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Chemistry Flashcards

1
Q

If the number of neutrons changes within an atom, then what new form of that atom has been created?
a. an ion
b. an isotope
c. an element
d. a cation

A

B

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2
Q
  1. Hydrogen gas (H2) and oxygen gas (O2) can be combined to make water (H2O). In this situation, water is the
    a. product
    b. reactant
    c. enzyme
    d. substrate
A

A

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3
Q
  1. The contents of the human stomach are very acidic, whereas the interior of the small intestine that receives the food from the stomach tends to be basic. Relative to that of the stomach, the pH of the small intestine should be
    a. higher
    b. lower
    c. equal
    d. neutral
A

A

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4
Q
  1. Two pure substances are combined to make a third substance by sharing electrons evenly between them. The type of bond described is a
    a. hydrogen bond
    b. ionic bond
    c. polar covalent bond
    d. nonpolar covalent bond
A

D

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5
Q
  1. Water is used as a reactant during which of the following types of reactions?
    a. dehydration synthesis
    b. hydrolysis
    c. condensation
    d. both a and c
A

B

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6
Q
  1. Monosaccharides are to polysaccharides as amino acids are to
    a. nucleic acids
    b. dipeptides
    c. polynucleotides
    d. polypeptides
A

D

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7
Q
  1. All of the following are considered lipids except
    a. waxes
    b. oils
    c. sugars
    d. fats
A

C

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8
Q
  1. If a triathlete is preparing for a race and needs sustained energy, which of the following foods would be best to consume shortly before the competition?
    a. beef jerky for complete proteins
    b. fruit juice for simple sugars
    c. pasta for complex carbohydrates
    d. nuts for healthy fats
A

C

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9
Q
  1. Which of the following macromolecules is responsible for storing the genetic code?
    a. DNA
    b. proteins
    c. RNA
    d. phospholipids
A

A

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10
Q
  1. Protons are
    a. used to determine mass number
    b. positive in charge
    c. used to determine atomic number
    d. all of the above
A

D

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11
Q
  1. What is a common metric unit of mass used in the laboratory?
A

G kg

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12
Q
  1. What is a common metric unit of length used for measuring small objects in the laboratory?
A

Cm mm

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13
Q
  1. What is a common metric unit of volume used in the laboratory?
A

ml

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14
Q
  1. What is a common metric unit of pressure used in the laboratory?
A

Milliliter of mercury

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15
Q
  1. What is a common metric unit of energy?
A

Joule

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16
Q
  1. What is the metric prefix that represents 1,000?
A

Kilo

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17
Q
  1. What is the metric prefix that represents 1/1000?
A

Mili

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18
Q
  1. What is the metric prefix that represents 1/100?
A

Centi

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19
Q
  1. What is the metric prefix that represents 10^–9?
A

Nano

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20
Q
  1. What is the metric prefix that represents 10^6?
A

Mega

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21
Q
  1. Which metric unit is most appropriate for expressing the mass of an adult human?
A

Kg

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22
Q
  1. Which metric unit is most appropriate for recording the volume of a child’s wooden block?
A

Cubic centimeters

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23
Q
  1. Which metric unit would a scientist use to measure the temperature on a warm autumn day?
A

C*

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24
Q
  1. Which metric unit is most often used for small doses of solid medications?
A

mg

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25
Q
  1. Which SI base unit is named after a person?
A

Kelvin or ampere

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26
Q
  1. Which English unit is most similar in volume to a liter?
A

Quart

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27
Q
  1. Which English unit is most similar in length to a meter?
A

Yard

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28
Q
  1. How many fluid ounces are in a cup?
A

8

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29
Q
  1. An Olympic swimmer competes in the 100-meter freestyle. What is the comparableEnglish unit?
A

Yard

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30
Q
  1. If a wooden board’s width is 6 in., what is an appropriate metric unit to express this width?
A

Cm

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31
Q
  1. Which phase of matter doesn’t have a definite shape or a definite volume under normal conditions?
A

Gas

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32
Q
  1. Which phase of matter has a definite shape and a definite volume?
A

Solid

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33
Q
  1. Which phase of matter has a definite volume but takes the shape of the containerthat it’s in?
A

Liquid

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34
Q
  1. When matter changes from a liquid to a solid, which phase change is it going through?
A

Freezing

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35
Q
  1. When matter changes from a gas to a liquid, which phase change is it going through?
A

Condensation

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36
Q
  1. When matter changes from a liquid to a gas, which phase change is it going through?
A

Vaporization

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37
Q
  1. When matter changes from a solid to a gas without becoming a liquid in between, which phase change is it going through?
A

Sublimation

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38
Q
  1. When matter changes from a gas to a solid without becoming a liquid in between, which phase change is it going through?
A

Deposition

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39
Q
  1. Gold
A

Pure substance
Element

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40
Q
  1. Table sugar
A

Pure
Compound

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41
Q
  1. Fresh air
A

Mix homogeneous

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42
Q
  1. Oxygen
A

Pure
Element

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43
Q
  1. Vegetable soup
A

mixture heterogeneous.

