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Chem Final Combined

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10) In the Rutherford nuclear-atom model, ________. A) the heavy subatomic particles, protons and neutrons, reside in the nucleus B) the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass C) the light subatomic particles, protons and neutrons, reside in the nucleus D) mass is spread essentially uniformly throughout the atom E) the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass and mass is spread essentially uniformly throughout the atom

10) Which of the following are combustion reactions? 1) CH4 (g) + O2 (g) → CO2 (g) + H2O (l) 2) CaO (s) + CO2 (g) → CaCO3 (s) 3) PbCO3 (s) → PbO (s) + CO2 (g) 4) CH3OH (l) + O2 (g) → CO2 (g) + H2O (l) A) 1 and 4 B) 1, 2, 3, and 4 C) 1, 3, and 4 D) 2, 3, and 4 E) 3 and 4

100) Which metal does not form cations of differing charges? A) Na B) Cu C) Co D) Fe E) Sn

13) The law of constant composition says ________. A) that the composition of a compound is always the same B) that all substances have the same composition C) that the composition of an element is always the same D) that the composition of a homogeneous mixture is always the same E) that the composition of a heterogeneous mixture is always the same

13) Which combination will produce a precipitate? A) Pb(NO3)2 (aq) and HCl (aq) B) Cu(NO3)2 (aq) and KC2H3O2 (aq) C) KOH (aq) and HNO3 (aq) D) AgC2H3O2 (aq) and HC2H3O2 (aq) E) NaOH (aq) and Sr(NO3)2 (aq)

13) Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number? A) 2d B) 2s C) 2p D) all of the above E) none of the above

14) For a given process at constant pressure, w is positive. This means that the process involves ________. A) work being done by the system on the surroundings B) work being done by the surroundings on the system C) no work being done D) an equal amount of work done on the system and by the system E) work being done against a vacuum

16) The molecular weight of the acetic acid (CH3CO2H), rounded to the nearest integer, is ________ amu. A) 60 B) 48 C) 44 D) 32

19) Which quantum number determines the energy of an electron in a hydrogen atom? A) n B) E C) ml D) l E) n and l

2) Of the following, ________ radiation has the shortest wavelength. A) X-ray B) radio C) microwave D) ultraviolet E) infrared

2) The internal energy of a system is always increased by ________. A) adding heat to the system B) having the system do work on the surroundings C) withdrawing heat from the system D) adding heat to the system and having the system do work on the surroundings E) a volume compression

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.

22) The mass % of H in methane (CH4) is ________. A) 25.13 B) 4.032 C) 74.87 D) 92.26 E) 7.743

23) Of the following, ________ is the largest mass. A) 25 kg B) 2.5 × 10-2 mg C) 2.5 × 1015 pg D) 2.5 × 109 fg E) 2.5 × 1010 ng

24) Which combination of protons, neutrons, and electrons is correct for the isotope of copper, 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-

24) Which one of the following is the highest temperature? A) 38 °C B) 96 °F C) 302 K D) none of the above E) the freezing point of water

27) Which isotope has 36 electrons in an atom? A) Kr B) Br C) Se D) Cl E) Hg

27) Which of the following is a valid set of four quantum numbers? (n, l, ml, ms) A) 2, 1, 0, +1/2 B) 2, 2, 1, -1/2 C) 1, 0, 1, +1/2 D) 2, 1, +2, +1/2 E) 1, 1, 0, -1/2

28) Calculate the percentage by mass of chlorine in PtCl2(NH3)2. A) 23.63 B) 11.82 C) 25.05 D) 12.53 E) 18.09

28) Of the choices below, which would be the best for the lining of a tank intended for use in storage of hydrochloric acid? A) copper B) zinc C) nickel D) iron E) tin

28) Which calculation clearly shows a conversion between temperatures in degrees Celsius, °C, and temperature in Kelvins, K? A) K = °C + 273.15 B) K = 273.15 - °C C) K = [°C - 32] / 1.8 D) K = [°C + 32] × 1.8 E) K = °C

29) You have to calculate the mass of a 30.0 mL liquid sample with density of 1.52 g/mL, but you have forgotten the formula. Which way of reasoning would help you in finding the correct mass? A) If 1 mL of a liquid has the mass of 1.52 g, then 30.0 mL has the mass of __________ g. B) If 1.52 mL of a liquid has the mass of 1 g, then 30.0 mL has the mass of __________ g.

3) When a hydrocarbon burns in air, what component of air reacts? A) oxygen B) nitrogen C) carbon dioxide D) water E) argon

30) Which of these metals will be oxidized by the ions of aluminum? A) magnesium B) zinc C) chromium D) iron E) nickel

30) You have to calculate the volume of a gas sample with mass of 1.000 × 103 g and density of 1.027 g/L, but you have forgotten the formula. Which way of reasoning would help you in finding the correct mass? A) If 1.027 g of a gas takes up a volume of 1 L, then 1.000 × 103 g of the same gas takes up a volume of __________. B) If 1.027 L of gas has a mass of 1 g, then __________ L has the mass of 1.000 × 103 g.

31) Different isotopes of a particular element contain the same number of ________. A) protons B) neutrons C) protons and neutrons D) protons, neutrons, and electrons E) subatomic particles

31) Osmium has a density of 22.6 g/cm3. What volume (in cm3) would be occupied by a 21.8 g sample of osmium? A) 0.965 B) 1.04 C) 493 D) 2.03 × 10-3 E) 2.03 × 103

33) Precision refers to ________. A) how close a measured number is to other measured numbers B) how close a measured number is to the true value C) how close a measured number is to the calculated value D) how close a measured number is to zero E) how close a measured number is to infinity

37) If an object is accelerating at a rate of 25 m/s2, how long (in seconds) will it take to reach a speed of 550 m/s? (Assume an initial velocity of zero.) A) 22 B) 1.4 × 104 C) 0.045 D) 1.2 × 104 E) 2.3 × 102

37) Which one of the following configurations depicts an excited carbon atom? A) 1s22s22p13s1 B) 1s22s22p3 C) 1s22s22p1 D) 1s22s23s1 E) 1s22s22p2

4) A small amount of salt dissolved in water is an example of a ________. A) homogeneous mixture B) heterogeneous mixture C) compound D) pure substance E) solid

41) Which of the following is an oxidation-reduction reaction? A) Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2 (aq) B) HCl (aq) + NaOH (aq) → H2O (l) + NaCl (aq) C) AgNO3 (aq) + HCl (aq) → AgCl (s) + HNO3 (aq) D) Ba(C2H3O2)2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaC2H3O2(aq) E) H2CO3 (aq) + Ca(NO3)2 (aq) → 2HNO3 (aq) + CaCO3 (s)

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. A) 41.54 B) 39.68 C) 39.07 D) 38.64 E) 33.33

43) In which one of the following numbers are all of the zeros significant? A) 100.090090 B) 0.143290 C) 0.05843 D) 0.1000 E) 00.0030020

44) How many oxygen atoms are there in 52.06 g of carbon dioxide? A) 1.424 × 1024 B) 6.022 × 1023 C) 1.204 × 1024 D) 5.088 × 1023 E) 1.018 × 1024

44) Which of the following elements has a ground-state electron configuration different from the predicted one? A) Cu B) Ca C) Xe D) Cl E) Ti

46) How many grams of sodium carbonate contain 1.773 × 1017 carbon atoms? A) 3.121 × 10-5 B) 1.011 × 10-5 C) 1.517 × 10-5 D) 9.100 × 10-5 E) 6.066 × 10-5

47) One angstrom, symbolized Å, is 10-10 m. 1 cm3 = ________ Å3. A) 1024 B) 10-24 C) 1030 D) 10-30 E) 10-9

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. A) 17.20 B) 16.90 C) 17.65 D) 17.11 E) 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, 99.75 B) 99.75, 0.25 C) 49, 51 D) 1.0, 99 E) 99, 1.0

48) What are the respective concentrations (M) of Fe3+ and I- afforded by dissolving 0.200 mol FeI3 in water and diluting to 725 mL? A) 0.276 and 0.828 B) 0.828 and 0.276 C) 0.276 and 0.276 D) 0.145 and 0.435 E) 0.145 and 0.0483

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) Ar B) K C) Cl D) Ca E) None of the above could be the unknown element.

5) Of the reactions below, which one is a decomposition reaction? A) NH4Cl → NH3 + HCl B) 2Mg + O2 → 2MgO C) 2N2 + 3H2 → 2NH3 D) 2CH4 + 4O2 → 2CO2 + 4H2O E) Cd(NO3)2 + Na2S → CdS + 2NaNO3

50) A tenfold dilution of a sample solution can be obtained by taking ________. A) 1 part sample and 9 parts solvent B) 1 part sample and 10 parts solvent C) 9 parts sample and 1 part solvent D) 10 parts sample and 1 part solvent E) 99 parts sample and 1 part solvent

53) A 0.100 M solution of ________ will contain the highest concentration of potassium ions. A) potassium phosphate B) potassium hydrogen carbonate C) potassium hypochlorite D) potassium iodide E) potassium oxide

53) 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

61) Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization? A) 10.0 mL of 0.0500 M phosphoric acid B) 20.0 mL of 0.0500 M nitric acid C) 5.0 mL of 0.0100 M sulfuric acid D) 15.0 mL of 0.0500 M hydrobromic acid E) 10.0 mL of 0.0500 M perchloric acid

62) Of the choices below, which one is not an ionic compound? A) PCl5 B) MoCl6 C) RbCl D) PbCl2 E) NaCl

64) A molecular formula always indicates ________. A) how many of each atom are in a molecule B) the simplest whole-number ratio of different atoms in a compound C) which atoms are attached to which in a molecule D) the isotope of each element in a compound E) the geometry of a molecule

7) Which of the following is insoluble in water at 25 °C? A) Mg3(PO4)2 B) Na2S C) (NH4)2CO3 D) Ca(OH)2 E) Ba(C2H3O2)2

