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Intro Chemistry CHEM 1000 > Chem Bonds Con. 4-6 > Flashcards

Chem Bonds Con. 4-6 Flashcards

1
Q

What is a covalent bond?

A

A bond where atoms share electrons to achieve stability.

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2
Q

How does electronegativity affect covalent bonds?

A

It determines if the bond is polar (unequal sharing) or nonpolar (equal sharing).

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3
Q

What is a polar covalent bond?

A

A bond where electrons are unequally shared, creating partial charges.

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4
Q

What is a nonpolar covalent bond?

A

A bond where electrons are equally shared with no charge separation.

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5
Q

Give an example of a polar molecule.

A

Water (H₂O).

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6
Q

Give an example of a nonpolar molecule.

A

Oxygen gas (O₂).

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7
Q

What is a single bond?

A

A covalent bond where two electrons are shared.

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8
Q

What is a double bond?

A

A covalent bond where four electrons are shared.

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9
Q

What is a triple bond?

A

A covalent bond where six electrons are shared.

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10
Q

What does VSEPR theory stand for?

A

Valence Shell Electron Pair Repulsion theory.

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11
Q

What does VSEPR theory explain?

A

How electron repulsions determine molecular shape.

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12
Q

What is an electron domain?

A

A region of electron density around an atom, including bonding and lone pairs.

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13
Q

What is a lone pair?

A

A pair of valence electrons not involved in bonding.

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14
Q

What molecular shape does CO₂ have?

A

Linear.

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15
Q

What molecular shape does H₂O have?

A

Bent.

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16
Q

What molecular shape does NH₃ have?

A

Trigonal pyramidal.

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17
Q

What determines a molecule’s shape?

A

The number of bonding and lone pairs around the central atom.

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18
Q

Why do lone pairs affect molecular shape?

A

They repel more strongly than bonding pairs, altering bond angles.

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19
Q

What is a dipole moment?

A

A measure of the separation of charge in a polar molecule.

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20
Q

What are intermolecular forces?

A

Forces that exist between molecules.

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21
Q

What are the three types of intermolecular forces?

A

Hydrogen bonding, dipole-dipole forces, and London dispersion forces.

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22
Q

Rank the intermolecular forces from strongest to weakest.

A

Hydrogen bonding > Dipole-dipole > London dispersion.

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23
Q

What is hydrogen bonding?

A

A strong attraction between molecules containing H-F, H-O, or H-N bonds.

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24
Q

What is dipole-dipole interaction?

A

Attraction between polar molecules.

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25
What are London dispersion forces?
Weak attractions due to temporary dipoles in all molecules.
26
What type of intermolecular force is in CH₄?
London dispersion forces.
27
What type of intermolecular force is in H₂O?
Hydrogen bonding.
28
What type of intermolecular force is in CO₂?
London dispersion forces.
29
Why do polar molecules have stronger intermolecular forces?
They have permanent dipoles that create stronger attractions.
30
Why do nonpolar molecules experience intermolecular forces?
Temporary dipoles form due to electron movement.
31
What happens to boiling point as intermolecular forces increase?
It increases.
32
Why does water have a high boiling point?
Strong hydrogen bonding.
33
What determines if a molecule is polar?
Electronegativity differences and molecular shape.
34
How does symmetry affect polarity?
Symmetric molecules are usually nonpolar.
35
What is the molecular formula for sulfur hexafluoride?
SF₆.
36
What is the name of the compound N₂O₅?
Dinitrogen pentoxide.
37
What is the name of CO₂?
Carbon dioxide.
38
What is the molecular formula for boron tribromide?
BBr₃.
39
What is the name of PCl₃?
Phosphorus trichloride.
40
What type of bond exists in N₂?
Triple covalent bond.
41
What type of bond exists in O₂?
Double covalent bond.
42
What is a diatomic element?
An element that naturally exists as two atoms bonded together (e.g., O₂).
43
What causes a molecule to have a dipole moment?
Unequal electron distribution due to electronegativity differences.
44
How do intermolecular forces affect viscosity?
Stronger forces increase viscosity.
45
How do intermolecular forces affect surface tension?
Stronger forces increase surface tension.
46
How do intermolecular forces affect evaporation rate?
Weaker forces increase evaporation.
47
What is the strongest type of intermolecular force?
Hydrogen bonding.
48
Why do noble gases have boiling points?
London dispersion forces exist between their atoms.
49
What is an example of a molecule with dipole-dipole interactions?
HCl.
50
What is an example of a molecule with hydrogen bonding?
NH₃.
51
How does bond length relate to bond strength?
Shorter bonds are stronger.
52
How does bond type affect reactivity?
Triple bonds are less reactive than single bonds.
53
What is a resonance structure?
A molecule with multiple valid Lewis structures.
54
What is formal charge?
A method to determine the most stable Lewis structure.
55
Why do atoms form covalent bonds?
To achieve a full valence shell.
56
What is hybridization in molecular bonding?
The mixing of atomic orbitals to form new bonding orbitals.
57
What is the octet rule?
Atoms tend to form bonds to obtain 8 valence electrons.
58
What is an expanded octet?
When elements in period 3 or higher exceed 8 valence electrons.
59
Why do halogens form single bonds?
They need one more electron to complete their octet.
60
What type of bond is in HCl?
Polar covalent bond.
61
What is the strongest bond: single, double, or triple?
Triple.
62
How does bond polarity affect solubility?
Polar compounds dissolve in polar solvents.
63
What is the molecular geometry of CH₄?
Tetrahedral.
64
What is the molecular geometry of BF₃?
Trigonal planar.
65
What is the molecular geometry of HCN?
Linear.
66
What is the molecular geometry of PH₃?
Trigonal pyramidal.
67
How does molecular polarity affect boiling points?
Polar molecules have higher boiling points.
68
What causes London dispersion forces?
Temporary electron fluctuations.
69
Why is NaCl not a covalent compound?
It has ionic bonds due to electron transfer.
70
What is the weakest type of covalent bond?
Single bond.
71
What determines bond energy?
Bond type and bond length.
72
What is the general rule for naming covalent compounds?
Use prefixes to indicate the number of atoms and name the elements in the order they appear.
73
True or False: The prefix 'mono-' is used for the first element in a covalent compound.
False
74
Fill in the blank: The compound CO2 is named __________.
carbon dioxide
75
What prefix is used to indicate 3 atoms of an element?
tri-
76
Name the compound N2O5.
dinitrogen pentoxide
77
What is the correct name for the compound PCl3?
phosphorus trichloride
78
Multiple Choice: Which of the following is the correct name for SiO2? A) silicon dioxide B) silicon oxide C) silicon di-oxide
A) silicon dioxide
79
True or False: In naming covalent compounds, the second element's name is modified to end with 'ide'.
True
80
What is the prefix for 5 atoms in covalent compound naming?
penta-
81
Name the compound SCl6.
sulfur hexachloride

Intro Chemistry CHEM 1000 (1 decks)

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