PRINCE GEORGE’S COMMUNITY COLLEGE
CHM1010 (SHAH)
MULTIPLE CHOICES FOR PRACTICE
Note: Answers are given only for chapter 1. Do by yourself for Chapter 2 and 3
Chapter 1
1) A substance that can't be chemically broken down into simpler substances is
A) a homogeneous mixture. B) an element. C) a heterogeneous mixture.
D) a compound.
E) an electron.
Answer: B
2) A substance composed of two or more elements in a fixed, definite proportion is
A) a homogeneous mixture. B) a heterogeneous mixture. C) a compound.
D) a solution.
E) an alloy.
Answer: C
3) Choose the element from the list below.
A) sodium chloride B) water
C) carbon dioxide
D) helium
Answer: D
4) Choose the compound from the list below.
A) magnesium
B) water
C) neon
Answer: B
D) helium
E) lithium
5) Decanting is
A) a process in which the more volatile liquid is boiled off.
B) dissolving a solid into a liquid.
C) separating a solid from a liquid by pouring off the liquid.
D) pouring a mixture through a filter paper to separate the solid from the liquid.
E) heating a mixture of two solids to fuse them together.
Answer: C
6) Two or more substances in variable proportions, where the composition is constant
throughout are
A) a compound.
B) an element.
C) a heterogeneous mixture. D) a homogeneous
mixture.
E) a crystalline solid.
Answer: D
7) Two or more substances in variable proportions, where the composition is variable
throughout are
A) a solution. B) a homogeneous mixture. C) a compound.
D) an amorphous solid..
E) a heterogeneous mixture.
Answer: E
8) Choose the heterogeneous mixture from the list below.
A) sports drink
B) chlorine gas
C) black coffee
D) chicken noodle soup
Answer: D
9) Choose the homogeneous mixture from the list below.
A) cola
B) mud C) ice water
D) salad dressing
Answer: A
E) salsa
10) Choose the homogeneous mixture from the list below.
A) soda (pop) B) air C) concrete D) trail mix
E) blood
Answer: B
11) Which of the following are examples of physical change?
A) sugar is dissolved in water B) coffee is brewed C) dry ice sublimes
D) ice (solid water) melts
E) All of these are examples of physical change.
Answer: E
12) Which of the following are examples of physical change?
A) dew forms on a blade of grass
B) a halloween light stick glows after shaking
C) an egg solidifies during cooking D) a hydrogen balloon explodes when contacted with a
flame E) None of the above are physical changes.
Answer: A
13) Which of the following are examples of a chemical change?
A) copper building materials develop a green patina over time
B) a match burns
C) ethanol evaporates
D) Both A and B are examples of chemical change.
E) All of the above are examples of chemical change.
Answer: D
14) Which of the following are examples of a chemical change?
A) coffee brewing
B) water boiling
C) leaves turning color in the fall
D) salt dissolves in water
E) None of the above are chemical changes.
Answer: C
15) A physical change
A) occurs when iron rusts. B) occurs when sugar is heated into caramel.
C) occurs when glucose is converted into energy within your cells.
D) occurs when water is evaporated.
E) occurs when propane is burned for heat.
Answer: D
16) A chemical change
A) occurs when methane gas is burned.
B) occurs when paper is shredded.
C) occurs when water is vaporized.
D) occurs when salt is dissolved in water.
E) occurs when powdered lemonade is stirred into water.
Answer: A
17) Which of the following represents a physical property?
A) Sodium metal is extremely reactive with chlorine gas.
B) Mercury is a silvery liquid at room temperature.
C) Aluminum has a tendency to "rust."
D) Butane is highly flammable.
E) Argon has an unreactive nature.
Answer: B
18) Which of the following represents a chemical property of hydrogen gas?
A) It is gaseous at room temperature.
B) It is less dense than air.
C) It reacts explosively with oxygen.
D) It is colorless.
E) It is tasteless.
Answer: C
19) Which of the following statements about energy is FALSE?
A) Energy can be converted from one type to another.
