Download grade 11 review

GRADE 11 REVIEW
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Determine the number of significant figures.
Adding and subtracting values using significant figures.
Multiplying and dividing values using significant figures.
Determine the number of electrons, protons, neutrons for neutral elements and
ions.
Draw Bohr diagrams for both neutral atoms and ions.
What are valence electrons and the valence shell?
Draw Lewis diagrams
Define period and group in the Periodic Table.
Describe the properties of the elements in the same group.
Identify the location of the following:
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
d)
halogens
e)
actinoids
f)
lanthanoids
g)
transition metals
Define chemical bonding.
Define covalent and ionic bonding.
Use Lewis dot diagrams to draw ionic compounds and molecular compounds.
Define Periodic Trends:
atomic size, ionization energy
Use electronegativity and electronegativity to determine type of bonds.
Define molecular shape. Define central atom, ligands, lone pair electrons, and
bonding pair electrons.
Determine the molecular shape of molecules. There are four different shapes:
a)
tetrahedral
b)
linear
c)
trigonal pyramidal
d)
angular/bent
You must memorize:
the name of the molecular shapes, angles, and
drawings.
Determine the polarity of molecules.
Naming ionic compounds and molecular compounds.
Balancing Chemical Reactions
Identifying, completing, and balancing different types of chemical equations:
Synthesis, decomposition, single displacement, double displacement,
combustion reactions (complete and incomplete), and neutralization.
Mole calculations.
Percentage composition
Empirical and Molecular formula
Stoichiometric Problems and Percentage yield.
Define unsaturated, saturated, and supersaturated solutions
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Be able to determine if molecular compounds can dissolve in water.
Calculating mass percent.
Molarity and Molar concentration calculations.
Dilution problems.
Solution Stoichiometry.
Define strong acids and bases
List the properties of acids and bases
Define and Arrhenius acid and base.
List the pH scale
Purpose of indicators
Define strong and weak bases. Identify 2 strong acids and 2 strong bases.
Define pressure, STP, kinetic molecular theory of gases, absolute zero
Gas Laws. (Boyle’s Law, Charle’s Law, Combined gas law, Ideal gas law,
density of a gas using the ideal gas law)
Gases and Stoichiometry
REVIEW QUESTIONS
1.
2.
3.
4.
Page 613 # 1 and 2
Page 614 a) - g)
Page 615 a) - e)
Express the following values to Scientific Notation and round to 3 significant
figures.
a)
0.00006764
(Answers:
5.
396500
b)
3.97 x 105)
Determine the number of significant digits in each measurement.
a)
b)
c)
32
891 m
15.764
Answers:
6.
a) 6.76 x 10-5
b)
a)
b)
c)
d)
e)
f)
2
3
5
0.0280
3690
50.80000
d)
e)
f)
3
3
7
Perform the following calculations, rounding off your answer to the correct
number of
significant figures.
a)
b)
c)
9.745 - 4.2
8.33 + 0.4 + 56.358
16.9 x 0.00756
(Answer = 5.5)
(Answer = 65.1)
(Answer = 0.128)
d)
e)
8.
463.8/0.660
580.62 x 1.02/0.7
Determine the number of electrons, protons, and neutrons for the following:
a)
P
(Answers:
9.
15 e, 15 p, 16 n;
b) 10 e, 8, p, 8 n)
Cl
b)
M2+
N
b)
Ar
c)
K+
Use Lewis diagrams to draw the following molecules or ionic compounds.
a)
12.
a)
O2-
Draw the Lewis diagram for the following:
a)
11.
b)
Draw the Bohr diagrams for the following:
a)
10.
(Answer = 703)
(Answer = 9 x 102)
CH4
b)
CS2
c)
CaF2
d)
Na3P
Which element has the largest ionization energy? Explain.
P
Na
Si
(Answer = P, since it has the greatest number of protons and the same number
of shells as the other 2 atoms, it will exert the greatest amount of attraction on its
valence electrons. As a result, it would require more energy to remove the
electron.)
13.
Which element has the smallest electron affinity?
Cs
14.