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44
Q
  1. Fruit salad
A

mixture heterogeneous

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45
Q
  1. Calcium
A

Pure
Element

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46
Q
  1. Concrete
A

Mix het

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47
Q
  1. Smog
A

Mix heterogeneous

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48
Q
  1. Which type of property of matter doesn’t depend on the amount of the substance that’s present?
A

Intensive

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49
Q
  1. Which type of change involves a change in the form of a substance?
A

Physical

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50
Q
  1. Which type of change involves a change in the identity of a substance?
A

Chemical

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51
Q
  1. Which type of property of matter depends on exactly how much of the substance is present?
A

Extensive

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52
Q
  1. Density is a(n) _______________ (chemical/extensive physical/intensive physical) property.
A

Intensive physical

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53
Q
  1. Length is a(n) _______________ (chemical/extensive physical/intensive physical) property.
A

Extensive physical

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54
Q
  1. Color is a(n) _______________ (chemical/extensive physical/intensive physical) property.
A

Intensive physical

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55
Q
  1. Flammability is a(n) _______________ (chemical/extensive physical/intensive physical) property.
A

Chemical

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56
Q
  1. Mass is a(n) _______________ (chemical/extensive physical/intensive physical) property.
A

Extensive physical

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57
Q
  1. Odor is a(n) _______________ (chemical/extensive physical/intensive physical) property.
A

Intensive physical

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58
Q
  1. Ductility is a(n) _______________ (chemical/extensive physical/intensive physical) property.
A

Intensive physical

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59
Q
  1. Electrical conductivity is a(n) _______________ (chemical/extensive physical/intensive physical) property.
A

Intensive physical

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60
Q
  1. Solubility is a(n) _______________ (chemical/extensive physical/intensive physical) property.
A

Intensive physical

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61
Q
  1. Which unit represents the amount of energynecessary to raise the temperature of 1 g of water by 1°C?
A

Calorie

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62
Q
  1. Which SI unit is used to express the heat content of a mole of a chemical?
A

Kilojoules or mole

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63
Q
  1. Which unit is used to express the energy found in food?
A

Calorie

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64
Q
  1. A bucket on a ladder has __________ (kinetic/potential) energy, which is the energy of __________ (motion/position).
A

Potential
Position

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65
Q
  1. A rolling ball has __________ (kinetic/potential) energy, which is the energy of __________ (motion/position).
A

Kinetic
Motion

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66
Q
  1. Fuels contain __________ (moving/stored) energy, which is __________ (kinetic/potential) energy.
A

Stored
Potential

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67
Q
  1. Average kinetic energy can be measured in what units?
A

Celsius, Fahrenheit kelvin’s

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68
Q
  1. If water is heated to 80.0°C, how many kelvins is that?
A

80 k

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69
Q
  1. The melting point of sodium chloride is 1,074 K. What temperature is this in degrees Celsius?
A

801 C

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70
Q
  1. How many protons are in an atom of sodium?
A

11 protons

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71
Q
  1. How many electrons are in an atom of bromine?
A

35 electrons

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72
Q
  1. How many electrons are in an atom of nickel?
A

28 electrons

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73
Q
  1. How many protons are in an atom of radon?
A

86 protons

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74
Q
  1. How many neutrons are in an atom of isotope potassium-40?
A

21 neutron

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75
Q
  1. How is the atomic number related to the number of protons in an atom?
A

Atomic #= # protons

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76
Q

.. 197. How is the mass number of an atom related to the number of neutrons?

A

Atomic mass = protons +neutrons

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77
Q
  1. How many protons, electrons, and neutrons are in an atom of isotope copper-63?
A

29 protons, 29 electrons, 34 neutrons

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78
Q
  1. An atom has a mass number of 14 and 6electrons. How many protons and neutrons does it have?
A

6 protons 8 neutrons

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79
Q
  1. An atom has 40 electrons and 51 neutrons. What is its mass number, and how many protons does it have?
A

Mass # 91, 40 protons

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80
Q
  1. What does the top number in isotope notation represent?
A

Mass #

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81
Q
  1. What does the bottom number in isotope notation represent?
A

protons

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82
Q
  1. How many protons and neutrons are in 18/9 ^ F
A

9 protons 9 neutrons

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83
Q
  1. How many protons and neutrons are in 25/11 ^ Na
A
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84
Q
  1. What is the isotope notation for an atom of carbon-12?
A
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85
Q
  1. What is the isotope notation for an atom of chlorine-37?
A
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86
Q
  1. What is the name of 35/18 ^Ar
A
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87
Q
  1. How does an ion differ from an atom of the same element with regard to the numbers ofsubatomic particles?
A
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88
Q
  1. When two atoms or ions have the same number of electrons, they’re said to be __________.
A
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89
Q
  1. When an ion has a positive charge, how do the numbers of subatomic particles differ?
A
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90
Q
  1. When an ion has a negative charge, how do the numbers of subatomic particles differ?
A
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91
Q
  1. How many protons and electrons does 40/20 ^ Ca ^2+ have?
A
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92
Q
  1. How many protons and electrons does 131/53 ^ I ^1-
A
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93
Q
  1. How many protons and electrons does 30/13 ^ Al ^3+ have?
A
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94
Q
  1. How many protons and electrons does 33^ P ^3-
A
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95
Q
  1. What is the isotope notation for an ion of silver-109 with a charge of positive 1?
A
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96
Q
  1. What is the isotope notation for an ion of sulfur-34 with a charge of negative 2?
A
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97
Q
  1. How many protons, neutrons, and electrons are in 52^ Cr^ 6+
A
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98
Q
  1. How many protons, neutrons, and electrons are in 62^Ni^3+
A
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99
Q
  1. What is the name of the premise that one electron fills each orbital in a subshell until all orbitals contain one electron and then electrons are added to fill in the second available spot in the subshell?
A
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100
Q
  1. What rule or principle describes the order in which electrons fill orbitals?
A
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101
Q
  1. What is the maximum number of electrons that can be in the f orbitals?
A
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102
Q
  1. What is the maximum number of electrons that can be in the p orbitals?
A
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103
Q
  1. What is the electron configuration of carbon?
A
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104
Q
  1. What is the electron configuration of magnesium?
A
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105
Q
  1. What is the electron configuration of argon?
A
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106
Q
  1. What is the electron configuration of bromine?
A
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107
Q
  1. What is the electron configuration of zirconium?
A
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108
Q
  1. What is the expected electron configuration of plutonium?
A
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109
Q
  1. Which quantum number describes the spin of the electron?
A
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110
Q
  1. Which quantum number describes the average distance between the nucleus and the orbital?
A
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111
Q
  1. Which quantum number describes how the various orbitals are oriented in space?
A
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112
Q
  1. Which quantum number describes the shape of the orbital?
A
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113
Q
  1. What are the possible values for the spin quantum number?
A
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114
Q
  1. The decimal numbers in the blocks of the periodic table represent the __________.
A

