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WorksheetsWeek 16 Final Exam Review
Total questions: 94
Worksheet time: 47mins
Which number below has 4 significant figures?
0.0001
0.001
100.0
1000
22.4 lb/in³ is equal to ____ kg/m³?
4.00x10²
6.20x10⁵
4.31x10³
8.10x10⁻⁴
When vinegar is boiled and condensed two separate liquids are isolated. Identify the type of matter for vinegar.
pure substance
heterogeneous mixture
compound
homogeneous mixture
Which process below is a physical change?
combustion of methane
rusting of iron
evaporating a liquid
electrolysis of water
What is the formula for calcium phosphide?
Ca₃(PO₄)₂
CaPO₃
CaPO₄
Ca₃P₂
What is the name for Mn(C₂H₃O₂)₂?
Manganese (II) carbonate
Magnesium cyanide
Manganese (II) acetate
Manganese oxalate
What is the formula for phosphorous acid?
H₃PO₄
H₃PO₃
H₂PO₄
H₃P
What is the formula for iodine trichloride?
ICl₃
ICl₄
ICl₂
I₂Cl₆
What is the name for HMnO4?
Manganese oxide acid
Manganate acid
Hypomanganic acid
Permanganic acid
What are the number of protons and electrons for Ca2+?
protons-20, electrons-20
protons-22, electrons-20
protons-22, electrons-22
protons-20, electrons-18
What do these have in common? 20Ne, 19F–, 24Mg2+
The same number of protons
The same number of neutrons
The same number of electrons
The same size
Which pair represents isotopes?
54Cr and 54Fe
235U and 238U
116Cd and 150U
239Np and 239Pu
Which of the following is a false statement?
Al is a metalloid
Cl is a nonmetal
Fe is a transition metal
He is a noble gas
The element X occurs naturally to the extent of 20.0% 12X and 80.0% 13X. The atomic mass of X is nearest?
12.2
12.5
12.8
13.0
A compound consisting of an element having a low ionization energy and a second element having a high electron affinity is likely to have
Covalent bonds
Metallic bonds
Coordinate covalent bonds
Ionic bonds
What is the mass percent of oxygen in Fe2(SO4)3?
15.40%
18.76%
30.80%
48.01%
What is the empirical formula for the substance with this analysis: 54.0% by mass Na, 8.50% by mass B, and 37.5% by mass O?
Na3BO3
Na3BO3
Na4BO4
Na3B2O2
A hydrocarbon is found to have the empirical formula CH₂. If the molecular mass is 42.07 g/mol, what is its molecular formula?
C₂H₄
C₃H₆
C₄H₈
C₅H₁₀
A typical silicon chip, such as those in electronic calculators, has a mass of 2.3x10⁻⁴ g. Assuming the chip is pure silicon, how many silicon atoms are in such a chip?
4.9x10¹⁸
1.4x10²⁰
3.9x10²¹
2.6x10²⁷
What mass of Na₂SO₄ contains 12.5 g of oxygen?
0.178 g
6.72
0.0360 g
27.7 g
How many sodium ions are present in 15.0 g of Na₂SO₄?
6.36x10²² ions
1.27x10²³ ions
2.54x10²³ ions
1.27x10⁴ ions
If the formula of an oxide of element X is X₂O₃, what is the formula of the chloride of X?
XCl₃
XCl
X₃Cl
XCl₆
A simple method of showing experimentally that a solid substance may be ionic is to show that it
Has a high melting point
Is soluble in polar solvents
Depresses the freezing point of water
Conducts current when dissolved in water
An element emits radiation at a wavelength of 435 nm, what is the frequency of the emitted light?
6.89x10⁵ Hz
6.89x10¹⁴ Hz
1.45x10⁶ Hz
1.45x10⁸ Hz
The energy of a photon is greatest in the case of
X-rays
Ultraviolet radiation
Visible light
Infrared radiation
Which ground state electron configuration is possible for an atom in the second period?
1s²2s¹
1s²2s¹2p¹
1s²2s²2d¹
1s²2p⁴
The number of unpaired electrons in gaseous selenium atom is?
2
3
4
5
Which electron transition in a hydrogen atom is associated with the largest emission of energy?
n=2 to n=1
n=2 to n=3
n=2 to n=4
n=3 to n=2
Which emission line in the hydrogen spectrum occurs at the highest frequency?
n=3 → n=1
n=7 → n=5
n=4 → n=2
n=10 → n=8
The maximum number of electrons that can occupy an orbital labeled dxy is
2
3
5
10
Which species has this ground state electron arrangement? 1s²2s²2p⁶3s²3p⁶3d¹⁰
Ni
Ni²⁺
Zn
Zn²⁺
What is the sublevel with the shape shown
s
p
d
f
Which set of quantum numbers is correct and consistent for an electron in a 4f orbital?
l = 3, ml = -3, ms = +½
l = 4, ml = +2, ms = -½
l = 2, ml = +3, ms = +½
l = 3, ml = -3, ms = +1
Of the series of atoms below, which is arranged in order of increasing effective nuclear charge?
