Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

MCAT Prep > General Chemistry > Flashcards

General Chemistry Flashcards

(84 cards)

Start Studying
1
Q

Principle quantum number

A

(n) – larger the value = higher energy level and radius of electron shell
max # of e- in a shell = 2n^2

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

Azimuthal Quantum number

A 
(l) angular momentum 
l=0 --- s
l=1 --- p
l=2 --- d
l=3 --- f
max # of electrons within subshell = 4l + 2
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Hund’s Rule

A

within electron sub shell, e- will only begin pairing up once all orbitals are half-filled

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

Paragmagnetic

A

unpaired e- orient to align with magnetic field

–meaning that a magnetic field will cause parallel spins in unpaired electrons and cause an attraction

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

Diamagnetic

A

paired electrons will be slightly repelled by a magnetic field

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

Ionization Energies (Periodic Table)

A

Increasing moving to the right and up

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

Electron Affinity (Periodic Table)

A

Increasing moving to the right and up (just like ionization energy)

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

Atomic and Ionic Radii (Periodic Table)

A

increases moving to the left and down

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

Alkali Metals (Periodic Table)

A

Group 1

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

Alkaline Earth Metals (Periodic Table)

A

Group 2

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

Halogens (Periodic Table)

A

Group 17

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

Noble Gases (Periodic Table)

A

Group 18

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

Stable with incomplete octet (5)

A 
Hydrogen H (2)
Helium He (2) 
Lithium Li (2)
Beryllium Be (4)
Boron B (6)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Stable with expanded octet

A 
elements in group 3 (or greater)
Phosphorus P (10) 
Sulfur S (12)
Chlorine Cl (14)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Ionic Bonds

A

one low ionization with atom of high electron affinity
typically between metal (become cation) and nonmetal (becomes anion)
Physical properties:
very high melting and boiling points
dissolved readily in water and other polar solvents
great conductors

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

covalent bonding

A

e- pair shared between 2 atoms, how they are shared determines polarity
Typically between two metals
Physical Properties:
weak intermolecular interactions
tend to have lower boiling and melting points

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

Coordinate Covalent Bonds

A

both shared e- originate from the same atom

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

Lewis Acid

A

any compound that will accept lone pair of e

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

lewis Base

A

any compound that will donate a lone pair of e

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

electronic vs. molecular geometry

A

electronic: spatial arrangement of electron pairs around central atom
molecular: spatial arrangement of only bonding pairs (coordination # determines molecular geometry)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Intermolecular Forces (weakest to strongest) 3

A

Dispersion forces then dipole-dipole interactions then H bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Dispersion Forces

A

attractive and repulsive interactions (rapidly)

Important key element for why noble gases can liquify

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Dipole-Dipole interactions

A

oppositely charged ends orient to be closer together

longer duration of attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Hydrogen Bonding

A

strong
no sharing or transferring of electrons (no actual bond)
Only exists in HIGHLY electronegative atoms
high boiling points