Atomic mass

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115
Q
  1. What is the average atomic mass of lithium that is 7.59% lithium-6 (mass of 6.0151 amu) and 92.41% lithium-7 (mass of 7.0160 amu)?
A
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116
Q
  1. What is the average atomic mass of chlorine that is 75.78% chlorine-35 (mass of 34.96885 amu) and 24.22% chlorine-37 (mass of 36.9659 amu)?
A
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117
Q
  1. If the average atomic mass of boron is 10.81amu, what is the percent abundance of boron-11 (mass of 11.009306 amu) if the only other isotope is boron-10 (mass of 10.012937 amu)?
A
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118
Q
  1. What is the primary nuclear process that occurs in the sun?
A
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119
Q
  1. In which nuclear process does a nucleus split into two or more smaller elements and possibly some extra neutrons?
A
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120
Q
  1. What is it called when a helium nucleus is ejected from the nucleus of an atom during a nuclear reaction?
A
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121
Q
  1. When a 0/0 ^ y ray is a byproduct of a nuclear reaction, what nuclear process has occurred?
A
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122
Q
  1. What is the isotope (nuclear) notation for a particle that is produced from beta decay?
A
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123
Q
  1. A 0/+1 ^ e particle is a product of which nuclear reaction?
A
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124
Q
  1. 7/4 ^ Be + 0/-1 ^ e —> 7/3 ^ Li is an example of what type ofnuclear reaction?
A
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125
Q
  1. 228/92 ^ U —> 234/90 ^ Th + 4/2^He is an example of what type of nuclear reaction?
A
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126
Q
  1. 60/27 ^ Co —> 60/27 ^ Co + 0/0 ^ y is an example of what type of nuclear reaction?
A
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127
Q
  1. 32/15 ^ P —> 22/16 ^ S + 0/-1 ^e is an example of what type of nuclear reaction?
A
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128
Q
  1. ____ —> 230/86 ^ Rn + 4/2 ^ He
A
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129
Q
  1. 247/96 ^ Cm —> ____ + 4/2 ^ He
A
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130
Q
  1. 241/94 ^ Pu —> ___ + 241/95 ^Am
A
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131
Q
  1. 192/77 ^ Ir —> 192/77 ^ Ir + ____
A
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132
Q
  1. ___ + 0/-1 ^ e- —> 93/41 ^ Nb
A
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133
Q
  1. 2/1 ^H + ___ —> 4/2 ^ He + 1/0 ^ n
A
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134
Q
  1. 4/2 ^ He + 14/7 ^N —> ____+ 1/1 ^H
A
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135
Q
  1. 235/92 ^ U + 1/0 ^ n —> 134/54 ^ Xe t 100/38 ^Sr + ___
A
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136
Q
  1. After five half-lives, how many grams of a 400.-g radioactive sample remain undecayed?
A
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137
Q
  1. After three half-lives, how many grams of a 50.0-g radioactive sample have decayed?
A
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138
Q
  1. If 5.15 g of a radioactive sample remains undecayed after six half-lives, how many grams were in the original sample?
A
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139
Q
  1. A radioactive sample starts with 1.500 × 10^20 undecayed atoms. When measured again at a later date, the sample has 9.375 × 10^18 undecayed atoms. How many half-lives havepassed?
A
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140
Q
  1. What fraction of a sample remains undecayed after 39 hours if the half-life of the sample is 13 hours?
A
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141
Q
  1. Iodine-131 has a half-life of 8.02 days. If the original sample contained 25.0 g of iodine-131, how many grams have decayed after 56.14 days?
A
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142
Q
  1. Strontium-90 has a half-life of 28.9 years. How many grams were in the original sample if 11 g remain undecayed after 115.6years?
A
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143
Q
  1. In 5 minutes, a radioactive sample decays from 2.56 × 10^10 atoms to 8.00 × 10^8 atoms. How long is the isotope’s half-life?
A
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144
Q
  1. What fraction of a sample has decayed after 320 days if the half-life of the sample is 160days?
A
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145
Q
  1. If a radioactive sample decays from 2.5 kg to 0.61 g and the isotope has a half-life of 9.35 hours, how much time has passed?
A
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146
Q
  1. What is the symbol for the element carbon?
A

Co

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147
Q
  1. What is the symbol for the element chlorine?
A

Cl

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148
Q
  1. What is the symbol for the element aluminum?
A
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149
Q
  1. What is the symbol for the element cadmium?
A
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150
Q
  1. What is the symbol for the element copper?
A
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151
Q
  1. What is the symbol for the element arsenic?
A
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152
Q
  1. What is the symbol for the element sodium?
A

Na

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153
Q
  1. What is the symbol for the element potassium?
A

K

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154
Q
  1. What is the symbol for the element iron?
A
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155
Q
  1. What is the symbol for the element silver?
A
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156
Q
  1. What is the name of the element that has the symbol N?
A

Nitrogen?

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157
Q
  1. What is the name of the element that has the symbol S?
A
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158
Q
  1. What is the name of the element that has the symbol Br?
A
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159
Q
  1. What is the name of the element that has the symbol P?
A
160
Q
  1. What is the name of the element that has the symbol Mn?
A

Magnesium?

161
Q
  1. What is the name of the element that has the symbol At?
A
162
Q
  1. What is the name of the element that has the symbol Ra?
A
163
Q
  1. What is the name of the element that has the symbol Hg?
A
164
Q
  1. What is the name of the element that has the symbol Sn?
A
165
Q
  1. What is the name of the element that has the symbol Pa?
A
166
Q
  1. A period goes in which direction on the periodic table?
A