7) 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

72) The species ________ contains 16 neutrons. A) 31P B) 34S2- C) 36Cl D) 80Br- E) 16O

77) Which species has 48 electrons? A) Sn+2 B) Sn+4 C) Cd+2 D) Ga E) Ti

79) Which pair of elements is most apt to form an ionic compound with each other? A) barium, bromine B) calcium, sodium C) oxygen, fluorine D) sulfur, fluorine E) nitrogen, hydrogen

8) All of the orbitals in a given electron shell have the same value as the ________ quantum number. A) principal B) angular momentum C) magnetic D) spin E) psi

8) Of the following, which one is a state function? A) H B) q C) w D) heat E) none of the above

8) When aqueous solutions of ________ are mixed, a precipitate forms. A) NiBr2 and AgNO3 B) NaI and KBr C) K2SO4 and CrCl3 D) KOH and Ba(NO3)2 E) Li2CO3 and CsI

8) Which states of matter are significantly compressible? A) gases only B) liquids only C) solids only D) liquids and gases E) solids and liquids

84) The formula for a salt is XBr. The X-ion in this salt has 46 electrons. The metal X is ________. A) Ag B) Pd C) Cd D) Cu E) Cs

88) The suffix -ide is used primarily ________. A) for monatomic anion names B) for polyatomic cation names C) for the name of the first element in a molecular compound D) to indicate binary acids E) for monoatomic cations

89) Which one of the following compounds is chromium(III) oxide? A) Cr2O3 B) CrO3 C) Cr3O2 D) Cr3O E) Cr2O4

90) Which one of the following compounds is copper(I) chloride? A) CuCl B) CuCl2 C) Cu2Cl D) Cu2Cl3 E) Cu3Cl2

94) The correct name for HNO2 is ________. A) nitrous acid B) nitric acid C) hydrogen nitrate D) hyponitrous acid E) pernitric acid

98) Which element forms an ion with the same charge as the ammonium ion? A) potassium B) chlorine C) calcium D) oxygen E) nitrogen

Atomic radius generally increases as we move __________. (a).down a group and from right to left across a period (b).up a group and from left to right across a period (c). down a group and from left to right across a period (d).there is no trend

Element M reacts with chlorine to form a compound with the formula MCl2. Element M is more reactive than magnesium and has a smaller radius than barium. This element is __________. (a). Sr (b). K (c). Na (d). Ra

For molecules with only one central atom, how many lone pairs on the central atom guarantees molecular polarity? (a). 1 (b). 2 (c).1 or 2 (d).Any number greater than 1.

How many unpaired electrons are there in the Lewis structures of a N3- ion? (a). 0 (b). 1 (c). 2 (d). 3

Lattice energy is __________. (a).the energy required to convert a mole of ionic solid into its constituent ions in the gas phase. (b).the energy given off when gaseous ions combine to form one mole of an ionic solid. (c). the energy required to produce one mole of an ionic compound from its constituent elements in their standard states (d).the sum of ionization energies of the components in an ionic solid

Of the atoms below, __________ is the least electronegative. (a). Cs (b). F (c). Si (d). Cl

Of the molecules below, which one is nonpolar? (a). BF3 (b). NF3 (c). IF3 (d). PBr3

Oxides of most nonmetals combine with water to form __________. (a).an acid (b).a base (c). water and a salt (d). water

Oxides of the active metals combine with water to form __________. (a).metal hydroxides (b).metal hydrides (c). water and a salt (d).oxygen gas

Screening by the valence electrons in atoms is __________. (a).less efficient than that by core electrons (b).more efficient than that by core electrons (c). essentially identical to that by core electrons (d).both more efficient than that by core electrons and responsible for a general increase in atomic radius going across a period.

The electron-domain geometry and the molecular geometry of a molecule of the general formula ABn will always be the same if __________. (a).there are no lone pairs on the central atom (b).there is more than one central atom (c). n is greater than four (d).the octet rule is obeyed

The first ionization energies of the elements __________ as you go from left to right across a period of the periodic table, and __________ as you go from the bottom to the top of a group in the table. (a).increase, increase (b).increase, decrease (c). decrease, increase (d).decrease, decrease

The hybridization of the carbon atom in carbon dioxide is __________. (a). sp (b). sp2 (c). sp3 (d). sp3d

The molecular geometry of the BeCl2 molecule is __________, and this molecule is __________. (a).linear, nonpolar (b).linear, polar (c). bent, nonpolar (d).bent, polar

The principal quantum number of the electrons that are lost when tungsten forms a cation is __________. (a). 6 (b). 5 (c). 4 (d). 3

There are ______ σ and _______ π bonds in the H C C H molecule. (a).3 and 2 (b).3 and 4 (c).4 and 3 (d).2 and 3

To convert from one resonance structure to another, __________. (a).only electrons can be moved (b).electrons and atoms can both be moved (c). only atoms can be moved (d).electrons must be added

What is the maximum number of double bonds that a hydrogen atom can form? (a). 0 (b). 1 (c). 2 (d). 3

Which of the following is not a characteristic of metals? (a).acidic oxides (b).low ionization energies (c). malleability (d). ductility

__________ have the lowest first ionization energies of the groups listed. (a).Alkali metals (b).Transition elements (c). Halogens (d).Alkaline earth metals

__________ is isoelectronic with argon and __________ is isoelectronic with neon. (a).C1-, F- (b).C1-, C1+ (c). F+, F- (d).Ne-, Kr+

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 proportions B) the law of constant composition C) the law of conservation of mass D) the law of conservation of energy E) none of the above

10) 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

11) A ________ ΔH corresponds to an ________ process. A) negative, endothermic B) negative, exothermic C) positive, exothermic D) zero, exothermic E) zero, endothermic

11) Which of the following are decomposition reactions? 1) CH4 (g) + O2 (g) → CO2 (g) + H2O (l) 2) CaO (s) + CO2 (g) → CaCO3 (s) 3) Mg (s) + O2 (g) → MgO (s) 4) PbCO3 (s) → PbO (s) + CO2 (g) A) 1, 2, and 3 B) 4 only C) 1, 2, 3, and 4 D) 2 and 3 E) 2, 3, and 4

12) Which one of the following is not a valid value for the magnetic quantum number of an electron in a 5d subshell? A) 2 B) 3 C) 0 D) 1 E) -1

13) In the absence of magnetic or electric fields, cathode rays ________. A) do not exist B) travel in straight lines C) cannot be detected D) become positively charged E) bend toward a light source

14) Of the three types of radioactivity characterized by Rutherford, which is/are electrically charged? A) β-rays B) α-rays and β-rays C) α-rays, β-rays, and γ-rays D) α-rays E) α-rays and γ-rays

14) Which of the following is an illustration of the law of constant composition? A) Water boils at 100 °C at 1 atm pressure. B) Water is 11% hydrogen and 89% oxygen by mass. C) Water can be separated into other substances by a chemical process. D) Water and salt have different boiling points. E) Water is a compound.

15) 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 rusting of iron

15. The molecular geometry of the left-most carbon atom in the molecule below is __________. O H || | C H | / \ / H--C O | H (a). trigonal planar (b).tetrahedral (c). trigonal bipyramidal (d). octahedral

16) An electron cannot have the quantum numbers n = ________, l = ________, ml = ________. A) 6, 1, 0 B) 3, 2, 3 C) 3, 2, -2 D) 1, 0, 0 E) 3, 2, 1

16. The molecular geometry of the right-most carbon in the molecule below is __________. O H || | C H | / \ / H--C O | H (a). T-shaped (b).trigonal planar (c). tetrahedral (d). octahedral

17) Which one of the following is an incorrect subshell notation? A) 4f B) 2d C) 3s D) 2p E) 3d

18) The formula weight of calcium nitrate (Ca(NO3)2), rounded to one decimal place, is ________ amu. A) 102.1 B) 164.0 C) 204.2 D) 150.1 E) 116.1

19) 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

19) Which one of the following is an intensive property? A) mass B) temperature C) heat content D) volume E) amount

20) Of the following, only ________ is an extensive property. A) density B) volume C) boiling point D) freezing point E) temperature

20) Which atom has the smallest number of neutrons? A) carbon-14 B) nitrogen-14 C) oxygen-16 D) fluorine-19 E) neon-20

23) The ________ orbital is degenerate with 5py in a many-electron atom. A) 5s B) 5px C) 4py D) 5dxy E) 5d2

23) The balanced reaction between aqueous potassium hydroxide and aqueous acetic acid is ________. A) KOH (aq) + HC2H3O2 (aq) → OH- (l) + HC2H3O2+ (aq) + K (s) B) KOH (aq) + HC2H3O2 (aq) → H2O (l) + KC2H3O2 (aq) C) KOH (aq) + HC2H3O2 (aq) → H2C2H3O3 (aq) + K (s) D) KOH (aq) + HC2H3O2 (aq) → KC2H3O3 (aq) + H2 (g) E) KOH (aq) + HC2H3O2 (aq) → H2KC2H3O (aq) + O2 (g)

24) Calculate the percentage by mass of nitrogen in PtCl2(NH3)2. A) 4.67 B) 9.34 C) 9.90 D) 4.95 E) 12.67

25) Which isotope has 45 neutrons? A) Kr B) Br C) Se D) Cl E) Rh

26) In which reaction does the oxidation number of hydrogen change? A) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) B) 2Na (s) + 2H2O (l) → 2NaOH (aq) + H2 (g) C) CaO (s) + H2O (l) → Ca(OH)2 (s) D) 2HClO4 (aq) + CaCO3 (s) → Ca(ClO4)2 (aq) + H2O (l) + CO2 (g) E) SO2 (g) + H2O (l) → H2SO3 (aq)

26) Which one of the following is true about the liter? A) It is the SI base unit for volume. B) It is equivalent to a cubic decimeter. C) It is slightly smaller than a quart. D) It contains 106 cubic centimeters. E) It is slightly smaller than a gallon.

26) Which pair of atoms constitutes a pair of isotopes of the same element? A) X X B) X X C) X X D) X X E) X X

29) Which electron configuration represents a violation of the Pauli exclusion principle? A) B) C) D) E)

3) A combination of sand, salt, and water is an example of a ________. A) homogeneous mixture B) heterogeneous mixture C) compound D) pure substance E) solid

30) One mole of ________ contains the largest number of atoms. A) S8 B) C10H8 C) Al2(SO4)3 D) Na3PO4 E) Cl2

32) Different isotopes of a particular element contain different numbers of ________. A) protons B) neutrons C) protons and neutrons D) protons, neutrons, and electrons E) None of the above is correct.

32) Of the reactions below, only ________ is not spontaneous. A) Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2(g) B) 2Ag (s) + 2HNO3 (aq) → 2AgNO3 (aq) + H2 (g) C) 2Ni (s) + H2SO4 (aq) → Ni2SO4 (aq) + H2 (g) D) 2Al (s) + 6HBr (aq) → 2AlBr3 (aq) + 3H2 (g) E) Zn (s) + 2HI (aq) → ZnI2(aq) + H2 (g)

32) One million argon atoms is ________ mol (rounded to two significant figures) of argon atoms. A) 3.0 B) 1.7 × 10-18 C) 6.0 × 1023 D) 1.0 × 10-6 E) 1.0 × 106

34) A 30.5 gram sample of glucose (C6H12O6) contains ________ mol of glucose. A) 0.424 B) 0.169 C) 5.90 D) 2.36 E) 0.136

34) Based on the activity series, which one of the reactions below will occur? A) Fe (s) + ZnCl2 (aq) → FeCl2 (aq) + Zn (s) B) Mn (s) + NiCl2 (aq) → MnCl2 (aq) + Ni (s) C) Pb (s) + NiI2 (aq) → PbI2 (aq) + Ni (s) D) SnBr2 (aq) + Cu (s) → CuBr2 (aq) + Sn (s) E) None of the reactions will occur.

34) In the symbol below, X = ________. X A) N B) C C) Al D) K E) not enough information to determine

34) The ground-state electron configuration of the element ________ is [Kr]5s14d5. A) Nb B) Mo C) Cr D) Mn E) Tc

35) Which of the following has the same number of significant figures as the number 1.00310? A) 1 × 106 B) 199.791 C) 8.66 D) 5.119 E) 100

36) Sodium does not occur in nature as Na (s) because ________. A) it is easily reduced to Na- B) it is easily oxidized to Na+ C) it reacts with water with great difficulty D) it is easily replaced by silver in its ores E) it undergoes a disproportionation reaction to Na- and Na+

36) Which one of the following configurations depicts an excited oxygen atom? A) 1s22s22p2 B) 1s22s22p23s2 C) 1s22s22p1 D) 1s22s22p4 E) [He]2s22p4

37) How many atoms of nitrogen are in 10 g of NH4NO3? A) 3.5 B) 1.5 × 1023 C) 3.0 × 1023 D) 1.8 E) 2

38) Gravitational forces act between objects in proportion to their ________. A) volumes B) masses C) charges D) polarizability E) densities

39) Which electron configuration represents a violation of Hund's rule for an atom in its ground state? A) B) C) D) E)

4) Aqueous solutions of a compound did not form precipitates with Cl-, Br-, I-, SO42-, CO32-, PO43-, OH-, or S2-. This highly water-soluble compound produced the foul-smelling gas H2S when the solution was acidified. This compound is ________. A) Pb(NO3)2 B) (NH4)2S C) KBr D) Li2CO3 E) AgNO3

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

40) Expressing a number in scientific notation ________. A) changes its value B) removes ambiguity as to the significant figures C) removes significant zeros D) allows to increase the number's precision E) all of the above

40) The total number of atoms in 0.111 mol of Fe(CO)3(PH3)2 is ________. A) 15.0 B) 1.00 × 1024 C) 4.46 × 1021 D) 1.67 E) 2.76 × 10-24

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. A) 219.7 B) 220.4 C) 220.42 D) 218.5 E) 221.0

42) How many significant figures should be retained in the result of the following calculation? 12.00000 × 0.9893 + 13.00335 × 0.0107 A) 2 B) 3 C) 4 D) 5 E) 6

42) The ground-state configuration of tungsten is ________. A) [Ar]4s23d3 B) [Xe]6s24f145d4 C) [Ne]3s1 D) [Xe]6s24f7 E) [Kr]5s24d105p5

42) Which of the following reactions will not occur as written? A) Zn (s) + Pb(NO3)2 (aq) → Pb (s) + Zn(NO3)2 (aq) B) Mg (s) + Ca(OH)2 (aq) → Ca (s) + Mg(OH)2 (aq) C) Sn (s) + 2AgNO3 (aq) → 2Ag (s) + Sn(NO3)2 (aq) D) Co (s) + 2AgCl (aq) → 2Ag (s) + CoCl2 (aq) E) Co (s) + 2HI (aq) → H2 (g) + CoI2 (aq)

44) Which one of the following is not true concerning 2.00 L of 0.100 M solution of Ca3(PO4)2? A) This solution contains 0.200 mol of Ca3(PO4)2. B) This solution contains 0.800 mol of oxygen atoms. C) 1.00 L of this solution is required to furnish 0.300 mol of Ca2+ ions. D) There are 6.02 × 1022 phosphorus atoms in 500.0 mL of this solution. E) This solution contains 0.600 mol of Ca2+.

45) How many moles of sodium carbonate contain 1.773 × 1017 carbon atoms? A) 5.890 × 10-7 B) 2.945 × 10-7 C) 1.473 × 10-7 D) 8.836 × 10-7 E) 9.817 × 10-8

45) Round the number 0.007222 to three significant figures. A) 0.007 B) 0.00722 C) 0.0072 D) 0.00723 E) 0.007225

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. A) 30.20 B) 33.20 C) 34.02 D) 35.22 E) 32.73

47) The compound responsible for the characteristic smell of garlic is allicin, C6H10OS2. The mass of 1.00 mol of allicin, rounded to the nearest integer, is ________ g. A) 34 B) 162 C) 86 D) 61 E) 19

5) When a system ________, ΔE is always negative. A) absorbs heat and does work B) gives off heat and does work C) absorbs heat and has work done on it D) gives off heat and has work done on it E) None of the above is always negative.

50) In the periodic table, the elements are arranged in ________. A) alphabetical order B) order of increasing atomic number C) order of increasing metallic properties D) order of increasing neutron content E) reverse alphabetical order

52) You are given two clear solutions of the same unknown monoprotic acid, but with different concentrations. Which statement is true? A) There is no chemical method designed to tell the two solutions apart. B) It would take more base solution (per milliliter of the unknown solution) to neutralize the more concentrated solution. C) A smaller volume of the less concentrated solution contains the same number of moles of the acid compared to the more concentrated solution. D) If the same volume of each sample was taken, then more base solution would be required to neutralize the one with lower concentration. E) The product of concentration and volume of the less concentrated solution equals the product of concentration and volume of the more concentrated solution.

53) 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) 94.5

55) The elements in groups 1A, 6A, and 7A are called ________, respectively. A) alkaline earth metals, halogens, and chalcogens B) alkali metals, chalcogens, and halogens C) alkali metals, halogens, and noble gases D) alkaline earth metals, transition metals, and halogens E) halogens, transition metals, and alkali metals

58) An element that appears in the lower left corner of the periodic table is ________. A) either a metal or metalloid B) definitely a metal C) either a metalloid or a nonmetal D) definitely a nonmetal E) definitely a metalloid

6) Which one of the following elements has a symbol that is not derived from its foreign name? A) tin B) aluminum C) mercury D) copper E) lead

60) Which one of the following molecular formulas is also an empirical formula? A) C6H6O2 B) C2H6SO C) H2O2 D) H2P4O6 E) C6H6

61) Which compounds do not have the same empirical formula? A) C2H2, C6H6 B) CO, CO2 C) C2H4, C3H6 D) C2H4O2, C6H12O6 E) C2H5COOCH3, CH3CHO

62) Which one of the following substances is produced during the reaction of an acid with a metal hydroxide? A) H2 B) H2O C) CO2 D) NaOH E) O2

69) Which species has 54 electrons? A) Xe+ B) Te2- C) Sn2+ D) Cd E) Xe2+

70) Which species has 16 protons? A) 31P B) 34S2- C) 36Cl D) 80Br- E) 16O

71) Which species has 18 electrons? A) 39K B) 32S2- C) 35Cl D) 27Al3+ E) 64Cu2+

76) There are ________ protons, ________ neutrons, and ________ electrons in U+5. A) 146, 92, 92 B) 92, 146, 87 C) 92, 146, 92 D) 92, 92, 87 E) 146, 92, 146

8) ________-rays consist of fast-moving electrons. A) Alpha B) Beta C) Gamma D) X E) none of the above

9) 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 Thomson's model of the atom D) utilized the deflection of beta particles by gold foil E) proved the law of multiple proportions

9) Which of the following are combination reactions? 1) CH4 (g) + O2 (g) → CO2 (g) + H2O (l) 2) CaO (s) + CO2 (g) → CaCO3 (s) 3) Mg (s) + O2 (g) → MgO (s) 4) PbCO3 (s) → PbO (s) + CO2 (g) A) 1, 2, and 3 B) 2 and 3 C) 1, 2, 3, and 4 D) 4 only E) 2, 3, and 4

99) 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

A double bond consists of __________ pairs of electrons shared between two atoms. (a). 1 (b).2 (c). 3 (d). 4

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).trigonal bipyramidal (c). tetrahedral (d).trigonal planar

According to VSEPR theory, if there are four electron domains on a central atom, they will be arranged such that the angles between the domains are __________. (a). 120° (b).109.5° (c). 180° (d). 90°

According to valence bond theory, which orbitals overlap in the formation of the bond in HBr? (a). 1s on H and 4s on Br (b).1s on H and 4p on Br (c). 1s on H and 3p on Br (d).2s on H and 4p on Br

Based on the octet rule, magnesium most likely forms a __________ ion. (a). Mg2- (b).Mg2+ (c). Mg6- (d). Mg6+

Elements from opposite sides of the periodic table tend to form __________. (a) covalent compounds (b) ionic compounds (c) ionic compounds that are gaseous at room temperature (d) homonuclear diatomic compounds

For a given arrangement of ions, the lattice energy increases as ionic radius __________ and as ionic charge __________. (a). increases, decreases (b).decreases, increases (c). increases, increases (d).decreases, decreases

For a molecule with the formula AB2 the molecular shape is __________. (a). linear or trigonal planar (b).linear or bent (c). linear or T-shaped (d). T-shaped

In order to produce sp3 hybrid orbitals, ____ s atomic orbital(s) and ____ p atomic orbitals (s) must be mixed. (a). one, two (b).one, three (c). one, one (d).two, two

Of the atoms below, __________ is the most electronegative. (a). Si (b).Br (c). Rb (d). Ca

Of the following atoms, which has the largest first ionization energy? (a). Br (b).O (c). C (d). P

The Lewis structure of PF3 shows that the central phosphorus atom has __________ nonbonding and __________ bonding electron pairs. (a). 2, 2 (b).1, 3 (c). 3, 1 (d).1, 2

The combination of two atomic orbitals results in the formation of __________ molecular orbitals. (a). 1 (b).2 (c). 3 (d). 0

The element phosphorus exists in two forms in nature called white phosphorus and red phosphorus. These two forms are examples of __________. (a). isotopes (b).allotropes (c). azeotropes (d). metrotropes

The hybridization of iodine in IF3 and IF5 are __________ and __________, respectively. (a). sp3, sp3d (b).sp3d, sp3d2 (c). sp3d, sp3 (d).sp3d2, sp3d

The hybridization of orbitals on the central atom in a molecule is sp. The electron- domain geometry around this central atom is __________. (a). octahedral (b).linear (c). trigonal planar (d). tetrahedral

The ion ICI4- has __________ valence electrons. (a). 34 (b).36 (c). 35 (d). 28

The sp2 atomic hybrid orbital set accommodates __________ electron domains. (a). 2 (b).3 (c). 4 (d). 5

Thereare______σand________π bonds in the H2C==C==CH2 molecule (a). 4, 2 (b).6, 2 (c). 2, 2 (d).2, 6

Three sulfur fluorides are observed: SF2, SF4, and SF6. Of these, __________ is/are polar. (a).SF2 only (b).SF2 and SF4 only (c).SF4 only (d).SF6 only

What is the coefficient of M when the following equation is completed and balanced if M is an alkali metal? M (s) + H2O (1) (a). 1 (b).2 (c). 3 (d). 0

When two elements combine to form a compound, the greater the difference in metallic character between the two elements, the great the likelihood that the compound will be __________. (a). a gas at room temperature (b).a solid at room temperature (c). metallic (d). nonmetallic

Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)? (a). O < F < S < Mg < Ba (b).F < O < S < Mg < Ba (c). F < O < S < Ba < Mg (d).O < F < S < Ba < Mg

Which of the following has the largest second ionization energy? (a). Ca (b).K (c). Ga (d). Ge

Which of the following is an isoelectronic series? (a). B5-, Si4-, As3-, Te2- (b).O2-, F-, Ne, Na+ (c). S, C1, Ar, K (d).None of the above

1) Of the species below, only ________ is not an electrolyte. A) HCl B) Rb2SO4 C) Ar D) KOH E) NaCl

1) What is the physical state in which matter has no specific shape but does have a specific volume? A) gas B) solid C) liquid D) salts E) ice

10) The uncertainty principle states that ________. A) matter and energy are really the same thing B) it is impossible to know anything with certainty C) it is impossible to know the exact position and momentum of an electron D) there can only be one uncertain digit in a reported number E) it is impossible to know how many electrons there are in an atom

10) Which one of the following compounds is insoluble in water? A) K2SO4 B) Ca(C2H3O2)2 C) MgC2O4 D) ZnCl2 E) Mn(NO3)2

103) What is the molecular formula for 1-propanol? A) CH4O B) C2H6O C) C3H8O D) C4H10O E) C5H12O

11) An element cannot ________. A) be part of a heterogeneous mixture B) be part of a homogeneous mixture C) be separated into other substances by chemical means D) interact with other elements to form compounds E) be a pure substance

11) Cathode rays are ________. A) neutrons B) X-rays C) electrons D) protons E) atoms

12) A ________ ΔH corresponds to an ________ process. A) negative, endothermic B) positive, exothermic C) positive, endothermic D) zero, exothermic E) zero, endothermic

14) The formula weight of silver chromate (Ag2CrO4) is ________ amu. A) 159.87 B) 223.87 C) 331.73 D) 339.86 E) 175.87

15) Of the three types of radioactivity characterized by Rutherford, which is/are not electrically charged? A) α-rays B) α-rays, β-rays, and γ-rays C) γ-rays D) α-rays and β-rays E) α-rays and γ-rays

16) The net ionic equation for the reaction between aqueous nitric acid and aqueous sodium hydroxide is ________. A) H+ (aq) + HNO3 (aq) + 2OH- (aq) → 2H2O (l) + NO3- (aq) B) HNO3 (aq) + NaOH (aq) → NaNO3 (aq) + H2O (l) C) H+ (aq) + OH- (aq) → H2O (l) D) HNO3 (aq) + OH- (aq) → NO3- (aq) + H2O (l) E) H+ (aq) + Na+ (aq) + OH- (aq) → H2O (l) + Na+ (aq)

16. Given the electronegativities below, which covalent single bond is most polar? Atom H C N O Electronegativity 2.1 2.5 3.0 3.5 (a). C-H (b). N-H (c). O-H (d). O-N

17) Of the following, only ________ is a chemical reaction. A) melting of lead B) dissolving sugar in water C) tarnishing of silver D) crushing of stone E) dropping a penny into a glass of water

18) Of the following, the smallest and lightest subatomic particle is the ________. A) neutron B) proton C) electron D) nucleus E) alpha particle

18) Which one of the following is an incorrect orbital notation? A) 2s B) 3py C) 3f D) 4dxy E) 4s

19) The formula weight of magnesium fluoride (MgF2), rounded to one decimal place, is ________ amu. A) 86.6 B) 43.3 C) 62.3 D) 67.6 E) 92.9

19) Which one of the following is a triprotic acid? A) nitric acid B) chloric acid C) phosphoric acid D) hydrofluoric acid E) sulfuric acid

2) The law of constant composition applies to ________. A) solutions B) heterogeneous mixtures C) compounds D) homogeneous mixtures E) solids

21) The mass % of C in methane (CH4) is ________. A) 25.13 B) 133.6 C) 74.87 D) 92.26 E) 7.743

21) 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, 3, 4 C) 1, 3 D) 1, 2 E) 1, 4

22) 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) NH4+ B) K+ C) Cr3+ D) Rb+ E) Na+

25) Calculate the percentage by mass of lead in Pb(NO3)2. A) 38.6 B) 44.5 C) 62.6 D) 65.3 E) 71.2

25) Which of the following is (are) the lowest temperature? A) The freezing point of water B) 5 °C C) 30 °F D) 280 K E) A and D

27) Which compound has the atom with the highest oxidation number? A) CaS B) Na3N C) MgSO3 D) Al(NO2)3 E) NH4Cl

28) Isotopes are atoms that have the same ________ but differing ________. A) atomic masses, charges B) mass numbers, atomic numbers C) atomic numbers, mass numbers D) charges, atomic masses E) mass numbers, charges

28) Which electron configuration represents a violation of the Pauli exclusion principle? A) B) C) D) E)

29) Which of these metals will be oxidized by the ions of cobalt? A) nickel B) tin C) iron D) copper E) silver

3) Aqueous potassium chloride will react with which one of the following in an exchange (metathesis) reaction? A) calcium nitrate B) sodium bromide C) lead nitrate D) barium nitrate E) sodium chloride

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) only C) (ii) and (iii) D) (iii) only E) (iii) and (iv)

3) The photoelectric effect is ________. A) the total reflection of light by metals giving them their typical luster B) the production of current by silicon solar cells when exposed to sunlight C) the ejection of electrons by a metal when struck with light of sufficient energy D) the darkening of photographic film when exposed to an electric field E) a relativistic effect

30) The subatomic particles located in the nucleus with no overall charges are ________. A) electrons B) protons C) neutrons D) protons and neutrons E) protons, neutrons, and electrons

30) Which electron configuration represents a violation of the Pauli exclusion principle? A) B) C) D) E)

32) Iron has a density of 7.9 g/cm3. What is the mass of a cube of iron with the length of one side equal to 55.0 mm? A) 2.1 × 104 g B) 4.3 × 102 g C) 1.3 × 103 g D) 1.4 g E) 2.3 × 10-2 g

33) Based on the activity series, which one of the reactions below will occur? A) Zn (s) + MnI2 (aq) → ZnI2 (aq) + Mn (s) B) SnCl2 (aq) + Cu (s) → Sn (s) + CuCl2 (aq) C) 2AgNO3 (aq) + Pb (s) → 2Ag (s) + Pb(NO3)2 (aq) D) 3Hg (l) + 2Cr(NO3)3 (aq) → 3Hg(NO3)2 + 2Cr (s) E) 3FeBr2 (aq) + 2Au (s) → 3Fe (s) + 2AuBr3 (aq)

