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186 Cards in this Set

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2 Which particle has the least mass?

(1) alpha particle (2) beta particle
(3) neutron (4) proton
(2) beta particle
3 A sample of matter must be copper if
(1) each atom in the sample has 29 protons (2) atoms in the sample react with oxygen (3) the sample melts at 1768 K
(4) the sample can conduct electricity
(1) each atom in the sample has 29 protons
In the electron cloud model of the atom, an orbital is defined as the most probable
(1) charge of an electron
(2) conductivity of an electron (3) location of an electron
(4) mass of an electron
(3) location of an electron
The elements on the Periodic Table are arranged in order of increasing
(1) atomic number
(2) mass number
(3) number of isotopes (4) number of moles
(1) atomic number
Which element has the highest melting point?

(1) tantalum (2) rhenium
(3) osmium (4) hafnium
(2) rhenium
In a chemical reaction, there is conservation of
(1) energy, volume, and mass (2) energy, volume, and charge (3) mass, charge, and energy (4) mass, charge, and volume
(3) mass, charge, and energy
At STP, both diamond and graphite are solids composed of carbon atoms. These solids have
(1) the same crystal structure and the same properties
(2) the same crystal structure and different properties
(3) different crystal structures and the same properties
(4) different crystal structures and different properties
(4) different crystal structures and different properties
The gram-formula mass of a compound is 48 grams. The mass of 1.0 mole of this compound is

(1) 1.0 g (2) 4.8 g
(3) 48 g (4) 480 g
(3) 48 g
Given the balanced equation representing a reaction:
Cl2 →Cl+Cl What occurs during this reaction?
(1) A bond is broken as energy is absorbed. (2) A bond is broken as energy is released. (3) A bond is formed as energy is absorbed. (4) A bond is formed as energy is released.
(1) A bond is broken as energy is absorbed.
Which atom has the weakest attraction for the electrons in a bond with an H atom?
(1) Cl atom (3) O atom (2) F atom (4) S atom
(4) S atom
Which substance can not be broken down by a chemical change?

(1) ammonia (2) mercury
(3) propane (4) water
(2) mercury
At standard pressure, how do the boiling point and the freezing point of NaCl(aq) compare to the boiling point and the freezing point of H2O(l)?
(1) Both the boiling point and the freezing point of NaCl(aq) are lower.
(2) Both the boiling point and the freezing point of NaCl(aq) are higher.
(3) The boiling point of NaCl(aq) is lower, and the freezing point of NaCl(aq) is higher.
(4) The boiling point of NaCl(aq) is higher, and
the freezing point of NaCl(aq) is lower.
(4) The boiling point of NaCl(aq) is higher, and
the freezing point of NaCl(aq) is lower.
The temperature of a sample of matter is a measure of the
(1) average kinetic energy of its particles (2) average potential energy of its particles (3) total kinetic energy of its particles
(4) total potential energy of its particles
(1) average kinetic energy of its particles
According to the kinetic molecular theory, the particles of an ideal gas
(1) have no potential energy
(2) have strong intermolecular forces
(3) are arranged in a regular, repeated geometric
pattern
(4) are separated by great distances, compared
to their size
(4) are separated by great distances, compared
to their size
Giventheequationrepresentingaclosedsystem:
N2O4(g) 2NO2(g)
Which statement describes this system at equilibrium?
(1) The volume of the NO2(g) is greater than the volume of the N2O4(g).
(2) The volume of the NO2(g) is less than the volume of the N2O4(g).
(3) The rate of the forward reaction and the rate of the reverse reaction are equal.
(4) The rate of the forward reaction and the rate of the reverse reaction are unequal.
(3) The rate of the forward reaction and the rate of the reverse reaction are equal.
In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is equal to the:

(1) activation energy (2) kinetic energy
(3) heat of reaction (4) rate of reaction
(3) heat of reaction
For a given chemical reaction, the addition of a catalyst provides a different reaction pathway that
(1) decreases the reaction rate and has a higher activation energy
(2) decreases the reaction rate and has a lower activation energy
(3) increases the reaction rate and has a higher activation energy
(4) increases the reaction rate and has a lower activation energy
(4) increases the reaction rate and has a lower activation energy
Which atoms can bond with each other to form chains, rings, or networks?
(1) carbon atoms (3) oxygen atoms (2) hydrogen atoms (4) nitrogen atoms
(1) carbon atoms
Amoleculeofanunsaturatedhydrocarbonmust have
(1) at least one single carbon-carbon bond
(2) at least one multiple carbon-carbon bond (3) two or more single carbon-carbon bonds (4) two or more multiple carbon-carbon bonds
(2) at least one multiple carbon-carbon bond
Which statement describes where the oxidation and reduction half-reactions occur in an operating electrochemical cell?

