Physical Science Survey 2 Midterm Flashcards

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

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

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

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

A. Element

B. Compound

C. Homogeneous mixture

D. Heterogeneous mixture

E. Solvent

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

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

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

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

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

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

Which of the following is an extensive property?

A. Density

B. Temperature

C. Mass

D. Specific Heat

E. Pressure

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

The density of a substance is an intensive property.

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

A row of the periodic table is called a

A) group

B) period

C) isotopic mixture

D) family

E) subshell

Which of these elements is chemically similar to oxygen?

A) sulfur

B) calcium

C) iron

D) nickel

E) potassium

Which of these elements is chemically similar to potassium?

A) calcium

B) arsenic

C) phosphorus

D) cerium

E) cesium

What is the name of PCl₃?

A) phosphorus chloride

B) phosphoric chloride

C) phosphorus trichlorate

D) trichlorophosphid

E) phosphorus trichloride

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

What is the name of P₄Se₃?

A) phosphorus selenide

B) phosphorus triselenide

C) tetraphosphorus selenide

D) phosphoric selenide

E) tetraphosphorus triselenide

What is the name of ClO^-?

A) hypochlorite

B) chlorate

C) chlorite

D) perchlorate

E) perchlorite

What is the formula for the permanganate ion?

A) MnO₂ ^-

B) MnO₄ ^-

C) MgO₄ ^2-

D) Mn₂O₇ ^-

E) MgO₂ ^2-

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

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

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

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

A) CaSe

B) Ca₂Se

C) CaSe₂

D) Ca₃Se

E) CaSe₃

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

The formula for magnesium sulfate is

A) MnS

B) MgS

C) MnSO₃

D) MgSO₄

E) MnSO₄

The formula for sodium sulfide is

A) NaS

B) K₂S

C) NaS₂

D) Na₂S

E) SeS

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

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

What is the formula for lead (II) oxide?

A) PbO

B) PbO₂

C) Pb₂O

D) PbO₄

E) Pb₂O₃

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

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

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)

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)

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)

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)

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)

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

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

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

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)

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)

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)

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)

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)

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)

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)

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.

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

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

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.

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.

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.

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.

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

A) covalent

B) ionic

C) metallic

D) double

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

A) calcium fluorine

B) calcium fluoride

C) calcium difluoride

D) monocalcium difluoride

What is the correct name for the compound, CuCl₂?

A) copper chloride

B) copper dichloride

C) copper(II) chloride

D) copper chloride(II)

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

A) 44 u

B) 45 u

C) 75 u

D) 78 u

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

A) 43.4%

B) 32.5%

C) 21.7%

D) 62.1%

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

A) decomposition

B) combination

C) replacement

D) ion exchange

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

A) decomposition

B) combination

C) replacement

D) ion exchange

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

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.

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.

The reaction between water solutions of sodium chloride and silver nitrate produces a precipitate: NaCl_(aq) + AgNO_{3 (aq)} ® NaNO_{3 (aq)} + AgCl_(s). This is an example of

A) decomposition

B) combination

C) replacement

D) ion exchange

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

Calculate the molecular mass of potassium permanganate, KMnO₄.

A) 52 amu

B) 70 amu

C) 110 amu

D) 158 amu

E) 176 amu

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

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

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.

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

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)

Which element has the following ground-state electron configuration?

1s²2s²2p⁶3s²

A) Na

B) Mg

C) Al

D) Si

E) Ne

Which element has the following ground-state electron configuration?

[Kr]5s²4d¹⁰5p³

A) Sn

B) Sb

C) Pb

D) Bi

E) Te

Which element has the following ground-state electron configuration?

[Kr]5s²4d¹⁰5p²

A) Sn

B) Sb

C) Pb

D) Ge

E) Te

The electron configuration of a ground-state vanadium atom is

A) [Ar]4s²4d³

B) [Ar]4s²4p³

C) [Ar]4s²3d³

D) [Ar]3d⁵

The electron configuration of a ground-state Co atom is

A) [Ar]4s²3d⁷

B) 1s²2s²2p⁶3s²3d⁹

C) [Ne]3s²3d⁷

D) [Ar]4s¹3d⁵

E) [Ar]4s²4d⁷

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