Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

MCAT by TD :) > Chemistry MCAT > Flashcards

Chemistry MCAT Flashcards

You may prefer our related Brainscape-certified flashcards:
MCAT flashcards
1
Q

Plank constant

A

6.63 x 10^(-34) m^2kg/s or Js

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Speed of light in vacuum

A

3 x 10^(8) m/s

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Avogadro’s number

A

1 mole = 6.022 x 10^(23) atoms or molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

To calculate energy of electromagnetic radiation

A

E = hf = hc/wavelength

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Rydberg constant

A

R = 2.18 x 10^(-18) J
Or
R = 1.097 x 10^7 m^-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Calculate energy of the emitted/ absorbed photon when electron is moved between energy level n

A

Delta E = (Rydberg constant) x (1/n_final^2 - 1/n_initial^2)

Delta E < 0 : E is released, electron moves from higher to lower energy level

Delta E > 0 : E is absorbed, electron moves from lower to a higher energy level

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Michaelis-Menten equation

A

Enzyme kinetics
How reaction rate (v) changes when substrate concentration [S] changes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Lineweaver - Burk plots

A

Enzyme kinetics
Double-reciprocal transformation of Michaelis-Menten plot

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Oxidation

A

Loss of electrons
Increased oxidation state
More C-O/ C-N bonds
Less C-H bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Reduction

A

Gain electrons
Decreased oxidation state
Less C-O / C-N bonds
More C-H bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

OIL RIG

A

Oxidation is Loss of electrons
Reduction is Gain of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Reduction of alkene

A

Hydrogenation of alkene. This is reduction because new C-H bonds are formed.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Oxidation of alkene

A

New C-O bonds are formed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Calculate the heat q at phase change

A

Unit: J, kJ, cal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Calculate heat q between phase change (related to temperature change!)

A

Unit: J, kJ, cal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Volume of 1 mole of any gas at STP (T = O celcius, p = 1 atm)

A

1 mol = 22.4 L

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Avogadro’s law

A

V1/ n1 = V2/ n2

Assume T and p are constant.
V and n are directly proportional to each other.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Kinetic molecular theory (Ideal Gases)

A
  1. Gas particles are in continuous, random motion
  2. Avg kinetic energy of gas particles is directly proportional to temperature; all gas particles will have the same kinetic energy at a given T.
    Avg KE = (3/2)kT
  3. (*) Gas particles have no volume (negligible volume compared to their container)
  4. (*) Gas particles do not interact with each other (no attraction/ repulsion). Pressure of gas comes from collision btw gas particles and wall of container.
  5. All gas particle collisions are elastic; the overall kinetic energy is conserved.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Conditions favor ideal gas behavior

A

High T
Low pressure
Large volume

Any conditions favoring the formation of liquid make the gas deviate from ideal behavior.
Molecules with polar bonds exert more attractive force with each other -> less likely to behave like ideal gas.

20
Q

Boyle’s Law

A

Volume and pressure of a gas are inversely proportional at constant T.

P1V1 = P2V2

21
Q

Charles’s law

A

V1 / T1 = V2 / T2

Volume and temperature of a gas are directly proportional under constant pressure and mole of gas.

22
Q

Gay-Lussac’s Law

A

P1 / T1 = P2 / T2

Assume constant volume and number of moles, pressure of gas is proportional to its temperature.

23
Q

Ideal Gas Law

A

PV = nRT

R = 0.08 L.atm/K.mol
or
R = 8.314 J / K.mol

24
Q

Van der Waals equation (for real gas)

A
25
Q

Compare pressure of real gas vs. ideal gas under STP (T = 273K or OoC; p = 1 atm)

A

Under STP, real gas has a smaller pressure compared to an ideal gas.

26
Q

Compare pressure of real gas vs. ideal gas at extreme pressure (container of small V)

A

Real gas has higher pressure than ideal gas because size of gas particle (b value) is no longer negligible. When the V of container is too small, the gas particles press against the wall more often, and the bigger particles increase pressure against the wall.

27
Q

Compare pressure of real vs. ideal gas at low T.

A

Real gas has lower pressure compared to ideal gas at low T.

28
Q

Dalton’s Law

A

The total pressure of a mixture of gases equals the sum of the partial pressure of its components.

29
Q

Graham’s Law of diffusion (gases)

A

When a gas is effusing (escaping from a small opening), the smaller, lighter particles escape faster.

30
Q

IR peak values for some types of bonds

A
31
Q

Calculate the number of stereoisomers

A

2^n
n = the number of chiral centers

32
Q

What is a chiral center?

A

Chiral center is a tetrahedral atom with 4 different groups / substituents bonded to the atom so that the compound cannot be superimposed on its own mirror image.

33
Q

VSEPR theory

A
34
Q

Relation btw Km and affinity of enzyme

A

Km is the concentration of substrate at which point the enzyme achieves half Vmax.
Higher Km value indicates that enzyme has lower affinity for its substrate because it requires a greater substrate concentration to achieve Vmax.

35
Q

T/F
Phase changes from solid -> liquid -> gas are endothermic reactions.

A

True
Because gas contains more heat energy than liquid, and liquid contains more heat E than solid.

36
Q

T/ F
Phase changes from gas to liquid to solid are endothermic.

A

False.
Gas -> Liquid -> Solid are exothermic (release heat).

37
Q

Some common strong acids and bases

A
38
Q

Effective nuclear charge (Zeff)

A

The actual attractive force of the positively-charged nucleus on the atom’s valence electrons.

39
Q

Symbol of atom (atomic number Z and atomic mass A)

A
40
Q

T/F
There is increase in the avg kinetic energy, so there is an increase in entropy (S)

A

True

41
Q

T/F
Electrons in orbitals that are more spatially compact are held more tightly to the positively charged nucleus. Therefore, the ionization energy is predicted to be higher.

A

True

42
Q

Relationship btw delta(G) and reduction potential Ecell

A
43
Q

Is alcohol more polar than aldehyde/ ketone?

A

Yes, alcohol is more polar than aldehyde and ketone due to its ability to donatebhydrogen bond.

44
Q

Is silica gel polar or nonpolar?

A

Silica gel is polar

45
Q

Coordinate covalent bond

A

A covalent bond in which both electrons come from the same atom.

Ex: Lewis acid w/ Lewis base
Metal cation w/ an electron pair donor

46
Q

How to determine the relative thermodynamic stability of isomers?

A

Based in the amount of heat produced when the compound is combusted.
Less heat, greater stability

MCAT by TD :) (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions