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Name: ______________________ Class: _________________ Date: _________ ID: A
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Chapter 2 all questions
____ 1) A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of __________.A) the law of multiple proportionsB) the law of constant compositionC) the law of conservation of massD) the law of conservation of energyE) none of the above
____ 2) Which one of the following is not one of the postulates of Dalton's atomic theory?A) Atoms are composed of protons, neutrons, and electrons.B) All atoms of a given element are identical; the atoms of different elements are
different and have different properties.C) Atoms of an element are not changed into different types of atoms by chemical
reactions: atoms are neither created nor destroyed in chemical reactions.D) Compounds are formed when atoms of more than one element combine; a given
compound always has the same relative number and kind of atoms.E) Each element is composed of extremely small particles called atoms.
____ 3) Consider the following selected postulates of Dalton's atomic theory:(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.Which of the postulates is(are) no longer considered valid?A) (i) and (ii)B) (ii) onlyC) (ii) and (iii)D) (iii) onlyE) (iii) and (iv)
____ 4) Which pair of substances could be used to illustrate the law of multiple proportions?A) SO2, H2SO4
B) CO, CO2
C) H2O, O2
D) CH4, C6H12O6
E) NaCl, KCl
Name: ______________________ ID: A
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____ 5) Which statement below correctly describes the responses of alpha, beta, and gamma radiation to an electric field?A) Both beta and gamma are deflected in the same direction, while alpha shows no
response.B) Both alpha and gamma are deflected in the same direction, while beta shows no
response.C) Both alpha and beta are deflected in the same direction, while gamma shows no
response.D) Alpha and beta are deflected in opposite directions, while gamma shows no
response.E) Only alpha is deflected, while beta and gamma show no response.
____ 6) Which one of the following is not true concerning cathode rays?A) They originate from the negative electrode.B) They travel in straight lines in the absence of electric or magnetic fields.C) They impart a negative charge to metals exposed to them.D) They are made up of electrons.E) The characteristics of cathode rays depend on the material from which they are
emitted.
____ 7) The charge on an electron was determined in the __________.A) cathode ray tube, by J. J. ThompsonB) Rutherford gold foil experimentC) Millikan oil drop experimentD) Dalton atomic theoryE) atomic theory of matter
____ 8) __________-rays consist of fast-moving electrons.A) AlphaB) BetaC) GammaD) XE) none of the above
____ 9) The gold foil experiment performed in Rutherford's lab __________.A) confirmed the plum-pudding model of the atomB) led to the discovery of the atomic nucleusC) was the basis for Thomson's model of the atomD) utilized the deflection of beta particles by gold foilE) proved the law of multiple proportions
Name: ______________________ ID: A
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____ 10) In the Rutherford nuclear-atom model, __________.A) the heavy subatomic particles, protons and neutrons, reside in the nucleusB) the three principal subatomic particles (protons, neutrons, and electrons) all have
essentially the same massC) the light subatomic particles, protons and neutrons, reside in the nucleusD) mass is spread essentially uniformly throughout the atomE) the three principal subatomic particles (protons, neutrons, and electrons) all have
essentially the same mass and mass is spread essentially uniformly throughout the atom
____ 11) Cathode rays are __________.A) neutronsB) x-raysC) electronsD) protonsE) atoms
____ 12) Cathode rays are deflected away from a negatively charged plate because __________.A) they are not particlesB) they are positively charged particlesC) they are neutral particlesD) they are negatively charged particlesE) they are emitted by all matter
____ 13) In the absence of magnetic or electric fields, cathode rays __________.A) do not existB) travel in straight linesC) cannot be detectedD) become positively chargedE) bend toward a light source
____ 14) Of the three types of radioactivity characterized by Rutherford, which is/are electrically charged?A) -raysB) -rays and -raysC) -rays, -rays, and -raysD) -raysE) -rays and -rays
Name: ______________________ ID: A
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____ 15) Of the three types of radioactivity characterized by Rutherford, which is/are not electrically charged?A) -raysB) -rays, -rays, and -raysC) -raysD) -rays and -raysE) -rays and -rays
____ 16) Of the three types of radioactivity characterized by Rutherford, which are particles?A) -raysB) -rays, -rays, and -raysC) -raysD) -rays and -raysE) -rays and -rays
____ 17) Of the three types of radioactivity characterized by Rutherford, which is/are not particles?A) -raysB) -rays and -raysC) -raysD) -raysE) -rays, -rays, and -rays
____ 18) Of the following, the smallest and lightest subatomic particle is the __________.A) neutronB) protonC) electronD) nucleusE) alpha particle
____ 19) All atoms of a given element have the same __________.A) massB) number of protonsC) number of neutronsD) number of electrons and neutronsE) density
____ 20) Which atom has the smallest number of neutrons?A) carbon-14B) nitrogen-14C) oxygen-16D) fluorine-19E) neon-20
Name: ______________________ ID: A
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____ 21) Which atom has the largest number of neutrons?A) phosphorus-30B) chlorine-37C) potassium-39D) argon-40E) calcium-40
____ 22) There are __________ electrons, __________ protons, and __________ neutrons in an atom of
54132 Xe.
A) 132, 132, 54B) 54, 54, 132C) 78, 78, 54D) 54, 54, 78E) 78, 78, 132
____ 23) An atom of the most common isotope of gold, 197Au, has __________ protons, __________ neutrons, and __________ electrons.A) 197, 79, 118B) 118, 79, 39C) 79, 197, 197D) 79, 118, 118E) 79, 118, 79
____ 24) Which combination of protons, neutrons, and electrons is correct for the isotope of copper, 2963 Cu?
A) 29 p+, 34 n°, 29 e-
B) 29 p+, 29 n°, 63 e-
C) 63 p+, 29 n°, 63 e-
D) 34 p+, 29 n°, 34 e-
E) 34 p+, 34 n°, 29 e-
____ 25) Which isotope has 45 neutrons?
A) 3680 Kr
B) 3580 Br
C) 3478 Se
D) 1734 Cl
E) 45103 Rh
Name: ______________________ ID: A
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____ 26) Which pair of atoms constitutes a pair of isotopes of the same element?
A) 614 X 7
14 X
B) 614 X 6
12 X
C) 917 X 8
17 X
D) 1019 X 9
19 X
E) 1020 X 11
21 X
____ 27) Which isotope has 36 electrons in an atom?A) Kr
B) Br
C) Se
D) Cl
E) Hg
____ 28) Isotopes are atoms that have the same number of __________ but differing number of __________.A) protons, electronsB) neutrons, protonsC) protons, neutronsD) electrons, protonsE) neutrons, electrons
____ 29) The nucleus of an atom does not contain __________.A) protonsB) protons or neutronsC) neutronsD) subatomic particlesE) electrons
____ 30) The nucleus of an atom contains __________.A) electronsB) protonsC) neutronsD) protons and neutronsE) protons, neutrons, and electrons
Name: ______________________ ID: A
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____ 31) Different isotopes of a particular element contain the same number of __________.A) protonsB) neutronsC) protons and neutronsD) protons, neutrons, and electronsE) subatomic particles
____ 32) Different isotopes of a particular element contain different numbers of __________.A) protonsB) neutronsC) protons and neutronsD) protons, neutrons, and electronsE) None of the above is correct.
____ 33) In the symbol shown below, x = __________.
x13 C
A) 7B) 13C) 12D) 6E) not enough information to determine
____ 34) In the symbol below, X = __________.
613 X
A) NB) CC) AlD) KE) not enough information to determine
____ 35) In the symbol below, x = __________.
6xC
A) 19B) 13C) 6D) 7E) not enough information to determine
Name: ______________________ ID: A
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____ 36) In the symbol below, x is __________.
6xC
A) the number of neutronsB) the atomic numberC) the mass numberD) the isotope numberE) the elemental symbol
____ 37) Which one of the following basic forces is so small that it has no chemical significance?A) weak nuclear forceB) strong nuclear forceC) electromagnetismD) gravityE) Coulomb's law
____ 38) Gravitational forces act between objects in proportion to their __________.A) volumesB) massesC) chargesD) polarizabilityE) densities
____ 39) Silver has two naturally occurring isotopes with the following isotopic masses:
47107 Ar 47
107 Ar
106.90509 108.9047The average atomic mass of silver is 107.8682 amu. The fractional abundance of the lighter of the two isotopes is __________.A) 0.24221B) 0.48168C) 0.51835D) 0.75783E) 0.90474
____ 40) The atomic mass unit is presently based on assigning an exact integral mass (in amu) to an isotope of __________.A) hydrogenB) oxygenC) sodiumD) carbonE) helium
Name: ______________________ ID: A
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____ 41) 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.
Isotope Abundance Mass221X 74.22 220.9220X 12.78 220.0218X 13.00 218.1
A) 219.7B) 220.4C) 220.42D) 218.5E) 221.0
____ 42) 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.
Isotope Abundance Mass38X 5.07 37.91939X 15.35 39.01742X 79.85 42.111
A) 41.54B) 39.68C) 39.07D) 38.64E) 33.33
____ 43) 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 Abundance Mass159X 30.60 159.37163X 15.79 162.79164X 53.61 163.92
A) 161.75B) 162.03C) 162.35D) 163.15E) 33.33
Name: ______________________ ID: A
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____ 44) 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 Abundance Mass53X 19.61 52.6256X 53.91 56.2958X 26.48 58.31
A) 33.33B) 55.74C) 56.11D) 57.23E) 56.29
____ 45) The element X has two 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.
Isotope Abundance (%) Mass (amu)31X 35.16 31.1634X 64.84 34.30
A) 30.20B) 33.20C) 34.02D) 35.22E) 32.73
____ 46) The average atomic weight of copper, which has two naturally occurring isotopes, is 63.5. One of the isotopes has an atomic weight of 62.9 amu and constitutes 69.1% of the copper isotopes. The other isotope has an abundance of 30.9%. The atomic weight (amu) of the second isotope is __________ amu.A) 63.2B) 63.8C) 64.1D) 64.8E) 28.1
Name: ______________________ ID: A
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____ 47) 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.
