Midterm Review Packet for
General Chemistry
COVERING:
Unit
1
2
3
4
5
6
Chapter/Section
2
5.1 – 5.5, 10.1
4.1 – 4.2, 5.6, 6.1
6.2 – 6.6
8.1 – 8.3, 8.5, 15.1-15.2
7.1 – 7.5
Subject
Measurements
Quantum Theory
Elements, Periodic Table-Trends, Octet Rule
Nomenclature and Bonding
Chemical Equations and Reactions
Chemical Quantities
This study guide is NOT intended to teach - it should jog your memory so that you recall all the
many topics that were learned during the first semester. It includes questions on each section,
subject, and selected labs. The results should act as a guide to indicate topics which you
already know and only need to review, topics on which you are a little rusty and need to
practice, and topics which you still need to master with more intensive study. Do not wait until
the last minute to ‘cram’ for the midterm. You should start now doing a little at a time at home.
Take your book and your classroom notes/ work-packets/ old labs home with you and use them
to help review and study for the midterm.
UNIT 1: Chp. 2 Measurement
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Units of Measurement
Measured Numbers and Significant Figures
Prefixes and Equalities (Metric System)
Writing Conversion Factors (Dimensional Analysis)
Problem Solving (Dimensional Analysis)
MULTIPLE CHOICE: Pick the answer which BEST answers the questions or completes the statement.
Match Questions 1-3 to the pictures below.
1
A.
1. beaker
B.
C.
D.
E.
C.
2. device which would give the LEAST accurate volume measurement
C.
3. The gram is the metric base unit of :
A) temperature
B) length
C) weight
D) mass
E) volume
5. What is the correct reading for the volume of liquid in the measuring device
seen at the right?
A) 10.2 mL
B) 9 mL
C) 8.0 mL
D) 8 mL
E) 12.0 mL
6. Which of the following is correct concerning the use of significant figures?
A) sig figs create uncertainty
B) sig figs record uncertainty
C) sig figs increase uncertainty
D) sig figs decrease uncertainty
E) sig figs have nothing to do with uncertainty
7.
Three students were asked to determine the volume of a liquid by a method of their choosing. Each
did three trials. The table below shows the results.
Student
A
B
C
Average
(mL)
24.7
24.3
24.3
Average
deviation
± 0.0 mL
± 0.2 mL
± 0.2mL
%
Error
0.4
0.4
2
Which students' measurements represent data that is closest to the accepted value?
A) A and B
B) A and C
C) B and C
D) C only
E) A only
8. 1 milliliter is the same volume as ___
A) 1000 L
B) 1 cm3
2
C) 1 gram
D) 100 L
E) 10 cm
9. 85.0 seconds is the same as ___ centiseconds.
A) 0.000 0850
B) 8.50 x 104
C) 8.50
D) 8,500
E) 8.5 x 109
10. 250 mL is the same as 2.50 __?
A) liters
B) microliters
C) deciliters
D) cubic centimeters
E) cubic meters
11. Which of the following is set up correctly to convert
A) km
1m
hr 1000 km
60 min
1 hr
B) km
1 km
hr 1000 m
1 hr
60 min
C) km 1000 m
hr 1 km
1 hr
60 min
𝑘𝑚
ℎ𝑜𝑢𝑟
to
𝑚
𝑚𝑖𝑛
?
D) km 100 m
hr 1 km
60 min
1 hr
E) km
hr
1 hr
60 min
1m
100 km
UNIT 2: Chp. 5.1-5.5, 10.1: Quantum Theory
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Electromagnetic Radiation
Atomic Spectra and Energy Levels
Sublevels and Orbitals
Drawing Orbital Diagrams and Writing Electron Configurations
Electron Configurations and the Periodic Table
1. When an electron jumps up to a higher energy level it
A) emits a photon
B) creates an emission spectrum
C) absorbs energy
D) causes the atom to have less energy
E) This is a trick!, electrons cannot jump "up" energy levels, they can only jump "down"
3
The energy of a visible photon of electromagnetic radiation is greater than that of ________
2.
A) cosmic radiation
B) infrared radiation
C) gamma radiation
D) ultraviolet radiation
E) X-radiation
3.
4.
An s sublevel can hold___ electrons and has a ___ shape
A) 6, figure-8
B) 8, square
C) 2, spherical
D) 10, flower
The number of electron levels (not sublevels) in a magnesium atom is ________.
A) 1
B) 2
D) 4
C) 3
E) 18, dumbbell
E) 5
5.
The maximum number of electrons that may occupy the third electron energy level is ________.
A) 10
B) 2
C) 8
E) 32
D) 18
6.
A 3-d orbital can hold ____ electrons.