33) The ground state electron configuration of Ga is ________. A) 1s22s23s23p64s23d104p1 B) 1s22s22p63s23p64s24d104p1 C) 1s22s22p63s23p64s23d104p1 D) 1s22s22p63s23p64s23d104d1 E) [Ar]4s23d11

36) In the symbol below, x is ________. C A) the number of neutrons B) the atomic number C) the mass number D) the isotope number E) the elemental symbol

37) Zinc is more active than cobalt and iron but less active than aluminum. Cobalt is more active than nickel but less active than iron. Which of the following correctly lists the elements in order of increasing activity? A) Co < Ni < Fe < Zn < Al B) Ni < Fe < Co < Zn < Al C) Ni < Co < Fe < Zn < Al D) Fe < Ni < Co < Al < Zn E) Zn < Al < Co < Ni < Fe

38) Gaseous argon has a density of 1.40 g/L at standard conditions. How many argon atoms are in 1.00 L of argon gas at standard conditions? A) 4.76 × 1022 B) 3.43 × 1025 C) 2.11 × 1022 D) 1.59 × 1025 E) 6.02 × 1023

38) Oxidation is the ________ and reduction is the ________. A) gain of oxygen, loss of electrons B) loss of oxygen, gain of electrons C) loss of electrons, gain of electrons D) gain of oxygen, loss of mass E) gain of electrons, loss of electrons

38) Which electron configuration represents a violation of Hund's rule for an atom in its ground state? A) B) C) D) E)

39) Silver has two naturally occurring isotopes with the following isotopic masses: Ar Ar 106.90509 108.9047 The average atomic mass of silver is 107.8682 amu. The fractional abundance of the lighter of the two isotopes is ________. A) 0.24221 B) 0.48168 C) 0.51835 D) 0.75783 E) 0.90474

4) Which one of the following is considered to be ionizing radiation? A) visible light B) radio waves C) X-rays D) microwaves E) infrared radiation

41) The number with the most significant zeros is ________. A) 0.00002510 B) 0.02500001 C) 250000001 D) 2.501 × 10-7 E) 2.5100000

43) How many carbon atoms are there in 52.06 g of carbon dioxide? A) 5.206 × 1024 B) 3.134 × 1025 C) 7.122 × 1023 D) 8.648 × 10-23 E) 1.424 × 1024

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. A) 161.75 B) 162.03 C) 162.35 D) 163.15 E) 33.33

43) Which one of the following is a correct expression for molarity? A) mol solute/L solvent B) mol solute/mL solvent C) mmol solute/mL solution D) mol solute/kg solvent E) μmol solute/L solution

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. A) 33.33 B) 55.74 C) 56.11 D) 57.23 E) 56.29

44) Which of the following is not an exact number? A) the number of seconds in a year B) the number of millimeters in a kilometer C) the number of liters in a gallon D) the number of centimeters in an inch E) the number of grams in a kilogram

45) A 0.200 M K2SO4 solution is produced by ________. A) dilution of 250.0 mL of 1.00 M K2SO4 to 1.00 L B) dissolving 43.6 g of K2SO4 in water and diluting to a total volume of 250.0 mL C) diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL D) dissolving 20.2 g of K2SO4 in water and diluting to 250.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mL E) dilution of 1.00 mL of 250 M K2SO3 to 1.00 L

46) How many different principal quantum numbers can be found in the ground-state electron configuration of nickel? A) 2 B) 3 C) 4 D) 5 E) 6

47) Which solution has the same number of moles of KCl as 75.00 mL of 0.250 M solution of KCl? A) 20.0 mL of 0.200 M solution of KCl B) 25.0 mL of 0.175 M solution of KCl C) 129 mL of 0.145 M solution of KCl D) 50.0 mL of 0.125 M solution of KCl E) 100 mL of 0.0500 M solution of KCl

48) The molecular formula of aspartame, the generic name of NutraSweet®, is C14H18N2O5. The molar mass of aspartame, rounded to the nearest integer, is ________ g. A) 24 B) 156 C) 294 D) 43 E) 39

5) Of the following transitions in the Bohr hydrogen atom, the ________ transition results in the emission of the lowest-energy photon. A) n = 1 → n = 6 B) n = 6 → n = 1 C) n = 6 → n = 3 D) n = 3 → n = 6 E) n = 1 → n = 4

5) The net ionic equation for formation of an aqueous solution of NiI2 accompanied by evolution of CO2 gas via mixing solid NiCO3 and aqueous hydriodic acid is ________. A) 2NiCO3 (s) + HI (aq) → 2H2O (l) + CO2 (g) + 2Ni2+ (aq) B) NiCO3 (s) + I- (aq) → 2H2O (l) + CO2 (g) + Ni2+ (aq) + HI (aq) C) NiCO3 (s) + 2H+ (aq) → H2O (l) + CO2 (g) + Ni2+ (aq) D) NiCO3 (s) + 2HI (aq) → 2H2O (l) + CO2 (g) + NiI2 (aq) E) NiCO3 (s) + 2HI (aq) → H2O (l) + CO2 (g) + Ni2+ (aq) + 2I- (aq)

5) Which one of the following has the element name and symbol correctly matched? A) S, sodium B) Tn, tin C) Fe, iron D) N, neon E) B, bromine

50) A nitrogen oxide is 63.65% by mass nitrogen. The molecular formula could be ________. A) NO B) NO2 C) N2O D) N2O4 E) either NO2 or N2O4

51) Mixing 10.00 mL of an aqueous solution with 10.00 mL of water represents a ________. A) crystallization B) neutralization C) twofold dilution D) tenfold dilution E) titration

52) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? A) H, Li B) Cs, Ba C) Ca, Sr D) Ga, Ge E) C, O

54) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? A) As, Br B) Mg, Al C) I, At D) Br, Kr E) N,O

54) Which solution contains the largest number of moles of chloride ions? A) 10.0 mL of 0.500 M BaCl2 B) 4.00 mL of 1.000 M NaCl C) 7.50 mL of 0.500 M FeCl3 D) 25.00 mL of 0.400 M KCl E) 30.00 mL of 0.100 M CaCl2

56) Which pair of elements below should be the most similar in chemical properties? A) C and O B) B and As C) I and Br D) K and Kr E) Cs and He

58) What volume (L) of 0.250 M HNO3 is required to neutralize a solution prepared by dissolving 17.5 g of NaOH in 350 mL of water? A) 50.0 B) 0.44 C) 1.75 D) 0.070 E) 1.75 ×

6) In the Bohr model of the atom, ________. A) electrons travel in circular paths called orbitals B) electrons can have any energy C) electron energies are quantized D) electron paths are controlled by probability E) both A and C

6) Which one of the following substances is the product of this combination reaction? Al (s) + I2 (s) → ________ A) AlI2 B) AlI C) AlI3 D) Al2I3 E) Al3I2

64) ________ is an oxidation reaction. A) Ice melting in a soft drink B) Table salt dissolving in water for cooking vegetables C) Rusting of iron D) The reaction of sodium chloride with lead nitrate to form lead chloride and sodium nitrate E) Neutralization of HCl by NaOH

65) An empirical formula always indicates ________. A) which atoms are attached to which in a molecule B) how many of each atom are in a molecule C) the simplest whole-number ratio of different atoms in a compound D) the isotope of each element in a compound E) the geometry of a molecule

66) The molecular formula of a compound is always ________ the empirical formula. A) more complex than B) different from C) an integral multiple of D) the same as E) simpler than

7) According to the Heisenberg Uncertainty Principle, it is impossible to know precisely both the position and the ________ of an electron. A) mass B) color C) momentum D) shape E) charge

7) The charge on an electron was determined in the ________. A) cathode ray tube, by J. J. Thomson B) Rutherford gold foil experiment C) Millikan oil drop experiment D) Dalton atomic theory E) atomic theory of matter

7) Which one of the following is not true concerning automotive air bags? A) They are inflated as a result of a decomposition reaction. B) They are loaded with sodium azide initially. C) The gas used for inflating them is oxygen. D) The two products of the decomposition reaction are sodium and nitrogen. E) A gas is produced when the air bag activates.

73) Which species is an isotope of 39Cl? A) 40Ar+ B) 34S2- C) 36Cl- D) 80Br E) 39Ar

75) There are ________ protons, ________ neutrons, and ________ electrons in I-. A) 131, 53, 54 B) 131, 53, 52 C) 53, 78, 54 D) 53, 131, 52 E) 78, 53, 72

78) Which of the following compounds would you expect to be ionic? A) H2O B) CO2 C) SrCl2 D) SO2 E) H2S

80) Which pair of elements is most apt to form a molecular compound with each other? A) aluminum, oxygen B) magnesium, iodine C) sulfur, fluorine D) potassium, lithium E) barium, bromine

9) 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

9) The de Broglie wavelength of a ________ will have the shortest wavelength when traveling at 30 cm/s. A) marble B) car C) planet D) uranium atom E) hydrogen atom

93) A correct name for Fe(NO3)2 is ________. A) iron nitrite B) ferrous nitrite C) ferrous nitrate D) ferric nitrite E) ferric nitrate

97) Which one of the following polyatomic ions has the same charge as the hydroxide ion? A) ammonium B) carbonate C) nitrate D) sulfate E) phosphate

Chlorine is much more apt to exist as an anion than is sodium. This is because __________. (a). chlorine is bigger than sodium (b).chlorine has a greater ionization energy than sodium does (c). chlorine has a greater electron affinity than sodium does (d).chlorine is a gas and sodium is a solid

For molecules of the general formula ABn, n can be greater than four _________. (a). for any element A (b).only when A is boron or beryllium (c). only when A is an element from the third period or below the third period (d).only when A is Kr

For resonance forms of a molecule or ion, __________. (a). one always corresponds to the observed structure (b).all the resonance structures are observed in various proportions (c). the observed structure is an average of the resonance forms (d).the same atoms need not be bonded to each other in all resonance forms

