Brainscape's Knowledge GenomeTM

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


See full index

OAT > General Chemistry > Flashcards

General Chemistry Flashcards

1
Q

Isoelectronic Series

A

Same number of electrons but different number of protons.
Anions: larger radius
Cations: smaller radius

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

Effective Nuclear Charge

A

amount of positive charge experienced by electrons.
Increases as you move right and up.

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

Ionization energy

A

Energy needed to remove an electron from an atom.
Increases as you move right and up.
2nd, 3rd, and 4th ionization energies are increasingly harder.
Exceptions: Group 2>13
Group 15 >16

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

Electron Affinity

A

Amount of energy released when an electron is added.
Increases as you move right and up; noble gases are zero.
Exceptions: Group 4A>5A

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

Electronegativity

A

Ability to draw electrons from other atoms.
Increases as you move right and up.

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

Principal Quantum Number

A

First number in QN, denoted by n.
Gives the main energy level of the electron; must be greater than or equal to 1.

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

Azimuthal Quantum Number

A

Second number in QN, denoted by L.
Describes the orbital shape.
Will be between zero and n-1.
L=0, 1, 2, and 3 are s, p, d, and f, respectively.

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

Magnetic Quantum Number

A

Third number in QN, denoted by ml.
Describes orbital orientation.
Will be between +L and -L.

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

Spin Quantum Number

A

4th number in QN, denoted by ms.
Describes angular momentum.
Will be either +1/2 or -1/2.

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

Pauli’s Exclusion Principle

A

No two electrons in the same atom can have the same Quantum Number.

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

Percent Composition

A

Mass of element in compound/Molar mass of molecule

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

Percent Yield

A

Actual Yield/Theoretical Yield x 100

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

Soluble Salts

A

Group 1 Cations
Acetate
NO3-
ClO4-
NH4+

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

Insoluble Salts

A

Ag+
Pb2+
Hg2+
OH-
S2-
CO3 2-
PO4 3-

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

Strong Acids

A

HCl
HBr
HI
HClO4
HClO3
H2SO4
HNO3

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

Strong Bases

A

Group 1 metal Hydroxides
Ba(OH)2
Sr(OH)2
Ca(OH)2

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

Molarity vs. Molality

A

Molarity: number of moles of solute per one liter of solution.
Molality: number of moles of solute per 1 kg of solvent.

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

Colligative Properties

A

Depend on concentration of solute molecules/ions, but not on identity of the solute.
Vapor pressure depression, boiling point elevation, freezing point depression, osmotic pressure.

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

Non-Colligative Properties

A

Depend on identity of solute and solvent.
Surface tension, color, viscosity, solubility, density.

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

Altitude Effects on Boiling Point

A

BP is when vapor pressure = atmospheric pressure.
At higher elevation, there is less atm pressure, so less vapor pressure is required to reach boiling point, so BP is lower.
Vice versa for lower elevation.

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

Boyle’s Law

A

Pressure and Volume are inversely proportional.

P1 V1 = P2 V2

22
Q

Charles’s Law

A

Volume and Temperature are directly proportional.

V1/T1 = V2/T2

23
Q

Avogadro’s Law

A

Volume and Moles are directly proportional.

V1/n1 = V2/n2

24
Q

Gay-Lussac’s Law

A

Pressure and Temperature are directly proportional.

P1/T1 = P2/T2

25
Q

Ideal Gases

A

Follow 5 Rules:
1) constant random motion
2) combined volume of particles is negligible.
3) particles exert no forces on one another.
4) gas molecule collisions are completely elastic (no IMF).
5) all gases have same avg KE at a given temp.

Gases are ideal at low pressure and high temperature.

26
Q

Effusion

A

Confined gas escaping through a hole.
Lower molecular weight will effuse faster.

27
Q

Phase Diagrams:
Triple Point
Critical Point

A

TP: where all lines meet; substance present in all three phases.
CP: gas and liquid phases are indistinguishable; supercritical fluid.

28
Q

Phase Change Equation

A

q = mH

H = heat of fusion or vaporization.

29
Q

Hess’s Law

A

Total enthalpy change for the reaction is the sum of all changes.

30
Q

Entropy

A

Degree of disorder or randomness.
Higher entropy is favored because is lower in energy and more stable.

31
Q

Laws of Thermodynamics

A

1: Energy can’t be created or destroyed.
2: Entropy of the universe is always increasing.
3: Entropy of a pure crystalline substance at 0 Kelvin is zero.

