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OAT General Chemistry > Concepts > Flashcards

Concepts Flashcards

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1
Q

Bohr Model

A

A hydrogen atom consists of a central proton around which an electron travels in a circular orbit, centripetal force, and electrical force, electrons can only exist in fixed-energy states

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2
Q

Heisenberg Uncertainty Principle

A

Impossible to simultaneously determine the momentum and the position of an electron

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3
Q

Pauli Exclusion Principle

A

No two electrons in a given atom can possess the same four quantum numbers

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4
Q

Principal Quantum Number

A

n, represents the shell where an electron is present in an atom, the element’s row (N -> 1,2)

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5
Q

Quantum Numbers

A

n, l, ml, ms

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6
Q

Magnetic Quantum Number

A

ml, the orientation of the orbital in space (i.e. p subshell (-1,0,+1)

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7
Q

Spin Quantum Number

A

ms, spin of a particle up or down, (+1/2, -1/2)

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8
Q

Paired Electron

A

Electrons with opposite spins, different ms, but the same ml

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9
Q

Aufbau Principle

A

Subshells are filled from lowest to highest energy

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10
Q

Phase Diagram

A

Right (Gas), Left (Solid), Middle (Liquid), Critical Point (Top of l/g)

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11
Q

Hund’s Rule

A

Electrons prefer empty orbitals to half-filled ones

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12
Q

Raoult’s Law

A

Vapor pressure of a pure solvent is equal to the product of the mole fraction of the solvent and the vapor pressure of the solvent

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13
Q

Paramagnetic

A

A material has unpaired electrons, the magnetic field will align the spins

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14
Q

Boyle’s Law

A

P1V1 = P2V2

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15
Q

Charles Law

A

V1/T1 = V2/T2

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16
Q

Nuclear Effective (Zeff)

A

Net positive charge from the nucleus as felt by an electron, max at top right of PT

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17
Q

Ionization Energy

A

The energy required to remove an electron from an atom, max at top right PT

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18
Q

Atomic Radius Trend

A

Decreases up/right, Largest Bottom Left, Smallest Top Right

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19
Q

Electronegativity Trend

A

Increasing Up/Right, Highest Top Right

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20
Q

Soluble Salts

A

SO4-2, Cl-, Br-, I-, NH4+, Alkali metals

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21
Q

Insoluble Salts

A

Metal oxides, hydroxides, salts with CO3-2, PO4-3, SO3-2

22
Q

Combination Reactions

A

Two or more reactants form one product

23
Q

Decomposition Reactions

A

A compound breaks down into two or more substances (electrolysis

24
Q

Spectator Ions

A

Ions do not take part in the chemical reaction

25
Q

Double-Displacement Reaction

A

Elements from two different compounds displace each other to form two new compounds

26
Q

Oxidation Electrode

A

Anode

27
Q

Reduction Electrode

A

Cathode

28
Q

Electrolytic Cell

A

Nonspontaneous, electrical energy required, same container, no salt bridge, presence of a battery or power source used to drive nonspontaneous reactions

29
Q

Lewis Acid

A

Electron-pair acceptor

30
Q

Lewis Base

A

Electron-pair donor

31
Q

Bronsted Acid

A

Donates protons

32
Q

Bronsted Base

A

Accepts Protons

33
Q

Alpha Decay

A

A-4, Z-2

34
Q

Beta (-) Decay

A

A, Z+1

35
Q

Gamma Decay

A

No change, emission of gamma particle (high-energy photon)

36
Q

Electron Capture

A

A, Z-1 (add e-)

37
Q

Le Chetelier’s Principle

A

Stress on an environment:
1. Concentration -> shift to relieve pressure
2. Pressure -> shift decrease moles
3. Temperature -> heat as a product/reactant

38
Q

Bond-Dissociation

A

Energy required to break a specific chemical bond in one mole of a gaseous molecule, bond breaking is endothermic

39
Q

Titrations

A
  1. Strong acid/base of known concentration
  2. Titrate added in small amounts
  3. Neutral = equivalents equal
  4. SB/SA -> pH 7
  5. SB/WA -> above pH 7
  6. WB/SA -> below pH 7
40
Q

Nerst Equation

A

Potential under non-standard conditions

41
Q

Galvanic Cell

A

Supply energy, used to do work, separate containers for oxidation and reduction half-reactions, connected by an apparatus, allow flow of electrons

42
Q

Angular Momentum Quantum Number

A

l, the shape of the orbitals (0(s),1(p), 2(d), 3(f))

43
Q

Isobaric

A

Constant pressure

44
Q

Isochoric

A

Constant volume

45
Q

Isothermal

A

No temperature change

46
Q

Adiabatic

A

No heat exchange

47
Q

Deposition

A

Gas to solid

48
Q

Sublimation

A

Solid to gas

49
Q

Avogadro’s Principle

A

n1/V1 = n2/V2

50
Q

Ideal Gas Law

A

PV = nRT

51
Q

Beta (+) Decay

A

A, Z-1

OAT General Chemistry (1 decks)

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