Physical Science Survey 2 Midterm Flashcards


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Midterm Exam
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1

Which one of the following is a "substance" in the sense of the word as used in your textbook?

A) Air

B) Tap Water

C) Sea Water

D) Water

E) Toothpaste

D. Water

2

Which of the following cannot be separated into a simpler substance by chemical means?

A. Element

B. Emulsion

C. Compound

D. Homogeneous mixture

E. Heterogeneous mixture

A. Element

3

If a liquid contains 60% sugar and 40% water throughout its composition, what is it called?

A. Solute

B. Compound

C. Homogeneous mixture

D. Heterogeneous mixture Solvent

C. Homogeneous mixture

4

Which of the following does not have a uniform composition throughout?

A. Element

B. Compound

C. Homogeneous mixture

D. Heterogeneous mixture

E. Solvent

D. Heterogeneous mixture

5

Which of the following is a chemical change?

A. Boiling of water

B. Melting wax

C. Broiling a steak on a grill

D. Condensing water vapor into rainfall

E. Carving a piece of wood

C. Broiling a steak on a grill

6

Which of these is an example of a physical property?

A. Corrosiveness of sulfuric acid

B. Toxicity of cyanide

C. Flammability of gasoline

D. Neutralization of stomach acid with an antacid

E. Lead becomes a liquid when heated to 601oC

E. Lead becomes a liquid when heated to 601oC

7

Which one of these represents a physical change?

A. Water, when heated, forms steam

B. Bleach turns hair yellow

C. Sugar, when heated, becomes brown

D. Milk turns sour

E. Apples, when exposed to air, turn brown

A. Water, when heated, forms steam

8

Which one of these represents a chemical change?

A. Boiling water to form steam

B. Turning hair yellow with bleach

C. Melting butter

D. Mixing powdered charcoal and oxygen at room temperature

E. Cutting a bar of sodium metal into pieces with a knife

B. Turning hair yellow with bleach

9

Which of the following is an extensive property of oxygen?

A. Boiling point

B. Temperature

C. Average kinetic energy of molecules

D. Density

E. Mass

E. Mass

10

When the value of something does not depend on the amount of the matter, what is this called?

A. Empirical property

B. Intensive property

C. Inclusive property

D. Extensive property

E. Exclusive property

B. Intensive property

11

Which of the following is an extensive property?

A. Density

B. Temperature

C. Mass

D. Specific Heat

E. Pressure

C. Mass

12

The ripening of fruit, once picked, is an example of physical change. (True or False)

False

13

The density of a substance is an intensive property.

True

14

The volume of a substance is an intensive property. (True or False)

False

15

Boiling point and melting point are extensive properties. (True or False)

False

16

Rusting of a piece of iron under environmental conditions is a physical change. (True or False)

False

17

A dip of vanilla ice cream is a pure substance. (True or False)

False

18

The scientist who determined the magnitude of the electric charge of the electron was

A. John Dalton

B. Robert Millikan

C. J. J. Thomson

D. Henry Moseley

E. J. Burdge

B. Robert Millikan

19

When J. J. Thomson discovered the electron, what physical property of the electron did he measure?

A. its charge, e

B. its charge-to-mass ratio, e/m

C. its temperature, T

D. its mass, m

E. its atomic number, Z

B. its charge-to-mass ratio, e/m

20

What name is given to the concept that different samples of a given compound always contain the same elements in the same mass ratio?

A. Ration Law

B. Law of Equality

C. 1st Law of Thermodynamics

D. Law of Definite Proportions

E. 2nd Law of thermodynamics

D. Law of Definite Proportions

21

Which of these scientists developed the nuclear model of the atom?

A. John Dalton

B. Robert Millikan

C. J. J. Thomson

D. Henry Moseley

E. Ernest Rutherford

E. Ernest Rutherford

22

Rutherford's experiment with alpha particle scattering by gold foil established that

A. protons are not evenly distributed throughout an atom

B. electrons have a negative charge

C. electrons have a positive charge

D. atoms are made of protons, neutrons, and electrons

E. protons are 1840 times heavier than electrons

A. protons are not evenly distributed throughout an atom

23

J. J. Thomson studied cathode ray particles (electrons) and was able to measure the mass/charge ratio. His results showed that

A. the mass/charge ratio varied as the cathode material was changed

B. the charge was always a whole-number multiple of some minimum charge

C. matter included particles much smaller than the atom

D. atoms contained dense areas of positive charge

E. atoms are largely empty space

B. the charge was always a whole-number multiple of some minimum charge

24

Millikan's oil-drop experiment

A. established the charge on an electron

B. showed that all oil drops carried the same charge

C. provided support for the nuclear model of the atom

D. suggested that some oil drops carried fractional numbers of electrons

E. suggested the presence of a neutral particle in the atom

A. established the charge on an electron

25

Which one of the following statements about atoms and subatomic particles is correct?

A. Rutherford discovered the atomic nucleus by bombarding gold foil with electrons

B. The proton and the neutron have identical masses

C. The neutron's mass is equal to that of a proton plus an electron

D. A neutral atom contains equal numbers of protons and electrons

E. An atomic nucleus contains equal numbers of protons and neutrons

D. A neutral atom contains equal numbers of protons and electrons

26

What term is used to represent the number of protons in the nucleus of each atom of an element and is equal to the number of electrons outside the nucleus?

A. Isotope number

B. Mass number

C. Mass-to-charge ratio

D. Atomic number

E. Atomic mass units

D. Atomic number

27

What term is used to represent the total number of neutrons and protons in then nucleus of each atom of an element?

A. Isotope number

B. Mass number

C. Mass-to-charge ratio

D. Atomic number

E. Atomic mass units

B. Mass number

28

Bromine is the only nonmetal that is a liquid at room temperature. Consider the isotope bromine-81. Select the combination which lists the correct atomic number, neutron number, and mass number, respectively.

A. 35, 46, 81

B. 35, 81, 46

C. 81, 46, 35,

D. 46, 81, 35

E. 35, 81, 116

A. 35, 46, 81

29

How many neutrons are there in an atom of lead whose mass number is 208?

A. 82

B. 126

C. 208

D. 290

E. None of the above

B. 126

30

An atom of the isotope sulfur-31 consists of how many protons, neutrons, and electrons? (p=proton, n=neutron, e=electron)

A. 15 p, 16 n, 15 e

B. 16 p, 15 n, 16 e

C. 16 p, 31 n, 16 e

D. 32 p, 31 n, 32 e

E. 16 p, 16 n, 15 e

B. 16 p, 15n, 16 e

31

Give the number of protons (p), electrons (e), and neutrons (n) in one atom of chlorine-37.

A) 37 p, 37 e, 17 n

B) 17 p, 17 e, 37 n

C) 17 p, 17 e, 20 n

D) 37 p, 17 e, 20 n

E) 17 p, 37 e, 17 n

C. 17 p, 17 e, 20 n

32

Which of the following is a non-metal?

A) lithium, Li, Z = 3

B) bromine, Br, Z = 35

C) mercury, Hg, Z = 80

D) bismuth, Bi, Z = 83

E) sodium, Na, Z = 11

B) bromine, Br, Z = 35

33

Which of the following is a metal?

A) nitrogen, N, Z = 7

B) phosphorus, P, Z = 15

C) arsenic, Z = 33

D) thallium, Tl, Z = 81

E) silicon, Si, Z = 14

D) thallium, Tl, Z = 81

34

Which of the following is a metalloid?

A. carbon, C, Z = 6

B. sulfur, S, Z = 16

C. germanium, Ge, Z = 32

D. iridium, Z = 77

E. bromine, Br, Z = 35

C. germanium, Ge, Z = 32

35

A row of the periodic table is called a

A) group

B) period

C) isotopic mixture

D) family

E) subshell

B) period

36

Which of these elements is chemically similar to oxygen?

