AP Chemistry 1st Semester Final

200 terms by cmdancer927 

Create a new folder

Advertisement Upgrade to remove ads

Which one of the following statements concerning matter is correct?
a) a gas has a fixed volume but not a rigid shape
b) a liquid has a fixed volume and a rigid shape
c) a liquid takes on both the volume and the shape of its container
d) a solid has a fixed volume and a rigid shape
e) both b and d are correct

d

All of the following statements are true EXCEPT
a) of the 113 known elements, 91 occur naturally
b) an element cannot be broken down into two or more pure substances
c) a compound is a substance that contains two or more elements
d) a pure compound always contains the same elements in the same mass percentages
e) another name for a heterogeneous mixture is a solution

e

Which term best describes table salt (NaCl) at room temperature?
a) gas
b) element
c) compound
d) homogeneous mixture
e) heterogeneous mixture

c

All of the following statements are false EXCEPT
a) copper (Cu) is a homogeneous mixture of carbon (C) and uranium (U)
b) table salt is a heterogeneous mixture of sodium metal and chlorine gas
c) soda water is a homogeneous mixture of carbon dioxide gas and water
d) sugar dissolves completely in water to give a heterogeneous mixture
e) water (H20) is a homogeneous mixture containing hydrogen and oxygen

c

All of the following statements are true EXCEPT
a) potassium is represented by the symbol K
b) zinc is represented by the symbol Zn
c) argon is represented by the symbol Ar
d) iron is represented by the symbol Fe
e) nitrogen is represented by the symbol Ni

e

Which method is best for removing the pulp from orange juice?
a) distillation
b) light absorption
c) electrolysis
d) gas-liquid chromatography
e) filtration

e

Vinegar is a homogeneous mixture of two liquids: acetic acid and water. Which method is best for separating the components of vinegar?
a) distillation
b) filtration
c) electrolysis
d) gas-liquid chromatography
e) light absorption

a

The gravity on the surface of Earth is 6.02 times greater than that on the moon. If an object has both a mass and weight of 1.00 kg on earth, on the moon the same object will have
a) a mass of 1.00 kg and a weight of 0.166 kg
b) a mass of 1.00 kg and a weight of 1.00 kg
c) a mass of 1.00 kg and a weight of 6.02 kg
d) a mass of 0.166 kg and a weight of 0.166 kg
e) a mass of 0.166 kg and a weight of 1.00 kg

a

What is a correct method for converting Celsius to kelvin?
a) t(K)=9K/5C (tC-273.15C)
b) t(K)=5K/9C (tC+273.15C)
c) t(K)=1K/1C (tC-273.15C)
d) t(K)=1K/1C (tC+273.15C)
e) none of the above

d

If the outdoor temperature is 17.0 degrees Celsius, what is the temperature in Fahrenheit?
a) -1.40 degrees Fahrenheit
b) 30.6 degrees Fahrenheit
c) 41.4 degrees Fahrenheit
d) 62.6 degrees Fahrenheit
e) 74.6 degrees Fahrenheit

d

Which is a correct expression for converting Celsius to Fahrenheit?
a) degrees Fahrenheit=(5F/9C) tC-32F
b) degrees Fahrenheit=(5F/9C) tC+32F
c) degrees Fahrenheit=(5F/9C) (tC+32F)
d) degrees Fahrenheit=(9F/5C) tC-32F
e) degrees Fahrenheit=(9F/5C) tC+32F

e

Many experiments are conducted at 298 K. What is this temperature in Celsius?
a) 0 C
b) 25 C
c) 55 C
d) 273 C
e) 298 C

b

Express 4.220 x 10^2 mL in standard notation.
a) 0.0422 mL
b) 0.04220 mL
c) 422 mL
d) 422.0 mL
e) 4220 mL

d

How many significant figures are in the following mass: 0.00047800 kg?
a) 3
b) 5
c) 6
d) 8
e) 9

b

What is the correct answer to the expression below?
2.54cm/inch x (182.3 inch - 179.219 inch)
a) 8 cm
b) 7.8 cm
c) 7.83 cm
d) 7.826 cm
e) 7.8257 cm

b

All of the following are exact conversions EXCEPT
a) 1 pound=453.6 g
b) 1 m^3=1x10^3 L
c) 1 cm^3=1 mL
d) 2.54 cm=1 inch
e) 1 kg=1x10^3 g

a

All of the following are examples of chemical change EXCEPT
a) the fermentation of wine
b) the tarnishing of silver
c) the condensation of steam
d) the combustion of butane gas
e) the rusting of iron

c

An intensive property is
a) too small to be observed
b) dependent only on mass and temperature
c) visible to the human eye
d) dependent upon amount
e) independent of amount

e

An aqueous solution of copper sulfate is blue. This solution absorbs
a) blue light
b) red light
c) only infrared light
d) only ultraviolet light
e) only light with wavelengths shorter than 400 nm

b

Which description most accurately describes neptunium-239?
a) mass number=93, atomic number=239
b) mass number=93, number of neutrons=146
c) mass number=146, atomic number=93
d) number of protons=93, number of neutrons=146
e) number of protons=93, atomic number=239

d

Which two atoms below have the same number of neutrons?
(top:15, bottom:8) O,
(top:16, bottom:8) O,
(top:20, bottom:9) F,
(top:20, bottom:10) Ne,
(top:22, bottom:11) Na

a) (top:15, bottom:8) O and (top:16, bottom:8) O
b) (top:16, bottom:8) O and (top:22, bottom:11) Na
c) (top:20, bottom:9) F and (top:22, bottom:11) Na
d) (top:20, bottom:9) F and (top:22, bottom:11) Na
e) (top:20, bottom:10) Ne and (top:22, bottom:11) Na

d

Which two of the ions below have the same number of electrons?
(top:127, bottom:53) I^1-,
(top:119, bottom:50) Sn^2+,
(top:207, bottom:82) Pb^2+
(top:207, bottom:82) Pb^4+
(top:137, bottom:56) Ba^2+

a) (top:127, bottom:53) I^1- and (top:137, bottom:56) Ba^2+
b) (top:127, bottom:53) I^1- and
c) top:207, bottom:82) Pb^2+ and (top:137, bottom:56) Ba^2+
d) (top:119, bottom:50) Sn^2+ and (top:137, bottom:56) Ba^2+
e) top:207, bottom:82) Pb^2+ and (top:207, bottom:82) Pb^4+

