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Honors Chemistry > Module 5 Test > Flashcards

Module 5 Test Flashcards

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1
Q

Chemical bonds form by the attraction between ______?

A

the nucleus of one atom and the electrons of another atom

positive ions and negative ions

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2
Q

Noble gases are unreactive because they have ______?

A

filled outer energy levels

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3
Q

Elements tend to react to acquire ______?

A

the stable electron structure of a noble gas

a filled outer energy level

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4
Q

A positive ion forms when an atom ______?

A

loses one or more valence electrons in order to attain a noble gas configuration

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5
Q

In terms of electron configuration, a neutral sodium atom differs from the noble gas neon by ____ valence electron(s).

A

One

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6
Q

What is a positively charged ion called?

A

cation

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7
Q

Noble gases are unreactive because, except for helium, they have a stable arrangement of ____valence electrons in the outer energy level. This arrangement is called a(n) _______.

A

Eight, octet

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8
Q

Elements tend to react to acquire the stable electron structure of a(n) ______

A

Noble gas

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9
Q

A positive ion forms when an atom loses one or more ______ electrons in order to attain a _____ configuration.

A

Valence, noble, gas

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10
Q

What statements about the electron configurations of a neon atom, a sodium atom, and a sodium ion are true?

A

The electron configuration of the sodium ion is 1s22s22p6.

The electron configuration of sodium is 1s22s22p63s1.

Neon and the sodium ion have the same electron configuration.

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11
Q

What statements about transition metals and their ions are true?

A

Many transition metals form ions with a 2+ or a 3+ charge.

In general, transition metals have an outer energy level of ns2.

Transition metals commonly lose their two valence electrons, forming 2+ ions.

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12
Q

Elements in groups 11 through 14 lose electrons to form an outer energy level containing full s, p, and d sublevels. What are these relatively stable electron arrangements called?

A

pseudo-noble gas configurations and isoelectronic

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13
Q

True or false: Nonmetals easily lose one or more electrons to attain a stable outer electron configuration.

A

False

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14
Q

Why is this false: Nonmetals easily lose one or more electrons to attain a stable outer electron configuration.

A

Nonmetals have nearly full outer energy levels and gain electrons to attain noble-gas configurations.

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15
Q

Transition metal ions may lose their two valence electrons, forming ions with charges of 2+. But they may also lose electrons from an inner ______ sublevel, forming ions of 3+ or greater.

A

d

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16
Q

Why might transition metal ions also lose electrons from an inner d sublevel?

A

The transition metals have not begun filling their outer p sublevel yet. The electrons from p orbitals of inner principal energy levels will not be lost.

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17
Q

What statements about the electron configurations of an argon atom, a chlorine atom, and a chloride ion are true?

A

The electron configuration of chlorine is 1s22s22p63s23p5.

Argon and the chloride ion have the same electron configuration.

Argon and the chloride ion have filled outer energy levels.

The electron configuration of argon is 1s22s22p63s23p6.

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18
Q

To attain a stable outer electron configuration, nonmetals _____ one or more electrons.

A

Gain

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19
Q

To designate an anion formed when an atom gains one or more electrons, the ending ____ is added to the root name of the element.

A

Ide

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20
Q

The force that holds two atoms together, both in the attraction between ions and in the attraction between the nucleus of one atom and the electrons of another, is called a(n) ____ _____?

A

Chemical bond

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21
Q

Chemical bonds form by the attraction between ______.

A

the nucleus of one atom and the electrons of another atom

positive ions and negative ions

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22
Q

Noble gases are unreactive because they have ______.

A

filled outer energy levels

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23
Q

Elements tend to react to acquire the stable electron structure of a(n) ______ ______.

A

Noble gas

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24
Q

A positive ion forms when an atom loses one or more _____ electrons in order to attain a _____ _____ configuration.

A

Valence, noble, gas

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25
Q

A positive ion forms when an atom ______.

A

loses one or more valence electrons in order to attain a noble gas configuration

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26
Q

True or false: Nonmetals easily lose one or more electrons to attain a stable outer electron configuration.