In counting the electron domains around the central atom in VSEPR theory, a __________ is not included. (a). nonbonding pair of electrons (b).single covalent bond (c). core level electron pair (d).double covalent bond

Metals can be __________ at room temperature. (a). liquid only (b).solid only (c). solid or liquid (d).solid, liquid, or gas

Oxides of the active metals combine with acids to form __________. (a). hydrogen gas (b).metal hydrides (c). water and a salt (d).oxygen gas

The Cl-C-Cl bond angle in the CCl2O molecule (C is the central atom) is slightly __________. (a). greater than 109.5° (b).less than 109.5° (c). less than 120° (d).greater than 120°

The __________ have the most negative electron affinities (a). alkaline earth metals (b).alkali metals (c). halogens (d).transition metals

The ability of an atom in a molecule to attract electrons is best quantified by the __________. (a). paramagnetism (b). diamagnetism (c). electronegativity (d).electron affinity

The electron-domain geometry and molecular geometry of iodine trichloride are __________ and __________ respectively. (a). trigonal bipyramidal, trigonal planar (b).tetrahedral, trigonal pyramidal (c). trigonal bipyramidal, T-shaped (d).octahedral, trigonal planar

The electron-domain geometry and the molecular geometry of a molecule of the general formula ABn are __________. (a). never the same (b).always the same (c). sometimes the same (d).not related to each other

The electron-domain geometry of a sulfur-centered compound is trigonal bipyramidal. The hybridization of the central sulfur atom is __________. (a). sp (b). sp2 (c). sp3d (d). sp3

The hybridization of orbitals on the central atom in a molecule is sp2. The electron- domain geometry about this central atom is __________. (a). tetrahedral (b). linear (c). trigonal planar (d).trigonal bipyramidal

The only noble gas that does not have the ns2np6 valence electron configuration is __________. (a). radon (b). neon (c). helium (d). krypton

The only noble gas without eight valence electrons is __________. (a). Ar (b). Ne (c). He (d). Kr

The oxide of which element below can react with hydrochloric acid? (a). sulfur (b). selenium (c). sodium (d). nitrogen

The sp3d2 atomic hybrid orbital set accommodates __________ electron domains. (a). 2 (b). 3 (c). 6 (d). 5

The type of compound that is most likely to contain a covalent bond is __________. (a). one that is composed of a metal from the far left of the periodic table and a nonmental from the far right of the periodic table (b).a solid metal (c). one that is composed of only nonmetals (d).held together by the electrostatic forces between oppositely charged ions

What is the maximum number of double bonds that a carbon atom can form? (a). 4 (b). 1 (c). 2 (d). 0

Which ion below has the largest radius? (a). C1- (b). K+ (c). Br- (d). F-

Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration __________? O Sr Na Se Br (a). O, Se (b). Na (c). Sr (d). As

Which of the molecules has a see-saw shape? (i) PCl3 (ii) CCl4 (iii) TeCl4 (iv) XeF4 (v) SF6 (a). (i) only (b).(ii) only (c). (iii) only (d).(iv) only

_______ is a unique element and does not truly belong to any family. A) Nitrogen B) Radium C) Hydrogen D) Helium

10) The internal energy can be increased by ________. (a) transferring heat from the surroundings to the system (b) transferring heat from the system to the surroundings (c) doing work on the system A) a only B) b only C) c only D) a and c E) b and c

102) The correct name for Ni(CN)2 is ________. A) nickel (I) cyanide B) nickel cyanate C) nickel carbonate D) nickel (II) cyanide E) nickel (I) nitride

11) All of the orbitals in a given subshell have the same value as the ________ quantum number. A) principal B) angular momentum C) magnetic D) A and B E) B and C

11) Which combination will produce a precipitate? A) NaC2H3O2 (aq) and HCl (aq) B) NaOH (aq) and HCl (aq) C) AgNO3(aq) and Ca(C2H3O2)2 (aq) D) KOH (aq) and Mg(NO3)2 (aq) E) NaF (aq) and HCl (aq)

12) Cathode rays are deflected away from a negatively charged plate because ________. A) they are not particles B) they are positively charged particles C) they are neutral particles D) they are negatively charged particles E) they are emitted by all matter

12) The formula of nitrobenzene is C6H5NO2. The molecular weight of this compound is ________ amu. A) 107.11 B) 43.03 C) 109.10 D) 123.11 E) 3.06

13) The formula weight of potassium dichromate (K2Cr2O7 ) is ________ amu. A) 107.09 B) 255.08 C) 242.18 D) 294.18 E) 333.08

15) An electron cannot have the quantum numbers n = ________, l = ________, ml = ________. A) 2, 0, 0 B) 2, 1, -1 C) 3, 1, -1 D) 1, 1, 1 E) 3, 2, 1

15) The formula weight of ammonium sulfate ((NH4)2SO4), rounded to the nearest integer, is ________ amu. A) 100 B) 118 C) 116 D) 132 E) 264

15) The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is ________. A) H+ (aq) + HSO4- (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq) B) H+ (aq) + HSO4- (aq) + 2Na+ (aq) + 2OH- (aq) → 2H2O (l) + 2Na+ (aq) + SO42-(aq) C) SO42- (aq) + 2Na+ (aq) → 2Na+ (aq) + SO42-(aq) D) H+ (aq) + OH- (aq) → H2O( l) E) 2H+ (aq) + SO42- (aq) + 2Na+ (aq) + 2OH- (aq) → 2H2O (l) + 2Na+ (aq) + SO42- (aq)

16) Gases and liquids share the property of ________. A) compressibility B) definite volume C) incompressibility D) indefinite shape E) definite shape

17) Of the three types of radioactivity characterized by Rutherford, which type does not become deflected by a magnetic field? A) β-rays B) α-rays and β-rays C) α-rays D) γ-rays E) α-rays, β-rays, and γ-rays

17) 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

17) The reaction between strontium hydroxide and chloric acid produces ________. A) a molecular compound and a weak electrolyte B) two weak electrolytes C) two strong electrolytes D) a molecular compound and a strong electrolyte E) two molecular compounds

18) Which one of the following is not an intensive property? A) density B) temperature C) melting point D) mass E) boiling point

20) The formula weight of lead nitrate (Pb(NO3)2) is ________ amu. A) 269.2 B) 285.2 C) 317.2 D) 331.2 E) 538.4

20) Which one of the following is a weak acid? A) HNO3 B) HCl C) HI D) HF E) HClO4

20) Which one of the quantum numbers does not result from the solution of the Schrodinger equation? A) principal B) azimuthal C) magnetic D) spin E) angular momentum

21) Which atom has the largest number of neutrons? A) phosphorus-30 B) chlorine-37 C) potassium-39 D) argon-40 E) calcium-40

21) Which of the following are weak acids? A) HF, HBr B) HI, HNO3, HBr C) HI, HF D) HF E) none of the above

22) In the following list, only ________ is not an example of a chemical reaction. A) burning a plastic water bottle B) the production of hydrogen gas from water C) the tarnishing of a copper penny D) chopping a log into sawdust E) charging a cellular phone

22) There are ________ electrons, ________ protons, and ________ neutrons in an atom of Xe. A) 132, 132, 54 B) 54, 54, 132 C) 78, 78, 54 D) 54, 54, 78 E) 78, 78, 132

24) The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is ________. A) HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + H2 (g) B) HNO3 (aq) + Sr(OH)2 (aq) → H2O (l) + Sr(NO3)2 (aq) C) HNO3 (aq) + SrOH (aq) → H2O (l) + SrNO3 (aq) D) 2HNO3 (aq) + Sr(OH)2 (aq) → 2H2O (l) + Sr(NO3)2 (aq) E) 2HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2(aq) + 2H2 (g)

24) Which one of the following orbitals can hold two electrons? A) 2px B) 3s C) 4dxy D) all of the above E) none of the above

26) Calculate the percentage by mass of lead in PbCO3. A) 17.96 B) 22.46 C) 73.05 D) 77.54 E) 89.22

27) Calculate the percentage by mass of oxygen in Pb(NO3)2. A) 9.7 B) 14.5 C) 19.3 D) 29.0 E) 33.4

27) Of the objects below, ________ is the most dense. A) an object with a volume of 2.5 L and a mass of 12.5 kg B) an object with a volume of 139 mL and a mass of 93 g C) an object with a volume of 0.00212 m3 and a mass of 4.22 × 104 mg D) an object with a volume of 3.91 × 10-24 nm3 and a mass of 7.93 × 10-1 ng E) an object with a volume of 13 dm3 and a mass of 1.29 × 103 g

3) The internal energy of a system ________. A) is the sum of the kinetic energy of all of its components B) is the sum of the rotational, vibrational, and translational energies of all of its components C) refers only to the energies of the nuclei of the atoms of the component molecules D) is the sum of the potential and kinetic energies of the components E) none of the above

31) Which one of the following is the correct electron configuration for a ground-state nitrogen atom? A) B) C) D) E) None of the above is correct.