A) sulfur

B) calcium

C) iron

D) nickel

E) potassium

A) sulfur

37

Which of these elements is chemically similar to potassium?

A) calcium

B) arsenic

C) phosphorus

D) cerium

E) cesium

E) cesium

38

What is the name of PCl3?

A) phosphorus chloride

B) phosphoric chloride

C) phosphorus trichlorate

D) trichlorophosphid

E) phosphorus trichloride

E) phosphorus trichloride

39

The compound, P4S10, is used in the manufacture of safety matches. What is its name?

A) phosphorus sulfide

B) phosphoric sulfide

C) phosphorus decasulfide

D) tetraphosphorus decasulfide

E) phosphorus sulfite

D) tetraphosphorus decasulfide

40

What is the name of P4Se3?

A) phosphorus selenide

B) phosphorus triselenide

C) tetraphosphorus selenide

D) phosphoric selenide

E) tetraphosphorus triselenide

E) tetraphosphorus triselenide

41

What is the name of ClO-?

A) hypochlorite

B) chlorate

C) chlorite

D) perchlorate

E) perchlorite

A) hypochlorite

42

What is the formula for the permanganate ion?

A) MnO2 -

B) MnO4 -

C) MgO4 2-

D) Mn2O7 -

E) MgO2 2-

B) MnO4 -

43

Which of these pairs of elements would be most likely to form an ionic compound?

A) P and Br

B) Cu and K

C) C and O

D) O and Zn

E) Al and Rb

D) O and Zn

44

Which pair of elements would be most likely to form an ionic compound?

A) P and Br

B) Zn and K

C) F and Al

D) C and S

E) Al and Rb

C) F and Al

45

What is the formula for the ionic compound formed by calcium ions and nitrate ions?

A) Ca3N2

B) Ca(NO3)2

C) Ca2NO3

D) Ca2NO2

E) CaNO3

B) Ca(NO3)2

46

What is the formula for the ionic compound formed by calcium and selenium?

A) CaSe

B) Ca2Se

C) CaSe2

D) Ca3Se

E) CaSe3

A) CaSe

47

Which is the correct formula for copper (II) phosphate?

A) Cu2PO4

B) Cu3(PO4)2

C) Cu2PO3

D) Cu(PO4)2

E) Cu(PO3)2

B) Cu3(PO4)2

48

The formula for magnesium sulfate is

A) MnS

B) MgS

C) MnSO3

D) MgSO4

E) MnSO4

D) MgSO4

49

The formula for sodium sulfide is

A) NaS

B) K2S

C) NaS2

D) Na2S

E) SeS

D) Na2S

50

The chemical formula for iron (II) nitrate is

A) Fe2(NO3)3

B) Ir(NO2)2

C) Fe2N3

D) Fe(NO3)2

E) Fe(NO2)2

D) Fe(NO3)2

51

Which one of the following formulas of ionic compounds is the least likely to be correct?

A) NH4Cl

B) Ba(OH)2

C) Na2SO4

D) Ca2NO3

E) Cu(CN)2

D) Ca2NO3

52

What is the formula for lead (II) oxide?

A) PbO

B) PbO2

C) Pb2O

D) PbO4

E) Pb2O3

A) PbO

53

Potassium permanganate is a strong oxidizer that reacts explosively with easily oxidized materials. What is its formula?

