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chem 24 > quiz 1 > Flashcards

quiz 1 Flashcards

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1
Q

what is the formal charge formal

A

FC= #valence e - 1/2 shared - unshared

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2
Q

When does a hydrogen have a neutral charge?

A

1 bond

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3
Q

when does a carbon have a neutral charge

A

4 bonds

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4
Q

when does a carbon become a carbocation

A

when it has 3 bonds

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5
Q

When is nitrogen neutral

A

3 bonds 1 lone pair

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6
Q

when does nitrogen have a +1

A

4 bonds

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7
Q

when is oxygen neutral

A

2 bonds 2 lone pairs (divalent)

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8
Q

when is oxygen +1

A

when it has 3 bonds and one lone pair

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9
Q

when is oxygen -1

A

when it has 1 bond and 3 lone pairs

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10
Q

what is the mass #

A

protons +neutrons

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11
Q

when are halogens neutral

A

with one bond and 3 lone pairs (monovalent)

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12
Q

what are atoms of the same element with different numbers of neutrons called?

A

isotopes

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13
Q

what is the mass # representative of?

A

the average masses of the naturally occurring isotopes

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14
Q

what is aufau principle?

what is poly exclusion principle?

what is hund’s rule?

A
  1. building up in orbitals (1s–> 2s—-2p—-)
  2. only two electrons per oribital with opposite spins
  3. if you have empty orbitals of same energy level, fill them with one e at a time with parallel spins
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15
Q

what are isomers

A

same molecular formula, different structure, different properties

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16
Q

what are resonance structures

A

electrons from π orbitals can shift, forming resonance structures of the same compound

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17
Q

what are the rules of resonance

A
  1. only real lewis structures
  2. hybrids are real, resonance structures are imaginary,
  3. only electrons move, not atoms
  4. the resonance hybrid is more stable
  5. a resonance structure is more stable with complete octets and delocalized charge
  6. resonance structures with the lowest FC’s are more stable
  7. more covalent bonds are lower in energy and more stable
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18
Q

carbon can be

A

electron rich or poor since it can be more or less electronegative than the atom its bonding to

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19
Q

what determines a bond’s polarity

A

unequal sharing on electrons

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20
Q

when is a structure tetrahedral

A

4 e groups, no lone pairs, 109.5

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21
Q

when is a structure linear

A

2 e groups, no lone pairs, 180

22
Q

when is a structure trigonal planar

A

3 e groups, no lone pairs, 120

23
Q

How do you identify the °Carbon?

A

1° Primary, 2° Secondary, 3° tertiary, 4° quaternary carbons are defined by the number of carbon atoms attached to the carbon analyzed

24
Q

How do you identify the °carbo cation?

A

carbocations are defined by the number of carbons attached to the carbocation

25
Q

How do you identify the °alcohol? or alkyl Halid

A

by the number of carbons attached to the carbon that the hydroxyl group is attached to

26
Q

How do you identify the °amine/amide?

A

the number of carbons directly attached to the nitrogen

27
Q

what makes a resonance structure more stable/ major contributing

A
  • delocalization of charge
  • lowest FC
  • negative charge is on the most EN atom
  • octet rule is fulfilled for the most amount of atoms
  • highest # of covalent bonds
28
Q

what are branched alkyl groups?

A

constitutional isomers of alkyl groups

29
Q

whats the shortened name of isobutyl

A

i-Bu

30
Q

whats the shortened name of sec butyl

A

sec-Bu

31
Q

whats the shorted name of tert butyl

A

tert-bu

32
Q

whats the shortened name of isopropyl

A

i-pr

33
Q

what are the IMF’s by strength?

A

Ion-Ion, Dipole Dipole, H-Bonds, Dispersion Forces

34
Q

What are ion ion forces

A

they are attractions between opposite charges

35
Q

what are dip dip forces

A

interactions between dipoles

36
Q

what is H bonding

A

interactions that occur when Hydrogen is bonded to an electronegative atom (FON)

37
Q

what are dispersion forces

A

temporary distributions in partial charges that cause weak attractions

38
Q

what causes a molecule with dispersion forces to have a higher boiling point?

A

increased surface area (straight chains > branched chains)

39
Q

What is the stretch of a C=O bond

A

1700 cm^-1

40
Q

what is the stretch of a C-H bond

A

2900 cm^-1

41
Q

what is the stretch of a C(≡)C

A

2100 cm^-1

42
Q

what is the stretch of O-H

A

3500 cm^-1

43
Q

for a primary amine, how many peaks are possible? (NH2)

A

two, due to the symmetric and asymmetry bond stretches

44
Q

for a secondary amine, how many peaks are possible? (NH)

A

one

45
Q

what is a bronsted lowry acid

A

proton donor

46
Q

what is a bronsted lowry base

A

proton acceptor

47
Q

what is a lewis acid

A

e pair acceptor

48
Q

what is a lewis base

A

e pair donor

49
Q

a high Ka indicates what?

A

stronger acid

50
Q

a low pka means what?

A

stronger acid

51
Q

the strongest acid will have the

A

weakest base

52
Q
A

chem 24 (22 decks)

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