Chem 109 Final
a
Potassium forms an ion with a charge of __________. a. 1+ b. 2+ c. 2- d. 0 e. 1-
d
1 kilogram = __________ milligrams a. 1 ´ 10-6 b. 1,000 c. 10,000 d. 1,000,000 e. none of the above
a
1 picometer = __________ centimeters a. 1 ´ 10-10 b. 1 ´ 1010 c. 1 ´ 10-8 d. 1 ´ 10-12 e. 1 ´ 108
1) A
1) In the following list, only __________ is not an example of matter. A) light B)elemental phosphorus C)dust D) table salt E)planets
SnF4
Determine the empirical formula of the following compound if a sample contains 5.28 gSn and 3.37 gF;
10) A
10) Which of the following is an illustration of the law of constant composition? A) Water is 11% hydrogen and 89% oxygen by mass. B)Water and salt have different boiling points. C)Water is a compound. D) Water can be separated into other substances by a chemical process. E)Water boils at 100 C at 1 atm pressure.
11) C
11) Which one of the following is not a physical property of water? A) It boils at 100C at 1 atm pressure. B)It freezes at 0C at 1 atm pressure. C)It reacts rapidly with potassium metal to form potassium hydroxide. D) It is clear and colorless. E)Water exists in solid, liquid and gaseous forms.
12) B
12) Of the following, only __________ is a chemical reaction. A) melting of lead B)tarnishing of silver C)crushing of stone D) dissolving sugar in water E)dropping a penny into a glass of water
13) D
13) Which one of the following is an intensive property? A) mass B)volume C)heat content D) temperature E)amount
14) D
14) Of the following, only __________ is an extensive property. A) density B)boiling point C)freezing point D) mass E)pressure
15) E
15) Which of the following are chemical processes? 1. rusting of a nail 2. freezing of water 3. decomposition of water into hydrogen and oxygen gases 4. compression of oxygen gas A) 2, 3, 4 B)1, 2 C)1, 4 D) 1, 3, 4 E)1, 3, 2
16) B
16) Which of the following is a chemical property of sodium chloride? A) It is a solid at room temperature. B)It can be decomposed into sodium metal and chlorine gas. C)It is not significantly compressible. D) It melts at a high temperature. E)It dissolves in water.
17) C
17) Intensive properties __________ depend on the amount of matter present. Extensive properties __________ depend on the amount of matter present. A) do, sometimes B)don't, don't C)don't, do D) do, do E)do, don't
18) A
18) Of the objects below, __________ is the most dense. A) an object with a volume of 3.91 x 10-24nm3 and a mass of 7.93 x 10-1ng B)an object with a volume of 13 dm3and a mass of 1.29 x10 3g C)an object with a volume of 139 mL and a mass of 93 g D) an object with a volume of 0.00212 m3 and a mass of 4.22 x 10 4mg E)an object with a volume of 2.5 L and a mass of 12.5 kg
19) E
19) The temperature of 25C is __________ in Kelvins. A) 166 B)248 C)103 D) 138 E)298
2) A
2) What is the physical state in which matter has no specific shape but does have a specific volume? A) liquid B)solid C)ice D) gas E)salts
20) A
20) Express the temperature, 422.35 K, in degrees Celsius and in degrees Fahrenheit. A) 149.20C, 300.56F B)50.89C, 324.04F C)22.78C, 98.60F D) 695.50C, 354.39F E)792.23C, 519.08F
21) E
21) A temperature of __________ K is the same as 63F. A) 336 B)17 C)276 D) 29 E)290
22) A
22) What is the volume of a 12.2 g piece of metal with a density of 9.43 g/cm3? A) 1.29 cm 3 B)12.2 cm 3 C)115 cm 3 D) 0.773 cm 3 E)none of the above
23) E
23) What is the density (in g/cm 3) of a gold nugget that has a volume of 1.68 cm 3 and a mass of 32.4 g? A) 54.4 B)0.0519 C)32.4 D) 0.0184 E)19.3
24) E
24) The density of silver is 10.5 g/cm 3. What volume (cm 3) would be occupied by a piece of silver with a mass of 61.3 g? A) 0.171 B)10.5 C)0.00155 D) 644 E)5.84 3
E
25) Osmium has a density of 22.6 g/cm 3. What volume (in cm 3) would be occupied by a 21.8 g sample of osmium? A) 1.04 B)493 C)2.03 x 10 3 D) 2.03 x 10 -3 E)0.965
C
26) A cube of an unknown metal measures 1.61 mm on one side. The mass of the cube is 36 mg. Which of the following is most likely the unknown metal? Metal Density (g/cm 3) rhodium 12.4 copper 8.96 niobium 8.57 vanadium 6.11 zirconium 6.51 A) copper B)zirconium C)niobium D) vanadium E)rhodium
27) B
27) Precision refers to __________. A) how close a measured number is to the true value B)how close a measured number is to other measured numbers C)how close a measured number is to infinity D) how close a measured number is to the calculated value E)how close a measured number is to zero
28) D
28) How many significant figures are there in the number 0.00230? A) 5 B)6 C)4 D) 3 E)2
29) E
29) What is the correct answer (reported to the proper number of significant figures) to the following? 6.3 x 3.25 = _____ A) 20.5 B)20.48 C)21 D) 20.475 E)20
3) E
3) A combination of sand, salt, and water is an example of a __________. A) pure substance B)homogeneous mixture C)compound D) solid E)heterogeneous mixture
c
3.337 g/cm3 = __________ kg/m3 a. 0.3337 b. 333.7 c. 3337 d. 3.337 ´ 10-5 e. 3.337 ´ 10-9
30) D
30) One side of a cube measures 1.55 m. What is the volume of this cube in cm 3? A) 2.40 B)155 C)2.40 x 10 4 D) 3.72 x 10 6 E)3.72
D
31) The number with the most significant zeros is __________. A) 0.00002510 B)2.5100000 C)2.501 10 -7 D) 250000001 E)0.02500001
A
32) The correct result of the following addition is __________. 12 1.2 0.12 + 0.012 A)13 B)13.3 C)13.33 D) 13.332 E)none of the above
C
33) There are 6 significant figures in the number __________. A) 4.2010 B)1.003702 C)1000.00 D) 0.003702 E)none of the above
4) D
4) Which one of the following has the element name and symbol correctly matched? A) P, potassium B)Mg, manganese C)Sn, silicon D) Ag, silver E)C, copper
E
34) (0.002843) (12.80184) 0.00032 = __________ A) 113.7 B)113.74 C)113.73635 D) 113.736 E)1.1 x 10 2
B
35) Round the number 0.007225 to three significant figures. A) 0.00723 B)0.00722 C)0.007225 D) 0.007 E)0.0072
36) A
36) Round the number 0.07535 to two significant figures. A) 0.075 B)0.07535 C)0.076 D) 0.0754 E)0.08
37) B
37) How many significant figures should be retained in the result of the following calculation? (11.13 - 2.6) x 10 4 (103.05 + 16.9) x 10 -6 A) 1 B)2 C)3 D) 4 E)5
38) C
38) The output of a plant is 4335 pounds of ball bearings per week (five days). If each ball bearing weighs 0.0113 g, how many ball bearings does the plant make in a single day? A) 3.84 x 10 5 B)7.67 x 10 4 C)3.48 x 10 7 D) 2.91 x 10 6 E)867
39) E
39) One edge of a cube is measured and found to be 13 cm. The volume of the cube in m 3 is __________. A) 2.2 x 10 -6 B)2.2 C)2.2 x 10 3 D) 2.2 x 10 6 E)2.2 x 10 -3 5
5) E
5) Which one of the following is a pure substance? A) salt water B)concrete C)milk D) wood E)elemental copper
6) Tin
6) Sn is the symbol for the element __________.
mole
6.02 x 10^23
7) C
7) The symbol for the element magnesium is __________.
8) B
8) If matter is uniform throughout and cannot be separated into other substances by physical means, it is _ _________. A) a compound B)either an element or a compound C)a homogeneous mixture D) an element E)a heterogeneous mixture
9) B
9) Homogeneous mixtures are also known as __________. A) elements B)solutions C)compounds D) solids E)substances
Of the following ____ wavelength has the shortest wavelength A)xray B)radio C)microwave D)ultraviolet E)infared
A
in the reaction below, delta H f is zero for _____. Ni(s)+2CO(g)+2PF3--->Ni(CO)2(PF3)2 A) Ni B)Co C)PF3 D)NiCO2PF3 E) both B and C
A
a
A 100-watt electric incandescent light bulb consumes __________ J of energy in 24 hours. [1 Watt (W) = 1 J/sec] a. 8.64 ´ 106 b. 2.40 ´ 103 c. 8.64 ´ 103 d. 2.10 ´ 103 e. 4.17
0.423
A 17.5 mL sample of an acetic acid (CH3CO2H) solution required 29.6 mL of 0.250 M NaOH for neutralization. The concentration of acetic acid was __________ M.
