Module 5 Test Flashcards
(142 cards)
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
2
Q
Noble gases are unreactive because they have ______?
A
filled outer energy levels
3
Q
Elements tend to react to acquire ______?
A
the stable electron structure of a noble gas
a filled outer energy level
4
Q
A positive ion forms when an atom ______?
A
loses one or more valence electrons in order to attain a noble gas configuration
5
Q
In terms of electron configuration, a neutral sodium atom differs from the noble gas neon by ____ valence electron(s).
A
One
6
Q
What is a positively charged ion called?
A
cation
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
8
Q
Elements tend to react to acquire the stable electron structure of a(n) ______
A
Noble gas
9
Q
A positive ion forms when an atom loses one or more ______ electrons in order to attain a _____ configuration.
A
Valence, noble, gas
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.
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.
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
13
Q
True or false: Nonmetals easily lose one or more electrons to attain a stable outer electron configuration.
A
False
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.
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
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.
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.
18
Q
To attain a stable outer electron configuration, nonmetals _____ one or more electrons.
A
Gain
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
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
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
22
Q
Noble gases are unreactive because they have ______.
A
filled outer energy levels
23
Q
Elements tend to react to acquire the stable electron structure of a(n) ______ ______.
A
Noble gas
24
Q
A positive ion forms when an atom loses one or more _____ electrons in order to attain a _____ _____ configuration.
A
Valence, noble, gas
25
A positive ion forms when an atom ______.
loses one or more valence electrons in order to attain a noble gas configuration
26
True or false: Nonmetals easily lose one or more electrons to attain a stable outer electron configuration.
True false question.
False
27
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.
D
28
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?
pseudo-noble gas configurations
29
To attain a stable outer electron configuration, nonmetals _____one or more electrons.
Gain
30
What is the term for the electrostatic force that holds oppositely charged particles together in an ionic compound?
ionic bond
31
What are compounds that contain ionic bonds called?
ionic compounds
32
The two main types of ionic compounds are ______.
oxides and salts
33
Binary ionic compounds ______.
contain a metallic cation and a nonmetallic anion
contain only two different elements
34
Which statements about the formation of ionic bonds in sodium chloride are true?
The oppositely charged ions attract each other in an ionic bond.
A sodium atom transfers its valence electron to a chlorine atom.
35
If ionic bonds occur between metals and the nonmetal oxygen, _____form. Most other ionic compounds are called _______.
Oxides, salts
36
Binary ionic compounds contain only two different ______. They contain a metallic _____ and a nonmetallic ______.
Elements, cation, anion
37
Which are mainly responsible for determining the physical properties of ionic compounds?
their ionic bonds
their unique physical structures
38
In an ionic compound, positive and negative ions are packed into a regular repeating pattern that balances the forces of _____ and ________ between the ions.
Attraction, repulsion
39
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.
Structures
40
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) ______ ______.
Crystal lattice
41
Which of these descriptions match the physical structure of an ionic compound?
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.
42
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.
Six, six
43
Minerals that contain fluoride, chloride, bromide, or iodide ions are called ____ . Minerals containing anions made up of silicon and oxygen are called ______.
Halides, silicates
44
Which physical properties are typical of ionic compounds?
have high melting and boiling points
conduct electricity when dissolved
hard and brittle
do not conduct electricity as solids
45
What do silicates contain?
contain an anion that is a combination of silicon and oxygen
46
What do halides contain?
contain fluoride, chloride, bromide, or iodide ions
47
What do borates contain?
have anions that contain boron and oxygen
48
What do carbonates contain?
have anions that contain carbon and oxygen
49
Ionic crystals have high melting points and high boiling points because ______.
ionic bonds are relatively strong
50
Because ionic bonds are relatively strong, ionic compounds tend to be ______.
hard and rigid
51
Which of the following best describes a reason that ionic compounds tend to be brittle?
A force strong enough to push ions out of alignment results in like-charged ions being next to each other.
52
The electrostatic force that holds oppositely charged particles together in an ionic compound
Ionic bond
53
The attraction of a metallic cation for delocalized electrons
metallic bond
54
What is an electrolyte?
An electrolyte is an ionic compound whose aqueous solution conducts an electric current.
55
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?
Crystal lattice
56
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?
Lattice energy
57
What is the simplest ratio of ions represented in an ionic compound?
Formula unit
58
What is a monatomic ion?
Is an ion made up of a single atom with a positive or negative charge
59
What is a polyatomic ion?
A group of atoms bonded together that acts as a single unit with a net charge.
60
What is an oxyanion?
An oxyanion is a polyatomic ion composed of an element bonded to one or more oxygen atoms.
61
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?
The name of this model is the electron sea model.
62
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 ____.
Delocalized
63
What is an alloy?
An alloy is a mixture of elements that has metallic properties.
64
A compound formed by electrostatic forces between positively and negatively charged particles is known as a(n) ______ compound.
Ionic
65
Ionic bonds require a _____ amount of energy to be broken apart because ionic bonds are relatively _____. Thus, ionic crystals have _____ melting and boiling points.
high, strong, high
66
Which physical properties are typical of ionic compounds?
conduct electricity when dissolved
have high melting and boiling points
hard and brittle
do not conduct electricity as solids
67
Ionic crystals are hard and rigid because the ionic bonds holding the ions in position are relatively _____.
Strong
68
Which statements about the conductivity of ionic compounds are true?
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
Ionic crystals have high melting points and high boiling points because ______.
ionic bonds are relatively strong
70
Typical ionic compounds have _____ melting and boiling points.
High
71
What is an ionic compound whose aqueous solution conducts an electric current?
electrolyte
72
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.
Liquid, solution, solid
73
Which are mainly responsible for determining the physical properties of ionic compounds?
their unique physical structures
their ionic bonds
74
Every chemical process is either exothermic or endothermic. The formation of ionic compounds from positive ions and negative ions is always _______.
exothermic
75
Which of the following best describes a reason that ionic compounds tend to be brittle?
A force strong enough to push ions out of alignment results in like-charged ions being next to each other.
76
The energy required to separate 1 mol of the ions of an ionic compound is referred to as the ______ ______.
Lattice energy
77
In terms of energy change, the formation of ionic compounds from positive ions and negative ions ______.
is always exothermic
78
True or false: Smaller ions produce weaker interionic attractions and smaller lattice energies.
False
79
Ions with larger positive or negative charges generally result in a ______ lattice energy.
Higher
80
Which statements about formula units and the composition of ionic compounds are true?
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
What is the term for the chemical formula for an ionic compound, which represents the simplest ratio of the ions involved?
a formula unit
82
What term identifies a one-atom ion, such as Mg2+ or Br–?
monatomic ion
83
Which statement about how ion size affects lattice energy is true?
Smaller ions produce greater lattice energies.
84
Why is "Smaller ions produce greater lattice energies" true?
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
Which statement about how ion charge affects lattice energy is true?
Larger charges generally result in a greater lattice energy.
86
A formula unit represents the simplest _____ of the ions that make up an ionic compound.
Ratio
87
Why is "Smaller ions produce weaker interionic attractions and smaller lattice energies" false?
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
For an element in an ionic compound, the number of electrons transferred from the atom to form the ion is the ______ number.
Oxidation
89
Ions with larger positive or negative charges generally result in a _______ lattice energy.
Larger
90
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 ________.
Cation, subscripts
91
Most transition metals and group 13 and 14 metals have ______.
more than one possible ionic charge
92
Which statements describe how to write formulas for binary ionic compounds?
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
A polyatomic ion composed of an element, usually a nonmetal, bonded to one or more oxygen atoms is called a(n) ______.
Oxyanion
94
The naming system for ionic compounds must account for both ______.
anions and cations
95
What are polyatomic ions that are composed of an element, usually a nonmetal, bonded to one or more oxygen atoms?
oxyanions
96
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 _______.
Per, ate
97
The bonding in both metals and ionic compounds is based on the attraction of particles with _____ charges.
Opposite
98
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 ____ _____.
Delocalized electrons
99
Which properties do metals and ionic compounds share?
They form lattice structures in the solid state.
They involve bonding that is based on the attraction of unlike charges.
100
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?
the electron sea model
101
The attraction of a metallic cation for delocalized electrons is a(n) _____ ______.
Metallic bond
102
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?
delocalized electrons
103
According to the electron sea model, the melting points of metals are not as extreme as the boiling points because ______.
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
Metals are good thermal and electrical conductors because their ______ electrons can move around within the solid.
Delocalized
105
What is the attraction of a metallic cation for delocalized electrons called?
metallic bond
106
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.
Mobile, strong
107
Transition metals tend to be harder and stronger than alkali metals because atoms of transition metals ______.
have a greater number of delocalized electrons
108
Metals conduct heat and electrical current well due to the ______ of delocalized electrons.
movement from place to place
109
What is a mixture of elements that has metallic properties called?
An alloy
110
Compared with the properties of the primary element or elements they contain, the properties of alloys are ______,
somewhat different
111
Metals are malleable and ductile because ______.
the mobile particles involved in metallic bonding can be pushed or pulled past each other
112
The two basic types of alloys are _____ alloys and ______ alloys.
substitutional, interstitial
113
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.
substitutional
114
The alloy that is formed when the small holes in a metallic crystal are filled with smaller atoms is called a(n) ______ alloy.
interstitial
115
According to the electron sea model, the melting points of metals are not as extreme as the boiling points because ______.
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
What is an ion in which it has gained a - electron?
Anion
117
A cation has what type of charge?
Positive charge
118
In binary compounds, the anion ends in what?
-ide
119
Binary acids start with what?
Hydro
120
Which is not a property of ionic compounds?
Low melting points
121
Which factors affect lattice energy?
Charge and radius/size
122
The Octet rule states?
2nd row elements can have a maximum of 8 electrons
123
What is a hydrate?
A compound that has water chemically attached to its ions
124
What is an ion?
An atom with extra or less electrons than normal
125
What is an ionic bond?
The force of attraction between the opposite charges
126
What does isoelectronic mean?
Having the same number of electrons
127
What is a chemical bond?
The force that holds two atoms together
128
What is a cation?
A cation is a positive ion
129
How does a cation form?
A positive ion forms when an atom loses one or more valence electrons in order to attain a noble gas configuration.
130
Why do the ions of transition metals vary?
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
What is an anion?
An anion is a negative ion
132
How does a anion form?
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
What is an ionic bond?
An ionic bond is the electrostatic force that holds oppositely charged particles together in an ionic compound.
134
What are ionic compounds made of?
Ionic compounds are made of ionic bonds
135
What are binary ionic compounds?
They are ionic compounds that contain only two different elements
136
Consider the binary compound NaCl. What happens to the valence electrons of sodium and chlorine when they form this bond?
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
What type of structure forms when ionic bonds are made?
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
What is a crystal lattice?
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
What is an electrolyte?
An electrolyte is an ionic compound whose aqueous solution conducts an electric current.
140
What is an oxidation number?
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
What is a polyatomic ion?
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
Where could you find a list of the polyatomic ions?
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.