a

Which species has 63 neutrons?
a) (top:112, bottom:48) Cd
b) (top:112, bottom:49) In
c) (top:63, bottom:29) Zn
d) (top:152, bottom:63) Eu
e) none of the above

b

What is the identity of (top:55, bottom:25) X?
a) zinc
b) silver
c) iridium
d) cesium
e) manganese

e

Beta particles have identical properties to
a) helium atoms that have been stripped of their electrons
b) elemental helium
c) high energy radiation
d) neutrons
e) electrons

e

How many protons and electrons are in a sulfate ion, SO4^2-?
a) 46 protons and 48 electrons
b) 48 protons and 48 electrons
c) 48 protons and 50 electrons
d) 50 protons and 48 electrons
e) none of the above

c

All of the following groups are considered main group elements EXCEPT
a) group 2
b) group 7
c) group 14
d) group 17
e) group 18

b

Which group of three elements contains a transition metal, a halogen, and a noble gas?
a) S, I, Cu
b) Br, Kr, Ba
c) Ar, Hg, Rn
d) Ce, N, He
e) Cu, I, Xe

e

How many elements are contained in period 4?
a) 3
b) 8
c) 10
d) 18
e) 32

d

How many nonmetals, metalloids, and metals are in group 14?
a) 0 nonmetals, 3 metalloids, and 2 metals
b) 1 nonmetals, 2 metalloids, and 2 metals
c) 2 nonmetals, 2 metalloids, and 1 metals
d) 2 nonmetals, 1 metalloids, and 2 metals
e) 3 nonmetals, 0 metalloids, and 2 metals

b

A strontium ion has ____ electrons.
a) 35
b) 36
c) 37
d) 38
e) 39

b

Identify the ions and their charges in Na2SO4.
a) Na^+, SO4^-
b) Na^+, SO4^2-
c) Na^+, SO^4-
d) Na^2+, SO^4-
e) Na^2+, SO4^2-

b

Identify the ions and their charges in Mg3N2
a) Mg^+, N^3-
b) Mg^2+, N^3-
c) Mg^3+, N^2-
d) Mg3^2+, N2^3-
e) Mg3^6+, N2^6-

b

What are the values for x and y, respectively, in CaxHyPO4?
a) 1 and 2
b) 2 and 1
c) 1 and 3
d) 2 and 2
e) 1 and 1

e

What is the correct name for Ag2O?
a) silver (I) oxide
b) silver (I) monoxide
c) silver (II) oxide
d) silver dioxide
e) disilver monoxide

a

What is the correct formula for chromium (II) nitrate?
a) Cr3NO3
b) Cr(NO3)3
c) Cr2(NO3)3
d) Cr3(NO3)2
e) Cr3(NO3)3

b

What is the correct name for N203?
a) nitrogen oxide
b) nitrogen (II) oxide
c) nitrogen (III) oxide
d) trioxygen dinitride
e) dinitrogen trioxide

e

What is the correct name for PF5?
a) phosphorous pentafluoride
b) phosphorous (V) fluoride
c) phosphorofluoride
d) pentafluorophosphorus
e) pentafluorophosphate

a

What is the correct formula for sulfur dichloride?
a) SCl
b) SCl2
c) S2Cl
d) S2Cl2
e) S4Cl2

b

What is the correct formula for potassium dichromate?
a) K2Cr2O7
b) K2(Cr2O7)2
c) K2CrO4
d) (K2CrO4)2
e) KCrO4

a

What is the formula for chlorous acid?
a) HCl
b) HClO
c) HClO2
d) HClO3
e) HClO4

c

What is the correct name for HI (aq)?
a) hydroiodic acid
b) hydrogen iodide ion
c) monohydrogen monoiodide
d) iodate acid
e) iodine hydride

a

Gallium has an atomic mass of 69.7 amu. In a typical sample, 60.4% of Ga exists as Ga-69 (68.9257 amu). What is the identity and the atomic mass of the other isotope?
a) (top:70, bottom:30) Ga; 70.9 amu
b) (top:70, bottom:31) Ga; 70.9 amu
c) (top:71, bottom:31) Ga; 70.9 amu
d) (top:71, bottom:31) Ga; 71.9 amu
e) (top:72, bottom:31) Ga; 71.9 amu

c

An element has three naturally occurring isotopes with the following abundances and masses:
abundance: 78.99%, mass (amu): 23.985042
abundance: 10.00%, mass (amu): 24.985837
abundance: 11.01%, mass (amu): 25.982593

Determine the atomic mass of the element
a) 24.31
b) 24.98
c) 74.95
d) 2431
e) none of the above

a

The average molar mass of lithium is 6.941. A sample of lithium consists of two isotopes with masses of 6.01512 amu and 7.01600 amu. Determine the percent abundance of each isotope.
a) 74.9% Li-6 and 92.51% Li-7
b) 8.45% Li-6 and 91.55% Li-7
c) 12.49% Li-6 and 87.51% Li-7
d) 91.55% Li-6 and 8.45% Li-7
e) 92.51% Li-6 and 7.49% Li-7

a

The mass of a single atom of ziroconium is 1.515x10^-22 grams. Which is a correct method for determining the molar mass of Zr.
a) (1 g/1.515x10^-22 atoms)(1 atom/6.022x10^23 moles)
b) (1 g/1.515x10^-22 atoms)(6.022x10^23 atoms/1 mole)
c) (1.515x10^-22 g/1 atom)(1 atom/6.022x10^23 moles)
d) (1.515x10^-22 g/1 atom)(6.022x10^23 atoms/1 mole)
e) none of the above

d

The mass of a single atom of sulfur is 5.325x10^-23 grams. Which is a correct method for determining molar mass of elemental sulfur, S8?
a) (5.325x10^-23 g S/1 atom)(1 atom/6.022x10^23 moles)(1 mole S8/ 8 mole S)
b) (5.325x10^-23 g S/1 atom)(6.022x10^23 atoms/1 mole S)(8 mole S/1 mole S8)
c) (5.325x10^-23 g S/1 atom)(1 atom/6.022x10^23 moles)(8 mole S/1 mole S8)
d) (1 atom/5.325x10^-23 g S)(6.022x10^23 moles/1 atom)(1 mole S8/ 8 mole S)
e) (5.325x10^-23 g S/1 atom)(6.022x10^23 atoms/1mole S)(1 mole S8/ 8 mole S)