Isotope Abundance (%) Mass (amu)15X 28.60 15.3317X 13.30 17.2616X 58.10 18.11
A) 17.20B) 16.90C) 17.65D) 17.11E) 16.90
____ 48) Vanadium has two naturally occurring isotopes, 50V with an atomic mass of 49.9472 amu and 51V with an atomic mass of 50.9440. The atomic weight of vanadium is 50.9415. The percent abundances of the vanadium isotopes are __________% 50V and __________% 51V.A) 0.25, 99.75B) 99.75, 0.25C) 49, 51D) 1.0, 99E) 99, 1.0
____ 49) An unknown element is found to have three naturally occurring isotopes with atomic masses of 35.9675 (0.337%), 37.9627 (0.063%), and 39.9624 (99.600%). Which of the following is the unknown element?A) ArB) KC) ClD) CaE) None of the above could be the unknown element.
____ 50) In the periodic table, the elements are arranged in __________.A) alphabetical orderB) order of increasing atomic numberC) order of increasing metallic propertiesD) order of increasing neutron contentE) reverse alphabetical order
Name: ______________________ ID: A
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____ 51) Elements __________ exhibit similar physical and chemical properties.A) with similar chemical symbolsB) with similar atomic massesC) in the same period of the periodic tableD) on opposite sides of the periodic tableE) in the same group of the periodic table
____ 52) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties?A) H, LiB) Cs, BaC) Ca, SrD) Ga, GeE) C, O
____ 53) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties?A) O, SB) C, NC) K, CaD) H, HeE) Si, P
____ 54) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties?A) As, BrB) Mg, AlC) I, AtD) Br, KrE) N,O
____ 55) The elements in groups 1A, 6A, and 7A are called, __________, respectively.A) alkaline earth metals, halogens, and chalcogensB) alkali metals, chalcogens, and halogensC) alkali metals, halogens, and noble gasesD) alkaline earth metals, transition metals, and halogensE) halogens, transition metals, and alkali metals
____ 56) Which pair of elements below should be the most similar in chemical properties?A) C and OB) B and AsC) I and BrD) K and KrE) Cs and He
Name: ______________________ ID: A
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____ 57) An element in the upper right corner of the periodic table __________.A) is either a metal or metalloidB) is definitely a metalC) is either a metalloid or a non-metalD) is definitely a non-metalE) is definitely a metalloid
____ 58) An element that appears in the lower left corner of the periodic table is __________.A) either a metal or metalloidB) definitely a metalC) either a metalloid or a non-metalD) definitely a non-metalE) definitely a metalloid
____ 59) Elements in the same group of the periodic table typically have __________.A) similar mass numbersB) similar physical properties onlyC) similar chemical properties onlyD) similar atomic massesE) similar physical and chemical properties
____ 60) Which one of the following does not occur as diatomic molecules in elemental form?A) oxygenB) nitrogenC) sulfurD) hydrogenE) bromine
____ 61) Which one of the following molecular formulas is also an empirical formula?A) C6H6O2
B) C2H6SOC) H2O2
D) H2P4O6
E) C6H6
____ 62) Which compounds do not have the same empirical formula?A) C172H2, C6H6
B) CO, CO2
C) C2H4, C3H6
D) C2H4O2, C6H12O6
E) C2H5COOOCH3, CH3CHO
Name: ______________________ ID: A
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____ 63) Of the choices below, which one is not an ionic compound?A) PCl5
B) MoCl6
C) RbClD) PbCI2
E) NaCl
____ 64) Which type of formula provides the most information about a compound?A) empiricalB) molecularC) simplestD) structuralE) chemical
____ 65) A molecular formula always indicates __________.A) how many of each atom are in a moleculeB) the simplest whole-number ratio of different atoms in a compoundC) which atoms are attached to which in a moleculeD) the isotope of each element in a compoundE) the geometry of a molecule
____ 66) An empirical formula always indicates __________.A) which atoms are attached to which in a moleculeB) how many of each atom are in a moleculeC) the simplest whole-number ratio of different atoms in a compoundD) the isotope of each element in a compoundE) the geometry of a molecule
____ 67) The molecular formula of a compound is always __________ the empirical formula.A) more complex thanB) different fromC) an integral multiple ofD) the same asE) simpler than
____ 68) Formulas that show how atoms are attached in a molecule are called __________.A) molecular formulasB) ionic formulasC) empirical formulasD) diatomic formulasE) structural formulas
Name: ______________________ ID: A
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____ 69) Of the following, __________ contains the greatest number of electrons.A) P3+