B) 10
A) 2
7.
C) 8
D) 6
E) 18
The following orbital notation for carbon violates ___.
A) Pauli exclusion principle
B) the Aufbau principle
C) Hund's rule
D) the octet rule
E) every law known to man
8. How many valence electrons would be in an atom with the following electron configuration?
1
2
A) 5
2
3
3
4
3
B) 15
4
C) 10
D) 7
E) 2
9. The abbreviated electron configuration for a boron atom (Atomic number = 5) is ________.
A) 1s2 2s2 2p6
C) 1s2 2s2 2p1
D) [Ne]2s2 2p1
E) [H]2s2 2p1
B) [He]2s2 2p1
10. What neutral element is represented by the following electron configuration?
1s2 2s2 2p6 3s2 3p6 4s2 3d1
A) Sc
B) Ar
4
C) Ca
D) F
E) La
UNIT 3: Chp. 4.1-4.2, 5.6, 6.1:
Elements, Periodic Table-Trends, Octet Rule
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Elements and Symbols
The Periodic Table
Periodic Trends of the Elements
Octet rule
1. In the modern Periodic Table, ___ are horizontal and ___ are vertical.
A) periods, groups
B) groups, periods
C) families, groups
D) periods, series
E) families, groups
Questions 2 thru 7 refer to the following figure:
5
2. Is(are) in the s - block.
A) A
B) B and C
C) C
D) D and E
E) E
5. Is a noble gas.
A) A
B) B
C) C
D) D
E) E
3. Is in period 3.
A) A
B) B
C) C
D) D
E) E
6. NOT representative elements.
A) B and C
B) A, D, and E
C) A only
D) D and E only
E) B, C, and D
4. Is (are) transition elements.
A) A and B
B) D and E
C) E only
D) B and C
E) C and D
7. Is (are) metalloids.
A) A and B
B) B and C
C) D and E
D) A
E) D only
8. In general, ionization energy tends to ___ left to right across a period.
A) remain the same
B) increase
C) decrease
D) decrease then increase
E) who knows?!, it can’t be predicted
9. In genral, Electronegativity
A) increases from left-to-right across a row
B) decreases from left-to-right across a row
C) stays the same down a column
D) increases down a column
E) stays the same from left-to-right across a row
10. Which of the following neutral atoms has the largest radius?
A) As
B) Ge
C) Ga
D) Ca
E) K
UNIT 4: Chp. 6.2-6.6: Nomenclatue and Bonding
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Octet Rule and Ions
Ionic and Covalent Compounds
Naming and Writing Ionic Formulas
Polyatomic Ions
Naming and Writing Covalent Formulas
6
1. Which of the following represents an ionic bond?
A) NO2
B) H2S
C) CO
D) XeF4
E) NaCl
2. Which of the following compounds contains a cation with a +2 charge?
A) PbO
B) OF2
C) SO2
D) Al2O3
E) Fe(OH)3
3. Which compound contains both covalent and ionic bonds?
A) Al2O3
B) Li2O
C) Cu(NO3)2
D) C6H12O6
E) AlP
4. Which of the following is the correct name for NO2
A) nitride
B) nitrogen oxide
C) mononitrogen oxide
D) nitrogen dioxide
E) nitrite
5. Which of the following is the correct formula for potassium bromide?
A) KBrO3
B) K2BrO34
C) KBr
D) K2Br
E) KBr2
6. Which of the following is the correct formula for copper (II) nitride?
A) CuN
B) Cu3N2
C) Cu2N3
D) CuNO2
E) Cu(NO3)2
7. Which of the following is the correct name for Sc(PO3)3?
A) scandium phosphorus trioxide
B) scandium phosphate
C) scandium phosphite
D) scandium phosphide
E) scandium phosphorus oxide
8. What is the correct formula for oxygen difluroide?
A) OF2
7
B)
C)
D)
E)
O2F2
O2F
2 OF
OF
9. Which of the following chemical formulas represents a molecule with a covalent bond?
A) MgCl2
B) CO2
C) NaF
D) PbS2
E) AlBr3
10. Which of the following does NOT obey the octet rule?
A) O2−
B) Mg2+
C) Fe3+
D) P3−
E) I2−
UNIT 5: 8.1 – 8.3, 8.5, 15.1 – 15.2
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Chemical Equations
Types of Reactions
Redox Reactions
True/False
Indicate whether the statement is true or false.
1. The sum of the oxidation numbers of all atoms in a neutral compound is 0.
A) True
B) False
2. Which type of reaction can be recognized by the general pattern
A) combustion
B) combination
C) single replacement
D) double replacement
E) decomposition
?