b

A 1.45 g sample of chromium contains _____ atoms.
a) 1.25x10^22
b) 1.6x10^22
c) 8.73x10^23
d) 2.16x10^25
e) 4.54x10^25

b

You have a 5.0 g sample of each of the following elements: Ra, Rb, Rh, Rn, Ru. Which sample contains the most atoms?
a) Ra
b) Rb
c) Rh
d) Rn
e) Ru

b

Which of the following samples contains the largest number of atoms?
a) 2.0 moles of H3PO4
b) 3.0 moles of H2SO3
c) 4.0 moles of HNO3
d) 6.0 moles of HClO
e) 8.0 moles of HBr

c

Which of the following samples contains the largest number of hydrogen atoms?
a) 2.0 moles of C6H16
b) 3.0 moles of C3H8
c) 4.0 moles of C3H6
d) 6.0 moles of C2H4
e) 8.0 moles of C2H2

a

What is the mass in grams of 0.362 moles nitric acid (HNO3)?
a) 0.00574 g
b) 0.0438 g
c) 22.8 g
d) 53.8 g
e) 174 g

c

What is the percent composition of silicon nitride (Si3N4)?
a) 30.21% Si and 69.79% N
b) 42.92% Si and 57.08% N
c) 54.03% Si and 45.97% N
d) 60.06% Si and 39.94% N
e) 69.40% Si and 30.60% N

d

What is the percent composition of iron (II) sulfate hexahydrate?
a) 4.2% Fe; 4.2% S; 41.6% O; 50.0% H
b) 16.7% Fe; 16.7% S; 66.6% O
c) 21.5% Fe; 12.3% S; 24.6% O; 41.6% H
d) 21.5% Fe; 12.3% S; 61.5% O; 4.7% H
e) 36.8% Fe; 21.1% S; 42.1% O

d

Isopentyl acetate, a molecule composed of C, H, and O, smells like bananas. Combustion analysis of 1.750 grams of this molecule yields 1.695 g H2O and 4.142 g CO2. What is the simplest formula for isopentyl acetate?
a) C7H14O2
b) C7H7O4
c) C8H10O3
d) C8H16O
e) C9H6O

a

The catalytic conversion of ammonia to nitric oxide is the first step in a three-step process which ultimately results in nitric acid. Balance the equation for the reaction.

aNH3(g) + bO2(g) -> cNO(g) + dH2O(g)

a) a=2, b=1, c=2, d=1
b) a=3, b=2, c=3, d=3
c) a=4, b=3, c=2, d=6
d) a=4, b=5, c=4, d=6
e) a=6, b=15, c=6, d=9

d

The combustion of methanol, CH3OH, yields carbon dioxide and water as products. Which of the reactions below is correct and properly balanced?
a) CH3OH(l) + O2(g) -> CO2(g) + H2O(g)
b) CH3OH(l) + O2(g) -> CO2(g) + 2H2O(g)
c) 2CH3OH(l) + O2(g) -> 2CO2(g) + 4H2O(g)
d) 2CH3OH(l) + 2O2(g) -> 2CO2(g) + 2H2O(g)
e) 2CH3OH(l) + 3O2(g) -> 2CO2(g) + 4H2O(g)

e

Aluminum reacts with oxygen to form aluminum oxide. Which of the reactions below is correct and properly balanced?
a) Al(s) + O(g) -> AlO(s)
b) 2Al(s) + O(g) -> 2AlO(s)
c) 3Al(s) + O(g) -> Al3O2(s)
d) 4Al(s) + O(g) -> 2Al2O(s)
e) 4Al(s) + 3O(g) -> 2Al2O3(s)

e

If 16.4 g of oxygen gas react with excess hydrogen, what mass of water is produced?
2H2(g) + O2(g) -> 2H2O(g)
a) 9.23 g
b) 18.5 g
c) 20.4 g
d) 23.9 g
e) 36.9 g

b

Which method is correct for determining the mass of carbon dioxide that can be made by the combustion of 3.219 grams of ethanol with excess oxygen?
C2H5OH(l) + 3O2(g) -> 2CO2(g) + 3H2O(l)
a) 3.219 g C2H5OH (1 mole/46.07g)(2 mole CO2/1 mole C2H5OH)(44.01g CO2/1 mole)
b) 3.219 g C2H5OH (1 mole/46.07g)(1 mole CO2/2 mole C2H5OH)(44.01g CO2/1 mole)
c) 3.219 g C2H5OH (1 mole/46.07g)(1 mole CO2/1 mole C2H5OH)(44.01g CO2/1 mole)
d) 3.219 g C2H5OH (46.07 mole/1g)(2 mole CO2/1 mole C2H5OH)(44.01g CO2/1 mole)
e) 3.219 g C2H5OH (46.07 mole/1g)(1 mole CO2/2 mole C2H5OH)(44.01g CO2/1 mole)

a

How many moles of ammonia can be made by reacting 7.0 moles of N2 with 4.0 moles of H2?
N2(g) + 3H2(g) -> 2NH3(g)
a) 2.7 mol
b) 4.0 mol
c) 7.0 mol
d) 11 mol
e) 14 mol

a

What mass of oxygen will react with 2.64 g of magnesium?
2Mg(s) + O2(g) -> MgO(s)
a) 0.487 g
b) 1.00 g
c) 1.26 g
d) 1.74 g
e) 3.47 g

d

A mass of 8.15 g C2H4(g) reacts with excess oxygen. If 16.2 g CO2(g) is collected, what is the percent yield of the reaction?
C2H4(g) + 3O2(g) -> 2CO2(g) + 2H2O(g)
a) 25.6%
b) 31.7%
c) 41.0%
d) 57.1%
e) 63.3%

e

2.500 grams of MgSO4xH2O, a hydrated salt with an unknown water content, is dried in an oven to remove the water. After drying, the anhydrous salt has a mass of 1.221 grams. How many moles of water are present per mole of hydrated magnesium sulfate?
a) 1
b) 3
c) 5
d) 7
e) 9