B) PC) P2-
D) P3-
E) P2+
____ 70) Which one of the following is most likely to lose electrons when forming an ion?A) FB) PC) RhD) SE) N
____ 71) Which species has 54 electrons?
A) 54132 Xe+
B) 52128 Te2
C) 50118 Sn2 +
D) 48112 Cd
E) 54132 Xe2 +
____ 72) Which species has 16 protons?A) 31PB) 34S2-
C) 36ClD) 80Br-
E) 16O
____ 73) Which species has 18 electrons?A) 39KB) 32S-2
C) 35ClD) 27Al+3
E) 64Cu+2
Name: ______________________ ID: A
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____ 74) The species __________ contains 16 neutrons.A) 31PB) 34S2-
C) 36ClD) 80Br-
E) 16O
____ 75) Which species is an isotope of 39Cl?A) 40Ar+
B) 34S2-
C) 36Cl-
D) 80BrE) 39Ar
____ 76) Which one of the following species has as many electrons as it has neutrons?A) 1HB) 40Ca2+
C) 14CD) 19F-E) 14C2+
____ 77) There are __________ protons, __________ neutrons, and __________ electrons in 131I-.A) 131, 53, and 54B) 131, 53, and 52C) 53, 78, and 54D) 53, 131, and 52E) 78, 53, and 72
____ 78) There are __________ protons, __________ neutrons, and __________ electrons in 238U+5.A) 146, 92, and 92B) 92, 146, and 87C) 92, 146, and 92D) 92, 92, and 87E) 146, 92, and 146
Name: ______________________ ID: A
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____ 79) Which species has 48 electrons?
A) 50118 Sn+2
B) 50116 Sn+4
C) 480112 Cd+2
D) 3168 Ga
E) 2248 Ti
____ 80) Which of the following compounds would you expect to be ionic?A) SF6
B) H2OC) H2O2
D) NH3
E) CaO
____ 81) Which of the following compounds would you expect to be ionic?A) H2OB) CO2
C) SrCI2
D) SO2
E) H2S
____ 82) Which pair of elements is most apt to form an ionic compound with each other?A) barium, bromineB) calcium, sodiumC) oxygen, fluorineD) sulfur, fluorineE) nitrogen, hydrogen
____ 83) Which pair of elements is most apt to form a molecular compound with each other?A) aluminum, oxygenB) magnesium, iodineC) sulfur, fluorineD) potassium, lithiumE) barium, bromine
Name: ______________________ ID: A
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____ 84) Which species below is the nitride ion?A) Na+
B) NO3-C) NO2-D) NH4+E) N3-
____ 85) Which species below is the sulfite ion?A) SO2-2
B) S O3-2
C) S2-
D) SO4-2
E) HS-
____ 86) Which species below is the nitrate ion?A) NO2-B) NH4+C) NO3-D) N3-E) N3-
____ 87) Which species below is the nitrite ion?A) NO2-B) NH4+C) NO3-D) N3-E) N3-
____ 88) Barium reacts with a polyatomic ion to form a compound with the general formula Ba3(X)2. What would be the most likely formula for the compound formed between sodium and the polyatomic ion X?A) NaXB) Na2XC) Na2X2
D) Na3XE) Na3X2
____ 89) 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) 3AB) 4AC) 5AD) 6AE) 7A
Name: ______________________ ID: A
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____ 90) The formula for a salt is XBr. The X-ion in this salt has 46 electrons. The metal X is __________.A) AgB) PdC) CdD) CuE) Cs
____ 91) The charge on the copper ion in the salt CuO is __________.A) +1B) +2C) +3D) -1E) -2
____ 92) The charge on the iron ion in the salt Fe2O3 is __________.A) +1B) +2C) +3D) -5E) -6
____ 93) Which formula/name pair is incorrect?A) Mn(NO2)4 manganese(II) nitriteB) Mg(NO3)2 magnesium nitrateC) Mn(NO3)2 manganese(II) nitrateD) Mg3N2 magnesium nitriteE) Mg(MnO4)2 magnesium permanganate
____ 94) Which formula/name pair is incorrect?A) FeSO4 iron(II) sulfateB) Fe2(SO3)3 iron(III) sulfiteC) FeS iron(II) sulfideD) FeSO3 iron(II) sulfiteE) Fe2(SO4)3 iron(III) sulfide
____ 95) Which one of the following is the formula of hydrochloric acid?A) HClO3
B) HClO4
C) HClOD) HClE) HClO2
Name: ______________________ ID: A
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____ 96) The suffix -ide is used primarily __________.A) for monatomic anion namesB) for polyatomic cation namesC) for the name of the first element in a molecular compoundD) to indicate binary acidsE) for monoatomic cations
____ 97) Which one of the following compounds is chromium(III) oxide?A) Cr2O3
B) CrO3
C) Cr3O2
D) Cr3OE) Cr2O4
____ 98) Which one of the following compounds is copper(I) chloride?A) CuClB) CuCl2
C) Cu2ClD) Cu2Cl3
E) Cu3Cl2
____ 99) The correct name for MgF2 is __________.A) monomagnesium difluorideB) magnesium difluorideC) manganese difluorideD) manganese bifluorideE) magnesium fluoride
____ 100) The correct name for NaHCO3 is __________.A) sodium hydrideB) persodium carbonateC) persodium hydroxideD) sodium bicarbonateE) carbonic acid
____ 101) A correct name for Fe(NO3)2 is __________.A) iron nitriteB) ferrous nitriteC) ferrous nitrateD) ferric nitriteE) ferric nitrate
Name: ______________________ ID: A
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____ 102) The correct name for HNO2 is __________.A) nitrous acidB) nitric acidC) hydrogen nitrateD) hyponitrous acidE) pernitric acid
____ 103) The proper formula for the hydronium ion is __________.A) H-
B) OH-
C) N-3
D) H3O+
E) NH4+
