Download Chapter 7-8-9

Quarterly Study-guide-MP2- CP Chem M
Bonding-Naming and properties for Ionic and Covalent Bonding, Lewis structures and shapes
Chapter 7-8-9
Multiple Choice: Identify the choice that best completes the statement or answers the question.
1. Which of these is the correct Lewis Dot Diagram for Calcium?
a.
b.
c.
d.
a
b
c
d
e.
f.
g.
h.
e
f
g
h
2. Which of these is the correct Lewis Dot Diagram for Chlorine?
a.
b.
c.
d.
a
b
c
d
e.
f.
g.
h.
3.Which is the charge that results when magnesium
becomes an ion?
a. +2
c. +3
b. -3
d. -2
4. Which is the correct formula for the compound
formed between beryllium and nitrogen?
a. BeN
c. Be3N2
b. Be3N
d. Be2N3
5. What is the correct formula for the compound
formed between magnesium and the phosphate ion?
a. MgPO4
c. Mg3(PO4)2
e
f
g
h
b. Mg3PO2
d. MgP2O8
6. Which is the correct name for the compound CoCO3?
a. Carbon Oxygen
c. Cobalt Carbonate
Carbonate
b. Cobalt (II) Carbonate d. Cobalt Carbonoxide
7. What is the formula unit of sodium nitride?
a. NaN
c. Na N
b. Na N
d. NaN
8. What is the name of the ionic compound formed
from potassium and chlorine?
a. potassium chlorine
c. potassium chloride
9.
10.
11.
12.
13.
14.
15.
16.
17.
b. potassium chlorium
d. potassium chlorate
An ionic bond is a bond between ____.
a. a cation and an anion c. the ions of two
different metals
b. valence electrons and d. the ions of two
cations
different nonmetals
Which of the following is true about the melting
temperature of potassium chloride?
a. The melting temperature is relatively high.
b. The melting temperature is variable and
unpredictable.
c. The melting temperature is relatively low.
d. Potassium chloride does not melt.
Which of the following pairs of elements is most
likely to form a covalent compound?
a. magnesium and
c. oxygen and chlorine
fluorine
d. sodium and
b. lithium and bromine
aluminuim
Which is a physical property of ionic compounds in
their solid state?
a. good conductor of electricity
b. weak attractive forces between ions
c. low boiling point
d. high melting point
Under what conditions can potassium bromide
conduct electricity?
a. only when melted
b. only when dissolved
c. only when it is in crystal form
d. only when melted or dissolved in water
Covalent compounds display which of these
properties?
a. They are hard, brittle solids
b. They have high melting and boiling points
c. They display luster.
d. Their intermolecular forces are relatively weak.
Which is the correct name for the compound N2O4?
a. tetranitrogen dioxide
c. dinitrogen quadoxide
b. dinitrogen tetroxide
d. nitrogen oxide
Which is the formula for the compound sulfur
hexachloride?
a. S6Cl
c. SCl5
b. SCl6
d. S2Cl3
How do atoms achieve noble-gas electron
configurations in single covalent bonds?
a. One atom completely loses two electrons to the
other atom in the bond.
b. Two atoms share two pairs of electrons.
c. Two atoms share two electrons.
d. Two atoms share one electron.
18. How many covalent bonds are formed between two
iodine atoms?
a. 1
c. 3
b. 2
d. 4
19. Which of the following elements can form diatomic
molecules held together by triple covalent bonds?
a. carbon
b. oxygen
c. fluorine
d. nitrogen
20. What molecular shape does the compound CBr4
have?
a. trigonal planar
c. linear
b. tetrahedral
d. bent
21. Choose the correct molecular geometries for the
following molecules or ions below
a. linear
c. trigonal planar
b. bent
d. tetrahedral
22. Why do atoms share electrons in covalent bonds?
a. to become ions and attract each other
b. to attain a noble-gas electron configuration
c. to become more polar
d. to increase their atomic numbers
23. Which molecule has a single covalent bond?
a. CO
b. Cl
c. CO
d. N
24. What causes water molecules to have a bent shape,
according to VSEPR theory?
a. repulsive forces between unshared pairs of
electrons
b. interaction between the fixed orbitals of the
unshared pairs of oxygen
c. ionic attraction and repulsion
d. the unusual location of the free electrons
25. What is the shape of a molecule with a triple bond?
a. tetrahedral
b. pyramidal
c. bent
d. linear
26. Which of the following compounds contains the
Mn ion?
a. MnS
b. MnBr
c. Mn O
d. MnO
27. Which of the following formulas represents an ionic
compound?
a. CS
b. BaI
c. N O
d. PCl
28. Which of the following shows correctly an ion pair
and the ionic compound the two ions form?
a. Sn , N ; Sn N
b. Cu , O ; Cu O
c. Cr , I ; CrI
d. Fe , O ; Fe O
29. In which of the following is the name and formula
given correctly?
a. sodium oxide, NaO
b. barium nitride, BaN
c. cobaltous chloride, CoCl
d. stannic fluoride, SnF
30. Which of the following compounds contains the
lead(II) ion?
a. PbO
b. PbCl4
c. Pb2O
d. Pb2S
31. Which of the following correctly shows a prefix used
in naming binary molecular compounds with its
corresponding number?
a. deca-, 7
b. nona-, 9
c. hexa-, 8
d. octa-, 4
Numeric Response
32. How many electrons are shared in a single covalent bond?
33. How many unshared pairs of electrons does the nitrogen atom in ammonia (NH3) possess?
CHEMISTRY TEST STUDY GUIDE
Ch. 11 – Chemical Reactions
Read over your notes, and rework your homework assignments, labs, quizzes, and tests. You will do
AWESOME on this test if you can do the following things.