d

Which of the following methods correctly describes the preparation of 1.00L of an aqueous solution of 0.500 M NaOH?
a) place 0.500 g NaOH(s) in a flask and dilute to 1.00 L with water
b) place 0.500 g NaOH(s) in a flask and add 1.00 L of water
c) place 20.0 g NaOH(s) in a flask and dilute to 1.00 L with water
d) place 20.0 g NaOH(s) in a flask and add 1.00 L of water
e) place 40.0 g NaOH(s) in a flask and add 500 g of water

c

If 17 g MgCl2 is dissolved in 5.0 L of water, what is the chloride ion molarity in the solution?
a) 0.036 M
b) 0.071 M
c) 0.68 M
d) 0.77 M
e) 7.8 M

b

Which of the following methods is correct for calculating the moles of Al^3+ in 125 mL of 0.234 M Al(NO3)3?
a) (0.234 mol Al(NO3)3/125 mL)(1000 mL/1 L)(1 mol Al^3+/1 mol Al(NO3)3)
b) (0.234 mol Al(NO3)3/125 mL)(1000 mL/1 L)(1 mol Al^3+/3 mol Al(NO3)3)
c) 125 mL(1 L/1000 mL)(0.234 mol Al(NO3)3/1 L)(1 mol Al^3+/3 mol Al(NO3)3)
d) 125 mL(1000 mL/1 L)(1 L/0.234 mol Al(NO3)3)(1 mol Al^3+/1 mol Al(NO3)3)
e) 125 mL(1 L/1000 mL)(0.234 mol Al(NO3)3/1 L)(1 mol Al^3+/1 mol Al(NO3)3)

e

A mass of 12.0 g of calcium chloride is diluted to a volume of 250 mL in a volumetric flask. Which of the equations below is a correct method for determining the chloride ion concentration?
a) (12.0g CaCl2/250 mL)(1000mL/1 L)(1 mole CaCl2/111.0 g)
b) (12.0g CaCl2/250 mL)(1L/1000mL)(1 mole CaCl2/111.0 g)(2 mole Cl-/1 mole CaCl2)
c) (12.0g CaCl2/250 mL)(1000mL/1L)(1 mole CaCl2/111.0 g)(2 mole Cl-/1 mole CaCl2)
d) (12.0g CaCl2/250 mL)(1L/1000mL)(1 mole CaCl2/111.0 g)(1 mole CaCl2/2 mole Cl-)
e) (12.0g CaCl2/250 mL)(1000mL/1L)(1 mole CaCl2/111.0 g)(1 mole CaCl2/2 mole Cl-)

c

What mass of potassium ions is present in 25.0 mL of 0.50 M K2SO4?
a) 0.250 g
b) 0489 g
c) 0.978 g
d) 2.18 g
e) 4.36 g

c

Which of the following ionic compounds are likely to be soluble in water: Mg(OH)2, Pb(NO3)2, AgI, Na2CO3, and Cu3(PO4)3?
a) Na2CO3 only
b) Pb(NO3)2 and Na2CO3
c) Mg(OH)2, Na2CO3, and Cu3(PO4)3
d) Mg(OH)2, AgI ,and Cu3(PO4)3
e) Pb(NO3)2, AgI, Na2CO3, and Cu3(PO4)3

b

What reaction occurs when aqueous solutions of magnesium nitrate and potassium iodide are mixed?
a) Mg^2+(aq) + 2K^+(aq) -> MgK2(s)
b) Mg^2+(aq) + 2I^-(aq) -> MgI2(s)
c) NO3^-(aq) + K^+(aq) -> KNO3(s)
d) Mg^2+(aq) + 2 NO3^-(aq) + 2K^+(aq) + 2I^-(aq) -> MgI2(s) + 2KNO3(s)
e) no reaction occurs

e

Write a balanced net ionic equation for the reaction of aluminum hydroxide, Al(OH)3, with nitric acid.
a) Al(OH)3(s) + 3H^+(aq) -> Al^3+(aq) + 3H2O
b) Al(OH)3(s) + 3H^+(aq) -> AlH3(s) + 3OH^-(aq)
c) (OH)3(aq) + 3H^+(aq) -> 3H2O
d) 3OH^-(aq) + 3H^+(aq) -> 3H2O
e) Al^3+(aq) + 3NO3^-(aq) -> Al(NO3)3(aq)

a

Write a balanced net ionic equation for the reaction of aqueous solutions of lead (II) nitrate and potassium chloride.
a) Pb(NO3)2(aq) + 2KCl(aq) -> PbCl2(s) + 2 KNO3(aq)
b) Pb^2+(aq) + 2K^+(aq) -> PbK2(s)
c) Pb^2+(aq) + 2Cl^-(aq) -> PbCl2(s)
d) NO3^-(aq) + K^+(aq) -> KNO3(s)
e) no precipitation occurs

c

Identify all of the spectator ions in the precipitation reaction below.
Ca^2+(aq) + 2Br^-(aq) + 2Li^+(aq) + CO3^2-(aq) -> CaCO3(s) + 2Li^+(aq) + 2Br^-(aq)
a) Ca^2+ and Li^+
b) Br^- and CO3^2-
c) Br^- and Li^+
d) CaCO3
e) Ca^2+, Br^-, Li^+, and CO3^2-

c

According to the Arrhenius acid-base definition
a) acids produce H^+ in aqueous solutions and bases produce OH^- in aqueous solutions
b) acids produce OH^- in aqueous solutions and bases produce H^+ in aqueous solutions
c) acids only react with bases
d) all hydrogen halides are strong acids
e) acids and bases are strong electrolytes

a

Which list contains only strong acids?
a) HCl, HNO3, HF, HClO4
b) H2SO4, H3PO4, HClO4, NH3
c) HCl, HNO3, H3PO4, HClO4
d) HCl, H2SO4, HClO4, HI
e) HNO3, H2SO4, NaOH, H3PO4

d

NH3(aq) is a
a) strong base
b) strong acid
c) weak base
d) weak acid
e) neither an acid nor a base