____ 104) The charge on the __________ ion is -3.A) sulfateB) acetateC) permanganateD) oxideE) nitride
____ 105) Which one of the following polyatomic ions has the same charge as the hydroxide ion?A) ammoniumB) carbonateC) nitrateD) sulfateE) phosphate
____ 106) Which element forms an ion with the same charge as the ammonium ion?A) potassiumB) chlorineC) calciumD) oxygenE) nitrogen
____ 107) Which element forms an ion with the same charge as the sulfate ion?A) magnesiumB) copperC) ironD) phosphorusE) oxygen
Name: ______________________ ID: A
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____ 108) When a fluorine atom forms the fluoride ion, it has the same charge as the __________ ion.A) sulfideB) ammoniumC) nitrateD) phosphateE) sulfite
____ 109) The formula for the compound formed between aluminum ions and phosphate ions is __________.A) Al3(PO4)3
B) AlPO4
C) Al(PO4)3
D) Al2(PO4)3
E) AlP
____ 110) Which metal does not form cations of differing charges?A) NaB) CuC) CoD) FeE) Sn
____ 111) Which metal forms cations of differing charges?A) KB) CsC) BaD) AlE) Sn
____ 112) The correct name for Ni(CN)2 is __________.A) nickel (I) cyanideB) nickel cyanateC) nickel carbonateD) nickel (II) cyanideE) nickel (I) nitride
____ 113) The correct name for Na2O2 is __________.A) sodium oxideB) sodium dioxideC) disodium oxideD) sodium peroxideE) disodium dioxide
Name: ______________________ ID: A
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____ 114) Which metal is not required to have its charge specified in the names of ionic compounds it forms?A) MnB) FeC) CuD) CaE) Pb
____ 115) What is the molecular formula for 1-propanol?A) CH3OHB) C2H5OHC) C3H7OHD) C4H9OHE) C5H11OH
____ 116) 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 compositionB) multiple proportionsC) conservation of matterD) conservation of massE) octaves
____ 117) __________ and __________ reside in the atomic nucleus.A) Protons, electronsB) Electrons, neutronsC) Protons, neutronsD) none of the aboveE) Neutrons, only neutrons
____ 118) 200 pm is the same as __________ Å.A) 2000B) 20C) 200D) 2E) 0.0002
____ 119) The atomic number indicates __________.A) the number of neutrons in a nucleusB) the total number of neutrons and protons in a nucleusC) the number of protons or electrons in a neutral atomD) the number of atoms in 1 g of an elementE) the number of different isotopes of an element
Name: ______________________ ID: A
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____ 120) The nucleus of an atom contains __________.A) electronsB) protons, neutrons, and electronsC) protons and neutronsD) protons and electronsE) protons
____ 121) In the periodic table, the rows are called __________ and the columns are called __________.A) octaves, groupsB) staffs, familiesC) periods, groupsD) cogeners, familiesE) rows, groups
____ 122) Which group in the periodic table contains only nonmetals?A) 1AB) 6AC) 2BD) 2AE) 8A
____ 123) Horizontal rows of the periodic table are known as __________.A) periodsB) groupsC) metalloidsD) metalsE) nonmetals
____ 124) Vertical columns of the periodic table are known as __________.A) metalsB) periodsC) nonmetalsD) groupsE) metalloids
____ 125) Elements in Group 1A are known as the __________.A) chalcogensB) alkaline earth metalsC) alkali metalsD) halogensE) noble gases
Name: ______________________ ID: A
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____ 126) Elements in Group 2A are known as the __________.A) alkaline earth metalsB) alkali metalsC) chalcogensD) halogensE) noble gases
____ 127) Elements in Group 6A are known as the __________.A) alkali metalsB) chalcogensC) alkaline earth metalsD) halogensE) noble gases
____ 128) Elements in Group 7A are known as the __________.A) chalcogensB) alkali metalsC) alkaline earth metalsD) halogensE) noble gases
____ 129) Elements in Group 8A are known as the __________.A) halogensB) alkali metalsC) alkaline earth metalsD) chalcogensE) noble gases
____ 130) Potassium is a __________ and chlorine is a __________.A) metal, nonmetalB) metal, metalC) metal, metalloidD) metalloid, nonmetalE) nonmetal, metal
____ 131) Lithium is a __________ and magnesium is a __________.A) nonmetal, metalB) nonmetal, nonmetalC) metal, metalD) metal, metalloidE) metalloid, metalloid
Name: ______________________ ID: A
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____ 132) Oxygen is a __________ and nitrogen is a __________.A) metal, metalloidB) nonmetal, metalC) metalloid, metalloidD) nonmetal, nonmetalE) nonmetal, metalloid
____ 133) Calcium is a __________ and silver is a __________.A) nonmetal, metalB) metal, metalC) metalloid, metalD) metal, metalloidE) nonmetal, metalloid
____ 134) __________ are found uncombined, as monatomic species in nature.A) Noble gasesB) ChalcogensC) Alkali metalsD) Alkaline earth metalsE) Halogens
____ 135) When a metal and a nonmetal react, the __________ tends to lose electrons and the __________ tends to gain electrons.A) metal, metalB) nonmetal, nonmetalC) metal, nonmetalD) nonmetal, metalE) None of the above, these elements share electrons.