0.0102
A 31.5 mL aliquot of HNO3 (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was __________. 1.02 0.0051 0.0204 0.227 0.0102
d
A 36.3 mL aliquot of 0.0529 M H2SO4 (aq) is to be titrated with 0.0411 M NaOH (aq). What volume (mL) of base will it take to reach the equivalence point? a. 3.84 b. 1.92 c. 187 d. 93.4 e. 46.7
e
A compound that is composed of carbon, hydrogen, and oxygen contains 70.6% C, 5.9% H, and 23.5% O by mass. The molecular weight of the compound is 136 amu. What is the molecular formula? a. C9H12O b. C5H6O2 c. C4H4O d. C8H4O e. C8H8O2
d
A compound was found to be soluble in water. It was also found that addition of acid to an aqueous solution of this compound resulted in the formation of carbon dioxide. Which one of the following cations would form a precipitate when added to an aqueous solution of this compound? a. Na+ b. Rb+ c. NH4+ d. Cr3+ e. K+
e
A correct name for Fe(NO3)2 is __________. a. ferrous nitrite b. ferric nitrite c. ferric nitrate d. iron nitrite e. ferrous nitrate
d
A mole of red photons of wavelength 725 nm has __________ kJ of energy. a. 227 b. 2.74 ´ 10-19 c. 4.56 ´ 10-46 d. 165 e. 6.05 ´ 10-3
c
A neutralization reaction between an acid and a metal hydroxide produces __________. a. ammonia b. sodium hydroxide c. water and a salt d. hydrogen gas e. oxygen gas
B
A sample of CH4O with a mass of 32.0 g contains ________ molecules of CH4O. A)5.32x10^-23 B)1.00 C)1.88x10^22 D)6.02x10^23 E) 32.0
d
A sample of aluminum metal absorbs 9.86 J of heat, upon which the temperature of the sample increases from 23.2°C to 30.5°C. Since the specific heat capacity of aluminum is 0.90 J/g-K, the mass of the sample is __________ g. a. 8.1 b. 65 c. 72 d. 1.5 e. 6.6
b
A strong electrolyte is one that __________ completely in solution. a. reacts b. ionizes c. disappears d. associates
79.7%
A student performs an experiment that produces 5.78 grams of silver chloride. He calculated that 7.25 grams of silver chloride should have precipitated if all of the limiting reactant reacted. What is his percent yield? 125% 20.3% 79.724% 79.7%
a
A valid Lewis structure of __________ cannot be drawn without violating the octet rule. a. CCl4 b. ClF3 c. PCl3 d. CO2 e. SO3
e
A valid Lewis structure of __________ cannot be drawn without violating the octet rule. a. NI3 b. SiF4 c. SO2 d. CO2 e. ICl5
b
A weak electrolyte exists predominantly as __________ in solution. a. an isotope b. molecules c. ions d. electrons e. atoms
d
According to VSEPR theory, if there are five electron domains in the valence shell of an atom, they will be arranged in a(n) __________ geometry. a. octahedral b. tetrahedral c. trigonal planar d. trigonal bipyramidal e. linear
B
All atoms of a given element have the same __________. A) mass B) number of protons C) number of neutrons D) number of electrons and neutrons E) density
b
Aluminum forms an ion with a charge of __________. a. 1+ b. 3+ c. 3- d. 2+ e. 1-
d
Aluminum reacts with a certain nonmetallic element to form a compound with the general formula Al2X3. Element X must be from Group __________ of the Periodic Table of Elements. a. 4A b. 3A c. 7A d. 6A e. 5A
a
Aluminum reacts with a certain nonmetallic element to form a compound with the general formula AlX. Element X is a diatomic gas at room temperature. Element X must be __________. a. nitrogen b. fluorine c. chlorine d. sulfur e. oxygen
False
Amnomia is a strong base
a
An object will sink in a liquid if the density of the object is greater than that of the liquid. The mass of a sphere is 9.83 g. If the volume of this sphere is less than __________ cm3, then the sphere will sink in liquid mercury (density = 13.6 g/cm3). a. 0.723 b. 1.38 c. 134 d. 7.48 e. none of the above
(NH4)2S
Aqueous solutions of a compound did not form precipitates with Cl-, Br-, I-, SO4 2-, CO3 2-, PO4 3-, OH-, or S2-. This highly water-soluble compound produced the foul-smelling gas H2S when the solution was acidified. This compound is __________. AgNO3 Pb(NO3)2 KBr Li2CO3 (NH4)2S
0
As in As4
The ____ orbital is degeneraate with the 5py in a many electron atom A)5s B)5px C)4py D)5dxy E)5d2
B
The deBroglie wavelength of a 6 gram bullet at the speed of sound is _____. speed of sound is 331 m/sec. A)2.7 x10^-34 B)3.3x10^-34 C)3.35x10^-33 D)2.7x10^-37 E)6.6x10^-31
B
the energy released by combustion of 1 g of a substance is called the ____ of the substance. A)specific heat B)fuel value C) nutritional calorie content D) heat capacity E)enthalpy
B
which one of the following is an incorrect sub shell notation? A)4f B)2d C)3s D)2p E) 3d
B
a
Barium forms an ion with a charge of __________. a. 2+ b. 3- c. 3+ d. 2- e. 1+
SnBr2 (aq) + Cu (s) → CuBr2 (aq) + Sn (s)
Based on the activity series, which one of the reactions below will occur? Pb (s) + NiI2 (aq) → PbI2 (aq) + Ni (s) SnBr2 (aq) + Cu (s) → CuBr2 (aq) + Sn (s) Mn (s) + NiCl2 (aq) → MnCl2 (aq) + Ni (s) Fe (s) + ZnCl2 (aq) → FeCl2 (aq) + Zn (s) None of the reactions will occur.
d
Based on the equations below, which metal is the most active? Pb(NO3)2 (aq) + Ni (s) ® Ni(NO3)2 (aq) + Pb (s) Pb(NO3)2 (aq) + Ag (s) ® No reaction Cu(NO3)2 (aq) + Ni (s) ® Ni(NO3)2 (aq) + Cu (s) a. Cu b. Pb c. Ag d. Ni e. N
1
Br in HBrO
According to the Heisenberg uncertainty principle, it is impossible to know precisely both the position and ____ of an electron. A)mass B)color C) momentum D)shape E)charge
C
the kinetic energy of a 10.3 g golf ball traveling at 48.0 m/s is _______ kJ. A) 1.2x10^3 B)66 C)11.9 D)1.3x10^2 E)23.7
C
4
C in COCl2
c
Calcium forms an ion with a charge of __________. a. 1+ b. 2- c. 2+ d. 0 e. 1-
B) metal, metal
Calcium is a __________ and silver is a __________. A) nonmetal, metal B) metal, metal C) metalloid, metal D) metal, metalloid E) nonmetal, metalloid
46.1 amu
Calculate the formula weight of ethanol, C2H5OH.
