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CHM 142B Dr. Mark Cybulski > Exam 3 > Flashcards

Exam 3 Flashcards

1
Q

Lewis acid

A

accepts a pair of electrons, compounds with less than an octet around the central atom can and metal ions act as lewis acids, negatively charged

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2
Q

Lewis base

A

donates a pair of electrons

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3
Q

coordinate bond

A

a covalent bond formed when one anion/molecule donates a pair of electrons to another ion/molecule

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4
Q

ligand

A

a lewis base bonded to the central metal ion of a complex ion

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5
Q

complex ion

A

ionic species consisting of a metal ion bonded to one or more lewis bases

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6
Q

formation constant (Kf)

A

an equilibrium constant describing the formation of a metal complex from a free metal ion and its ligands

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7
Q

Trend with acid strength and cation charge

A

direct

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8
Q

Nonamphoteric hydroxides

A
  1. Fe(OH)3
  2. Fe(OH)2
  3. Cu(OH)2
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9
Q

Amphoteric hydroxides

A
  1. Al(OH)3
  2. Pb(OH)2
  3. Sn(OH)2
  4. Be(OH)2
  5. Zn(OH)2
  6. Cd(OH)2
  7. Cr(OH)3
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10
Q

how do common ions affect solubility?

A

common ions decrease solubility, but don’t affect the solubility product constant

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11
Q

How do uncommon ions affect solubility?

A

the increase solubility

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12
Q

when can you neglect s?

A

when it is <0.01

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13
Q

Affect of pH on salt solubility

A

acidity increases the solubility of salts with basic anions due to shift in equilibrium reactions, weaker acids increases solubility more

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14
Q

Q and Ksp relationship and effects

A

Q>Ksp, precipitate forms

Q

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15
Q

reversible process formula

A

△S=qrev / T

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16
Q

Second law of thermodynamics

A

Irreversible: △Suniverse=△Ssurroundings+△Ssystem>0

Reversible: △Suniverse=△Ssurroundings+△Ssystem> or = 0

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17
Q

Standard molar entropy trends

A

Gases and molecules with the highest molar mass have the highest molar entropies. Entropy increases as the complexity of the molecular structure increases

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18
Q

Which △G values indicate spontaneity in which direction?

A

△G<0: spontaneous in forward direction

△G>0: spontaneous in reverse direction

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19
Q

△Grxn equation

A

△Grxn=△Gºrxn + RTln(Q)

20
Q

Relationship between △G◦ and K

A

indirect

21
Q

van’t hoff equation

A

ln(k1/k2)=△Hº/R(1/T2 - 1/T1)

22
Q

bolts,amm equation

A

s=kb x ln(w)

23
Q

Anode

A

electrode at which the oxidation half reaction takes place

24
Q

Cathode

A

electrode at which reduction half-reaction takes place

25
Q

△H and △S when a rxn is spontaneous at lower temperatures

A

both are negative

26
Q

△H and △S when aren is spontaneous at higher temperatures

A

both are positive

27
Q

△H and △S when a rxn is always spontaneous

A

negative △H and positive △S

28
Q

△H and △S when a rxn is never spontaneous

A

positive △H and negative △S

29
Q

Standard reductio potential

A

(Eºred), the voltage for a reduction reaction at an electrode when all solutes have activities=1 and gases=1 bar

30
Q

Standard oxidation potential

A

(Eºox) equal in magnitude but opposite in sign to Eºred

31
Q

Eºcell formulas

A

ºEcell=Eºred(cathode)-Eºred(anode)=Eºred(cathode)+Eºox(anode)

32
Q

What do standard reduction potentials tell you about their strengths as agents?

A

Higher positive value=stronger oxidizing agents and lower negative value = stronger reducing agents

33
Q

Spotaneity of reduction potentials

A

higher=more spontaneous

lower=nonspontaneous

34
Q

work formula

A

wmax=-QEcell=△G=nFEcell
w=work in joules
Q=total charge that passes through a cell

35
Q

what does emf stand for

A

electrical potential

36
Q

nernst equation forms with and without temperature

A

With T: Ecell=Eºcell - RT/nF ∙ lnQ

Without T: Ecell=Eºcell - 0.0592/n ∙ logQ

37
Q

primary battery

A

cannot be recharged

38
Q

secondary battery

A

can be recharged

39
Q

Faraday law of electrolysis

A

m = aM/nF= aM/nF I t

a/n= coefficients
Q=charge
I=current
t=time

40
Q

Current variable and units

A

Variable: I
Units: A

41
Q

corrosion

A

process in which metals react with oxidizing agents resulting in the formation of other compounds

42
Q

sacrificial anode

A

aka cathodic protection, a metal with a lower reduction potential making iron the the cathode

43
Q

ekectrolysis

A

process in which electrical energy causes a nonspontaneous reaction to occur. Oxidiation is at anode, reduction is at cathode, signs of electrodes are reversed, cathode is negative and anode is positive

44
Q

Where do cations and anions migrate to in battery cells?

A

cations to cathode, anions to anode

45
Q

How is the mass of each electrode affected in a battery?

A

Anode doesn’t always lose mass because of gases, cathode always gains mass

46
Q

Sigma bonds

A
  1. end to end overlap of orbitals
  2. s-s, s-p, or p-p orbitals
  3. stronger
  4. one symmetrical electron cloud symmetrical to internuclear axis
47
Q

Pi bonds

A
  1. lateral overlap of orbitals
  2. p-p orbitals only
  3. weak bond
  4. electron is not symmetrical and lies above nuclear plane

CHM 142B Dr. Mark Cybulski (4 decks)

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