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

B

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.

B

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)

C

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

B

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.

D

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.

E

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

C

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

B

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

B

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

A

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

C

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

D

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

B

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

B

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

C

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

E

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

D

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

C

All atoms of a given element have the same ________.
A) mass
B) number of protons
C) number of neutrons
D) number of electrons and neutrons
E) density

B

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

B

Which of the following atoms has the smallest number of neutrons?
A) carbon-14
B) chlorine-35
C) carbon-12
D) carbon-13
E) bromine-79

C

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

D

An atom of the most common isotope of gold, ¹⁹⁷Au, 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

E

Which combination of protons, neutrons, and electrons is correct for the isotope of copper, ⁶³ ₂₉Cu?
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-

A

Which isotope has 45 neutrons?

B

Which pair of atoms constitutes a pair of isotopes of the same element?

B

Which isotope has 36 electrons in an atom?

A

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

C

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

E

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

C

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

A

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.

B

In the symbol shown below, x = ________.
¹⁴ _xC
A) 7
B) 13
C) 12
D) 6
E) not enough information to determine

D

In the symbol below, X = ________.
¹³ ₆X
A) N
B) C
C) Al
D) K
E) not enough information to determine

B

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

E

In the symbol below, x is ________.
^x ₆C
A) the number of neutrons
B) the atomic number
C) the mass number
D) the number of electrons
E) the elemental symbol

C

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

D

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

B

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

C

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

D

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

B

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

A

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

C

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

C

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

B

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

D

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

A

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

A

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.

A

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) increasing atomic mass

B

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

E

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

C

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

A

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, Br
D) Br, Kr
E) N, O

C

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

B

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

C

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

D

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

B

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

E

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

B

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

B

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

A

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

D

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

A

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

C

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

C

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

E

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

D

Which species has 54 electrons?

B

Which species has 16 protons?
A) ³¹P
B)³⁴S^2-
C) ³⁶Cl
D) ⁸⁰BR^-
E) ¹⁶O

B

Which species has 18 electrons?
A) ³⁹K
B) ³²S²-
C) ³⁵Cl
D) ²⁷Al³⁺
E) ⁴⁵Sc³⁺

B

Which of the following species contains 18 electrons?
A) ³¹P
B) ³⁴S^2-
C) ³⁶Cl
D) ⁸⁰Br^-
E) ¹⁶O

B

Which of the following species is an isotope of 79Br?
A) ⁴⁰Ar+
B) 3⁴S^2-
C) ⁷⁹Br^-
D) ⁸⁰Br
E) ⁷⁹Se

D

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

D

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

C

There are ________ protons, ________ neutrons, and ________ electrons in ²³⁸U⁺⁵.
A) 146, 92, 92
B) 92, 146, 87
C) 92, 146, 92
D) 92, 92, 87
E) 146, 92, 97

B

Which species contains 68 neutrons?

A

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

C

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

A

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

C

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

E

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

D

Aluminum reacts with a certain nonmetallic element to form a compound with the general formula Al2X3. Element X must be from Group ________ of the Periodic Table of Elements.
A) 3A
B) 4A
C) 5A
D) 6A
E) 7A

D

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

A

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

D

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

E

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

D

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

A

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

A

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

A

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

E

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

D

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

C

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

A

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

D

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

E

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

C

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

A

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

B

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

A

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

E

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

D

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

C

Methane and ethane are both made up of carbon and hydrogen. In methane, there are 12.0 g of carbon for every 4.00 g of hydrogen, a ratio of 3:1 by mass. In ethane, there are 24.0 g of carbon for every 6.00 g of hydrogen, a ratio of 4:1 by mass. This is an illustration of the law of ________.
A) constant composition
B) multiple proportions
C) conservation of matter
D) conservation of mass
E) octaves

B

________ and ________ reside in the atomic nucleus.
A) Protons, electrons
B) Electrons, neutrons
C) Protons, neutrons
D) Neutrons, only neutrons
E) none of the above

C

520 pm is the same as ________ Å.
A) 5200
B) 52
C) 520
D) 5.2
E) 0.00052

D

The atomic number indicates ________.
A) the number of neutrons in a nucleus
B) the total number of neutrons and protons in a nucleus
C) the number of protons or electrons in a neutral atom
D) the number of atoms in 1 g of an element
E) the number of different isotopes of an element

C

The nucleus of an atom contains ________.
A) electrons
B) protons, neutrons, and electrons
C) protons and neutrons
D) protons and electrons
E) protons

C

In the periodic table, the elements touching the steplike line are known as ________.
A) transition elements
B) noble gases
C) metalloids
D) nonmetals
E) metals

C

Which group in the periodic table contains only nonmetals?
A) 1A
B) 6A
C) 2B
D) 2A
E) 8A

E

Horizontal rows of the periodic table are known as ________.
A) periods
B) groups
C) metalloids
D) metals
E) nonmetals

A

Vertical columns of the periodic table are known as ________.
A) metals
B) periods
C) nonmetals
D) groups
E) metalloids

D

Elements in Group 1A are known as the ________.
A) chalcogens
B) alkaline earth metals
C) alkali metals
D) halogens
E) noble gases

C

Elements in Group 2A are known as the ________.
A) alkaline earth metals
B) alkali metals
C) chalcogens
D) halogens
E) noble gases

A

Elements in Group 6A are known as the ________.
A) alkali metals
B) chalcogens
C) alkaline earth metals
D) halogens
E) noble gases

B

Elements in Group 7A are known as the ________.
A) chalcogens
B) alkali metals
C) alkaline earth metals
D) halogens
E) noble gases

D

Elements in Group 8A are known as the ________.
A) halogens
B) alkali metals
C) alkaline earth metals
D) chalcogens
E) noble gases

E

Potassium is a ________ and chlorine is a ________.
A) metal, nonmetal
B) metal, metal
C) metal, metalloid
D) metalloid, nonmetal
E) nonmetal, metal

A

Lithium is a ________ and magnesium is a ________.
A) nonmetal, metal
B) nonmetal, nonmetal
C) metal, metal
D) metal, metalloid
E) metalloid, metalloid

C

Oxygen is a ________ and nitrogen is a ________.
A) metal, metalloid
B) nonmetal, metal
C) metalloid, metalloid
D) nonmetal, nonmetal
E) nonmetal, metalloid

D

Calcium is a ________ and silver is a ________.
A) nonmetal, metal
B) metal, metal
C) metalloid, metal
D) metal, metalloid
E) nonmetal, metalloid

B

________ are found uncombined, as monatomic species in nature.
A) Noble gases
B) Chalcogens
C) Alkali metals
D) Alkaline earth metals
E) Halogens

A

When a metal and a nonmetal react, the ________ tends to lose electrons and the ________ tends to gain electrons.
A) metal, metal
B) nonmetal, nonmetal
C) metal, nonmetal
D) nonmetal, metal
E) None of the above; these elements share electrons.

C

The empirical formula of a compound with molecules containing 12 carbon atoms, 14 hydrogen atoms, and 6 oxygen atoms is ________.
A) C12H14O6
B) CHO
C) CH2O
D) C6H7O3
E) C2H4O

D

________ only form ions with a 2+ charge.
A) Alkaline earth metals
B) Halogens
C) Chalcogens
D) Alkali metals
E) Transition metals

A

What is the formula of the compound formed between strontium ions and nitrogen ions?
A) SrN
B) Sr3N2
C) Sr2N3
D) SrN2
E) SrN3

B

Magnesium reacts with a certain element to form a compound with the general formula MgX. What would the most likely formula be for the compound formed between potassium and element X?
A) K2X
B) KX2
C) K2X3
D) K2X2
E) KX

A

The charge on the manganese in the salt MnF3 is ________.
A) 1+
B) 1-
C) 2+
D) 2-
E) 3+

E

Aluminum reacts with a certain nonmetallic element to form a compound with the general formula AlX. Element X is a diatomic gas at room temperature. Element X must be ________.
A) oxygen
B) fluorine
C) chlorine
D) nitrogen
E) sulfur