32) Which electron configuration denotes an atom in its ground state? A) B) C) D) E)

33) How many molecules of CH4 are in 48.2 g of this compound? A) 5.00 × 1024 B) 3.00 C) 2.90 × 1025 D) 1.81 × 1024 E) 4.00

33) In the symbol shown below, x = ________. C A) 7 B) 13 C) 12 D) 6 E) not enough information to determine

34) 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 the true value E) how close a measured number is to infinity

35) A sample of CH2F2 with a mass of 19 g contains ________ atoms of F. A) 2.2 × 1023 B) 38 C) 3.3 × 1024 D) 4.4 ×1023 E) 9.5

35) The ground-state electron configuration of ________ is [Ar]4s13d5. A) V B) Mn C) Fe D) Cr E) K

35) The net ionic equation for the dissolution of zinc metal in aqueous hydrobromic acid is ________. A) Zn (s) + 2Br- (aq) → ZnBr2 (aq) B) Zn (s) + 2HBr (aq) → ZnBr2 (aq) + 2H+ (aq) C) Zn (s) + 2HBr (aq) → ZnBr2 (s) + 2H+ (aq) D) Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g) E) 2Zn (s) + H+ (aq) → 2Zn2+ (aq) + H2 (g)

36) A sample of CH4O with a mass of 32.0 g contains ________ molecules of CH4O. A) 5.32 × 10-23 B) 1.00 C) 1.88 × 1022 D) 6.02 × 1023 E) 32.0

37) Which one of the following basic forces is so small that it has no chemical significance? A) weak nuclear force B) strong nuclear force C) electromagnetism D) gravity E) Coulomb's law

38) If an object is accelerating at a rate of 25 m/s2, how fast will it be moving (in m/s) after 1.50 min? (Assume an initial velocity of zero.) A) 17 B) 3.6 C) 38 D) 2.3 × 103 E) 0.060

39) A wooden object has a mass of 10.782 g and occupies a volume of 13.72 mL. What is the density of the object determined to an appropriate number of significant figures? A) 8 × 10-1 g/mL B) 7.9 × 10-1 g/mL C) 7.86 × 10-1 g/mL D) 7.859 × 10-1 g/mL E) 7.8586 × 10-1 g/mL

39) How many oxygen atoms are contained in 2.74 g of Al2(SO4)3? A) 12 B) 6.02 × 1023 C) 7.22 × 1024 D) 5.79 × 1022 E) 8.01 × 10-3

4) When a hydrocarbon burns in air, a component produced is ________. A) oxygen B) nitrogen C) carbon D) water E) argon

4) Which one of the following conditions would always result in an increase in the internal energy of a system? A) The system loses heat and does work on the surroundings. B) The system gains heat and does work on the surroundings. C) The system loses heat and has work done on it by the surroundings. D) The system gains heat and has work done on it by the surroundings. E) None of the above is correct.

40) The atomic mass unit is presently based on assigning an exact integral mass (in amu) to an isotope of ________. A) hydrogen B) oxygen C) sodium D) carbon E) helium

40) Which electron configuration represents a violation of Hund's rule for an atom in its ground state? A) B) C) D) E)

41) How many sulfur dioxide molecules are there in 1.80 mol of sulfur dioxide? A) 1.08 × 1023 B) 6.02 × 1024 C) 1.80 × 1024 D) 1.08 × 1024 E) 6.02 × 1023

41) The ground-state configuration of fluorine is ________. A) [He]2s22p2 B) [He]2s22p3 C) [He]2s22p4 D) [He]22s22p5 E) [He]2s22p6

46) Round the number 3456.5 to two significant figures. A) 3400.0 B) 3400 C) 3000 D) 3500 E) 3000.0

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) 63.2 B) 63.8 C) 64.1 D) 64.8 E) 28.1

47) The valence shell of the element X contains 2 electrons in a 5s subshell. Below that shell, element X has a partially filled 4d subshell. What type of element is X? A) main group element B) chalcogen C) halogen D) transition metal E) alkali metal

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.

52) Which hydrocarbon pair below has identical mass percentage of C? A) C3H4 and C3H6 B) C2H4 and C3H4 C) C2H4 and C4H2 D) C2H4 and C3H6 E) none of the above

55) What volume (mL) of a concentrated solution of magnesium chloride (9.00 M) must be diluted to 350. mL to make a 2.75 M solution of magnesium chloride? A) 2.75 B) 50.0 C) 45.0 D) 107 E) 350

56) 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? A) 2.64 B) 176 C) 26.4 D) 29.3 E) 50.0

57) An element in the upper right corner of the periodic table ________. A) is either a metal or metalloid B) is definitely a metal C) is either a metalloid or a nonmetal D) is definitely a nonmetal E) is definitely a metalloid

59) An aliquot (28.7 mL) of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization. What mass (g) of KOH was in the original sample? A) 1.64 B) 7.28 C) 0.173 D) 0.207 E) 0.414

6) The net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and aqueous nitric acid is ________. A) Al(OH)3 (s) + 3HNO3 (aq) → 3H2O (l) + Al(NO3)3 (aq) B) Al(OH)3 (s) + 3NO3- (aq) → 3OH- (aq) + Al(NO3)3 (aq) C) Al(OH)3 (s) + 3NO3- (aq) → 3OH- (aq) + Al(NO3)3 (s) D) Al(OH)3 (s) + 3H+ (aq) → 3H2O (l) + Al3+ (aq) E) Al(OH)3 (s) + 3HNO3 (aq) → 3H2O (l) + Al3+ (aq) + NO3- (aq)

60) The point in a titration at which the indicator changes is called the ________. A) setpoint B) indicator point C) standard point D) end point E) volumetric point

63) Which type of formula provides the most information about a compound? A) empirical B) molecular C) simplest D) structural E) chemical

68) Of the following, ________ contains the greatest number of electrons. A) P3+ B) P C) P2- D) P3- E) P2+

7) Which one of the following is an exothermic process? A) ice melting B) water evaporating C) boiling soup D) condensation of water vapor E) Ammonium thiocyanate and barium hydroxide are mixed at 25 °C: the temperature drops.

74) Which one of the following species has as many electrons as it has neutrons? A) 1H B) 40Ca2+ C) 14C D) 19F- E) 14C2+

82) 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) NaX B) Na2X C) Na2X2 D) Na3X E) Na3X2

83) 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) 3A B) 4A C) 5A D) 6A E) 7A

85) Which formula/name pair is incorrect? A) Mn(NO2)2 manganese(II) nitrite B) Mg(NO3)2 magnesium nitrate C) Mn(NO3)2 manganese(II) nitrate D) Mg3N2 magnesium nitrite E) Mg(MnO4)2 magnesium permanganate

87) Which one of the following is the formula of hydrochloric acid? A) HClO3 B) HClO4 C) HClO D) HCl E) HClO2

9) Which of the following is a statement of the first law of thermodynamics? A) Ek = m B) A negative ΔH corresponds to an exothermic process. C) ΔE = Efinal - Einitial D) Energy lost by the system must be gained by the surroundings. E) 1 cal = 4.184 J (exactly)

9) Which one of the following compounds is insoluble in water? A) Na2CO3 B) K2SO4 C) Fe(NO3)3 D) ZnS E) AgNO3

92) The correct name for NaHCO3 is ________. A) sodium hydride B) persodium carbonate C) persodium hydroxide D) sodium bicarbonate E) carbonic acid

95) The proper formula for the hydronium ion is ________. A) H- B) OH- C) N3- D) H3O+ E) NH4+

A __________ covalent bond between the same two atoms is the longest. (a). They are all the same length. (b). double (c). triple (d).single

According to VSEPR theory, if there are three electron domains on a central atom, they will be arranged such that the angles between the domains are __________. (a). 90° (b). 180° (c). 109.5° (d).120°

According to valence bond theory, which orbitals on bromine atoms overlap in the formation of the bond in Br2? (a). 3s (b). 3p (c). 4s (d).4p

An electron domain consists of __________ (a). a nonbonding pair of electrons (b). a single bond (c). a multiple bond (a). a and b only (b).b and c only (c). a and c only (d).a, b, and c

As the number of covalent bonds between two atoms increases, the distance between the atoms __________ and the strength of the bond between them __________. (a). increases, increases (b).decreases, decreases (c). increases, decreases (d).decreases, increases

Based on the octet rule, phosphorus most likely forms a __________ ion. (a). P3+ (b). P5- (c). P5+ (d).P3-

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group. (a). decreases, increases (b).increases, increases (c). stays the same, increases (d).increases, decreases

Elements in the modern version of the periodic table are arranged in order of increasing __________. (a). oxidation number (b).atomic mass (c). average atomic mass (d).atomic number

In which of the molecules does the central atom utilize d orbitals to form hybrid orbitals? (i) PCl3 (ii) CCl4 (iii) TeCl4 (iv) XeF4 (v) SF6 (a). (i) and (ii) (b).(iii) only (c). (i) and (v) (d).(iii), (iv), and (v)

Na reacts with element X to form an ionic compound with the formula Na3X. Ca will react with X to form __________. (a). CaX2 (b). CaX (c). Ca2X3 (d).Ca3X2

Of the following elements, which has the largest first ionization energy? (a). Na (b). A1 (c). Se (d).C1

Of the halogens, which are gases at room temperature and atmospheric pressure? (a). fluorine, bromine, and iodine (b).fluorine, chlorine, and bromine (c). fluorine, chlorine, bromine, and iodine (d).fluorine and chlorine

Of the hydrogen halides, only __________ is a weak acid. (a). HC1 (aq) (b).HBr (aq) (c). HI (aq) (d).HF (aq)

Of the molecules below, only __________ is polar. (a). CCl4 (b). CH4 (c). SiCl4 (d).SeF4

Of the possible bonds between carbon atoms (single, double, and triple), __________. (a). a triple bond is longer than a single bond (b).a double bond is stronger than a triple bond (c). a single bond is stronger than a triple bond (d).a double bond is longer than a triple bond

Resonance structures differ by __________. (a). number and placement of electrons (b).number of electrons only (c). placement of atoms only (d).placement of electrons only

The Lewis structure of HCN (H bonded to C) shows that __________ has __________ nonbonding electron pairs. (a). C, 1 (b).N, 2 (c). H, 1 (d).N, 1

The O-C-O bond angle in the CO32- ion is approximately __________. (a). 90° (b). 109.5° (c). 180° (d).120o

The atomic radius of main-group elements generally increases down a group because __________. (a). effective nuclear charge increases down a group (b).effective nuclear charge decreases down a group (c). both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases (d).the principal quantum number of the valence orbitals increases

The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively. (a).7, 4, and 6 (b).1, 5, and 7 (c).8, 2, and 3 (d).7, 1, and 2

The hybridizations of bromine in BrF5 and of arsenic in AsF5 are __________ and __________, respectively. (a). sp3, sp3d (b).sp3d, sp3d2 (c). sp3d, sp3 (d).sp3d2, sp3d

The ion with the smallest radius is __________. (a). Br- (b). C1- (c). O2- (d).F-

There are __________ paired and __________ unpaired electrons in the Lewis symbol for a phosphorus atom. (a). 4, 2 (b).2, 4 (c). 4, 3 (d).2, 3

Which equation correctly represents the first ionization of aluminum? (a). Al- (g) ➡️ Al (g) + e- (b).Al (g) ➡️ Al - (g) + e- (c).Al(g) + e- ➡️ Al- (g) (d).Al (g) ➡️ Al + (g) + e-

Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)? (a). F < K < Ge < Br < Rb (b).F < Ge < Br < K < Rb (c). F < K < Br < Ge < Rb (d).F < Br < Ge < K < Rb

Which of the following has the largest second ionization energy? (a). Si (b). Mg (c). A1 (d).Na

1) Objects can possess energy as ________. (a) endothermic energy (b) potential energy (c) kinetic energy A) a only B) b only C) c only D) a and c E) b and c

1) When the following equation is balanced, the coefficients are ________. C8H18 + O2 → CO2 + H2O A) 2, 3, 4, 4 B) 1, 4, 8, 9 C) 2, 12, 8, 9 D) 4, 4, 32, 36 E) 2, 25, 16, 18

1) Which one of the following is correct? A) ν + λ = c B) ν ÷ λ = c C) ν = cλ D) λ = c ν E) νλ = c

101) Which metal forms cations of differing charges? A) K B) Cs C) Ba D) Al E) Sn

12) Homogeneous mixtures are also known as ________. A) solids B) compounds C) elements D) substances E) solutions

12) Which combination will produce a precipitate? A) NH4OH (aq) and HCl (aq) B) AgNO3 (aq) and Ca(C2H3O2)2 (aq) C) NaOH (aq) and HCl (aq) D) NaCl (aq) and HC2H3O2 (aq) E) NaOH (aq) and Fe(NO3)2 (aq)

13) ΔH for an endothermic process is ________ while ΔH for an exothermic process is ________. A) zero, positive B) zero, negative C) positive, zero D) negative, positive E) positive, negative

14) Which of the subshells below do not exist due to the constraints upon the angular momentum quantum number? A) 4f B) 4d C) 4p D) 4s E) none of the above

14) With which of the following will the ammonium ion form an insoluble salt? A) chloride B) sulfate C) carbonate D) sulfate and carbonate E) none of the above

16) Of the three types of radioactivity characterized by Rutherford, which are particles? A) β-rays B) α-rays, β-rays, and γ-rays C) γ-rays D) α-rays and γ-rays E) α-rays and β-rays

18) Which one of the following is a diprotic acid? A) nitric acid B) chloric acid C) phosphoric acid D) hydrofluoric acid E) sulfuric acid

2) Of the reactions below, which one is not a combination reaction? A) C + O2 → CO2 B) 2Mg + O2 → 2MgO C) 2N2 + 3H2 → 2NH3 D) CaO + H2O → Ca(OH)2 E) 2CH4 + 4O2 → 2CO2 + 4H2O

2) The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is ________. A) 2H+ (aq) + 2OH- (aq) → 2H2O (l) B) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq) C) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq) D) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s) E) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq)

21) Which quantum numbers must be the same for the orbitals that they designate to be degenerate in a one-electron system (such as hydrogen)? A) n, l, and ml B) n and l only C) l and ml D) ml only E) n only

22) In a px orbital, the subscript x denotes the ________. A) energy of the electron B) spin of the electrons C) probability of the shell D) size of the orbital E) axis along which the orbital is aligned

23) An atom of the most common isotope of gold, Au, has ________ protons, ________ neutrons, and ________ electrons. A) 197, 79, 118 B) 118, 79, 39 C) 79, 197, 197 D) 79, 118, 118 E) 79, 118, 79

23) The mass % of F in the binary compound KrF2 is ________. A) 18.48 B) 45.38 C) 68.80 D) 81.52 E) 31.20

25) In which reaction does the oxidation number of oxygen increase? A) Ba(NO3)2 (aq) + K2SO4 (aq) → BaSO4 (s) + 2KNO3 (aq) B) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) C) MgO (s) + H2O (l) → Mg(OH)2 (s) D) 2SO2 (g) + O2 (g) → 2SO3 (g) E) 2H2O (l) → 2H2 (g) + O2 (g)

25) Which quantum numbers must be the same for the orbitals that they designate to be degenerate in a many-electron system? A) n, l, and ml B) n only C) n, l, ml, and ms D) ms only E) n and l only

26) Which of the following is not a valid set of four quantum numbers? (n, l, ml, ms) A) 2, 0, 0, +1/2 B) 2, 1, 0, -1/2 C) 3, 1, -1, -1/2 D) 1, 0, 0, +1/2 E) 1, 1, 0, +1/2

29) Calculate the percentage by mass of hydrogen in PtCl2(NH3)2. A) 1.558 B) 1.008 C) 0.672 D) 0.034 E) 2.016

29) The nucleus of an atom does not contain ________. A) protons B) protons or neutrons C) neutrons D) subatomic particles E) electrons

31) One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution? A) zinc B) cobalt C) lead D) copper E) none of these

31) One mole of ________ contains the smallest number of atoms. A) S8 B) C10H8 C) Al2(SO4)3 D) Na3PO4 E) NaCl

35) In the symbol below, x = ________. O A) 17 B) 8 C) 6 D) 7 E) not enough information to determine

36) Acceleration due to gravity of a free-falling object is 9.8 m/s2. Express this in millimeters/millisecond2. A) 9.8 × 10-9 B) 9.8 × 103 C) 9.8 × 10-6 D) 9.8 × 106 E) 9.8 × 10-3

39) Oxidation and ________ mean essentially the same thing. A) activity B) reduction C) metathesis D) decomposition E) corrosion

40) Oxidation cannot occur without ________. A) acid B) oxygen C) water D) air E) reduction

42) How many sulfur dioxide molecules are there in 0.180 mol of sulfur dioxide? A) 1.80 × 1023 B) 6.02 × 1024 C) 6.02 × 1023 D) 1.08 × 1024 E) 1.08 × 1023

43) The lowest orbital energy is reached when the number of electrons with the same spin is maximized. This statement describes ________. A) Pauli Exclusion Principle B) Planck's constant C) deBroglie hypothesis D) Heisenberg Uncertainty Principle E) Hund's rule

45) Which two elements have the same ground-state electron configuration? A) Pd and Pt B) Cu and Ag C) Fe and Cu D) Cl and Ar E) No two elements have the same ground-state electron configuration.

46) Which solution has the same number of moles of NaOH as 50.0 mL of 0.100 M solution of NaOH? A) 20.0 mL of 0.200 M solution of NaOH B) 25.0 mL of 0.175 M solution of NaOH C) 30.0 mL of 0.145 M solution of NaOH D) 50.0 mL of 0.125 M solution of NaOH E) 100.0 mL of 0.0500 M solution of NaOH

49) There are ________ oxygen atoms in 30 molecules of C20H42S3O2. A) 6.0 × 1023 B) 1.8 × 1025 C) 3.6 × 1025 D) 1.2 × 1024 E) 60

49) What are the respective concentrations (M) of Mg2+ and C2H3O2- afforded by dissolving 0.600 mol Mg(C2H3O2)2 in water and diluting to 135 mL? A) 0.444 and 0.889 B) 0.0444 and 0.0889 C) 0..889 and 0.444 D) 0.444 and 0.444 E) 4.44 and 8.89

51) A sulfur oxide is 50.0% by mass sulfur. This molecular formula could be ________. A) SO B) SO2 C) S2O D) S2O4 E) either SO2 or S2O4

51) Elements ________ exhibit similar physical and chemical properties. A) with similar chemical symbols B) with similar atomic masses C) in the same period of the periodic table D) on opposite sides of the periodic table E) in the same group of the periodic table

57) What mass (g) of potassium chloride is contained in 430.0 mL of a potassium chloride solution that has a chloride ion concentration of 0.193 M? A) 0.0643 B) 0.0830 C) 12.37 D) 0.386 E) 6.19

59) Elements in the same group of the periodic table typically have ________. A) similar mass numbers B) similar physical properties only C) similar chemical properties only D) similar atomic masses E) similar physical and chemical properties

6) Which one of the following is an endothermic process? A) ice melting B) water freezing C) boiling soup D) Hydrochloric acid and barium hydroxide are mixed at 25 °C: the temperature increases. E) Both A and C

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.

63) What volume (mL) of 7.48 × 10-2 M perchloric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide? A) 125 B) 8.60 C) 188 D) 750 E) 375

67) Formulas that show how atoms are attached in a molecule are called ________. A) molecular formulas B) ionic formulas C) empirical formulas D) diatomic formulas E) structural formulas

8) The reaction used to inflate automobile airbags ________. A) produces sodium gas B) is a combustion reaction C) is a combination reaction D) violates the law of conservation of mass E) is a decomposition reaction

81) Which species below is the nitride ion? A) Na+ B) NO3- C) NO2- D) NH4+ E) N3-

86) Which formula/name pair is incorrect? A) FeSO4 iron(II) sulfate B) Fe2(SO3)3 iron(III) sulfite C) FeS iron(II) sulfide D) FeSO3 iron(II) sulfite E) Fe2(SO4)3 iron(III) sulfide

91) The correct name for MgF2 is ________. A) monomagnesium difluoride B) magnesium difluoride C) manganese difluoride D) manganese bifluoride E) magnesium fluoride

96) The charge on the ________ ion is -3. A) sulfate B) acetate C) permanganate D) oxide E) nitride

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