Chemistry 121 Mid Term: Chapters 1-5

Front 1

INTERRELATED

Back 1

Matter and energy are

a) similar to work and distance.
b) interrelated.
c) not related to each other.
d) similar to mass and weight.

Front 2

10^3

Back 2

One millimeter is equal to how many meters?

Front 3

WEIGHT DEPENDS ON GRAVITY

Back 3

Which of the following is true?

a) Mass is the same as weight.
b) Mass and weight are always proportional to each other.
c) Weight depends on gravity.
d) Mass depends on gravity.

Front 4

2.7 x 10^3

Back 4

Perform the following calculation, maintaining the correct number of significant figures. Apply scientific notations if necessary: 18567 / 6.9=

a) 2690.8696
b) 2.7 x 10^3
c) 2.69 x 10^4
d) 2.691 x 10^3

Front 5

2.78 x 10^26

Back 5

Express the following number in scientific notation. Keep all significant digits: 278,000,000,000,000,000,000,000,000=

Front 6

9.8 x 10^6 microliters

Back 6

Perform the following conversion: 2.6 gallons ---> ? µ L

a) 9.841 x 10^6 microliters
b) 6.87 x 10^5 microliters
c) 6.9 x 10^5 microliters
d) 9.8 x 10^6 microliters

Front 7

0.214 liters

Back 7

A normal heart beats approximately 70 times in one minute. If the total amount of blood circulating in the human body is around 5.00 liters and all this blood goes through the heart in one minute, how much blood runs through the heart in three beats?

Front 8

ALL OF THE ABOVE

Back 8

Energy is

a) neither created nor destroyed.
b) transferred between different forms.
c) transferred from place to place.
d) all of the above
e) none of the above

Front 9

IS DIRECTLY RELATED TO THE MOLECULAR SPEED OF IT'S PARTICLES.

Back 9

The temperature of a substance

A) is a measure of how much energy the substance has.
B) is directly related to the molecular speed of its particles.
C) increases as the speed of its particles decreases.
D) is a measure of the potential energy of the substance.

Front 10

THE SAME ATOMIC NUMBER

Back 10

Every atom of the same element has

a) the same mass
b) the same atomic number
c) the same number of neutrons
d) the same weight

Front 11

78 protons, 117 neutrons

Back 11

How many protons and neutrons are in this element: 195Pt?

Front 12

THE VISIBLE REGION OF LIGHT INCLUDES WAVELENGTHS FROM 300 NM TO 900 NM

Back 12

Which of the following is not true of light?

a) it is the visible form of electromagnetic radiation
b) it can be absorbed by chemicals, causing electrons to jump to higher energy levels
c) it is a form of energy
d) the visible region of light includes wavelengths from 300 nm to 900 nm.

Front 13

THE LOWEST ENERGY OF AN ATOM

Back 13

The ground state of an atom is considered

a) an atom that is has only one electron in its closest shell.
b) to be the energy an atom has at 0 K.
c) the highest energy of an electron.
d) an atom that is not bonded to any other elements.
e) the lowest energy of an atom.

Front 14

20 protons, 18 electrons

Back 14

How many protons and electrons are present in a Ca2+ ion?

Front 15

Ca

Back 15

Which of the following elements is most likely to be a good conductor of electricity?

a) Ca
b) C
c) Ne
d) I
e) S

Front 16

As

Back 16

Which element will have the greatest ionization energy?

a) Ga
b) As
c) K
d) Pb
e) Na

Front 17

Ar, Ca2+

Back 17

Which of the following pairs of atoms and / or ions are isoelectronic?

a) He, Ne
b) F, O
c) Ar, Ca2+
d) K+, Na+

Front 18

1s2,2s2,2p6,3s2,3p6,4s1

Back 18

The electronic configuration for K is

a) 1s2,2s2,2p6,3s2,3p6,4s0,3d1
b) 1s2,2s2,2p6,3s2,3p6,4s2
c) 1s2,2s2,2p6,3s2,3p6,3d6,4s1
d) 1s2,2s2,2p6,3s2,3p6,4s1

Front 19

A CATION

Back 19

An atom that has more protons than electrons is

a) a cation
b) an anion
c) a polyatomic ion
d) a neutral atom

Front 20

PROTONS ARE NOT EVENLY DISTRIBUTED THROUGHOUT AN ATOM.

Back 20

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

a) electrons have a negative charge.
b) protons are 1840 times heavier than electrons
c) protons are not evenly distributed throughout an atom.
d) atoms are made of protons, neutrons and electrons.
e) the nucleus contains protons and neutrons.

Front 21

16 protons, 18 electrons

Back 21

How many protons and electrons are present in a S2– ion?

Front 22

39.95 u

Back 22

Naturally occurring argon consists of three isotopes, the atoms of which occur in the following abundances: 0.34% 36Ar (35.9676 u), 0.07% 38Ar (37.9627 u), and 99.59% 40Ar (39.9624 u). The calculated atomic weight of argon is:

Front 23

J.J. Thomson

Back 23

The scientist who determined the charge of the electron was ____________.

Front 24

17 p, 22 n, 17 e

Back 24

An atom of the isotope chlorine-39 consists of how many protons, neutrons, and electrons? (p = proton, n = neutron, e = electron)

Front 25

THE EXISTENCE OF MORE THAN ONE ISOTOPE OF AN ELEMENT

Back 25

Which of the following is NOT explained by Dalton's atomic theory?

a) The existence of more than one isotope of an element.
b) Conservation of mass in a chemical reaction.
c) Different elements have different masses.
d) The formation of compounds from elements.

Front 26

AN ELEMENT

Back 26

A pure substance that cannot be changed into a simpler form of matter by any chemical reaction is:

a) a compound
b) a mixture
c) an element
d) a molecule

Front 27

CALCIUM

Back 27

Which element matches the following electron configuration: 1s2,2s2,2p6,3s2,3p6,4s2

a) potassium
b) sodium
c) calcium
d) magnesium

Front 28

ELECTRONS IN THE OUTERMOST SHELL OF AN ATOM

Back 28

Valence electrons are

a) electrons that are not involved in bonding.
b) the total number of electrons in an atom.
c) electrons in the innermost shell of an atom.
d) electrons in the outermost shell of an atom.

Front 29

6

Back 29

The maximum number of electrons that the p subshell can hold is

a) 2
b) 4
c) 6
d) 10

Front 30

DUMBBELL

Back 30

What is the shape of a p orbital?

a) tetrahedral
b) sphere
c) clover leaf shape
d) two lobes and a donut
e) dumbbell

Front 31

ELECTRONS FILL THE LOWEST ENERGY LEVELS FIRST

Back 31

What order do electrons fill orbitals in the ground state?

a) Electrons fill the lowest energy levels first.
b) Electrons fill p orbitals first.
c) Electrons fill the 3rd orbital first.
d) Electrons enter the highest energy orbitals first.
e) Electrons are placed two at a time in any orbital.

Front 32

METALLOID

Back 32

A substance that exhibits both metallic and nonmetallic properties is called a _______.

a) transition element
b) lanthanide
c) actinide
d) metalloid
e) alkaline earth metal

Front 33

DIHYDROGEN SULFITE

Back 33

The chemical name for SO32- is sulfite ion. Therefore, the name of H2SO3 is:

a) dihydrosulfuric acid
b) sulfuric acid
c) dihydrogen sulfite
d) hydrogen sulfite
e) hyposulfurous acid

Front 34

BaF2

Back 34

Which is the formula for the binary compound of barium and fluoride?

a) Ba2F3
b) BaF
c) BaF2
d) Ba2F
e) BaF3

Front 35

SULFUR

Back 35

Which of the following does not exist as a diatomic molecule?

a) iodine
b) sulfur
c) oxygen
d) carbon monoxide
e) nitrogen

Front 36

O

Back 36

Which of the following elements is most likely to form an ionic compound with K?

a) Na
b) Ca
c) C
d) O
e) Ne

Front 37

B - O

Back 37

Which one of the following is the most polar bond?

a) B - C
b) S - O
c) C - O
d) B - O
e) C - C

Front 38

Cl

Back 38

Which element has the greatest electronegativity?

a) C
b) Si
c) As
d) Cl
e) Sr

Front 39

O–C, H–N, N–C

Back 39

Considering the following isolated bonds, which listing orders the bonds from the most to the least ionic character?

a) O–C, N–C, H–N
b) N–C, H–N, O–C
c) O–C, H–N, N–C
d) H–N, N–C, O–C
e) N–C, O–C, H–N

Front 40

SO4^2-

Back 40

The correct formula for the polyatomic ion, sulfate, is

a) SO3
b) SO3^2-
c) SO4^2-
d) SO4
e) S^2-

Front 41

NH3

Back 41

Which species is not planar?

a) NH3
b) NO3^1-
c) BCl3
d) SO3

Front 42

TETRAHEDRAL

Back 42

The shape of NH4^+ is best described by:

a) linear
b) planar
c) pyramidal
d) tetrahedral
e) octahedral

Front 43

MnO2

Back 43

What is the formula for manganese dioxide?