1. Oxidation and reduction both occur at the anode
2. Oxidation and reduction both occur at the cathode
3. Oxidation occurs at the anode, and reduction occurs at the cathode.
4. Oxication occurs at the cathode and reduction occurs at the anode.
3. Oxidation occurs at the anode, and reduction occurs at the cathode.
Potassium hydroxide is classified as an Arrhenius base because KOH contains
(1) OH− ions (3) K+ ions (2) O2− ions (4) H+ ions
(1) OH− ions
Energy is released during the fission of Pu-239
atoms as a result of the
(1) formation of covalent bonds (2) formation of ionic bonds
(3) conversion of matter to energy (4) conversion of energy to matter
(3) conversion of matter to energy
Atoms of I-131 spontaneously decay when the
(1) stable nuclei emit alpha particles (2) stable nuclei emit beta particles
(3) unstable nuclei emit alpha particles (4) unstable nuclei emit beta particles
(4) unstable nuclei emit beta particles
Compared to the atoms of nonmetals in Period 3, the atoms of metals in Period 3 have
(1) fewer valence electrons (2) more valence electrons (3) fewer electron shells (4) more electron shells
(1) fewer valence electrons
Which elements are malleable and good conductors of electricity?
(1) iodine and silver (3) tin and silver (2) iodine and xenon (4) tin and xenon
(3) tin and silver
Which atom in the ground state requires the least amount of energy to remove its valence electron?

1) lithium atom (2) potassium atom (3)Rubidium atom
(4) sodium atom
(2) Fe2S3
What is the percent composition by mass of sulfur in the compound MgSO4 (gram-formula mass = 120. grams per mole)?
(1) 20.% (3) 46% (2) 27% (4) 53%
(2) 27%
Which compound becomes less soluble in water as the temperature of the solution is increased?

(1) HCl (2) KCl
(3) NaCl (4) NH4Cl
(1) HCl
Given the balanced equation representing a reaction:
2H2 + O2 → 2H2O
What is the mass of H2O produced when 10.0 grams of H2 reacts completely with 80.0 grams of O2?
(1) 70.0 g (3) 180. g (2) 90.0 g (4) 800. g
(2) 90.0 g
Given the balanced equation representing a reaction:
Zn(s)+H SO (aq)→ZnSO (aq)+H (g) 2442
Which type of reaction is represented by this equation?
(1) decomposition (3) single replacement (2) double replacement (4) synthesis
(3) single replacement
In a laboratory where the air temperature is 22°C, a steel cylinder at 100.°C is submerged in a sample of water at 40.°C. In this system, heat flows from
35 What is the percent composition by mass of sulfur in the compound MgSO4 (gram-formula mass = 120. grams per mole)?
(1) 20.% (3) 46% (2) 27% (4) 53%
36 Which compound becomes less soluble in water as the temperature of the solution is increased?
38
CH3
Which statement describes these formulas?
(1) HCl (2) KCl
(3) NaCl (4) NH4Cl
40
(1) (2) (3)
(4)
both the air and the water to the cylinder both the cylinder and the air to the water the air to the water and from the water to the cylinder
the cylinder to the water and from the water to the air
(4)the cylinder to the water and from the water to the air
Which temperature change would cause a sample of an ideal gas to double in volume while the pressure is held constant?
(1) from 400. K to 200. K (2) from 200. K to 400. K (3) from 400.°C to 200.°C (4) from 200.°C to 400.°C
(2) from 200. K to 400. K
A 36-gram sample of water has an initial temperature of 22°C. After the sample absorbs 1200 joules of heat energy, the final temperature of the sample is
47 Which solution reacts with LiOH(aq) to produce a salt and water?
48 Which volume of 2.0MNaOH(aq)is needed to completely neutralize 24 milliliters of 1.0 M HCl(aq)?
(1) 8.0°C (2) 14°C
(3) 30.°C (4) 55°C
(2) 12 mL
Which type of reaction releases the greatest amount of energy per mole of reactant?
(1) combustion
(2) decomposition
(3) nuclear fusion
(4) oxidation-reduction
(3) nuclear fusion
Potassium hydroxide is classified as an Arrhenius base because KOH contains
(1) OH− ions (3) K+ ions (2) O2− ions (4) H+ ions
(1) OH− ions
In which laboratory process is a volume of solution of known concentration used to determine the concentration of another solution?
(1) deposition (2) distillation
(3) filtration (4) titration
(4) titration
Which energy conversion occurs in an operating electrolytic cell?
(1) chemical energy to electrical energy (2) electrical energy to chemical energy (3) nuclear energy to thermal energy (4) thermal energy to nuclear energy
2) electrical energy to chemical energy
Whichcompoundscanbeclassifiedaselectrolytes?
(1) alcohols
(2) alkynes
(3) organic acids
(4) saturated hydrocarbons
(3) organic acids
What is the total number of valence electrons in a calcium atom in the ground state?
(1) 8 (3) 18 (2) 2 (4) 20
2) 2
Which subatomic particles are located in the nucleus of an He-4 atom?
(1) electrons and neutrons
(2) electrons and protons
(3) neutrons and protons
(4) neutrons, protons, and electrons
(3) neutrons and protons
Inthelate1800s,experimentsusingcathoderay tubes led to the discovery of the
(1) electron (3) positron (2) neutron (4) proton
1) electron
The atomic mass of titanium is 47.88 atomic mass units. This atomic mass represents the
(1) total mass of all the protons and neutrons in an atom of Ti
(2) total mass of all the protons, neutrons, and electrons in an atom of Ti
(3) weighted average mass of the most abundant isotope of Ti
(4) weighted average mass of all the naturally occurring isotopes of Ti
(4) weighted average mass of all the naturally occurring isotopes of Ti
Anatomofwhichelementhasthelargestatomic radius?

(1) Fe (2) Mg
(3) Si (4) Zn
(2) Mg
Which element requires the least amount of energy to remove the most loosely held electron from a gaseous atom in the ground state?
(1) bromine (3) sodium (2) calcium (4) silver
(3) sodium
A balanced equation representing a chemical reaction can be written using
(1) chemical formulas and mass numbers
(2) chemical formulas and coefficients
(3) first ionization energies and mass numbers (4) first ionization energies and coefficients
(2) chemical formulas and coefficients
Every water molecule has two hydrogen atoms bonded to one oxygen atom. This fact supports the concept that elements in a compound are
(1) chemically combined in a fixed proportion
(2) chemically combined in proportions that
vary
(3) physically mixed in a fixed proportion
(4) physically mixed in proportions that vary
(1) chemically combined in a fixed proportion
Which Group 15 element exists as diatomic
molecules at STP?
(1) phosphorus (3) bismuth (2) nitrogen (4) arsenic
(2) nitrogen
What is the total number of electrons shared in a double covalent bond?
(1) 1 (3) 3 (2) 2 (4) 4
(4) 4
Given the balanced equation representing a reaction:
Br2 +energy→Br+Br
Which statement describes the energy change and
bonds in this reaction?
(1) Energy is released as bonds are broken. (2) Energy is released as bonds are formed. (3) Energy is absorbed as bonds are broken. (4) Energy is absorbed as bonds are formed.
(3) Energy is absorbed as bonds are broken.
Which substance can not be broken down by a chemical change?
18
19
20
21
Which gas sample at STP has the same total number of molecules as 2.0 liters of CO2(g) at STP?
(1) 5.0 L of CO2(g) (2) 2.0 L of Cl2(g)
(3) 3.0 L of H2S(g) (4) 6.0 L of He(g)
(1) methane (2) propanal
(3) tungsten (4) water
(3) tungsten
Object A at 40.°C and object B at 80.°C are placed in contact with each other. Which statement describes the heat flow between the objects?
(1) Heat flows from object A to object B.
(2) Heat flows from object B to object A.
(3) Heat flows in both directions between the
objects.
(4) No heat flow occurs between the objects.
(2) Heat flows from object B to object A.
Which unit can be used to express the concentration of a solution?

(1) L/s (2) J/g
(3) ppm (4) kPa
(3) ppm
Petroleum can be separated by distillation because the hydrocarbons in petroleum are
(1) elements with identical boiling points (2) elements with different boiling points (3) compounds with identical boiling points (4) compounds with different boiling points
(4) compounds with different boiling points
Which compound is insoluble in water?
1) KOH (2) NH4Cl
(3) Na3PO4 (4) PbSO4
(4) PbSO4
TheisotopesK-37andK-42havethesame
(1) decay mode
(2) bright-line spectrum
(3) mass number for their atoms
(4) total number of neutrons in their atoms
(2) bright-line spectrum
Which element is present in all organic compounds?

(1) carbon (2) hydrogen
(3) nitrogen (4) oxygen
(1) carbon
Which energy conversion occurs during the operation of an electrolytic cell?
(1) chemical energy to electrical energy (2) electrical energy to chemical energy (3) nuclear energy to electrical energy (4) electrical energy to nuclear energy
(2) electrical energy to chemical energy
Which compound is an Arrhenius acid? (1) CaO (3) K2O
(2) HCl (4) NH3
(2) HCl
Based on the results of testing colorless solutions with indicators, which solution is most acidic?
(1) a solution in which bromthymol blue is blue (2) a solution in which bromcresol green is blue (3) a solution in which phenolphthalein is pink (4) a solution in which methyl orange is red
(4) a solution in which methyl orange is red
Accordingtooneacid-basetheory,wateractsas an acid when an H2O molecule
(1) accepts an H+ (3) accepts an H− (2) donates an H+ (4) donates an H−
(2) donates an H+
In which type of reaction is an atom of one element converted to an atom of a different element?
(1) decomposition (2) neutralization
(3) saponification (4) transmutation
(4) transmutation
Which nuclide is listed with its half-life and decay mode?
(1) K-37, 1.24 h, α
(2) N-16, 7.2 s, β−
(3) Rn-222, 1.6 × 103 y, α (4) U-235, 7.1 × 108 y, β−
(2) N-16, 7.2 s, β−
The greatest composition by mass in an atom
of 17O is due to the total mass of its 8
(1) electrons (3) positrons (2) neutrons (4) protons
(2) neutrons
The bond between which two atoms is most polar?