Li
K
(Answer = Since Cs has the largest radius it will have the weakest force of
attraction on a valence electron. As a result, it will have the smallest electron
affinity)
Using electronegativity values to predict whether the bond between each pair of
atoms will be non-polar covalent, polar covalent, or ionic.
a)
b)
c)
carbon and fluorine
oxygen and nitrogen
chlorine and chlorine
d)
e)
iron and oxygen
manganese and oxygen
(Answers
15.
a) polar covalent; b) polar covalent; c) nonpolar; d) polar covalent;
e) ionic)
Predict the shape and polarity of each of the following molecules. Indicate the
bond angles in each molecule.
a)
b)
c)
CH4 (tetrahedral, nonpolar)
polar)
CHF3 (tetrahedral, polar)
H2S (angular/bent, polar)
(Answers:
d)
PH3
(trigonal pyramidal,
e)
CS2
(linear, nonpolar)
a) tetrahedral, nonpolar, 109.5; b) tetrahedral, polar, 109.5
c) angular bent, polar, less than 109.5
d) trigonal pyramidal, polar, less than 109.5
e) linear, nonpolar, 180)
16.
Draw the shapes of the molecules listed in question 15. How many bonding
electron pairs and nonbonding electron pairs are found around the central atom
of each molecule listed in question 15.
(Answers:
a) 4 bonding pairs; b) 4 bonding pairs; c) 2 bonding and 2
nonbonding; d) 3 bonding and 1 nonbonding; e) 2 bonding)
17.
Name the following ionic and molecular compounds.
a)
b)
c)
C3H8
CuCl2
BeF2
(Answers:
d)
e)
f)
Au3(PO3)2
Na2O
N2O5
g)
h)
i)
Ti(OH)4
FeCl3∙7H2O
Al2S3
a) tricarbon octahydride; b) copper(II) chloride; c) beryllium fluoride;
d) gold(II) phosphite; e) sodium oxide; f) dinitrogen pentaoxide;
g) titanium(IV) hydroxide; h) iron(III) chloride heptahydrate;
i) aluminum sulfide
18.
Provide the chemical formula for the following molecules or ionic compound.
a)
b)
c)
sodium sulfate
aluminum cyanide
tetracarbon decahydrogen
d)
e)
f)
iron(III) sulfate
manganese(IV) carbonate heptahydrate
vanadium(V) carbide
(Answer: a) Na2SO4; b) Al(CN)3; c) C4H10; d) Fe2(SO4)3; e) Mn(CO3)2∙7H2O; f) V4C5)
19.
For the following reactions:
a)
Identify whether the reaction is synthesis, decomposition, single
displacement, double displacement, complete combustion, or incomplete
combustion.
b)
Predict the products
c)
Predict the states of the products
d)
Balance the equation
e)
If the reaction is a double displacement reaction, write out the total ionic
equation, and the net ionic equation.
Reaction 1:
Reaction 2:
Reaction 3:
Reaction 4:
Reaction 5:
Reaction 6:
Reaction 7:
Reaction 8:
Reaction 9:
Reaction 10:
Reaction 11:
Reaction 12:
Reaction 13:
Ca (s) + N2 (g) →
Fe (s) + O2 (g) →
K2O (s) + H2O (l)
→
MnCl5 (s)
→ (heat is added to this reaction)
K2CO3 (s)
→
Fe(OH)3 (s) →
(heat is added to this reaction)
C2H6 + O2 (g)
→
(complete)
C2H6 + O2 →
(incomplete)
Ca (s) + H2O →
Cr (s) + HCl
→
Al (s) + CuCl2 (aq) →
Fe(NO3)2 (aq) + NaOH (aq) →
Ca(OH)2 (aq) + H3PO4 (aq) →
Answers:
Reaction 1: 3 Ca + N2 → Ca3N2 (s), synthesis
Reaction 2: 4 Fe + 3 O2 → 2 Fe2O3 (s), synthesis
2 Fe + O2 → 2 FeO (s)
Reaction 3: K2O (s) + H2O (l) → 2 KOH (aq), synthesis
Reaction 4: 2 MnCl5 → 2 Mn (s) + 5 Cl2 (g), decomposition
Reaction 5: K2CO3 (s) → CO2 (g) + K2O (s), decomposition
Reaction 6: 2 Fe(OH)3 → Fe2O3 (s) + 3 H2O (g), decomposition
Reaction 7: 2 C2H6 + 7 O2 → 4 CO2 + 6 H2O, complete combustion
Reaction 8: 3 C2H6 + 6 O2 → CO + 4 C + CO2 + 9 H2O, incomplete combustion
Reaction 9: Ca + 2 H2O → Ca(OH)2 + H2, single displacement
Reaction 10:
Cr + 2 HCl → CrCl2 (aq) + H2 (g), and
2 Cr + 6 HCl → 2 CrCl3 (aq) + 3 H2 (g), single displacement
Reaction 11: 2 Al + 3 CuCl2 → 2 AlCl3 (aq) + 3 Cu (s), single displacement
Reaction 12: Fe(NO3)2 (aq) + 2 NaOH (aq) → Fe(OH)2 (s) + 2 NaNO3 (aq),
double displacement
Total Ionic Equation:
Fe2+ (aq) + 2 NO3- (aq) + 2 Na+ (aq) + 2 OH- (aq) → Fe(OH)2 (s) + 2 Na+ (aq) + NO3- (aq)
Net Ionic Equation
Fe2+ (aq) + 2 OH- (aq) → Fe(OH)2 (s)
Reaction 13: 3 Ca(OH)2 (aq) +
neutralization
2 H3PO4 (aq)
20.
386 grams C6H12O6 =
_____________________ moles (Answer = 2.14)
21.
3.28 x 1025 molecules of CH4
(Answer = 54.5)
22.
A 500 kg impure sample is 30 % Fe(OH)3, calculate the molecules of
Fe(OH)3 in the sample. (Answer = 8.0 x 1026)
23.
5.56 x 103 grams (NH4)2CO3•5H2O
(Answer = 29.9)
24.
1.25 x 10-2 moles of Ti3(PO4)4
(Answer = 6.54)
=
25.
6.78 moles of NaOH
(Answer = 4.08 x 1024)
=
_______________________ molecules
26.
7.89 mg Al2(SO4)3 =
(Answer = 2.36 x 1020)
___________________ atoms
27.
A 600 g sample is 45 % Cu(OH)2, how many atoms of oxygen are there in this
sample?
(Answer = 3.0 x 24)
28.
5.68 x 1026 atoms of carbon =
(Answer = 123)
29.
A 550 grams of an impure sample is 20 % Fe(OH)2 and 55 % Fe2(SO4)3,
many atoms of iron are there in this sample? (Answer = 1.55 x 1024)
30.
Calculate the percentage composition for the following molecule.
=
→ Ca3(PO4)2 (aq) + 6 H2O (l),
____________________ moles
= _________________ moles
_____________________ grams
_______________ grams of C6H6
FeCl3∙6H2O
(Answer = % Fe = 20.7 ; % Cl = 39.3; % H = 4.5; % O = 35.5)
how
31.
Determine the empirical formula for a compound that is found by analysis to
contain 27.37 % sodium, 1.200 % hydrogen, 14.30 % carbon, and 57.14 %
oxygen. (NaHCO3)
32.
Chemical analysis indicates that a compound is 28.64 % sulphur and 71.36 %
bromine. The molar mass of the compound is 223.94 g/mol. Determine the
molecular formula. (S2Br2)
33.
Given:
___ Ca3P2 + ___ H2O → ___ Ca(OH)2 + ___ PH3
How many moles of H2O must react with 0.56 moles of Ca3P2? (Answer = 3.4)
34.
Given:
___ C4H10 + ___ O2 → ___ CO2 +
___ H2O
How many grams of C4H10 must react with excess oxygen to produce
78 grams of CO2? (Answer = 26)
35.
Given:
___ FeS + ___ O2 → ___ Fe2O + ___ SO2
Calculate the mass of Fe2O that is produced when 37.62 grams of FeS and
22.56 grams of O2 are allowed to react. (Answer = 27.32)
36.
When 15.0 grams of copper and 4.83 grams of sulfur are heated, a
13.7 grams mass of copper(I) sulfide is produced. Calculate the percentage yield
of Cu2S. (Answer = 72.9)
___ Cu + ___ S → ___ Cu2S
37.
The following reaction has a 68.0 % yield.
___ AlCl3 + ___ NaOH → ___ NaAlO2 + ___ NaCl + ___ H2O
Calculate the actual mass of NaCl that is recovered if 18.2 g of AlCl3 reacts with
16.0 g of NaOH. (Answer = 11.9)
38.
