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MCAT - Kaplan > Gen Chem > Flashcards

Gen Chem Flashcards

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MCAT flashcards
1
Q

A first order rate law can be identified by the presence of _

A

One reactant

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2
Q

A second order rate law can be identified by the presence of __

A

Two Reactants

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3
Q

How would you sequentially determine the rate law for a multi-step mechanism?

A

Look at reactant 1 and see if there are any related changes in rate. Then look at reactant 2 and see if there are any related changes in rate

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4
Q

Trigonal Planar geometry uses ___ angles and the planar geometry allows for __ stabilization.

A

120 degree ; resonance

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5
Q

Trigonal pyramidal geometry leads to __ bond angles which are __ degrees.

A

distorted ; <120

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6
Q

The sigmoidal shape of an oxyhemoglobin dissociation curve is due to __ binding and eventual __.

A

Cooperative ; Saturation

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7
Q

Carbon monoxide poisoning results in a left shift. This is because CO increases __ binding affinity. As a result, saturation occurs quicker as CO results in fewer available __.

A

O2 ; bind sites

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8
Q

Cooperative Binding

A

When something (i.e. Oxygen) is bound to a subunit subsequently its affinity for additional i.e. oxygen increases and it can bond more readily to additional i.e. oxygen.

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9
Q

If concentration is __ than solubility than a precipitate will form

A

greater than

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10
Q

If concentration is __ to solubility then it can be considered as saturated.

A

=

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11
Q

If concentration is __ solubility then it can be considered unsaturated.

A

less than

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12
Q

Ideal gases have 1) __ molecular volume 2) ___ intermolecular forces and 3) their Kinetic Energy is proportional to __.

A

negligible ; negligible ; temperature

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13
Q

Liquids are incompressible, however, __ can be compressed.

A

Gases

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14
Q

In order for an object to float the density of the object must be __ than that of the fluid. If it was to sink then the density of the object must be __ than that of the fluid.

A

less ; greater

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15
Q

The electron configuration can be determined by the ___.

A

Atomic number ( then + or - any charges)

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16
Q

The maximum number of electrons in an atomic energy level is __

A

2n^2

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17
Q

The maximum number of electrons in a subshell is __

A

4l+ 2

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18
Q

According to the Heisenberg Uncertainty Principle we are unable to measure position and momentum both __ and __. This is due to an error in one variable as we attempt to measure the other.

A

exactly ; simultaneously

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19
Q

The atomic number indicates the ___.

A

Number of protons (A in A/Z)

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20
Q

The atomic weight is the ___ of isotopes. It is also the amount, in grams, for 1 mole.

A

average

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21
Q

The atomic mass is the mass number. This means that it indicates the number of __ and __.

A

Protons and Neutrons (note: # protons = # electrons if atom is neutral)

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22
Q

Charge is determined by __

A

electrons

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23
Q

Atomic number is determined by __

A

protons

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24
Q

Isotopes are determined by __.

A

Neutrons

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25
Q

Planck’s equation measures ___. Its formula includes planck’s constant and frequency __.

A

Energy ; E= hf

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26
Q

As the principal quantum number (n) increases the energy of the electron becomes less __ .

A

negative

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27
Q

The energy of a photon can be measured using what equation:

A

E = hc / wavelength

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28
Q

When n=1 (lower) goes to n=3 (higher) what occurs?

A

AHED (Absorb Light ; Higher Potential energy ; Excited ; Distant from Nucleus)

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29
Q

According to Pauli’s exclusion principle ___

A

No two electrons in a given atom can be described by quantum numbers (n, l, ml, ms) that are exactly the same

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30
Q

The angular momentum (l) is limited by the ___. It determines the shape and number of subshells.

A

Principle quantum number (n)

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31
Q

Magnetic Quantum number (ml) specifies __ and ranges between __.

A

the orbital within a subshell ; - l to + l including 0

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32
Q

Spin Quantum number (ms) can either be ___ or ___.

A

+ 1/2 or -1/2

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33
Q

If electrons are paired that means they are in the __ orbital with __ spins.

A

same ; opposite

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34
Q

If the electrons are parallel than they are in __ orbitals with ___ spins.

A

different ; same

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35
Q

Aufbau Principle suggests the following rule for filling shells and subshells__

A

N+ 1

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36
Q

If something is paramagnetic that means it is __ magnet and has all __ electrons.

A

attracted to ; unpaired

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37
Q

If something is diamagnetic that means it is __ magnet and has all __ electrons.

A

repelled from ; paired

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38
Q

Atomic radius __ left to right. It __ top to bottom.

A

decreases; increases

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39
Q

Ionic radius is bigger in __ than neutral atoms and is smaller in ___.

A

anions ; cations

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40
Q

Ionization energy ___ left to right. It __ top to bottom.

A

increases ; decreases

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41
Q

Electron affinity ___ left to right. It __ top to bottom.

A

increases; decreases

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42
Q

Electronegativity __ left to right. It __ top to bottom.

A

Increases ; Decreases

43
Q

The oxidation number of a ion is equal to __. It describes the degree of oxidation.

A

the charge of the ion

44
Q

Intramolecular bonding is “within” and examples include __ which have strong electrostatic attraction & electronegativity differences and __ which have weak electrostatic attraction and moderate electronegativity differences .

A

ionic ; polar covalent

45
Q

Intramolecular bonding also includes ___ which is when electrons in a bond come from one atom and __ which has neutral atoms, negligible electrostatic attraction and a small electronegativity difference.

A

coordinate covalent ; covalent

46
Q

In terms of intramolecular strength rank the following: covalent, polar covalent, ionic

A

Ionic > Polar Covalent > Covalent (based on electrostatic attraction)

47
Q

In terms of intermolecular strength rank the following: dipole-dipole, dispersion, ion-dipole, hydrogen bonding.

A

Ion Dipole > Hydrogen Bonding > Dipole- Dipole > Dispersion

48
Q

Hydrogen bonding requires N O or F and is a ___ interaction.

A

very strong dipole

49
Q

Ion-dipole involves strong electrostatic attraction, fully charged ions and __.

A

solvation

50
Q

Ionic bonds form between __ ions. Polar covalent bonds form between atoms with ___ .

A

fully charged ; different electronegativity

51
Q

Coordinate covalent bonds occur when the electrons come from __ . Covalent bonds form between atoms of ___.

A

a single atom ; similar electronegativities

52
Q

Tetrahedral Electronic Geometry (Associated Groups, Hybridization and Bond Angles)

A

4;Sp3; 109.5

53
Q

Trigonal Planar (Associated Groups, Hybridization and Bond Angles)

A

3; sp2; 120

54
Q

Trigonal bipyramidal (Associated Groups, Hybridization and Bond Angles)

A

5; sp3d; 90,120,180

55
Q

Charge is determined by the number of __

A

Electrons

56
Q

Atomic number is determined by the number of __

A

Protons

57
Q

Isotopes have the same atomic number but different __ due to a difference in the number of neutrons.

A

Mass Number

58
Q

E=hf where h is planck’s constant and f is frequency in J*s.

A

Planck’s equation for determining energy

59
Q

L= nh/ 2pi where h is planck’s number and n is the principal quantum number measures

A

Angular momentum

60
Q

E= -Rh/ n^2 where RH = 2.18 x 10^-18 J and the __ changes as n changes.

A

Energy of the electron

61
Q

The equation for the electromagnetic energy of a PHOTON.

A

E= hc / wavelength

62
Q

If we go from n=1 as the lower initial energy level to n=3 a higher final energy level what can we expect to happen?

A

Absorption of light, higher potential, excited, distant from nucleus

63
Q

The maximum number of electrons in a shell can be described as __

A

2n^2

64
Q

If two electrons are said to be PAIRED what does this mean about their orbital and spin?

A

They have the same orbital but are opposite spins

65
Q

If two electrons are said to be PARALLEL what does this mean about their orbital and spin?

A

They are in different orbitals but have the same spins

66
Q

The maximum number of electrons in the subshell can be defined by the equation 4l+2. This means that which quantum number limits the number of electrons within a subshell?

A

l which is the angular momentum

67
Q

According to Pauli’s exclusion principle what is true of 2 electrons in a given atom ?

A

No 2 electrons can be described with the exact same quantum mechanical numbers

68
Q

If it is said to be paramagnetic what does that mean for the electrons?

A

Attracted to magnet and all unpaired electrons

69
Q

If it is said to be diamagnetic what does that mean for the electrons?

A

Repelled from magnet and all paired electrons

70
Q

Effective Nuclear Charge (Zeff) __ left to right and __ from top to bottom.

A

increases ; increases

71
Q

Atomic radius __ left to right and __ top to bottom.

A

Decreases; Increases

72
Q

deltaG < 0

Q < Keq

A

forward reaction occurs

73
Q

deltaG > 0

Q > Keq

A

reverse reaction occurs

74
Q

deltaG = 0

Q =Keq

A

dynamic equilibrium- forward and reverse still occuring

equilibrium is reached when entropy is at its maximum and free energy is at its minimum

75
Q

Calculate Keq

A

I Products I / I ReactantsI

76
Q

Law of Mass Action

Keq >1

A

more products

77
Q

Law of Mass Action

Keq ~ 1

A

equal amount of products and reactants

78
Q

Law of Mass Action

Keq <1

A

more reactants

79
Q

Law of Mass Action

Keq «<1

A

negligible in comparison to initial concentration

80
Q

In one direction it is written as Keq, the equilibrium constant for the reverse reaction is written as __

A

1/ Keq

81
Q

If a reactant is added or a product is removed what impact would this difference in concentration have __

A

Qc < Keq
Forward
Up QC until equilibrium

82
Q

If a reactant is removed or a product is added what impact would this difference in concentration have __

A

Qc > Keq
Reverse
Qc until equilibrium

83
Q

If a reaction undergoes compression (volume down, pressure up) the reaction moves in the direction with __

A

less moles of gas

84
Q

If a reaction undergoes expansion (volume up, pressure down) then it moves in the direction of __

A

more moles of gas

85
Q

If a reaction is endothermic then dH>0 and heat is _

A

a reactant

86
Q

Temperature does not change Qc or Qp but it does effect

A

Keq

87
Q

If a reaction is exothermic then dH<0 and heat is _

A

a product

88
Q

If temperature increases in endothermic conditions or temperature decreases in exothermic conditions the reaction will shift to the __

A

right

89
Q

If temperature decreases in endothermic conditions or temperature increases in exothermic conditions the reaction will shift to the __

A

left

90
Q

The kinetic product is easier to reach the transition state. It is higher in __ __ , forms quicker and can form at __ temperatures

A

free energy ; low

91
Q

The thermodynamic product is more slow and stable. It is __ in free energy and is high in heat transfer. It is spontaneous which means that deltaG is __.

A

lower ; negative

92
Q

What does not appear in the equilibrium constant (Keq) equation?

A

pure solids and pure liquids

93
Q

Collision Theory

A

rate proportion to number of collisions / second

94
Q

Arrhenius Equation

A

as the frequency factor Ea increases the rate constant (k) increases
if T increases, the exponent becomes less negative (smaller) and constant (k) increases
Ea can be increased by increasing the number of molecules in the vessel

95
Q

Transition State Theory

A

+ deltaG endergonic : energy absorbed
- deltaG exergonic: energy given off
Ea can be lowered without deltaG

96
Q

Reaction Rates: Concentration

A

increased concentration:

increase collisions, increase freq. factor, increased rate except 0 order reactions

97
Q

Reaction Rates: Temperature

A

incr. rate ; incr. KE

98
Q

Reaction Rates: Change in Medium

A

aqueous / non aqueous
physical state
polar/nonpolar

99
Q

Reaction Rates: Catalysts

A

homogenous: same phase
heterogenous: different phase
lower Ea no change in Keq
does not transform nonspontaneous to spontaneous

100
Q

Zero Order Rate law

A

constant rate not dependent on concentration of reactant
changes only be change in Temp or catalyst
conc. v time linear ; slope = -k
rate = k[A]^0 [B]^0

101
Q

First Order Rate Law

A

nonconstant rate and dependent on concentration of reactant
conc. v time nonlinear ; slope ln[A] = -k
rate = k[A]^1 or rate = k[B]^1

102
Q

Second Order Rate Law

A

nonconstant rate and dependent on concentration of reactant
conc. v time nonlinear ; slope 1/[A] = k
rate = k[A]^1 [B]^1 or rate = k[A]^2 or rate = k[B]^2

103
Q

Broken Order Reaction

A

noninteger orders

104
Q

Mixed Order Reaction

A

rate order changes over time

MCAT - Kaplan (6 decks)

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