D

Sodium forms an ion with a charge of ________.
A) 1+
B) 1-
C) 2+
D) 2-
E) 0

A

Potassium forms an ion with a charge of ________.
A) 2+
B) 1-
C) 1+
D) 2-
E) 0

C

Calcium forms an ion with a charge of ________.
A) 1-
B) 2-
C) 1+
D) 2+
E) 0

D

Barium forms an ion with a charge of ________.
A) 1+
B) 2-
C) 3+
D) 3-
E) 2+

E

Aluminum forms an ion with a charge of ________.
A) 2+
B) 3-
C) 1+
D) 3+
E) 1-

D

Fluorine forms an ion with a charge of ________.
A) 1-
B) 1+
C) 2+
D) 3+
E) 3-

A

Iodine forms an ion with a charge of ________.
A) 7-
B) 1+
C) 2-
D) 2+
E) 1-

E

Oxygen forms an ion with a charge of ________.
A) 2-
B) 2+
C) 3-
D) 3+
E) 6+

A

Sulfur forms an ion with a charge of ________.
A) 2+
B) 2-
C) 3+
D) 6-
E) 6+

B

Predict the empirical formula of the ionic compound that forms from sodium and fluorine.
A) NaF
B) Na2F
C) NaF2
D) Na2F3
E) Na3F2

A

Predict the empirical formula of the ionic compound that forms from magnesium and fluorine.
A) Mg2F3
B) MgF
C) Mg2F
D) Mg3F2
E) MgF2

E

Predict the empirical formula of the ionic compound that forms from magnesium and oxygen.
A) Mg2O
B) MgO
C) MgO2
D) Mg2O2
E) Mg3O2

B

Predict the empirical formula of the ionic compound that forms from aluminum and oxygen.
A) AlO
B) Al3O2
C) Al2O3
D) AlO2
E) Al2O

C

The correct name for K2S is ________.
A) potassium sulfate
B) potassium disulfide
C) potassium bisulfide
D) potassium sulfide
E) dipotassium sulfate

D

The correct name for Al2O3 is ________.
A) aluminum oxide
B) dialuminum oxide
C) dialuminum trioxide
D) aluminum hydroxide
E) aluminum trioxide

A

The correct name for CaH2 is ________.
A) hydrocalcium
B) calcium dihydride
C) calcium hydroxide
D) calcium dihydroxide
E) calcium hydride

E

The correct name for SO is ________.
A) sulfur oxide
B) sulfur monoxide
C) sulfoxide
D) sulfate
E) sulfite

B

The correct name for CCl4 is ________.
A) carbon chloride
B) carbon tetrachlorate
C) carbon perchlorate
D) carbon tetrachloride
E) carbon chlorate

D

The correct name for N2O5 is ________.
A) nitrous oxide
B) nitrogen pentoxide
C) dinitrogen pentoxide
D) nitric oxide
E) nitrogen oxide

C

The correct name for H2CO3 is ________.
A) carbonous acid
B) hydrocarbonate
C) carbonic acid
D) carbohydrate
E) carbohydric acid

C

The correct name for H2SO3 is ________.
A) sulfuric acid
B) sulfurous acid
C) hydrosulfuric acid
D) hydrosulfic acid
E) sulfur hydroxide

B

The correct name for H2SO4 is ________.
A) sulfuric acid
B) sulfurous acid
C) hydrosulfuric acid
D) hydrosulfic acid
E) sulfur hydroxide

A

The correct name for HNO3 is ________.
A) nitrous acid
B) nitric acid
C) hydronitroxide acid
D) nitroxide acid
E) nitrogen hydroxide

B

The correct name for HClO3 is ________.
A) hydrochloric acid
B) perchloric acid
C) chloric acid
D) chlorous acid
E) hydrochlorous acid

C

The correct name for HClO is ________.
A) hydrochloric acid
B) perchloric acid
C) chloric acid
D) chlorous acid
E) hypochlorous acid

E

The correct name for HBrO4 is ________.
A) hydrobromic acid
B) perbromic acid
C) bromic acid
D) bromous acid
E) hydrobromous acid

B

The correct name for HBrO is ________.
A) hydrobromic acid
B) perbromic acid
C) bromic acid
D) bromous acid
E) hypobromous acid

E

The correct name for HBrO2 is ________.
A) hydrobromic acid
B) perbromic acid
C) bromic acid
D) bromous acid
E) hydrobromous acid

D

The correct name for HClO2 is ________.
A) perchloric acid
B) chloric acid
C) hypochlorous acid
D) hypychloric acid
E) chlorous acid

E

The correct name of the compound Na3N is ________.
A) sodium nitride
B) sodium azide
C) sodium trinitride
D) sodium(III) nitride
E) trisodium nitride

A

The formula of bromic acid is ________.
A) HBr
B) HBrO4
C) HBrO
D) HBrO3
E) HBrO2

D

The correct formula for molybdenum (IV) hypochlorite is ________.
A) Mo(ClO3)4
B) Mo(ClO)4
C) Mo(ClO2)4
D) Mo(ClO4)4
E) MoCl4

B

The name of PCl3 is ________.
A) potassium chloride
B) phosphorus trichloride
C) phosphorous(III) chloride
D) monophosphorous trichloride
E) trichloro potassium

B

The ions Ca²⁺ and PO4^3- form a salt with the formula ________.
A) CaPO4
B) Ca2(PO4)3
C) Ca2PO4
D) Ca(PO4)2
E) Ca3(PO4)2

E

The correct formula of iron (III) bromide is ________.
A) FeBr2
B) FeBr3
C) FeBr
D) Fe3Br3
E) Fe3Br

B

Magnesium and sulfur form an ionic compound with the formula ________.
A) MgS
B) Mg2S
C) MgS2
D) Mg2S2
E) Mg2S3

A

The formula of ammonium carbonate is ________.
A) (NH4)2CO3
B) NH4CO2
C) (NH3)2CO4
D) (NH3)2CO3
E) N2(CO3)3

A

The formula of the chromate ion is ________.
A) CrO₄ ^2-
B) CrO₂ ^3-
C) CrO^-
D) CrO₃2^-
E) CrO^2-

A

The formula of the carbonate ion is ________.
A) CrO₂2-
B) CrO₃2-
C) CrO₃3-
D) CO₂ ^-
E) CO^-

B

The correct name for Mg(ClO3)2 is ________.
A) magnesium chlorate
B) manganese chlorate
C) magnesium chloroxide
D) magnesium perchlorate
E) manganese perchlorate

A

What is the correct formula for ammonium sulfide?
A) NH4SO3
B) (NH4)2SO4
C) (NH4)2S
D) NH3S
E) N2S3

C

When calcium reacts with sulfur the compound formed is ________.
A) Ca2S2
B) Ca3S2
C) CaS
D) CaS2
E) Ca2S3

C

Chromium and chlorine form an ionic compound whose formula is CrCl3. The name of this compound is ________.
A) chromium chlorine
B) chromium (III) chloride
C) monochromium trichloride
D) chromium (III) trichloride
E) chromic trichloride

B

Iron and chlorine form an ionic compound whose formula is FeCl3. The name of this compound is ________.
A) iron chlorine
B) iron (III) chloride
C) moniron trichloride
D) iron (III) trichloride
E) ferric trichloride

B

Copper and chlorine form an ionic compound whose formula is CuCl2. The name of this compound is ________.
A) copper chlorine
B) copper (III) dichloride
C) monocopper dichloride
D) copper (II) dichloride
E) cupric chloride

E

The name of the binary compound N2O4 is ________.
A) nitrogen oxide
B) nitrous oxide
C) nitrogen (IV) oxide
D) dinitrogen tetroxide
E) oxygen nitride

D

The formula for zinc phosphate is Zn3(PO4)2. What is the formula for cadmium arsenate?
A) Cd4(AsO2)3
B) Cd3(AsO4)2
C) Cd3(AsO3)4
D) Cd2(AsO4)3
E) Cd2(AsO4)4

B

The formula for aluminum hydroxide is ________.
A) AlOH
B) Al3OH
C) Al2(OH)3
D) Al(OH)3
E) Al2O3

D

The name of the ionic compound V2O3 is ________.
A) vanadium (III) oxide
B) vanadium oxide
C) vanadium (II) oxide
D) vanadium (III) trioxide
E) divanadium trioxide

A

The name of the ionic compound NH4CN is ________.
A) nitrogen hydrogen cyanate
B) ammonium carbonitride
C) ammonium cyanide
D) ammonium hydrogen cyanate
E) cyanonitride

C

The name of the ionic compound (NH4)3PO4 is ________.
A) ammonium phosphate
B) nitrogen hydrogen phosphate
C) tetrammonium phosphate
D) ammonia phosphide
E) triammonium phosphate

A

What is the formula for perchloric acid?
A) HClO
B) HClO3
C) HClO4
D) HClO2
E) HCl

C

The correct name for HIO2 is ________.
A) hypoiodic acid
B) hydriodic acid
C) periodous acid
D) iodous acid
E) periodic acid

D

What is the molecular formula for propane?
A) C2H8
B) C3H6
C) C3H8
D) C4H8
E) C4H10

C

What is the molecular formula for butane?
A) C2H8
B) C3H6
C) C3H8
D) C4H8
E) C4H10

E

What are the primary atoms found in alkanes?
A) carbon, hydrogen, and oxygen
B) carbon and nitrogen
C) oxygen and hydrogen
D) carbon and oxygen
E) carbon and hydrogen

E

What is the correct name for the following alkane, C5H12?
A) heptane
B) propane
C) hexane
D) pentane
E) butane

D

How many carbon and hydrogen atoms are found in decane?
A) 10 carbons and 22 hydrogens
B) 9 carbons and 20 hydrogens
C) 10 carbons and 20 hydrogens
D) 9 carbons and 18 hydrogens
E) 10 carbons and 24 hydrogens

A

What is the molecular formula for heptane?
A) C6H12
B) C6H14
C) C7H14
D) C7H16
E) C7H18

D

What is the molecular formula for 1-hexanol?
A) C6H13O
B) C6H14O
C) C6H15O
D) C7H14O
E) C7H15O

B

A certain mass of carbon reacts with 128 g of oxygen to form carbon monoxide. ________ grams of oxygen would react with that same mass of carbon to form carbon dioxide, according to the law of multiple proportions.
A) 25.6
B) 64.0
C) 128
D) 1280
E) 256

E

An atom of 1³C contains ________ protons.
A) 6
B) 19
C) 7
D) 9
E) 13

A

Of the following, the subatomic particle with the smallest mass is the ________.
A) proton
B) neutron
C) electron
D) alpha particle
E) isotope

C

An atom of ¹¹⁸Xe contains ________ neutrons.
A) 54
B) 172
C) 64
D) 110
E) 118

C

There are ________ protons, ________ electrons, and ________ neutrons in an atom of Xe.
A) 129, 129, 129
B) 129, 129, 75
C) 54, 75, 129
D) 54, 54, 75
E) 54, 54, 129

D

An atom of ¹⁴C contains ________ electrons.
A) 14
B) 20
C) 8
D) 10
E) 6

E

87 pm is the same as ________ Angstroms.
A) 870
B) 8.7
C) 87
D) .87
E) .087

D

200 pm is the same as ________ Å.
A) 2000
B) 20
C) 200
D) 2
E) 0.0002

D

In the symbol below, X = ________.
⁴⁰ ₁₉X
A) Zr
B) K
C) Sc
D) Br
E) not enough information to determine

B

In the symbol below, x = ________.
^X ₁₇Cl
A) 17
B) 34
C) 16
D) 36
E) not enough information to determine

E

The mass number of an atom of ¹⁴C is ________.
A) 6
B) 20
C) 8
D) 14
E) 10

D

Which atom has the largest number of neutrons?
A) silicon-30
B) sulfur-36
C) argon-38
D) calcium-44
E) magnesium-24

D

How many neutrons are there in one atom of ¹⁸⁴W?
A) 74
B) 112
C) 258
D) 110
E) 184

D

How many protons are there in one atom of ⁷¹Ga?
A) 40
B) 70
C) 71
D) 31
E) 13

D

How many electrons are there in one atom of ⁷¹Ga?
A) 40
B) 70
C) 71
D) 31
E) 13

D

Which pair of atoms constitutes a pair of isotopes of the same element?

B

The atomic number of an atom of ⁸⁰Br is ________.
A) 115
B) 35
C) 45
D) 73
E) 80

B

How many total electrons are in the Li+ ion?
A) 2
B) 3
C) 4
D) 7
E) 8

A

How many total electrons are in the O^2- ion?
A) 10
B) 8
C) 6
D) 16
E) 4

A

If a iron atom loses 2 electrons to make an ion, what is the charge on that ion?
A) 2+
B) 1+
C) 3+
D) 2-
E) 1-

A

If an atom gains 3 electrons to make an ion, what is the charge on that ion?
A) 3+
B) 1+
C) 2+
D) 1-
E) 3-

E

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) 33.333
B) 220.40
C) 220.24
D) 219.00
E) 219.67

B

The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu.

A) 159.4
B) 162.0
C) 163.1
D) 161.5
E) 163.0

B

The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu.

A) 52.62
B) 56.14
C) 55.70
D) 55.40
E) 55.74

B

The element ________ is the most similar to helium in chemical and physical properties.
A) O
B) Mg
C) Be
D) Ar
E) Sr

D

Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties?
A) Li, F
B) Sr, Te
C) O, S
D) In, Sb
E) Ti, Ne

C

Which one of the following is a metalloid?
A) Se
B) Hf
C) Zr
D) Xe
E) Si

E

The element lithium is in a group known as the ________.
A) transition metals
B) alkaline earth metals
C) noble gases
D) halogens
E) alkali metals

E

The element chlorine is in a group known as the ________.
A) transition metals
B) noble gases
C) alkali metals
D) alkaline earth metals
E) halogens

E

The element calcium is in a group known as the ________.
A) transition metals
B) alkali metals
C) halogens
D) noble gases
E) alkaline earth metals

E

Of the following, only ________ is not a metalloid.
A) B
B) Po
C) Si
D) Ge
E) As

B

Which of the following elements is a nonmetal?
A) At
B) Rh
C) Tc
D) Mo
E) Zr

A

Which one of the following will occur as diatomic molecules in elemental form?
A) helium
B) argon
C) chlorine
D) phosphorous
E) sodium

C

How many electrons does the Al³⁺ ion possess?
A) 16
B) 10
C) 6
D) 0
E) 13

B

How many protons does the Br- ion possess?
A) 34
B) 36
C) 6
D) 8
E) 35

E

Which one of the following is most likely to gain electrons when forming an ion?
A) Mn
B) Zn
C) F
D) Li
E) Al

C

The formula of a salt is XCl2 . The X-ion in this salt has 24 electrons. The metal X is ________.
A) Ni
B) Fe
C) Zn
D) Cr
E) Ti

B

Predict the charge of the most stable ion of bromine.
A) 2+
B) 1+
C) 3+
D) 1-
E) 2-

D

Predict the charge of the most stable ion of aluminum.
A) 3-
B) 1+
C) 2+
D) 1-
E) 3+

E

Which of the following compounds would you expect to be ionic?
A) C2H6
B) NH3
C) H2O2
D) LiBr
E) None of the above.

D

Which species below is the sulfate ion?
A) CN^-
B) SO₄ ^2-
C) OH^-
D) SO₃ ^2-
E) None of the above

B

Which species below is the nitrate ion?
A) NO2-
B) NO3-
C) ClO3-
D) ClO4-
E) MnO4-

B

Which species below is the chromate ion?
A) Cr₂O₇ ^2-
B) CrO₄ ^2-
C) CH₃COO^-
D) CO₃ ^2-
E) None of the above

B

The correct name for CaO is ________.
A) calcium oxide
B) calcium hydroxide
C) calcium peroxide
D) calcium monoxide
E) calcium dioxide

A

Element M reacts with fluorine to form an ionic compound with the formula M . The M-ion has 21 electrons. Element M is ________.
A) Al
B) Cr
C) Mn
D) Fe
E) Sc

B

The charge on the copper ion in the salt CuO is ________.
A) +1
B) +2
C) +4
D) +3
E) +5

B

The charge on the silver ion in the salt AgCl is ________.
A) +2
B) +1
C) +3
D) +4
E) +5

B

The name of the ionic compound NaBrO4 is ________.
A) sodium perbromate
B) sodium bromate
C) sodium hypobromate
D) sodium perbromite
E) sodium bromide

A

When a bromine atom forms the bromide ion, it has the same charge as the ________ ion.
A) sulfide
B) ammonium
C) nitrate
D) phosphate
E) sulfite

C

Which element forms an ion with the same charge as the sulfate ion?
A) magnesium
B) sodium
C) fluorine
D) vanadium
E) sulfur

E

The correct name for Na2O2 is ________.
A) sodium oxide
B) sodium dioxide
C) disodium dioxide
D) sodium peroxide
E) disodium oxide

D

Which metal is not required to have its charge specified in the names of ionic compounds it forms?
A) Cr
B) Ni
C) Zr
D) Na
E) Mo

D

The following hypothetical element : x : can be found in which group on the periodic table?

VIA

Which element is found in Period 2 and Group VIIA?

fluorine

The formula for potassium sulfide is ________.

K₂S

What is the name of an alcohol derived from hexane?

hexanol

The possible oxidation numbers for iron are +1 and +2.

false

The formula for chromium (II) iodide is CrI2.

true

H2SeO4 is called selenic acid.

true

The correct name for Na3N is sodium azide.

false