601.93
Calculate the formula weight of the compound Ba3(PO4)2. 569.93 amu 184.30 amu 327.27 amu 601.93 amu
77.54
Calculate the percentage by mass of lead in PbCO3.
d
Cathode rays are __________. a. neutrons b. atoms c. x-rays d. electrons e. protons
C) electrons
Cathode rays are __________. A) neutrons B) x-rays C) electrons D) protons E) atoms
a
Chromium and chlorine form an ionic compound whose formula is CrCl3. The name of this compound is __________. a. chromium(III) chloride b. chromium(III) trichloride c. chromic trichloride d. monochromium trichloride e. chromium chlorine
a
ClF3 has "T-shaped" geometry. There are __________ non-bonding domains in this molecule. a. 2 b. 1 c. 4 d. 3 e. 0
A) Extensive B) Intensive C) Extensive D) Extensive E) Extensive
Classify each of the following as either intensive or extensive properties: A) mass B) temperature C) heat content D) volume E) amount
Na+ and i-
Combining aqueous solutions of BaI2 and Na2SO4 affords a precipitate of BaSO4. Which ion(s) is/are spectator ions in the reaction? Na+ and I− Ba2+ and SO42− SO42− and I− Ba2+ only Na+ only
e
Combining aqueous solutions of BaI2 and Na2SO4 affords a precipitate of BaSO4. Which ion(s) is/are spectator ions in the reaction? a. SO42- and I- b. Ba2+ only c. Ba2+ and SO42- d. Na+ only e. Na+ and I-
a
Combustion of a 1.031-g sample of a compound containing only carbon, hydrogen, and oxygen produced 2.265 g of CO2 and 1.236 g of H2O. What is the empirical formula of the compound? a. C3H8O b. C3H9O3 c. C3H5O d. C3H6O3 e. C6H16O2
(ii) and (iii)
Consider the following selected postulates of Dalton's atomic theory and identify the one(s) that are no longer valid: (i) Each element is composed of extremely small particles called atoms. (ii) Atoms are indivisible. (iii) Atoms of a given element are identical. (iv) Atoms of different elements are different and have different properties.
The wavelength of light emitted from a frequency of 5.75x10 ^14 Hz is _____. A)702 nm B)641 nm C)674 nm D)522 nm E) 583 nm
D
all of the orbitals in a given sub shell have the same value of the ___ quantum number A) principal B) angular momentum C)magnetic D)A and B E) B and C
D
which of the following is a statement of the first law of thermodynamics? A)Ek=(1/2)mv^2 B)A negative delta H corresponds to an exothermic process C) delta E=Efinal-Einitial D)Energy lost by the system must be gained by the surrounding E)1 cal= 4.184 J
D
K2CO3
Determine the empirical formula of the following compound if a sample contains 0.104 molK, 0.052 molC, and 0.156 molO;
NH2
Determine the empirical formula of the following compound if a sample contains 87.5% N and 12.5% H by mass.
electrons
Different isotopes of a particular element contain different numbers of __________.
protons
Different isotopes of a particular element contain the same number of __________.
in a px orbital, the subscript x denotes the ____ of an electron. A) energy B) spin of the electrons C) probability of the shell D) size of the orbital E) axis along which the orbital is aligned
E
which of the following is an endothermic process? A)ice melting B) water freezing C) boiling soup D)hydrochloric acid and barium hydroxide are mixed and temperature increases E) both A and C
E
a
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group. a. increases, decreases b. increases, increases c. stays the same, increases d. increases, stays the same e. decreases, increases
d
Element M reacts with fluorine to form an ionic compound with the formula MF3. The M-ion has 18 electrons. Element M is __________. a. P b. Ca c. Cr d. Sc e. Ar
c
Fluorine forms an ion with a charge of __________. a. 2+ b. 3- c. 1- d. 1+ e. 3+
e
For a given arrangement of ions, the lattice energy increases as ionic radius __________ and as ionic charge __________. a. This cannot be predicted. b. increases, increases c. increases, decreases d. decreases, decreases e. decreases, increases
C)
For which of the following can the composition vary? A) pure substance B) element C) both homogeneous and heterogeneous mixtures D) homogeneous mixture E) heterogeneous mixture
D)
Gases and liquids share the property of A) compressibility B) definite volume C) incompressibility D) indefinite shape E) definite shape
c
Given the data in the table below and DH°rxn for the reaction SO2Cl2 (g) + 2H2O (l) ® H2SO4 (l) + 2HCl (g) DH° = -62 kJ DH°f of HCl (g) is __________ kJ/mol. table: http://goo.gl/SsMwa a. -184 b. 60 c. -92 d. 30 e. Insufficient data are given.
c
Given the data in the table below, DH°rxn for the reaction Ca(OH)2 + 2H3AsO4 -> Ca(H2AsO4)2 + 2H2O table: http://goo.gl/wYa60 is __________ kJ. a. -4219 b. -76.4 c. -130.4 d. -744.9 e. -4519
e
Given the electronegativities below, which covalent single bond is most polar? Element: H C N O Electronegativity: 2.1 2.5 3.0 3.5 a. N-H b. O-N c. O-C d. C-H e. O-H
a
How many equivalent resonance structures can be drawn for the molecule of SO3 without having to violate the octet rule on the sulfur atom? a. 3 b. 5 c. 2 d. 4 e. 1
d
How many grams of CH3OH must be added to water to prepare 150 mL of a solution that is 2.0 M CH3OH? a. 4.3 b. 2.4 c. 9.6 ´ 103 d. 9.6 e. 4.3 ´ 102
a
How many grams of hydrogen are in 46 g of CH4O? a. 5.8 b. 2.8 c. 0.36 d. 184 e. 1.5
61.1
How many grams of sodium chloride are there in 550.0 mL of a 1.90 M aqueous solution of sodium chloride? 122 6.11 × 104 1.05 61.1 30.5
e
How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2? a. 2.00 b. 0.500 c. 0.160 d. 0.0400 e. 0.0800
1.31
How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4? 0.145 1.31 11.1 0.436 3.70
B
How many moles of carbon dioxide are in 52.06 g of carbon dioxide? A)0.8452 B)1.183 C)6.022x10^23 D)8.648x10^23 E)3.134x10^25
1.183
How many moles of carbon dioxide are there in 52.06 g of carbon dioxide? 8.648 ×1023 1.183 6.022 × 1023 3.134 × 1025 0.8452
5.79 ×1022
How many oxygen atoms are contained in 2.74 g of Al2(SO4)3? 12 8.01 ×10−3 7.22 ×1024 6.02 ×1023 5.79 ×1022
1.08 x 10^23
How many sulfur dioxide molecules are there in 0.180 mol of sulfur dioxide? 1.08 ×1024 1.80 ×1023 1.08 ×1023 6.02 ×1024 6.02 ×1023
B)
If matter is uniform throughout and cannot be separated into other substances by physical means, it is __________. A) a compound B) either an element or a compound C) a homogeneous mixture D) a heterogeneous mixture E) an element
63.4
In a titration of 35.00 mL of 0.737 M H2SO4, __________ mL of a 0.827 M KOH solution is required for neutralization. 35.0 25.8 62.4 1.12 39.3
e
In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii __________. a. increases, increase, increase b. decreases, increase, increase c. increases, decrease, increase d. increases, decrease, decrease e. increases, increase, decrease
e
In order to exhibit delocalized p bonding, a molecule must have __________. a. at least three s bonds b. trigonal planar electron domain geometry c. at least two p bonds d. at least four atoms e. at least two resonance structures
B)
In the following list, only __________ is not an example of a chemical reaction. A) dissolution of a penny in nitric acid B) the condensation of water vapor C) a burning candle D) the formation of polyethylene from ethylene E) the tarnishing of silver
e
In the resonance form of ozone shown below, the formal charge on the central oxygen atom is __________. http://goo.gl/8pXn6 a. +2 b. -1 c. -2 d. 0 e. +1
D
In the symbol shown below, x=_____. 13/x C A) 7 B)13 C)12 D)6 E) not enough information
e
In which of the molecules below is the carbon-carbon distance the shortest? a. H2CCCH2 b. H3C-CH2-CH3 c. H3C-CH3 d. H2CCH2 e. H-CºC-H
e
In which reaction does the oxidation number of hydrogen change? a. HCl (aq) + NaOH (aq) ® NaCl (aq) + H2O (l) b. SO2(g) + H2O (l) ® H2SO3 (aq) c. CaO (s) + H2O (l) ® Ca(OH)2 (s) d. 2 HClO4 (aq) + CaCO3 (s) ® Ca(ClO4)2 (aq) + H2O (l) + CO2 (g) e. 2 Na (s) + 2 H2O (l) ® 2 NaOH (aq) + H2 (g)
A) O, S, Se
In which set of elements would all members be expected to have very similar chemical properties? A) O, S, Se B) N, O, F C) Na, Mg, K D) S, Se, Si E) Ne, Na, Mg
K2SO4
In which species does sulfur have the highest oxidation number? S8 (elemental form of sulfur) K2SO4 H2S H2SO3 SO2
b
In which species does sulfur have the highest oxidation number? a. SO2 b. K2SO4 c. S8 (elemental form of sulfur) d. H2SO3 e. H2S
e
Iodine forms an ion with a charge of __________. a. 2+ b. 7- c. 1+ d. 2- e. 1-
C) protons, neutrons
Isotopes are atoms that have the same number of __________ but differing number of __________. A) protons, electrons B) neutrons, protons C) protons, neutrons D) electrons, protons E) neutrons, electrons
a
Lattice energy is __________. a. the energy required to convert a mole of ionic solid into its constituent ions in the gas phase b. the sum of electron affinities of the components in an ionic solid c. the sum of ionization energies of the components in an ionic solid d. the energy given off when gaseous ions combine to form one mole of an ionic solid e. the energy required to produce one mole of an ionic compound from its constituent elements in their standard states
C) metal, metal
Lithium is a __________ and magnesium is a __________. A) nonmetal, metal B) nonmetal, nonmetal C) metal, metal D) metal, metalloid E) metalloid, metalloid
a
Magnesium and sulfur form an ionic compound with the formula __________. a. MgS b. Mg2S c. Mg2S2 d. Mg2S3 e. MgS2
c
Methane and ethane are both made up of carbon and hydrogen. In methane, there are 12.0 g of carbon for every 4.00 g of hydrogen, a ratio of 3:1 by mass. In ethane, there are 24.0 g of carbon for every 6.00 g of hydrogen, a ratio of 4:1 by mass. This is an illustration of the law of __________. a. constant composition b. conservation of mass c. multiple proportions d. conservation of matter e. octaves
7
Mn in MnO−4
A) solid, liquid, or gas
Nonmetals can be __________ at room temperature. A) solid, liquid, or gas B) solid or liquid C) solid only D) liquid only E) liquid or gas
-1
O in K2O2
d
Of the choices below, which one is not an ionic compound? a. NaCl b. MoCl6 c. PbCl2 d. PCl5 e. RbCl
a
Of the following elements, __________ has the most negative electron affinity. a. Cl b. B c. Si d. P e. A
aluminum
Of the following elements, __________ is the most easily oxidized. oxygen fluorine nitrogen aluminum gold
e
Of the following elements, __________ is the most easily oxidized. oxygen fluorine nitrogen aluminum gold a. fluorine b. oxygen c. nitrogen d. gold e. aluminum
a
Of the following oxides, __________ is the most acidic. a. CO2 b. Na2O c. Al2O3 d. Li2O e. CaO
d
Of the following transitions in the Bohr hydrogen atom, the __________ transition results in the emission of the highest-energy photon. a. n = 1 ® n = 6 b. n = 6 ® n = 3 c. n = 3 ® n = 6 d. n = 6 ® n = 1 e. n = 1 ® n = 4
C)
Of the following, the smallest and lightest subatomic particle is the __________. A) neutron B) proton C) electron D) nucleus E) alpha particle
b
Of the molecules below, only __________ is polar. a. I2 b. AsH3 c. SF6 d. SbF5 e. CH4
c
Of the molecules below, only __________ is polar. a. I2 b. AsH3 c. SF6 d. SbF5 e. CH4
c
Of the reactions below, only __________ is not spontaneous. a. Zn (s) + 2HI (aq) ® ZnI2 (aq) + H2 (g) b. 2Ni (s) + H2SO4 (aq) ® Ni2SO4 (aq) + H2 (g) c. 2Ag (s) + 2HNO3 (aq) ® 2AgNO3 (aq) + H2 (g) d. 2Al (s) + 6HBr (aq) ® 2AlBr3 (aq) + 3H2 (g) e. Mg (s) + 2HCl (aq) ® MgCl2 (aq) + H2 (g)
d
Of the three types of radioactivity characterized by Rutherford, which is/are not particles? a. a-rays, b-rays, and g-rays b. a-rays c. b-rays d. g-rays e. a-rays and b-rays
loss of electrons, gain of electron
Oxidation is the __________ and reduction is the __________. loss of oxygen, gain of electrons loss of electrons, gain of electrons gain of oxygen, loss of electrons gain of electrons, loss of electrons gain of oxygen, loss of mass
d
Oxygen forms an ion with a charge of __________. a. 3+ b. 6+ c. 2+ d. 2- e. 3-
D) nonmetal, nonmetal
Oxygen is a __________ and nitrogen is a __________. A) metal, metalloid B) nonmetal, metal C) metalloid, metalloid D) nonmetal, nonmetal E) nonmetal, metalloid
a
Ozone is a (an) __________ of oxygen. a. allotrope b. free radical c. precursor d. peroxide e. isotope
A) metal, nonmetal
Potassium is a __________ and chlorine is a __________. A) metal, nonmetal B) metal, metal C) metal, metalloid D) metalloid, nonmetal E) nonmetal, metal
e
Predict the empirical formula of the ionic compound that forms from aluminum and oxygen. a. Al3O2 b. AlO c. Al2O d. AlO2 e. Al2O3
b
Predict the empirical formula of the ionic compound that forms from magnesium and fluorine. a. Mg2F3 b. MgF2 c. MgF d. Mg2F e. Mg3F2
a
Predict the empirical formula of the ionic compound that forms from magnesium and oxygen. a. MgO b. MgO2 c. Mg3O2 d. Mg2O2 e. Mg2O
c
Predict the empirical formula of the ionic compound that forms from sodium and fluorine. a. NaF2 b. Na3F2 c. NaF d. Na2F3 e. Na2F
B
Propane (C3H8) reacts with oxygen in the air to produce carbon dioxide and water. In a particular experiment, 38.0 grams of carbon dioxide are produced from the reaction of 22.05 grams of propane with excess oxygen. What is the % yield in this reaction? A)38.0 B)57.6 C)66.0 D)86.4 E)95.5
d
Question 125 Which solution has the same number of moles of NaOH as 50.00 mL of 0.100M solution of NaOH? a. 50.00 mL of 0.125M solution of NaOH b. 25.00 mL of 0.175M solution of NaOH c. 30.00 mL of 0.145M solution of NaOH d. 100.00 mL of 0.0500M solution of NaOH e. 20.00 mL of 0.200M solution of NaOH
4
S in SO2
c
Sodium forms an ion with a charge of __________. a. 0 b. 1- c. 1+ d. 2+ e. 2-
e
Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O2 (g) ® 2Al2O3 (s) In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of O2 produced 3.5 g of Al2O3. The % yield of the reaction is __________. a. 37 b. 66 c. 26 d. 47 e. 74
A
Solids have a ____ shape and are not appreciably ____. A) Definite, compressible B) definite, incompressible C) indefinite, compressible D) indefinite, incompressible E) sharp, convertible
Ca2+,OH−
Specify what ions are present in solution upon dissolving each of the following substances in water. Ca(OH)2
H+,NO3−
Specify what ions are present in solution upon dissolving each of the following substances in water. HNO3
Zn2+,Cl−
Specify what ions are present in solution upon dissolving each of the following substances in water. ZnCl2
a
Sulfur forms an ion with a charge of __________. a. 2- b. 6- c. 2+ d. 3+ e. 6+
b
The Cl-Si-Cl bond angle in the SiCl2F2 molecule is approximately __________. a. 120° b. 109.5° c. 180° d. 60° e. 90°
e
The DE of a system that releases 12.4 J of heat and does 4.2 J of work on the surroundings is __________ J. a. -8.2 b. 16.6 c. 12.4 d. 4.2 e. -16.6
e
The F-B-F bond angle in the BF2- ion is approximately __________. a. 90° b. 109.5° c. 60° d. 180° e. 120°
b
The Lewis structure of AsH3 shows __________ nonbonding electron pair(s) on As. a. This cannot be determined from the data given. b. 1 c. 3 d. 2 e. 0
c
The Lewis structure of HCN (H bonded to C) shows that __________ has __________ nonbonding electron pairs. a. N, 2 b. H, 1 c. N, 1 d. C, 1 e. C, 2
a
The Lewis structure of N2H2 shows __________. a. each nitrogen has one nonbonding electron pair b. each nitrogen has two nonbonding electron pairs c. a nitrogen-nitrogen triple bond d. a nitrogen-nitrogen single bond e. each hydrogen has one nonbonding electron pair
c
The Lewis structure of the CO32- ion is __________. http://goo.gl/TPj0l
e
The O-S-O bond angle in SO2 is slightly less than __________. a. 180° b. 109.5° c. 90° d. 60° e. 120°
a
The ability of an atom in a molecule to attract electrons is best quantified by the __________. a. electronegativity b. electron change-to-mass ratio c. first ionization potential d. paramagnetism e. diamagnetism
b
The acidity of carbonated water is due to the __________. a. presence of sulfur b. reaction of CO2 and H2O c. addition of acid d. nonmetal oxides e. none of the above
C) the number of protons or electrons in a neutral atom