A) KMnO3

B) KMnO4

C) K2MnO4

D) K(MnO4)2

E) K2Mn2O7

B) KMnO4

54

54. What is the name of Mn(CO3)2?

A) manganese carbide

B) magnesium (IV) carbonate

C) manganese (II) carbonate

D) magnesium (II) carbonate

E) manganese (IV) carbonate

E) manganese (IV) carbonate

55

Balance the following equation:

B2O3(s) + HF(l) ® BF3(g) + H2O(l)

A) B2O3(s) + 6HF(l) ® 2BF3(g) + 3H2O(l)

B) B2O3(s) + H6F6(l) ® B2F6(g) + H6O3(l)

C) B2O3(s) + 2HF(l) ® 2BF3(g) + H2O(l)

D) B2O3(s) + 3HF(l) ® 2BF3(g) + 3H2O(l)

E) B2O3(s) + 6HF(l) ® 2BF3(g) + 6H2O(l)

A) B2O3(s) + 6HF(l) ® 2BF3(g) + 3H2O(l)

56

Balance the following equation:

UO2(s) + HF(l) ® UF4(s) + H2O(l)

A) UO2(s) + 2HF(l) ® UF4(s) + H2O(l)

B) UO2(s) + 4HF(l) ® UF4(s) + 2H2O(l)

C) UO2 (s) + H4F4(l) ® UF4 (s) + H4O2(l)

D) UO2(s) + 4HF(l) ® UF4(s) + 4H2O(l)

E) UO2(s) + 8HF(l) ® 2UF4(s) + 4H2O(l)

B) UO2(s) + 4HF(l) ® UF4(s) + 2H2O(l)

57

Balance the following equation for the combustion of benzene:

C6H6(l) + O2(g) ® H2O(g) + CO2(g)

A) C6H6(l) + 9O2(g) ® 3H2O(g) + 6CO2(g)

B) C6H6(l) + 9O2(g) ® 6H2O(g) + 6CO2(g)

C) 2C6H6(l) + 15O2(g) ® 6H2O(g) + 12CO2(g)

D) C6H6(l) + 15O2(g) ® 3H2O(g) + 6CO2(g)

E) 2C6H6(l) + 9O2(g) ® 6H2O(g) + 12CO2(g)

C) 2C6H6(l) + 15O2(g) ® 6H2O(g) + 12CO2(g)

58

Balance the following equation:

C8H18O3(l) + O2(g) ® H2O(g) + CO2(g)

A) C8H18O3(l) + 8O2(g) ® 9H2O(g) + 8CO2(g)

B) C8H18O3(l) + 11O2(g) ® 9H2O(g) + 8CO2(g)

C) 2C8H18O3(l) + 22O2(g) ® 9H2O(g) + 16CO2(g

D) C8H18O3(l) + 13O2(g) ® 18H2O(g) + 8CO2(g)

E) 2C8H18O3(l) + 17O2(g) ® 18H2O(g) + 16CO2(g)

B) C8H18O3(l) + 11O2(g) ® 9H2O(g) + 8CO2(g)

59

Balance the following equation:

Ca3(PO4)2(s) + SiO2(s) + C(s) ® CaSiO3(s) + CO(g) + P4(s)

A) Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) ® 3CaSiO3(s) + 8CO(g) + P4(s)

B) Ca3(PO4)2(s) + 3SiO2(s) + 14C(s) ® 3CaSiO3(s) + 14CO(g) + P4(s)

C) Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) ® 3CaSiO3(s) + 8CO(g) + 2P4(s)

D) 2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) ® 6CaSiO3(s) + 10CO(g) + P4(s)

E) 2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) ® 6CaSiO3(s) + 10CO(g) + 4P4(s)

D) 2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) ® 6CaSiO3(s) + 10CO(g) + P4(s)

60

Balance the following equation using the smallest set of whole numbers, then add together the coefficients. Don't forget to count coefficients of one. The sum of the coefficients is

__ SF4 + __ H2O ® __ H2SO3 + __ HF

A) 4

B) 6

C) 7

D) 9

E) None of these

D) 9

61

Calculate the molecular mass of potassium permanganate, KMnO4.

A) 52 g/mol

B) 70 g/mol

C) 110 g/mol

D) 158 g/mol

E) 176 g/mol

D) 158 g/mol

62

Calculate the molecular mass of menthol, C10H20O.

A) 156 g/mol

B) 140 g/mol

C) 29 g/mol

D) 146 g/mol

E) 136 g/mol

A) 156 g/mol

63

Which of these chemical equations describes a disproportionation reaction?

A) 2C2H6(g) + 7O2(g) ® 4CO2(g) + 6H2O(l)

B) 2KBr(aq) + Cl2(g) ® 2KCl(aq) + Br2(l)

C) 2H2O2(aq) ® 2H2O(l) + O2(g)

D) CaBr2(aq) + H2SO4(aq) ® CaSO4(s) + 2HBr(g)

E) 2Al(s) + 3H2SO4(aq) ® Al2(SO4)3(aq) + 3H2(g)

C) 2H2O2(aq) ® 2H2O(l) + O2(g)

64

Which of these chemical equations describes a metal displacement reaction?

A) 2NaN3(s) ® 2Na(s) + 3N2(g)

B) Fe2O3(s) + 2Al(s) ® 2Fe(s) + Al2O3(s)

C) 3NO2(g) + H2O(l) ® 2HNO3(aq) + NO(g)

D) 2P(s) + 3Cl2(g) ® 2PCl3(g)

E) 2ZnS(s) + 3O2(g) ® 2ZnO(s) + 2SO2(g)

B) Fe2O3(s) + 2Al(s) ® 2Fe(s) + Al2O3(s)

65

Which of these chemical equations describes a halogen displacement reaction?

A) 2KBr(aq) + Cl2(g) ® 2KCl(aq) + Br2(l)

B) 2Na(s) + 2H2O(l) ® 2NaOH(aq) + H2(g)

C) CaBr2(aq) + H2SO4(aq) ® CaSO4(s) + 2HBr(g)

D) 2KNO3(s) ® 2KNO2(s) + O2(g)

E) 2LiOH(aq) + H2SO4(aq) ® Li2SO4(aq) + 2H2O(l)

A) 2KBr(aq) + Cl2(g) ® 2KCl(aq) + Br2(l)

66

Which of these chemical equations describes a precipitation reaction?

A) 2H2(g) + O2(g) ® 2H2O(l)

B) CaBr2(aq) + H2SO4(aq) ® CaSO4(s) + 2HBr(g)

C) 2KNO3(s) ® 2KNO2(s) + O2(g)

D) 2KBr(aq) + Cl2(g) ® 2KCl(aq) + Br2(l)

E) 2Al(s) + 3H2SO4(aq) ® Al2(SO4)3(aq) + 3H2(g)

B) CaBr2(aq) + H2SO4(aq) ® CaSO4(s) + 2HBr(g)

67

Which of these chemical equations describes an acid-base neutralization reaction?

A) 2Al(s) + 3H2SO4(aq) ® Al2(SO4)3(aq) + 3H2(g)

B) SO2(g) + H2O(l) ® H2SO3(g)

C) LiOH(aq) + HNO3(aq) ® LiNO3(aq) + H2O(l)

D) 2KBr(aq) + Cl2(g) ® 2KCl(aq) + Br2(l)

E) CaBr2(aq) + H2SO4(aq) ® CaSO4(s) + 2HBr(g)

C) LiOH(aq) + HNO3(aq) ® LiNO3(aq) + H2O(l)

68

Which of these chemical equations describes a hydrogen displacement reaction?

A) 2C2H6(g) + 7O2(g) ® 4CO2(g) + 6H2O(l)

B) 2KBr(aq) + Cl2(g) ® 2KCl(aq) + Br2(l)

C) N2(g) + 3H2(g) ® 2NH3(g)

D) CaBr2(aq) + H2SO4(aq) ® CaSO4(s) + 2HBr(g)

E) 2Al(s) + 3H2SO4(aq) ® Al2(SO4)3(aq) + 3H2(g)

E) 2Al(s) + 3H2SO4(aq) ® Al2(SO4)3(aq) + 3H2(g)

69

Which of these chemical equations describes a combustion reaction?

