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D1 Fall > Chemical Bonding, Water, Acid-Base Balance (1-2) > Flashcards

Chemical Bonding, Water, Acid-Base Balance (1-2) Flashcards

1
Q

6 atoms in covalent bonds

A

C, H, O, N, P, S

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2
Q

valence

A

of bonds, determines what structures form

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3
Q

electronegativity

A

tendency to attract electrons, determines how molecules interact with each other

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4
Q

geometry

A

bond angle, determines shape of molecules

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5
Q

covalent bond

A

a pair of electrons shared by 2 atoms

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6
Q

double bond

A

2 atoms share 2 pairs of electrons

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7
Q

delocalization

A

sharing of electrons, lowers energy

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8
Q

lower energy =

A

greater stability, bond strength

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9
Q

valence of H

A

1

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10
Q

valence of C

A

4

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11
Q

valence of O

A

2

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12
Q

valence of N

A

3

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13
Q

valence of S

A

2

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14
Q

valence of P

A

5

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15
Q

rank electronegativity

A

O>N>S=C>H=P

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16
Q

more electronegative atoms attract

A

electrons more strongly

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17
Q

less electronegative atoms attract

A

electrons less strongly

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18
Q

covalent bonds can be

A

polar or nonpolar

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19
Q

ions do not form

A

covalent bonds

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20
Q

ions form

A

electrostatic bonds with oppositely charged molecules

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21
Q

tetrahedral shape

A

CH4, NH3-, H2O

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22
Q

double bonds structure

A

flat planar structure

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23
Q

single bonds rotate

A

freely around single bonds

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24
Q

double bonds rotate

A

they do no rotate

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25
Q

which atoms have nonbonded electron pairs

A

O, N, S

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26
Q

N in NH3 has a tendency to

A

capture H+

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27
Q

O atom of a water molecule can accept both electrons from an OH bond and

A

release the hydrogen

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28
Q

acid is a H+

A

donor

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29
Q

base is an H+

A

acceptor

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30
Q

electron resonance

A

sharing of electrons by 3 or more atoms

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31
Q

what is the most stable structure of phosphoric acid

A

PO4H-2

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32
Q

most of the enrgy yielded by ATP hydrolysis comes from

A

additional resonance stabilization of ADP

33
Q

Carbon-oxygen groups

A

alcohol, aldehyde, ketone, carboxylic acid, ether, acid anhydride

34
Q

carbon-sulfur groups

A

sulfhydryl group, disulfide

35
Q

carbon-nitrogen groups

A

amino group, quaternary amine

36
Q

which groups are made up in a pyruvic acid

A

carboxyl, keto, methyl

37
Q

pyruvic acid modifications

A

decarboxylation, carboxylation, amino transfer, reduction

38
Q

non-covalent bonds

A

hydrogen bonds, electrostatic bonds, hydrophobic bonds, Van der Waals forces

39
Q

hydrogen bonds

A

attractive force between H atom in polar covalent bond and unpaired electrons of electronegative atoms

40
Q

strength of H bonds is dependent on

A

distance and orientation

41
Q

electrostatic bonds

A

attractive forces between + and - charged atoms

42
Q

strength of electrostatic bonds depends on

A

distance

43
Q

hydrophobic bonds

A

in water, water molecules push nonpolar molecules together

44
Q

rank bonds in terms of strength

A

covalent> H bonds> electrostatic bonds> hydrophobic bonds> Van der Waals

45
Q

OH bonds in water are

A

polar

46
Q

water is

A

-good solvent for polar molecules and ions

47
Q

what is insoluble in water

A

non-polar molecules

48
Q

Hydrogen bonds forms between

A

O and N atoms
H atoms in polar bonds

49
Q

water is a

A

charged dipole

50
Q

amphipathic molecules

A

partly polar and partly nonpolar
fatty acids, phospholipids

51
Q

fatty acids have

A

polar head, non-polar tail

52
Q

fatty acids packed into a spherical structure in water

A

micelle

53
Q

phospholipids have

A

a polar head and 2 non-polar tails

54
Q

in water phospholipids form

A

flat sheets and form spontaneously

55
Q

water weakens

A

hydrogen bonds and ionic bonds

56
Q

water creates

A

hydrophobic bonds

57
Q

acid is a

A

proton donor

58
Q

base is a

A

proton acceptor

59
Q

strong acids

A

dissociate completely
equilibrium very far right

60
Q

weak acids and bases

A

exist in equilibrium with their conjugate species

61
Q

molecule is an acid if

A

the uncharged form of a molecule is a proton donor (COOH)

62
Q

molecule is a base if

A

the uncharged form of a molecule is a proton acceptor (NH2)

63
Q

water can act as a

A

acid or base

64
Q

in pure water

A

[H3O+] = [OH-]

65
Q

pH equation

A

pH = log[H+]

66
Q

higher [H+] pushes equilibrium

A

left

67
Q

lower [H+] pulls equilibrium to the

A

right

68
Q

small changes in [H+] have a

A

big effect on protein molecules

69
Q

denaturation

A

caused by changes in protonation

70
Q

Ka =

A

acid dissociation constant

71
Q

Ka equation

A

Ka = [H+][A]/[HA]

72
Q

Henderson- Hasselbach equations

A

pH = pKa + log [A]/[HA]

73
Q

when pH = pKa

A

half of A is unprotonated, other half is unprotonated

74
Q

proton exchanges between acids and bases are

A

spontaneous that occur rapidly

75
Q

a substance can add to a buffer if

A

it reacts with added H+ or OH- to get rid of some of the added OH/H

76
Q

buffers are

A

weak acids or bases

77
Q

when do buffers work well

A

when their pH is near their pKa

78
Q

most important physiological buffer

A

bicarbonate

79
Q

what generates acidity in the body

A

metabolism

D1 Fall (14 decks)

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