The atomic number indicates __________. A) the number of neutrons in a nucleus B) the total number of neutrons and protons in a nucleus C) the number of protons or electrons in a neutral atom D) the number of atoms in 1 g of an element E) the number of different isotopes of an element
D
The average atomic weight of copper, which has two isotopes is 63.5. One of the isotopes has an atomic weight of 62.9 amu and constitutes 69.1 percent of copper isotopes. The other has an abundance of 30.9 percent. the atomic weight (amu) of the second isotope is ____. A) 63.2 B) 63.8 C) 64.1 D) 64.8 E)28.1
2NaN3(s)→2Na(s)+3N2(g)
The balanced equation for the decomposition of sodium azide is __________
2NaN3(s)→2Na(s)+3N2(g)
The balanced equation for the decomposition of sodium azide is __________. 2NaN3(s)→2Na(s)+2N2(g) 2NaN3(s)→2Na(s)+3N2(g) NaN3(s)→Na(s)+N2(g) NaN3(s)→Na(s)+N2(g)+N(g) 2NaN3(s)→Na2(s)+3N2(g)
e
The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is __________. a. 2H+ (aq) + 2KOH (aq) ® 2H2O (l) + 2K+ (aq) b. 2H+ (aq) + 2OH- (aq) ® 2H2O (l) c. H2SO4 (aq) + 2KOH (aq) ® 2H2O (l) + K2SO4 (s) d. H2SO4 (aq) + 2OH- (aq) ® 2H2O (l) + SO42- (aq) e. H2SO4 (aq) + 2KOH (aq) ® 2H2O (l) + K2SO4 (aq)
Ca2+ (aq) + CO3 2- (aq) → CaCO3 (s)
The balanced net ionic equation for precipitation of CaCO3 when aqueous solutions of Na2CO3 and CaCl2 are mixed is __________. Na+ (aq) + Cl- (aq) → NaCl (aq) 2Na+ (aq) + CO3 2- (aq) → Na2CO3 (aq) 2Na+ (aq) + 2Cl- (aq) → 2NaCl (aq) Na2CO3 (aq) + CaCl2 (aq) → 2NaCl (aq) + CaCO3 (s) Ca2+ (aq) + CO3 2- (aq) → CaCO3 (s)
c
What is the molecular formula for heptane? a. C6H12 b. C6H14 c. C7H16 d. C7H14 e. C7H18
2HNO3 (aq) + Sr(OH)2 (aq) → 2H2O (l) + Sr(NO3)2 (aq)
The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is __________. HNO3 (aq) + Sr(OH)2 (aq) → H2O (l) + Sr(NO3)2 (aq) HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + H2 (g) 2HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + 2H2 (g) 2HNO3 (aq) + Sr(OH)2 (aq) → 2H2O (l) + Sr(NO3)2 (aq) HNO3 (aq) + SrOH (aq) → H2O (l) + SrNO3 (aq)
b
The bond angles marked a, b, and c in the molecule below are about __________, __________, and __________, respectively. image: http://goo.gl/ein3i a. 109.5°, 90°, 120° b. 109.5°, 120°, 109.5° c. 120°, 120°, 109.5° d. 90°, 90°, 90° e. 120°, 120°, 90°
b
The charge on the __________ ion is -3. a. acetate b. nitride c. permanganate d. sulfate e. oxide
c
The charge on the manganese in the salt MnF3 is __________. a. 1+ b. 2+ c. 3+ d. 2- e. 1-
c
The concentration (M) of an aqueous methanol produced when 0.200 L of a 2.00 M solution was diluted to 0.800 L is __________. a. 0.400 b. 0.800 c. 0.500 d. 8.00 e. 0.200
e
The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is __________ M sodium ion and __________ M sulfate ion. a. 2.104, 1.052 b. 1.052, 1.052 c. 2.104, 2.104 d. 2.104, 4.208 e. 4.208, 2.104
b
The correct formula for molybdenum(IV) hypochlorite is __________. a. MoCl4 b. Mo(ClO)4 c. Mo(ClO3)4 d. Mo(ClO4)4 e. Mo(ClO2)4
a
The correct formula of iron(III) bromide is __________. a. FeBr3 b. Fe3Br c. FeBr2 d. FeBr e. Fe3Br3
e
The correct name for Al2O3 is __________. a. dialuminum trioxide b. aluminum trioxide c. dialuminum oxide d. aluminum hydroxide e. aluminum oxide
e
The correct name for CCl4 is __________. a. carbon tetrachlorate b. carbon chlorate c. carbon perchlorate d. carbon chloride e. carbon tetrachloride
d
The correct name for CaH2 is __________. a. calcium hydroxide b. calcium dihydride c. calcium dihydroxide d. calcium hydride e. hydrocalcium
c
The correct name for H2CO3 is __________. a. carbonous acid b. carbohydrate c. carbonic acid d. hydrocarbonate e. carbohydric acid
b
The correct name for H2SO3 is __________. a. sulfur hydroxide b. sulfurous acid c. hydrosulfuric acid d. hydrosulfic acid e. sulfuric acid
d
The correct name for HClO2 is __________. a. hypychloric acid b. perchloric acid c. hypochlorous acid d. chlorous acid e. chloric acid
b
The correct name for HClO3 is __________. a. perchloric acid b. chloric acid c. hydrochloric acid d. hydrochlorous acid e. chlorous acid
b
The correct name for HIO2 is __________. a. periodic acid b. iodous acid c. hypoiodic acid d. periodous acid e. hydriodic acid
d
The correct name for HNO2 is __________. a. nitric acid b. hydrogen nitrate c. hyponitrous acid d. nitrous acid e. pernitric acid
a
The correct name for K2S is __________. a. potassium sulfide b. potassium sulfate c. potassium bisulfide d. potassium disulfide e. dipotassium sulfate
d
The correct name for Mg(ClO3)2 is __________. a. manganese perchlorate b. magnesium chloroxide c. manganese chlorate d. magnesium chlorate e. magnesium perchlorate
c
The correct name for N2O5 is __________. a. nitrous oxide b. nitrogen oxide c. dinitrogen pentoxide d. nitrogen pentoxide e. nitric oxide
a
The correct name for Na2O2 is _________. a. sodium peroxide b. disodium oxide c. sodium oxide d. sodium dioxide e. disodium dioxide
a
The correct name for Ni(CN)2 is __________. a. nickel (II) cyanide b. nickel cyanate c. nickel carbonate d. nickel (I) cyanide e. nickel (I) nitride
d
The correct name for SO is __________. a. sulfate b. sulfite c. sulfoxide d. sulfur monoxide e. sulfur oxide
c
The correct name for SrO is __________. a. strontium peroxide b. strontium monoxide c. strontium oxide d. strontium hydroxide e. strontium dioxide
e
The correct name of the compound Na3N is __________. a. sodium trinitride b. trisodium nitride c. sodium(III) nitride d. sodium azide e. sodium nitride
b
The electron configuration of the phosphide ion (P3-) is __________. a. [Ne]3s23p1 b. [Ne]3s23p6 c. [Ne]3s23p3 d. [Ne]3p2 e. [Ne]3s2
b
The electron-domain geometry and molecular geometry of iodine trichloride are __________ and __________, respectively. a. octahedral, trigonal planar b. trigonal bipyramidal, T-shaped c. tetrahedral, trigonal pyramidal d. T-shaped, trigonal planar e. trigonal bipyramidal, trigonal planar
d
What is the molecular formula for n-hexanol? a. C7H13OH b. C7H14OH c. C6H14OH d. C6H13OH e. C6H12OH
a
The electron-domain geometry of a sulfur-centered compound is trigonal bipyramidal. The hybridization of the central nitrogen atom is __________. a. sp3d b. sp2 c. sp d. sp3 e. sp3d2
(.7825)(224.998 amu) + (.2025)(226.895 amu) + (229.999)(.01500) = 225.45 amu
The element X has three naturally occurring isotopes. The isotopic masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is __________ amu. Isotope Mass Relative Abundance X - 225 224.998 amu 78.25% X - 227 226.895 amu 20.25% X - 230 229.999 amu 1.500%
b
The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is __________ amu. image: http://goo.gl/R2ISu a. 221.0 b. 220.4 c. 218.5 d. 219.7 e. 220.42
d
The energy of a photon that has a wavelength of 13.2 nm is __________ J. a. 1.99 ´ 10-25 b. 4.42 ´ 10-23 c. 1.62 ´ 10-17 d. 1.51 ´ 10-17 e. 9.55 ´ 10-25
e
The enthalpy change for the following reaction is -483.6 kJ: 2H2 (g) + O2 (g) ® 2H2O (g) Therefore, the enthalpy change for the following reaction is __________ kJ: 4H2 (g) + 2O2 (g) ® 4H2O (g) a. 483.6 b. 2.34 ´ 105 c. 967.2 d. -483.6 e. -967.2
c
The formal charge on carbon in the molecule below is __________. image: http://goo.gl/w1fwu a. +2 b. +3 c. 0 d. +1 e. -1
d
The formal charge on nitrogen in NO3- is __________. image: http://goo.gl/IMZzJ a. +2 b. 0 c. -2 d. +1 e. -1
c
The formula for aluminum hydroxide is __________. a. Al2O3 b. Al2(OH)3 c. Al(OH)3 d. AlOH e. Al3OH
e
The formula for the compound formed between aluminum ions and phosphate ions is __________. a. Al(PO4)3 b. Al3(PO4)3 c. Al2(PO4)3 d. AlP e. AlPO4
b
The formula for zinc phosphate isZn3(PO4)2. What is the formula for cadmium arsenate? a. Cd2(AsO4)4 b. Cd3(AsO4)2 c. Cd3(AsO3)4 d. Cd2(AsO4)3 e. Cd4(AsO2)3
b
The formula of ammonium carbonate is __________. a. (NH3)2CO3 b. (NH4)2CO3 c. NH4CO2 d. (NH3)2CO4 e. N2(CO3)3
c
The formula of bromic acid is __________. a. HBrO2 b. HBrO4 c. HBrO3 d. HBr e. HBrO
123.11
The formula of nitrobenzene is C6H5NO2. The molecular weight of this compound is __________ amu.
