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NEW GEN CHM Flashcards

1
Q

What is the force/energy holding the nucleus together?

A

Nuclear Binding Force

Strong Nuclear Force

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2
Q

Unstable nuclei are radioactive.

What are the rules for stable nuclei?

A
  1. Even # of protons and/or neutrons are stable
  2. N/Z ratio = 1 (for Z<20)
  3. Magic numbers (2, 8, 20)
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3
Q

When do you do:

  1. B-decay (B emission)
  2. B-decay (positron emission)
  3. Electron capture?
A
  1. B-decay (B-emission): N/Z is too high
  2. B-decay (Positron emission): N/Z is too low
  3. Electron capture: N/Z is too low
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4
Q

What element has the highest nuclear binding energy?

A

Fe(56) (iron-56)

  • If you get a question that asks “which of the following has the highest nuclear binding energy?” look for the element that is closest to iron-56
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5
Q

What is the trend for ionic radius?

A

Going down and to the left on the periodic table

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6
Q

What is the trend for 1st ionization energy?

A

Same trend as electronegativity but He is the highest not F

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7
Q

What is the trend for electron affinity?

A

—>Cl

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8
Q

What is the electron domain geometry of:

  • 2e domains and zero non-bonding
A

Linear

Same as 5e domains with 3 non-bonding

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9
Q

What is the electron domain geometry of:

  • 3e domains and zero non-bonding
A

Trigonal planar

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10
Q

What is the electron domain geometry of:

  • 3e domains and 1 non-bonding
A

Bent

same as 4e domains with 2 non-bonding

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11
Q

What is the electron domain geometry of:

  • 4e domains and zero non-bonding
A

Tetrahedral

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12
Q

What is the electron domain geometry of:

  • 4e domains and 1 non-bonding
A

Trigonal pyramidal

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13
Q

What is the electron domain geometry of:

  • 4e domains and 2 non-bonding
A

Bent

same as 3e domains with 1 non-bonding

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14
Q

What is the electron domain geometry of:

  • 5e domains and zero non-bonding
A

Trigonal bipyramidal

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15
Q

What is the electron domain geometry of:

  • 5e domains and 1 non-bonding
A

See-saw

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16
Q

What is the electron domain geometry of:

  • 5e domains and 2 non-bonding
A

T-shaped

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17
Q

What is the electron domain geometry of:

  • 5e domains and 3 non-bonding
A

Linear

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18
Q

What is the electron domain geometry of:

  • 6e domains and zero non-bonding
A

Octahedral

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19
Q

What is the electron domain geometry of:

  • 6e domains and 1 non-bonding
A

Square pyramidal

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20
Q

What is the electron domain geometry of:

  • 6e domains and 2 non-bonding
A

Square planar

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21
Q

Name each of the following: (endothermic or exo?)

  1. solid –> liquid
  2. liquid –> gas
  3. solid –> gas
A
  1. solid –> liquid (melting/fusion)
  2. liquid –> gas (vaporization/boiling)
  3. solid –> gas (sublimation) ie dry ice

ENDOTHERMIC

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22
Q

Name each of the following: (endothermic or exo?)

  1. solid
A
  1. solid
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23
Q

What are the formulas for calorimetry?

A

q = mc(deltaT)

n(delta H)

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24
Q

What is Boyle’s Law?

A

Pressure is inversely proportional to volume

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25
Q

What is Charle’s Law?

A

Temperature and volume are directly proportional

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26
Q

What is Avogadro’s Law?

A

moles and volume are directly proportional

27
Q

What is the formula for Graham’s Law of Effusion?

A

r1/r2 = (M2/M1)^1/2

28
Q

What are the 2 solubility rules?

A
  1. All group 1 metals, NH4, NO3, ClO4 salts are soluble

2. Most Ag+, Pb, and Hg salts are INSOLUBLE

29
Q

What are the Phase Solubility in Liquids Rules?

A
  1. Solids are more soluble at higher temps
  2. Gases are less soluble at higher temps
  3. Gases are more soluble at higher pressures
30
Q

What is the formula for freezing pt. depression?

A

DeltaT = - iKm

31
Q

What is the formula for boiling pt. elevation?

A

DeltaT = iKm

32
Q

What is the formula for osmotic pressure?

A

pie = iMRT

33
Q

When Keq > 1, which way will the equilibrium shift?

A

To the right –> (Products)

34
Q

When Keq < 1, which way will the equilibrium shift?

A

To the left

35
Q

When K > Q, which way will the equilibrium shift?

A

To the right –> (Products)

36
Q

When K < Q, which way will the equilibrium shift?

A

To the left

37
Q

When K = Q, which way will the equilibrium shift?

A

At equilibrium

38
Q

According to Le Chatelier’s Principle, when pressure is increased which way will the equilibrium shift?

A

Least moles

39
Q

According to Le Chatelier’s Principle, when volume is increased which way will the equilibrium shift?

A

most moles

40
Q

When delta-H is negative and delta-S is positive ______________.

A

Spontaneous at ALL temps

41
Q

When delta-H is positive and delta-S is negative ______________.

A

Non-spontaneous at ALL temps

42
Q

When delta-H is positive and delta-S is positive ______________.

A

Spontaneous at HIGH temps

43
Q

When delta-H is negative and delta-S is negative ______________.

A

Spontaneous at LOW temps

44
Q

What is another word for Oxidant?

A

Oxidizing agent

45
Q

What is another word for Reductant?

A

Reducing agent

46
Q

What is the formula for a question that gives you

coulombs or amps?

A

(Amps)(T_s) / (n) (F) = moles product

n = number of electrons
1F = 96,500c
T_s = time in sec
47
Q

Rank these in order of increasing energy/frequency:

  • Cosmic
  • Gamma
  • X-ray
  • UV
  • Infrared
  • Microwave
  • TV
  • Radio waves
A
  1. Cosmic (highest energy/frequency)
  2. Gamma
  3. X-ray
  4. UV
  5. Infrared
  6. Microwave
  7. TV
  8. Radio waves (Lowest energy/frequency)
48
Q

Pollen grains were placed in a liquid. A student noted spontaneous jiggling of these particles. The term that best applies is:

A. Inertia
B. Brownian movement
C. Lysis
D. Diffusion
E. Osmosis
A

B. Brownian movement

Individual particles that appear to vibrate when placed in a liquid is termed brownian movement. The particles are tossed about by constantly moving liquid molecules smashing into them from various directions.

49
Q

What would be the best compound to use on an acid spill in lab?

A. HF
B. NaOH
C. NaHCO3
D. NH4OH
E. KOH
A

C. NaHCO3

  • If you put a strong base it would release a lot of heat
  • Obviously you wouldn’t use another acid
50
Q

What are the 3 assumptions for the Kinetic Molecular Theory?

A

Ideal gas assumptions (2)

  1. Gases have NO volume (only at low pressures)
  2. Gases have no intermolecular forces (only at high temps)
  3. avg kinetic energy is proportional to temperature

“VERY VERY VERY IMPORTANT”

51
Q

What’s the difference between standard conditions and STP?

A

STP is 0 degrees celcius (273 K) and 1atm

52
Q

What are the 3 ideas of the Collision Theory?

A
  1. Collision
  2. Proper orientation
  3. Sufficient energy

At high temps: Collisions increase as well as the percentage of high energy collisions

53
Q

What does increasing the temperature do to the AVERAGE kinetic energy?

A

the AVERAGE kinetic energy increases

54
Q
  1. How is activation energy related to the rate constant?
  2. How is temperature related to the rate constant?
  3. Does increasing the temperature lower the activation energy?
A
  1. activation energy is inversely proportional to the rate constant (k)
    eg. increasing the activation energy will lower the rate
  2. temperature is proportional to the rate constant (k)
    eg. increasing the temp will increase the rate of the rxn
  3. Increasing the temperature does not lower the activation energy of a rxn
55
Q

What is the formula for Rate Laws?

What is the rate law for the following:

2CO2 + O2 –> 3CO2 (elementary rxn)

A

rate = k (reactants)

rate = k [CO2]^2 [O2]

Rate laws ONLY include reactants!!!

56
Q

Which of the following will effect the rate constant (k)?

A. changing the temperature
B. changing the activation energy
C. changing the reactants concentration
D. A and B

A

D. A and B

Changing the temperature or the activation energy changes the rate constant (k) but changing the concentration of the reactants does NOT effect the rate constant (k)

Changing the temperature, activation energy, or concentration of reactants will effect the RATE of the rxn

57
Q

Which of the following will affect the rate constant of a reaction?

A. Reactant concentrations only
B. Catalyst only
C. Temperature only
D. Both a catalyst and temperature
E. Reactant concentrations, a catalyst, and temperature
A

D. Both a catalyst and temperature

58
Q

Why do most reactions proceed more quickly at higher temperatures?

A. Greater number of collisions at higher temperatures
B. A decrease in the activation energy at higher temperatures
C. Greater percentage of high energy collisions at higher temperatures
D. A and C
E. All of the above

A

D. A and C

59
Q

Which of the following will affect the rate of a reaction?

A. Reactant concentrations
B. Catalyst
C. Temperature
D. All of the above

A

D. All of the above

60
Q

What is the difference between an equilibrium constant expression and a rate law?

A

Equilibrium constant expression = Products/reactants (NO solids or liquids)

Rate Law = Reactants only (includes solids)

61
Q

Equilibrium constant expression is also referred to as _________.

A

Mass action ratio

62
Q

If you double the coefficients in a rxn, what does that do to the equilibrium constant? (Keq = 10)

A

Careful!!! it doubles the exponent of Keq

10^2

Coefficients become the exponents of a equilibrium constant expression

63
Q

What is the definition of Le Chatlier’s principle?

A

If a stress is placed on a system, the system will respond to counteract the stress

64
Q

How do you know if you’re doing a formation rxn?

A
  1. rxn can only have ONE mole of products

2. Reactants have to be in their standard states

GEN CHM (3 decks)

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