1
Q
What are the two types of pure substances?
A
Elements and compounds
2
Q
What is an element composed of?
A
Only 1 type of atom
3
Q
What is a compound composed of?
A
More than 1 type of atom
4
Q
What defines a pure substance?
A
Any matter that has a fixed, or unchanging composition
5
Q
What is a diatomic molecule?
A
A molecule made up of two atoms of the same element
6
Q
List the seven diatomic molecules.
A
- Hydrogen
- Nitrogen
- Oxygen
- Fluorine
- Chlorine
- Bromine
- Iodine
7
Q
Which diatomic elements are not gases at room temperature?
A
Bromine (liquid) and Iodine (solid)
8
Q
What is the structure of carbon graphite?
A
A complex structure with many C atoms joined together in a fixed repeating pattern of rings
9
Q
What is bonding in chemistry based on?
A
Electrostatic interactions among charged particles
10
Q
What does Coulomb’s law state?
A
Like charges repel and unlike charges attract
11
Q
What are the two extremes of bonding in chemistry?
A
Ionic and covalent bonding
12
Q
What occurs in ionic bonding?
A
Transfer of electrons from one atom to another
13
Q
What results from ionic bonding?
A
Charged particles called ions
14
Q
What occurs in covalent bonding?
A
Sharing of electrons between atoms
15
Q
What type of elements form covalent bonds?
A
Two non-metals
16
Q
What type of ions do metals form?
A
Cations
17
Q
What type of ions do non-metals form?
A
Anions
18
Q
What charge do Group 1 metals and hydrogen form?
A
+1 cations
19
Q
How many valence electrons do metals in Group 2 have and what charge do they form?
A
2 valence electrons; +2 cations
20
Q
What charge do metals in Group 13 form?
A
+3 cations
21
Q
Do transition metals have fixed charges?
A
No, their charges vary depending on the compound
22
Q
What charge do non-metals in Group 17 form?
A
-1 anions
23
Q
What charge do non-metals in Group 16 form?
A
-2 anions
24
Q
What charge do non-metals in Group 15 form?
A
-3 anions
25
What charge does carbon form when bonded to a metal?
-4 anion
26
Which elements do not form ions?
Boron, silicon, and the inert gases
27
What are the two main categories of pure substances?
Elements and compounds
28
What are binary compounds?
Compounds that contain two and only two different types of atoms
29
What are non-binary compounds?
Compounds that contain more than two types of atoms
30
Give an example of a binary compound
Water or hydrogen chloride
31
Give an example of a non-binary compound
Methanol or sulfur
32
What is methanol composed of?
Three different atom types
33
What type of atom does sulfur consist of?
Only one type of atom (element)
34
Binary compounds can be subdivided into which two categories?
Ionic and covalent
35
What do ionic compounds contain?
A metal and a non-metal
36
What are covalent compounds made from?
Two nonmetals
37
Fill in the blank: Compounds that contain more than two types of atoms are called _______.
Non-binary compounds
38
What is the first step in naming covalent compounds?
Write down the name of the first element
39
What should you do with the name of the second element in covalent compound naming?
Change the ending to -ide
40
What is the purpose of using prefixes in naming covalent compounds?
To indicate the number of atoms in the molecule
41
What prefix is used for 1 atom?
mono
42
What prefix is used for 2 atoms?
di
43
What prefix is used for 3 atoms?
tri
44
What prefix is used for 4 atoms?
tetra
45
What prefix is used for 5 atoms?
penta
46
What prefix is used for 6 atoms?
hexa
47
What prefix is used for 7 atoms?
hepta
48
What prefix is used for 8 atoms?
octa
49
What prefix is used for 9 atoms?
nona
50
What prefix is used for 10 atoms?
deca
51
In naming covalent compounds, which element's name is altered to end with -ide?
The second element
52
Fill in the blank: The prefix for 4 atoms is _______.
tetra
53
True or False: The prefix 'mono' is used for 2 atoms.