3. Which types of reactions are essentially opposites of one another?
A) combustion and combination
B) single replacement and double replacement
C) combination and single replacement
D) combination and decomposition
4. What are the correct coefficients when this equation is balanced? K + Br2  KBr
A) 1, 1, 1
8
B)
C)
D)
E)
1, 2, 1
2, 1, 2
2, 1, 1
2, 2, 2
5. Redox reactions involve the _____ of electrons.
A) combining
B) sharing
C) substitution
D) transfer
E) manufacture
6. When the following equation is balanced with the smallest whole number coefficients, what is
the coefficient for O2?
C3H8(g) + O2(g) → CO2(g) + H2O(g)
A)
B)
C)
D)
E)
4
5
10
7
None of the above
7. Which observation does NOT indicate that a chemical reaction has occurred?
A) formation of a precipitate
B) production of a gas
C) evolution of energy
D) change in total mass of substances
E) formation of bubbles
8. What is oxidized and what is reduced in the following unbalanced equation?
C3H8(g) + O2(g) → CO2(g) + H2O(g)
A)
B)
C)
D)
E)
O2 is reduced and the carbon in C3H8 is oxidized
the carbon in C3H8 is reduced and O2 is oxidized
in the compound C3H8, the hydrogen is oxidized and the carbon is reduced
the hydrogen in C3H8 is reduced and O2 is oxidized
the hydrogen in C3H8 is oxidized and the O2 is reduced
9. What type of reaction is shown for the following unbalanced equation?
C3H8(g) + O2(g) → CO2(g) + H2O(g)
A) single-replacement
9
B) double-replacement
C) combustion
D) combination
10. Which of the following gives the correct balanced equation for the following reaction?
Al(s) + Br2(l) → AlBr3(s)
A)
B)
C)
D)
E)
Al(s) + 3 Br2(l) → AlBr3(s)
Al(s) + 2Br2(l) → AlBr3(s)
3Al(s) + Br2(l) → 3AlBr3(s)
2Al(s) + Br2(l) → Al2Br2(s)
2 Al(s) + 3 Br2(l) → 2AlBr3(s)
UNIT 6: 7.1 – 7.5
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The Mole
Molar Mass and Calculations
% Composition and Empirical Formulas
Molecular Formulas
1) One mol of silicon contains how many atoms of silicon?
A) 28.093
B) 14
C) 6.022 × 1023
D) 3 × 10−10
E) 6.022 × 10−23
2) The number of particles in 1 mol of a substance is called ___.
A) molar mass
B) formula mass
C) Avogadro's number
D) relative atomic mass
E) moles in 6.022 × 1023 grams of an element.
3) How many grams of glucose (C6H12O6) are in 3.50 mol of glucose?
A) 426
B) 103
C) 631
D) 180.
E) 50.7
4) Fructose has the formula C6H12O6. How many moles of fructose are there in 0.100 g of fructose?
10
A) 5.55 × 10-4 mol
B) 5.55 mol
C) 180. mol
D) 0.0555 mol
E) 18.0 mol
5) What is the molar mass of lactic acid, C3H6O3?
A) 90.00
B) 90.08
C) 45.02
D) 29.02
E) 180.0
6) 1.00 mol of calcium hydroxide has how many oxygen atoms? The formula for calcium hydroxide is
Ca(OH)2.
A) 1.20 × 1023
B) 6.02 × 1024
C) 1.20 × 1024
D) 6.02 × 102
E) 3.01 × 1024
7) Oxygen gas, O2, has a molar mass of ________ g.
A) 32.00
B) 8.000
C) 48.00
D) 16.00
E) 64.00
8) What is the mass, in grams, of 4.00 x 1022 helium atoms?
A) 4.00
B) 0.0644
C) 96.3
D) 2.66
E) 0.266
9) What is the mass, in grams, of 6.022 x 1023 molecules of water?
A) 1.000 × 1023
B) 18.02
C) 1.000
D) 1.802 × 1024
E) 6.022 × 1025
10) What is the mass, in grams, of 2.75 mol of sodium hydrogen carbonate, NaHCO3?
A) 52.0
11
B) 250.
C) 84.0
D) 58.0
E) 231
11) How many moles of oxygen atoms are in 1 mole of silver nitrate, AgNO3?
A) 0
B) 1
C) 2
D) 3
E) 6.022 x 1023
12) How many hydroxide polyatomic ions are in 1 mole of aluminum hydroxide, Al(OH)3
A) 1.807 x 1024
B) 3
C) 6.022 x 1023
D) 1.204 x 1024
E) 2.007 x 1023
13) How many chlorine atoms are in 121 g of rubidium chloride RbCl?