Introduction to Chemical Reactions
• Know the difference between a skeleton equation and a balanced equation.
• Explain how the law of conservation of mass relates to atoms in a chemical reaction.
• Know where chemical reactions take place-Everywhere!
Balancing Equations
• Balance a written chemical equation.
• Translate and balance word equations (including states).
Types of Reactions
• Identify the type of reaction.
IDENTIFY THE TYPE OF THE REACTION, THEN BALANCE THE REACTION
1)
___Sb + ___I2 → ___SbI3
2)
___Li + ___H2O → ___LiOH + ___H2
3)
___AlCl3 → ___Al + ___Cl2
4)
___C6H12 + ___O2 → ___CO2 + ___H2O
5)
___AlCl3 + ___Na2CO3 → ___Al2(CO3)3 + ___NaCl
6)
___HNO3 + ___Ba(OH)2 → ___Ba(NO3)2 + ___H2O
7)
___Al + ___Pb(NO3)2 → ___Al(NO3)3 + ___Pb
WORD TO FORMULA, THEN IDENTIFY THE TYPE OF REACTION, THEN BALANCE.
8)
Aqueous solutions of ammonium chloride and lead(II) nitrate produce lead(II) chloride precipitate and
aqueous ammonium nitrate.
9)
Iron metal reacts with aqueous silver (I) nitrate to produce aqueous iron(III) nitrate and silver metal.
10) Solid potassium nitrate yields solid potassium nitrite and oxygen gas.
11) Calcium metal reacts with chlorine gas to produce solid calcium chloride.
12) Fluorine gas added to aqueous potassium chloride produces aqueous potassium fluoride and chlorine
gas.
13) Phosphorous reacts with oxygen gas to produce solid diphosphorous pentoxide.
Chemical Reactions Review – Ch. 8
ANSWER KEY
1.
synthesis
2Sb + 3I2 → 2SbI3
2.
single replacement
2Li + 2H2O → 2LiOH + H2
3.
decomposition
2AlCl3 → 2Al + 3Cl2
4.
combustion
C6H12 + 9O2 → 6CO2 + 6H2O
5.
double replacement
2AlCl3 + 3Na2CO3 → Al2(CO3)3 + 6NaCl
6.
double replacement
2HNO3 + Ba(OH)2 → Ba(NO3)2 + 2H2O
7.
single replacement
2Al + 3Pb(NO3)2 → 2Al(NO3)3 + 3Pb
8.
double replacement
2NH4Cl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2NH4NO3(aq)
9.
single replacement
Fe(s) + 3AgNO3(aq) → Fe(NO3)3(aq) + 3Ag(s)
10. decomposition
2KNO3(s) → 2KNO2(s) + O2(g)
11. synthesis
Ca(s) + Cl2(g) → CaCl2(s)
12. single replacement
F2(g) + 2KCl(aq) → 2KF(aq) + Cl2(g)
13. synthesis
4P(s) + 5O2(g) → 2P2O5(s)
Moles and Moles Calculations
Chapter 10:
Section 10.1: All
Section 10.2: Does not include mole-volume of gas.
Vocabulary:
Mole
1 mole = 1 molar mass (g)
1 mole = 6.02 x 1023 representative particles
Molar Mass (also known as formula mass
Avagadro’s Number
Representative Particles (molecules, atoms etc)
Skills and Mathematical Operations:
a. Convert moles to mass and mass to moles
b. Convert moles to number of representative particles and number of particles to moles.
c. Convert mass to number of particles and number of particles to mass.
Mole Road Map:
Mass
mole
particle
Hint: Review prior worksheets and quizzes. Pay attention to the units of the numbers in the problems.
Remember, you are only solving ratios.
Problems:
1. How many moles are in 220 g of CO2?
2. One mole of (NH4)2HPO4 contains _?_ moles of hydrogen atoms.
3. The atomic mass of sodium is 23. The number of moles in 46g of sodium is ________.
4. The molar mass of ammonia is _________.
5. What is the number of molecules in 4.25 g of ammonia?
6. How many grams of sulfur dioxide are there in 1.20 x 1024 molecules of the compound?
7. How many moles are in 45 molecules of NH3?
Answers:
1. 4 moles
moles
2. 9 moles
3. 2 moles
4. 17
5. 1.5 x 1023 moleules
6. 128 g
7. 7.5 x 10-23
Stoichiometry
Chapter 12
Section 12.1
Section 12.2 Does not include volume-volume calculations. Do understand molecules of product.
Skills:
a. Reading balanced chemical reactions.
b. Using the coefficients in the reaction to determine mole relationships between different substances in the
reaction.
c. Calculate moles from mass and mass from moles.
d. Use coefficients from reaction to relate moles.
Sample Problems:
1. Calculate the number of moles of hydrogen chloride produced from 10 moles of hydrogen.
H2(g) + Cl2(g) → 2HCl(g)
2. Calculate the number of moles of chlorine needed to form 14 moles of iron(III) chloride.
2Fe(s) + 3Cl2(g) → 2FeCl3(s)
3. Calculate the number of grams of nitrogen dioxide that are produced from 4 moles of nitric oxide.
2NO(g) + O2(g) → 2NO2(g)
4. Calculate the mass of oxygen produced from the decomposition of 75.0 g of potassium chlorate.
2KClO3(s) → 2KCl(s) + 3O2(g)
5. Calculate the mass of silver needed to react with chlorine to produce 84 g of silver chloride.
2Ag(s) + Cl2(g) 2AgCl(s)
Answers:
1. 20 moles
2. 21 moles
3. 184 g
4. 29.5 g
5. 63.4 g