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Chm 2010 > Ch 1 > Flashcards

Ch 1 Flashcards

1
Q

Methane

A

Structure: H-CH2-H
Formula: CH4

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2
Q

Ethane

A

Structure: H-CH2-CH2-H
CH3-CH3
Formula: C2H6

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3
Q

Propane

A

Structure: H-(CH2)3-H
CH3CH2CH3
Formula: C3H8
/\

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4
Q

Butane

A

Structure: H-(CH2)4-H
Formula: C4H10

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5
Q

Pentane

A

Structure: H-(CH2)5-H
Formula: C5H14

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6
Q

Hexane

A

Structure: H-(CH2)6-H
Formula: C6H14

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7
Q

Heptane

A

Structure: H-(CH2)7-H
Formula: C7H16

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8
Q

Octane

A

Structure: H-(CH2)8-H
Formula: C8H18

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9
Q

Nonane

A

Structure: H-(CH2)9-H
Formula: C9H20

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10
Q

Decane

A

Structure: H-(CH2)10-H
Formula: C10H22

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11
Q

Undecane

A

Structure: H-(CH2)11-H
Formula: C11H24

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12
Q

Dodecane

A

Structure: H-(CH2)12-H
Formula: C12H26

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13
Q

Alkane

A

Saturated hydrocarbon (C and H)
C H
n 2n+2

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14
Q

Bonding Molecular Orbitals vs Antibonding Molecular Orbitals

A

Bonding: lower energy than atomic orbitals
Antibonding: higher energy than atomic orbitals

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15
Q

Alkane vs Alkene vs Alkyne

A

Alkane: all single bonds
Alkene: double bond
Alkyne: triple bond

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16
Q

Node

A

Region around the nucleus where probability of e- is 0

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17
Q

Delocalization

A

E- pairs that can appear in one place and then another place in resonance structures

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18
Q

Isomers

A

Different compounds w/ same molecular formula

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19
Q

Resonance structure rules

A
  1. Must have net charge of 0
  2. Must have same # of unpaired e-
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20
Q

Major contributor resonance structure preference is determined by what factors

A
  1. Structure w/ the smallest separation of oppositely charged atoms
  2. Structure where the negative charge resides on the most electroneg atom and positive charge on least electroneg atom
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21
Q

Electronegative atoms favor…

A

Polar covalent bonds
(E- distribution is polarized ex. Oo)

22
Q

Dipole moment

A

Leans towards more electronegative atom
The larger the difference in electronegativity, between the bonded atoms, the larger the dipole moment

23
Q

Electrostatic / Coulombic

A

Forces between charged particles (ex. Ionic bond)

24
Q

Lattice energy

A

Force of attraction between cations and anions

25
Q

E- affinity

A

Energy change by e- addition

26
Q

Exothermic

A

Energy releasing reactions (-)

Ex. Cl + e- -> Cl-

27
Q

Endothermic

A

Processes that absorb energy to dislodge e- (+)

Ex. Na-> Na+ e-

28
Q

4 bond pairs

A

E- pair arrangement: Tetrahedral
Molecular shape: Tetrahedral

29
Q

2 bond pairs + 2 lone pairs

A

E- pair arrangement: Tetrahedral
Molecular shape: Bent
105

30
Q

3 bond pairs + 1 lone pair

A

E- pair arrangement: Tetrahedral
Molecular shape: Trigonal Pyramidal
107

31
Q

3 bond pairs

A

E- pair arrangement: Trigonal Planar
Molecular shape: Trigonal Planar
120 degrees

32
Q

Methyl group

A

-CH3

33
Q

Methylene group

A

-CH2

34
Q

Methine group

A

-CH

35
Q

Neopentane

A

CH3
CH3-C-CH3
CH3

36
Q

Ethylene

A

H H
\ /
C = C
/ \
H H

37
Q

Acetylene

A

H-C|||C-H

38
Q

Isobutane

A

CH3CHCH3
CH3

39
Q

Isopentane

A

CH3CHCH2CH3
CH3

40
Q

N-butane

A

CH3CH2CH2CH3

41
Q

N-pentane

A

CH3CH2CH2CH2CH3

42
Q

Butyl group (n-butyl)

A

CH3CH2CH2CH3-

43
Q

1-Methylpropyl group (sec-butyl)

A

CH3
CH3CH2CH-

44
Q

2-Methylpropyl group (isobutyl)

A

CH3
CH3CHCH2-

45
Q

1,1-Dimethylethyl group (tert-butyl)

A

CH3
CH3C-
CH3

46
Q

Alkyl groups

A

Remove hydrogen atom from alkane
CH4 - methane, CH3 - methyl

47
Q

Hexyl

A

CH3(CH2)4CH2-

48
Q

Heptyl

A

CH3(CH2)5CH2-

49
Q

Octadecyl

A

CH3(CH2)16CH2-

50
Q

Ethyl group

A

CH3CH2-

51
Q

Propyl group

A

CH3CH2CH2-

Chm 2010 (1 decks)

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