c

What is the balanced net ionic equation for the reaction between aqueous solutions of acetic acid and sodium hydroxide?
a) CH3CO2H(aq) + OH^-(aq) -> CH3(aq) + CO3^2-(aq) + H2(aq)
b) CH3CO2H(aq) + 3NaOH(aq) -> CCO2H^3-(aq) + 3Na^+(aq) + H2O
c) CH3CO2H(aq) + OH^-(aq) -> CH3^-(aq) + CO2(g) + H2O
d) CH3CO2H(aq) + OH^-(aq) -> CH3CO2^-(aq) + H2O
e) CH3CO2H(aq) + 2Na^+(aq) + 2OH^-(aq) -> CH3CO2^2-(aq) + 2Na^+(aq) + H2O

d

When HCl(g) and NH3(g) are mixed, a white solid forms. What is the balanced equation for this reaction?
a) HCl(g) + NH3(g) -> NH4Cl(s)
b) HCl(g) + NH3(g) -> NH2Cl(g) + H2(s)
c) HCl(g) + NH3(g) -> NH4(s) + Cl(g)
d) HCl(g) + NH3(g) -> NH2Cl(s) + H2(g)
e) 3HCl(g) + NH3(g) -> NCl3(s) + 3H2(g)

a

What is the balanced net ionic equation for the neutralization of aqueous solutions of sodium hydroxide and perchloric acid, HClO4?
a) OH^-(aq) + HClO4(aq) -> H2O + ClO4^-(aq)
b) NaOH(aq) + H^+(aq) -> H2O + Na^+(aq)
c) Na^+(aq) + ClO4^-(aq) -> NaClO4(s)
d) OH^-(aq) + H^+(aq) ->H2O
e) None of the above are correct

d

In the laboratory, acid spills are often neutralized by adding sodium bicarbonate. What mass of sodium bicarbonate reacts with 225 mL of 6.00 M HCl?
H^+(aq) + NaHCO3(s) -> H2O + CO2(g) + Na^+(aq)
a) 1.35 g
b) 71.5 g
c) 113 g
d) 143 g
e) 2240 g

c

A 25.00 mL sample of vinegar is diluted with water to a final volume of 250.0 mL. A 25.00 mL portion of the diluted vinegar is then titrated with 0.0998 M NaOH. If 22.43 mL of NaOH is required to reach the equivalence point, what is the original concentration of acetic acid in the vinegar?
CH3CO2H(aq) + OH^-(aq) -> CH3CO2^-(aq) + H2O
a) 0.0538 M
b) 0.0895 M
c) 0.538 M
d) 0.895 M
e) 5.38 M

d

The principle ingredient in Tums antacid tablets is calcium carbonate, CaCO3. A single tablet contains 0.500 g CaCO3. What volume of 0.2500 M HCl is required to titrate a tablet of Tums?
2H^+(aq) + CO3^2-(aq) -> H2O + CO2(g)
a) 0.0100 mL
b) 0.0200 mL
c) 10.0 mL
d) 20.0 mL
e) 40.0 mL

e

A reducing agent is a species that
a) takes a proton from an Arrhenius acid
b) is reduced in a chemical reaction
c) gains electrons in a chemical reaction
d) loses electrons in a chemical reaction
e) gives a proton to an Arrhenius base

d

Assign oxidation numbers to each atom in calcium perchlorate, Ca(ClO4)2.
a) Ca=0; Cl=0; O=0
b) Ca=0; Cl=-1; O=-2
c) Ca=+2; Cl=-1; O=-2
d) Ca=+2; Cl=+5; O=-2
e) Ca=+2; Cl=+7; O=-2

e

Assign oxidation numbers to each atom in manganese(IV) oxide.
a) Mn=+4;O=0
b) Mn=+4;O=-2
c) Mn=+2;O=0
d) Mn=+2;O=-2
e) Mn=0;O=0

b

What is the reduction half-reaction for the equation below?
5Fe^2+(aq) + MnO4^-(aq) + 8H^+(aq) -> 5Fe^3+(aq) + Mn^2+(aq) + 4H2O

a) MnO4^-(aq) + 5e^- -> Mn^2+(aq) + 2O2(g)
b) MnO4^-(aq) + 8 H^+(aq) +5e^- -> Mn^2+(aq) + 4H2O
c) Fe^2+(aq) + e^- -> Fe^3+(aq)
d) 8H^+(aq) + 8e^- -> 8H2O
e) none of the above

b

Identify the reaction type for the reaction between potassium metal and hydrochloric acid.
2K(s) + 2H^+(aq) -> 2K^+(aq) + H2(g)
a) precipitation
b) acid-base
c) oxidation-reduction
d) both a and c
e) none of the above

c

If the volume of a confined gas is doubled at constant temperature, what change is observed?
a) the pressure of the gas is decreased to 1/4 of its original value
b) the pressure of the gas is decreased to 1/2 of its original value
c) the pressure of the gas is increased to twice its original value
d) the density of the gas is doubled
e) the velocities of the molecules are doubled

b

Place the following units of pressure in order from lowest to highest pressure
a) 1 atm<1 Pa<1 mm Hg<1 bar
b) 1 mm Hg<1 bar<1 atm<1 Pa
c) 1 Pa<1 mm Hg<1 bar<1 atm
d) 1 Pa<1 mm Hg<1 atm<1 bar
e) 1 bar<1 mm Hg<1 Pa<1 atm

c

Avogadro's law states that
a) 1 liter of any gas contains 6.02 x 10^23 gas molecules
b) the volume of a gas is directly proportional to its temperature
c) the gas constant equals 0.0821 L x atm/(mol x K) for all gases
d) the volume of a gas must always be constant
e) equal volumes of all gases at the same pressure and temperature contain an equal number of moles

e

The molar mass of helium and oxygen are 4.0g/mol and 16g/mol, respectively. At the same temperature and pressure, 1 mole of helium will occupy
a) the same volume as 1 mole of oxygen
b) four times the volume of 1 mole of oxygen
c) twice the volume of 1 mole of oxygen
d) half the volume of 1 mole of oxygen
e) one fourth the volume of 1 mole of oxygen

a

A bicycle tire is filled to a pressure of 4.42 atm (65 psi) at a temperature of 12 degrees Celsius. If the temperature increases to 33 degrees Celsius, what is the pressure in the tire? Assume the volume of the tire is constant.
a) 4.75 atm
b) 5.91 atm
c) 9.28 atm
d) 12.1 atm
e) 16.1 atm

a

At 108 degrees Celsius, the pressure in a 10.0 L flask is 874 mm Hg. How many moles of gas are in the flask?
a) 0.368 mol
b) 0.873 mol
c) 1.30 mol
d) 348 mol
e) 986 mol

a

A 3.00 L flask contains 2.33 g of argon gas at 312 mm Hg. What is the temperature of the gas?
a) 151 K
b) 257 K
c) 292 K
d) 341 K
e) 4890 K

b

A mass of 5.0 grams of dry ice, CO2(s), is sealed in an evacuated 2.0 L plastic soda bottle. What is the pressure inside the bottle when the CO2 is heated to 35 degrees Celsius?
a) 0.16 atm
b) 1.4 atm
c) 8.9 atm
d) 18 atm
e) 63 atm

b

25.0 L of hydrogen gas at 50.0 atm and 25 degrees Celsius expands to 65.0 L and is subsequently heated to 35 degrees Celsius. What is the new pressure?
a) 19.9 atm
b) 25.2 atm
c) 26.9 atm
d) 28.4 atm
e) 31.2 atm

a

What volume of oxygen (O2) at 22 degrees Celsius and 1.00 atm contains the same number of molecules as 0.400 L H2 at 45 degrees Celsius and 1.00 atm?
a) 0.251 L
b) 0.298 L
c) 0.371 L
d) 0.400 L
e) 0.431 L

c

A volatile compound with a mass of 0.8822 grams is placed in an evacuated 0.250 L flask. The flask is heated to evaporate the compound. At 99 degrees Celsius, the pressure in the flask is 1.25 atm. What is the molar mass of the compound?
a) 86.2 g/mol
b) 116 g/mol
c) 229 g/mol
d) 257 g/mol
e) 303 g/mol

a

What is the density of argon gas at 25 degrees Celsius and 1.00 atm?
a) 0.0110 g/L
b) 1.63 g/L
c) 19.5 g/L
d) 977 g/L
e) 1.24 x 10^3 g/L

b

At 1.00 km above sea level, the atmospheric pressure is 675 mm Hg and the temperature is 282 K. If nitrogen comprises 78.1% (mole percent) of air, what is the density of nitrogen at this height?
a) 0.0238 g/L
b) 0.521 g/L
c) 0.839 g/L
d) 1.07 g/L
e) 638 g/L

c

A mass of 0.650 grams of calcium carbonate is added to 50.0 mL of 0.275 M HCl. If the CO2(g) gas is collected in a 1.00 L flask at 25 degrees Celsius, what is the pressure of CO2(g) in the flask?
CaCO3(s) + 2H^+(aq) -> Ca^2+(aq) + H2O(l) + CO2(g)
a) 0.0129 atm
b) 0.0583 atm
c) 0.159 atm
d) 0.314 atm
e) 15.9 atm

c

The composition (in mole percent) of the atmosphere is 78.1% N2, 21.0% O2, and 0.9% Ar. What is the partial pressure of each gas when the barometric pressure is 754.1 mm Hg
a) N2=21.1 atm, O2=6.5 atm, Ar=0.3 atm
b) N2=78.1 mm Hg, O2=21.0 mm Hg, Ar=0.9 mm Hg
c) N2=244 mm Hg, O2=244 mm Hg, Ar=244 mm Hg
d) N2=405 mm Hg, O2=234 mm Hg, Ar= 293 mm Hg
e) N2=589 mm Hg, O2=158 mm Hg, Ar=7 mm Hg

e

Sulfur burns in oxygen with a deep blue flame to produce sulfur dioxide. If 5.85 g S8 and 1.00 atm of O2 completely react in a 5.00 L flask at 25 degrees Celsius, determine the partial pressure of SO2 and the total pressure in the flask.
S8(s) + 8O2(g) -> 8SO2(g)
a) O2=0 atm , SO2=1.00 atm ,total pressure=1.00 atm
b) O2=0.093 atm , SO2=0.917 atm ,total pressure=1.00 atm
c) O2=0.107 atm , SO2=0.893 atm ,total pressure=1.00 atm
d) O2=0.855 atm , SO2=0.145 atm ,total pressure=1.00 atm
e) O2=0.917 atm , SO2=0.163 atm ,total pressure=1.08 atm

c

An unknown mass of ammonium perchlorate, NH4ClO4 (117.5 g/mol), is placed in an evacuated 1.00 L flask and heated to 251 degrees Celsius. At this temperature the NH4ClO4 decomposes violently. The gaseous products exert a pressure of 466 mm Hg at 251 degrees Celsius. What mass of NH4ClO4 was placed in the flask?
2NH4ClO4(s) -> N2(g) + Cl2(g) + 2O2(g) + 4H2O(g)
a) 0.149 g
b) 0.419 g
c) 0.682 g
d) 1.67 g
e) 3.19 g

b

Water can be decomposed by electrolysis to hydrogen gas and oxygen gas. What mass of water must decompose to yield 24.0 L of oxygen gas at 1.00 atm and 25 degrees Celsius?
2H2O(l) -> 2H2(g) + O2(g)
a) 11.1 g
b) 17.7 g
c) 23.6 g
d) 35.3 g
e) 70.7 g

d

A mixture of methane and helium is placed in a 2.0 L flask at 27 degrees Celsius. The partial pressure of CH4 is 0.72 atm and the partial pressure of helium is 0.22 atm. What is the mole fraction of methane?
a) 0.23
b) 0.29
c) 0.50
d) 0.77
e) 3.5

d

All of the following are properties of gases according to the kinetic theory EXCEPT
a) gases consist of mostly empty space
b) attractive forces cause gas molecules to collide
c) gas pressure is caused by collisions of molecules with the container walls
d) collisions between gas molecules are elastic
e) gas molecules are in constant motion

b

The average kinetic energy of a gas molecule is
a) directly proportional to its average speed
b) directly proportional to the square of its mass
c) directly proportional to the square of its average speed
d) inversely proportional to its average speed
e) inversely proportional to the square of its mass

c

If a gas effuses 1.73 times faster than Kr, what is its molar mass?
a) 16.0 g/mol
b) 28.0 g/mol
c) 36.6 g/mol
d) 55.4 g/mol
e) 126.9 g/mol