____ 136) The empirical formula of a compound with molecules containing 12 carbon atoms, 14 hydrogen atoms, and 6 oxygen atoms is __________.A) C12H14O6
B) CHOC) CH2OD) C6 H7O3
E) C2H4O
____ 137) __________ typically form ions with a 2+ charge.A) Alkaline earth metalsB) HalogensC) ChalcogensD) Alkali metalsE) Transition metals
Name: ______________________ ID: A
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____ 138) What is the formula of the compound formed between strontium ions and nitrogen ions?A) SrNB) Sr3N2
C) Sr2N3
D) SrN2
E) SrN3
____ 139) Magnesium reacts with a certain element to form a compound with the general formula MgX. What would the most likely formula be for the compound formed between potassium and element X?A) K2XB) KX2
C) K2X3
D) K2X2
E) KX
____ 140) The charge on the manganese in the salt MnF3 is __________.A) 1+B) 1-C) 2+D) 2-E) 3+
____ 141) 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) oxygenB) fluorineC) chlorineD) nitrogenE) sulfur
____ 142) Sodium forms an ion with a charge of __________.A) 1+B) 1-C) 2+D) 2-E) 0
____ 143) Potassium forms an ion with a charge of __________.A) 2+B) 1-C) 1+D) 2-E) 0
Name: ______________________ ID: A
28
____ 144) Calcium forms an ion with a charge of __________.A) 1-B) 2-C) 1+D) 2+E) 0
____ 145) Barium forms an ion with a charge of __________.A) 1+B) 2-C) 3+D) 3-E) 2+
____ 146) Aluminum forms an ion with a charge of __________.A) 2+B) 3-C) 1+D) 3+E) 1-
____ 147) Fluorine forms an ion with a charge of __________.A) 1-B) 1+C) 2+D) 3+E) 3-
____ 148) Iodine forms an ion with a charge of __________.A) 7-B) 1+C) 2-D) 2+E) 1-
____ 149) Oxygen forms an ion with a charge of __________.A) 2-B) 2+C) 3-D) 3+E) 6+
Name: ______________________ ID: A
29
____ 150) Sulfur forms an ion with a charge of __________.A) 2+B) 2-C) 3+D) 6-E) 6+
____ 151) Predict the empirical formula of the ionic compound that forms from sodium and fluorine.A) NaFB) Na2FC) Na F2
D) Na2F3
E) Na3F2
____ 152) Predict the empirical formula of the ionic compound that forms from magnesium and fluorine.A) Mg2F3
B) MgFC) Mg2FD) Mg3F2
E) MgF2
____ 153) Predict the empirical formula of the ionic compound that forms from magnesium and oxygen.A) Mg2OB) MgOC) MgO2
D) Mg2O2
E) Mg3O2
____ 154) Predict the empirical formula of the ionic compound that forms from aluminum and oxygen.A) AlOB) Al3O2
C) Al2O3
D) AlO2
E) Al2O
____ 155) The correct name for K2S is __________.A) potassium sulfateB) potassium disulfideC) potassium bisulfideD) potassium sulfideE) dipotassium sulfate
Name: ______________________ ID: A
30
____ 156) The correct name for Al2O3 is __________.A) aluminum oxideB) dialuminum oxideC) dialuminum trioxideD) aluminum hydroxideE) aluminum trioxide
____ 157) The correct name for Ca H2 is __________.A) hydrocalciumB) calcium dihydrideC) calcium hydroxideD) calcium dihydroxideE) calcium hydride
____ 158) The correct name for SO is __________.A) sulfur oxideB) sulfur monoxideC) sulfoxideD) sulfateE) sulfite
____ 159) The correct name for CCl4 is __________.A) carbon chlorideB) carbon tetrachlorateC) carbon perchlorateD) carbon tetrachlorideE) carbon chlorate
____ 160) The correct name for N2O5 is __________.A) nitrous oxideB) nitrogen pentoxideC) dinitrogen pentoxideD) nitric oxideE) nitrogen oxide
____ 161) The correct name for H2CO3 is __________.A) carbonous acidB) hydrocarbonateC) carbonic acidD) carbohydrateE) carbohydric acid
Name: ______________________ ID: A
31
____ 162) The correct name for H2CO3 is __________.A) sulfuric acidB) sulfurous acidC) hydrosulfuric acidD) hydrosulfic acidE) sulfur hydroxide
____ 163) The correct name for H2SO4 is __________.A) sulfuric acidB) sulfurous acidC) hydrosulfuric acidD) hydrosulfic acidE) sulfur hydroxide
____ 164) The correct name for HNO3 is __________.A) nitrous acidB) nitric acidC) hydronitroxide acidD) nitroxide acidE) nitrogen hydroxide
____ 165) The correct name for HClO3 is __________.A) hydrochloric acidB) perchloric acidC) chloric acidD) chlorous acidE) hydrochlorous acid
____ 166) The correct name for HClO is __________.A) hydrochloric acidB) perchloric acidC) chloric acidD) chlorous acidE) hypochlorous acid
____ 167) The correct name for HBrO4 is __________.A) hydrobromic acidB) perbromic acidC) bromic acidD) bromous acidE) hydrobromous acid
Name: ______________________ ID: A
