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MCAT EK Review > Chemistry & Organic Chemistry > Flashcards

Chemistry & Organic Chemistry Flashcards

1
Q

Changing the number of neutrons creates (ion/isotope/different element); changing the number of electrons create (ion/isotope/different element); changing the number of protons creates (ion/isotope/different element).

A
  • change neutrons=isotope
  • change electrons=ion
  • change protons=different element
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2
Q

energy needed to detach an electron from an atom

A

ionization energy

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3
Q

tendency of an atom to attract electrons shared in covalent bond

A

electronegativity

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4
Q

willingness of an atom to accept an additional electron

A

electron affinity

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5
Q

1st quantum number

A

(principal) shell level of electron (n)-energy level

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6
Q

2nd quantum number

A 
(azimuthal)- subshell- shape
s=0
p=1
d=2
f=3
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7
Q

3rd quantum number

A 
(magnetic) orbital (holds 2 e) ranging from -l to +l
s=2
p=8
d=18
f=32
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8
Q

4th quantum number

A

electronic spin number (+/-1/2)

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9
Q

Heinsenberg Uncertainty Principle

A
  • production of position or a particle

- momentum

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10
Q

Difference between empirical and molecular formula

A
  • empirical-smallest ratio of whole numbers used to represent proportions
  • molecular formula-exact number of elemental atoms in each molecule
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11
Q

Radioactive decay follows which order of kinetics?

A

1st order

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12
Q

Which type of decay occurs when a neutron becomes a proton

A

beta decay

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13
Q

When a proton becomes a neutron, electron is absorbed

A

electron capture

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14
Q

When a proton becomes a neutron, positron is emitted

A

positron emission

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15
Q

formal charge equation

A

formal charge= (#valence electrons)-(#bonds)-(#nonbonding electrons)

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16
Q

(T/F) Sigma bonds have the lowest energy and are the strongest type of bond.

A

true

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17
Q

Enantiomers have the same chemical and physical characteristics except for two cases.

A
  • interactions with other chiral compounds

- interactions with polarized light

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18
Q

(Cis/trans) have stronger intermolecular forces

A

Cis

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19
Q

Atoms with a greater number of electron shells (higher periods of periodic table) distribute charges and make good (leaving groups/nucleophiles)

A

leaving groups

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20
Q

(T/F) Nitrogen is more nucleophilic than oxygen

A

true

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21
Q

best nucleophiles are strong (acids/bases) and the best leaving groups are weak (acids/bases)

A

nucleophile-strong base

leaving group-weak base

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22
Q

Aldehyde and ketones undergo addition not substitution producing what type of product?

A

racemic mixtures

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23
Q

chain of glucose

A

amylose (starch)

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24
Q

Saturated or unsaturated fats have a lower melting point

A

unsaturated fats

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25
Q

average kinetic energy for a mole of molecules in fluid equation

A

KE= 3/2*RT

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26
Q

Which two variables allow for the transfer of energy between systems?

A

heat and work

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27
Q

0th law of thermodynamics

A
  • 2 systems in thermal equilibrium with a 3rd system are in thermal equilibrium with each other
  • temperature exists and is a state function
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28
Q

1st law of thermodynamics

A

-Total energy of the system and surroundings is always conserved: E=q-w

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29
Q

equation for enthalpy

A

internal energy + work (H=U + P*V)

30
Q

2nd law of thermodynamics

A

entropy of an isolated system will never decrease

31
Q

3rd law of thermodynamics

A

a perfect crystal at 0 K is assigned an entropy value of 0

32
Q

heat capacity equation

A

heat capacity= heat/temperature (C=Q/T)

33
Q

Bond breaking is (endothermic/exothermic) and bond formation is (endothermic/exothermic)

A
  • bond breaking-endothermic

- bond formation-exothermic

34
Q

When does a compound evaporate?

A

When vapor pressure of liquid phase is greater than the partial pressure of the gaseous phase

35
Q

When does boiling occur?

A

When the vapor pressure of liquid equals the atmospheric pressure

36
Q

crystallization is (endo/exo) thermic?

A

exothermic

37
Q

function of galvanic cell

A

turn chemical energy into electrical energy

38
Q

current flows from (anode/cathode) to (anode/cathode)

A

cathode to anode (opposite of electrons)

39
Q

When the pH is lower than the pKs, a species interprets the environment as (protic/aprotic) and is less likely to act (acidic/basic)

A

-protic and acts less acidic

40
Q

difference between heat and temperature

A

heat-amount of energy transferred due to change in temperature
temperature-average kinetic energy of molecules

41
Q

(T/F) Ionic compounds have higher melting and boiling points over hydrogen bonds

A

true

42
Q

What order is a saturated enzyme?

A

0th order

43
Q

Units of the rate law:

  • 0th
  • 1st
  • 2nd
A
  • 0th: (m/s)
  • 1st: (1/s)
  • 2nd: (1/ms)
44
Q

In a gas, as temperature goes up what happens to the solubility?

A

solubility decreases

45
Q

SN1 reaction creates (racemic/enantiomers)

A

racemic mixture (no longer optically active)

46
Q

How can you increase SN1 reactions?

A
  • highly substituted carbons (tertiary carbon)
  • polar (protic) solvent
  • weak base for leaving group
47
Q

How can you increase SN2 reactions?

A
  • attack primary carbons
  • nonpolar (aprotic) solvent
  • lots of nucleophiles
48
Q

How does gas chromatography separate compounds?

A

by boiling point and polarity

49
Q

galvanic cell vs electrolytic

A

galvanic- spontaneous, exergonic chemical reaction

electrolytic- non-spontaneous, endergonic chemical reaction (decomposition process)

50
Q

relation between boiling point and vapor pressure

A

inverse: lower BP= higher vapor pressure

51
Q

What type of bond do transition metals make?

A

coordinate covalent

52
Q

More solute particles present, the (lower/higher) the vapor pressure, and the (lower/higher) the boiling point

A

more solute particles present, the (lower) the vapor pressure, and the (higher) the boiling point

53
Q

△G < 0, Keq > 1, and E° > 0

A

spontaneous

54
Q

In reactions with gases, (increasing/decreasing) the volume, will shift the equilibrium to the side with more moles of gas (and vice versa)

A

increasing (decreasing pressure)

55
Q

purpose of salt bridge

A

balance growing positive charge in the anode and negative charge in the cathode; keep the electrochemical reaction from reaching equilibrium too quickly

56
Q

electrolytic cell: anode (+/-) and cathode (+/-)

galvanic cell: anode (+/-) and cathode (+/-)

A

electrolytic: anode (+) and cathode (-)
galvanic: anode (-) and cathode (+) (Spontaneous)

57
Q

Noble gases have very (low/high) melting and boiling points

A

low- inert gases

58
Q

What mechanism opens glucose’s ring structure?

A

hydrolysis (hydration)

59
Q

buffer

A
  • weak acid and conjugate base

- weak base and conjugate acid

60
Q

order of reactivity in nucleophilic addition-elimination reactions for acid derivatives

A

acid anhydrides > esters > amides

61
Q

specific activity

A
  • purity of an enzymatic mixture

- specific activity is equal to the activity of an enzyme per milligram of total protein in the mixture

62
Q

If Q < K

A

reaction is spontaneous in the direction written (shift right)

63
Q

An increase in pressure or decrease in volume will result in what shift for gas molecules?

A
  • An increase in pressure or decrease in volume will result in a shift to the side with fewer moles of gas
  • Conversely, an decrease in pressure or increase in volume will result in a shift in to the side with more moles of gas
64
Q

BH3 selectively reduces which molecule to primary alcohols?

A

carboxylic acids

65
Q

stereoisomers

A

2^n (n=stereocenters)

66
Q

Nucleophile vs leaving group

A

nucleophile- strong base and electron donor

leaving group- weak base and accept electrons

67
Q

increase boiling point

A

strong intermolecular forces and greater surface area (less branching)

68
Q

When do precipitates occur?

A

exceeds the solubility product constant (Q> Ksp)

69
Q

equilibrium constant

A

ΔG′° = –RTln(Keq)

70
Q

Henderson-Hasselbach equation

A

pH = pKa + log([base]/[acid])

71
Q

backside attack and 1 product

A

SN2

72
Q

planar carbocation and form 2 products

A

SN1

MCAT EK Review (5 decks)

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