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Kaplan MCAT Quick Sheets > Chemistry > Flashcards

Chemistry Flashcards

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MCAT flashcards
1
Q

Electron Configuration (Periodic Table)

A

S,P,D,F

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2
Q

Polar Covalent Bond

A

Bonding electron pair is not equally shared.

Pull toward more electronegative atom

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3
Q

Geometry of molecules

A 
Regions of electron density
2=linear, 180
3=bent,120
4=tetrahedral,109.5
5=trigonal bipyrimidal, 90,120,180
6=octahedral, 90,180
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4
Q

Intermolecular Forces

A

Hydrogen bonding
Dipole-Dipole Interactions
Dispersion Forces

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5
Q

Hydrogen Bonding

A

The partial positive charge of hydrogen atom interacts with partial negative charge located on electronegative atoms (F,O,N) of nearby molecules

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6
Q

Dipole-Dipole

A

Polar molecules orient themselves so that the positive region of one molecule is close to the negative region of another molecule

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7
Q

Isothermal Process

A

Temperature of system remains constant

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8
Q

Adiabatic Process

A

No heat exchange occurs

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9
Q

Isobaric Process

A

Pressure of system remains constant

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10
Q

Isovolumetric(Isochoric)

A

Volume remains constant

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11
Q

Heat

A

Transfer of thermal energy from one object to another

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12
Q

Endothermic

A

Reactions that absorb thermal energy

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13
Q

Exothermic

A

Reactions that release thermal energy

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14
Q

Enthalpy (H)

A

Used to express heat changes at constant pressure

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15
Q

Standard heat of formation

A

Delta Hf
The enthalpy change that would occur if one mole of a compound was formed directly from its elements in their standard states

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16
Q

Standard heat of reaction

A

Delta Hrxn
Hypothetical enthalpy change that would occur if the reaction were carried out under standard conditions

=Sum of Delta Hf of products - Sum of Delta Hf reactants

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17
Q

Hess’s Law

A

Enthalpies of reactions are additive

Reverse of any reaction has an enthalpy of same magnitude as forward reaction, but with opposite sign

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18
Q

Bond Dissociation Energy

A

Average of the energy required to break a particular type of bond in one mole of gaseous molecules

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19
Q

Bond Enthalpy

A

Standard heat of reaction can be calculated using bond dissociation energies of particular bonds (given from table)

Delta Hrxn= Sum Delta H bonds broken - Sum Delta H bonds formed

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20
Q

Entropy (S)

A

Measure of distribution of energy throughout a system

Delta S= Delta Ssystem + Delta Ssurroundings

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21
Q

Gibbs Free Energy (G)

A

Combines 2 factors that affect the spontaneity of a reaction. Changes in enthalpy and entropy

Detla G= Delta H-T Delta S

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22
Q

If G is negative the reaction is

A

Spontaneous

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23
Q

If G is positive the reaction is

A

Non-Spontaneous

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24
Q

If G=0 the reaction is

A

At equilibrium and Delta H=T delta S

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25
Q

At a moderately high pressure a gasses volume is…

A

less than would be predicted by ideal gas law due to intermolecular attraction

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26
Q

Boyles Law

A

k=PV or P1V1=P2V2

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27
Q

Charles Law

A

k=V/T or V1/T1=V2/T2

28
Q

Gay-Lussac;s Law

A

k=P/T or P1/T1=P2/T2

29
Q

Combined Gas Law

A

P1V1/T1=P2V2/T2

30
Q

Ideal gas law

A

PV=nRT

31
Q

Arrhenius Definition

A

An acid is a species that produces excess H+ in an aqueous solution and a base is a species that produces extra OH-

32
Q

Bronsted Lowry Definition

A

An acid is a species that donates protons while a base is a species that accepts protons

33
Q

Lewis Definition

A

An acid is an electron pair acceptor and a base is an electron pair donor

34
Q

pH=?

A

pH=-log[H] = log(1/[H+]

35
Q

pOH=?

A

pOH=-log[OH] = log(1/[OH-])

36
Q

Kw=?

A

Kw=[H+][OH-] = 10^-14

37
Q

pH+pOH=?

A

pH+pOH= 14

38
Q

Ka=?

A

[H3O+][A-]/[HA]

39
Q

Kb=?

A

[B+][OH-]/[BOH]

40
Q

Salt Formation

A

Acids and bases may react with each other, forming a salt and often water in a neutralization reaction

HA+BOH—>BA+H2O

41
Q

Hydrolysis

A

The reverse reaction where salt ions react with water to give back the acid and the base

42
Q

Amphoteric Species

A

One that can act either as an acid or base depending on its chemical environment

43
Q

Henderson-Hasselback Equation

A

pH=pKa+log[conjugate base]/[weak acid]

pOH=pKb+log[conjugate acid]/[weak base]

44
Q

Oxidation

A

Loss of electrons
Fewer Bonds to Hydrogen
More bonds to heteroatoms (O,N, halogens)
Typically goes from OH to O

45
Q

Reduction

A

Gain of electrons
More Bonds to Hydrogen
Fewer bonds to heteroatoms
Typically goes from O to OH

46
Q

Oxidizing Agent

A

Causes another atom to undergo oxidation and is itself reduced
High affinity for electrons (O2, O3, Cl2)

47
Q

Reducing Agent

A

Causes another atom to be reduce and is itself oxidized
Good reducing agents include sodium, magnesium, aluminum, and zinc
Low electronegativities and ionization energies

48
Q

Gibbs free energy in electrolytic cells

A

Delta G= -nFEcell

Ecell=electromotive force

49
Q

Nucleophile

A

Nucleus Loving

Tend to have lone pairs or pi bonds that can form new bonds to electrophile

50
Q

Electrophile

A

Electron Loving

Tend to have a positive charge or positively polarized atom that accepts an electron pair form a nucleophile

51
Q

Enantiomers

A

Non-superimposible mirror images
Have opposite stereochemistry at every chiral carbon
Same chemical and physical properties

52
Q

Diastereomers

A

Non mirror image stereoisomers

Have different chemical and physical properties

53
Q

Thin Layer Chromatography (Use, Mobile and Stationary Phase)

A

Identify a sample
Mobile Phase: Nonpolar solvent
Stationary Phase: Polar solvent

54
Q

Reverse Pahse (Use, Mobile and Stationary)

A

Identify a sample
Mobile Phase: Polar solvent
Stationary Phase: Nonpolar solvent

55
Q

Column Chromatography

A

Separates a sample into components
Mobile: Nonpolar solvent
Stationary: Polar gel or powder

56
Q

Ion Exchange Chromatography

A

Separates components by charge
Mobile: Nonpolar solvent
Stationary: Charged beads in column

57
Q

Size Exclusion Chromatography

A

Separate Components by size
Mobile: Nonpolar solvent
Stationary: Polar, porous beads in column

58
Q

Affinity Column

A

Purify a molecule of interest
Mobile: Nonpolar solvent
Stationary: Bead coated with antibody or receptor for target molecule

59
Q

Gas Chromatography

A

Separate vaporizable compounds
Mobile: Inert Gas
Stationary: Crushed metal or polymer

60
Q

High Performance liquid chromatography (HPLC)

A

Similar to column but more precise
Mobile: Nonpolar solvent
Stationary: Small column with concentration gradient

61
Q

IR Spectroscopy

A

Measures Molecular vibrations of characteristic functional groups

62
Q

Power equation

A

P=W/delta t

Work/ change in time

63
Q

Total Mechanical Energy equation

A

E=U+K

potential energy+kinetic energy

64
Q

Power by resistors

A

P=IV
V^2/R
I^2R

65
Q

Conjugate Acid

A

Formed when a proton is added to a base

H20–>H3O

66
Q

Conjugate Base

A

Formed when a proton is removed from an acid

H2PO4–>HPO4

Kaplan MCAT Quick Sheets (9 decks)

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