A) 121
B) 6.022 x 1023
C) 1.00
D) 1.204 x 1024
E) none
14) The percent composition, by mass, of calcium hydroxide[Ca(OH)2] is ___.
A) Ca = 69.09%, O = 27.58%, H = 3.48%
B) Ca = 70.20%, O = 28.03%, H = 1.77 %
C) Ca = 82.49%, O = 16.47%, H = 1.04 %
D) Ca = 33.33%, O = 33.33%, H = 33.33%
E) Ca = 54.09%, O = 43.18%, H = 2.73%
15) Calculate the empirical formula of a substance composed of 2.06 g of calcium, 2.66 g of
chromium, and 3.28 g of oxygen.
A) CaCrO
B) Ca(CrO)2
C) CaCrO4
D) CaCr2O7
E) Ca2CrO4
16) Calculate the empirical formula of a substance composed of 51.7% carbon, 6.95% hydrogen, and
41.3% oxygen
A) CHO
B) C5H8O3
C) CH2O
D) C2H3O
E) C4H7O3
12
17) Fructose, the carbohydrate found in honey and fruits, has a molar mass of ≈ 180 g and an empirical
formula of CH2O. What is its molecular formula?
A) CH2O
B) CHO
C) C6H12O6
D) C5H8O3
E) C2H6O
18) Mevalonic acid is 48.64% carbon, 8.16% hydrogen, and 43.20% oxygen. If mevalonic acid has a
molar mass of about 148 g, what is its molecular formula?
A) C6H12O4
B) CH2O
C) CH3O
D) C2H3O
E) C3H6O2
19) The empirical formula of dinitrogen tetraoxide is ___.
A) N2O3
B) NO3
C) N2O4
D) NO2
E) N2O
13
Solubility Rules
Soluble Compounds
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all ammonium (NH4+) compounds
all Group I compounds
all nitrates (NO3─) compounds
all acetate (CH3COO─) compounds
all chlorate (ClO3─) compounds
all perchlorates (ClO4─)
chlorides - except Ag+ Pb2+ , Hg22+
bromides - except Ag+ Pb2+ , Hg22+
iodides - except Ag+ Pb2+ , Hg22+
sulfates (SO42─) - except Ag+, Pb2+ , Ba2+, Sr2+, Ca2+
Insoluble Compounds
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sulfides – except Ba2+, Ca2+, Sr2+
carbonates (CO32─)
phosphates (PO43─)
hydroxides (OH─) – except Ba2+, Ca2+, Sr2+
14
Activity Series of Metals For Single Replacement Reactions
MOST REACTIVE ELEMENTS
(easiest to oxidize, hardest to reduce)
Metal
Lithium
Potassium
react with liquid water, steam, or acids by
Barium
displacing Hydrogn
Strontium
Calcium
EX: Ca(s) + 2 H20(l) → Ca(OH)2 (aq) + H2↑
Sodium
Magnesium
Aluminum
Manganese
do NOT react with liquid water
Zinc
react only with steam or acids by displacing hydrogen
Chromium
Iron
EX: Zn(s) + 2 H2O (g) → ZnO (s) + H2↑
Cadmium
Cobalt
Nickel
do NOT react with steam
Tin
react only with acids by displacing hydrogen
Lead
Hydrogen
EX: Ni (s) + 2 HCl(aq) → NiCl2 (aq) + H2↑
included for comparison
Antimony
Arsenic
do NOT react with acids
Bismuth
react with O2 from the air forming oxides
Copper
EX: 2 Cu (s) + O2 (g) → 2CuO (s)
Mercury
Palladium
Silver
Platinum
Gold
do NOT react with O2
LEAST REACTIVE ELEMENTS
(hardest to oxidize, easiest to reduce)
15
Flow Chart
For
Classifying Types of Chemical Reactions
Question To Ask
Types of Reactions:
Yes
One reactant?
Decomposition:
A reactant breaks up into pieces:
AB → A + B
Ex. MgO → Mg + O
No
Yes
Synthesis (combination):
One product?
Reactants combine to make a compound
A + B → AB
Ex. Mg + O → MgO
No
Yes
O2 a reactant and H2O a
product?
Combustion:
A hydrocarbon (H and C) burn in air (O2) to produce water, and CO2
CxHx + O2 → CO2 + H2O
No
An element and a
compound make a
different element and
compound?
Yes
Single Displacement (replacement):
An element takes the place of an element in a compound
A + BC → B + AC
Ex: Mg + BeO → Be + MgO
No
Yes
Two compounds make
two different compounds
Double Displacement (replacement):
Elements in two compounds switch places
AB + CD → AD + BC
Ex: MgO + BeS → MgS + BeO
16
17