32
____ 168) The correct name for HBrO is __________.A) hydrobromic acidB) perbromic acidC) bromic acidD) bromous acidE) hypobromous acid
____ 169) The correct name for HBrO2 is __________.A) hydrobromic acidB) perbromic acidC) bromic acidD) bromous acidE) hydrobromous acid
____ 170) The correct name for HClO2 is __________.A) perchloric acidB) chloric acidC) hypochlorous acidD) hypychloric acidE) chlorous acid
____ 171) The correct name of the compound Na3N is __________.A) sodium nitrideB) sodium azideC) sodium trinitrideD) sodium(III) nitrideE) trisodium nitride
____ 172) The formula of bromic acid is __________.A) HBrB) HBrO4
C) HBrOD) HBrO3
E) HBrO2
____ 173) The correct formula for molybdenum(IV) hypochlorite is __________.A) Mo(ClO3)4
B) Mo(ClO)4
C) Mo(ClO2)4
D) Mo(ClO4)4
E) MoCl4
Name: ______________________ ID: A
33
____ 174) The name of PCl3 is __________.A) potassium chlorideB) phosphorus trichlorideC) phosphorous(III) chlorideD) monophosphorous trichlorideE) trichloro potassium
____ 175) The ions Ca2+and PO43- form a salt with the formula __________.A) CaPO4
B) Ca2 (PO4)3
C) Ca2PO4
D) Ca(PO4)2
E) Ca3 (PO4)2
____ 176) The correct formula of iron(III) bromide is __________.A) FeBr2
B) FeBr3
C) FeBrD) Fe3Br3
E) Fe3Br
____ 177) Magnesium and sulfur form an ionic compound with the formula __________.A) MgSB) Mg2SC) Mg S2
D) Mg2S2
E) Mg2S3
____ 178) The formula of ammonium carbonate is __________.A) (NH4)2CO3
B) NH4CO2
C) (NH3)2CO4
D) (NH3)2CO3
E) N2(CO3)3
____ 179) The formula of the chromate ion is __________.A) CrO42-
B) CrO23-
C) CrO-
D) CrO32-
E) CrO2-
Name: ______________________ ID: A
34
____ 180) The formula of the carbonate ion is __________.A) CO22-
B) CO32-
C) CO23-
D) CO2-
E) CO-
____ 181) The correct name for Mg(ClO3)2 is __________.A) magnesium chlorateB) manganese chlorateC) magnesium chloroxideD) magnesium perchlorateE) manganese perchlorate
____ 182) What is the correct formula for ammonium sulfide?A) NH4SO3
B) (NH4)2SO4
C) (NH4)2SD) NH3SE) N2S3
____ 183) When calcium reacts with sulfur the compound formed is __________.A)Ca2S2
A) Ca3S2
B) CaS2
C) CaSD) CaS2
E) Ca2S3
____ 184) Chromium and chlorine form an ionic compound whose formula is CrCl3. The name of this compound is __________.A) chromium chlorineB) chromium(III) chlorideC) monochromium trichlorideD) chromium(III) trichlorideE) chromic trichloride
____ 185) Iron and chlorine form an ionic compound whose formula is FeCl3. The name of this compound is __________.A) iron chlorineB) iron (III) chlorideC) moniron trichlorideD) iron (III) trichlorideE) ferric trichloride
Name: ______________________ ID: A
35
____ 186) Copper and chlorine form an ionic compound whose formula is CuCl2. The name of this compound is __________.A) copper chlorineB) copper (III) dichlorideC) monocopper dichlorideD) copper (II) dichlorideE) cupric chloride
____ 187) The name of the binary compound N2O4 is __________.A) nitrogen oxideB) nitrous oxideC) nitrogen(IV) oxideD) dinitrogen tetroxideE) oxygen nitride
____ 188) The formula for zinc phosphate is Zn3(PO4)2. What is the formula for cadmium arsenate?A) Cd4 (AsO2)3
B) Cd3 (AsO4)2
C) Cd3 (AsO3)4
D) Cd2 (AsO4)3
E) Cd2 (AsO4)4
____ 189) The formula for aluminum hydroxide is __________.A) AlOHB) Al3OHC) Al2(OH)3
D) Al(OH)3
E) Al2O3
____ 190) The name of the ionic compound V2O3 is __________.A) vanadium(III) oxideB) vanadium oxideC) vanadium(II) oxideD) vanadium(III) trioxideE) divanadium trioxide
____ 191) The name of the ionic compound NH4CN is __________.A) nitrogen hydrogen cyanateB) ammonium carbonitrideC) ammonium cyanideD) ammonium hydrogen cyanateE) cyanonitride
Name: ______________________ ID: A
36