B) The total energy of a system remains constant.
C) Kinetic energy is the energy associated with its position or composition.
D) Energy is the capacity to do work.
E) Systems tend to change in order to lower their potential energy.
Answer: C
20) Define thermal energy.
A) energy associated with the temperature of an object
B) energy associated with the motion of an object
C) energy associated with the force of an object
D) energy associated with the gravity of an object
Answer: A
21) All of the following are SI base units of measurement, EXCEPT
A) meter
B) gram
C) second
D) kelvin
E) mole
Answer: B
22) Identify the unit of measurement which is a SI base unit of measurement.
A) second
B) Celsius
C) cup D) pound
E) yard
Answer: A
23) Kilogram is a measure of
A) mass
B) time
C) temperature
Answer: A
D) length
E) volume
24) Which of the following are examples of intensive properties?
A) density
B) volume
C) mass
D) None of the above are examples of intensive
properties.
E) All of the above are examples of intensive properties.
Answer: A
25) Which of the following are examples of extensive properties?
A) mass
B) color
C) density
D) temperature
E) taste
Answer: A
26) Identify the common substance that has the highest density.
A) sugar
B) water
C) glass
D) lead
E) aluminum
Answer: D
27) Identify the common substance that has the lowest density.
A) ice B) aluminum C) copper
D) table salt E) sugar
Answer: A
28) If the temperature is 178°F, what is the temperature in degrees celsius?
A) 352°C
B) 451°C
C) 67°C
D) 81.1°C
E) 378°C
Answer: D
29) If a solution has a temperature of 355 K, what is its temperature in degrees celsius?
A) 165°C
B) 628°C
C) 179°C
D) 279°C
E) 82°C
Answer: E
30) The outside temperature is 35°C, what is the temperature in K?
A) -238 K
B) 308 K
C) 95 K
D) 31 K
E) 63 K
Answer: B
31) Determine the density of an object that has a mass of 149.8 g and displaces 12 .1 mL of
water when placed in a graduated cylinder.
A) 8.08 g/mL B) 1.38 g/mL
C) 12 .4 g/mL D) 18.1 g/mL E) 11.4 g/mL
Answer: C
32) Determine the volume of an object that has a mass of 455.6 g and a density of 19.3 g/cm 3.
A) 87.9 mL
B) 42 .4 mL C) 18.5 mL
D) 23.6 mL
E) 31.2 mL
Answer: D
33) Determine the mass of an object that has a volume of 88.6 mL and a density of 9.77 g/mL.
A) 298 g
B) 1100 g
C) 907 g
D) 568 g
E) 866 g
Answer: E
34) The outside air temperature is 30°F, what is the temperature in Kelvin?
A) 303 K
B) 307 K
C) 274 K
D) 272 K
Answer: D
35) A student performs an experiment to determine the density of a sugar solution. She
obtains the following results: 1.79 g/mL, 1.81 g/mL, 1.80 g/mL, 1.81 g/mL. If the actual value
for the density of the sugar solution is 1.80 g/mL, which statement below best describes her
results?
A) Her results are precise, but not accurate.
B) Her results are accurate, but not precise.
C) Her results are both precise and accurate
D) Her results are neither precise nor accurate.
E) It isn't possible to determine with the information given.
Answer: C
36) Systematic error is defined as
A) error that tends to be too high or too low.
B) error that has equal probability of being too high and too low.
C) error that averages out with repeated trials.
D) error that is random.
Answer: A
37) Read the water level with the correct number of significant figures.
A) 5 mL
B) 5.3 mL
C) 5.32 mL
D) 5.320 mL E) 5.3200 mL
Answer: B
38) Read the temperature with the correct number of significant figures.
A) 87°C
Answer: C
B) 87.2°C
C) 87.20°C
D) 87.200°C
E) 87.2000°C
39) What answer should be reported, with the correct number of significant figures, for the
following calculation? (249.362 + 41) / 63.498
A) 4.6 B) 4.57
Answer: B
C) 4.573
D) 4.5728
E) 4.57277
40) What answer should be reported, with the correct number of significant figures, for the
following calculation? (965.43 × 3.911) + 9413.4136
A) 13189
B) 13189.2
C) 1.32 × 104 D) 1.3 × 104 E) 1.319 × 104
Answer: A
41) What wavelength of light would you report in units of nm, if the light had a wavelength of
7.60 × 10-10 m?
A) 7.60 × 10-3 nm
B) 7.60 × 10-19 nm C) 1.32 nm
D) 0.760 nm
E) 760 nm
Answer: D
Chapter 2
1) Determine the number of protons, neutrons and electrons in the following:
40
18 X
A) p+ = 18 n° = 18
B) p+ = 18 n° = 22
C) p+ = 22 n° = 18
e- = 22
e- = 18
e- = 18
D) p+ = 18 n° = 22
E) p+ = 40 n° = 22
e- = 40
e- = 18
2) Determine the number of protons, neutrons and electrons in the following:
25
12 X
A) p+ = 12
B) p+ = 12
C) p+ = 12
D) p+ = 25
E) p+ = 12
n° = 25
n° = 12
n° = 13
n° = 12
n° = 13
e- = 12
e- = 13
e- = 12
e- = 13
e- = 25
3) Determine the number of protons, neutrons and electrons in the following:
65
29 X
A) p+ = 36 n° = 29
B) p+ = 29 n° = 29
C) p+ = 36 n° = 36
D) p+ = 29 n° = 36
E) p+ = 29 n° = 36
e- = 36
e- = 36
e- = 29
e- = 29
e- = 36
4) What element is defined by the following information?
p+ = 17 n° = 20
e- = 17
A) calcium
B) rubidium
C) chlorine
5) How many electrons are in arsenic?
A) 33
B) 41 C) 42 D) 41.9
D) neon
E) oxygen
E) 75
6) How many protons are in arsenic?
A) 33
B) 41 C) 42
D) 41.9
E) 75
7) Which of the following statements about subatomic particles is TRUE?
A) A neutral atom contains the same number of protons and electrons.
B) Protons have about the same mass as electrons.
C) Electrons make up most of the mass of an atom.
D) Protons and neutrons have opposite, but equal in magnitude, charges.
E) Neutrons and electrons are found in the nucleus of an atom.
8) Isotopes differ in the number of
A) protons
B) neutrons C) electrons
D) none of the above E) all of the above
9) Give the symbol for fluorine.
A) F B) Fl C) Fo D) Fu E) Fr
10) Give the symbol for silver.
A) S B) Si C) Ar D) Ag E) Sl
11) Identify a cation.
A) An atom that has lost an electron.
B) An atom that has gained an electron.
C) An atom that has lost a proton.
D) An atom that has gained a proton.
12) What species is represented by the following information?
p+ = 12
n° = 14
e- = 10
A) Si4+ B) Mg C) Ne D) Si
E) Mg2+
13) What species is represented by the following information?
p+ = 47
n° = 62
e- = 46
A) Ag+ B) Nd C) Pd D) Ag E) Pd+
14) Predict the charge that an aluminum ion would have.
A) 5- B) 1+ C) 1- D) 2+ E) 3+
15) Predict the charge that a calcium ion would have.
A) 6- B) 2- C) 3+ D) 2+ E) 1+
16) Give the number of electrons in P-3.
A) 18 B) 12 C) 19 D) 15 E) 16
17) Give the number of protons in P-3.
A) 18 B) 12 C) 19 D) 15 E) 16
18) Which of the following elements is a metal?
A) As B) C C) I
D) Sn E) Se
19) Which of the following elements is a nonmetal?
A) Zn B) Cs C) Ca D) Co E) P
20) Which of the following elements is a noble gas?
A) Ar B) Br C) N D) O E) K
21) Which of the following is a transition element?
A) Pd B) Sn C) K D) U E) Pr
22) Which of the following statements is FALSE?
A) Halogens are very reactive elements.
B) The alkali metals are fairly unreactive.
C) Sulfur is a main group element.
D) Noble gases do not usually form ions.
E) Zn is a transition metal.
23) Which of the following does NOT describe a metal?
A) good conductor of heat
B) good conductor of electricity
C) tends to gain electrons
D) forms ionic compounds with nonmetals
E) found on the left side of the periodic table.
24) Semiconductors are
A) metalloids.
B) noble gases.
C) nonmetals.
D) metals.
25) Which of the following statements is FALSE?
A) Anions are usually larger than their corresponding atom.
B) Metals tend to form cations.
C) Atoms are usually larger than their corresponding cation.
D) The halogens tend to form 1+ ions.
E) Nonmetals tend to gain electrons.
26) The atomic mass for cadmium is
A) 48 B) 112.41
C) 40.08
D) 20
27) Calculate the atomic mass of silver if silver has 2 naturally occurring isotopes with the
following masses and natural abundances:
Ag-107
Ag-109
106.90509 amu
108.90476 amu
A) 107.90 amu
E) 108.19 amu
51.84%
48.46%
B) 108.00 amu
C) 107.79 amu
D) 108.32 amu
28) Calculate the atomic mass of gallium if gallium has 2 naturally occurring isotopes with the
following masses and natural abundances:
Ga-69
Ga-71
68.9256 amu
70.9247 amu
A) 69.72 amu
60.11%
39.89%
B) 69.93 amu
C) 70.00 amu
D) 69.80 amu
29) How many silver atoms are contained in 3.75 moles of silver?
A) 6.23 × 1024 silver atoms
B) 2.26 × 1024 silver atoms
C) 1.61 × 1023 silver atoms
D) 2.44 × 1026 silver atoms
30) How many xenon atoms are contained in 2.36 moles of xenon?
A) 3.92 × 1024 xenon atoms
B) 2.55 × 1023 xenon atoms
C) 1.42 × 1024 xenon atoms
D) 7.91 × 1025 xenon atoms
31) How many argon atoms are contained in 7.66 x 105 mmol of argon?
A) 4.61 × 1026 Ar atoms
B) 1.84 × 1028 Ar atoms
C) 1.15 × 1028 Ar atoms
D) 7.86 × 1020 Ar atoms
E) 3.24 × 1026 Ar atoms
32) What mass (in g) does 3.99 moles of Kr have?
A) 334 g
B) 476 g
C) 211 g
D) 240 g
E) 144 g
33) How many moles of potassium are contained in 449 g of potassium?
A) 11.5 moles B) 17.6 moles C) 69.2 moles D) 23.9 moles E) 41.5 moles
34) How many moles are in 2.16 x 1024 atoms of lead?
A) 35.9 moles B) 3.59 moles C) 0.359 moles
35) How many atoms are in 2.50 moles of CO2?
D) 6.08 moles E) 1.79 moles
A) 4.52 x 1024 atoms B) 1.52 x 1024 atoms
C) 5.02 x 1023 atoms D) 3.01 x 1024 atoms
36) How many molecules are in 2.50 moles of CO2?
A) 4.52 x 1024 atoms B) 1.51 x 1024 atoms C) 5.02 x 1023 atoms D) 3.01 x 1024 atoms
37) What mass (in kg) does 5.84 moles of titanium (Ti) have?
A) 0.352 kg B) 0.122 kg C) 0.820 kg
D) 0.280 kg
E) 0.632 kg
38) What mass (in mg) does 2.63 moles of nickel have?
A) 44.8 mg
B) 2.23 × 104 mg
C) 129 mg
D) 3.56 x 105 mg
E) 1.54 x 105 mg
39) How many moles of Kr are contained in 398 mg of Kr?
A) 4.75 × 10-3 moles Kr
moles Kr
B) 33.4 moles Kr
C) 2.11 × 10-4 moles Kr
40) How many iron atoms are contained in 354 g of iron?
A) 2.62 × 1025 Fe atoms
B) 2.13 × 1026 Fe atoms
C) 4.69 × 1024 Fe atoms
D) 3.82 × 1024 Fe atoms
E) 9.50 × 1022 Fe atoms
41) How many phosphorus atoms are contained in 158 kg of phosphorus?
A) 3.07 × 1027 phosphorus atoms B) 2.95 × 1027 phosphorus atoms
C) 3.25 × 1028 phosphorus atoms D) 1.18 × 1024 phosphorus atoms
E) 8.47 × 1024 phosphorus atoms
42) What is the chemical symbol for titanium?
A) Th B) Ti C) Tl D) Tm
43) What is the chemical symbol for mercury?
A) Ag B) Au C) Hg D) Pb
44) Which of the following represent isotopes?
A: 32
15 X
A) A and B
B: 32
16 X
31
X
C: 15
B) A and C
34
X
D: 17
C) A and D
D) C and D
45) How many protons (p) and neutrons (n) are in an atom of 90
38 Sr ?
A) 38 p, 52 n B) 38 p, 90 n C) 52 p, 38 n D) 90 p, 38 n
Chapter 3
1) An ionic bond is best described as
A) the sharing of electrons.
B) the transfer of electrons from one atom to another.
C) the attraction that holds the atoms together in a polyatomic ion.
D) the attraction between 2 nonmetal atoms.
E) the attraction between 2 metal atoms.
2) A covalent bond is best described as
A) the sharing of electrons between atoms.
B) the transfer of electrons.
C) a bond between a metal and a nonmetal.
D) 2.99 × 10-3
D) a bond between a metal and a polyatomic ion.
E) a bond between two polyatomic ions.
3) Identify the compound with ionic bonds.
A) Ne B) CO C) O2 D) H2O E) KBr
4) Identify the compound with covalent bonds.
A) CH4 B) Ne
C) KBr
D) Mg E) NaCl
5) What is the empirical formula for C4H10O2?
A) C2H5O
B) CHO C) C2H4O
D) CHO2
E) CH2O
6) Write a possible molecular formula for C4H4O.
A) C8H8O2
B) C12H12O2
C) C2H2O
7) Which of the following is an atomic element?
A) Br
B) H
C) N D) O
D) C8H8O
E) Mg
8) Which of the following is a molecular element?
A) Kr B) Ag
C) S D) Mg
E) Ti
9) Which of the following is a molecular compound?
A) CuCl2
B) KCl
C) NaNO3
D) CH3Cl
E) RbBr
10) Which of the following exists as a diatomic molecule?
A) N
B) C
C) P D) Na
E) Ne
11) Which of the following exists as a polyatomic molecule?
A) N B) C C) P D) Na E) Ne
12) Give the name for SnO.
A) tin (I) oxide B) tin (II) oxide C) tin (III) oxide
D) tin (IV) oxide
13) Write the formula for barium nitrite.
A) Ba3N2
B) BaNO3
C) BN
D) Ba(NO2)2
14) Write the formula for strontium nitride.
A) Sr3N2
B) Sr(NO3)2
C) SrN
15) Give the structure for sodium chlorate.
E) B(NO2)3
D) Sr2N3
E) Sr(NO2)2
A) NaClO
B) NaClO2
C) NaClO3
D) NaClO4
16) Write the name for Sn(SO4)2. Remember that Sn forms several ions.
A) tin (I) sulfite
B) tin (IV) sulfate
C) tin sulfide
D) tin (II) sulfite
E) tin (I) sulfate
17) What is the charge on the Cr ions in Cr2O3?
A) 2-
B) 1+
C) 2+
D) 3+
18) Write the name for Ca3(PO4)2.
A) calcium (III) phosphite
D) tricalcium phosphorustetraoxide
B) calcium (II) phosphite
E) calcium phosphite
C) calcium phosphate
19) Write the name for FeS.
A) iron (I) sulfate
B) iron (I) sulfide
C) iron (II) sulfide
D) iron (II) sulfate
20) Write the name for FeS.
A) ferrous sulfate
D) ferric sulfate
B) ferrous sulfide
E) iron sulfide
C) ferric sulfide