Is CCl4 soluble in water? Explain. (Answer: Since CCl4 is tetrahedral it is a
nonpolar molecule. As a result, it will not dissolve in water.)
39.
Is NaCl soluble in water? Explain.
(Answer: soluble. According to the
solubility table, any ionic compounds that contain Na are soluble in water)
Is NH3 soluble in water? Explain.
(Answer: Since NH3 is a trigonal
pyramidal it is a polar molecule. Since water is also polar, NH3 will dissolve in it.)
40.
41.
Is Fe(OH)3 soluble in water? Explain. (Answer: According to the solubility
table when Fe3+ is combined to OH- it is not soluble in water)
42.
A student dissolves 14.0 grams of CuSO4 in 70.0 mL of water, calculate the
concentration of the solution.
(Answer = 1.25)
43.
You have been asked to make 3.0 x 102 mL of 0.20 M NaOH. How would you do
it if you are given solid NaOH? (Answer = 2.4 grams of NaOH in 300 mL H2O)
44.
How many grams of FeCl3 are found in a 5.0 x 102 mL solution of 0.056 M FeCl3?
(Answer = 4.5)
45.
What volume of a 1.64 mol/L aqueous solution contains 12.8 grams of
CoCl3·6H2O?
(Answer = 28.5)
46.
How would you prepare 50.0 mL of 1.00 mol/L of H2SO4 from 3.70 mol/L H2SO4?
(Answer = 13.5 mL of 3 M H2SO4 is mixed with 36.5 mL of H2O)
47.
Given:
___ AgNO3 (aq) +
___ (NH4)2CO3 (aq) → ___ Ag2CO3 (s) + ___ NH4NO3 (aq)
When 75.0 mL of AgNO3 was treated with excess (NH4)2CO3, 2.47 grams of
Ag2CO3 was produced. Calculate the concentration of the original AgNO3
solution.
(Answer = 0.239)
48.
What mass of silver chloride can be produced from 75 mL of 0.25 mol/L AgNO3,
by adding excess MgCl2. (Answer = 1.3)
___ AgNO3 (aq) + ___ MgCl2 (aq) → ___ AgCl (s) + ___ Mg(NO3)2 (aq)
49.
What volume of 1.07 mol/L aqueous NaOH will completely react with
of 0.833 mol/L H3PO4?
(Answer = 58.4)
25.0 mL
___ NaOH (aq) + ___ H3PO4 (aq) → ___ Na3PO4 (aq) + ___ H2O (l)
50.
Calculate the mass of PbS that will precipitate when 6.75 g of Na2S is added to
2.50 x 102 mL of 0.200 mol/L Pb(NO3)2.
(Answer = 12.0)
___ Na2S (aq) + ___ Pb(NO3)2 (aq) → ___ PbS (s) + ___ NaNO3 (aq)
51.
Calculate the mass of Ag2CrO4 that is produced when 25.0 mL of 0.125 M
AgNO3 reacts with 20.0 mL of 0.150 M Na2CrO4.
(0.518)
2 AgNO3 (aq) + Na2CrO4 → Ag2CrO4 (s) + 2 NaNO3 (aq)
52.
53.
54.
55.
56.
57.
58.
59.
Complete Learning Check 2, 4, 5, 6 on page 457 (Answers on pages 659 – 660)
Complete questions 11, 12, and 13 on page 515
(Answers on 662)
Complete questions 11, 14, 16, 19 on page 522
(Answers on page 662)
3
3
Complete questions 1, 2, 3, 5, 10 (1 m = 1000 dm and 1 dm = 1 L) on page 542
(Answers on page 663)
Complete questions 11, 13, 14, 19 on page 549 (Answers on page 663)
Complete question 12 a) – c) on page 550 (Answers on page 664)
Complete questions 22 – 26 on page 556
(Answers on pages 663 – 664)
Complete the following questions on page 560: (Answers on page 664)
a)
31 (Mg + 2 HCl → MgCl2 + H2)
b)
32 (H2 + Cl2 → 2 HCl)
c)
33 (2 NaN3 → 2 Na + 3 N2)
d)
36 (2 Mg + O2 → 2 MgO),
e)
37 on page 560