True false question.

A

False

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27
Q

Transition metal ions may lose their two valence electrons, forming ions with charges of 2+. But they may also lose electrons from an inner ______ sublevel, forming ions of 3+ or greater.

A

D

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28
Q

Elements in groups 11 through 14 lose electrons to form an outer energy level containing full s, p, and d sublevels. What are these relatively stable electron arrangements called?

A

pseudo-noble gas configurations

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29
Q

To attain a stable outer electron configuration, nonmetals _____one or more electrons.

A

Gain

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30
Q

What is the term for the electrostatic force that holds oppositely charged particles together in an ionic compound?

A

ionic bond

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31
Q

What are compounds that contain ionic bonds called?

A

ionic compounds

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32
Q

The two main types of ionic compounds are ______.

A

oxides and salts

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33
Q

Binary ionic compounds ______.

A

contain a metallic cation and a nonmetallic anion

contain only two different elements

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34
Q

Which statements about the formation of ionic bonds in sodium chloride are true?

A

The oppositely charged ions attract each other in an ionic bond.

A sodium atom transfers its valence electron to a chlorine atom.

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35
Q

If ionic bonds occur between metals and the nonmetal oxygen, _____form. Most other ionic compounds are called _______.

A

Oxides, salts

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36
Q

Binary ionic compounds contain only two different ______. They contain a metallic _____ and a nonmetallic ______.

A

Elements, cation, anion

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37
Q

Which are mainly responsible for determining the physical properties of ionic compounds?

A

their ionic bonds

their unique physical structures

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38
Q

In an ionic compound, positive and negative ions are packed into a regular repeating pattern that balances the forces of _____ and ________ between the ions.

A

Attraction, repulsion

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39
Q

The physical properties of ionic compounds are determined by the nature of the bonds between ions and the unique physical ______ that form as a result.

A

Structures

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40
Q

A three-dimensional geometric arrangement of particles in which each positive ion is surrounded by negative ions and each negative ion is surrounded by positive ions is called a(n) ______ ______.

A

Crystal lattice

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41
Q

Which of these descriptions match the physical structure of an ionic compound?

A

The pattern of ions results in a balance between the forces of attraction and repulsion.

Ions form a regular repeating pattern.

Ions exist in a ratio that results in an overall charge of zero for the compound.

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42
Q

In a crystal of sodium chloride, NaCl, each sodium ion is surrounded by_______ negative chloride ions, and each chloride ion is surrounded by _______ positive sodium ions.

A

Six, six

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43
Q

Minerals that contain fluoride, chloride, bromide, or iodide ions are called ____ . Minerals containing anions made up of silicon and oxygen are called ______.

A

Halides, silicates

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44
Q

Which physical properties are typical of ionic compounds?

A

have high melting and boiling points

conduct electricity when dissolved

hard and brittle

do not conduct electricity as solids

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45
Q

What do silicates contain?

A

contain an anion that is a combination of silicon and oxygen

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46
Q

What do halides contain?

A

contain fluoride, chloride, bromide, or iodide ions

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47
Q

What do borates contain?

A

have anions that contain boron and oxygen

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48
Q

What do carbonates contain?

A

have anions that contain carbon and oxygen

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49
Q

Ionic crystals have high melting points and high boiling points because ______.

A

ionic bonds are relatively strong

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50
Q

Because ionic bonds are relatively strong, ionic compounds tend to be ______.

A

hard and rigid

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51
Q

Which of the following best describes a reason that ionic compounds tend to be brittle?

A

A force strong enough to push ions out of alignment results in like-charged ions being next to each other.

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52
Q

The electrostatic force that holds oppositely charged particles together in an ionic compound

A

Ionic bond

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53
Q

The attraction of a metallic cation for delocalized electrons

A

metallic bond

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54
Q

What is an electrolyte?

A

An electrolyte is an ionic compound whose aqueous solution conducts an electric current.

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55
Q

What is a three-dimensional geometric arrangement of particles in which each positive ion is surrounded by negative ions and each negative ion is surrounded by positive ions; vary in shape due to sizes and relative numbers of the ions bonded?

A

Crystal lattice

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56
Q

What is the energy required to separate one mole of the ions of an ionic compound, which is directly related to the size of the ions bonded and is also affected by the charge of the ions?

A

Lattice energy

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57
Q

What is the simplest ratio of ions represented in an ionic compound?

A

Formula unit

58
Q

What is a monatomic ion?

A

Is an ion made up of a single atom with a positive or negative charge

59
Q

What is a polyatomic ion?

A

A group of atoms bonded together that acts as a single unit with a net charge.

60
Q

What is an oxyanion?

A

An oxyanion is a polyatomic ion composed of an element bonded to one or more oxygen atoms.

61
Q

What is the name of the model that proposes that all metal atoms in a metallic solid contribute their valence electrons to flow between the metal cations, and can explain properties of metallic solids such as malleability, conduction, and ductility?

A

The name of this model is the electron sea model.

62
Q

In a metallic bond, the electrons are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom, and are said to be ____.

A

Delocalized

63
Q

What is an alloy?

A

An alloy is a mixture of elements that has metallic properties.

64
Q

A compound formed by electrostatic forces between positively and negatively charged particles is known as a(n) ______ compound.

A

Ionic

65
Q

Ionic bonds require a _____ amount of energy to be broken apart because ionic bonds are relatively _____. Thus, ionic crystals have _____ melting and boiling points.

A

high, strong, high

66
Q

Which physical properties are typical of ionic compounds?

A

conduct electricity when dissolved

have high melting and boiling points

hard and brittle

do not conduct electricity as solids

67
Q

Ionic crystals are hard and rigid because the ionic bonds holding the ions in position are relatively _____.

A

Strong

68
Q

Which statements about the conductivity of ionic compounds are true?

A

For an ionic compound to conduct an electric current, its ions must be able to move.

Ionic compounds in liquid solutions conduct electric current.

Ionic compounds in the solid state do not conduct an electric current.

69
Q

Ionic crystals have high melting points and high boiling points because ______.

A

ionic bonds are relatively strong

70
Q

Typical ionic compounds have _____ melting and boiling points.

A

High

71
Q

What is an ionic compound whose aqueous solution conducts an electric current?

A

electrolyte

72
Q

When an ionic compound is in the _______ state or is dissolved in a ________, it conducts electricity because the ions are free to move around. Ionic compounds in the ________ state do not conduct electricity because the ions are locked in position.

A

Liquid, solution, solid

73
Q

Which are mainly responsible for determining the physical properties of ionic compounds?

A

their unique physical structures

their ionic bonds

74
Q

Every chemical process is either exothermic or endothermic. The formation of ionic compounds from positive ions and negative ions is always _______.

A

exothermic

75
Q

Which of the following best describes a reason that ionic compounds tend to be brittle?

A

A force strong enough to push ions out of alignment results in like-charged ions being next to each other.

76
Q

The energy required to separate 1 mol of the ions of an ionic compound is referred to as the ______ ______.

A

Lattice energy

77
Q

In terms of energy change, the formation of ionic compounds from positive ions and negative ions ______.

A

is always exothermic

78
Q

True or false: Smaller ions produce weaker interionic attractions and smaller lattice energies.

A

False

79
Q

Ions with larger positive or negative charges generally result in a ______ lattice energy.

A

Higher

80
Q

Which statements about formula units and the composition of ionic compounds are true?

A

The overall charge of a formula unit is zero.

The formula unit represents the simplest ratio of the ions in an ionic compound.

The chemical formula for an ionic compound represents a formula unit.

81
Q

What is the term for the chemical formula for an ionic compound, which represents the simplest ratio of the ions involved?

A

a formula unit

82
Q

What term identifies a one-atom ion, such as Mg2+ or Br–?

A

monatomic ion

83
Q

Which statement about how ion size affects lattice energy is true?

A

Smaller ions produce greater lattice energies.