A) 2C2H6(g) + 7O2(g) ® 4CO2(g) + 6H2O(l)

B) LiOH(aq) + HNO3(aq) ® LiNO3(aq) + H2O(l)

C) N2(g) + 3H2(g) ® 2NH3(g)

D) 2Na(s) + 2H2O(l) ® 2NaOH(aq) + H2(g)

E) 2Al(s) + 3H2SO4(aq) ® Al2(SO4)3(aq) + 3H2(g)

A) 2C2H6(g) + 7O2(g) ® 4CO2(g) + 6H2O(l)

70

Select the correct set of products for the following reaction.

Ba(OH)2(aq) + HNO3(aq) ®

A) BaN2(s) + H2O(l)

B) Ba(NO3)2(aq) + H2O(l)

C) Ba(s) + H2(g) + NO2(g)

D) Ba2O(s) + NO2(g) + H2O(l)

E) No reaction occurs.

B) Ba(NO3)2(aq) + H2O(l)

71

What is the correct formula of the salt formed in the neutralization reaction of hydrochloric acid with calcium hydroxide?

A) CaO

B) CaCl

C) CaH2

D) CaCl2

E) CaClH

D) CaCl2

72

What is the chemical formula of the salt produced by the neutralization of hydrobromic acid with magnesium hydroxide?

A) MgBr

B) Mg2Br3

C) MgBr2

D) Mg3Br2

E) Mg2Br l

C) MgBr2

73

Robert Millikan discovered that

A) the charge to mass ratio of electrons was constant.

B) the electron carries the smallest unit of electrical charge.

C) the oil droplets all carried the same amount of charge.

D) the electrons contained most of the mass of an atom.

B) the electron carries the smallest unit of electrical charge.

74

J. J. Thomson reasoned that cathode rays were really charged particles because

A) a magnet deflected cathode rays.

B) cathode rays formed only when the air was pumped out of a discharge tube.

C) the properties of the cathode rays depended on the cathode material.

D) the cathode rays were attracted to the anode.

A) a magnet deflected cathode rays.

75

In an ionic compound, the metal

A) usually forms a negative ion.

B) takes the “-ide” ending.

C) has a Greek prefix like mono, di or tri.

D) is written first.

D) is written first.

76

The formation of a positive ion

A) occurs when an atom gains a proton.

B) involves a release of energy.

C) occurs when an electron is removed from an atom.

D) occurs in covalent bonding.

C) occurs when an electron is removed from an atom.

77

What type of chemical bond does the sharing of a pair of electrons form?

A) covalent

B) ionic

C) metallic

D) double

A) covalent

78

What is the correct name for the ionic compound, CaF2?

A) calcium fluorine

B) calcium fluoride

C) calcium difluoride

D) monocalcium difluoride

B) calcium fluoride

79

What is the correct name for the compound, CuCl2?

A) copper chloride

B) copper dichloride

C) copper(II) chloride

D) copper chloride(II)

C) copper(II) chloride

80

The formula weight of aluminum hydroxide, Al(OH)3 is

A) 44 u

B) 45 u

C) 75 u

D) 78 u

D) 78 u

81

What is the mass percent of sodium in washing soda, Na2CO3?

A) 43.4%

B) 32.5%

C) 21.7%

D) 62.1%

A) 43.4%

82

The reaction: potassium chlorate potassium chloride and oxygen gas is an example of

A) decomposition

B) combination

C) replacement

D) ion exchange

A) decomposition

83

The reaction: 2 NaI + Cl2 ® 2 NaCl + I2 is an example of

A) decomposition

B) combination

C) replacement

D) ion exchange

C) replacement

84

In a chemical equation, the reactants are found on the left side of the arrow. (True or False)

True

85

Which of the following is a sign of an ion exchange reaction?

A) a precipitate is formed.

B) a compound is broken down into simpler substances.

C) a reactant is oxidized.

