Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

CHEM 101 > Unit 2 > Flashcards

Unit 2 Flashcards

You may prefer our related Brainscape-certified flashcards:
Physics 101 flashcards AP® Chemistry flashcards Psychology 101 flashcards Periodic Table flashcards Chemistry 101 flashcards Biology 101 flashcards Organic Chemistry 101 flashcards Sociology 101 flashcards
1
Q

What are the 3 types of chemical bonds?

A

Ionic, covalent, and metallic bonding.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is ionic bonding?

A

Transfer of electrons between a metal and a nonmetal.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What structure do ionic compounds form?

A

Extended structures (lattice).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is Coulomb’s law formula for electrostatic force?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is lattice energy?

A

Energy released when gaseous ions form an ionic solid.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is covalent bonding?

A

Sharing of electrons between nonmetals.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Difference between molecular and extended covalent structures?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are polar covalent bonds?

A

Unequal sharing of electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is electronegativity?

A

Ability of an atom to attract shared electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is electron affinity?

A

Energy change when an electron is added to an atom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is metallic bonding?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Properties of metals?

A

Malleable, ductile, and good conductors.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Define Lewis structures.

A

Diagrams showing valence electrons and bonds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What rule do Lewis structures follow?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is a lone pair?

A

Non-bonding pair of electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What are expanded octets?

A

Period 3+ elements can hold >8 valence electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Give an example of an incomplete octet.

A

BF3 (Boron has only 6 electrons).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is a formal charge?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Why do resonance structures exist?

A

Electrons are delocalized; multiple valid Lewis structures.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is bond order?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is VSEPR theory?

A

Electron pairs arrange to minimize repulsion.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

AX2 geometry?

A

Linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

AX3 geometry?

A

Trigonal planar.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

AX4 geometry?

A

Tetrahedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

AX3E geometry?

A

Trigonal pyramidal.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

AX2E2 geometry?

A

Bent.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

AX5 geometry?

A

Trigonal bipyramidal.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

AX6 geometry?

A

Octahedral.

30
Q

What is a dipole moment?

A

Measure of molecule’s polarity.

31
Q

What is Molecular Orbital Theory?

A

Quantum mechanics applied to molecules.

32
Q

How are MOs formed?

A

Combination of atomic orbitals.

33
Q

How many MOs are formed?

A

Equal to the number of AOs combined.

34
Q

What is a bonding MO?

A

Lower energy, stabilizing.

35
Q

What is an antibonding MO?

A

Higher energy, destabilizing.

36
Q

What are homonuclear diatomic molecules?

A

B2 is paramagnetic due to unpaired electrons.

37
Q

Trend in bond length from N2 to O2.

A

Increasing antibonding e- weakens bonds, increases length.

38
Q

Difference: VBT vs. MOT for O2?

A

VBT predicts diamagnetic; MOT predicts paramagnetic.

39
Q

Define Arrhenius acid and base.

A

Acid: Increases H3O+; Base: Increases OH-.

40
Q

Define Bronsted-Lowry acid and base.

A

Acid: Proton donor; Base: Proton acceptor.

41
Q

Define Lewis acid and base.

A

Acid: Electron pair acceptor; Base: Electron pair donor.

42
Q

What is a conjugate acid-base pair?

A

Species differing by one H+.

43
Q

Example of conjugate pairs: HCl and Cl-.

A

HCl (acid) → Cl- (conjugate base).

44
Q

What is a strong acid?

A

Ionizes completely in water.

45
Q

What is a weak acid?

A

Ionizes partially in water.

46
Q

How does bond polarity affect acidity?

A

Higher bond polarity increases acidity.

47
Q

What is the trend of binary acid strength?

A

Down a group: stronger (longer bonds).
Across a period: stronger (more polar bonds).

48
Q

Rank HF, HCl, HBr, HI in acidity.

A

HI > HBr > HCl > HF.

49
Q

What are oxyacids?

A

Acids where H+ is bonded to oxygen.

50
Q

What affects oxyacid strength?

A

Electronegativity and number of oxygens.

51
Q

Which is stronger: HClO4 or HClO?

A

HClO4 (more oxygen atoms stabilize the conjugate base).

52
Q

Rank CH3COOH, CH2ClCOOH, CCl3COOH.

A

CCl3COOH > CH2ClCOOH > CH3COOH.

53
Q

What are diprotic acids?

A

Acids that can donate two protons (e.g., H2SO4).

54
Q

What is a Lewis acid-base adduct?

A

Product formed by a Lewis acid-base reaction.

55
Q

Factors affecting acid strength in binary acids?

A

Bond length and bond polarity.

56
Q

Example of a neutralization reaction?

A

HCl+NaOH→NaCl+H2O.

57
Q

What is hybridization?

A

Mixing of atomic orbitals to form hybrid orbitals.

58
Q

sp hybridization geometry?

A

Linear.

59
Q

sp2 hybridization geometry?

A

Trigonal planar.

60
Q

sp3 hybridization geometry?

A

Tetrahedral.

61
Q

What is a sigma bond?

A

End-to-end orbital overlap.

62
Q

What is a pi bond?

A

Side-to-side orbital overlap.

63
Q

How many bonds in C2H4?

A

5 sigma, 1 pi.

64
Q

Bond energy vs. bond length relationship?

A

Shorter bond = higher energy.

65
Q

What is resonance energy?

A

Stability gained from delocalized electrons.

66
Q

What is an amphoteric oxide?

A

Oxide acting as both acid and base (e.g., BeO).

67
Q

What are noble gases known for?

A

Unreactivity due to full valence shells.

68
Q

What are p-block anomalies?

A

Second-period elements differ due to size/electronegativity.

69
Q

Why is Li unique in Group 1?

A

Small size; forms Li2O instead of KO2.

70
Q

Why does N2 form pi bonds but P4 does not?

A

Small size of N allows efficient overlap.

71
Q

Example of a polar molecule?

A

H2O.

CHEM 101 (2 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions