7
40.0
90.9
3is5
8404.41
04-43
2+43
7.44
3.44
3+48
2,4?
1.402.483.
37
428 2.20
T
kIo
2+
Mb
Pd”AB
RIi
4+
RU
Cd
los
Y
Zr
4Rb,Sr
bfl*4*
4*2+,e
04*1.52
Wee
1.flm
—
40
R
m
8008
105.0
901.4
005.9
100.4
127.0
105.4
114.8
7
91.2
92.8
40.8
(1001
!‘
28
a
2-0
0—0
,...
‘_
24.3
,
Where are the
following?
0
• Atomic
Number
.
7
24
Si
49’
IC
5
‘He
.
N.
!!__
17:...”
—
b2
7
Ar
+0.9
—
—
90
Br
r
S.
9.?
02
000.9
2,
42611
7.9
00
2,
‘
(4
2*
48
1313
—
90
Cs
Be
I.s
141
Ta
W
Re
0.
F.
48
P.
At
Rn
*5..,
L..
51.4.5.
4.04..
4..
2*4...
1.o,,
lam
0>a...
144.
4*
7.54.,.
I..,
(.5.1.
ll4*E*
4
0)20
135.0
137.5
1085
1795
180.9
183.8
105.0
1462
10052
095.1
0978
209.9
304.4
507.9
030.5
0108>
1210>
2(254
0?
58
007
018..
Pr
Re
t*o.,7
4.5..
4e20).
(200)
2+
48
3.
Ac
004
92
—.
(22?)
(10011
0
— OW
—
‘0
18.0
.
‘8
4
01
3.
2+03
—5’0,
2+
n
1’.
0Sb
I
0.44..
—
PW(II+*
‘
• GrouplFamily
.
2-342-35
As
• Period
-.
ci
.029
o
23
10
• Alkali metals
000
007
005
0(5
III
0)2
004
040
006
55
—
(1000
En
H
Mt
Os
R
(Sub
24*4100
0044.5*’
*
*00
*
—
UiO
100.4..
(Sup
—
Uus
*
—
lSuq
Se
(202)
(4851
7040)
(281)
(278)
(1045)
(000)
(054)
(598)
(2909
4?)
aS4)
7a 2.
Yb 2.
11 24
LIIa
444,447
.5.
Jut
(Sub
• Transition
metals
• Metalloids
005
000
• Non-metals
0
—
(>
000
• Metals
—
• Alkaline earth
metals
• Halogens
3.
55
Ce ‘
24,
140.1
044.040 o,onsasu(C-12a) 12.00.
Any +5(00(5
parentl1458s
is tho mass 01 the 41001
(table of belt known isotope (or
tlwnents that do tot stair naturally.
34-
42
+4*fSO*4.0
140.9-
90 4*0.1
TI,
Pa
7841
‘
U--
*1400
*15.4+
lOW
0
500.0
226.0
24 08 ‘5+: 93- ‘5*
,44-2
l44.2,
S35
60
pm
(142)
0*54
4p
*0f4-
45(41
-O84
Pu
801.
4244)
04: 08
24
58
Dy
.
.2.
0?
2.8
46
.1.4
*04000
2*a
89+00,5.
004515.
8-’5..
4.10.,
90
04(4+
7010OW
‘OW
(347)
(54?)
(050)
94
54
2.
f003)
Bohr Diagrams: show
(2, 8, 8, 18, 18)
Valence electrons: electrons in the•
If the valence shell is full =
If the valence shell is not full =
5(98880,
(208>,
4+
40509
(5*0440
0162
appear in each electron shell around an atom.
ONLY.
What element is this?
°
°
°
®
°°
::•••
dl’
$P’
• Noble gases
1009
‘Si.Ot
157.3
149.8
184.9
147.9
town
1469
4I04.. 0+ 84 3+4? 5,43.483.0402)4008.4922.10334Cm
Bk
Cl
B.
Fm
000
1.7
t[Sm
190*884+ *18800*15515(5*
02371
00.
)3
r•
Ot has 2 + 8 + 8 = 18 electrons, and
therefore 18 protons
eo
lt has 8 electrons gn the outer (valence)
shell
(cations) &
Ionic Bonds: Formed between
Valence electrons are transferred from
Covalent Bonds: Formed between two or more
Valence electrons are
l8p
22
-
(anions).
to
between atoms.
00
0
0
ii:,
0
Lewis Diagrams:
Only
are
shown.
are placed around the element
Dots representing
symbols (on 4 sides, imagine a box around the symbol)
1
are plar”
‘lv, then they
are paired.
Nitrogen Ion
Lewis Diagrams for Ions:
add electron dots to make
and the
Remove
Lewis
or
are placed around each ion.
Diagrams For Covalent Bonds:
valence electrons are drawn to show
All atoms “like” to have a
The shared pairs (“bonding pairs”) of electrons
“lone pairs” are the electrons not shared
of electrons.
Remember:
•
H
+
.
*
e
.
are usually drawn as a straight line
or
.
7
This ‘ine represents
the pair of electrons
shared by the atoms.
Date:
Block:
Name:
4.1
Science 10
-
Subatomic Particles
Assignment
1) Use your periodic table to help you fill in the chart below:
Atomic Mass # # of
# of
Element Name
# of
Protons Neutrons Electrons
#
man
ATOM
a) potassium
20
19
-
b)phosphorus
c)
d)
IC
2
7
2
Ca
40
e) nitrogen
7
f)
5
g) argon
40
h)
10
N/A
3
13
i) chlorine
j)
# of
Electrons
inthe
ION
15
31
3
Ion
Symbol
and
Charge
53
N/A
13
10
20
18
74
2) Why don’t elements “f’ and “g” in question #1 form ions?
3) How many neutrons are in the following atoms:
a.
Carbon-13
c.
Strontium-88
b.
Chromium-51
d.
Boron-lU
4) How many protons are in each of the following atoms/ions:
a.
Li
c.
S 2-
b.
Si
d.
Neon
5) How many electrons are in each of the following atoms/ions:
a.
Li
c.
Barium atom
b.
Se
d.
Magnesium ion
NAME:
0
Element symbol
orbital shells
electron_____
He-4
—
mass number
number of protons
iumber of neutrons
Draw and complete the following Bohr Diagrams for the first twenty elements. Some have been setup for you. Label the families and
number of valence electrons in each group.
BOHR DIAGRAM WORKSHEET
NAME:
j)
0
Element symbol
orbital shells
—
electron_____
He4
—
mass number
number of protons
number of neutrons
Draw and complete the following Bohr Diagrams for the most common ion for each of the elements below. Some have been setup
for you. Be careful whether you are adding or subtracting electrons!
BOHR DIAGRAM WORKSHEET
Name:
Block:_______
Date:
4.1 Bohr Models & Lewis Structures
Science 10
1. Complete the following Bohr & Lewis diagrams.
B
—
Lewis Structure
N=
=
E=
Bohr Diagram
B
P=
He
a
Lewis Structure
C
N=
Bohr Diagram
He
0
Lewis Structure
Mg
Ne
P=
E=
Bohr Diagram
Li
P=
a
Lewis Structure
Ne
p
N=
N=
E=
E=
Bohr Diagram
0
Lewis Structure
P=
N=
Bohr Diagram
a
Li
Bohr Diagram
C
Lewis Structure
P=
p
P=
H
N=
Bohr Diagram
Bohr Diagram
0
Lewis Structure
S
Lewis Structure
Mg
Lewis Structure
H
2. Bohr Diagram Sequences. Draw the beginning atoms and final compound formed.
A) Ionic Bonds. (Show brackets and final ion charges).
i. magnesium and chlorine
B) Covalent Bonds.
i. hydrogen and phosphorous
3. Lewis Diagram Sequences. Draw the beginning atoms and final compound formed.
A) Ionic Bonds. (Show brackets and final ion charges).
i. calcium and chlorine
ii. sodium and fluorine
iii. lithium and phosphorous
B) Covalent Bonds. (Indicate any bonding pairs with either dots or dashes.)
i. hydrogen and nitrogen
ii. hydrogen and carbon
Hi. a diatomic chlorine molecule
4.2 Ionic & Covalent Compound Naming Note Outline
-
Ionic Compounds:
are made up of______
Covalent Molecules:
are made up of atoms
arranged in a crystal structure.
-
-
Naming Ionic Compounds: name of an ionic compound = cation anion-ide
Ex. 1: magnesium and oxygen
Magnesium ox + ide
cation anion-ide
-
-
-
?
2
N
3
Ex.2: what is the name of Ca
=
calcium;
N
nitrogen
Ca
Drop the end of the anion and add —ide
?
2
Ex.3: What is the name of BaC1
Writing formulas for Ionic Compounds
must =
Remember:
phosphide?
for
magnesium
formula
1:
What
is
the
Ex.
Drawing Formula Diagrams: Examples on overhead:
—Lithium nitride
—
—Barium suiphide
Ionic Compound with a Multivalent Metal.
rKMu]Itivalent: some transition elements have
are used after the metal name to
indicate which ion was used
2±
Manganese
549
Ex. 1 What is the formula manganese(llI) sulphide?
Sulphur is g2_
3
This manganese is Mn
SLowest common multiple of 3 and 2 is 6
2 ions
ions and 3 S
•2
You try!
?
4
What is the name for TiF
Titaniumcanbe
25
22
4+
3+
Titanium
S:
Fluorine is
From the ratio in the formula you can find out it is
1 Ti ion and 4 F ions
Polyatomic Ions
Eare made up of several atoms joined together by
has a + or
—The whole
Ex. 1 What is the formula of sodium sulphate?
Ex.2: What is the name of the compound KC1O?
—
charge, not individual atoms.
Na and S0
2
4
K = potassium
Ex.3: What is the formula for Calcium nitrate?
*
2
Ca
C10
and
=
hypochlorite
3
N0
3 show there are two of the nitrate ions present
Note the brackets around NO
Naming Simple Covalent Compounds
E1Prefixes are used before the atom name to indicate the
Ex.l
What
is
the
name
of
the
molecule
in the molecule.
?
6
P
3
Si
Ex.2 What is the chemical formula for the molecule trinitrogen tetrachloride?
How do you know which type it is?
5To determine whether a compound is ionic or covalent:
Examine the formula
•
start with a metal or the ammonium ion
•
start with a non-metal
-
Name:
Science 10
Block:_______
4.2 Names & Formulae of Simple Ionic Compounds
1. For each name, draw the appropriate diagram and write the formula
. Remember to include the charges of the ions in your diagrams.
Diagram (1 mark each)
Name
a) Aluminum sulfide
b) Sodium phosphide
c) Gallium fluoride
d) Sodium chloride
e) Magnesium oxide
f) Beryllium phosphide
Date:
Formula (1 mark)
2. Write the names of the following ionic compounds.
a)
b) MgBr
2
N
3
Li
c) Ag
0
2
d) RbF
e) AgI
3
f) AIBr
2
g) Cal
h) Gal
3
i) Ag
N
3
j) MgSe
k) Ca
2
P
3
0
2
1) Na
m) CdS
n) Sr
2
P
3
-
3. Write the formulas of the compounds containing the following ions.
a)
Na
with
Br
2 with 1
b) Zn
2
c) K with S
d) Al
3 with S
2
e) Ca
2 with 02-
3
3 with P
f) Al
4. Write the ion symbol & charge and the formula of the following ionic compounds.
Formula
Ion symbol & charge
Ionic Compound
a.
strontium nitride
b.
lithium oxide
c.
silver sulfide
d.
barium phosphide
e.
sodium nitride
f.
potassium selenide
g.
cesium sulfide
IL
aluminum nitride
i.
zinc oxide
j.
aluminum iodide
Ic
lithium fluoride
1.
sodium sulfide
2N
Sr
3
2
N
3
Sr
Name:
Block:_______
4.2 Names and Formulas of Ionic Compounds
Science 10
1.
Write
the formulas of the following compounds containing multivalent metals.
Ionic Compound
Ion symbol & charge
a.
copper (I) nitride
3
CuN
b.
c.
d.
e.
iron (UI) phosphide
manganese (II) oxide
manganese (IV) oxide
chromium (NI) bromide
chromium (Ill) bromide
f.
g.
h.
i.
j.
k.
I.
m.
2.
2
O
3
Fe
b.
c.
Fe
3
0
2
4
PbF
2
Eel
d.
2
Hgl
e.
2
N
3
Hg
f.
SnP
g.
MnS
2
MnS
k.
Vc1
5
3
NiS
NiS
I.
3
MoO
m.
6
UCI
n.
7
ReE
o.
2
TiS
j.
Formula
N
3
Cu
Write the ion symbol, charge and the names of the following compounds.
Ion symbol
h.
i.
-
lead (IV) chloride
iron (III) phosphide
tin (DI) sulfide
tin (Dl) nitride
tin (IV) nitride
mercury (II) fluoride
copper (II) selenide
Formula
a.
Date:________
&
charge
Ionic Compound
iron (Ill) oxide
COO
3
a) KCH
p.192) on Polyatomic Ions as you do #3 and #4
of the following compounds with polyatomic ions.
COO)
3
Ca(CH
2
P
3
)
4
(NH
0
4
P
3
(NH4)
Refer to data
3.
c)
book
(or
Write the names
3
Fe(OH)
3
e) AI(OH)
g)
I)
h)
CrO
2
K
4
Cr
2
K
7
0
3 (P0
Mg
)
4
2
)
3
Ca(HCO
2
4. Write the formulas of the following compounds containing polyatomic ions.
Formula
Ion symbol &
Ionic Compound
charge
-
a.
potassium permanganate
b.
sodium chromate
c.
d.
e.
f.
g.
h.
i.
ammonium nitrate
lithium hydroxide
aluminum hydroxide
lead (II) perchiorate
iron (Ill) hydrogen sulfide
vanadium (V) nitrate
magnesium acetate
j.
tin(Dl) cyanide
5. Write the formulas of the following ionic compounds. p. 201 #7)
Formula
Ion symbol &
Ionic Compound
charge
a.
sodium bromide
b.
calcium fluoride
c.
iron(lll) bromide
(I)
iodide
d.
gold
e.
vanadium (V) oxide
f.
molybdenum (Ill) nitride
g.
h.
i.
ammonium phosphate
potassium nitrate
manganese (II) perchlorate
6. Write the names of each of the following compounds. (p. 201 #8— watch out for
roman numeras
Formula
Ion symbol &
charge
a.
b.
LiE
2
MgI
c.
3
0
2
Fe
d.
N
3
Ag
e.
N
3
Au
f.
)
4
Pt(S0
g.
h.
2
C0
2
(NH 3
)
4
3
CsNO
Ionic Compound (only 2 words)
Name:________________________________
Science
Block:_______
4.2 Covalent Naming Assignment
10
(20 marks)
1. Write the chemical names for following COVALENT compounds:
1) PBr
3
2) CF
4
3) SO
3
4) P
5
O
2
5)
2
OBr
6)
2
SC1
7) N
0
2
2.
8)
4
0
2
N
9)
10
S
4
P
10)
3
NI
Write the
1)
formulae of the following COVALENT compounds:
nitrogen tribromide
2) sulphur hexafluoride
3)
dinitrogen tetrasuiphide
4)
oxygen difluoride
5)
carbon
tetraiodide
6) sulphur trioxide
7) phosphorus pentachioride
8) diiodine hexachioride
9) dichiorine monoxide
10) xenon hexafluoride
Date:______________
Name:________________________________
Science 10
Block:_______
4.2 Mixed Chemical Naming
(20 marks)
I or C
1. NF
3
2. LiF
3. NaSO
4
4.CH
3
5. BC1
6. (NH
N
3
)
4
7. NaCO
3
N
3
8. B
COO)
3
Ca(CH
9. 2
10. NaOH
11. P
3
S
4
12. Fl
2
13. CuC1
14. N}LOH
15. 4
P0
3
K
16. Sn(S0
2
)
3
17. FeO
18. Fe
3
0
2
19. SeF
4
20. CO
Chemical Name
Date:
Date:
-
I4ere the subscript ‘2’ refers to the chlorine (Cl) and tells us
that there are two chlorine atoms in tbis compound
4The fact that there is no number beside the calcium (Ca)
atom infers there is only one calcium atom in the
compound
-
iiere t1e sulzscript ‘‘ appiies to both. the 0 atom and
the II atom inside the brackets.
4 There is one calcium atom, two oxygen atoms, and
two hydrogen atoms inthis compound
2NaC1
-
Ierewe have a 2 in front of the formula for sodium
chloride. Because coefficients apply to ALL atoms in
the formula this tells us. that there are two molecules
of NaC.
4OR if we count atoms, there are two sodium (Na) atoms
and two chlorine (Cl) atoms present
A coefficient is a BIG number that is written in front of a compound
and, unlike a subscript, applies to all atoms in the chemical formula.
For example:
2
Ca(0
W
We have also seen that eubcripts are applied to all atoms in a
compound when brackets are use&
2
CaC1
Recall that subscripts are
that are written to the
lower right hand aide of the element of which it belongs. For example:
foyt1a.
NOW, we will. trovlLcC a vew wa of LoolLg at ehe&tcaL forw.t..1ae cu.i4
will lear how to ttse oef
to write he.icel. eqi.atio.s.
We have alreac{t.j dLsc,s&c( the pw-pose of the sbse.rLpt i. a ehetcaL
forwaLLa, av4 we have aLso
L.eoI how t affeots how we I.k.i2rpret the
What ia the difference? When do we use them?
UBCR1PT v’ :COPP1C1NT
Name:
Block______
•
V
.
V
V
(C0
5
A1
)
S3
3 Ba(N0
2
)
3
V V
11
4
C
10 10
4 CllCOOli
V
V
FORMULA
NaC1
2 12
11
C
6
0
3
V
V
atoms
V
Total#Atoms=
V
Total#Atorns
V
V
Total#Atoms
V
Total#Atoina
V
Total#Atoms:
V
V
V
V
V
V
V
V
V
V
ATOMIC TALLY.
V Total#Atoms6
CL 3
Na 3 atoms
V
V
V
V
V
V
V
Please complete the following table by calculating the number of
atoms fri the formula written the way that it is. There will be both
subscripts and coefficients that you will have to take into account
V
V
V
L
C
4.3 Chemical Equations Note Outline
•A Chemical change means new
created.
are
matter is not created or
destroyed; atoms are just rearranged.
Chemical reactions can be written in different ways.
-A
Nitrogen monoxide + oxygen —> nitrogen dioxide
-A
(
2
2NO( + O2( -* 2NO
indicate the ratio of compounds
in the reaction. In the example above, there is twice as
2 than there is 02
much NO and NO
-
State ofmatter
Letters indicate
the state ofeach
compound
(aq) aqueous/
dissolved in water
(s) solid
(1) liquid
(g) gas
-
=
=
=
Writing and Balancing Chemical Equations
of the chemicals
•word equation — uses the
•Example:
0
2
K
->
K
02
+
+
Writing and Balancing Chemical Equations
equation shows only the formulas of the
elements/compounds. Shows atoms, but is
0(s)
2
K
) +02 (g)
3
.K(
chemical equation shows the correct number of each atom
•A
on both sides of the
—Balancing ensures that the number of each atom is the
*Always
ratio
whole
number
the
smallest
use
reaction arrow.
+
02 (g) +
18
2
0
He
Hints for Writing Chemical Equations
to represent single elements.
—Use the chemical
•Be careful of____________ and
4 and S
8
elements such as 02, P
all diatomic elements (hockey
•The”
, ‘2
2
, Cl
2
, Br
2
,N
2
, 02, F
2
stick & puck): H
15
14
16
17
4.0
12.9
fl,
36
3t0
2&
At
Ge
G_.
72.4
38.9
32.1
3—34
32
2-P?18
2—ç 38
elm
74.9
83.8
78.0
2-
Sn
2.
118.7
101.9
127.9
833
94
’ SI
4
Pb
0
Xe
T
•_
L!
-,54
Sb 2- Ti
1
-
0
Kr
Ge
131.3
2,
’At
4
Pe
—
94
Rn
0
Balancing Equations Examples
Balance the following:
Ex. 1
— Sn(N0
4+
)
2
Ex.2
P0 —+
3
K
4
02—*
2
KNO
+
0
2
+H
3 (P0
Sn
)
4
Balancing Chemical Equations
Science 10
Practice Problems n. 211
1 .Balance each of the following skeleton equations.
3
AlT
3 —*
Aid
NaC1 +
NaT +
a.
b.
Li+
LiBr
—+
2
Br
+0
4
c.CH
—
2
*
+
2
C0
HO
d.
PbO—+
e.
C+Ca—*
4
Na
C
2
Na+Ca
f.
+0
8
H
3
C
—
2
*
+
2
C0
g.
2+
)
3
Ca(N0
h.
N—*Na+N
3
Na
2
i.
Mg(ClO +
j
3
Aid
—
2
Pb+0
SO
2
Cu
4
—+
Na —
Al +
2
Cl
0
2
H
4+
CaSO
4+
NaC1O
3
CuNO
Mg
Examples
2.Write the skeleton equation for each of the following reactions. Then balance each of
the equations.
a. nitrogen monoxide + oxygen —* nitrogen dioxide
b. iron(III) bromide
+
sodium hydroxide
—
sodium bromide
+
iron(III) hydroxide
c. methane + oxygen — carbon dioxide + water
d. calcium nitrate
+
potassium carbonate —* potassium nitrate + calcium carbonate
e. phosphorous trichioride + chlorine
—*
phosphorus pentachioride
f. potassium permanganate + nickel(ll) nitrate — potassium nitrate + nickel(II) permanganate
g. iron + copper(II) chloride
—
iron(II) chloride
h. sodium phosphate + barium hydroxide
—*
+
copper
sodium hydroxide + barium phosphate
Balancing Equations Race
1)
O
_O
_H
_C
8
H
3
_C
+
2
O
2)
Al
+
—
2
N
3
Fe
-
—
AIN
3)
I
CI
_NaC
2
_Na+_
-
4)
+_O
-_H
O
_H
O
2
+
—
Fe
O
2
_O
+_C
_H
1
H
6
C
+
5
O
O
2
5)
6)
O
_O
+_C
O_C
_H
2
+
8
H
7
7)
IO
_NaCI+_O
2
_NaC
3
8)
9)
10)
11)
—
—
P0
3
)
4
(NH
+
3
SF
0
3
S
2
L1
+
—
—
4
)
3
Pb(N0
-
—
-
(P0
3
_Pb
4
)
(S0
2
B
3
)
+
—
+
O
7
C
_H
CO
_
1
H
7
÷_
+
2
O
—
3÷
CaCO
—
0
4
P
3
H
-
—
P0
4
(
3
Ca
2
)
+
—
0
3
C
2
H
_S
g
4_Ag+
8
_A
S
2
13)
r
H)
+_FeB
_Fe(O
_KOH
_KBr+
4
3
14)
0
O3
_HNO
0
C
2
4_K
+
_H
_KN
+
3
C
2
16)
17)
18)
19)
20)
O
3
N
4
NH
LIF
12)
15)
—
—
—
—
—
—
4
Pb(OH)
+
)
2
Cr(N0
+
KOH
+
+
0
2
Cu
—
—
4
)
2
Sn(N0
r
6
8
2
8
—
+
—
-
S0
2
)
4
(NH
P0
4
(
3
Co
2
)
—
—
-
44
N
3
Pt
34
HNO
2
Pb0
-
—
—
+
4
CrSO
0
4
P
3
K
4
N
3
Sn
)
3
B(N0
—
+
+
+
—
+
—
1
_AIP4_Zn
_A
_ZnS÷
+
2
P
3
S
http://www. chemfiesta. corn
CuOH
—
O
2
N
4
NH
2
Co(OH)
4
)
2
Pt(N0
HBr
Name:_______________________________
Science 10
Block:_______
Date:
4.3 Writing & Balancing Chemical Equations
(24 marks)
A. Convert each formula equation below into a word equation. (2 marks each)
PO
3
1. H
+
3
MgCO
-
(P0
3
Mg
2
)
4
+
2
CO
+
0
2
H
+Ag
2
2. Zn+AgCD—* ZnCI
B. Convert each word equation below into a formula equation, then balance it.
Include the states of matter subscripts in the equation
1.
Aqueous magnesium chloride and aqueous sodium hydroxide combine to form
aqueous sodium chloride and aqueous magnesium hydroxide.