123.11
The formula of nitrobenzene is C6H5NO2. The molecular weight of this compound is __________ amu. 109.10 3.06 107.11 43.03 123.11
b
The formula of the carbonate ion is __________. a. CO2- b. CO32- c. CO- d. CO22- e. CO33-
b
The formula of the chromate ion is __________. a. CrO23- b. CrO42- c. CrO2- d. CrO32- e. CrO-
D
The formula weight of a substance is_____. A)identical to the molar mass B)the same as the percent by mass weight C)determined by combustion analysis D)the sum of the atomic weights of each atom in its chemical formula E)the weight of a sample of the substance
132
The formula weight of ammonium sulfate ((NH4)2SO4), rounded to the nearest integer, is __________ amu.
B) led to the discovery of the atomic nucleus
The gold foil experiment performed in Rutherford's lab __________. A) confirmed the plum-pudding model of the atom B) led to the discovery of the atomic nucleus C) was the basis for Thompson's model of the atom D) utilized the deflection of beta particles by gold foil E) proved the law of multiple proportions
d
The hybridization of the central atom in the XeF4 molecule is __________. a. sp b. sp3 c. sp2 d. sp3d2 e. sp3d
b
The ion NO- has __________ valence electrons. a. 16 b. 12 c. 15 d. 10 e. 14
c
The ion with the smallest diameter is __________. a. O2- b. Br- c. F- d. I- e. Cl-
b
The ions Ca2+ and PO43- form a salt with the formula __________. a. Ca(PO4)2 b. Ca3(PO4)2 c. Ca2PO4 d. Ca2(PO4)3 e. CaPO4
Co²⁺ [Ar] 3d⁷
The largest principal quantum number in the ground state electron configuration of cobalt is __________.
B
The mass % of Al in aluminum sulfate (Al2(SO4)3)? A) 7.886 B)15.77 C)21.93 D)45.70 E)35.94
d
The molar heat capacity of a compound with the formula C2H6SO is 88.0 J/mol-K. The specific heat of this substance is __________ J/g-K. a. 6.88 ´ 103 b. 4.89 c. -88.0 d. 1.13 e. 88.0
d
The molecular geometry of __________ is square planar. a. PH3 b. XeF2 c. CCl4 d. XeF4 e. ICl3
a
What is the molecular formula for n-propanol? a. C3H7OH b. C4H9OH c. CH3OH d. C2H5OH e. C5H11OH
d
The molecular geometry of the CHCl3 molecule is __________. a. trigonal pyramidal b. trigonal planar c. T-shaped d. tetrahedral e. bent
a
The molecular geometry of the CS2 molecule is __________. a. linear b. bent c. T-shaped d. trigonal planar e. tetrahedral
e
The molecular geometry of the PF4+ ion is __________. a. trigonal bipyramidal b. trigonal pyramidal c. trigonal planar d. octahedral e. tetrahedral
c
The molecular geometry of the SF2 molecule is __________. a. linear b. trigonal planar c. bent d. octahedral e. tetrahedral
b
The molecular geometry of the SiH2Cl2 molecule is __________. a. T-shaped b. tetrahedral c. trigonal pyramidal d. trigonal planar e. octahedral
e
The name of PCl3 is __________. a. monophosphorous trichloride b. potassium chloride c. trichloro potassium d. phosphorous(III) chloride e. phosphorus trichloride
d
The name of the binary compound N2O4 is __________. a. oxygen nitride b. nitrous oxide c. nitrogen(IV) oxide d. dinitrogen tetroxide e. nitrogen oxide
c
The name of the ionic compound (NH4)3PO4 is __________. a. ammonia phosphide b. nitrogen hydrogen phosphate c. ammonium phosphate d. triammonium phosphate e. tetrammonium phosphate
b
The name of the ionic compound KBrO4 is __________. a. potassium bromate b. potassium perbromate c. potassium perbromite d. potassium hypobromate e. potassium bromide
c
The name of the ionic compound NH4CN is __________. a. ammonium hydrogen cyanate b. cyanonitride c. ammonium cyanide d. nitrogen hydrogen cyanate e. ammonium carbonitride
a
The name of the ionic compound V2O3 is __________. a. vanadium(III) oxide b. vanadium oxide c. vanadium(III) trioxide d. vanadium(II) oxide e. divanadium trioxide
H+ (aq) + OH- (aq) → H2O (l)
The net ionic equation for the reaction between aqueous nitric acid and aqueous sodium hydroxide is __________. H+ (aq) + OH- (aq) → H2O (l) HNO3 (aq) + NaOH (aq) → NaNO3 (aq) + H2O (l) H+ (aq) + Na+ (aq) +OH- (aq) → H2O (l) + Na+ (aq) HNO3 (aq) + OH- (aq) → NO3 - (aq) + H2O (l) H+ (aq) + HNO3 (aq) + 2OH- (aq) → 2H2O (l) + NO3 - (aq)
E) electrons
The nucleus of an atom does not contain __________. A) protons B) protons or neutrons C) neutrons D) subatomic particles E) electrons
b
The number 1.00430 has __________ significant figures. a. 4 b. 6 c. 2 d. 5 e. 3
c
The number 1.00430 has __________ significant figures. a. 4 b. 6 c. 2 d. 5 e. 3
e
The oxidation number of phosphorus in PF3 is __________. a. +2 b. -2 c. +1 d. -3 e. +3
d
What is the molecular formula for nonane? a. C10H22 b. C10H24 c. C9H18 d. C9H20 e. C10H20
c
What is the molecular formula for propane? a. C3H6 b. C2H8 c. C3H8 d. C4H8 e. C4H10
a molecular compound and a strong electrolyte
The reaction between strontium hydroxide and chloric acid produces __________. a molecular compound and a strong electrolyte two molecular compounds two strong electrolytes a molecular compound and a weak electrolyte two weak electrolytes
d
The species __________ contains 16 neutrons. a. 36Cl b. 80Br- c. 16O d. 31P e. 34S2-
c
The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J) is required to raise the temperature of 10.0 mL of bromine from 25.00°C to 27.30°C? The density of liquid bromine: 3.12 g/mL. a. 32.4 b. 300 c. 16.2 d. 10.4 e. 5.20
1.00 x 10^24
The total number of atoms in 0.111 mol of Fe(CO)3(PH3)2 is __________. 1.00 ×1024 2.76 ×10−24 1.67 4.46 ×1021 15.0
b
The value of DH° for the reaction below is -1107 kJ: 2Ba (s) + O2 (g) ® 2BaO (s) How many kJ of heat are released when 15.75 g of Ba (s) reacts completely with oxygen to form BaO (s)? a. 35.1 b. 63.5 c. 20.8 d. 114 e. 70.3
b
The value of DH° for the reaction below is -6535 kJ. __________ kJ of heat are released in the combustion of 16.0 g of C6H6 (l)? 2C6H6 (l) + 15O2 (g) ® 12CO2 (g) + 6H2O (l) a. 1.34 ´ 103 b. 669 c. 5.23 ´ 104 d. -6535 e. 2.68 ´ 103
100
There are __________ hydrogen atoms in 25 molecules of C4H4S2. 3.8 ×1024 1.5 ×1025 100 25 6.0 ×1025
c
There are __________ s and __________ p bonds in the H-CºC-H molecule. a. 3 and 4 b. 4 and 3 c. 3 and 2 d. 2 and 3 e. 5 and 0
c
There are __________ s bonds and __________ p bonds in H3C-CH2-CH=CH-CH2-CºCH. a. 12, 2 b. 14, 2 c. 16, 3 d. 10, 3 e. 13, 2
c
There are __________ sulfur atoms in 25 molecules of C4H4S2. a. 1.5 ´ 1025 b. 3.0 ´ 1025 c. 50 d. 6.02 ´ 1023 e. 4.8 ´ 1025
a
There are __________ unpaired electrons in a ground state phosphorus atom. a. 3 b. 4 c. 2 d. 0 e. 1
e
There is/are __________ p bond(s) in the molecule below. image: http://goo.gl/exggt a. 4 b. 16 c. 0 d. 1 e. 2
a
There is/are __________ s bond(s) in the molecule below. image:http://goo.gl/3d9w3 a. 12 b. 18 c. 13 d. 1 e. 2
c
This element reacts with hydrogen to produce a gas with the formula HX. When dissolved in water, HX forms an acidic solution. X is __________, a. Na b. C c. Br d. O e. H
0.752 and 0.376
What are the respective concentrations (M) of Na+ and SO42− afforded by dissolving 0.500 mol Na2SO4 in water and diluting to 1.33 L? 0.376 and 0.752 0.665 and 0.665 0.665 and 1.33 0.752 and 0.376 1.33 and 0.665
SiO2
What is the chemical formula for quartz?