(1) BrandCl (2) BrandF
(3) IandCl (4) I and F
(4) IandF
In the formula X2(SO4)3, the X represents a metal. This metal could be located on the Periodic Table in
(1) Group 1 (2) Group 2
(3) Group 13 (4) Group 14
(3) Group 13
At STP, which element is solid, brittle, and a poor conductor of electricity?
(1) Al (2) K
(3) Ne (4) S
(4) S
Given the balanced equation representing a reaction:
2NaCl(l) → 2Na(l) + Cl2(g)
A 1170.-gram sample of NaCl(l) completely reacts, producing 460. grams of Na(l). What is the total mass of Cl2(g) produced?
(1) 355 g (3) 1420. g (2) 710. g (4) 1630. g
(2) 710. g
Which element forms an ionic compound when it reacts with lithium?

1) K (2) Fe
(3) Kr (4) Br
(4) Br
Given the formula representing a molecule:
HCCH The molecule is
(1) symmetrical and polar
(2) symmetrical and nonpolar (3) asymmetrical and polar
(4) asymmetrical and nonpolar
(2) symmetrical and nonpolar
Which compound has both ionic and covalent bonds?
(1) CO2
(2) CH3OH
(3) NaI
(4) Na2CO3
(4) Na2CO3
A cylinder with a movable piston contains a sample of gas having a volume of 6.0 liters at 293 K and 1.0 atmosphere. What is the volume of the sample after the gas is heated to 303 K, while the pressure is held at 1.0 atmosphere?
(1) 9.0 L (3) 5.8 L (2) 6.2 L (4) 4.0 L
(2) 6.2 L
What is the minimum amount of heat required to completely melt 20.0 grams of ice at its melting point?

(1) 20.0 J (2) 83.6 J
(3) 6680 J (4) 45 200 J
3) 6680
Asthetemperatureofachemicalreactioninthe gas phase is increased, the rate of the reaction increases because
(1) fewer particle collisions occur
(2) more effective particle collisions occur
(3) the required activation energy increases
(4) the concentration of the reactants increases
(2) more effective particle collisions occur
The entropy of a sample of CO2 increases as the CO2 changes from
(1) gas to liquid (3) liquid to solid (2) gas to solid (4) solid to gas
(4) solid to gas
Which two factors must be equal when a chemical reaction reaches equilibrium?
(1) the concentration of the reactants and the concentration of the products
(2) the number of reactant particles and the number of product particles
(3) the rate of the forward reaction and the rate of the reverse reaction
(4) the mass of the reactants and the mass of the products
(3) the rate of the forward reaction and the rate of the reverse reaction
46 Which formula represents an unsaturated hydrocarbon?
(1) C5H12 (3) C7H16 (2) C6H14 (4) C8H14
(4) C8H14
The reaction between an organic acid and an alcohol produces
(1) an aldehyde (2) a ketone
(3) an ether (4) an ester
Which balanced equation represents a redox reaction?
(1) AgNO3(aq)+NaCl(aq)→AgCl(s)+NaNO3(aq) (2) H2CO3(aq) → H2O(l) + CO2(g)
(3) NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) (4) Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
(4) Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)
A solution with a pH of 2.0 has a hydronium ion concentration ten times greater than a solution with a pH of
(1) 1.0 (3) 3.0 (2) 0.20 (4) 20.
(3) 3.0
Which isotope is used to treat cancer?
(1) C-14 (3) Co-60 (2) U-238 (4) Pb-206
(3) Co-60
An orbital is a region of space where there is a high probability of finding
(1) a proton (3) a neutron (2) a positron (4) an electron
(4) an electron
Which statement matches a subatomic particle with its charge?
(1) A neutron has a negative charge. (2) A proton has a negative charge. (3) A neutron has no charge.
(4) A proton has no charge.
3) A neutron has no charge.
An atom of any element must contain
(1) an equal number of protons and neutrons (2) an equal number of protons and electrons (3) more electrons than neutrons
(4) more electrons than protons
(2) an equal number of protons and electrons
Which statement compares the masses of two subatomic particles?
(1) The mass of an electron is greater than the mass of a proton.
(2) The mass of an electron is greater than the mass of a neutron.
(3) The mass of a proton is greater than the mass of an electron.
(4) The mass of a proton is greater than the mass of a neutron.
(3) The mass of a proton is greater than the mass of an electron.
Thebright-linespectrumofsodiumisproduced when energy is
(1) absorbed as electrons move from higher to lower electron shells
(2) absorbed as electrons move from lower to higher electron shells
(3) released as electrons move from higher to lower electron shells
(4) released as electrons move from lower to higher electron shells
(3) released as electrons move from higher to lower electron shells
The valence electrons of a germanium atom in the ground state are located in the
(1) first shell (3) third shell (2) second shell (4) fourth shell
(4) fourth shell
The elements on the Periodic Table are arranged in order of increasing
(1) atomic mass
(2) atomic number
(3) first ionization energy (4) selected oxidation state
2) atomic number
Which list of elements contains a metal, a metalloid, a nonmetal, and a noble gas?
(1) Be, Si, Cl, Kr (3) K, Fe, B, F (2) C,N,Ne,Ar (4) Na,Zn,As,Sb
(1) Be, Si, Cl, Kr
Thetwoformsofoxygen,O2(g)andO3(g),have
(1) different molecular structures and identical properties
(2) different molecular structures and different properties
(3) identical molecular structures and identical properties
(4) identical molecular structures and different properties
different molecular structures and different properties
The sum of the atomic masses of the atoms in one molecule of C3H6Br2 is called the
(1) formula mass
(2) isotopic mass
(3) percent abundance (4) percent composition
1) formula mass
What is the total number of electron pairs shared between the two atoms in an O2 molecule?
(1) 1 (3) 6 (2) 2 (4) 4
(2) 2
When an atom of lithium loses an electron, the atom becomes a
(1) negative ion with a radius smaller than the radius of the atom
(2) negative ion with a radius larger than the radius of the atom
(3) positive ion with a radius smaller than the radius of the atom
(4) positive ion with a radius larger than the radius of the atom
(3) positive ion with a radius smaller than the radius of the atom
Given the balanced equation representing a reaction:
2NaCl → 2Na + Cl2