____ 192) The name of the ionic compound (NH4)3PO4 is __________.A) ammonium phosphateB) nitrogen hydrogen phosphateC) tetrammonium phosphateD) ammonia phosphideE) triammonium phosphate
____ 193) What is the formula for perchloric acid?A) HClOB) HClO3
C) HClO4
D) HClO2
E) HCl
____ 194) The correct name for HIO2 is __________.A) hypoiodic acidB) hydriodic acidC) periodous acidD) iodous acidE) periodic acid
____ 195) What is the molecular formula for propane?A) C2H8
B) C3H6
C) C3H8
D) C4H8
E) C4H10
____ 196) What is the molecular formula for butane?A) C2H8
B) C3H6
C) C3H8
D) C4H8
E) C4H10
____ 197) What is the molecular formula for octane?A) C4H10
B) C5H10
C) C6H14
D) C14H28
E) C8H18
Name: ______________________ ID: A
37
____ 198) What is the molecular formula for pentane?A) C2H8
B) C3H6
C) C4H8
D) C5H12
E) C5H10
____ 199) What is the molecular formula for nonane?A) C9H18
B) C9H20
C) C10H20
D) C10H22
E) C10H24
____ 200) What is the molecular formula for heptane?A) C6H12
B) C6H14
C) C7H14
D) C7H16
E) C7H18
____ 201) What is the molecular formula for 1-hexanol?A) C6H12OHB) C6H13OHC) C6H14OHD) C7H13OHE) C7H14OH
____ 202) A certain mass of carbon reacts with 23.3 g of oxygen to form carbon monoxide. __________ grams of oxygen would react with that same mass of carbon to form carbon dioxide, according to the law of multiple proportions?A) 25.6B) 11.7C) 23.3D) 233E) 46.6
____ 203) An atom of 14C contains __________ protons.A) 6B) 20C) 8D) 10E) 14
Name: ______________________ ID: A
38
____ 204) An atom of 118Xe contains __________ neutrons.A) 54B) 172C) 64D) 110E) 118
____ 205) An atom of 131Xe contains __________ electrons.A) 131B) 185C) 77D) 123E) 54
____ 206) 420 pm is the same as __________ Angstroms.A) 4200B) 42C) 420D) 4.2E) 0.42
____ 207) 400 pm is the same as __________ Å.A) 4000B) 40C) 400D) 4E) 0.0004
____ 208) The mass number of an atom of 128Xe is __________.A) 54B) 182C) 74D) 128E) 120
____ 209) The atomic number of an atom of 80Br is __________.A) 115B) 35C) 45D) 73E) 80
Name: ______________________ ID: A
39
____ 210) An ion has 8 protons, 9 neutrons, and 10 electrons. The symbol for the ion is __________.A) 17O2-
B) 17O2+
C) 19F+D) 19F-E) 17Ne2+
____ 211) The element __________ is the most similar to chlorine in chemical and physical properties.A) LiB) RbC) OD) BrE) Ba
____ 212) Which one of the following is a metal?A) SbB) GeC) BrD) PE) W
____ 213) Of the following, only __________ is not a metal.A) HgB) SeC) VD) LuE) Y
____ 214) Which of the following elements is a nonmetal?A) PB) SiC) AsD) BE) Sr
____ 215) How many electrons does the Al3+ ion possess?A) 16B) 10C) 6D) 0E) 13
Name: ______________________ ID: A
40
____ 216) How many protons does the Br- ion possess?A) 34B) 36C) 6D) 8E) 35
____ 217) The formula of a salt is XCI2. The X-ion in this salt has 27 electrons. The metal X is __________.A) NiB) CuC) CoD) FeE) Zn
____ 218) Predict the charge of the most stable ion of bromine.A) 2+B) 1+C) 3+D) 1-E) 2-
____ 219) Predict the charge of the most stable ion of potassium.A) 3+B) 1-C) 2+D) 2-E) 1+
____ 220) The correct name for SrO is __________.A) strontium oxideB) strontium hydroxideC) strontium peroxideD) strontium monoxideE) strontium dioxide
____ 221) Element M reacts with fluorine to form an ionic compound with the formula MF3. The M-ion has 22 electrons. Element M is __________.A) AlB) MnC) FeD) ScE) Cr
Name: ______________________ ID: A
41
____ 222) The name of the ionic compound RbBrO4 is __________.A) rubidium perbromateB) rubidium bromateC) rubidium hypobromateD) rubidium perbromiteE) rubidium bromide
223) What group in the periodic table would the fictitious element : : be found?
224) Which element in Group IA is the most electropositive?
225) The formula for potassium sulfide is __________.
226) What is the name of an alcohol derived from hexane?
____ 227) The possible oxidation numbers for iron are +1 and +2.
____ 228) The formula for chromium (II) iodide is CrI2.
____ 229) H2SeO4 is called selenic acid.
____ 230) The correct name for Na3N is sodium azide.