Rows left to right

167
Q
  1. Where are the metalloids located in the periodic table?
A
168
Q
  1. Where on the periodic table are the alkaline earth metals located?
A
169
Q
  1. Where on the periodic table are the transition metals located?
A
170
Q
  1. Where on the periodic table are the noble gases located?
A
171
Q
  1. Where on the periodic table are the inner transition metals located?
A
172
Q
  1. Where on the periodic table are the alkali metals located?
A
173
Q
  1. Which chemist is most often recognized for basing the arrangement of the periodic table on atomic mass and other physical properties of the elements?
A
174
Q
  1. Which scientist placed the elements in order of increasing atomic number on the periodic table?
A
175
Q
  1. Where on the periodic table are most of the elements that exist as gases at room temperature?
A
176
Q
  1. To which family does the element potassium belong?
A
177
Q
  1. To which family does the element silver belong?
A
178
Q
  1. To which family does the element selenium belong?
A
179
Q
  1. To which family does the element tin belong?
A
180
Q
  1. To which family does the element iodine belong?
A
181
Q
  1. To which family does the element calcium belong?
A
182
Q
  1. To which family does the element aluminum belong?
A
183
Q
  1. To which family does the heaviest naturally occurring element belong?
A
184
Q
  1. Which family of elements contains the only metal that’s liquid at room temperature?
A
185
Q
  1. Which family of elements contains the only nonmetal that’s liquid at room temperature?
A
186
Q
  1. Members of which family have three valence electrons?
A
187
Q
  1. Members of which family have five valence electrons?
A
188
Q
  1. Members of which family have two valence electrons?
A
189
Q
  1. The atomic masses of the elements generally __________ (increase/decrease/remain the same) going from left to right in a period and __________ (increase/decrease/remain the same) going down a family.
A

Increase , increase ?

190
Q
  1. What term describes the amount of energy needed to remove an electron from a gaseous atom?
A
191
Q
  1. What term describes the energy change that results from adding an electron to a gaseous atom or ion?
A
192
Q
  1. The ionic radius of an anion is __________ (larger than/smaller than/the same size as) the atomic radius of the neutral atom because the ion has __________ (more/fewer/an equal number of) electrons compared to the atom.
A
193
Q
  1. The atomic radii of the elements __________ (increase/decrease/remain the same) going from left to right in a period because the effective nuclear charge __________ (increases/decreases).
A
194
Q
  1. Rank the following elements from smallest to largest atomic radius: Ba, Be, Ca.
A
195
Q
  1. Rank the following elements from smallest to largest atomic radius: Cl, P, S.
A
196
Q
  1. Rank the following elements from lowest to highest ionization energy: B, C, Li.
A
197
Q
  1. Rank the following elements from lowest to highest ionization energy: Br, Cl, I.
A
198
Q
  1. Rank the following elements from lowest to highest electron affinity: F, O, N.
A
199
Q
  1. Rank the following elements from lowest to highest electron affinity: S, Se, Te.
A
200
Q
  1. Rank the following elements from most to least metallic character: Cl, Si, Sn.
A
201
Q
  1. Rank the following elements from smallest to largest atomic radius: K, Mg, Na.
A
202
Q
  1. Rank the following ions from largest to smallest ionic radius: F–, O2–, S2–.
A
203
Q
  1. Rank the following elements from highest to lowest ionization energy: Cs, F, Li.
A
204
Q
  1. Rank the following elements from lowest to highest ionization energy: Ba, Bi, N.
A
205
Q
  1. What is the name of NaCl?
A

