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Org Chem > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

cation

A

positively charge ion

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2
Q

anion

A

negatively charged ion

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3
Q

s orbital

A

sphere; lowest energy (1s < 2s < 3s)

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4
Q

p orbital

A

dumbbell shape, 3 orbitals px, py, pz

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5
Q

Pauli Exclusion principle

A

2 electrons per orbital, opposite spins

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6
Q

2nd shell

A

2s and 2p (8 electrons)

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7
Q

3rd shell

A

3s, 2d, 3p (18 electrons)

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8
Q

covalent bond

A

sharing of valence electrons between two or more atoms

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9
Q

lower energy corresponds to __.

A

greater stability

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10
Q

Shorter bond length corresponds to ___.

A

stronger bonds

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11
Q

non-polar

A

equal sharing of electrons

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12
Q

polar

A

dipole or uneven electronegative and sharing

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13
Q

ionic bond

A

large enough electronegativity that the cation takes electrons from anion - larger than 1.7 (non-metal and metal)

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14
Q

resonance theory

A

more than one lewis structure; differ only in difference in electrons not atoms

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15
Q

resonance hybrid

A

weighted average of all resonance structure; resembles lowest energy structure

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16
Q

Better resonance structures

A

don’t have formal charges, don’t violate the octet, have more bonds, and distribute charges based on electronegativity

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17
Q

rules for line structures

A

carbon atoms are not drawn explicitly, heteroatoms are drawn, bonds to hydrogen are not drawn, zig zag structure and lone pairs aren’t shown

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18
Q

alkanes

A

only single C-H and C-C bonds

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19
Q

reactivity is governed by

A

functional groups

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20
Q

Amino acids (Table 1-7)

A

20 known side chains from protein chains

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21
Q

Carbohydrates

A

only carbon, oxygen, and hydrogen - CxH2yOy

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22
Q

monosacharides

A

same number of oxygen atoms as carbon atoms CxH2xOx - can switch between acyclic and cyclic

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23
Q

nucleic acid

A

DNA and RNA made with nucleotides

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24
Q

Nucleotides

A
  • inorganic phosphate
  • cyclic monosaccharide
  • nitrogenous base
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25
Q

electron geometry

A

arrangement of electrons around an atom

26
Q

molecular geometry

A

arrangement of atoms in a molecule

27
Q

electron group; 2

A

electron geometry; linear (180)
m; linear

28
Q

electron group; 3

A

e geometry; trigonal
m; 2 atoms - trigonal planar (120) or 3 atoms - bent (120)

29
Q

electron group; 4

A

e geometry; tetrahedral
m; 2 atoms - bent (109.5), 3 atoms - trigonal pyramidal (109.5), 4 -atoms; tetrahedral

30
Q

wedge

A

towards you

31
Q

dash

A

away from you

32
Q

polar bonds, dipoles cancel

A

non-polar molecule

33
Q

polar bonds, dipoles don’t cancel

A

polar molecule

34
Q

non-polar bonds

A

non-polar molecule

35
Q

ion-ion

A

strongest because of high concentration of negative and positive charge

36
Q

dipole-dipole

A

partial changes - much weaker than ion-ion so lower mp and bp

37
Q

hydrogen bonding -concept

A

requires hydrogen bond donor and acceptor (donors; high electronegative - H) (acceptor - any atom with large negative charge and lone pair)

38
Q

Hydrogen bonding

A

weaker than ion-ion; sometimes stronger that diople-dipole
- depends on
- number of possible acceptors and donors
- concentration of charges

39
Q

Induced dipole

A

London dispersion
instantaneous dipole for non-polar molecules induces dipoles of others
generally the weakest of all the intermolecular forces
- strength determined by polarizability (# of electrons)
- more surface area = stronger as well and higher bp, mp

40
Q

ion-dipole

A

ions break up and the separate ions and interact with dipoles.
- between ion-ion and dipole-dipole in strength

41
Q

melting point ________ the intermolecular interactions in solids

A

decreases

42
Q

boiling point _______ the intermolecular forces in liquids

A

overcomes the remaining

43
Q

melting point increases as ________ increases

A

intermolecular forces in a solid

44
Q

boiling point increases as ________ increases

A

intermolecular forces in a liquid

45
Q

entropy

A

thermodynamic quantity increases with disorder, encourages mixing of substances

46
Q

Solubility

A

ability to break bonds so it goes stronger IMB to lower IMB

46
Q

Solubility

A

ability to break bonds so it goes stronger IMB to lower IMB

47
Q

Steric Hindrance

A

bond strength hindered by shape of molecule

48
Q

protic solvent

A

has H-Bond donor - easily accessible partial charges

49
Q

aprotic solvent

A

has no H-bond donor - non easily accessible charges

50
Q

Valence Bond Theory

A

A covalent bond forms when two half valence orbitals from two separate atoms overlap
- overlapping orbitals mix to create a new orbital
- new orbital accomodates bonding electrons allowing them to be shared

51
Q

Sigma Bond

A

single bond along the bonding axis

52
Q

any atom that has ______ electron geometry is sp3 hybridized

A

tetrahedral (25% s, 75% p)

53
Q

any atom that has ______ electron geometry is sp2 hybridized

A

trigonal planar (33.3% s, 67.7% p) one unhybridized p orbital

54
Q

Pi bond

A

bond on opposite sides of the bonding axis

55
Q

liner electron geometry =

A

sp hybridization with two sp orbitals and 2 p orbitals

56
Q

free rotation

A

around single bonds

57
Q

cis

A

same side

58
Q

trans

A

opposite

59
Q

hybridization goes down bonds are? why?

A

shorter and stronger more s characteristic

60
Q

hybridization goes down
EFFECTIVE electronegativity

A

increases

61
Q

quantum mechanics

A

wave-particle duality

Org Chem (3 decks)

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