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CHEM 101 > Unit 2 > Flashcards

Unit 2 Flashcards

1
Q

What are the 3 types of chemical bonds?

A

Ionic, covalent, and metallic bonding.

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2
Q

What is ionic bonding?

A

Transfer of electrons between a metal and a nonmetal.

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3
Q

What structure do ionic compounds form?

A

Extended structures (lattice).

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4
Q

What is Coulomb’s law formula for electrostatic force?

A

E=(q1*q2)/(d^2)

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5
Q

What is lattice energy?

A

Energy released when gaseous ions form an ionic solid.

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6
Q

Trend: NaCl (801°C) vs. NaI (661°C) vs. MgO (2852°C). Why?

A

Higher charge and smaller ion size increase lattice energy.

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7
Q

What is covalent bonding?

A

Sharing of electrons between nonmetals.

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8
Q

Difference between molecular and extended covalent structures?

A

Molecular: gases/liquids, low melting points.
Extended: hard solids, high melting points.

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9
Q

What are polar covalent bonds?

A

Unequal sharing of electrons.

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10
Q

What is electronegativity?

A

Ability of an atom to attract shared electrons.

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11
Q

What is electron affinity?

A

Energy change when an electron is added to an atom.

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12
Q

What is metallic bonding?

A

Metals with delocalized electrons (“sea of electrons”).

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13
Q

Properties of metals?

A

Malleable, ductile, and good conductors.

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14
Q

Define Lewis structures.

A

Diagrams showing valence electrons and bonds.

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15
Q

What rule do Lewis structures follow?

A

Octet rule (8 valence e-) or 2 for hydrogen.

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16
Q

What is a lone pair?

A

Non-bonding pair of electrons.

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17
Q

What are expanded octets?

A

Period 3+ elements can hold >8 valence electrons.

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18
Q

Give an example of an incomplete octet.

A

BF3 (Boron has only 6 electrons).

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19
Q

What is a formal charge?

A

FC=valencee-−(lonepairs+ (1/2)bonding e-)

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20
Q

Why do resonance structures exist?

A

Electrons are delocalized; multiple valid Lewis structures.

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21
Q

What is bond order?

A

Number of bonds between atoms (1=single, 2=double).

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22
Q

What is VSEPR theory?

A

Electron pairs arrange to minimize repulsion.

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23
Q

AX2 geometry?

A

Linear

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24
Q

AX3 geometry?

A

Trigonal planar.

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25
AX4 geometry?
Tetrahedral
26
AX3E geometry?
Trigonal pyramidal.
27
AX2E2 geometry?
Bent.
28
AX5 geometry?
Trigonal bipyramidal.
29
AX6 geometry?
Octahedral.
30
What is a dipole moment?
Measure of molecule's polarity.
31
What is Molecular Orbital Theory?
Quantum mechanics applied to molecules.
32
How are MOs formed?
Combination of atomic orbitals.
33
How many MOs are formed?
Equal to the number of AOs combined.
34
What is a bonding MO?
Lower energy, stabilizing.
35
What is an antibonding MO?
Higher energy, destabilizing.
36
What are homonuclear diatomic molecules?
B2 is paramagnetic due to unpaired electrons.
37
Trend in bond length from N2 to O2.
Increasing antibonding e- weakens bonds, increases length.
38
Difference: VBT vs. MOT for O2?
VBT predicts diamagnetic; MOT predicts paramagnetic.
39
Define Arrhenius acid and base.
Acid: Increases H3O+; Base: Increases OH-.
40
Define Bronsted-Lowry acid and base.
Acid: Proton donor; Base: Proton acceptor.
41
Define Lewis acid and base.
Acid: Electron pair acceptor; Base: Electron pair donor.
42
What is a conjugate acid-base pair?
Species differing by one H+.
43
Example of conjugate pairs: HCl and Cl-.
HCl (acid) → Cl- (conjugate base).
44
What is a strong acid?
Ionizes completely in water.
45
What is a weak acid?
Ionizes partially in water.
46
How does bond polarity affect acidity?
Higher bond polarity increases acidity.
47
What is the trend of binary acid strength?
Down a group: stronger (longer bonds). Across a period: stronger (more polar bonds).
48
Rank HF, HCl, HBr, HI in acidity.
HI > HBr > HCl > HF.
49
What are oxyacids?
Acids where H+ is bonded to oxygen.
50
What affects oxyacid strength?
Electronegativity and number of oxygens.
51
Which is stronger: HClO4 or HClO?
HClO4 (more oxygen atoms stabilize the conjugate base).
52
Rank CH3COOH, CH2ClCOOH, CCl3COOH.
CCl3COOH > CH2ClCOOH > CH3COOH.
53
What are diprotic acids?
Acids that can donate two protons (e.g., H2SO4).
54
What is a Lewis acid-base adduct?
Product formed by a Lewis acid-base reaction.
55
Factors affecting acid strength in binary acids?
Bond length and bond polarity.
56
Example of a neutralization reaction?
HCl+NaOH→NaCl+H2O.
57
What is hybridization?
Mixing of atomic orbitals to form hybrid orbitals.
58
sp hybridization geometry?
Linear.
59
sp2 hybridization geometry?
Trigonal planar.
60
sp3 hybridization geometry?
Tetrahedral.
61
What is a sigma bond?
End-to-end orbital overlap.
62
What is a pi bond?
Side-to-side orbital overlap.
63
How many bonds in C2H4?
5 sigma, 1 pi.
64
Bond energy vs. bond length relationship?
Shorter bond = higher energy.
65
What is resonance energy?
Stability gained from delocalized electrons.
66
What is an amphoteric oxide?
Oxide acting as both acid and base (e.g., BeO).
67
What are noble gases known for?
Unreactivity due to full valence shells.
68
What are p-block anomalies?
Second-period elements differ due to size/electronegativity.
69
Why is Li unique in Group 1?
Small size; forms Li2O instead of KO2.
70
Why does N2 form pi bonds but P4 does not?
Small size of N allows efficient overlap.
71
Example of a polar molecule?
H2O.

CHEM 101 (2 decks)

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