Se < S < Cl
S < Cl < Se
Cl < S < Se
S < Se < Cl
When the three elements S, Se, and Cl are arranged in order of increasing atomic radius, which is the correct order?
Se < S < Cl
S < Cl < Se
Cl < S < Se
S < Se < Cl
In which pair of species is the first member larger than the second member?
Li⁺ and Be²⁺
Li⁺ and Na⁺
Li⁺ and Li
Be and Mg
Which ion has the largest radius?
Cl⁻
P³⁻
K⁺
Cu²⁺
The first three ionization energies of an element X are 590, 1145, and 4912 kJ/mol. What is the most likely formula for a stable ion of X?
X
X³⁺
X⁺
X²⁺
Which of the atoms below has the largest first ionization energy?
Mg
Na
Cl
K
Identify the type of reaction given below. C + H₂O → CO + H₂
decomposition reaction
synthesis reaction
double displacement reaction
single displacement reaction
Identify the coefficients that would balance the equation below. C₅H₁₀ + O₂ → CO₂ + H₂O
1, 2, 5, 1
2, 10, 10, 5
1, 7, 5, 10
2, 15, 10, 10
Identify the products formed from the reactants given below. Ca(NO₃)₂ + Na₂SO₄ →
NaN + O₂ + CaS
CaS + O₂ + Na₃N
CaSO₄ + NaNO₃
Na₂Ca + N₂(SO₄)₃
What is the net ionic equation for the molecular reaction Na₃PO₄ + H₂SO₄ → H₃PO₄ + Na₂SO₄
There is no net ionic equation
Na₃PO₄ + H₂SO₄ → H₃PO₄ + Na₂SO₄
2 Na⁺ + SO₄²⁻ → Na₂SO₄
2 PO₄³⁻ + 6 H⁺ → 2 H₃PO₄
Which of the compounds below has the smallest lattice energy
NaCl
KI
MgS
AlCl₃
Which molecule has exactly two unshared (lone) pairs of electrons on the central atom?
BF₃
OF₂
NF₃
XeF₂
Molecules of which compounds violate the octet rule?
I NO₂,
II CH₂Cl₂,
III XeF₄,
IV NCl₃
I and II
I and III
II and III
II and IV
Which species has both ionic and covalent bonds?
NH₃BF₃
H₃O⁺
NaKS
Mg(CN)₂
How many sigma and pi bonds respectively are here in
6, 3
7, 2
8, 1
9, 0
What is the formal charge for the nitrogen in the structure shown? The lone pairs are not shown.
0
+1
-1
+2
Which bond below will have the smallest polarity?
N-Cl
O-Cl
F-Cl
S-Cl
Consider the Lewis structure for CH₃Cl. What is the best description of the molecular shape?
Bent
Square
Square pyramidal
Tetrahedral
According to the VSEPR model, the electron group geometry of H₂O is
Linear
Trigonal planar
Tetrahedral
Bent
The hybridization of the sulfur atom in sulfur dioxide is
sp
sp²
sp³
sp³d
Which of these is a nonpolar molecule?
H₂CO
H₂O
C₂H₄
ICl
For which molecule can the bonding be described in terms of sp² hybrid orbitals on the central atom?
SF₆
BF₃
PCl₅
NH₃
Which is planar?
NH₃
SO₃²⁻
CO₃²⁻
CCl₄
Consider the given Lewis structure for BrF₅. What is the predicted shape for the molecule as a whole?
square pyramidal
trigonal bipyramidal
trigonal pyramidal
octahedral
Which set of species is arranged in order of increasing O-N-O bond angle?
NO₂, NO₂⁻, NO₂⁺
NO₂⁻, NO₂, NO₂⁺
NO₂⁺, NO₂, NO₂⁻
NO₂, NO₂⁺, NO₂⁻
Which compound would be expected to have the largest dipole moment?
CO₂
SO₂
BF₃
CF₄
Which compound would be expected to have the highest boiling point?
CO₂
SO₂
BF₃
CF₄
Which compound would be expected to have the lowest vapor pressure?
CO₂
SO₂
BF₃
CF₄
How many moles of iron react with 1.75 mol of oxygen gas? 3 O₂ (g) + 4 Fe (s) → 2 Fe₂O₃ (s)
1.31 mol
1.75 mol
2.33 mol
5.25 mol
Calculate the mass of SbF₃ needed to produce 1.00 g of Freon-12, CCl₂F₂. The reaction is represented by this equation. 3CCl₄ + 2SbF₃ → 3CCl₂F₂ + 2SbCl₃
0.667 g
0.986 g
1.48 g
2.22 g
What volume of 0.100 M SO₃²⁻(aq) is needed to titrate 24.0 mL of 0.200 M Fe³⁺(aq)?
2 Fe³⁺(aq) + SO₃²⁻(aq) + H₂O → 2Fe²⁺(aq) + SO₄²⁻(aq) + 2 H⁺(aq)
48.0 mL
24.0 mL
12.0 mL
6.00 mL
What is the percent yield of PbI₂ if 5.00 g of PbI₂ results from a solution containing 10.0 g of Pb(C₂H₃O₂)₂ with a solution containing an excess of KI? Chemical equation: Pb(C₂H₃O₂)₂ (aq) + 2KI (aq) → PbI₂ (s) + 2 KC₂H₃O₂ (aq)
17.6%
35.3%
50.0%
70.5%
Which set of substances are arranged in order of decreasing solubility in water?
CH₄ > CH₃OH > HOCH₂OH
HOCH₂OH > CH₃OH > CH₄
CH₃OH > CH₄ > HOCH₂OH
CH₃OH > HOCH₂OH > CH₄
The solubility of a substance is 60 g per 100 mL of water at 15°C. A solution of this substance is prepared by dissolving 75 g in 100 mL of water at 75°C. The solution is then cooled slowly to 15°C without any solid separating. The solution is
supersaturated at 75°C.
supersaturated at 15°C.
unsaturated at 15°C.
saturated at 15°C.
A solution is made by dissolving 60 g of NaOH (MW = 40.00 g/mol) in enough distilled water to make 300 mL of a stock solution. What volumes of this solution and distilled water when mixed, will result in a solution that is approximately 1 M NaOH?
20 mL stock solution, 80 mL distilled water
20 mL stock solution, 100 mL distilled water
60 mL stock solution, 30 mL distilled water
60 mL stock solution, 90 mL distilled water
What mass of NaOH (MW = 40.00 g/mol) is needed to make 300 mL of a stock 6.00 M NaOH solution?
0.800 g
800 mL
72.0 g
72,000 g
What is the concentration of a solution made by dissolving 25.00 g of NaOH (MW = 40.00 g/mol) in water to make 300.0 mL solution?
2.083 M
3.333 M
0.002083 M
83.33 M
What is the concentration of Na⁺ in a 0.600 M solution of Na₂SO₄?
0.300 M
0.600 M
1.20 M
2.40 M
Which substance below would not conduct electricity when dissolved in water?
HC₂H₃O₂
NaOH
NaCl
C₂H₅OH
Which substance below would be a strong electrolyte in water?
C₆H₁₂O₆
HNO₃
NH₄OH
AgCl
What volume of 0.131 M BaCl₂ is required to react completely with 42.0 mL of 0.453 M Na₂SO₄?
Ba²⁺ (aq) + SO₄²⁻ (aq) → BaSO₄ (s)
12.1 mL
72.6 mL
145 mL
290 mL
What is the oxidation number of phosphorus in H₃PO₄?
+2
+3
+4
+5
Consider this reaction: 2 Fe³⁺ (aq) + 2 I⁻ (aq) → 2 Fe²⁺ (aq) + I₂ (aq) Which statement is true for the reaction?
Fe³⁺ is oxidized.
Fe³⁺ increases in oxidation number.
Fe³⁺ is reduced.
I⁻ is reduced.
Consider this reaction: 2 Fe³⁺ (aq) + 2 I⁻ (aq) → 2 Fe²⁺ (aq) + I₂ (aq) Which statement is true for the reaction?
Fe³⁺ is the oxidizing agent.
Fe³⁺ is the reducing agent.
Fe²⁺ is the oxidizing agent.
Fe²⁺ is the reducing agent.
In which pair does the named element have the same oxidation number?
Sulfur in H₂S₂O₇ and H₂SO₄
Mercury in Hg⁺ and Hg₂²⁺
Oxygen in Na₂O₂ and in H₂O
Cobalt in Co(NH₃)₆³⁺ and Co(NO₃)₂
The graph below shows particle speed curves for several gases all at the same temperature and pressure. Which gas is represented by curve 2?
O₂
N₂
He
H₂
A mixture of 0.5 mol of CH₄, 0.5 mol H₂, and 0.5 mol SO₂ is introduced into a 10.0 L container at 25°C. If the container has a pinhole leak, which describes the relationship between the partial pressure of the individual components in the container after 3 hours?