32
Q

Exergonic vs. Endergonic

A

Ex: energy is released; G<0; spontaneous.
End: energy is absorbed; G>0; nonspontaneous.

33
Q

Factors that Effect Reaction Rate

A

Increase T: increase k, increase rate.
Decrease Ea: increase k, increase rate.
Increasing [reactants]: no effect on k, increases rate.

34
Q

Reactions:
Intermediate
Catalyst

A

I: product then reactant.
C: reactant then product, but not in overall reaction.

35
Q

Acid and Base Definitions:
Arrhenius
Bronsted-Lowry
Lewis

A

A: acids produce H+ in aqueous solution; bases produce OH-.
BL: acids are proton donors, bases are proton acceptors.
L: acids are electron pair acceptors; bases are electron pair donors.

36
Q

Calculating pH and pOH from concentration

A

pH = -log[H+]
pOH = -log[OH-]

37
Q

Types of Salts Produced through Neutralization Reactions

A

Strong Acid + Strong Base = neutral salt.
Strong Acid + Weak Base = acidic salt.
Weak Acid + Strong Base = basic salt.

38
Q

Making Acidic Buffers

A

Weak Acid + Salt (CB) 1:1
Weak Acid + Strong Base 2:1
Salt (CB) + Strong Acid 2:1

39
Q

Making Alkaline Buffers

A

Weak Base + Salt (CA) 1:1
Weak Base + Strong Acid 2:1
Salt (CA) + Strong Base 2:1

40
Q

Equivalence Point
Half Equivalence Point

A

EP: amount of titrant added is just enough to neutralize the analyte solution; steepest part of the curve.
N1V1 = N2V2
HEP: SA + WB or WA + SB. midpoint of the buffering/flat region.
pH=pKa.

41
Q

Equivalence Points in Titrations:
Strong Bases
Strong Acids

A

When involving strong bases and weak acids, the EP will be greater than 7.
When involving strong acids, the EP will be less than 7.
When involving strong acids and strong bases, the EP will be 7.

42
Q

Equilibrium Constant

A

Product concentrations over reactant concentrations.
Keq < 1: greater concentration of reactants at equilibrium.
Keq > 1: greater concentration of products at equilibrium.
Keq = 1: ratio of products and reactants is equal.

43
Q

Reaction Quotient

A

Concentration of reactants and products at any point in the reaction.

Q< Keq: higher reactant concentration than at Eq, proceeds forward.
Q > Keq: higher product concentration than at Keq, proceeds in reverse.
Q = Keq: dynamic equilibrium

44
Q

Compression and Expansion effects on reaction rates

A

Compression: shift to side with fewer gas molecules.
Expansion: shift to side with more gas molecules.

45
Q

Solubility Product Constant

A

Describes extend to which an ionic compound dissolves in water.

Qsp < Ksp: unsaturated
Qsp = Ksp: saturated
Qsp > Ksp: supersaturated

46
Q

Oxidizing Agents vs. Reducing Agents

A

OA: oxidizes other species, gets reduced.
Ex: O2, O3, H2SO4, halogens

RA: reduces other species, gets oxidized.
Ex: H2, Fe, Zn, Alkali metals

47
Q

What happens at anode and cathode of electrochemical cells

A

Anode: oxidation
Cathode: reduction
An Ox and Red Cat
Electrons always flow from anode to cathode.

48
Q

Galvanic/Voltaic Cells vs. Electrolytic Cells

A

G/V: (battery) spontaneous (G<0), converts chemical energy to electrical energy; - anode and +cathode; Ecell>0.

E: (charging battery) nonspontaneous (G>0), converts electrical energy to chemical energy; +anode and -cathode; Ecell<0.

49
Q

Dissociation Constant of Water

A

Kw at room temperature is 1e-14.
For pure water, Ka = Kb.

50
Q

Standard Temperature and Pressure

A

T: 273 K
P: 1 atm
Any 1 mole of gas will have a volume of 22.4 L.

51
Q

What determines Specific Heat Capacity?

A

Strength of intermolecular forces.
Stronger IMF = higher SHC

52
Q

Paramagnetic vs. Diamagnetic

A

P: elements with unpaired electrons; attracted to magnetic field.
D: elements with paired electrons; repelled by magnetic field.

O2: paramagnetic
N2: diamagnetic
F2: diamagnetic

OAT (7 decks)

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