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Combination Reactions
2 or more reactants form 1 product
26
Decomposition Reactions
one reactant forms 2 or more products | usually due to heating, high freq. radiation, electrolysis
27
Combustion reaction
``` involves oxidation (hydrocarbon fuels, or S, or sugars) products: CO2, H2O is almost always present ```
28
Single Displacement Reaction
1 atom or ion in a compound is replaced with another | RedOx Rxns
29
Double Displacement Reaction
elements of 2 compounds swap to form 2 new compounds
30
Neutralization Reactions
type of double displacement | acid reacts with base to produce a salt
31
Three types of systems
isolated, closed, open
32
Isolated System
cannot exchange energy (heat or work) OR matter with surroundings
33
Closed System
can exchange energy (heat or work), but NOT matter with surroundings
34
Open System
Can exchange BOTH energy (heat and work) and matter with surroundings
35
First law of thermodynamics
deltaU = Q - W
36
Four types of Processes
Isothermal Process Adiabatic Process Isobaric Process Isovolumetric Process
37
Isothermal Process
system's temperature is constant = U is constant U is constant (deltaU=0) Q = W
38
Adiabatic Process
no heat exchange, thermal energy is constant Temperature is not held constant Q = 0, deltaU = -W
39
Isobaric Process
Pressure is held constant
40
Isovolumetric Process
(Isochoric Process) Volume is constant, no work is being done deltaU = Q
41
State Functions
P, density, T, V, enthalpy (H), Internal energy (U), Gibbs Free Energy (G), Entropy (S) independent of path taken, but they relate to eachother
42
standard conditions versus standard Temperature and Pressure
Standard conditions = 25C (298K), I atm P, I [M] = used for kinetics, equilibrium, and thermodynamics STP = 0C (273K), I atm P = used for ideal gas calculations
43
deltaQ > 0
Endothermic Reaction
44
deltaQ < 0
Exothermic Reaction
45
Bond formation (endothermic or exothermic?)
Exothermic process
46
Bond dissociation (endothermic or exothermic?)
Endothermic Process
47
Solvation
"Dissolution" | breaking of intermolecular interactions between solute molecules and solvent molecules to form new interactions together
48
Solvation: Exothermic reaction
when new interactions are STRONGER than original ones | Favored at low temperature
49
Solvation: Endothermic reaction
when new interactions are WEAKER than original ones | favorite at high temperatures
50
Solvation: Ideal Solution
when overall strengths between original and new interactions are approximately equal
51
Two prominent solubility rules
1. All salts with ammonium (NH4+) and alkali metals (group 1) cations are water soluble 2. All salts with nitrate (NO3-) and acetate (CH3COO-) anions are water soluble
52
Ion Product (IP)
allows you to determine where the system is with respect to equilibrium position
53
IP < Ksp
not at equilibrium "unsaturated" Dissolution is thermodynamically favored
54
IP > Ksp
Beyond equilibrium "supersaturated" Thermodynamically unstable
55
IP = Ksp
at equilibrium saturated solution "molar solubility"
56
Kf constant
formation/stability constant | significantly larger than Ksp
57
Ka constant
acid dissociation constant =Products/Reactants =higher value is a weaker acid (higher dissociation in more reactive acids)
58
Kb constant
base dissociation constant | similarly to Ka
59
Q < Keq , deltaG < 0
reaction proceeds in the forward direction
60
Q = Keq , deltaG = 0
reaction @ dynamic equilibrium
61
Q > Keq , deltaG > 0
reaction proceeds in the reverse direction
62
Le Chatelier's Principle
3 main types of stress | Concentration, pressure/volume, temperature
63
Le Chatelier's Principle: increase [R], decrease [P]
increase [R], decrease [P] = shift reaction to the right | vice versa will shift to the left
64
Le Chatelier's Principle: increase P, decrease V
increase P, decrease V = shift in direction of fewer mols of gas vice versa will shift towards more mols of gas
65
Le Chatelier's Principle: increasing/decreasing T of Endothermic Reaction
increasing T will shift rxn to the right | decreasing T will shift rxn to the left
66
Le Chatelier's Principle: increasing/decreasing T of Exothermic Reaction
increasing T will shift rxn to the left | decreasing T will shift rxn to the right
67
Strong Bases
NaOH Sodium Hydroxide | KOH Potassium Hydroxide
68
Strong Acids
``` HCl: hydrochloric acid HBr: hydrobromic acid HI: hydroiodic acid H2SO4: sulfuric acid HNO3: nitric acid HClO4: perchloric acid ```
69
Electrochemical Cells
- any cell with red-ox reactions - anode: site of oxidation - cathode: site of reduction - e flow anode to cathode - current flows cathode to anode
70
Galvanic (voltaic) Cell
-spontaneous reaction (deltaG<0) w/ positive electromotive force -anode (-) charge -cathode (+) charge (electromotive force (+) and deltaG (-) )
71
Electrolytic Cells
-nonspontaneous reactions (deltaG>0) w/ negative electromotive force -anode (+) charge -cathode (-) charge (electromotive force (-) and deltaG (+) )
72
3 type of rechargeable battery cell systems
1. lead-acid battery 2. nickel-cadmium batteries 3. nickel-metal hydride (NiMH)
73
Lead-Acid battery
discharging: Pb anode and PbO2 cathode concentrated in H2SO4 charging: PbSO4- electrodes are dissociated to restore original Pb and PbO2 electrodes - low energy density
74
Nickel-Cadmium Battery
discharging: Cd anode, NiO(OH) cathode in concentrated KOH charging: Ni(OH)2 and Cd(OH)2 electrodes are dissociated - high energy density than lead-acid
75
Nickel-Metal Hydride Battery
-replaced Ni-Cd batteries -higher energy density surge content: above average content @ start of discharge phase
76
concentration cell
specialized galvanic cell -both electrodes are made of the same material -concentration gradient causes movement of charge (electromotive force (0) and deltaG (0) )
77
relationship between electromotive force and Keq constant
Keq > 1 = E cell is + Keq < 1 = E cell is - Keq = 1 = E cell is 0
78
Pauli Exclusion Principle
no 2 e- can possess the same set of 4 quantum numbers
79
Aufbau Principle
e- will fill lower energy orbitals before filling higher energy orbitals
80
Pauli Exclusion Principle
no 2 e- can possess the same set of 4 quantum numbers
81
Aufbau Principle
e- will fill lower energy orbitals before filling higher energy orbitals
82
Nucleophiles
negative charge long pairs of e- or pi bonds amino groups are common
83
Electrophiles
positive charge | alcohols, aldehydes, ketones, carboxylic acids
84
Oxidation of: primary alcohol aldehyde secondary alcohol
primary = aldehyde, or carboxylic acid aldehyde = carboxylic acid secondary alcohol = ketone (tertiary alcohol cannot be oxidized)

MCAT Prep (11 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions