Date:___________________________________
Explain : Give a detailed account including reasons or causes.
Explore : Undertake a systematic process of discovery.
Interpret : Use knowledge and understanding to recognize trends and draw conclusions from
given information.
Justify : Give valid reasons or evidence to support an answer or conclusion.
Predict : Give an expected result.
Show : Give the steps in a calculation or derivation.
Sketch : Represent by means of a diagram or graph (labelled as appropriate). The sketch should
give a general idea of the required shape or relationship, and should include relevant features.
Solve : Obtain the answer(s) using algebraic and/or numerical and/or graphical methods.
Suggest Propose a solution, hypothesis or other possible answer.
Chemistry Guide – pg.
190
Topic 1:
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 15 of 248
Date:___________________________________
Stoichiometric
relationships
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 16 of 248
Class Work
Date:___________________________________
Classwork:
Ø Write the formulas of the following ionic compounds:
Name
1. Rubidium oxide
Criss-cross
Formula
I. Rbs 0
2. Potassium nitride
KzN
2.
3. Calcium sulfide
3. Cas
4. Copper ( II) Sulfide
4.
Cus
5.
CoI3
6. Zinc oxide
6.
ZnO
7. Manganese (VII) fluoride
7. Mn Ift
8. Chromium (VI) iodide
8. GIG
9. Ammonium iodide
9. NHuI
10. Zinc sulphite
10
5. Cobalt (III) iodide
11. Iron (II) carbonate
11
12. Cobalt (III) nitrate
12
13. Nickel (II) perchlorate
13
14. Copper (I) Phosphate
16. Tin (IV) sulphide
¥ "¥
:
16
Co ( NO 3) 3
.
Ni
.
.
15
1
G11 – Chemistry – SL – Term 1 – 2021/2022
Ee COs
.
14
15. Chromium (II) oxide
Znsoz
.
( cloy)z
Cee , Poy
.
.
GO
sñsz
2
Page 35 of 248
HL p. 36
Am p. 29
Class Work
Date:___________________________________
Ø Write the name for the following compounds:
NaOH
1. Sodium hydroxide
K3PO4
2. Potassium phosphate
Ba (ClO4)2
3. Barium perchlorate
NH4F
4. Ammonium flouride
Cs2 CO3
5. Cesium carbonate
CaSO4
6. Calcium sulfate
HCN
7. Hydrogen cyanide
Fe (NO3)3
8. Iron (III) nitrate
Fe (NO2)3
9. Iron (III) nitrite
Ø Writing the formulas for diatomic molecules:
1.
2.
3.
4.
Oxygen O2
Nitrogen N2
Hydrogen H2
Flourine F2
(For Covalent)
Students need to know the diatomic
elements
Chlorine Cl2
5.
6. Bromine
7. Iodine
Br2
I2
Ø Naming Covalent Compounds
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 36 of 248
HL p. 37
Am p. 30
Class Work / Home Work
Date:___________________________________
Classwork:
Carbon tetrachloride
Diphosphorus pentaoxide
Xxxxx
Tetra phosphorus decaoxide
Xxxx
Sulfur hexaflouride
Dinitrogen trioxide
Xxxx
Sulfur trioxide
Oxygen dichloride
Carbon dioxide
Xxxxx
Iodine monochloride
Carbon disulfide
Sulfur triiodide
Selenium dichloride
Dinitrogen trioxide
Dichlorine heptaoxide
3
Phosphorus trichloride
Nitrogen trihydride
or ammonia
G11 – Chemistry – SL – Term 1 – 2021/2022
Nitrogen tribromide
Xxxxx
Dihydrogen monoxide
Tetra phosphorus decasulfide
Carbon monoxide
Xxxx
Page 37 of 248
HL p. 38
Am p. 31
Home Work
Date:___________________________________
Bos :
V02
Ifs
N 203
NH3
PI }
Si 02
BzBru
Cay
PA3
Nz Os
NIS
SBU
NO
502
Bfs
Cay
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 38 of 248
SL p. 38
HL p. 39
Am p. 32
Date:___________________________________
Class Work
Synthesis
CO2 (g)
Double replacement
3 NaNO3 + Au
3
2
2 H2 O + O 2
FeF2 + I2
G11 – Chemistry – SL – Term 1 – 2021/2022
Single replacement
Decomposition
Single replacement
Page 40 of 248
HL p. 41
Am p. 38
Date:___________________________________
Home Work
Ø Writing a balanced net Ionic equation for reactions in aqueous solutions:
Complete ionic equations: show all chemicals that exist as ions in solution as ions. The equations
reflect all of the ions shown in a normal equation. Only aqueous chemicals are shown as ions!
Note that barium sulfate is NOT written as ions because it is a (s) forming out of solution… in
other words a precipitate
Example:
Regular equation:
Li2SO4 (aq) + Ba(NO3)2 (aq) à 2 LiNO3 (aq) + BaSO4 (s)
Complete ionic equation:
2 Li+ (aq) + SO42- (aq) + Ba2+ (aq) + 2 NO3- (aq) à BaSO4 (s) + 2 Li+ (aq) + 2 NO3- (aq)
Spectator ions: Sometimes a complete ionic equation shows ions that are unchanged by the reaction.
These ions are known as spectator ions. In the above example both lithium ions and nitrate ions
are spectators because the terms 2 Li+ (aq) and 2 NO3- (aq) appear unchanged on both sides of the
equation.
Complete ionic equation with spectator ions circled:
2 Li+ (aq) + SO42- (aq) + Ba2+ (aq) + 2 NO3- (aq) à BaSO4 (s) + 2 Li+ (aq) + 2 NO3- (aq)
Net ionic equations: When the spectator ions are cancelled out of a complete ionic equation, the
equation is greatly simplified! This is known as a net ionic equation.
Ba2+ (aq) + SO42- (aq) à BaSO4 (s)
For the above example the net ionic equation is:
Like regular equations, ionic equations are balanced for atoms and also for charge!
Practice: for each equation, write the complete ionic equation first, then the net ionic equation.
1) Ba(ClO3)2 (aq) + Na2S (aq) à
Complete net
Ba ?aq -12605
BaS (s)
+ 2 NaClO3 (aq)
:
'
,aa
,
,
Net ionic
:
-12
Nate SEE ,→
+
,,
,
Bases, -12%9++2605
Bases)
Ba "caq, -1 S }
2) 2 Na3PO4 (aq) + 3 ZnSO4 (aq) à 3 Na2SO4 (aq) + Zn3(PO4)2 (s)
Complete :
6 Na
Net :
+
+
2 POP
zzn
+
37h2-1+38042 → 6N
2++2,3043lag
lag )
-
→
/
G11 – Chemistry – SL – Term 1 – 2021/2022
-1+3805 Znz ( Poul is,
-
-
-
a
+
>
Znz IPO4) 21st
Page 41 of 248
HL p. 42
Am xx
Date:___________________________________
Home Work
3) SnCl4 (aq) + 2 (NH4)2S (aq)
Complete:
-
Sncetiyce
Net
+
à
4 NH4Cl (aq) +
4NHñ+2S2-→4NHut_ 46
Sn4+ -1252laal→
-
:
SnS2 (s)
caqj
-
+
Snszcs ,
Snszcs )
Complete and balance these two first! The precipitates formed will be aluminum hydroxide and silver
sulfate
4)
5)
2AlBr3 (aq) + 3 Ba(OH)2 (aq) à JALLOH )zcs ,
2 AgNO3 (aq) +
MgSO4 (aq) à
G11 – Chemistry – SL – Term 1 – 2021/2022
-BBaBñzcaq )
Ag2S04lsj+M9lN03)2(
Page 42 of 248
HL p. 43
Am xxx
aq ,
Class Work
Date:___________________________________
Section 1.1 Questions
Worksheet [1]: States of Matter Simulation Lab
Substance Selected: Argon
Solid
Liquid
Gas
Solid particles are
arranged in a fixed
lattice.
Held by strong
intermolecular forces.
Liquid particles are a bit
far away from each
other. Held by weak
intermolecular forces
Gas particles are very far away
from each other. Spreading out
and filling the space in the
container.
No intermolecular forces between
the gas particles
Diagram of
molecules
Sentence
explaining
how
molecules
are moving.
arranged
Book
4. Now use the menu on the right side of the program to select Water and Solid. Next, use the slider on the
bottom of the program to Add Heat. Notice the thermometer at the top of the program. What temperature scales is
this thermometer showing? Kelvin and degrees Celsius
5. What happens to water particles as you increase the temperature?
Increasing the temperature allowed the water particles to move faster.
6. a. What is the melting/freezing point of water in Celsius?
b. What is the melting/freezing point of water in Kelvin?
°
0C
273 K
ÉÉ%
so
-
273
c. Predict the conversion relationship between the Kelvin and the Celsius melting/freezing point of water
showing your work: Temp in K = Temp in C + 273
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 43 of 248
HL p. 44
Am p. 39
Class Work
Date:___________________________________
0
7 a. What is the boiling/condensation point of water in Celsius?
100 C
b. Calculate the boiling/condensation point of water in Kelvin? Show your calculations. Check your answer
using the thermometer on the simulation.
Temp = 100 + 273 = 373 K
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 44 of 248
HL p. 45
Am p. 41
Class Work
Date:___________________________________
Worksheet [3]: HEATING CURVES
Heating curves are usually introduced when discussing intermolecular forces and states of matter. Heat is added to
a substance at a constant rate and the temperature is measured. Analysis of the curve can be related to the concept
of kinetic energy (particle motion).
Exothermic
Depending
variable
OU
Temperature
%
Boiling or
evaporation
Exothermic
Liquid to gas
E.
Solid to liquid
Liquid
Only
Gas
Only
Endothermic
Melting
Endothermic
Solid
Only
Heat or time
Independent variable
1. Label the x- and y-axes on the graph using you independent and dependent variables. Don’t forget the units.
2. On the graph identify the phase(s) present in each segment (A®B, B®C, etc.). You may use the simulation for
assistance. Use water as an example.
3. Is the kinetic energy changing during segment A®B? Explain.
_________________________________________________________________________________________
Yes;
_________________________________________________________________________________________
temperature
is increasing Average kinetic energy of the particles increases.
________________________________________
particles
in the solid state vibrate FASTER.
4. Explain why the temperature is constant during segment D®E even though energy is being added?
During boiling; temperature remains constant.
_________________________________________________________________________________________
Heat added is used to BREAK the intermolecular forces
_________________________________________________________________________________________
liquid will change into gas
_____________________________________
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 45 of 248
HL p. 46
Am p. 42
Date:___________________________________
Home Work
Worksheet [3]: Heating and Cooling Curve Questions
1
The solid and liquid phases of water can exist in a state of equilibrium at 1 atmosphere of pressure and a
temperature of:
①
o
(1) 0 C
Melting (heat added to weaken IMF)
o
o
(2) 100 C (3) 273 C
o
(4) 373 C
T.a.
Freezing pt = melting pt
2
Solid
The table below shows the normal boiling point of four compounds.
Liquid
Woo
Freezing (heat removed to strengthen IMF)
g
When explaining Boiling points always
relate to the strength of the
intermolecular forces
1)
The higher the boiling point
2) the stronger the intermolecular forces
Which compound has the strongest intermolecular forces?
☐
(1) HF(l) (2) CH3Cl(l) (3) CH3F(l)
3
(4) HCl(l)
3) the more heat energy needed to break the
Intermolecular forces
A sample of water is heated from a liquid at 40 oC to a gas at 110 oC
Gas only
Li
qu
id
on
ly
Boiling
Liquid to gas
a)
On the heating curve diagram provided above, label each of the following regions:
Liquid, only QR
ST
Gas, only
Phase change RS
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 46 of 248
HL p. 47
Am p. 43
Date:___________________________________
Home Work
b)
For section QR of the graph, state what is happening to the water molecules as heat is added.
The temperature is increasing ;
Average Kinetic energy increases; the liquid particles are moving FASTER.
c)
For section RS of the graph, state what is happening to the water molecules as heat is added.
Temperature is constant.
Heat added is used to BREAK the intermolecular forces.
liquid is changing into gas. Boiling or evaporation.
4
The graph below represents the heating curve of a substance that starts as a solid below its freezing point.
Melting point is the
temperature at which solid
starts to melt
MP *
.
.
.
-
-
--
.
-
Find it from the y-intercept
What is the melting point of this substance?
(1) 30 oC (2) 55 oC (3) 90 oC (4) 120 oC
0
Base your answers to questions 5 through 8 on the information below.
Given the heating curve where substance X starts as a solid below its melting point and is heated uniformly:
Ga
s
In general
Boiling point
-
-
-
-
-
-
-
-
.
Boiling
Li
qu
-
Melting
⑧
-
-
--
-
-
-
>
So
l
id
Melting point
he
.
-
id
←
-
-
G11 – Chemistry – SL – Term 1 – 2021/2022
e.
Inclined lines (sloped)
Relate temperature to the speed
of the particles and state the
phase of matter only.
Plateau lines
Temperature is constant
Heat added is used to weaken or
break the intermolecular forces
Or heat removed to make or
strengthen the intermolecular forces.
State the phase change melting,
freezing....
Page 47 of 248
HL p. 48
Am p. 44
Home Work
Date:___________________________________
5
Identify the process that takes place during line segment DE of the heating curve. Boiling
6
Identify a line segment in which the average kinetic energy is increasing. AB / CD / EF
7
Using "o" to represent particles of substance X, draw at least five particles as
they would appear in the substance at point F.
8
Describe, in terms of particle behavior or energy, what is happening to substance X during line segment BC.
☐
Temperature remains constant during melting
heat added is used to WEAKEN the intermolecular forces
Solid changes to liquid
.
Base your answers to questions 9 and 10 on the heating curve below, which represents a substance starting
as a solid below its melting point and being heated at a constant rate over a period of time.
9
What is happening to the average kinetic energy of the particles during segment BC?
temperature is constant; KE will remain constant.
10
In which process does a solid change directly into a vapor?
o
(1) condensation (2) sublimation (3) deposition (4) solidification
Sublimation
Mess
Solid
Gas
I.
Deposition
Example
Iacs ,
G11 – Chemistry – SL – Term 1 – 2021/2022
:
→
Ing)
Page 48 of 248
HL p. 49
Am p. 45
Date:___________________________________
Home Work
Worksheet [4]: Mixtures Worksheet
Heterogeneous mixture
Pure substance (compound)
Heterogeneous mixture
Homogenous mixture
Homogenous mixture
Homogenous mixture
Heterogeneous mixture
Pure substance (compound)
8
8
Not a physical technique
Filtration
Filtration
Crystallization
Distillation
Chromatography
Electrolysis
Distillation
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 49 of 248
HL p. 50
Am p. 46
Date:___________________________________
Home Work
Filtration then distillation
Fractional distillation
Filtration
Crystallization
Paper chromatography
Use a magnet.
Iron is magnetic but Aluminium is non magnetic.
Iron will be attracted by a magnet and collected
Place the mixture in a beaker and add water. Stir the mixture using a stirring rod
To allow sodium chloride to dissolve in water. Sand is insoluble in water and will
Precipitate or settle in the bottom of the beaker. Perform filtration where sand will be collected on the
filter paper. Heat the salt solution, until all the water evaporates and salt remains in the beaker.
Yes, air must be condensed first to change all the gas components into liquids.
Perform fractional distillation to separate the different liquids of different boiling points.
The distillate is pure water. Pure water has a fixed boiling point 100 oC.
Take a sample of the collected distillate and place it in a test tube. Heat the sample
until it starts boiling, record the temperature using a thermometer. If the sample boils
at 100 degrees then it is pure water.
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 50 of 248
HL p. 51
Am p. 47
Date:___________________________________
Home Work
①
Worksheet [5]: Naming and Writing the chemical formulas:
(I) Write the formulas for the following compounds:
Hg kDa
1. magnesium cyanide :_______________________________
Brz
2. mercury(II) bromide: _______________________________
3.
Hg
silver nitrate : ______________________________________
AGNOS
4. zinc(II) hydroxide: __________________________________
Znl OH )z
Mq¥É
¥YÉ
#
5. Iron(III) sulfate : ___________________________________
Fez (SO a) 3
Hg%
6. mercury(II) chloride: ________________________________
7. sodium phosphate: __________________________________
Naz Pole
¥E
8. sodium hydroxide : __________________________________
Nao 't
9. ammonium chloride : _________________________________
Nitya
Mgsou
10. magnesium sulfate : __________________________________
⑦
Ng¥pis
-
11. potassium cyanide : ___________________________________
KCN
ii.
12. Lithuim phosphate : ___________________________________
a
kzs
13. potassium sulfide : ________________________________________
⑨
NH¥9
É
"
14. tin(IV) chloride : __________________________________________
Senate
Alf,
15. aluminum fluoride : ________________________________________
¥11
Mgclz
16. magnesium chloride: _______________________________________
Cao
①
17. calcium oxide : _____________________________________________
Fez
3) 3
18. iron(III) carbonate: __________________________________________
⑤
A
:¥§
"
⑦
k¥N
,
%pAoBo£¥¥④sn¥%
ca
14
"
↳I
⑧+¥G11 – Chemistry – SL – Term 1 – 2021/2022
HL p. 52
Am p. 33
Page 51 of 248
"
Date:___________________________________
Class Work/ Home Work
(II) Name the following compounds:
1. CuCl : _________________________________
Copper (I) chloride
Tin (IV) hydroxide
2. Sn(OH)4 : ______________________________
Ammonium carbonate
3. (NH4)2CO3 : _____________________________
Hydrogen sulfate (sulfuric acid)
4. H2SO4 : _________________________________
Sodium cyanide
5. NaCN : _________________________________
6. Na2SO4 : ________________________________
Sodium sulfate
Copper (II) hydroxide
7. Cu(OH)2 : _______________________________
Iron (III) chloride
8. FeCl3 : __________________________________
9. K2CO3 : _________________________________
Potassium carbonate
10. LiNO3 : _________________________________
Lithium nitrate
Sodium phosphate
11. Na3PO4 : _________________________________
Calcium sulfide
12. CaS : ____________________________________
Iron (III) chloride
13. FeCl3 : ___________________________________
14. NiCl2 : ___________________________________
Nickel (II) chloride
15. K2S : _____________________________________
Potassium sulfide
Copper (I) iodide
16. CuI : _____________________________________
17. HF : ______________________________________
Hydrogen flouride
Hydrogen carbonate
18. H2CO3 : ___________________________________
19. K3PO4 : ___________________________________
Potassium phosphate
Sodium sulfate
20. Na2SO4 : __________________________________
Aluminum hydroxide
21. Al(OH)3 : __________________________________
Mercury oxide
22. HgO : _____________________________________
Ammonium sulfate
23. (NH4)2SO4 : __________________________________
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 52 of 248
HL p. 53
Am p. 34
Home Work
Date:___________________________________
Worksheet [6]: Naming and Writing the chemical formulas:
Name the following ionic compounds:
1)
Ammonium chloride
NH4Cl _____________________________________
2)
Iron (III) nitrate
Fe(NO3)3 _____________________________________
3)
Titanium (III) bromide
TiBr3 _____________________________________
4)
Copper (I) phosphide
Cu3P _____________________________________
5)
Tin (III) phosphate
SnPO4 _____________________________________
6)
Magnesium nitrite
Mg(NO2)2 _____________________________________
7)
Lead (IV)sulfate
Pb(SO4)2 _____________________________________
8)
Beryllium hydrogen carbonate
Be(HCO3)2 _____________________________________
9)
Manganese sulfite
Mn2(SO3)3 _____________________________________
10)
Aluminum cyanide
Al(CN)3 _____________________________________
Write the formulas for the following compounds:
÷ *BMqwqj*µ
"
"
11)
chromium (VI) phosphate _____________________________________
12)
vanadium (IV) carbonate _____________________________________
13)
tin (II) nitrite _____________________________________
14)
C. 0203
cobalt (III) oxide _____________________________________
15)
Ti
titanium (II) phosphite _____________________________________
2
16)
vanadium (V) sulfide _____________________________________
17)
chromium (III) hydroxide _____________________________________
18)
LII
lithium iodide_____________________________________
19)
"
lead (II) nitride _____________________________________
20
silver bromide _____________________________________
Snark
3)
:*
⑤t;¥¥
AgBr
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 53 of 248
HL p. 54
Am p. 35
Date:___________________________________
Class Work
Worksheet [7]: Balance the equations below:
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 54 of 248
HL p. 55
Am p. 48
Home Work
Date:___________________________________
Worksheet [8: Balance the following equations and indicate the type of reaction taking place:
3
3
Double replacement
3
2
3
Double replacement
2
3
3
Single replacement
3
2
2
Combustion
(2, 2, 1)
1/2
Decomposition
2
3
3
Single replacement
1
1
1
Synthesis
2
2
Double replacement
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 55 of 248
HL p. 56
Am p. 49
Class Work (mandatory lab)
Date:___________________________________
5. Using a test tube holder, heat the CaCO3 strongly for about 3 minutes. Insert a burning wood splint into the test
tube. If carbon dioxide gas (CO2) is present, it will put the flame out. Note any change in the appearance of the
residue in the test tube
PART C SINGLE REPLACEMENT
6. Stand a clean, dry test tube in the test tube rack. Add about 5 mL of 3 M hydrochloric acid (HCl)
to the tube. CAUTION. Handle acids with care. They can cause painful burns. Do not inhale
any HCl fumes. Now carefully drop a small piece of zinc metal (Zn) into the acid in the test tube.
Observe and record what happens.
7. Using a test tube holder, invert a second test tube over the
mouth of the test tube in which the reaction is taking place.
See the diagram to the right. Remove the inverted tube
after 30 seconds and quickly insert a burning wood splint
into the mouth of the tube. (A “pop” indicates the presence
of hydrogen gas.) Note the appearance of the substance
in the reaction test tube.
8. Add about 5 mL of 1 M copper (II) sulfate (CuSO4) solution to
a
clean, dry test tube. Place a
small amount of zinc metal in the solution. Note the appearance
of the
solution and the zinc before
and after the reaction.
PART D DOUBLE REPLACEMENT
9. Add about 2 mL of 0.1 M Lead Nitrate Pb(NO3)2 to a clean, dry test tube. Next, add about
2 mL of 0.1 M Potassium Iodide (KI) to the test tube. Observe what happens and note any changes in the
mixture
OBSERVATIONS AND DATA
DATA TABLE
Sample
Before reaction
After reaction
A. Synthesis
1. Copper
2. Magnesium
Solid shiny metal
Shiny silvery metal strip
White solid is formed.
White powder substance
B. Decomposition
Thermal decomposition
3. Copper (II) carbonate
C. Single Replacement
4. Zinc + Hydrochloric acid
5. Zinc + Copper (II) sulfate
6. Bromine water + potassium iodide
G11 – Chemistry – SL – Term 1 – 2021/2022
Green powder (solid)
Bubbles form (gas is produced)
Black substance is formed
Zinc is a metal strip
And HCl is a clear solution
Bubbles appear (gas in formed)
Zinc strip decreases in size
Copper sulfate is a blue
aqueous solution
Blue color starts to fade
Zinc strip decreases in size
Bromine is yellow/
orange in color
Potassium iodide is
colorless solution
Page
of
The reaction
turns58
from
orange to brown
248
SL p. 58
HL p. 61
Am p. 53
Class Work (mandatory lab)
Date:___________________________________
D. Double Replacement
7. lead (II) nitrate(aq) + potassium iodide(aq)
Two clear solutions
A yellow precipitate is formed
A yellow precipitate is formed
8. silver nitrate + potassium iodide
Two clear solutions
EQUATIONS:
Write the chemical equation and Balance each of the equations by inserting the proper coefficients where
needed.
PART A SYNTHESIS
1.
(One product is formed)
Copper + oxygen —> Copper (II) oxide
2Cu + O2 —> 2CuO
Shiny metal
2.
white/ greenish
Magnesium + oxygen —> magnesium oxide
2Mg + O2 —> 2MgO
Silver color
White
PART B DECOMPOSITION
(One reactant only)
thermal decomposition (Breaking down using heat)
3. CuCO3 —> CuO + CO2
Green
black
Gas
PART C SINGLE REPLACEMENT
4. Zn + 2HCl —> ZnCl2 + H2
5. Zn + CuSO4 —> ZnSO4 + Cu
6.
Hydrogen gas in experimentally identifies by
the “pop sound” test. Approach a lighted
match near the gas; if it turns off with a pop
sound this indicates that the gas is a
hydrogen gas.
Blue solution
Br2 + 2KI —> 2KBr + I2
PART D DOUBLE REPLACEMENT
7.
Pb(NO3)2 + 2KI —> PbI2 + 2KNO3
Yellow
precipitate
8.
AgNO3 + KI —> AgI + KNO3
yellow
Precipitate
G11 – Chemistry – SL – Term 1 – 2021/2022
Page 59 of 248
HL p. 62
Am p. 54
Date:___________________________________
Class Work (mandatory lab)
CONCLUSIONS AND QUESTIONS:
1.
In Part D: Double Replacement Reaction, state which product is the precipitate. Explain what that indicates
regarding that species solubility.
PbI2 and AgI are the precipitate.
A precipitate is an insoluble solid product.
3.
Balance the equations below using the smallest whole number coefficients.
Identify the type of reaction represented by each equation.
a.2AgNO3(aq) + Cu(s) → Cu(NO3)2(aq) + 2 Ag(s) ↓
Single replacement
b. BaCl2(aq) + Na2SO4(aq) → BaSO4(s) ↓ + 2 NaCl(aq)
c. Cl2(g) + 2 NaBr(aq) →2 NaCl(aq) + Br2(l)
d.2KClO3(s) → 2KCl(s) + 3 O2(g) ↑
G11 – Chemistry – SL – Term 1 – 2021/2022
Double replacement
Single replacement
Decomposition
Page 60 of 248
HL p. 63
Am p. 55
Class Work (mandatory lab)
Date:___________________________________
e. AlCl3(aq) + 3NH4OH(aq) →3 NH4Cl(aq) + Al(OH)3(s) ↓
f.2H2(g) +1 O2(g) → 2 H2O(g)
G11 – Chemistry – SL – Term 1 – 2021/2022
Double replacement
Synthesis
Page 61 of 248
HL p. 64
Am p. 55