Sodium chloride

206
Q
  1. What is the name of CaO?
A
207
Q
  1. What is the name of AlBr^3?
A
208
Q
  1. What is the name of K^2 S?
A
209
Q
  1. What is the name of Al^2 O^3?
A
210
Q
  1. What is the name of Li^3 N?
A
211
Q
  1. What is the name of MgI^2?
A
212
Q
  1. What is the name of SrSe?
A
213
Q
  1. What is the name of BaF^2?
A
214
Q
  1. What is the name of NaH?
A
215
Q
  1. What is the name of Zn^3 P^2?
A
216
Q
  1. What is the name of CuBr^2?
A
217
Q
  1. What is the name of AuCl^3?
A
218
Q
  1. What is the name of CoS?
A
219
Q
  1. What is the name of MnF^3?
A
220
Q
  1. What is the name of Hg^2 I^2?
A
221
Q
  1. What is the name of SnO^2?
A
222
Q
  1. What is the name of NaClO?
A
223
Q
  1. What is the name of KOH?
A
224
Q
  1. What is the name of SrSO^3?
A
225
Q
  1. What is the name of CaCO^3?
A
226
Q
  1. What is the name of AlPO^4?
A
227
Q
  1. What is the name of NaClO^3?
A
228
Q
  1. What is the name of GaPO^3?
A
229
Q
  1. What is the name of NH^4Cl?
A
230
Q
  1. What is the name of ZnSO^4?
A
231
Q
  1. What is the name of (NH^4)^2 C^2 O^4?
A
232
Q
  1. What is the name of KMnO^4?
A
233
Q
  1. What is the name of Be(NO^2)^2?
A
234
Q
  1. What is the name of Cu(CN)^2?
A
235
Q
  1. What is the name of AgBrO?
A
236
Q
  1. What is the name of (NH^4)^3 PO^4?
A
237
Q
  1. What is the name of Ni^2 (SO^4)^3?
A
238
Q
  1. What is the name of Pb(C^2 H^3 O^2)^2?
A
239
Q
  1. What is the chemical formula for cesium chloride?
A
240
Q
  1. What is the chemical formula for indium(III) fluoride?
A
241
Q
  1. What is the chemical formula for magnesium oxide?
A
242
Q
  1. What is the chemical formula for barium bromide?
A
243
Q
  1. What is the chemical formula for potassium iodide?
A
244
Q
  1. What is the chemical formula for aluminum chloride?
A
245
Q
  1. What is the chemical formula for chromium(III) fluoride?
A
246
Q
  1. What is the chemical formula for iron(II) sulfide?
A
247
Q
  1. What is the chemical formula for copper(I) nitride?
A
248
Q
  1. What is the chemical formula for lead(II) oxide?
A
249
Q
  1. What is the chemical formula for nickel(I) selenide?
A
250
Q
  1. What is the chemical formula for silver oxide?
A
251
Q
  1. What is the chemical formula for strontium bromide?
A
252
Q
  1. What is the chemical formula for magnesium nitride?
A
253
Q
  1. What is the chemical formula for lithium hydride?
A
254
Q
  1. What is the chemical formula for zinc chloride?
A
255
Q
  1. What is the chemical formula for chromium(II) sulfide?
A
256
Q
  1. What is the chemical formula for manganese(II) selenide?
A
257
Q
  1. What is the chemical formula for tin(IV) fluoride?
A
258
Q
  1. What is the chemical formula for copper(I) iodide?
A
259
Q
  1. What is the chemical formula for nickel(III) phosphide?
A
260
Q
  1. What is the chemical formula for aluminum selenide?
A
261
Q
  1. What is the chemical formula for tin(IV) oxide?
A
262
Q
  1. What is the chemical formula for calcium phosphide?
A
263
Q
  1. What is the chemical formula for iron(III) oxide?
A
264
Q
  1. What is the chemical formula for manganese(IV) sulfide?
A
265
Q
  1. What is the chemical formula for rubidium hypochlorite?
A
266
Q
  1. What is the chemical formula for beryllium carbonate?
A
267
Q
  1. What is the chemical formula for aluminum phosphite?
A
268
Q
  1. What is the chemical formula for sodium hydrogen carbonate?
A
269
Q
  1. What is the chemical formula for sodium hydroxide?
A
270
Q
  1. What is the chemical formula for potassium hydrogen sulfate?
A
271
Q
  1. What is the chemical formula for lithium perchlorate?
A
272
Q
  1. What is the chemical formula for barium oxalate?
A
273
Q
  1. What is the chemical formula for chromium(III) arsenate?
A
274
Q
  1. What is the chemical formula for silver nitrate?
A
275
Q
  1. What is the chemical formula for lead(II) sulfite?
A
276
Q
  1. What is the chemical formula for thallium(I) bromite?
A
277
Q
  1. What is the chemical formula for gold(III) phosphate?
A
278
Q
  1. What is the chemical formula for iron(II) sulfate?
A
279
Q
  1. What is the chemical formula for calcium thiosulfate?
A
280
Q
  1. What is the chemical formula for sodium peroxide?
A
281
Q
  1. What is the chemical formula for ammonium nitrite?
A
282
Q
  1. What is the chemical formula for beryllium chlorite?
A
283
Q
  1. What is the chemical formula for sodium cyanide?
A
284
Q
  1. What is the chemical formula for magnesium permanganate?
A
285
Q
  1. What is the chemical formula for ammonium dichromate?
A
286
Q
  1. What is the chemical formula for cobalt(III) periodate?
A
287
Q
  1. What is the chemical formula for lead(IV) oxalate?
A
288
Q
  1. What is the chemical formula for calcium hydrogen phosphate?
A
289
Q
  1. What is the chemical formula for iron(III) acetate?
A
290
Q
  1. What is the chemical formula for potassium thiocyanate?
A
291
Q
  1. What is the chemical formula for copper(II) hydrogen sulfite?
A
292
Q
  1. What is the chemical formula for mercury(II) peroxide?
A
293
Q
  1. What is the chemical formula for gold(I) cyanate?
A
294
Q
  1. What is the chemical formula for aluminum dihydrogen phosphate?
A
295
Q
  1. How many atoms does the prefix di- represent?
  2. How many atoms does the prefix hexa- represent?
  3. How many atoms does the prefix hepta- represent?
  4. How many atoms does the prefix tetra- represent?
  5. How many atoms does the prefix nona- represent?
  6. How many atoms does the prefix tri- represent?
  7. How many atoms does the prefix mono- represent?
  8. How many atoms does the prefix penta- represent?
  9. How many atoms does the prefix octa- represent?
  10. How many atoms does the prefix deca- represent?
A
296
Q
  1. What is the name of CO?
A
297
Q
  1. What is the name of SBr^2?
A
298
Q
  1. What is the name of ICl?
A
299
Q
  1. What is the name of SO^2?
A
300
Q
  1. What is the name of PCl^5?
A
301
Q
  1. What is the name of XeF^2?
A
302
Q
  1. What is the name of SF^6
A
303
Q
  1. What is the name of CBr^4?
A
304
Q
  1. What is the name of BCl^3?
A
305
Q
  1. What is the name of SiO^2?
A
306
Q
  1. What is the name of AsCl^5?
A
307
Q
  1. What is the name of SbCl^3?
A
308
Q
  1. What is the name of SiI^4?
A
309
Q
  1. What is the name of NF^3?
A
310
Q
  1. What is the name of CS^2?
A
311
Q
  1. What is the name of ClO^2?
A
312
Q
  1. What is the name of XeO^4?
A
313
Q
  1. What is the name of H^2 O?
A