To break the bonds in NaCl, the reactant must

(1) absorb energy (2) create energy
(3) destroy energy (4) release energy
(1) absorb energy
A molecular compound is formed when a chemical reaction occurs between atoms of
(1) chlorine and sodium (2) chlorine and yttrium (3) oxygen and hydrogen (4) oxygen and magnesium
(3) oxygen and hydrogen
Which substance can not be broken down by chemical means?
(1) ammonia (2) antimony
(3) methane (4) water
(2) antimony
The gold foil experiment led to the conclusion that each atom in the foil was composed mostly of empty space because most alpha particles directed at the foil
(1) passed through the foil
(2) remained trapped in the foil
(3) were deflected by the nuclei in gold atoms
(4) were deflected by the electrons in gold
atoms
(1) passed through the foil
Which subatomic particles are located in the nucleus of a carbon atom?
(1) protons, only
(2) neutrons, only
(3) protons and neutrons (4) protons and electrons
3
Which part of a helium atom is positively charged?
(1) electron (2) neutron
(3) nucleus (4) orbital
3
The mass of a proton is approximately equal to the mass of
1) an alpha particle (2) an electron
(3) a neutron (4) a positron
3
At STP, solid carbon can exist as diamond and graphite. Compared to the molecular structure and chemical properties of diamond, graphite has
(1) a different molecular structure and different properties
(2) a different molecular structure and the same properties
(3) the same molecular structure and different properties
(4) the same molecular structure and the same properties
1
Which Group 14 element is classified as a metal?

(1) carbon
(2) germanium
(3) silicon (4) tin
4
The light emitted from a flame is produced when electrons in an excited state
(1) absorb energy as they move to lower energy states
(2) absorb energy as they move to higher energy states
(3) release energy as they move to lower energy states
(4) release energy as they move to higher energy states
3
An atom of which element has the greatest attraction for electrons in a chemical bond

(1) As (2) Ga
(3) Ge (4) Se
4
Which formula represents a polar molecule? (1) H2 (3) CO2
(2) H2O (4) CCl4
2
Twocategoriesofcompoundsare
(1) covalent and molecular (2) covalent and metallic (3) ionic and molecular
(4) ionic and metallic
3
Which type of bond is found between atoms of solid cobalt?

(1) nonpolar covalent (2) polar covalent
(3) metallic (4) ionic
3
Which equation represents sublimation? (1) I2(s) → I2(g) (3) I2(l) → I2(g)
(2) I2(s) → I2(l) (4) I2(l) → I2(s)
1
Which sample of ethanol has particles with the
highest average kinetic energy?
(1) 10.0 mL of ethanol at 25°C (2) 10.0 mL of ethanol at 55°C (3) 100.0 mL of ethanol at 35°C (4) 100.0 mL of ethanol at 45°C
2
The molarity of an aqueous solution of NaCl is defined as the
(1) grams of NaCl per liter of water (2) grams of NaCl per liter of solution (3) moles of NaCl per liter of water (4) moles of NaCl per liter of solution
4
A real gas behaves least like an ideal gas under the conditions of
(1) low temperature and low pressure (2) low temperature and high pressure (3) high temperature and low pressure (4) high temperature and high pressure
2
Which sample of matter can be separated into different substances by physical means?