Front 44

SULFUR TRIOXIDE

Back 44

What is the name of SO3?

a) sulfur oxygen
b) sulfite
c) sulfate
d) sulfur trioxide

Front 45

AMMONIA

Back 45

What is the name of NH3?

a) ammonium
b) ammonia
c) nitrogen trihydrogen
d) nitrogen hydride

Front 46

THE ABILITY OF AN ATOM TO ATTRACT ELECTRONS TO ITSELF IN A CHEMICAL BOND.

Back 46

Electronegativity is _______________.

a) the ability of an atom to attract electrons to itself in a chemical bond.
b) the measure of an atom's ability to make ionic bonds.
c) the amount of energy required for an atom to accept an electron.
d) the amount of energy required for an atom to lose an electron.

Front 47

AlCl3

Back 47

Identify the ionic compound among the following:

a) SO2
b) AlCl3
c) CH4
d) HF

Front 48

H2O

Back 48

Which of the following is a polar molecule?

a) CCl4
b) H2O
c) CO2
d) H2Be

Front 49

NONPOLAR COVALENT

Back 49

What is the overall polarity of methane?

a) nonpolar covalent
b) polar covalent
c) ionic
d) nonpolar ionic

Front 50

ONE END OF THE MOLECULE IS SLIGHTLY NEGATIVE WHILE THE OTHER END IS SLIGHTLY POSITIVE

Back 50

What does it mean when a molecule is said to be polar?

a) one end of the molecule is slightly negative while the other end is slightly positive
b) both ends of the molecule are slightly positive
c) both ends of the molecule is slightly negative
d) the molecule is neutral
e) the difference in electronegativities is zero

Front 51

BENT

Back 51

The shape of a water molecule is _________________.

a) trigonal
b) bent
c) linear
d) tetrahedral

Front 52

BETWEEN MOLECULES

Back 52

Intermolecular forces are forces _______________.

a) within molecules
b) between molecules
c) pushing molecules apart
d) of attraction between the protons and electrons

Front 53

CH3Cl

Back 53

Which of the following is a polar molecule?

a) CCl4
b) CO2
c) CH4
d) CH3Cl

Front 54

120 DEGREES

Back 54

What is the predicted bond angle for a molecule with a trigonal planar electron-pair geometry?

a) 180 degrees
b) 120 degrees
c) 109.5 degrees
d) 45 degrees
e) 90 degrees

Front 55

TETRAHEDRAL

Back 55

What is the electron-pair geometry for a molecule with three electron pairs around the central atom?

a) Linear
b) Trigonal planar
c) Tetrahedral
d) Trigonal bipyramidal
e) Octahedral

Front 56

CH3OH

Back 56

Which of the following molecules dissolves in water?

a) CCl4
b) CBr4
c) C6H6
d) CH3OH

Front 57

180 g

Back 57

What is the molar mass of acetylsalicylic acid (aspirin), C9H8O4?

Front 58

1,2,2,3

Back 58

The reaction Fe3O4 + C ---> CO2 + Fe can be balanced with the coefficients:

a) 1,2,2,3
b) 1,4,4,3
c) 2,4,4,3
d) 1,1,1,3

Front 59

2.1 x 10^24

Back 59

How many hydrogen atoms are present in 42 g of ammonium carbonate?

Front 60

4.99 x 10^22 atoms

Back 60

How many phosphorus atoms are in 2.57 g of P?

Front 61

0.981 g

Back 61

What is the mass of 5.45 x 10^-3 mol of glucose C6H12O6?

Front 62

95.8 %

Back 62

What is the percent yield of PI3, if 58.62 g of I2 are reacted with an excess of phosphorus according to the following equation and 60.75 g are actually obtained? 2 P(s) + 3 I2(s) ---> 2PI3(s)

a) 84.97 %
b) 1.57 %
c) 48.37 %
d) 37.6 %
e) 95.8 %

Front 63

0.2

Back 63

In the reaction of Fe3O4 with carbon to form carbon dioxide and iron, the number of moles of carbon required to convert 23 g of Fe3O4 to products is:

a) 0.05
b) 0.1
c) 0.2
d) 0.3
e) 0.4

Front 64

16 g O2 reacts to form 18 g H2O

Back 64

Given the reaction CH4 + 2O2 ----------> 2H2O + CO2 which statement is FALSE?

a) 16 g O2 reacts to form 18 g H2O
b) 16 g CH4 combines with 64 g O2
c) 1 mol CO2 is formed from 2 mol O2
d) 1 mol CH4 reacts to form 2 mol H2O
e) 18 g H2O is produced from 1 mol O2

Front 65

1,11,7,8

Back 65

The reaction C7H16 + O2 ---> CO2 + H2O can be balanced with the coefficients:

a) 1, 9, 6, 8
b) 2, 10, 7, 8
c) 1, 11, 7, 8
d) 1, 10, 7, 8

Front 66

contains 6.022 x 10^23 molecules

Back 66

A mole of H2

a) contains 6.022 x 10^23 atoms.
b) contains 6.022 x 10^23 molecules.
c) contains 1 gram of hydrogen.
d) is 6.022 x 1023 grams of hydrogen.

Front 67

8

Back 67

What is the coefficient of CO2 when the following equation is properly balanced with the smallest set of whole numbers? C4H10 + O2 ---> CO2 + H2O

a) 1
b) 4
c) 6
d) 12
e) 8

Front 68

2,3,1,6

Back 68

The correct coefficients for the unbalanced equation below are: CoBr3 + Na2CO3 ---> Co2(CO3)3 + NaBr

a) 1,3,1,6
b) 2,3,1,6
c) 2,1,1,2
d) 1,1,1,3

Front 69

1019 g

Back 69

Caustic soda, NaOH, can be prepared commercially by the reaction of Na2CO3 with slaked lime, Ca(OH)2. How many grams of NaOH can be obtained by treating 1.350 kg of Na2CO3 with Ca(OH)2?

Front 70

2,1,2

Back 70

The coefficients needed to balance the second step of the Ostwald process, __ NO. + __ O2 -----> __ NO2 , are

a) 1, 1, 1
b) 2, 1, 2,
c) 2, 5/2, 2
d) 4, 5, 4

Front 71

283.89 g/mole

Back 71

What is the molar mass of P4O10 to 5 significant figures?

Front 72

68.15 g/mole

Back 72

What is the molar mass of (NH4)2S to 4 significant figures?

Front 73

733.0

Back 73

How many grams of biotin (C10H16N2O3S) are in 3 moles?

Front 74

6.76 x 10^23 molecules

Back 74

How many molecules are in 137g of the B vitamin Nicotinamide. (C6H6N2O)?

a) 6.76 x 10^23 molecules
b) 6.81 x 10^23 molecules
c) 6.74 x 10^23 molecules
d) 6.77 x 10^22 molecules

Front 75

26.0 g

Back 75

How many grams of glucose (C6H12O6) are consumed if 15.6 ml of water are produced? (density = 1.00 g/ml) C6H12O6 + 6O2 -> 6H2O + 6CO2

Front 76

0.130 moles

Back 76

How many moles of mercury are in 1.93 mL? (density = 13.55 g/mL)

Front 77

81.6 mL

Back 77

How many mL of ethanol (C2H6O) are present in 1.39 moles? (density = .785 g/ml)

a) 81.6 mL
b) 50.3 mL
c) 42.2 mL
d) 75.2 mL

Front 78

73.3 kg

Back 78

How many kg of carbon dioxide are produced when 150 kg of glucose (C6H12O6) are fermented? C6H12O6 -> 2C2H5OH + 2CO2

a) 18.3 kg
b) 73.3 kg
c) 37.9 kg
d) 36.6 kg

Front 79

6.29 x 10^23 molecules

Back 79

How many molecules of nitrogen are produced when 35.6 g of NH3 react in the following equation? 4NH3 + 3O2 -> 2N2 + 6H2O

Front 80

1.37 g

Back 80

What is the mass in grams of 4.59 x 1022 molecules of water?

a) 1.22 g
b) 1.37 g
c) 0.687 g
d) 2.74 g

Front 81

139.3 g

Back 81

How many grams of oxygen are consumed when 130.7 g of glucose (C6H12O6) burns in excess oxygen? C6H12O6 + 6O2 -> 6CO2 + 6H2O

Front 82

retains shape easily

Back 82

Which of the following is not characteristic of gases?

a) have much lower densities than solids or liquids
b) formation of homogenous mixtures regardless of the nature of gases
c) retains shape easily
d) high compressibility

Front 83

6.38 atm

Back 83

What is the gas pressure in atmospheres of 485 cm Hg?

a) 0.64 atm
b) 33.0 atm
c) 6.38 atm
d) 5.50 atm
e) 6.46 atm

Front 84

1.96 mg/mL

Back 84

What is the density of carbon dioxide at STP?

Front 85

2.07 L

Back 85

A sample of gas occupies 3.00 L at 760 torr. Calculate the volume it will occupy at 1.45 atm and the same temperature.

Front 86

11.2 L

Back 86

A 14.0 g sample of N2 gas occupies what volume at STP?