b

In an experiment, argon is allowed to effuse through a tiny opening into an evacuated 5.00 x 10^2 mL flask for 30.0 seconds, at which point the pressure in the flask is found to be 15.0 mm Hg. The experiment is repeated using unknown gas at the same temperature and pressure. After 30.0 seconds, the pressure is found to be 47.4 mm Hg. What is the molar mass of the gas?
a) 4.00 g/mol
b) 16.0 g/mol
c) 28.0 g/mol
d) 32.0 g/mol
e) 83.8 g/mol

a

The lowest frequency available on a radio's AM dial is 570 kHz. What is the wavelength of this light?
a) 1.8 x 10^-7 m
b) 1.8 x 10^-6 m
c) 1.9 x 10^-3 m
d) 5.3 x 10^2 m
e) 5.3 x 10^4 m

d

A microwave oven emits radiation at a frequency of 6.00 x 10^10 Hz. What is the wavelength of this light?
a) 3.98 x 10^-23 m
b) 1.67 x 10^-11 m
c) 5.00 x 10^-3 m
d) 2.00 x 10^-2 m
e) 2.00 x 10^-1 m

c

Place the following regions of the electromagnetic spectrum in order from longest to shortest wavelength.
a) radio> microwave> visible> ultraviolet> gamma ray
b) gamma ray> microwave> radio> visible> ultraviolet
c) ultraviolet> visible> microwave> radio> gamma ray
d) microwave> radio> ultraviolet> visible> gamma ray
e) visible> gamma ray> radio> ultraviolet> microwave

a

Place the following regions of the electromagnetic spectrum in order from highest to lowest energy.
a) infrared> gamma rays> x-rays> visible> radio
b) gamma rays> x-rays> visible> infrared> radio
c) x-rays> gamma rays> infrared> visible> radio
d) radio> x-rays> gamma rays> visible> infrared
e) visible> infrared> radio> x-rays> gamma rays

b

When Cs-137 decays, it emits gamma radiation. The energy of one photon is 1.06 x 10^-13 J. What is the wavelength of this radiation?
a) 1.87 x 10^-12 m
b) 2.08 x 10^-12 m
c) 2.44 x 10^-12 m
d) 1.88 x 10^-11 m
e) 1.58 x 10^-10 m

a

The Schrodinger wave equation
a) proves electrons have positive and negative spins
b) calculates the precise and momentum of an electron at any given time
c) is used to compute the wavelength of small particles
d) can be solved to find the probability of finding an electron in a region of space
e) proves that photons are particles

d

Which of the following sets of quantum numbers refers to a 2s orbital?
a) n=1,l=2,m(little l)=2,m(little s)=+1/2
b) n=1,l=2,m(little l)=1,m(little s)=+1/2
c) n=2,l=2,m(little l)=0,m(little s)=+1/2
d)n=2,l=1,m(little l)=-1,m(little s)=+1/2
e) n=2,l=0,m(little l)=0,m(little s)=+1/2

e

How many orbitals have the following quantum numbers: n=4, l=1
a) 0
b) 1
c) 3
d) 4
e) 5

c

How many orbitals have the following quantum numbers: n=6, l=2, m(little l)=-2
a) 0
b) 1
c) 3
d) 5
e) 6

b

What is the total capacity of electrons in n=5, l=3
a) 2
b) 6
c) 10
d) 14
e) 32

d

What type of orbital is designated by n=5, l=2, m(little l)=+1
a) 5d
b) 2f
c) 5p
d) 2s
e) 5p

a

What is the symbol of the atom or ion with the following orbital diagram?

1s: (^v) 2s: (^v) 2p: (^v)(^ )(^ )

a) 5B
b) 7N
c) 8O
d) 16S
e) 9F

c

What is the symbol of the atom or ion with the following orbital diagram?

1s: (^v) 2s: (^v) 2p: (^v)(^v)(^v) 3s: (^v)

3p: (^v)(^v)(^v) 3d: (^v)(^v)(^v)(^ )(^ )

4s: ( )

a) 26Fe
b) 26Fe^2+
c) 27Co^+
d) 28Ni
e) 28Ni^2+

e

What is the correct orbital diagram for phosphorous?
a) 1s: (^v) 2s: (^v) 2p: (^ )(^ )(^ )

b) 1s: (^v) 2s: (^v) 2p: (^v)(^ )( )

c) 1s: (^v) 2s: (^v) 2p: (^v)(^v)(^v) 3s: (^v) 3p: (^v)(^ )( )

d) 1s: (^v) 2s: (^v) 2p: (^v)(^v)(^v) 3s: (^v) 3p: (^ )(^ )(^ )

e) 1s: (^v) 2s: (^v) 2p: (^v)(^v)(^v) 3s: (^ ) 3p: (^v)(^ )(^ )

d

What is the correct orbital diagram for Fe^2+?
a) [Ar] 3d: (^ )(^ )(^ )(^ )( ) 4s: (^v)
b) [Ar] 3d: (^ )(^ )(^ )(^ )(^ ) 4s: (^ )
c) [Ar] 3d: (^ )(^ )(^ )(^ )(^ ) 4s: ( )
d) [Ar] 3d: (^v)(^ )(^ )(^ )(^ ) 4s: ( )
e) [Ar] 3d: (^v)(^v)(^ )( )( ) 4s: ( )

c

In general, ionization energies
a) increase down a group and increase across a period
b) increase down a group and decrease across a period
c) decrease down a group and increase across a period
d) decrease down a group and decrease across a period
e) increase with atomic mass and increase with atomic radii

c

In general, atomic radii
a) increase down a group and decrease across a period
b) increase down a group and increase across a period
c) decrease down a group and decrease across a period
d) are proportional to atomic mass
e) decrease down a group and increase across a period

a

Place the following atoms in order of increasing size: Al, Cl, Mg, O, and P
a) Cl<O<P<Al<Mg
b) Cl<P<Al<Mg<O
c) O<Cl<P<Al<Mg
d) O<Mg<Al<P<Cl
e) none of the above

c

Electronegativity increases
a) moving down a group in the periodic table
b) moving from left to right across the periodic table
c) with increasing atomic mass
d) when electrons are paired
e) with increasing atomic radii

b

What is the expected number of valence electrons for an element in group 15?
a) 0
b) 1
c) 3
d) 5
e) 8

d

How many total valence electrons are present in nitrogen dioxide?
a) 8
b) 12
c) 17
d) 18
e) 24

c

Which of the following is a correct Lewis structure for C2H60O?
a) central atoms: O (connected to a H and surrounded by 2 electrons on both the top and bottom), C1 (connected to 2 H's), and C2 (connected to 3 H's)

b) central atoms: O (connected to a H, surrounded by 2 electrons on the top, and double bonded to C1), C1 (connected to 2 H's), and C2 (connected to 3 H's)

c) central atoms: O (in the center, surrounded by 2 electrons on both the top and bottom), C1 (connected to 3 H's), and C2 (connected to 3 H's)

d) answers a and c are correct
e) answers a, b, and c are correct

d

Which Lewis structure is possible for N2O?
a) N1(has 2 electrons on left, triple bond on right), N2(triple bonded to N1 on left, double bonded to O on right), O(double bonded to N2 on left, 2 pairs of valence electrons on right)

b) N1(has 2 electrons on left, triple bond on right), N2(triple bonded to N1 on left,bonded to O on right), O(bonded to N2 on left, 3 pairs of valence electrons on right)

c) N1(has 2 electrons on left, triple bond on right), N2(triple bonded to N1 on left, 2 electrons on top, bonded to O on right), O(bonded to N2 on left, 3 pairs of valence electrons on right)

d) N1(has 2 pairs of electrons on left, double bond on right), N2(double bonded to N1 on left, bonded to O on right), O(bonded to N2 on left, 3 pairs of valence electrons on right)

e) N1(has 2 electrons on left, double bond on right), N2(double bonded to N1 on left, 2 electrons on top, bonded to O on right), O(bonded to N2 on left, 3 pairs of valence electrons on right)

b

Which of the following is not a correct Lewis structure?
NO2: O(2 pairs)-N(1 e)-O(3 pairs)
NO2^-: [O(2 pairs)=N(1 pair)-O(3 pairs)]-
NO: N(2 pairs)=O(2 pairs)
N2O: N(1 pair)triple bondN-O(3 pairs)

a) NO2
b) NO2^-
c) NO
d) N2O
e) all of the above are correct structures

c

Which of the following elements is most likely to form a molecule or ion that exceeds the octet rule?
a) Na
b) S
c) B
d) F
e) C

b

What is the correct Lewis structure of SF4?
a) S in middle connected to 4 F's with 3 pairs each
b) S in middle with 1 pair connected to 4 F's with 3 pairs each
c) S in middle with 3 single bonded F's with 3 pairs each and 1 double bonded F with 3 pairs
d) S in middle with 2 pairs connected to 4 F's with 3 pairs each (making an X)
e) S in middle with 2 pairs on left connected to 4 F's with 3 pairs each (making a K)

b

Which of the following are correct resonance structures of SO3?
1: S in the middle double bonded to 2 O's with 3 pairs on one and 2 pairs on the other and single bonded to another O with 3 pairs

2: S in the middle single bonded to 2 O's with 3 pairs each and double bonded to another O with 2 pairs

3: O in the middle single bonded to 2 O's with 3 pairs each and double bonded to one S with 2 pairs

4: S in the middle double bonded to an O with 2 pairs and single bonded to 2 O's with 3 pairs each

5: S in the middle single bonded to 3 O's, 2 with 3 pairs and 1 with 2 pairs

a) 1 and 5
b) 2 and 4
c) 1, 2, and 4
d) 2, 3, and 4
e) 1, 2, 4, and 5

b

How many possible resonance structures exist for sulfur trioxide?
a) 3
b) 4
c) 5
d) 6
e) 8

a

How many possible resonance structures exist for the formate ion, HCO2^-
a) 0
b) 2
c) 3
d) 4
e) 8

b

Which of the following species has a Lewis structure with a molecular geometry similar to CS2?
a) H2S
b) NO2^-
c) NO2
d) H2O
e) SCN^-

e

Which of the following species has a Lewis structure with a molecular geometry similar to NH3?
a) CO3^2-
b) BH3
c) H3O^+
d) ICl3
e) SO3

c

Which of the following species has a Lewis structure with a molecular geometry similar to SO3?
a) NH3
b) ICl3
c) CO3^2-
d) SO3^2-
e) PCl3

c

Use VSEPR theory to predict the molecular geometry of SO3^2-.
a) bent
b) tetrahedral
c) square planar
d) triangular planar
e) triangular pyramidal

e

Use VSEPR theory to predict the molecular geometry of SF6.
a) bent
b) linear
c) triangular planar
d) t-shaped
e) octahedral

e

Use VSEPR theory to predict the molecular geometry of NH4^+.
a) triangular pyramidal
b) square pyramidal
c) see-saw
d) tetrahedral
e) triangular planar

d

Which of the following species have the same molecular geometry: XeF4, ClF4^+, SF4, PO4^3-?
a) XeF4 and SF4
b) ClF4^+ and SF4
c) ClF4^+ and PO4^3-
d) XeF4 and ClF4^+
e) XeF4, SF4, and PO4^3-

b

What are the bond angles in a phosphate ion?
a) 90 degrees
b) 109.5 degrees
c) 120 degrees
d) 90 and 120 degrees
e) 180 degrees

b

What are the approximate bond angles in SF4?
a) 90 degrees
b) 109.5 degrees
c) 120 degrees
d) 90 and 120 degrees
e) 180 degrees

d

See More

Please allow access to your computer’s microphone to use Voice Recording.

Having trouble? Click here for help.

We can’t access your microphone!

Click the icon above to update your browser permissions above and try again

Example:

Reload the page to try again!

Reload

Press Cmd-0 to reset your zoom

Press Ctrl-0 to reset your zoom

It looks like your browser might be zoomed in or out. Your browser needs to be zoomed to a normal size to record audio.

Please upgrade Flash or install Chrome
to use Voice Recording.

For more help, see our troubleshooting page.

Your microphone is muted

For help fixing this issue, see this FAQ.

Star this term

You can study starred terms together

NEW! Voice Recording

Create Set