D) a metal ion is reduced.

A) a precipitate is formed.

86

Because of our belief in the law of conservation of mass, it seems reasonable that

A) in combustion reactions, part of the mass of the reactants must be converted into fire.

B) the mass of a newly formed compound cannot be changed.

C) molecules cannot be broken down for the mass would be reduced.

D) the number of atoms of reactants must equal the number of atoms of products.

D) the number of atoms of reactants must equal the number of atoms of products.

87

The reaction between water solutions of sodium chloride and silver nitrate produces a precipitate: NaCl(aq) + AgNO3 (aq) ® NaNO3 (aq) + AgCl(s). This is an example of

A) decomposition

B) combination

C) replacement

D) ion exchange

D) ion exchange

88

What is the molar mass of nicotine, C10H14N2?

A) 134 g/mol

B) 148 g/mol

C) 158 g/mol

D) 210 g/mol

E) 162 g/mol

E) 162 g/mol

89

Calculate the molecular mass of potassium permanganate, KMnO4.

A) 52 amu

B) 70 amu

C) 110 amu

D) 158 amu

E) 176 amu

D) 158 amu

90

What is the coefficient of H2O when the following equation is properly balanced with the smallest set of whole numbers?

___ Na + ___ H2O ® ___ NaOH + ___ H2

A) 1

B) 2

C) 3

D) 4

E) 5

B) 2

91

What is the coefficient of H2O when the following equation is properly balanced with smallest set of whole numbers?

___ Al4C3 + ___ H2O ® ___ Al(OH)3 + ___ CH4

A) 3

B) 4

C) 6

D) 12

E) 24

D) 12

92

The element oxygen consists of three naturally occuring isotopes: 16O, 17O, and 18O. The atomic mass of oxygen is 16.0 amu. What can be implied about the relative abundances of these isotopes?

A) More than 50% of all O atoms are 17O.

B) Almost all O atoms are 18O.

C) Almost all O atoms are 17O.

D) The isotopes all have the same abundance, i.e. 33.3%.

E) The abundances of 17O and 18O are very small.

E) The abundances of 17O and 18O are very small.

93

An average atom of uranium (U) is approximately how many times heavier than an atom of potassium?

A) 6.1 times

B) 4.8 times

C) 2.4 times

D) 12.5 times

E) 7.7 times

A) 6.1 times

94

Predict the products of the following single replacement reaction.

Fe(s) + CuSO4(aq) ®

A) Cu(s) + FeSO4(aq)

B) Fe(s) + Cu(s) + SO4(aq)

C) CuS(s) + Fe2SO4(aq)

D) FeCuSO4(aq)

E) FeO(s) + CuSO3(aq)

A) Cu(s) + FeSO4(aq)

95

Which element has the following ground-state electron configuration?

1s22s22p63s2

A) Na

B) Mg

C) Al

D) Si

E) Ne

B) Mg

96

Which element has the following ground-state electron configuration?

[Kr]5s24d105p3

A) Sn

B) Sb

C) Pb

D) Bi

E) Te

B) Sb

97

Which element has the following ground-state electron configuration?

[Kr]5s24d105p2

A) Sn

B) Sb

C) Pb

D) Ge

E) Te

A) Sn

98

The electron configuration of a ground-state vanadium atom is

A) [Ar]4s24d3

B) [Ar]4s24p3

C) [Ar]4s23d3

D) [Ar]3d5

C) [Ar]4s23d3

99

The electron configuration of a ground-state Co atom is

A) [Ar]4s23d7

B) 1s22s22p63s23d9

C) [Ne]3s23d7

D) [Ar]4s13d5

E) [Ar]4s24d7

A) [Ar]4s23d7

100

Which of the following is the ground-state electron configuration of a calcium atom?

A) [Ne]3s2

B) [Ne]3s23p6

C) [Ar]4s13d1

D) [Ar]4s2

E) [Ar]3d2

D) [Ar]4s2