SO₂ > CH₄ > H₂
SO₂ = CH₄ = H₂
SO₂ < CH₄ < H₂
SO₂ < CH₄ > H₂
What is the final temperature when an ideal gas at 25°C in a container with an adjustable volume that decreases from 10.0 L to 5.00 L while the pressure goes from 745 torr to 926 torr?
25°C
207°C
-88°C
-273°C
What is the molar mass of an ideal gas if a 0.622 g sample of this gas occupies a volume of 300 mL at 35°C and 789 mmHg?
44.8 g/mol
48.9 g/mol
50.5 g/mol
54.5 g/mol
What is the density of H₂S gas if it occupies a volume of 250 mL at 25°C and 755 mmHg?
1.38 g/L
0.762 g/L
795 g/L
0.00126 g/L
Which is true about equal volumes of CH₄ (MM=16.04 g/mol) and O₂ (32.00 g/mol) gases at 20°C and 1 atm pressure?
The CH₄ sample has a mass that is one-half that of the O₂ sample.
The number of O₂ molecules is twice as large as the number of CH₄ molecules.
The average kinetic energy of the O₂ molecules is one-half that of the CH₄ molecules.
The average velocity of the O₂ molecules is one-half that of the CH₄ molecules.
What mass of CaCO₃ will produce 8.0 L of CO₂, measured at standard temperature and pressure conditions? CaCO₃ (s) → CaO (s) + CO₂ (g)
45 g
13 g
36 g
70 g
If a 17.0 g sample of impure nickel metal reacts with excess CO forming 6.25 L of Ni(CO)₄(g) under STP conditions, what is the percent by mass of nickel in the impure metal sample?
24.1%
25.0%
96.5%
100%
13.8 g carbon monoxide (MM=28.01 g/mol) reacts with excess nickel metal forming Ni(CO)₄ (MM=170.7 g/mol) that is collected over water. What volume of Ni(CO)₄ is collected at 21.4°C and 772 torr? PH₂O(21.4°C) = 19.113 torr.
11.7 L
2.93 L
3.01 L
0.0154 L
A system transfers 12.6 kJ of heat to the surroundings and the surroundings do 15.9 kJ of work on the system. What is the change in internal energy for the system?
-3.3 kJ
28.5 kJ
3.3 kJ
-28.5 kJ
Given the following reaction and standard enthalpy of reaction: 2 Mg (s) + O₂ (g) → 2 MgO (s) ΔH = -1204 kJ. Calculate the amount of heat transferred when 3.45 g of Mg(s) reacts at constant pressure.
-171 kJ
-342 kJ
-37.8 kJ
-85.4 kJ
A 50.0-g sample of water (specific heat = 4.184 J/g°C) at 100.00°C was placed in an insulated cup. Then a piece of zinc (specific heat = 0.388 J/g°C) at 25.00°C was added to the water. The temperature of the water dropped to 96.68°C. What was the mass of the piece of zinc?
171 g
9.66 g
19.2 g
259 g
When 15.3 g of sodium nitrate (MM=85.00 g/mol) was dissolved in water in a calorimeter, the temperature fell from 25.00°C to 21.56°C. If the heat capacity of the solution and the calorimeter is 1071 J/°C, what is the enthalpy change for the reaction? NaNO₃ (s) → Na⁺ (aq) + NO₃⁻ (aq)
-0.241 kJ/mol
20.8 kJ/mol
0.241 kJ/mol
-20.8 kJ/mol
Given the following enthalpies of reaction:
P₄ (s) + 3 O₂ (g) → P₄O₆ (s) ΔH = –1640.1 kJ
P₄ (s) + 5 O₂ (g) → P₄H₁₀ (s) ΔH = –2940.1 kJ
Calculate the enthalpy change for the reaction: P₄O₆ (s) + 2 O₂ (g) → P₄H₁₀ (s)
-4580.2 kJ
-1300.0 kJ
4580.2 kJ
1300.0 kJ
Calculate the ΔH° for the reaction: C₂H₄ (g) + F₂ (g) → CF₄ (g) + HF (g)
Given: ΔH°f (kJ/mol) C₂H₄ (g) = -52.3, CF₄ (g) = -680, HF (g) = -537
-1164.7 kJ
1164 kJ
-3460 kJ
3460 kJ
Calculate the ΔH° for the reaction: CH₄ (g) + O₂ (g) → CO₂ (g) + H₂O (g)
Given bond enthalpies (kJ/mol):
C-H = 413, O-O = 146, O=O = 498, C=O = 351, C=O (double bond) = 805, O-H = 464
-614 kJ
-388 kJ
-818 kJ
-1522 kJ