d
What is the concentration (M) of KCl in a solution made by mixing 25.0 mL of 0.100 M KCl with 50.0 mL of 0.100 M KCl? a. 0.0333 b. 0.0500 c. 0.0250 d. 0.100 e. 125
b
What is the correct formula for ammonium sulfide? a. NH3S b. (NH4)2S c. NH4SO3 d. N2S3 e. (NH4)2SO4
e
What is the empirical formula of a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by mass? a. SOCl b. SO2Cl c. ClSO4 d. S2OCl e. SOCl2
e
What is the formula for perchloric acid? a. HClO2 b. HCl c. HClO3 d. HClO e. HClO4
148.3 amu
What is the formula weight of Mg(NO3)2?
C6H12O6
What is the molecular formula of a compound with a molar mass of 180.16 grams/mole and the empirical formula CH2O? C2H6O2 C1.5H3O1.5 C6H12O6 C2H4O
1.23
What mass (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO3 is treated with an excess of aqueous hydrobromic acid? 1.23 34.5 188 1.44 53.6
c
What mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s) + 2H2O (l) ® Mg(OH)2 (s) + H2 (g) a. 0.204 b. 0.219 c. 0.102 d. 0.0162 e. 0.0485
e
What volume (mL) of 7.48 ´ 10-2 M perchloric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide? a. 750 b. 8.60 c. 188 d. 125 e. 375
375
What volume (mL) of 7.48 × 10-2 M perchloric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide? 8.60 125 375 750 188
29.3
What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200.0 mL to make a 0.880 M solution of sodium hydroxide? 29.3 2.64 176 26.4 50.0
129
What volume (ml) of a 3.45 M lead nitrate solution must be diluted to 450.0 ml to make a 0.990 M solution of lead nitrate? 56 45 129 109 101
b
When aqueous solutions of AgNO3 and KI are mixed, AgI precipitates. The balanced net ionic equation is __________. a. AgNO3 (aq) + KI (aq) ® AgI (s) + KNO3 (aq) b. Ag+ (aq) + I- (aq) ® AgI (s) c. AgNO3 (aq) + KI (aq) ® AgI (aq) + KNO3 (s) d. Ag+ (aq) + NO3- (aq) ® AgNO3 (aq) e. Ag+ (aq) + NO3- (aq) ® AgNO3 (s)
NiBr2 and AgNO3
When aqueous solutions of __________ are mixed, a precipitate forms. NaI and KBr K2SO4 and CrCl3 KOH and Ba(NO3)2 Li2CO3 and CsI NiBr2 and AgNO3
d
When calcium reacts with sulfur the compound formed is __________. a. Ca2S3 b. Ca3S2 c. Ca2S2 d. CaS e. CaS2
c
When the following equation is balanced, the coefficient of C3H8O3 is __________. C3H8O3 (g) + O2 (g) ® CO2 (g) + H2O (g) a. 5 b. 7 c. 2 d. 1 e. 3
2
When the following equation is balanced, the coefficient of H2O is __________. Ca(s)+H2O(l)→Ca(OH)2(aq)+H2(g)
d
When the following equation is balanced, the coefficient of H2S is __________. FeCl3 (aq) + H2S (g) ® Fe2S3 (s) + HCl (aq) a. 4 b. 2 c. 5 d. 3 e. 1
3
When the following equation is balanced, the coefficient of H2S is __________. FeCl3(aq)+H2S(g)→Fe2S3(s)+HCl(aq)
d
When the following equation is balanced, the coefficient of H3PO4 is __________. H3PO4 (aq) + NaOH (aq) ® Na3PO4 (aq) + H2O (l) a. 4 b. 3 c. 0 d. 1 e. 2
a
When the following equation is balanced, the coefficient of HNO3 is __________. HNO3 (aq) + CaCO3 (s) ® Ca(NO3)2 (aq) + CO2 (g) + H2O (l) a. 2 b. 1 c. 5 d. 3 e. 4
b
When the following equation is balanced, the coefficient of dinitrogen pentoxide is __________. N2O5 (g) + H2O (l) ® HNO3 (aq) a. 5 b. 1 c. 3 d. 2 e. 4
D)
Which atom has the largest number of neutrons? A) phosphorous-30 B) chlorine-37 C) potassium-39 D) argon-40 E) calcium-40
a
Which atom has the smallest number of neutrons? a. nitrogen-14 b. fluorine-19 c. oxygen-16 d. neon-20 e. carbon-14
MgSO3
Which compound has the atom with the highest oxidation number? MgSO3 NH4Cl Al(NO2)3 Na3N CaS
Li2Co3
Which compound has the highest percentage composition of oxygen? Li2CO3 KNO3 La2O3 Al(OH)3
B
Which compounds do not have the same empirical formula? A) C2H2,C6H6 B) CO2,CO C)C2H4, C3H6 D)C2H4O2,C6H12O6 E)C2H5COOCH3,CH3CHO
a
Which compounds do not have the same empirical formula? a. CO, CO2 b. C2H4, C3H6 c. C2H5COOCH3, CH3CHO d. C2H4O2, C6H12O6 e. C2H2, C6H6
a
Which element forms an ion with the same charge as the ammonium ion? a. potassium b. calcium c. chlorine d. oxygen e. nitrogen
C
Which element is oxidized in this reaction? Fe2O3+3CO→2Fe+3CO2
a
Which equation correctly represents the first ionization of calcium? a. Ca (g) ® Ca+ (g) + e- b. Ca+ (g) + e- ® Ca (g) c. Ca- (g) ® Ca (g) + e- d. Ca (g) ® Ca- (g) + e- e. Ca (g) + e- ® Ca- (g)
b
Which formula/name pair is incorrect? a. Fe2(SO3)3 iron(III) sulfite b. Fe2(SO4)3 iron(III) sulfide c. FeSO4 iron(II) sulfate d. FeSO3 iron(II) sulfite e. FeS iron(II) sulfide
c
Which formula/name pair is incorrect? a. Mg(MnO4)2 magnesium permanganate b. Mn(NO3)2 manganese(II) nitrate c. Mg3N2 magnesium nitrite d. Mn(NO2)2 manganese(II) nitrite e. Mg(NO3)2 magnesium nitrate
Sr(OH)2, KOH, NaOH, Ba(OH)2
Which hydroxides are strong bases? Sr(OH)2 KOH NaOH Ba(OH)2 KOH, Ba(OH)2 KOH, NaOH KOH, NaOH, Ba(OH)2 Sr(OH)2, KOH, NaOH, Ba(OH)2 None of these is a strong base.
d
Which hydroxides are strong bases? Sr(OH)2 KOH NaOH Ba(OH)2 a. KOH, Ba(OH)2 b. KOH, NaOH c. KOH, NaOH, Ba(OH)2 d. Sr(OH)2, KOH, NaOH, Ba(OH)2 e. None of these is a strong base.
b
Which ion below has the largest radius? a. K+ b. Br- c. Cl- d. F- e. Na+
b
Which metal does not form cations of differing charges? a. Cu b. Na c. Fe d. Sn e. Co
b
Which of the following are chemical processes? 1. rusting of a nail 2. freezing of water 3. decomposition of water into hydrogen and oxygen gases 4. compression of oxygen gas a. 1, 2 b. 1, 3 c. 1, 3, 4 d. 1, 4 e. 2, 3, 4
a
Which of the following are strong acids? HI HNO3 HF HBr a. HI , HNO3 , HBr b. HI , HNO3 , HF , HBr c. HI , HF , HBr d. HF , HBr e. HNO3 , HF , HBr
e
Which of the following are strong electrolytes? HCl HC2H3O2 NH3 KCl a. HCl, NH3, KCl b. HC2H3O2, KCl c. HCl, HC2H3O2, KCl d. HCl, HC2H3O2, NH3, KCl e. HCl, KCl
c
Which of the following are weak electrolytes? HCl HC2H3O2 NH3 KCl a. HCl , KCl b. HCl , HC2H3O2 , NH3 , KCl c. HC2H3O2 , NH3 d. HCl , HC2H3O2 , KCl e. HC2H3O2 , KCl
e
Which of the following has the largest second ionization energy? a. Mg b. Al c. P d. Si e. Na
d
Which of the following is an illustration of the law of constant composition? a. Water can be separated into other substances by a chemical process. b. Water and salt have different boiling points. c. Water is a compound. d. Water is 11% hydrogen and 89% oxygen by mass. e. Water boils at 100°C at 1 atm pressure.
b
Which of the following names is/are correct for the compound SnCl4? a. tin chloride and tin (II) tetrachloride b. tin tetrachloride and tin (IV) chloride c. tin (IV) tetrachloride d. tin chloride e. tin (II) chloride and tin (IV) chloride
a
Which of the following names is/are correct for the compound TiO2? a. titanium dioxide and titanium (IV) oxide b. titanium (II) oxide c. titanium (IV) dioxide d. titanium oxide e. titanium oxide and titanium (IV) dioxide
e
Which of these metals is the least easily oxidized? Na Au Fe Ca Ag a. Na b. Fe c. Ag d. Ca e. Au
c
Which one of the following compounds is copper(I) chloride? a. CuCl2 b. Cu3Cl2 c. CuCl d. Cu2Cl e. Cu2Cl3
b
Which one of the following compounds produces a basic solution when dissolved in water? a. OF2 b. Na2O c. SO2 d. O2 e. CO2
d
Which one of the following has the element name and symbol correctly matched? a. P, potassium b. Mg, manganese c. Sn, silicon d. Ag, silver e. C, copper
D)
Which one of the following is a pure substance? A) concrete B) wood C) salt water D) elemental copper E) milk
D)
Which one of the following is not an intensive property? A) density B) temperature C) melting point D) mass E) boiling point
A)
Which one of the following is often easily separated into its components by simple techniques such as filtering or decanting? A) heterogeneous mixture B) compounds C) homogeneous mixture D) elements E) solutions
a
Which one of the following is the formula of hydrochloric acid? a. HClO2 b. HClO3 c. HClO d. HClO4 e. HCl
e
Which one of the following is the formula of hydrochloric acid? a. HClO2 b. HClO3 c. HClO d. HClO4 e. HCl
a
Which one of the following polyatomic ions has the same charge as the hydroxide ion? a. nitrate b. carbonate c. sulfate d. ammonium e. phosphate
A
Which pair of elements is most apt to form an ionic compound with eachother? A)barium, bromine B) calcium, sodium C) oxygen, fluorine D) sulfur, fluorine E)nitrogen, hydrogen
d
Which pair of substances could be used to illustrate the law of multiple proportions? a. NaCl, KCl b. CH4, C6H12O6 c. H2O, O2 d. CO, CO2 e. SO2, H2SO4
129 mL of 0.145M solution of KCl
Which solution has the same number of moles of KCl as 75.00 mL of 0.250M solution of KCl? 129 mL of 0.145M solution of KCl 25.0 mL of 0.175M solution of KCl 20.0 mL of 0.200M solution of KCl 50.0 mL of 0.125M solution of KCl 100 mL of 0.0500M solution of KCl
b
Which species below is the nitride ion? a. NH4+ b. N 3- c. NO3- d. Na+ e. NO2-
A) 118 Sn²⁺ 50
Which species has 48 electrons? A) 118 Sn²⁺ 50 B) 116 Sn⁺⁴ 50 C) 112 Cd⁺² 48 D) 68 Ga 31 E) 48 Ti 22
B) 128 Te²⁻ 52
Which species has 54 electrons? A) 132 Xe⁺ 54 B) 128 Te²⁻ 52 C) 118 Sn²⁺ 50 D) 112 Cd 48 E) 132 Xe²⁺ 54
A
Which states of matter are significantly compressible? A) gases only B) liquids only C) solids only D) liquids and gases E) solids and liquids
none of the above
With which of the following will the ammonium ion form an insoluble salt? carbonate sulfate sulfate and carbonate chloride none of the above
d
[Ar]4s2,3d10,4p3 is the electron configuration of a(n) __________ atom. a. P b. Sn c. Sb d. As e. V
products
______ appear on the right side of the equation
b
__________-rays consist of fast-moving electrons. a. Alpha b. Beta c. Gamma d. X e. none of the above
reactants
____appear on the left side of the equation
D
accuracy refers to_____. A) how close a measured number is to zero B)how close a measured number is to the calculated value C)how close a measured number is to other measured numbers D) how close a measured number is to true value E) how close a measured number is to infinity
participation reactions
cations and anions come together to form an insoluble ionic compound
e
dH for the reaction IF5 (g) ® IF3 (g) + F2 (g) is __________ kJ, give the data below. IF (g) + F2 (g) -> IF3 (g) DH = -390 kJ IF (g) + 2 F2 (g) -> IF5 (g) DH = -745 kJ a. +35 b. -1135 c. -35 d. +1135 e. +355
oxidTION reaction
electrons are transferred from one recant to another
reduction
gain of electrons
neutralization reaction
h+ ions and OH- ions come together to from h20 molecules
k2So3
hat is the empirical formula of a compound that contains 49.4% K, 20.3% S, and 30.3% O by mass? K2SO3 KSO4 KSO3 KSO2 K2SO4
132
he formula weight of ammonium sulfate ((NH4)2SO4), rounded to the nearest integer, is __________ amu. 132 116 118 100 264
acids
ionize in aqueous solutions to form H + ions, combination of H+and an anion
oxidation
loss of electrons
nonelectrolyte
may dissolve in water but it doesn't associate into ions when it does so
molarity
measure concentration in a solution
62.4
n a titration of 35.00 mL of 0.737 M H2SO4, __________ mL of a 0.827 M KOH solution is required for neutralization. 35.0 25.8 62.4 1.12 39.3
decomposition reaction
one substance breaks down into two or more substances
combustion reaction
rapid reactions that produce a flame. involve oxygen as a reactant
bases
react with H+ ions. combination of a cation and OH-
neutralization reactions
reactions between an acid and a base
precipitate
salt falling from a solution like snow from the key
electrolyte
substance that dissociates into ions when dissolved in water
molecular weight
sum of the atomic weight of the atoms in a molecule
molar mass
the mass of 1 mol of a substance
theoretical yeild
the maximum amount of product that can be made
limiting reactant
the reactant present in the smallest stoichmetric amount
formula weight
the sum of the atomic weights of atoms in a chemical formula
combination reaction
two or more substances react to form one product
B
which of the following is the highest temperature? A) the boiling point of water B) 220 degrees F C) 373 K D) 100 degrees C E) all of the above are identical
A
which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? A) O,S B) C,N C) K, Ca D) H,He E) Si,P