Front 87

1.1 x 10^4 L

Back 87

A balloon has a volume of 1.5 x 10^3 L of helium at 1.0 atm and 25 oC. At an altitude of 21 km the temperature is -50. oC and the atmospheric pressure is 76.0 mm Hg. What is the volume of this balloon at 21 km?

Front 88

Avogadro's

Back 88

The volume of an ideal gas is directly proportional to the number of moles of the gas at constant temperature and pressure is a statement of _____________ Law.

a) Charles's
b) Boyle's
c) Amonton's
d) Avogadro's
e) Dalton's

Front 89

356 mm Hg

Back 89

A mixture of three gases has a pressure at 298 K of 1380 mm Hg. The mixture is analysed and found to contain 302 mm Hg of CO2 and 722 mm Hg of CO. What is the partial pressure of Ar?

Front 90

the valence electrons of a given metal atom are delocalized over all of the atoms in the piece of metal

Back 90

Which of the following best describes the bonding between atoms in metals.

a) the transfer of electrons from one atom to another, producing charges which then interact with each other
b) by sharing pairs of electrons with adjacent atoms
c) by fusing the atomic nuclei to produce a continuous malleable array
d) the valence electrons of a given metal atom are delocalized over all of the atoms in the piece of metal
e) the fusion of the protons, neutrons and electrons to form a hard solid mass

Front 91

amorphous solid

Back 91

Butter, like glass, melts over a range of temperatures, rather than with a sharp melting point. Butter might be classified as a/an:

a) covalent solid
b) ionic crystal
c) metallic crystal
d) amorphous solid
e) molecular crystal

Front 92

the strength/weakness of the intermolecular forcers

Back 92

The boiling point of a substance is most strongly influenced by:

a) the molecular weight of a substance
b) the specific heat of the substance
c) the melting point
d) the strength/weakness of the intermolecular forces
e) the amount of the substance involved

Front 93

the temperature is increased

Back 93

Viscosity of liquids typically increases when which of the following is considered, except:

a) the temperature is increased
b) compounds with ionic bonds are involved
c) substances that can hydrogen bond are used
d) longer molecules are used
e) compounds with greater molecular weights are used

Front 94

covalent forces

Back 94

All of the following are intermolecular forces except:

a) dipole-dipole interactions
b) London forces
c) covalent forces
d) van der Waals forces

Front 95

Ge

Back 95

Which one of the following is not an example of a covalent network solid?

a) diamond
b) SiO2
c) Ge
d) graphite

Front 96

NH3

Back 96

Which of the following exhibits the most hydrogen bonding?

a) LiH
b) CH4
c) NH3
d) H2S

Front 97

why water and ethanol mix

Back 97

The phrase "like dissolves like" describes

a) the interaction of a polar and a nonpolar substance
b) why water is hydrogen bonded
c) why water and ethanol mix
d) solubility of ionic compounds in nonpolar solvents

Front 98

cooler

Back 98

When water evaporates off of an object, the object is

a) cooler
b) warmer
c) experiences no temperature change
d) becomes heavier

Front 99

0.464 atm

Back 99

Convert 353 torr to atm.

Front 100

2.10 atm

Back 100

Calculate the pressure in atm of a balloon filled with 7.50 grams of helium gas if the balloon's volume decreases to 7.50 L. Suppose the balloon's pressure and volume are originally 799 mmHg and 15.0 L.

Front 101

V x P = constant

Back 101

Which of the following is a correct statement of Boyle's Law?

a) P/T = constant
b) V/P = constant
c) V x P = constant
d) T/V = constant
e) V/T = constant
f) T x V = constant
g) P x T = constant

Front 102

25.9 L

Back 102

If 4.29 grams of gas occupies 25.6 L at 49.0 oC at a pressure of 759 mmHg, what volume will 4.29 grams of gas will occupy at 53.0 oC (assume the pressure is unchanged)?

Front 103

0.153 mole

Back 103

Calculate the number of moles there are when a gas occupies a volume of 3.95 L at 37.0 oC and 0.985 atm.

Front 104

6.36 L

Back 104

The metabolic breakdown of glucose, C6H12O6, in our bodies produces CO2 gas as following: C6H12O6 (s) + 6O2 (g) --> 6CO2 (g) + 6H2O (l) Calculate the volume of dry CO2 gas produced at 37 oC and 1.00 atm when 7.50 g of glucose is consumed in this reaction.

Front 105

weak attractive forces

Back 105

The following are characteristics of a solid except:

a) distances between molecules, ions, or atoms in a solid are very close
b) virtually incompressible
c) strong attractive forces
d) weak attractive forces
e) fixed volume

Front 106

CO2

Back 106

The major event in the greenhouse effect is that some of the IR radiation heading back towards space is absorbed by the "greenhouse gases" of the atmosphere. The major "greenhouse gas" is __.

a) NO2
b) CO2
c) SO2
d) SO3

Front 107

partially burned hydrocarbons and NO

Back 107

Automobile emissions that cause smog are __.

a) carbon monoxide and nitrogen
b) carbon dioxide and carbon monoxide
c) partially burned hydrocarbons and NO
d) carbon monoxide and sulfur dioxide

Front 108

O2 and N2

Back 108

Air consists primarily of what two molecules?

Front 109

are malleable

Back 109

A characteristic of metals is that they

a) are malleable.
b) are brittle.
c) shatter.
d) are dull.

Front 110

(CH3)3N

Back 110

Which of the following is not likely to exhibit hydrogen bonding?

a) CH3CH2OH
b) CH3NH2
c) H2O
d) (CH3)3N
e) NH2OH

Front 111

1.43 g/L

Back 111

What is the density of O2 gas at STP?

Front 112

1.80 X 10^-5

Back 112

Provide the answer to the following problem using scientific notation and the proper number of significant digits: (6.00 x 10^-2)(3.00 x 10^-4) = ?

Front 113

3.5 x 10^3 cm

Back 113

How many cm are in 3.5 x 10^-2 km?

Front 114

0.545

Back 114

What is the specific gravity of an object that weighs 13.35 g and has a volume of 25.00 mL? The density of water under the same conditions is 0.980 g/mL.

Front 115

$568/oz

Back 115

The cost of a drug is 125 francs per gram. What is the cost in dollars per ounce? [Use: $1 = 6.25 francs and 1 ounce = 28.4 g]

Front 116

chemical

Back 116

What kind of change always results in the formation of new materials?

a) molecular
b) exothermic
c) endothermic
d) physical
e) chemical

Front 117

electromagnetic radiation

Back 117

Microwaves, light, and X-rays are all forms of __________?

a) electricity
b) high energy electrons
c) electron repulsion
d) electromagnetic radiation
e) radioactivity

Front 118

period

Back 118

What do we call a complete horizontal row of elements on the periodic table?

a) group
b) period
c) family
d) representative elements
e) transition elements

Front 119

group

Back 119

What do we call a complete vertical row of elements on the periodic table?

a) group
b) period
c) family
d) representative elements
e) transition elements

Front 120

2n^2

Back 120

Which of the following correctly gives the electron capacity of a principal energy level in terms of the number n?

a) n
b) 2n
c) 2n + 2
d) n^2
e) 2n^2

Front 121

Rb

Back 121

Which of the following atoms has the biggest size (radius)?

a) Na
b) Al
c) Cl
d) Rb
e) I

Front 122

carbon tetrachloride

Back 122

Provide the name of CCl4.

Front 123

iron(III) sulfate

Back 123

Give the name of Fe2(SO4)3 in the stock system.

a) iron monosulfuric acid
b) iron (II) sulfate
c) iron (III) Sulfate
d) ferrous sulfate
e) ferric sulfate

Front 124

SO2

Back 124

Which of the following molecules is polar?

a) CF4
b) BeH2
c) SO2
d) F2
e) CO2

Front 125

formed when two nonmetals share a pair of electrons

Back 125

A covalent bond is

a) formed when two metals share a pair of electrons
b) formed when a metal and nonmetal share a pair of electrons.
c) formed when a nonmetal donates an electron to a metal.
d) formed between cations and anions.
e) formed when two nonmetals share a pair of electrons.

Front 126

P2O5

Back 126

What is the correct formula of diphosphorous pentaoxide?

Front 127

1.72 x 10^23 molecules

Back 127

Dinitrogen monoxide or laughing gas (N2O) is used as dental anesthetic and as an aerosol propellant. How many moles of N2O are present in 12.6 g of the compound? How many molecules of N2O are present in 12.6 g of the compound? [Use molar masses: N, 14.01 g/mol, O, 16.00 g/mol]

Front 128

80.09 g

Back 128

How many grams of sodium hydroxide will react with a solution containing 73.00 g HCl? [Use molar masses: NAOH, 39.99 g/mol; HCl, 36.45 g/mol]
NaOH(aq) + HCl(aq) ---> NaCl(aq) + H2O(l)

Front 129

2.91 x 10^24 atoms

Back 129

How many atoms of sulfur are present in 155 g of sulfur? [Use atomic mass: S, 32.06 amu]

Front 130

179.4 g

Back 130

Iron reacts with oxygen to form iron(III) oxide (Fe2O3). How many grams of product will be formed from 125.5 g of Fe? [Use atomic masses: FE, 55.85 AMU; O, 16.00 amu]

Front 131

precipitation

Back 131

Classify the following reacting:
Na2S(aq) + CuSO4(aq) ---> NaSO4(aq) + CuS(s)

a) precipitation
b) acid-base
c) oxidation-reduction
d) decomposition
e) combustion

Front 132

All of the choices are correct

Back 132

To which elements must hydrogen be bonded in order to display hydrogen bonding?

a) fluorine
b) oxygen
c) nitrogen
d) All of the choices are correct
e) Both B and C are correct

Front 133

1.03 x 10^3 L

Back 133

A balloon filled with helium has a volume of 1.00 x 10^3 L at 20 degress C. What would be the balloon's volume at 30 degree C, if the pressure surrounding the balloon remains constant?

Front 134

All of the statements are true

Back 134

A balloon containing helium at constant pressure and temperature has the volume doubled by adding a more helium. Which statement(s) is (are) true?

a) The number of helium atoms doubled
b) The number of moles of helium doubled
c) The mass of helium in the balloon doubled
d) All of the statements are true
e) Statements A, B, and C, are false

Front 135

2.67 mol

Back 135

How many moles of gas are there in a gas-filled balloon, which has a volume of 67.0 L at a pressure of 742 mmHg and a temperature of 25.0 degree C?

Front 136

3.00 L

Back 136

A sample of oxygen occupies 1.00 L. If the temperature remains constant, and the pressure on the oxygen is decreased to one third the original pressure, what is the new volume?`

Front 137

i and iii

Back 137

A hypothesis:

i. must be testable.
ii. is a theory that has been supported by experiments.
iii. is a tentative guess that explains an observation.
iv. is used to make predictions.
v. is a set of conceptual assumptions

a) i and ii
b) only ii
c) i and iii
d) iii and iv
e) iv and v

Front 138

mile

Back 138

Which of these is NOT an SI unit?

a) liter
b) mile
c) gram
d) second
e) meter

Front 139

9.50 x 10^2 g

Back 139

9.50 x 10-1 kg converted to the basic unit (with no prefix) and expressed in standard exponential notation to the proper number of significant digits is:

Front 140

4

Back 140

How many significant figures does the sum of the following contain? 8.3801 + 2.57

Front 141

accurate and precise

Back 141

If a measurement is not very reproducible but close to the actual value it is very _______ but not very ________ .

a) accurate, precise
b) precise, accurate
c) random, systematic
d) calibrated, precise
e) systematic, precise

Front 142

22.3 cm^3

Back 142

Calculate the volume of 450. g of gold (density = 19.3 g/cm3)

Front 143

1.47 x 10^3 cm^3

Back 143

Convert 1.47 L to cubic centimeters.

Front 144

5

Back 144

How many significant figures are there in 5.0390 g?

a) 4
b) 5
c) 6
d) 2
e) 3

Front 145

19.1 cm

Back 145

A small pizza has a diameter of 7.50 inches. Its diameter in centimeters is:

a) 19.1 cm
b) 12.0 cm
c) 4.65 cm
d) 2.95 cm
e) 0.169 cm

Front 146

Glycerol will have a greater surface tension than dimethyl ether

Back 146

Glycerol is a very popular compound. Dimethyl ether is only slightly polar. Which statement is TRUE?

a) Glycerol is less viscous than dimethyl ether.
b) Glycerol will have a greater surface tension than dimethyl ether.
c) Dimethyl ether has a lower vapor pressure than glycerol
d) The viscosity of both substances will increase with increasing temperature.
e) Glycerol will evaporate at a greater rate than dimethyl ether.

Front 147

gas

Back 147

What state(s) of matter is most compressible?

a) solid
b) liquid
c) gas
d) solid and liquid
e) liquid and gas

Front 148

N2

Back 148

Of the following gases, which will behave most like an ideal gas?

a) N2
b) HF
c) NH3
d) CH3Cl
e) CO

Front 149

1.25 g/L

Back 149

Calculate the density of nitrogen gas (N2) at STP, in g/L. [Use molar mass: N2, 28.0 g/mol]

Front 150

29.7 L

Back 150

What is the volume (L) occupied by a mole of an ideal gas, if the pressure is 626 mmHg and the temperature is 25.0 degree C?

Front 151

higher

Back 151

At the membrane barrier in lung tissue between the blood and the surrounding atmosphere, what is the relationship between the partial pressure of atmospheric oxygen to that of the oxygen present in blood?

a) equal
b) proportional
c) zero
d) lower
e) higher

Front 152

incompressible

Back 152

Which of the following is NOT a physical property of a gas?

a) expands to fill the container
b) low density
c) distance between molecules is very large
d) incompressible
e) takes on the shape of the container

Front 153

Torricelli

Back 153

Who invented the first barometer?

a) Boyle
b) Charles
c) Dlaton
d) Gay-Lussac
e) Torricelli

Front 154

surface tension

Back 154

What property of liquids explains the formation of spherical water droplets on green leaves?

a) viscosity
b) surface tension
c) adhesion
d) vapor pressure
e) none of the choices are correct

Front 155

once equilibrium is established between the liquid and the vapor, the rate of the evaporation process will equal the rate of condensation.

Back 155

When a liquid is placed in a sealed container,

a) evaporation of the liquid cannot occur
b) once equilibrium is established between the liquid and the vapor, the rate of the evaporation process will equal the rate of condensation.
c) all molecules stay in the liquid state
d) condensation of the evaporated molecules in the jar can only occur once all of the liquid molecule are in the vapor (or gaseous) state.
e) a set vapor pressure will be reached, which is the same at all temperatures.

Front 156

absolute temperature

Back 156

What quantity is directly proportional to the kinetic energy of the particles in a gas?

a) distance between molecules
b) absolute temperature
c) atomic mass
d) formula mass
e) volume of the individual particles

Front 157

gases are mostly empty space

Back 157

According to the kinetic molecular theory,

a) gases are mostly empty space
b) the average kinetic energy of the molecules increases with decreasing temperature
c) gases molecules are attracted to each other
d) when molecules collide they lose energy
e) gas molecules are very closely packed together

Front 158

Absorbing infrared radiation

Back 158

Carbon dioxide acts as a greenhouse gas by ____________.

a) absorbing visible radiation
b) absorbing ultraviolet radiation
c) absorbing infrared radiation
d) sorting solar energy
e) trapping sunlight during photosynthesis

Front 159

76 torr

Back 159

Which one of the following pressures is not equal to one atmosphere?

a) 76 cmHg
b) 14.7 lb/in^2
c) 30 inches of Hg
d) 101 kPa
e) 76 torr

Front 160

The total pressure of a mixture of gases is the sum of the partial pressure of each gas that makes up the mixture.

Back 160

Which of the following is a statement of Dalton's law of partial pressure?

a) The total pressure of a mixture of gases is the sum of the partial pressure of each gas that makes up the mixture.
b) The partial pressure of a gas is equal to the total pressure of the mixture,
c) Gases can exist as mixtures at STP only.
d) The total pressure of a mixture of gases is the product of the partial pressures of each gas in the mixture.
e) In a mixture of two gases, the pressure of each gas is the 1/2 the total pressure.

Front 161

is lowered by surfactants

Back 161

Surface tension _______________.

a) increases with increasing temperature
b) is unaffected by temperature
c) is higher for nonpolar substances than for polar ones
d) is lowered by surfactants
e) is the same as viscosity

Front 162

Boyle

Back 162

Who formulated the relationship between the volume and the pressure of a gas?

a) Boyle
b) Charles
c) Dalton
d) Gay-Lussac
e) Torricelli

Front 163

1.92 x 10^-3 L

Back 163

Consider 1.00 L of air in a patient's lungs at 37.0 degree C and 1.00 atm pressure. What volume would this air occupy if it were at 25.0 degree C under a pressure of 5.00 x 10^2 atm (a typical pressure in a compressed air cylinder)?

Front 164

760 mmHg

Back 164

Express one standard atmosphere of pressure in units of mmHg.

a) 14.7 mmHg
b) 380 mmHg
c) 760 mmHg
d) 0.333 mmHg
e) 30 mmHg

Front 165

pressure

Back 165

The pascal (Pa) is a unit for expressing what quantity?

a) volume
b) amount of matter
c) temperature
d) energy
e) pressure

Front 166

25 atm

Back 166

A gas with pressure of 5.0 atm is compressed at constant temperature from 10.0 L to 2.0 L. What is the pressure of the gas after it is compressed?

Front 167

6.022 x 10^23

Back 167

How many mercury atoms are present in one mole of mercury?

Front 168

1.0 mol H2

Back 168

How many moles of hydrogen gas are needed to react with 0.50 mole of oxygen to form one mole of water?
2H2(g) + O2(g) -----> 2H2O(l)

Front 169

7.15g

Back 169

Iron reacts with oxygen to form iron (III) oxide (Fe2O3). What is the theoretical yield of product when 5.00 grams of Fe reacts with an excess of O2? [Use molar masses: Fe, 55.85 g/mol; O, 16.00 g/mol]

Front 170

4

Back 170

What is the coefficient of iron when the following equation is balanced with smallest whole number coefficients?
Fe(s) + O2(g) -----> Fe2O3(s)

Front 171

acid-base

Back 171

Classify the following reaction:
H2SO4(aq) + 2KOH(aq) ----> K2SO4(aq) + 2H2O(aq)

Front 172

precipitation

Back 172

Choose the best classification of the reaction represented by the following equation:
Pb(NO3)2(aq) + CaCl2(aq) -----> PbCl2(s) + Ca(NO3)2(aq)

Front 173

single-replacement

Back 173

Choose the best classification of the reaction represented by the following equation:
Zn(s) + CuSO4(aq) ----> ZnSO4(aq) + Cu(s)

Front 174

117 g

Back 174

What is the mass of 4.35 moles of aluminum?

Front 175

3.3 mol

Back 175

Consider the hypothetical reaction: 3A2 + 2B ---> C + 2D
How many moles of D can be formed from 5.0 mol of A2 and excess B?

Front 176

2C6H14(l) + 19O2(g) ----> 12CO2(g) + 14H2O(l)

Back 176

Which of the choices is the correctly balanced form of the following equation?
C6H14(l) + O2(g) ---> CO2(g) + H2O(l)

a) C6H14(l) + 13O2(g) ----> 6CO2(g) + 7H2O(l)
b) C6H14(l) + 19O(g) ----> 6CO2(g) + 7H2O(l)
c) C6H14(l) + 19O2(g) ----> 6CO2(g) + 7H2O(l)
d) 2C6H14(l) + 19O2(g) ----> 12CO2(g) + 14H2O(l)
e) C12H28(l) + 38O(g) ----> 12CO2(g) + 14H2O(l)

Front 177

2.91 x 10^24 atoms

Back 177

How many atoms of sulfur are presented in 155 g of sulfur? [Use atomic mass: S, 32.06 amu]

Front 178

3.32 x 10^23

Back 178

How many iron atoms are presented in 0.552 mol of iron?

Front 179

1.80 x 10^-3 mol

Back 179

Aspirin is the common name for acetyl salicylic acid, C9H8O4. A tablet has 0.325 g of aspirin. How many moles is this? [Use formula mass: aspirin, 180.2 amu]

Front 180

2.6 g

Back 180

What is the mass of 3.5 X 10^22 molecules of CO2?

Front 181

4.81 g

Back 181

How many grams of sulfur are found in 0.150 mol of sulfur? [Use atomic mass: S, 32.06 g/mol]

Front 182

179.4 g

Back 182

Iron reacts with oxygen to form iron (III) oxide (Fe2O3). How many grams of product will be formed from 125.5 g of Fe? [Use atomic masses: Fe, 55.85 amu; O, 16.00 amu]

Front 183

MgS

Back 183

Select the ionic compound which is insoluble in water.

a) Na2CO3
b) Fe(NO3)3
c) KBr
d) MgS
e) NH4Br

Front 184

3.24 g

Back 184

How many grams are there in 0.0200 mol of nicotine, a yellow liquid? [Use formula mass: nicotine, 162.2 amu]

Front 185

precipitation

Back 185

Classify the following reaction:
Na2S(aq) + CuSO4(aq) ---> Na2SO4(aq) + CuS(s)

Front 186

acid-base

Back 186

Classify the reaction:
2HCl(aq) + Ba(OH)2(aq) ----> BaCl2(aq) + 2H2O(l)

Front 187

combustion

Back 187

Choose the best classification of the reaction represented by the following equation:
C6H1206(s) + 6O2(g) ---> 6CO2(g) + 6H2O(l)

Front 188

6.53 g

Back 188

Magnesium hydroxide (Mg(OH)2), as "Milk of Magnesia" can be used to neutralize excess stomach acid, represented by HCl(aq):
Mg(OH)2(s) + 2HCl(aq) ---> MgCl2(aq) + 2H20(l)
When 5.00 g of HCl are combined with an excess of Mg(oh)2, what mass of MgCl2 can be produced? [Use molar masses: H, 1.01 g/mol; O, 16.00 g/mol; Mg, 24.31 g/mol; Cl. 35.45 g/mol]

Front 189

4 mol

Back 189

How many moles of HCl can be formed when 2 mol of hydrogen gas react with chlorine?
H2(g) + Cl2(g) ---> HCl(g) (unbalanced)

Front 190

0.0570 mol

Back 190

Calculate the number of moles in 10.0 grams of BaF2.

Front 191

double-replacement

Back 191

The reaction
Na2SO4(aq) + Ba(OH)2(aq) ---> BaSO4(s) + 2NaOH(aq) is classified as:

Front 192

oxidation-reduction

Back 192

Classify the following reaction:
Ce^4+(aq) + Fe^2+(aq) ----> Ce^3+(aq) + Fe^3+(aq)

Front 193

63.55 g

Back 193

The average mas of one atom of copper is 63.55 amu. What is the mass of Avagadro's number of atoms?

Front 194

FePO4

Back 194

What is the precipitate which forms when solutions of NaPO4 and FE(NO2)3 are mixed?

a) NaNO3
b) NaFe
c) FePO4
d) PO4NO3

Front 195

6.02 x 10^23 atoms/1 mol

Back 195

To convert a given number of moles into the number of atoms, you would multiply by which of the following factors?

a) 6.02 x 10^23 atoms/1 mol
b) 1 mol/6.02 x 10^23 atoms
c) 1.66 x 10^-24 atoms/1 mol
d) 1 mol/1.66 x 10^-24 atoms
e) molar mass

Front 196

copper(II) fluoride

Back 196

What is the name of CuF2 in the Stock system?

a) copper(I) fluoride
b) copper(II) fluorate
c) copper difluoride
d) copper fluoride
e) copper(II) fluoride

Front 197

They have high electron affinities

Back 197

Which one of the following is NOT true about elements that form cations?

a) The atoms lose electrons in forming ions
b) The elements are metals
c) They are located to the left of the periodic table
d) They have low ionization energies
e) They have high electron affinities

Front 198

ionic

Back 198

What kind of bond results when electron transfer occurs between atoms of two different elements?

a) ionic
b) covalent
c) nonpolar
d) single
e) double

Front 199

carbon and oxygen

Back 199

Assuming reactions between the following pairs of elements, which pair is most likely to form a covalent compound?

a) lithium and iodine
b) sodium and oxygen
c) calcium and chlorine
d) copper and tin
e) carbon and oxygen

Front 200

consists of four electrons shared between A and B

Back 200

A double bond between two atoms, A and B, ____________.

a) is longer than a single bond between the same two atoms.
b) has slower bond energy than a single bond between the same two atoms.
c) arises when two electrons are transferred from A to B.
d) consists of two electrons shared between A and B.
e) consists of four electrons shared between A and B.

Front 201

a nonelectrolyte solution

Back 201

What term describes a solution of a compound in water that does not conduct an electric current?

a) amorphous solution
b) an electrolyte solution
c) a nonelectrolyte solution
d) superconducting solution
e) isoelectric solution

Front 202

The bond between the nitrogen atoms in N2 is stronger than the bond in F2 and O2.

Back 202

Draw the Lewis structure of F2, O2, and N2. Which statement is true?

a) All three molecules have single bond between the atoms.
b) Both O2 and N2 have double bonds connecting the atoms.
c) Fluorine has the shortest bond between the two atoms.
d) The bond between the nitrogen atoms in N2 is stronger than the bond in F2 and O2.
e) All three molecules have triple bonds between the atoms.

Front 203

FeBr3

Back 203

The formula of iron(III) bromide is

a) FeBr
b) Fe3Br
c) Fe3Br3
d) FeBr3
e) Fe2Br3

Front 204

bent, bond angle close to 109.5 degrees

Back 204

In the molecule AX2, the central atom A has two lone pairs of electrons in addition to the two bond pairs in the A --- X bonds. What is the shape of this molecule?

a) bent, bond angle close to 109.5 degrees
b) bent, bond angle close to 120 degrees
c) linear
d) trigonal planer
e) trigonal pyramid

Front 205

magnesium cyanide

Back 205

Give the correct name for Mg(CN)2.

a) manganese carbon nitride
b) manganese dicyanide
c) magnesium dicarbon dinitride
d) magnesium(II) dicyanide
e) magnesium cyanide

Front 206

10

Back 206

How many bonding electrons are shown in the Lewis structure for the bicarbonate ion, HCO3^- ?

a) 6
b) 8
c) 10
d) 12
e) 14

Front 207

trigonal pyramidal

Back 207

According to the VSEPR theory, if the central atom has three bonded atoms and one lone pair, the geometry (shape) at this atom will be _____________.

a) linear
b) bent (angular)
c) trigonal planar
d) trigonal pyramidal
e) tetrahedral

Front 208

Cl

Back 208

Which of the following has the greatest electronegativity?

a) Si
b) P
c) Cl
d) Ar
e) Br

Front 209

linear

Back 209

What is the molecular geometry of CO2?

a) linear
b) trigonal Planar
c) angular
d) trigonal Pyramidal
e) tetrahedral

Front 210

nitrite ion

Back 210

What is the name of the ion NO2^- ?

a) nitrogen dioxide ion
b) nitrate ion
c) nitrote ion
d) nitrite ion
e) nitride ion

Front 211

A polar substance is soluble in water

Back 211

Which statement is true concerning the solubility of a substance in H2O?

a) Polar and nonpolar substances are equally soluble in water.
b) A nonpolar substance is soluble in water.
c) All substances are soluble in water.
d) Solubility of a substance in water has no relationship to the polarity of the substance being dissolved.
e) A polar substance is soluble in water.

Front 212

. .
[ : E ]^-
. .

Back 212

Which of the following Lewis structures of ions is incorrect?

a) [Na]^+
b) [Ca]^2+
c) [Sn]^4+
. .
d) [ : N : ]^3-
. .
. .
e) [ : E ]^-
. .

Front 213

dinitrogen pentoxide

Back 213

Give the correct name for N2O5.

a) nitrogen(IV) oxide
b) dinitrogen pentoxide
c) nitrogen oxide
d) nitrate
e) nitrite

Front 214

Na2CO3

Back 214

Write the formula of sodium carbonate.

a) NaCO2
b) Na2CO2
c) Na2CO3
d) Na(CO3)2
e) Na3CO3

Front 215

Na2SO4

Back 215

A certain compound has a very high melting point and when it dissolves in water the solution conducts electricity. Which one of the following compounds would have these properties?

a) O2
b) Cr
c) CCl4
d) Na2SO4
e) He

Front 216

F

Back 216

Which of the following has the greatest electronegativity?

a) H
b) Cl
c) O
d) F
e) Na

Front 217

Option B

Back 217

Which of the following Lewis structures would NOT have a resonance

. . . .
A. [ : O - N = O : ]^-
. .
. . . .
B. [ : N = O : ]^-

. .
: O :
. . I . .
C. [ : O - C = O : ]^2-
. . . .
. . . . . .
D. : O - S = O:
. .

: O :
. . II . .
E. : O - S - O :
. . . .

Front 218

The Lewis structure has a double bond between phosphorus and one of the fluorine atoms.

Back 218

Which of the following would NOT describe the Lewis structure of PF3?

a) The Lewis structure has a double bond between phosphorus and one of the fluorine atoms.
b) No resonance structures can be drawn.
c) The molecule has a lone pair (nonbonding pair) on the central atom.
d) The Lewis structure has 26 valence electrons.
e) The Lewis structure is not an exception to the octet rule.

Front 219

8

Back 219

How many bonding electrons are in CO2?

a) 1
b) 2
c) 3
d) 4
e) 8

Front 220

S^2

Back 220

Which of the following atoms and ions will have the largest radius?

a) S^2-
b) S
c) Cl
d) F
e) He

Front 221

1s2, 2s2, 2p6

Back 221

Give the complete electronic configuration of sodium ion.

a) 1s2, 2s2, 2p5
b) 1s2, 2s2, 2p6
c) 1s2, 2s2, 2p6, 3s1
d) 1s2, 2s2, 2p6, 3s2
e) 1s2, 2s2, 2p6, 3s2, 3p6, 4s1

Front 222

number of neutrons

Back 222

What does the mass number minus the atomic number represent?

a) number of protons
b) number of electrons
c) number of neutrons
d) number of protons - number of neutrons
e) number of neutrons - number of protons

Front 223

Cl

Back 223

Which one of the following elements has the highest electron affinity?

a) Li
b) K
c) Kr
d) O
e) Cl

Front 224

The model led to the understanding that the energy that the energy of an electron is quantized.

Back 224

Which statement is TRUE concerning Bohr's model of an atom?

a) The model involved the study of helium.
b) The model led to the understanding that the energy that the energy of an electron is quantized.
c) When electrons in an excited state return to the ground state, they absorb light.
d) Bohr's model explains that electrons have a negative charge.
e) The model defines the existence of orbitals.

Front 225

Rutherford

Back 225

Who discovered the existence of the atomic nucleus?

a) Crookes
b) Thompson
c) Geiger
d) Rutherford
e) Bohr

Front 226

de Broglie

Back 226

Who proposed that electrons could behave like waves, as well as like particles?

a) Thompson
b) Rutherford
c) Bohr
d) de Broglie
e) Heisenberg

Front 227

2000

Back 227

The total mass of the protons in any neutral atom is about _________ times the total mass of electrons in the atom.

a) 0.0005
b) 0.3
c) 1
d) 2
e) 2000

Front 228

S^2-

Back 228

Which of the following gives the correct charge of the ion according to the octet rule?

a) F+
b) Ba^2-
c) S^2-
d) P^3+
e) C^2+

Front 229

isotopes

Back 229

Which of the following accounts for the fact that chlorine has an atomic mass of 35.45 amu rather than a whole number?

a) isotopes
b) electrons
c) protons
d) radioactivity
e) isomers

Front 230

exothermic

Back 230

What kind of change is accompanied by the release of heat?

a) molecular
b) endothermic
c) exothermic
d) all physical changes
e) all chemical changes

Front 231

physical

Back 231

Conversion of ice to liquid water or liquid water to steam is an example of what kind of change?

a) physical
b) chemical
c) molecular
d) analytical
e) Both A and B are correct

Front 232

1.684 x 10^-3 lb

Back 232

How many pounds are represented by 764.6 mg? [Use: 1 pound = 454 g]

Front 233

2.65 L

Back 233

If the density of carbon tetrachloride is 1.59 g/mL, what is the volume in L, of 4.21 kg of carbon tetrachloride?

Front 234

2.18 y

Back 234

If a person smokes 10.0 packs of cigarettes a week and each cigarette contains 5.00 mg of tar, how many years will she have to smoke to inhale 0.250 pounds of tar? [Use: 20 cigarettes = 1 pack, 1 pound = 454 g and 1 year = 52 weeks]

Front 235

1.55 x 10^3 mL

Back 235

What volume, in milliliters, will 2.00 g of air occupy if the density is 1.29 g/L?

Front 236

10^6

Back 236

What does mega(M) equal?

Front 237

10^3

Back 237

What does kilo(k) equal?

Front 238

10^1

Back 238

What does deka(da) equal?

Front 239

10^-1

Back 239

What does deci(d) equal?

Front 240

10^-2

Back 240

What does centi(c) equal?

Front 241

10^-3

Back 241

What does milli(m) equal?

Front 242

10^-6

Back 242

What does micro(u) equal?

Front 243

10^-9

Back 243

What does nano(n) equal?

Front 244

chemistry

Back 244

Name the branch of science that involves the study of matter and the changes it undergoes?

Front 245

matter

Back 245

What do we call anything that has a mass and occupies space?

Front 246

scientific law

Back 246

A summary of a large amount of scientific information, is meant by what term?

Front 247

technology

Back 247

What word means the application of scientific principles to meeting human needs?

Front 248

number and units

Back 248

When the value of an experimental quantity or measurement (e.g. the mass of a tablet) is reported, it should consist of two parts. What are they?

Front 249

unit

Back 249

What do we call a basic quantity of mass, volume, time, etc.?

Front 250

error

Back 250

What is defined as the difference between the true value and our measurement of that value?

Front 251

accuracy

Back 251

The agreement between the true value and the measured value of a quantity, is defined as what?

Front 252

precision

Back 252

What do we call the degree of agreement between replicate measurements of the same quantity?

Front 253

uncertainty

Back 253

What do we call the degree of doubt in a single measurement?

Front 254

mass

Back 254

The quantity of matter in a sample measured comparing to a standard weight, is meant by what word?

Front 255

a balance

Back 255

What instrument is used to measure the mass of an object?

Front 256

weight

Back 256

What experimental quantity gives the force resulting from the pull of gravity upon an object?

Front 257

heat

Back 257

What form of energy is usually absorbed or liberated during chemical reactions?

Front 258

kinetic energy and potential energy

Back 258

In the swinging of a pendulum, what two forms of energy are constantly being interconverted?

Front 259

potential energy

Back 259

What kind of energy is stored or the result of position or composition?

Front 260

concentration

Back 260

What do we call the experimental quantity which gives the number of particles of a substance (or their mass) contained per unit volume?

Front 261

mass; volume

Back 261

The density of an object is the ratio of its _______ to its ________.

Front 262

analytical chemistry

Back 262

What is the branch of chemistry that is being applied in measuring the concentration of an air pollutant?

a) analytical chemistry
b) biochemistry
c) inorganic chemistry
d) organic chemistry
e) physical chemistry

Front 263

law

Back 263

What do we call a statement of observed behavior for which no exceptions have been found?

a) hypothesis
b) theory
c) law
d) model
e) result

Front 264

solid

Back 264

In which state does matter have a definite shape and volume?

Front 265

gas

Back 265

In which state of matter are forces between particles least dominant?

Front 266

physical

Back 266

What kind of change does not alter the composition or identity of the substance undergoing the change?

Front 267

chemical

Back 267

what type of change is represented by the decay of a fallen tree?

Front 268

reactants and products

Back 268

What do we call the starting and final materials in a chemical reaction?

Front 269

intensive

Back 269

What type of property of matter is independent of the quantity of the substance?

Front 270

pure substance

Back 270

The substance consists of only one component; it has a fixed composition throughout, is meant in chemistry by what term?

Front 271

elements and compounds

Back 271

what are two kinds of pure substance?

Front 272

compound

Back 272

A pure substance consisting of two or more elements chemically combined in a definite ratio, is meant in chemistry by what term?

Front 273

homogeneous and heterogeneous

Back 273

What are the two classes of mixtures?

Front 274

homogeneous

Back 274

What kind of mixture is a solution of alcohol and water?

Front 275

anions

Back 275

What do we call electrically charged particles that result from the gain of one or more electrons by a parent atom?

Front 276

J.J. Thompson

Back 276

Who announced in 1897 that cathode rays consisted of a stream of electrons?

Front 277

spectroscopy

Back 277

What word means the study of wavelengths of light emitted and absorbed by atoms?

Front 278

quantum number

Back 278

In Bohr's theory of the atom, what is the number n (n = 1, 2, 3, 4) called?

Front 279

flash point

Back 279

Which of the following is NOT a physical property of matter?

a) odor
b) compressibility
c) flash point
d) melting point
e) color

Front 280

physical

Back 280

What kind of change does NOT alter the composition of identity of the substance undergoing the change?

a) molecular
b) endothermic
c) exothermic
d) physical
e) chemical

Front 281

flammability

Back 281

Which of the following is a chemical property?

a) flammability
b) color
c) hardness
d) odor
e) taste

Front 282

mass

Back 282

Which one of the following is an example of an extensive property?

a) density
b) specific gravity
c) mass
d) hardness
e) boiling temperature

Front 283

ethyl alcohol

Back 283

Which one of the following is an example of a pure substance?

a) ethyl alcohol
b) sugar water
c) salt and pepper
d) milk
e) sand

Front 284

mixture

Back 284

Air is a/an

a) element
b) compound
c) mixture
d) molecule
e) pure substance

Front 285

heterogeneous

Back 285

What type of mixture is represented by a collection of salt and pepper?

a) atoms
b) molecules
c) solution
d) heterogeneous
e) homogeneous

Front 286

protons and neutrons

Back 286

What kind(s) of particles can be found in the nucleus of an atom?

a) protons
b) neutrons
c) electrons
d) protons and electrons
e) protons and neutrons

Front 287

hydrogen - 3

Back 287

Which isotope of hydrogen has two neutrons?

a) hydrogen - 1
b) hydrogen - 2
c) hydrogen - 3
d) deuterium
e) H2

Front 288

alpha

Back 288

In Rutherford's & Geiger's experiment which led to the discovery of the atomic nucleus, what type of particle or ray was fired at the gold foil target?

a) alpha
b) beta
c) gamma
d) neutrons
e) cathode rays

Front 289

Mendeleev and Meyer

Back 289

Which two scientists in 1869 arranged the elements in order of increasing atomic masses to form a precursor of the modern periodic table of elements?

Front 290

Dimitri Mendeleev

Back 290

Who stated that the elements, when arranged according to their atomic masses, showed a distinct periodicity of their properties?

Front 291

increasing atomic number

Back 291

In the modern periodic table, the elements are arranged according to what system?

Front 292

atomic number

Back 292

The modern periodic law states that the physical and chemical properties of the elements are periodic functions of what property?

Front 293

seven

Back 293

How many periods are found on the periodic table?

Front 294

metalloids

Back 294

What term is used for the elements straddling the "staircase" boundary between the metals and nonmetals?

Front 295

1

Back 295

How many orbitals are in the s sub level?

Front 296

3

Back 296

How many orbitals are in the p sub level?

Front 297

Aufbau Principle

Back 297

Electrons occupy the available orbital of lowest energy first, is known as what principle?

Front 298

Octet Rule

Back 298

Elements tend to react in such a way as to attain the electron configuration of the atoms of the noble gas nearest to them in the Periodic Table, is known as what rule?

Front 299

bottom left

Back 299

Atoms with the biggest radii occur in the __________ __________ region of the Periodic Table.

Front 300

atomic mass

Back 300

In Mendeleev's table of the elements, they were arranged according to

a) atomic number
b) mass number
c) atomic mass
d) neutron number
e) density

Front 301

representative elements

Back 301

What are all the elements in the A-groups often called?

a) transition elements
b) lanthanides
c) metals
d) non-metals
e) representative elements

Front 302

3

Back 302

How many sublevels are there in the third principle energy level?

a) 3
b) 2
c) 1
d) 0
e) 4

Front 303

3

Back 303

How many orbitals are there in a p sub level?

a) 2
b) 3
c) 1
d) 0
e) 4

Front 304

1s2, 2s1

Back 304

Which one of the following electron configurations is appropriate for a normal atom?

a) 1s1, 2s1
b) 1s2, 2s1
c) 1s2, 2s2, 2p8
d) 1s2, 2s2, 2p4, 3s1
e) 1s2, 2s2, 2p6, 3d1

Front 305

Al

Back 305

Which of the following elements is most likely to form a 3+ ion?

a) Li
b) K
c) Al
d) N
e) Cu

Front 306

Cl^2-

Back 306

Which of the following ions does not follow the octet rule?

a) Na+
b) Ca^2+
c) Al^3+
d) N^3-
e) Cl^2-

Front 307

Ne

Back 307

Which of the following elements has the highest ionization energy?

a) Li
b) B
c) O
d) F
e) Ne

Front 308

Li

Back 308

Which of the following elements has the lowest ionization energy?

a) Li
b) B
c) O
d) F
e) Ne

Front 309

the energy released when an isolated atom gains an electron

Back 309

The electron affinity is

a) the energy required to remove an electron from an isolated atom
b) the force between two electrons in the same orbital
c) the force between two ions of opposite charge
d) the energy released when an isolated atom gains and electron
e) the attraction of an atom for an electron in a chemical bond

Front 310

valence electrons

Back 310

In Lewis structure, what do the dots represent?

Front 311

ionic and covalent bonding

Back 311

What are the two principle types of bonding called?

Front 312

metal and nonmetal

Back 312

Name the two classes of element which are most likely to form an ionic compound if they are allowed to react with each other?

Front 313

Pauling

Back 313

Who first assigned electronegativity values to many of the elements?

Front 314

crystal lattice

Back 314

What do we call the three-dimensional arrangement of positive and negative ions in an ionic solid?

Front 315

lower positive charge

Back 315

What does the suffix "-ous" on the common names of ions means?

Front 316

polyatomic

Back 316

What is the term used for ions that are composed of two or more atoms bonded together?

Front 317

ammonium

Back 317

What is the name of the ion NH4+?

Front 318

covalent

Back 318

What kind of bonding exists in substances which consist of discrete molecules?

Front 319

boiling point

Back 319

At what temperature is a liquid converted into a gas?

Front 320

amorphous

Back 320

What is the term that describes a solid with no regular structure?

Front 321

electrolyte

Back 321

What is the term that describes a compound that, when dissolved in water conducts an electric current?

Front 322

covalent

Back 322

What kind of bonding is present in substances which are non electrolytes?

Front 323

10

Back 323

How many bonding electrons are shown in the Lewis structure for the bicarbonate ion, HCO3^-?

Front 324

energy

Back 324

What is defined as the amount of energy needed to break a bond holding two atoms together?

Front 325

bond length

Back 325

What is defined as the distance of separation of two nuclei in a covalent bond?

Front 326

Valence Shell Electron Pair Repulsion

Back 326

What do the letters VSEPR stand for?

Front 327

120 degrees

Back 327

If the shape of a molecule is trigonal planar, what are the values of the bond angles?

Front 328

.
. Al .

Back 328

Which of the following Lewis structures of neutral atoms is correct?

a) K
b) . Ba

.
c) . Al .

d) . Sn .

.
e) . O .
.

Front 329

[ Sn]^2+

Back 329

Which of the following Lewis structures of ions is incorrect?

a) [ Na ] ^+
b) [ Ca ] ^2+
c) [ Sn ] ^2+

. .
d) [ : N : ]^3-
. .

Front 330

polar covalent

Back 330

In the compound CH3Cl, the bond between carbon and chlorine is

a) intermolecular
b) ionic
c) nonpolar covalent
d) polar covalent

Front 331

They have high electron affinities

Back 331

Which one of the following is NOT true about elements that form cations?

a) The atoms lose electrons in forming ions
b) The elements are metals
c) They are located to the left of the periodic table
d) They have low ionization energies
e) They have high electron affinities

Front 332

Li, Mg

Back 332

Which of the following pairs of atoms are least likely to form an ionic compound?

a) Ni, O
b) Na, F
c) Cu, Cl
d) Li, Mg
e) Li, F

Front 333

triple bond

Back 333

The bond in dinitrogen (N2) is a:

a) double bond
b) single bond
c) triple bond
d) lone pair
e) none of the above

Front 334

H - F

Back 334

Which of the following bonds is most polar?

a) H - F
b) H - Cl
c) H - H
d) F - F
e) H - I

Front 335

cesium and iodine

Back 335

Assuming reactions between the following pairs of elements, which pair is most likely to form an ionic compound?

a) copper and tin
b) chlorine and oxygen
c) cesium and iodine
d) carbon and chlorine
e) fluorine and iodine

Front 336

cuprous ion

Back 336

What is the old name of Cu+?

a) cupric ion
b) cuprous ion
c) copper(I) ion
d) copper(II) ion
e) ferrous ion

Front 337

melting point

Back 337

What term describes the temperature at which a solid is converted into a liquid?

a) critical point
b) flash point
c) sublimation point
d) melting point
e) boiling point

Front 338

0

Back 338

How many nonbonding electrons are in CH4?

a) 0
b) 1
c) 2
d) 3
e) 8

Front 339

32

Back 339

How many valence electrons are in SO4^2-?

a) 2
b) 64
c) 32
d) 12
e) 16

Front 340

trigonal pyramidal

Back 340

According to VSEPR theory, if the valance electrons on a central atom are 3 bond pairs and one nonbonding (lone) pair, the geometry (shape) of this atom will be

a) linear
b) bent (angular)
c) trigonal planar
d) trigonal pyramidal
e) tetrahedral

Front 341

law of conservation of mass

Back 341

What law states that matter cannot be gained or lost during a chemical reaction?

Front 342

The reactant or product to which this applies is aqueous, i. e. dissolved in water

Back 342

what does the symbol "(aq)", often found in chemical equations mean?

Front 343

Ca(s) + 2HCl(g) ---> CaCl2(s) + H2(g)

Back 343

Balance the following equation:

Ca(s) + HCl(g) ---> CaCl2(s) + H2(g)

Front 344

Mg(OH)2(s) + 2HCl(g) ----> MgCl2(s) + 2H2O(l)

Back 344

Balance the following equation:

Mg(OH)2(s) + HCl(g) ----> MgCl2(s) + H2O(l)

Front 345

2Na(s) + Cl2(g) ----> 2NaCl(s)

Back 345

Balance the following equation:

Na(s) + Cl2(g) ----> NaCl(s)

Front 346

2C8H18(l) + 25O2(g) ----> 16CO2(g) + 18H20(l)

Back 346

Balance the equation for the combustion of octane, a component of gasoline, using smallest whole number coefficients:

C8H18(l) + O2(g) ----> CO2(g) + H20(l)

Front 347

C6H12O6(l) + 6O2(g) ----> 6CO2(g) + 6H2O(l)

Back 347

Balance the equation for the complete oxidation of glucose (C6H12O6), an important metabolic process:

C6H12O6(l) + O2(g) ----> CO2(g) + H2O(l)

Front 348

1.01 g

Back 348

What is the weight, in grams, of one mole of hydrogen atoms? [Use atomic weight: H, 1.01 amu]

a) 1.01 g
b) 2.02 g
c) 2.52 g
d) 6.02 x 10^23 g
e) 1.81 x 10^24 g

Front 349

4

Back 349

What number will be found in front of "Al" when the following equation is balanced with smallest whole number coefficients?

Al(s) + O2(g) ----> Al2O3(s)

a) 1
b) 2
c) 3
d) 4
e) 8

Front 350

solids and liquids

Back 350

Which two states of matter are the least compressible?

Front 351

barometer

Back 351

What device is used to measure atmospheric pressure?

Front 352

pressure

Back 352

What experimental quantity measures force per unit area?

Front 353

Boyle's Law

Back 353

The volume of a gas is inversely proportional to the pressure, if the number of moles (or mass) and the temperature of the gas are kept constant, is known as who's law?

Front 354

Charle's Law

Back 354

The volume of a gas is directly proportional to the absolute temperature, if the number of moles (or mass) and the pressure of the gas are kept constant, is known as who's law?

Front 355

Avogadro's Law

Back 355

Equal volumes of any ideal gas, at the same temperature and pressure, contain the same number of moles, is known as who's law?

Front 356

Avagadro's

Back 356

What law predicts the expansion of a balloon when helium is added?

Front 357

Dalton

Back 357

Who found that a mixture of gases exerts a total pressure that is the sum of the pressures that each gas would exert if each were present alone under similar conditions?

Front 358

kinetic molecular theory

Back 358

What is the name of the theory which deals with particle behavior in the gas phase?

Front 359

viscosity

Back 359

The resistance of a liquid to flow, is meant by what term?

Front 360

surface tension

Back 360

What experimental quantity is a measure of the attractive forces between molecules at the surface of a liquid?

Front 361

condensation

Back 361

What process is responsible for the formation of dew on the grass early in the morning?

Front 362

Fritz London

Back 362

Who postulated the existence of temporary dipole attraction among nonpolar molecules?

Front 363

atmospheric pressure

Back 363

A barometer measures

a) the pressure of a gas sample in a container
b) the difference in pressure between two gas samples
c) the difference in pressure between a gas sample and atmospheric pressure
d) atmospheric pressure
e) the pressure of an ideal gas

Front 364

Boyle

Back 364

Who formulated the relationship between the volume and the pressure of a gas?

a) Boyle
b) Charles
c) Dalton
d) Gay-Lussac
e) Torricelli

Front 365

Charles

Back 365

Who formulated the relationship between the volume and temperature of a gas?

a) Boyle
b) Charles
c) Dalton
d) Gay-Lussac
e) Torricelli

Front 366

22.4 L

Back 366

What is the volume occupied by one mole of helium at 0 degree C and 1 atm pressure?

a) 1.0 L
b) 22.4 L
c) 4.0 L
d) 40.0 L
e) 12.2 L

Front 367

Gas particles lose energy only when they collide with walls of the container.

Back 367

Which of the following statements conflicts with the kinetic molecular theory of gases?

a) There are no forces between gas particles.
b) Gas particles occupy a negligible volume compared with the volume of their container.
c) The average kinetic energy of the gas particles is proportional to the absolute temperature.
d) Gas particles lose energy only when they collide with walls of the container.
e) Gas particles are in constant, random motion.

Front 368

absolute temperature

Back 368

What quantity is directly proportional to the kinetic energy of the particles in a gas?

a) distance between molecules
b) absolute temperature
c) atomic mass
d) formula mass
e) volume of the individual particles

Front 369

H2

Back 369

Of the following gases, which will behave most like an ideal gas?

a) H2
b) HF
c) NH3
d) CH3Cl
e) CO

Front 370

viscosity

Back 370

What is the experimental quantity that serves as a measure of resistance to flow of a liquid?

a) vapor pressure
b) surface tension
c) resistivity
d) viscosity
e) compressibility

Front 371

evaporation

Back 371

What is the term that describes a liquid changing to a vapor at a temperature less than its boiling point?

a) evaporation
b) sublimation
c) dissociation
d) condensation
e) supercooling

Front 372

FeSO4(aq) + 2 NaOH(aq) ----> Fe(OH)2(s) + Na2SO4(aq)

Back 372

Complete the products and balance the following equation for a precipitation reaction:

FeSO4(aq) + NaOH(aq)

Front 373

HCl(aq) + KOH(aq) ----> KCl(aq) + H2O(l)

Back 373

Complete the products and balance the following equation for acid-base reaction:

HCl(aq) + KOH(aq)

Front 374

decomposition

Back 374

Classify the following reaction:

2H2O(l) -----> 2H2(g) + O2(g)

Front 375

double-replacement

Back 375

Classify the following reaction:

H2SO4(aq) + Ba(OH)2(aq) -----> BaSO4(s) + 2H2O(g)

Front 376

single-replacement

Back 376

Classify the following reaction:

Mg(s) + 2HCl(aq) ----> MgCl2(g) + H2(g)

Front 377

combination

Back 377

Classify the following reaction:

2Na(s) + Cl2(g) -----> 2NaCl(s)

Front 378

acid-base

Back 378

Choose the best classification of the reaction represented by the following equation:

HNO3(aq) + KOH(aq) ---> KNO3(aq) + H20(l)

a) combustion
b) acid-base
c) precipitation
d) decomposition
e) combination

Front 379

oxidation-reduction

Back 379

Choose the best classification of the reaction represented by the following equation:

2Fe^3+(aq) + Fe(s) ----> 3Fe^2+(aq)

a) combustion
b) acid-base
c) precipitation
d) decomposition
e) oxidation-reduction

Front 380

combination

Back 380

Choose the best classification of the reaction represented by the following equation:

MgO(s) + CO2(g) ----> MgCO3(s)

a) single-replacement
b) double replacement
c) combination
d) decomposition
e) precipitation

Front 381

decomposition

Back 381

Choose the best classification of the reaction represented by the following equation:

CuSO45H2O(s) -----> CuSO4(s) + 5H2O(l)

a) single-replacement
b) double replacement
c) combination
d) decomposition
e) oxidation-reduction

Front 382

double-replacement

Back 382

Choose the best classification of the reaction represented by the following equation:

BaCl2(aq) + K2SO4(aq) ------> BaSO4(s) + 2KCl(aq)

a) single-replacement
b) double replacement
c) combination
d) decomposition
e) oxidation-reduction