(1) LiCl(aq) (2) LiCl(s)
(3) NH3(g) (4) NH3(l)
1
At STP, 1.0 liter of helium contains the same total number of atoms as
(1) 1.0LofNe (3) 0.5LofRn (2) 2.0LofKr (4) 1.5LofAr
1
Which statement describes the particles of an ideal gas?
(1) The particles move in well-defined, circular paths.
(2) When the particles collide, energy is lost.
(3) There are forces of attraction between the
particles.
(4) The volume of the particles is negligible.
4
Giventheequationrepresentingaphasechange at equilibrium:
H2O(s)
4
A molecule of an organic compound contains at least one atom of:

(1) carbon (2) chlorine
(3) nitrogen (4) oxygen
4
In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is equal to the
(1) activation energy
(2) entropy of the system (3) heat of fusion
(4) heat of reaction
4
A carbon-carbon triple bond is found in a molecule of:

(1) butane (2) butanone
(3) butene (4) butyne
4
Which statement describes one characteristic of an operating electrolytic cell?
(1) It produces electrical energy.
(2) It requires an external energy source.
(3) It uses radioactive nuclides.
(4) It undergoes a spontaneous redox reaction.
2
Which compound when dissolved in water is an Arrhenius acid?

(1) CH3OH (2) HCl
(3) NaCl
2
An acid can be defined as an
(1) H+ acceptor (3) OH− acceptor
(2) H+ donor (4) OH− donor
2
Which nuclear emission has no charge and no
mass?
(1) alpha particle (3) gamma ray (2) beta particle (4) positron
3
During which process can 10.0 milliliters of a 0.05 M HCl(aq) solution be used to determine the unknown concentration of a given volume of NaOH(aq) solution?
(1) evaporation (3) filtration (2) distillation (4) titration
4
Which radioisotope is matched with its decay mode?
(1) H-3 and γ (3) N-16 and α (2) K-42 and β+ (4) P-32 and β−
4
Whichreactionisaccompaniedbythereleaseof the greatest amount of energy?
(1) combustion of 10. g of propane (2) electrolysis of 10. g of water
(3) nuclear fission of 10. g of uranium (4) oxidation of 10. g of iron
3
Whichelementformsacompoundwithchlorine with the general formula MCl?
(1) Rb (3) Re (2) Ra (4) Rn
1
A sample of an element has a mass of 34.261 grams and a volume of 3.8 cubic centimeters. To which number of significant figures should the calculated density of the sample be expressed?

(1) 5 (2) 2
(3) 3 (4) 4
2
Which characteristics both generally decrease when the elements in Period 3 on the Periodic Table are considered in order from left to right?
(1) nonmetallic properties and atomic radius (2) nonmetallic properties and ionization energy (3) metallic properties and atomic radius
(4) metallic properties and ionization energy
3
Which formula is both a molecular and an empirical formula?
(1) C6H12O6 (2) C2H4O2
(3) C3H8O (4) C4H8
3
An atom of argon in the ground state tends not to bond with an atom of a different element because the argon atom has
(1) more protons than neutrons
(2) more neutrons than protons
(3) a total of two valence electrons (4) a total of eight valence electrons
4
Whichcompoundhasthelowestvaporpressure at 50°C?