False
54
What is the last step in the naming process of covalent compounds?
Add the prefix to the name of the second element and change the ending to -ide
55
What is the exception for the prefix when there is only 1 atom of the first element?
Do not use the prefix mono-
## Footnote
Example: CO is carbon monoxide, not monocarbon monoxide.
56
What is the rule for naming when the second element is oxygen?
Drop the -o and -a endings from the prefix
## Footnote
Example: CO2 is carbon dioxide, not carbon dioxygen.
57
What is the charge of transition metal indicated by?
A roman numeral
58
What is the chemical formula for copper oxide?
CuO
59
What is the name of CuO?
copper(II) oxide
60
What is the name of Fe₂O₃?
iron(III) oxide
61
What is the name of CoCl₂?
cobalt(II) chloride
62
What is the name of V₂S₇?
vanadium(VII) sulfide
63
Fill in the blank: The charge of the transition metal is indicated by a _______.
roman numeral
64
True or False: The naming convention for transition metal compounds requires a roman numeral to indicate the charge.
True
65
What is the charge of copper in copper(I) oxide?
I
66
What is the charge of cobalt in cobalt(II) chloride?
II
67
What is the name of the compound with the formula CoCl₂?
cobalt(II) chloride
68
What is the name of the compound with the formula V₂S₇?
vanadium(VII) sulfide
69
What is the chemical formula for Diphosphorous pentoxide?
P2O5
70
What is the chemical formula for Beryllium oxide?
BeO
71
What is the chemical formula for Aluminum phosphate?
AlPO4
72
What is the chemical formula for Nitrogen trichloride?
NCl3
73
What is the chemical formula for Sulfur hexafluoride?
SF6
74
What is the chemical formula for Lead (IV) oxide?
PbO2
75
What is the chemical formula for Ammonium carbonate?
(NH4)2CO3
76
What is the chemical formula for Carbon tetrachloride?
CCl4
77
What is the chemical formula for Iron (1) phosphate?
Fe3(PO4)
78
What is the chemical formula for Nickel (I) dichromate?
Ni2Cr2O7
79
What is the chemical formula for Zinc (II) sulfate?
ZnSO4
80
What is the chemical name for SiF4?
Silicon tetrafluoride
81
What is the chemical name for PCl5?
Phosphorus pentachloride
82
What is the chemical name for P2O6?
Diphosphorus hexoxide
83
What is the chemical name for Rb2O?
Rubidium oxide
84
What is the chemical name for V2O5?
Vanadium (V) pentoxide
85
What is the chemical name for SeO2?
Selenium dioxide
86
What is the chemical name for NO?
Nitric oxide
87
What is the chemical name for MgO?
Magnesium oxide
88
What is the chemical name for FeO?
Iron (II) oxide
89
What is the chemical name for Fe2O3?
Iron (III) oxide
90
What is the chemical name for CaO?
Calcium oxide
91
Who formulated a theory of bonding to help us understand covalent molecules?
GN Lewis
92
What characteristic do the electron configurations of noble gases have?
Completely filled valence shells
93
Why are noble gases considered chemically stable?
They are unreactive
94
What model did Lewis use to explain the chemical stability of covalent molecules?
Filled electron shell model
95
What must every atom in a stable covalent molecule achieve?
Noble gas configuration
96
To which elements is Lewis's theory most appropriate?
1st and 2nd row elements
97
What is the duet rule related to?
Helium with 2 valence electrons
98
What is the octet rule related to?
Neon with 8 valence electrons
99
True or False: The filled electron shell model explains the stability of ionic compounds.
False
100
What is used to show bond polarity in a molecule?
Partial negative and partial positive charges
## Footnote
This indicates that the molecule is polar.
101
How is polarity indicated in a molecule?
Using a dipole moment
## Footnote
A dipole moment is represented by an arrow extending from the positive side to the negative side.
102
What concept can be used to estimate the polarity of a bond?
Electronegativity
103
What is electronegativity a measure of?
The ability of an atom to attract electrons towards its nuclear center.
104
Which method is commonly used to measure electronegativity?
Pauling method
105
What is the electronegativity of Fluorine?
4.0
106
What is the electronegativity of Francium?
0.7
107
How does electronegativity generally change across a period?
Increases as you go across a period.
108
How does electronegativity generally change up a group?
Increases as you go up a group.
109
What happens to electronic density when H and F form a bond?
Electronic density lies closer to the F atom.
110
What does the larger electronegativity difference between two atoms indicate?
The more polar the bond that forms between them.
111
What results from a polar bond in a molecule made up of two atoms?
A polar molecule
112
What is necessary to discuss a molecule's polarity when it has three or more atoms?
The arrangement of the molecule's atoms in space, known as molecular geometry.
113
What influences the geometries that molecules form?
Electrostatic interactions
114
True or False: The geometry of a molecule can be predicted based on its polarity.
False
115
How many bonds does H usually form?
H always forms only 1 bond
## Footnote
H has 0 lone pairs and needs to share 1 electron to achieve a duet.
116
How many bonds does O usually form?
O usually forms 2 bonds
## Footnote
O has 2 lone pairs and needs to share 2 electrons to achieve an octet.
117
How many bonds does N usually form?
N usually forms 3 bonds
## Footnote
N has 1 lone pair and needs to share 3 electrons to achieve an octet.
118
How many bonds does C usually form?
C usually forms 4 bonds
## Footnote
C has 0 lone pairs and needs to share 4 electrons to achieve an octet.
119
Fill in the blank: H usually forms _______ bonds.
1
120
Fill in the blank: O usually forms _______ bonds.
2
121
Fill in the blank: N usually forms _______ bonds.
3
122
Fill in the blank: C usually forms _______ bonds.
4
123
True or False: O needs to share 2 electrons to achieve an octet.
True
124
True or False: N has 2 lone pairs.
False. N has 1 lone pair
125
True or False: C has 0 lone pairs.
True
126
What factors determine bond length and strength?
The number of electrons being shared.
127
Which type of bond is the longest and the weakest?
Single bonds.
128
What is the electron count in a single bond?
2 electrons.
129
Which type of bond is the shortest and the strongest?
Triple bonds.
130
What is the electron count in a triple bond?
6 electrons.
131
True or False: It takes more energy to break shorter (stronger) bonds than longer (weaker) bonds.
True.
132
Fill in the blank: Single bonds are the _______ and _______.
longest; weakest.
133
Fill in the blank: Triple bonds are the _______ and _______.
shortest; strongest.
134
What type of molecules align in a magnet?
Polar molecules
135
What type of molecules do not align in a magnet?
Non-polar molecules
136
What is the chemical formula for ammonia?
NH₃
137
True or False: Carbon dioxide is a polar molecule.
False
138
Despite having polar covalent bonds, carbon dioxide is classified as what type of molecule?
Non-polar molecule
139
What do the stoichiometric coefficients in a balanced chemical equation signify?
The combining ratio of reactants and products, not the actual number of molecules that react.
140
Fill in the blank: The stoichiometric coefficients indicate the _______ of reactants and products.
combining ratio
141
True or False: The stoichiometric coefficients represent the actual number of molecules that react.
False
142
What is defined as the system in a chemical reaction?
The actual substances involved in the chemical reaction, including both the reactants and products.
143
What constitutes the surroundings in a chemical reaction?
Everything else, including the solvent, glassware, and nearby air.
144
Fill in the blank: The system in a chemical reaction includes both the _______ and products.
reactants
145
True or False: The surroundings include only the solvent in a chemical reaction.
False
146
What is the importance of distinguishing between the system and surroundings in a chemical reaction?
To clearly identify what substances are undergoing change and what is influencing them.
147
What is the term for a reaction where energy is transferred from the system to the surroundings?
Exothermic
## Footnote
An example of an exothermic reaction is the gummy reaction, where the beaker feels hot.
148
What happens to the potential energy of the system in an exothermic reaction?
Decreases
## Footnote
This decrease in potential energy results in the beaker feeling hot.
149
What is the term for a reaction where energy is transferred from the surroundings into the system?
Endothermic
## Footnote
In an endothermic reaction, the beaker feels cold.
150
What happens to the potential energy of the system in an endothermic reaction?
Increases
## Footnote
The increase in potential energy results in the beaker feeling cold.
151
How is heat represented in a chemical equation for an endothermic reaction?
As a reactant
## Footnote
This indicates that the system absorbs heat from the surroundings.
152
In a potential energy diagram for an endothermic reaction, how is potential energy represented?
APE being greater than zero
## Footnote
This shows that the potential energy of the system increases.
153
What does the beaker feel like during an endothermic reaction?
Cold
## Footnote
This occurs because the surroundings lose energy.
154
Fill in the blank: If energy is transferred from the surroundings into the system, the reaction is called _______.
Endothermic
155
Fill in the blank: In an exothermic reaction, the beaker feels _______.
Hot
156
True or False: An exothermic reaction results in an increase in potential energy of the system.
False
## Footnote
Exothermic reactions result in a decrease in potential energy.
157
What is the heat of a chemical reaction due to?
Making and breaking of bonds
158
What does the potential energy of the system change do?
Releases or absorbs heat
159
How is the change in enthalpy related to potential energy under normal laboratory conditions?
Change in enthalpy is the same as change in potential energy
160
What is the heat of a reaction represented by?
ΔH of a reaction
161
What happens to the potential energy of the system in an exothermic reaction?
Goes down
162
In an exothermic reaction, what is the sign of ΔH?
ΔH < 0
163
What happens to the energy in an endothermic reaction?
Energy is absorbed by the system
164
In an endothermic reaction, what is the sign of ΔH?
ΔH > 0
165
What is the relationship between bond formation and ΔH?
Energy is released when bonds are formed, thus ΔH < 0
166
What is required to break a bond in terms of ΔH?
Energy is required, thus ΔH > 0
167
What is bond formation primarily about?
Going to lower energy states
## Footnote
This process contributes to the stability of molecules.
168
What happens to energy when atoms get closer together beyond the bond length (optimum distance apart?
Energy goes up due to proton repulsion
## Footnote
Protons in the nuclei begin to repel one another.
169
What happens to the potential energy (PE) of a system when bonds are formed?
PE of the system goes down
## Footnote
This results in AH being negative.
170
What does AH represent in chemistry?
AH represents the change in enthalpy
## Footnote
AH is calculated as H final - H initial.
171
What is the potential energy in chemistry related to?
The potential to make a bond
## Footnote
When a bond is made, this potential energy is lost.
172
When is AH negative?
When bonds are formed
## Footnote
This indicates a release of energy.
173
Fill in the blank: When bonds are formed, the potential energy of the system goes _______.
down
174
True or False: The formation of bonds increases the potential energy of a molecule.
False
## Footnote
Bond formation decreases potential energy.
Chem 1
flashcards
Decks in class (18)
# Cards
-
Polyatomic ions29
-
Elements And Their Names60
-
Topic 1 Matter Models Math153
-
Topic 6 Energy Consideration10
-
Topic 2 Atoms and Orbitals79
-
Topic 3 Basic Bonding Principles174
-
Topic 10 Molecular Geometry111
-
Topic 11 Valence Bond Theory63
-
Topic 12 Molecular Orbital Theory72
-
Topic 7 Periodic Trends70
-
Topic 8 Atomic Spectroscopy65
-
Topic 9 The Electron96
-
Topic 13 The Mole18
-
Topic 14 Stoichiometry Calculations10
-
Topic 15 Empirical and Molecular Formula15
-
Topic 16 Phase Change and IMFs148
-
Topic 17 Gases84
-
Topic 18 Applications of Stoichiometry37