2. Solid potassium and liquid water combine to form aqueous potassium hydroxide
and hydrogen gas. **note: hydrogen gas is diatomic
C. Balance the following equations.
a)
02
2
CO
HBr
b)
-’2
H
—*
2
Br
c)
K+
O—
2
H
KOH+
I12
positive
positive
negative
shell
shell
electron
electron
C.
0.
02008 McOraw-HC R5ereen limited
B.
ntrleus
proton
A.
neutron
Charge
neutral
Location
nucleus
1
Particle
Subatomic
the subatomic larticle with its charge and
location in an atom?
7. Wttich of the Rllowing correctly matches
0. compound
C. molecUle
Latom
A. ion
itselr?
6. Wttich of the following is the smallest
partIcle of an element that con exist by
._
—
Match the Term on the Iefl with the best
Descriptor on the right. Each Descriptor may be
used only once.
Oescrl,tor
Term
1..__shell A.ahorizorttalrowonthopellodic
table
2.__
petiod
B. a vertical column on the periodic
3..___
table
family
C. an area around the nucleus where
electrons exist
4,
ionic
bonding
U. chemical bonding that resuits tram
a sharing ol valence electrons
5.
covalent
E. chemical bonding that reacts
bonding
when see or more electrons
trarrsters from each atom of a
metal to each atom of a non-metal
bonding
Atomic theory and
Use with textbook pages 16848O.
Assessment
—
atomic number
+
D. 7
C. fi
8.4
A.2
Atomic Theory and Bonding • MIIR
63
number of protons
11. How many valence electrons are there in
this atom?
0. number of electrons
C. mass nutuber + atomic number
B. mass number
A. atomic number
(c) equivalent to?
10. What is the number of subatomic particle
0. (d)
C. (c)
B. (hi
A. (a)
represents a neutron?
9. Which labelled part in the diagram
0
00
liar the following diagram of an atom to
answer questions 9 to Ii.
D. electrons
C. neutrons
B. protons
A. nurici
bonding?
8. Winch of the following are responsible for
Section 4.1
Data
negmbe
positive
positive
neutral
___
electrons
protons and electrons
protons and neutrons
SUBATOMIC PARTICI.E(S)
PRESENT
electrons and neutrons
i.
has etial numbers of electrons and
otons
64
B.
C.
A.
39
39
39
19
Mass
Number
MHR • Section 4.1
—i-——
19
19
19
Atomic
Number
19
20
20
20
Number
of
Neutrons
20
19
20
19
•a
i:
o•
Nh
I
I
Se
\ \
Oil
02008 McGraw HIS
D. a fluorine atom
C. a sodium atom
B. a socliunt
A. a neon atom
Ryeracn limited
16. Which of the following does the Bohr
model represent?
tip
i/_____\
Use the following Bohr model of an element
to answer question 16.
D.Nh
C. So
B. Di
A.Ma
15. Which of the hypothetical elements shown
above represents a metal?
Electrons
of
Assessment
Use the following Lewis diagrams of fur
hypothetical elements to answer
question 15.
Number
Atomic Theory and Bonding
19
39
20
19
Number
of
Protons
correctly for an atom of potassium?
14. Which row of the table is completed
0. L IL and Ill
C. II mid III only
B. I and lii only
A. land II only
11.
nchtde Ca and tW
ametalatranthathaslostelectrons
LJ examples
13. Which of the following describes a cation?
.-___
C
B.
A.
CHARGE
12. Which of the following describes
structure (e)?
Date
—
enilcalf’muia
A. $01
B. SCI
C.
0. StrOll)
E. Sa(Cl0
F. Sn(Cl0
G. Sn(Gl0).
II, Sr(Cl0.
I. Sr(0I0
2
0. Sc,O,
8. SeO,
0.6
8. 4
Date
02008 McGrew+titl Ryomon Limited
Section 42
0. carbon gains electrons, while oxygen
loses electrons
C. oxygen gains electrons, while carbon
loses electrons
B. both oxygen and carbon lose electrons
A. oxygen and carbon share electrons
7. Which of the followiqg occurs when carbon
forms a compound with oxygen?
C. 5
14.2
6. What is the total number of alom.s that
make up iodine pentachioride?
0. magnesium bromide
C. silicon teiralluoride
B. calcium carbonate
A. silver
5. In which of the following rio covalent
bonds hold the atoms together?
C. Sn0
1
A. SrO
compound?
4. Which 01 the following is a covalent
.
._
1._ tin1) chlorate
2.
sulphur dichioride
3._ strontiuni perchlorala
rnn’.Latie
Match each Chemical Name on the left with the
correct Chemical Formula on the right.
Nams and formu’as of
compounds
Use with textbook pages 184-197.
Name
D. 1. II, and 11.1
D. Mn(OX{1
4
B. MnBr
5
0. 1. II. and ill
B, I and ill only
Names and Formulae of Compounds
0. it can form three positive ions
C. it has gained three electrons
B. ii has an ion charge of 3+
A. it has an ion charge of 3—
•
MHR
73
12. In the name arsenic(ill) chloride, what does
the Roman numeral reveal about arsenic?
C. II and iii only
GaOl).
5
CuCI
0
2
Gu
A. I and Ii only
[1
[IL
I.
the ion charge on copper the same?
11. In which of the following compounds is
C. MnSO,
A. Mn0
5
10. In which of the following compounds does
manganese have the highest ion charge?
0. 7
Cr,0
5
)
4
(NH
C. NHCr,O
),
7
B. 4
1,Cr0
(Nl’1
A. 2
Cr
4
NH
5
O
9. Which of the following, is die formula for
the compound formed by arnmonium and
dichromale’?
C. II and 111 only
B. I and Ill only
CeO
2
GaOl)
A. I and 11 only
J!_
IL
U.
Co.
B. in the chemical reaction CuO + CO
2
. which of the following are ionic
3
CuCO
compounds?
Assessment
80
Date
MHR • Section 4.3
0. 1. U, and Ill
C, 11 and 111 only
8. 1 and lii only
A. I and Ii only
Chemical Equations
The total number at each kind of atom at the
start of the reaction Is equal to the total num
tier of each kind ol atom after the reaction.
The total mass of the products is equal to
the total mess attire reactants in a chemIcal
reaction,
The marts is conserved inst chemical
reaction.
B. Which of following describes the law of
conservation of mass?
_.
Match tire Term on the left with the best
Descriptor on the right. Each Descriptor may be
used only once.
Term
Descriptor
1._product
A.aduanicaltttatreactslna
2.
reactant
chemical reaction
3.
8. a chemical that faints in a
coefficient
chemical reactIon
4.
word
C. a chemical change In which
equation
new substances are formed
5.
skeleton V.a chemical equaton that is
equation
written using chemical names
8
.._chemical E.anintegerplacedinlmntof
reaction
a formula in a chemical
7.
chemical
equation
equation
F. a chemical equation that is
written using chemical
formulas
G. aset of cherrrical lormulas
that kientify the reactants
end products In a chemical
maclion
Chmko quatons
Use with textbook pages 202-211.
Name
0.16
V.8
0. 1, 11. and III
C. II and Ut only
-.
HCI + HPO
4
D. 1,4,2, I
LI.,i4.l
B, hydrogen
A. oxygen
carbon dioxide
0 scioe McOrmv4tilI Ryerson Litattad
0. carbon monoxide
.
a solution of sulphuric acid, 4
S0 A
2
H
.
compound. aluminum sulphate, fornis and
bubbles are seen going to tIre surface. Whut
type of gas fronted during this reaction?
13. A piece of aluminum metal is placed in
0. 3
SO and 2
2
Na
NO
Cu
C. Na
S and Cu(NC)
2
)
5
B. CuS and NaNO
5
A. NaS and CuS
12. .A solution of sodium sulpitide is mixed
with a solution of coppesU> nitrate. A
precipitate of copper sulphide is formed in
a solulton of sodium nitrate. What are the
reactants in this chemical reaction?
C. 1,3.5,2
A. I. 4. 5. 1
11. Which of the foflowlnrt sets of coefficients
will balance the equation?
PCIç +
Use the following unbalanced equation to
answer question II.
B. land Ill only
A. I and II only
hydrogen
nitrogen
II.
Ii.
iodine
I.
10. Which of the following are diatom Ic
elements?
8.4
14.2
9. How marry oxygen atoms are there in the
compound lead(lV) bisulphate, Pb(HSO
?
>
4
Assessment