Water

314
Q
  1. What is the name of SeF^6?
A
315
Q
  1. What is the name of S^2 Cl^2?
A
316
Q
  1. What is the name of N^2 O^3?
A
317
Q
  1. What is the name of P^4 O^6?
A
318
Q
  1. What is the name of B^2 Cl^4?
A
319
Q
  1. What is the name of BrF^3?
A
320
Q
  1. What is the name of S^2 F^10?
A
321
Q
  1. What is the chemical formula of silicon tetrabromide?
A
322
Q
  1. What is the chemical formula of nitrogen triiodide?
A
323
Q
  1. What is the chemical formula of carbon dioxide?
A
324
Q
  1. What is the chemical formula of arsenic pentafluoride?
A
325
Q
  1. What is the chemical formula of nitrogen monoxide?
A
326
Q
  1. What is the chemical formula of sulfur trioxide?
A
327
Q
  1. What is the chemical formula of chlorine monofluoride?
A
328
Q
  1. What is the chemical formula of xenon tetrafluoride?
A
329
Q
  1. What is the chemical formula of nitrogen dioxide?
A
330
Q
  1. What is the chemical formula of carbon tetrachloride?
A
331
Q
  1. What is the chemical formula of iodine heptafluoride?
A
332
Q
  1. What is the chemical formula of phosphorus tribromide?
A
333
Q
  1. What is the chemical formula of selenium tetrafluoride?
A
334
Q
  1. What is the chemical formula of chlorine dioxide?
A
335
Q
  1. What is the chemical formula of boron trifluoride?
A
336
Q
  1. What is the chemical formula of dinitrogen pentoxide?
A
337
Q
  1. What is the chemical formula of diphosphorus trioxide?
A
338
Q
  1. What is the chemical formula of dinitrogen dichloride?
A
339
Q
  1. What is the chemical formula of tetraphosphorus decoxide?
A
340
Q
  1. What is the chemical formula of arsenic trifluoride?
A
341
Q
  1. What is the chemical formula of dinitrogen oxide?
A
342
Q
  1. What is the chemical formula of tetraphosphorus trioxide?
A
343
Q
  1. What is the chemical formula of xenon trioxide?
A
344
Q
  1. What is the chemical formula of antimony pentachloride?
A
345
Q
  1. What is the chemical formula of dichlorine heptoxide?
A
346
Q
  1. How many electrons are in the Lewis dot diagram of a boron atom?
A
347
Q
  1. How many electrons are in the Lewis dot diagram of a barium atom?
A
348
Q
  1. How many electrons are in the Lewis dot diagram of a chlorine atom?
A
349
Q
  1. How many electrons are in the Lewis dot diagram of an O2– ion?
A
350
Q
  1. How many electrons are in the Lewis dot diagram of a sodium ion?
A
351
Q
  1. What is the name for a measure of an atom’s strength to attract a bonding pair ofelectrons?
A
352
Q
  1. What kind of bond forms between elements with the same or nearly the same electronegativity?
A
353
Q
  1. What kind of bond forms between elements when the electronegativity difference is moderate?
A
354
Q
  1. For the representative elements, metals areexpected to have a __________ (lower/higher) electronegativity, and nonmetals areexpected to have a __________ (lower/higher) electronegativity.
A
355
Q
  1. Based on their relative electronegativity values, what type of bond will form betweencarbon and bromine?
A
356
Q
  1. Based on their relative electronegativity values, what type of bond will form betweencarbon and fluorine?
A
357
Q
  1. Based on their relative electronegativity values, what type of bond will form betweenchlorine and fluorine?
A
358
Q
  1. Based on their relative electronegativity values, what type of bond will form betweenboron and hydrogen?
A
359
Q
  1. Based on their relative electronegativity values, what type of bond will form betweencarbon and hydrogen?
A
360
Q
  1. Based on their relative electronegativity values, what type of bond will form betweenphosphorus and fluorine?
A
361
Q
  1. Arrange the following bonds in order of increasing polarity. Si–Cl, S–Cl, O–S
A
362
Q
  1. What molecular shape has bond angles that are approximately 180°?
A
363
Q
  1. What type of reaction is the following reaction?
    2NaCl —> 2Na +Cl^2
A
364
Q
  1. What type of reaction is the following reaction?
    2Na + 2HCl —> H^2 + 2NaCl
A
365
Q
  1. What type of reaction is the following reaction? Ca + S —> CaS
A
366
Q
  1. What type of reaction is the following reaction? 2(C^2 H^2) +5O^2 —> 4CO^2 + 2(H^2 O)
A
367
Q
  1. What type of reaction is the following reaction? KOH + HNO^3 —> KNO^3 + H^2 O
A
368
Q
  1. What type of reaction is the following reaction? 2H^2 +O^2 —> 2(H^2 O)
A
369
Q
  1. What type of reaction is the following reaction? CH^4 + 2O^2 —> CO^2 +2(H^2 O)
A
370
Q
  1. What type of reaction is the following reaction? N^2 +3H^2 —> 2(NH^3)
A
371
Q
  1. What type of reaction is the following reaction? 2(H^2 O^2) —> 2 (H^2 0) + O^2
A
372
Q
  1. What type of reaction is the following reaction? K + AgCl —> KCl +Ag
A
373
Q
  1. What type of reaction is the following reaction?
    Aluminum + oxygen —> aluminum oxide
A
374
Q
  1. What type of reaction is the following reaction?
    Sodium hydroxide + lead (ll) nitrate —> sodium nitrate + lead (ll) hydroxide
A
375
Q
  1. What type of reaction is the following reaction?
    Magnesium + hydrogen chloride —> magnesium chloride + hydrogen gas
A
376
Q
  1. What type of reaction is the following reaction?
    Mercury (ll) oxide—> mercury + oxygen gas
A
377
Q
  1. What type of reaction is the following reaction?
    butane + oxygen —> carbon dioxide gas + water vapor
A
378
Q

561.What type of reaction is the following reaction?
iron + copper(ll) chloride—> iron(ll) chloride + copper

A
379
Q
  1. What type of reaction is the following reaction?
    sodium bicarbonate —> sodium oxide + water vapor + carbon dioxide gas
A
380
Q
  1. What type of reaction is the following reaction?
    ethanol + oxygen gas—> carbon dioxide gas + water vapor
A
381
Q
  1. What type of reaction is the following reaction?
    calcium oxide + water —> calcium hydroxide
A
382
Q
  1. What type of reaction is the following reaction?
    carbon monoxide + oxygen gas —> carbon dioxide gas
A
383
Q
  1. Predict the type of reaction these reactants would undergo; Zn + H^2 SO^4—>
A
384
Q
  1. Predict the type of reaction these reactants would undergo when heated; N^2 O—>
A
385
Q

568.Predict the type of reaction these reactants would undergo; Ca(OH)^2 + H^2 SO^4—>

A
386
Q
  1. Predict the type of reaction these reactants would undergo; Li+O^2—>
A
387
Q
  1. Predict the type of reaction these reactants would undergo;
    C^3 H^8 +O^2—>
A
388
Q
  1. Predict the type of reaction these reactants would undergo;
    silver nitrate + sodium chloride—>
A
389
Q
  1. Predict the type of reaction these reactants would undergo: sodium + hydrogen gas —>
A
390
Q
  1. Predict the type of reaction these reactants would undergo; potassium bromide + chlorine gas—>
A
391
Q
  1. Predict the type of reaction these reactants would undergo when heated; copper(ll) hydroxide—>
A
392
Q
  1. Predict the type of reaction these reactants would undergo; aluminum sulfate +calcium phosphate—>
A
393
Q
  1. What are the coefficient of the following equation when its balanced? () N^2 O^4 —> () N0^2
A
394
Q
  1. What are the coefficient of the following equation when its balanced? () CS^2 +() Cl^2—> () CCl^4+ () S^2 Cl^2
A
395
Q
A

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