(1) ethanoic acid (2) ethanol
(3) propanone (4) water
1
A sample of gas confined in a cylinder with a movable piston is kept at constant pressure. The volume of the gas doubles when the temperature of the gas is changed from
(1) 400. K to 200. K (3) 400.°C to 200.°C (2) 200. K to 400. K (4) 200.°C to 400.°C
2
AccordingtoTableF,whichcompoundissoluble in water?
(1) barium phosphate (2) calcium sulfate
(3) silver iodide
(4) sodium perchlorate
4
Given the equation representing a system at equilibrium:
N2(g) + 3H2(g)
4
Which half-reaction equation represents the reduction of an iron(II) ion?
(1) Fe2+ →Fe3+ +e−
(3) Fe3+ +e− →Fe2+
(2) Fe2+ +2e− →Fe
(4) Fe→Fe2+ +2e−
2
Which metal is more active than H2?
(1) Ag (3) Cu (2) Au (4) Pb
(4) Pb
Given the balanced ionic equation representing the reaction in an operating voltaic cell:
Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)
The flow of electrons through the external
circuit in this cell is from the
(1) Cu anode to the Zn cathode (2) Cu cathode to the Zn anode (3) Zn anode to the Cu cathode (4) Zn cathode to the Cu anode
(3) Zn anode to the Cu cathode
Which laboratory test result can be used to determine if KCl(s) is an electrolyte?
(1) pH of KCl(aq)
(2) pH of KCl(s)
(3) electrical conductivity of KCl(aq) (4) electrical conductivity of KCl(s)
(3) electrical conductivity of KCl(aq)
Which compound is produced when HCl(aq) is neutralized by Ca(OH)2(aq)?
(1) CaCl2 (3) HClO (2) CaH2 (4) HClO2
(1) CaCl2
Which nuclides are used to date the remains of a once-living organism?
(1) C-14 and C-12
(2) Co-60 and Co-59
(3) I-131 and Xe-131
(4) U-238 and Pb-206
1
Which two particles have opposite charges?
(1) an electron and a neutron
(2) an electron and a proton
(3) a proton and a neutron
(4) a proton and a positron
2
Which statement describes how an atom in the
ground state becomes excited?
(1) The atom absorbs energy, and one or more
electrons move to a higher electron shell.
(2) The atom absorbs energy, and one or more
electrons move to a lower electron shell.
(3) The atom releases energy, and one or more
electrons move to a higher electron shell.
(4) The atom releases energy, and one or more
electrons move to a lower electron shell.
1
An element that has a low first ionization energy
and good conductivity of heat and electricity is
classified as a
(1) metal (3) nonmetal
(2) metalloid (4) noble gas
1
The chemical properties of calcium are most
similar to the chemical properties of
(1) Ar (3) Mg
(2) K (4) Sc
3
Which element is a liquid at STP?
(1) argon (3) chlorine
(2) bromine (4) sulfur
2
Which statement describes a chemical property
of aluminum?
(1) Aluminum is malleable.
(2) Aluminum reacts with sulfuric acid.
(3) Aluminum conducts an electric current.
(4) Aluminum has a density of 2.698 g/cm3 at
STP.
2
Which element has an atom in the ground state
with a total of three valence electrons?
(1) aluminum (3) phosphorus
(2) lithium (4) scandium
1
Which substance can be broken down by
chemical means?
(1) magnesium (3) mercury
(2) manganese (4) methanol
4
The gram-formula mass of NO2 is defined as the
mass of
(1) one mole of NO2
(2) one molecule of NO2
(3) two moles of NO
(4) two molecules of NO
1
In which type of reaction do two or more
substances combine to produce a single substance?
(1) synthesis
(2) decomposition
(3) single replacement
(4) double replacement
1
Which formula represents a nonpolar molecule?
(1) HCl (3) NH3
(2) H2O (4) CH4
4
Which symbol represents an atom in the ground
state with the most stable valence electron
configuration?
(1) B (3) Li
(2) O (4) Ne
4
Which element has an atom with the greatest
tendency to attract electrons in a chemical
bond?
(1) carbon (3) silicon
(2) chlorine (4) sulfur
2
The nitrogen atoms in a molecule of N2 share a
total of
(1) one pair of electrons
(2) one pair of protons
(3) three pairs of electrons
(4) three pairs of protons
3
An ionic compound is formed when there is a
reaction between the elements
(1) strontium and chlorine
(2) hydrogen and chlorine
(3) nitrogen and oxygen
(4) sulfur and oxygen
1
Which compound has both ionic and covalent
bonding?
(1) CaCO3 (3) CH3OH
(2) CH2Cl2 (4) C6H12O6
1
The liquids hexane and water are placed in a test
tube. The test tube is stoppered, shaken, and
placed in a test tube rack. The liquids separate
into two distinct layers because hexane and
water have different
(1) formula masses
(2) molecular polarities
(3) pH values
(4) specific heats
2
Which statement describes the particles of an
ideal gas based on the kinetic molecular theory?
(1) The gas particles are relatively far apart and
have negligible volume.
(2) The gas particles are in constant, nonlinear
motion.
(3) The gas particles have attractive forces
between them.
(4) The gas particles have collisions without
transferring energy.
1
Under which conditions of temperature and
pressure would a 1-liter sample of a real gas
behave most like an ideal gas?
(1) 100 K and 0.1 atm
(2) 100 K and 10 atm
(3) 500 K and 0.1 atm
(4) 500 K and 10 atm
3
Which type of energy is associated with the
random motion of the particles in a sample of
gas?
(1) chemical energy
(2) electromagnetic energy
(3) nuclear energy
(4) thermal energy
4
The particles in which sample of LiCl(s) have
the same average kinetic energy as the particles
in a 2.0-mole sample of H2O() at 25°C?
(1) 1.0 mol at 75°C
(2) 2.0 mol at 50.°C
(3) 3.0 mol at 25°C
(4) 4.0 mol at 0°C
3
Which rigid cylinder contains the same number
of gas molecules at STP as a 2.0-liter rigid
cylinder containing H2(g) at STP?
(1) 1.0-L cylinder of O2(g)
(2) 2.0-L cylinder of CH4(g)
(3) 1.5-L cylinder of NH3(g)
(4) 4.0-L cylinder of He(g)
2
Hydrogen bonding is a type of
(1) strong covalent bond
(2) weak ionic bond
(3) strong intermolecular force
(4) weak intermolecular force
3
The data collected from a laboratory titration
are used to calculate the
(1) rate of a chemical reaction
(2) heat of a chemical reaction
(3) concentration of a solution
(4) boiling point of a solution
3
When one compound dissolves in water, the
only positive ion produced in the solution is
H3O+(aq). This compound is classified as
(1) a salt
(2) a hydrocarbon
(3) an Arrhenius acid
(4) an Arrhenius base
3
Which nuclear emission has the greatest mass
and the least penetrating power?
(1) an alpha particle (3) a neutron
(2) a beta particle (4) a positron
1
Which radioisotope has an atom that emits a
particle with a mass number of 0 and a charge of
+1?
(1) 3H (3) 19Ne
(2) 16N (4) 239Pu
3
In which type of reaction do two lighter nuclei
combine to form one heavier nucleus?
(1) combustion (3) nuclear fission
(2) reduction (4) nuclear fusion
4
For which compound is the process of dissolving
in water exothermic?
(1) NaCl (3) NH4Cl
(2) NaOH (4) NH4NO3
2
Which quantities must be equal for a chemical
reaction at equilibrium?
(1) the activation energies of the forward and
reverse reactions
(2) the rates of the forward and reverse reactions
(3) the concentrations of the reactants and
products
(4) the potential energies of the reactants and
products
2
Which formula represents copper(I) oxide?
(1) CuO (3) Cu2O
(2) CuO2 (4) Cu2O2
3
At STP, a 7.49-gram sample of an element has a
volume of 1.65 cubic centimeters. The sample
is most likely
(1) Ta (3) Te
(2) Tc (4) Ti
4
Which element, represented by X, reacts with
fluorine to produce the compound XF2?
(1) aluminum (3) magnesium
(2) argon (4) sodium
3
As atomic number increases within Group 15 on
the Periodic Table, atomic radius
(1) decreases, only
(2) increases, only
(3) decreases, then increases
(4) increases, then decreases
2
Given the balanced equation representing a
reaction:
CaO(s) + CO2(g) →CaCO3(s) + heat
What is the total mass of CaO(s) that reacts
completely with 88 grams of CO2(g) to produce
200. grams of CaCO3(s)?
(1) 56 g (3) 112 g
(2) 88 g (4) 288 g
3
What is the empirical formula of a compound
that has a carbon-to-hydrogen ratio of 2 to 6?
(1) CH3 (3) C3H
(2) C2H6 (4) C6H2
1
Given the balanced equation representing a
reaction:
H2(g) + Cl2(g) →2HCl(g) + energy
Which statement describes the energy changes
in this reaction?
(1) Energy is absorbed as bonds are formed,
only.
(2) Energy is released as bonds are broken,
only.
(3) Energy is absorbed as bonds are broken,
and energy is released as bonds are formed.
(4) Energy is absorbed as bonds are formed,
and energy is released as bonds are broken.
3
Which solution has the highest boiling point at
standard pressure?
(1) 0.10 M KCl(aq)
(2) 0.10 M K2SO4(aq)
(3) 0.10 M K3PO4(aq)
(4) 0.10 M KNO3(aq)
3
What is the molarity of 1.5 liters of an aqueous
solution that contains 52 grams of lithium
fluoride, LiF, (gram-formula mass =26 grams/mole)?
(1) 1.3 M (3) 3.0 M
(2) 2.0 M (4) 0.75 M
1
What occurs when a 35-gram aluminum cube at
100.°C is placed in 90. grams of water at 25°C in
an insulated cup?
(1) Heat is transferred from the aluminum to
the water, and the temperature of the water
decreases.
(2) Heat is transferred from the aluminum to
the water, and the temperature of the water
increases.
(3) Heat is transferred from the water to the
aluminum, and the temperature of the water
decreases.
(4) Heat is transferred from the water to the
aluminum, and the temperature of the water
increases.
2
Which temperature is equal to 120. K?
(1) −153°C (3) +293°C
(2) −120.°C (4) +393°C
1
A rigid cylinder contains a sample of gas at STP.
What is the pressure of this gas after the sample
is heated to 410 K?
(1) 1.0 atm (3) 0.67 atm
(2) 0.50 atm (4) 1.5 atm
4
Given the balanced equation representing a
phase change:
C6H4Cl2(s) + energy →C6H4Cl2(g)
Which statement describes this change?
(1) It is endothermic, and entropy decreases.
(2) It is endothermic, and entropy increases.
(3) It is exothermic, and entropy decreases.
(4) It is exothermic, and entropy increases.
2
In a biochemical reaction, an enzyme acts as a
catalyst, causing the
(1) activation energy of the reaction to decrease
(2) potential energy of the reactants to decrease
(3) kinetic energy of the reactants to increase
(4) heat of reaction to increase
1
Butanal and butanone have different chemical
and physical properties primarily because of
differences in their
(1) functional groups
(2) molecular masses
(3) molecular formulas
(4) number of carbon atoms per molecule
1
Which salt is produced when sulfuric acid and
calcium hydroxide react completely?
(1) CaH2 (3) CaS
(2) CaO (4) CaSO4
4
Which radioisotope is used to treat thyroid
disorders?
(1) Co-60 (3) C-14
(2) I-131 (4) U-238
2