Intramolecular Forces Flashcards
(151 cards)
1
Q
Chris
Brown’s
Mom
Stinks
A
Covalent
Bonds
Mutal
Sharing
2
Q
Caitlin
Clark
Often
Acts
Stupid
A
Coordinate
Covalent
One
Atom
Sharing
3
Q
What is a covalent bond?
A
A covalent bond is a chemical bond formed by the sharing of one or more pairs of electrons between two atoms.
4
Q
True or False: Sigma bonds are formed by the head-on overlap of atomic orbitals.
A
True
5
Q
What is a pi bond?
A
A pi bond is a type of covalent bond that occurs when two lobes of one involved orbital overlap with two lobes of another in a side-by-side manner.
6
Q
Fill in the blank: The strength of a covalent bond is often measured in terms of __________.
A
bond energy
7
Q
What does bond order indicate?
A
Bond order indicates the number of shared electron pairs between two atoms.
8
Q
What is the bond length?
A
Bond length is the distance between the nuclei of two bonded atoms.
9
Q
How many sigma bonds are present in a double bond?
A
One sigma bond
10
Q
How many pi bonds are present in a triple bond?
A
Two pi bonds
11
Q
True or False: Higher bond order generally results in shorter bond lengths.
A
True
12
Q
What is the relationship between bond strength and bond length?
A
Generally, shorter bonds are stronger than longer bonds.
13
Q
Which type of bond is typically weaker, sigma or pi bonds?
A
Pi bonds are typically weaker than sigma bonds.
14
Q
Fill in the blank: The energy required to break a covalent bond is known as __________.
A
bond dissociation energy
15
Q
What is the bond order of a single bond?
A
The bond order of a single bond is 1.
16
Q
True or False: All covalent bonds have the same bond energy.
A
False
17
Q
What is the bond energy of a double bond compared to a single bond?
A
The bond energy of a double bond is generally higher than that of a single bond.
18
Q
What is the typical bond length of a C-H bond?
A
Approximately 1.09 Å (angstroms)
19
Q
What happens to bond energy as the number of shared electron pairs increases?
A
Bond energy generally increases.
20
Q
Which bond has a bond order of 3?
A
A triple bond
21
Q
Fill in the blank: A bond length can be measured in __________.
A
angstroms or picometers
22
Q
True or False: Bond strength is independent of bond length.
A
False
23
Q
What is the bond order of a molecule with one single bond and one double bond?
A
1.5
24
Q
Which type of bond typically involves the overlap of p orbitals?
A
Pi bonds
25
True or False: Bond length can be affected by the presence of lone pairs on bonded atoms.
True
26
What is the bond energy trend for bonds in the same group of the periodic table?
Bond energy generally decreases down a group.
27
Fill in the blank: The bond length of a double bond is __________ than that of a single bond.
shorter
28
What is the bond order for a molecule with two double bonds?
4
29
True or False: A higher bond order usually correlates with increased stability of a molecule.
True
30
What is the typical bond length of a C=C double bond?
Approximately 1.34 Å (angstroms)
31
Which type of bond involves a direct overlap of orbitals?
Sigma bonds
32
Fill in the blank: The bond energy is higher for __________ bonds than for single bonds.
double or triple
33
What is the effect of electronegativity on bond strength?
Higher electronegativity differences generally lead to stronger bonds.
34
True or False: Bond length can be determined using X-ray diffraction techniques.
True
35
What type of bond is formed between two atoms that share three pairs of electrons?
Triple bond
36
Fill in the blank: The bond energy of a bond is the __________ required to break it.
energy
37
What is the difference between a sigma bond and a pi bond in terms of orbital overlap?
Sigma bonds involve head-on overlap, while pi bonds involve side-by-side overlap.
38
What is the bond order of a molecule with one triple bond?
3
39
True or False: A molecule can have both sigma and pi bonds.
True
40
How does bond length change with increased bond order?
Bond length decreases with increased bond order.
41
What is the typical bond length of a C-C single bond?
Approximately 1.54 Å (angstroms)
42
True or False: Polar covalent bonds occur when electrons are shared equally between two atoms.
False
43
Fill in the blank: In a polar covalent bond, one atom has a __________ electronegativity than the other.
higher
44
What is electronegativity?
Electronegativity is a measure of an atom's ability to attract and hold onto electrons.
45
Which type of bond has a significant difference in electronegativity between the two atoms?
Ionic bond
46
Multiple Choice: Which of the following bonds is considered polar? A) H-H B) O-H C) C-C
B) O-H
47
True or False: Nonpolar covalent bonds have an electronegativity difference of 0.
True
48
What is the typical electronegativity difference range for polar covalent bonds?
0.4 to 1.7
49
Fill in the blank: Molecules with polar covalent bonds may have a __________ dipole moment.
net
50
What determines the polarity of a molecule?
The shape of the molecule and the distribution of polar bonds.
51
Multiple Choice: Which of the following molecules is nonpolar? A) CO2 B) H2O C) NH3
A) CO2
52
True or False: A molecule can be polar if it contains only nonpolar bonds.
False
53
What is a dipole moment?
A dipole moment is a measure of the separation of positive and negative charge in a molecule.
54
Fill in the blank: The greater the difference in electronegativity, the __________ the polarity of the bond.
greater
55
What role do lone pairs play in molecular polarity?
Lone pairs can affect the shape of a molecule and contribute to its overall dipole moment.
56
Multiple Choice: Which atom is more electronegative? A) Oxygen B) Carbon
A) Oxygen
57
True or False: All polar molecules are soluble in water.
True
58
What is a common property of polar molecules?
They tend to dissolve well in polar solvents like water.
59
Fill in the blank: __________ is the term for a molecule that has both a positive and a negative end.
Dipole
60
How does the presence of polar bonds affect the boiling point of a substance?
Polar bonds generally lead to higher boiling points due to stronger intermolecular forces.
61
What is a diatomic molecule?
A molecule composed of two atoms.
62
Which of the following is NOT a diatomic molecule? A) H2 B) O2 C) CO2
C) CO2
63
True or False: All diatomic molecules are composed of the same type of atoms.
False
64
Fill in the blank: The seven diatomic elements are H2, N2, O2, F2, Cl2, Br2, and _____.
I2
## Footnote
BrINCHIHOF
65
Which diatomic molecule is essential for respiration in humans?
O2 (oxygen)
66
What type of bond is typically found in diatomic molecules composed of the same element?
Covalent bond
67
Multiple Choice: Which diatomic molecule is a gas at room temperature? A) I2 B) Cl2 C) Br2
B) Cl2
68
What is the molecular formula for nitrogen gas?
N2
69
True or False: H2 is the lightest diatomic molecule.
True
70
What is the significance of diatomic molecules in chemical reactions?
They often act as reactants or products in various chemical processes.
71
Fill in the blank: Diatomic molecules can be either _____ or _____ in nature.
homonuclear, heteronuclear
72
Which diatomic molecule is known as the most abundant in the Earth's atmosphere?
N2 (nitrogen)
73
Multiple Choice: Which of the following diatomic molecules is a halogen? A) H2 B) Cl2 C) N2
B) Cl2
74
What is the primary characteristic of homonuclear diatomic molecules?
They consist of two identical atoms.
75
Name one example of a heteronuclear diatomic molecule.
CO (carbon monoxide)
76
What is a Lewis dot structure?
A diagram that shows the bonding between atoms of a molecule and the lone pairs of electrons.
77
True or False: Lewis dot structures can represent both ionic and covalent compounds.
True
78
What do the dots in a Lewis dot structure represent?
Valence electrons.
79
How many valence electrons does carbon have?
4 valence electrons.
80
Fill in the blank: The formal charge is calculated using the formula ___ = (valence electrons) - (nonbonding electrons) - (1/2 bonding electrons).
Formal charge
81
What is the purpose of calculating formal charges?
To determine the most stable Lewis structure.
82
Which of the following atoms can have expanded octets: P, S, Cl, or all of the above?
All of the above.
83
True or False: A resonance structure represents a single arrangement of electrons in a molecule.
False
84
What is resonance in chemistry?
The phenomenon where a molecule can be represented by two or more valid Lewis structures.
85
What is the difference between a resonance structure and a Lewis structure?
A resonance structure is one of multiple forms, while a Lewis structure is a specific representation.
86
Which element typically does not follow the octet rule?
Hydrogen.
87
What is the octet rule?
Atoms tend to bond in a way that gives them eight valence electrons.
88
Fill in the blank: The total number of valence electrons in a molecule is the sum of the valence electrons of all ___ atoms.
Bonded
89
What is a coordinate covalent bond?
A bond formed when one atom donates both electrons to a bond.
90
True or False: All resonance structures contribute equally to the resonance hybrid.
False
91
What is a resonance hybrid?
A representation of a molecule that is an average of all its resonance structures.
92
Which of the following has a formal charge of zero: O2, CO2, or H2O?
CO2
93
How can you determine the most stable resonance structure?
By evaluating formal charges and minimizing them.
94
What role do lone pairs play in Lewis structures?
They represent non-bonding valence electrons.
95
What is the significance of formal charge in predicting molecular stability?
Lower formal charges generally indicate greater stability.
96
True or False: Resonance structures can be drawn with different arrangements of atoms.
False
97
Which molecule has resonance structures: O3, H2O, or CH4?
O3
98
What is the maximum number of bonds an atom can form based on the octet rule?
4 bonds.
99
Fill in the blank: The ___ of a molecule determines how electrons are distributed in Lewis structures.
Geometry
100
What does a double bond consist of?
One sigma bond and one pi bond.
101
True or False: All atoms in a molecule must have a formal charge of zero.
False
102
What is a common mistake when drawing Lewis structures?
Not fulfilling the octet rule for all atoms.
103
What is the preferred resonance structure?
The one with the least formal charges.
104
Fill in the blank: In Lewis structures, hydrogen can only form ___ bond(s).
One
105
What does the term 'delocalized electrons' refer to?
Electrons that are spread out over several atoms in resonance structures.
106
What is the typical charge of a highly electronegative atom in a Lewis structure?
Negative charge.
107
How many resonance structures can a molecule have?
It varies; there is no fixed number.
108
Fill in the blank: The ___ charge on an atom can help predict its reactivity.
Formal
109
What does a triple bond consist of?
One sigma bond and two pi bonds.
110
True or False: Resonance structures can help explain certain properties of molecules, such as bond length.
True
111
What is the relationship between the number of resonance structures and the stability of a molecule?
More resonance structures generally lead to greater stability.
112
What is hybridization?
Hybridization is the mixing of atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons to form chemical bonds.
113
True or False: Hybridization can occur in both main group and transition metals.
True
114
What are the main types of hybridization?
The main types of hybridization are sp, sp2, and sp3.
115
In sp3 hybridization, how many orbitals are hybridized?
Four orbitals are hybridized.
116
Fill in the blank: VSEPR stands for __________.
Valence Shell Electron Pair Repulsion
117
What is the primary goal of VSEPR theory?
To predict the geometry of molecules based on the repulsion between electron pairs.
118
Which molecular shape corresponds to a steric number of 2?
Linear
119
What molecular geometry is associated with a steric number of 4 and no lone pairs?
Tetrahedral
120
True or False: Lone pairs of electrons occupy more space than bonding pairs.
True
121
What is the molecular geometry of CH4?
Tetrahedral
122
What determines the polarity of a molecule?
The difference in electronegativity between atoms and the geometry of the molecule.
123
Fill in the blank: A molecule is considered polar if it has a __________ dipole moment.
net
124
Which of the following molecules is nonpolar: CO2, H2O, NH3?
CO2
125
What is the angle between the bonds in a trigonal planar geometry?
120 degrees
126
True or False: A molecule with a symmetrical shape is always nonpolar.
False
127
What is the hybridization of the central atom in BF3?
sp2
128
What is the molecular geometry of NH3?
Trigonal pyramidal
129
Fill in the blank: In sp hybridization, the hybrid orbitals are formed from __________ and __________ orbitals.
one s and one p
130
What is the bond angle in a tetrahedral molecule?
109.5 degrees
131
Which hybridization corresponds to a linear geometry?
sp
132
True or False: A molecule with polar bonds can be nonpolar overall.
True
133
What is the effect of lone pairs on bond angles in VSEPR theory?
Lone pairs decrease the bond angles between bonding pairs.
134
What shape does a molecule with a steric number of 5 and no lone pairs take?
Trigonal bipyramidal
135
Fill in the blank: The hybridization of carbon in ethylene (C2H4) is __________.
sp2
136
What is the molecular geometry of a molecule with a steric number of 3 and one lone pair?
Bent
137
What type of hybridization does the central atom in a water molecule have?
sp3
138
True or False: Electronegativity differences greater than 1.7 typically indicate ionic bonds.
True
139
What is the molecular geometry of a molecule with two bonding pairs and two lone pairs?
Bent
140
Which hybridization is associated with a bond angle of approximately 180 degrees?
sp
141
What is the molecular geometry of SO2?
Bent
142
Fill in the blank: A molecule with the formula AB2E has a __________ molecular geometry.
bent
143
What hybridization is present in a molecule with a triple bond?
sp
144
True or False: All molecules with polar bonds are polar molecules.
False
145
What is the bond angle in a molecule with sp3 hybridization?
109.5 degrees
146
What determines whether a molecule is polar or nonpolar?
The arrangement of polar bonds and the overall symmetry of the molecule.
147
What is the molecular geometry of a molecule with four bonding pairs and one lone pair?
Seesaw
148
Fill in the blank: The hybridization of nitrogen in NH3 is __________.
sp3
149
What is the molecular shape of carbon dioxide (CO2)?
Linear
150
True or False: VSEPR theory can be used to predict the shape of complex molecules.
True
151
What is the hybridization of the central atom in a molecule with a trigonal bipyramidal shape?
sp3d
152
What are intramolecular forces?
Intramolecular forces are the forces that hold atoms together within a molecule.
153
True or False: Intramolecular forces are generally weaker than intermolecular forces.
False
154
Fill in the blank: The two primary types of intramolecular forces are ______ and ______.
ionic bonds, covalent bonds
155
Which type of intramolecular force involves the sharing of electron pairs between atoms?
Covalent bonds
156
Multiple Choice: What type of intramolecular force is formed between oppositely charged ions? A) Covalent bond B) Ionic bond C) Hydrogen bond
B) Ionic bond
