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Chemistry 120 > Quiz 1 > Flashcards

Quiz 1 Flashcards

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1
Q

Nitric Acid

A

HNO₃
Acid

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2
Q

Barium Hydroxide

A

Ba(OH)₂
Base

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3
Q

Hydrobromic Aicd

A

HBr (aq)
Acid

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4
Q

Hydroxide Ion

or Compounds containg Hydroxide

A

HO-
Base

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5
Q

Phosphoric Acid

A

H₃PO₄

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6
Q

Calcium Hydroxide

A

Ca(OH)₂
Base

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7
Q

Sulfuric Acid

A

H₂SO₄

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8
Q

Potassium Hydroxide

A

KOH
Base

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9
Q

Hydromiun Ion

What you get when you mix a strong acid in water

A

H₃O+
Acid

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10
Q

Lithium Hydroxide

A

LiOH
Base

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11
Q

Hydroiodic Acid

A

HI (aq)

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12
Q

Hydrochloric Acid

A

HCl (aq)

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13
Q

Any Molcules with an Amine

A

R₃N, R₂NH, RNH₂
Base

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14
Q

Perchloric Acid

A

HClO₄
Acid

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15
Q

Sodium Hydroxide

A

NaOH
Base

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16
Q

Sodium Carbonate

A

Na₂CO₃

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17
Q

Any molecule with a Carboxylic Acid

A

R-CO₂H
Acid

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18
Q

Ammonia

A

NH₃
Base

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19
Q

Sodium Bicarbonate

A

NaHCO₃

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20
Q
A

Linear
* 2 Bonding Groups
* 0 lone Pairs
* 120 Degree Bond Angle

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21
Q
A

Trigonal Planar
* 3 Bonding Groups
* 0 lone Pairs
* 120 Degree Bond Angle

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22
Q
A

Bent
* 2 Bonding Groups
* 1 lone Pairs
* <120 Degree Bond Angle

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23
Q
A

Tetrahedral
* 4 Bonding Groups
* 0 lone Pairs
* 120 Degree Bond Angle

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23
Q
A

Tetrahedral
* 4 Bonding Groups
* 0 lone Pairs
* 109 Degree Bond Angle

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24
Q
A

Trigonal Pyramidal
* 3 Bonding Groups
* 1 lone Pairs
* 120 Degree Bond Angle

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25
Q
A

Bent
* 2 Bonding Groups
* 2 lone Pairs
* &laquo_space;109 Degree Bond Angle

26
Q
A

Trigonal Bipyramidal
* 5 Bonding Groups
* 0 lone Pairs
* 120 & 90 Degree Bond Angle

27
Q
A

See Saw
* 4 Bonding Groups
* 1 lone Pairs
* <120&<90 Degree Bond Angle

28
Q
A

T shape
* 3 Bonding Groups
* 2 lone Pairs
* <90 Degree Bond Angle

29
Q
A

Linear
* 2 Bonding Groups
* 3 lone Pairs
* 120 Degree Bond Angle

30
Q
A

Octahedral
* 6 Bonding Groups
* 0 lone Pairs
* 90 Degree Bond Angle

31
Q
A

Square Pyrimidal
* 5 Bonding Groups
* 1 lone Pairs
* 120 Degree Bond Angle

32
Q
A

Square Planar
* 4 Bonding Groups
* 2 lone Pairs
* 90 Degree Bond Angle

33
Q
A

T-shape
* 3 Bonding Groups
* 3 lone Pairs
* <90 Degree Bond Angle

34
Q
A

Linear
* 2 Bonding Groups
* 4 lone Pairs
* 180 Degree Bond Angle

35
Q

Saturated

A

Single bonds

36
Q

Unsaturated

A

double bonds

37
Q

Constitutional (structural) isomers

A

Have the same molecular formula but the atom has diffrent connectivity.

38
Q

Stereoisomers

A

Any two molecules that have the same connectivity between the atoms but atoms are arranged diffrently in space

39
Q

conformatinal Isomers

A

diffrent only by a rotation of a single bond

40
Q

Cis

A

atoms on same side of molecule

41
Q

trans

A

atoms on diffrent sides of the molecule

42
Q

If there is an ionic bond

A

Show the ion as separate and charged

43
Q
A

Aromatic Ring

44
Q

Acids

A

Proton (H) donator

45
Q

Base

A

Proton (H) acceptor

46
Q

What happens to H₂CO₃

A

It is not stable so it decomposes into water and carbon dioxide

47
Q

Solubility Rule of Thumb

A

Need <4 carbons per H binding functional group to be solule in water

48
Q

Hybrid Atomic Orbital: SP

A
  • Linear VSEPR
  • 2 unused p-orbial
  • Double or triple bond
49
Q

Hybrid Atomic Orbital: SP2

A
  • Trigonal Planar VSEPR
  • 1 unused p-orbial
  • Double bond
50
Q

Hybrid Atomic Orbital: SP3

A
  • Tetrahedral VSEPR
  • 0 unused p-orbial
  • single bonds
51
Q

Delocalization of electrons (conjugation and resonance) is stablilizing

A
52
Q

LUMO

A

lowest unoccipied molecular orbial

53
Q

HOMO

A

Highest occupied molecular orbital

54
Q

the smaller the HOMO, LUMO gap

A

the longer the wavelenght

55
Q

Congucation leads to

A

a smaller HOMO-LUMO gap

56
Q

Calculating Formal Charge

A

valence shell electrons(free atom)-#lone pair electrons - 1/2 # bonding electrons

57
Q

Coordinate covalent bond

A

where electrons are coming from one atom/molecule and are going to the metal

58
Q

Ligands

A

Atoms/molecules that are binding to the metal

59
Q

Chelating Ligands

A

can bond more than once (multiple doantion sites)

60
Q

Cordination number

A

number of groups bonded to the metal

61
Q

Stability Rules

A
  • octet rule-All atoms have there octet unless ir is 3rd period or lower then it can have an expanded octet
  • Minimize formal charges
  • Have negative charge on the more electronegative atoms
62
Q

Boiling Point

A
  • the stronger the IMFs the higher the boiling point (and melting point)
  • IMFs= the bonds molecules can make with other molecules
  • Hydrogen bonds - strong happen between N,O,F and hydrogen
  • Dipole-Dipole
  • Dispersion forces - weak

Chemistry 120 (6 decks)

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