84
Q

Why is “Smaller ions produce greater lattice energies” true?

A

Reason: The electrostatic force of attraction increases as opposite charges get closer together, so smaller ions, which can get closer together than larger ions, produce greater lattice energies.

85
Q

Which statement about how ion charge affects lattice energy is true?

A

Larger charges generally result in a greater lattice energy.

86
Q

A formula unit represents the simplest _____ of the ions that make up an ionic compound.

A

Ratio

87
Q

Why is “Smaller ions produce weaker interionic attractions and smaller lattice energies” false?

A

Reason: The electrostatic force of attraction between opposite charges increases as the distance between charges decreases. Therefore, smaller ions produce stronger attractions and greater lattice energies.

88
Q

For an element in an ionic compound, the number of electrons transferred from the atom to form the ion is the ______ number.

A

Oxidation

89
Q

Ions with larger positive or negative charges generally result in a _______ lattice energy.

A

Larger

90
Q

When writing formulas for binary ionic compounds, the symbol for the _____ is always written first. The number of ions of each element in a formula unit is represented by ________.

A

Cation, subscripts

91
Q

Most transition metals and group 13 and 14 metals have ______.

A

more than one possible ionic charge

92
Q

Which statements describe how to write formulas for binary ionic compounds?

A

The sum of the oxidation number of each ion multiplied by the number of ions in a formula unit must equal zero.

If no subscript is written, it is assumed to be one.

Subscripts represent the number of ions of each element in a formula unit of the compound.

93
Q

A polyatomic ion composed of an element, usually a nonmetal, bonded to one or more oxygen atoms is called a(n) ______.

A

Oxyanion

94
Q

The naming system for ionic compounds must account for both ______.

A

anions and cations

95
Q

What are polyatomic ions that are composed of an element, usually a nonmetal, bonded to one or more oxygen atoms?

A

oxyanions

96
Q

hen naming chlorine oxyanions, the oxyanion with the greatest number of oxygen atoms is named using the prefix ______ , the root of the nonmetal, and the suffix _______.

A

Per, ate

97
Q

The bonding in both metals and ionic compounds is based on the attraction of particles with _____ charges.

A

Opposite

98
Q

The electrons in the outer energy levels of the bonding metallic atoms that are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom are called ____ _____.

A

Delocalized electrons

99
Q

Which properties do metals and ionic compounds share?

A

They form lattice structures in the solid state.

They involve bonding that is based on the attraction of unlike charges.

100
Q

Which is the model that proposes that all the metal atoms in a metallic solid contribute their valence electrons to form a “sea” of electrons that surrounds the metal cations in the lattice?

A

the electron sea model

101
Q

The attraction of a metallic cation for delocalized electrons is a(n) _____ ______.

A

Metallic bond

102
Q

What is the name for the electrons involved in metallic bonding that are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom?

A

delocalized electrons

103
Q

According to the electron sea model, the melting points of metals are not as extreme as the boiling points because ______.

A

cations and anions are mobile in a metal, so they can move past each other relatively easily, even though they are strongly attracted to each other.

104
Q

Metals are good thermal and electrical conductors because their ______ electrons can move around within the solid.

A

Delocalized

105
Q

What is the attraction of a metallic cation for delocalized electrons called?

A

metallic bond

106
Q

According to the electron sea model, the melting points of metals are not as extreme as the boiling points. This is because the cations and electrons are _____ in a metal. It does not take much energy for a solid to become liquid. But metallic bonds are very _____ , so it does require a lot of energy to separate atoms from the cations in their sea of electrons.

A

Mobile, strong

107
Q

Transition metals tend to be harder and stronger than alkali metals because atoms of transition metals ______.

A

have a greater number of delocalized electrons

108
Q

Metals conduct heat and electrical current well due to the ______ of delocalized electrons.

A

movement from place to place

109
Q

What is a mixture of elements that has metallic properties called?

A

An alloy

110
Q

Compared with the properties of the primary element or elements they contain, the properties of alloys are ______,

A

somewhat different

111
Q

Metals are malleable and ductile because ______.

A

the mobile particles involved in metallic bonding can be pushed or pulled past each other

112
Q

The two basic types of alloys are _____ alloys and ______ alloys.

A

substitutional, interstitial

113
Q

An alloy in which some of the atoms in the original metallic solid are replaced by other metals of similar atomic size is called a(n) _______ alloy.

A

substitutional

114
Q

The alloy that is formed when the small holes in a metallic crystal are filled with smaller atoms is called a(n) ______ alloy.

A

interstitial

115
Q

According to the electron sea model, the melting points of metals are not as extreme as the boiling points because ______.

A

cations and anions are mobile in a metal, so they can move past each other relatively easily, even though they are strongly attracted to each other.

116
Q

What is an ion in which it has gained a - electron?

A

Anion

117
Q

A cation has what type of charge?

A

Positive charge

118
Q

In binary compounds, the anion ends in what?

A

-ide

119
Q

Binary acids start with what?

A

Hydro

120
Q

Which is not a property of ionic compounds?

A

Low melting points

121
Q

Which factors affect lattice energy?

A

Charge and radius/size

122
Q

The Octet rule states?

A

2nd row elements can have a maximum of 8 electrons

123
Q

What is a hydrate?

A

A compound that has water chemically attached to its ions

124
Q

What is an ion?

A

An atom with extra or less electrons than normal

125
Q

What is an ionic bond?

A

The force of attraction between the opposite charges

126
Q

What does isoelectronic mean?

A

Having the same number of electrons

127
Q

What is a chemical bond?

A

The force that holds two atoms together

128
Q

What is a cation?

A

A cation is a positive ion

129
Q

How does a cation form?

A

A positive ion forms when an atom loses one or more valence electrons in order to attain a noble gas configuration.

130
Q

Why do the ions of transition metals vary?

A

The ions of transition metals vary because of how atoms fill in an inner d sublevel. When forming positive ions, they commonly lose their two valence electrons which forms 2+ ions. Though, d electrons can be lost which could cause transition metals to also form ions of 3+ or greater.

131
Q

What is an anion?

A

An anion is a negative ion

132
Q

How does a anion form?

A

It forms when an atom gains an electron. There are now more electrons. Therefore, the ion will have a charge equal to the number of electrons gained.

133
Q

What is an ionic bond?

A

An ionic bond is the electrostatic force that holds oppositely charged particles together in an ionic compound.

134
Q

What are ionic compounds made of?

A

Ionic compounds are made of ionic bonds

135
Q

What are binary ionic compounds?

A

They are ionic compounds that contain only two different elements

136
Q

Consider the binary compound NaCl. What happens to the valence electrons of sodium and chlorine when they form this bond?

A

In the binary ionic compound NaCl, Na (sodium) transfers one electron to Cl (chlorine) to form a complete Cl outer shell of 8 electrons.

137
Q

What type of structure forms when ionic bonds are made?

A

A crystal lattice is formed when ionic bonds are made because of the strong attractions among the positive ions and the negative ions in an ionic compound.

138
Q

What is a crystal lattice?

A

A crystal lattice is a three-dimensional geometric arrangement of particles where each positive ion is surrounded by negative ions, and each negative ion is surrounded by positive ions.

139
Q

What is an electrolyte?

A

An electrolyte is an ionic compound whose aqueous solution conducts an electric current.

140
Q

What is an oxidation number?

A

The oxidation number of a monatomic ion, or its oxidation state, is equal to the net charge of the ion. The oxidation number of an element in an ionic compound equals the number of electrons transferred from the atom to form the ion.

141
Q

What is a polyatomic ion?

A

A polyatomic ion is a charged group of two or more covalently bonded atoms that acts as a single unit in an ionic compound.

142
Q

Where could you find a list of the polyatomic ions?

A

You could find a list of the polyatomic ions on polyatomic tables like Table 9 on page 183, or on the front page on Google Classroom.

Honors Chemistry (13 decks)

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