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Chem 102 > Final > Flashcards

Final Flashcards

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1
Q

What electronic configurations lead to stable entities?

A

Fully filled, half filled and fully empty

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2
Q

Coordination bond

A

Chemical bonds that occur with the ligand donating two electrons to the metal

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3
Q

Monodentate

A

One bond (one electron pair)

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4
Q

Constitutional Isomers

A

Isomers that have different atomic connectivity

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5
Q

Coordination Isomers

A

Isomers that have different ligand connectivity

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6
Q

Linkage Isomers

A

Isomers that have different attachment of ligand

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7
Q

Isomers

A

Entities with the same chemical formula but different bonding and different properties

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8
Q

Stereoisomers

A

Isomers that have the same connectivity but different arrangement of atoms

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9
Q

Ligand Field Theory

A

The application of molecular orbital theory to transition metal complexes

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10
Q

Octahedral Complexes

A

The ligands interact directly with the d(x2-y2) and d(z2) orbitals

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11
Q

Tetrahedral Complexes

A

The ligands interact more with the d(xy) d(xz) and d(yz) orbitals

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12
Q

Spectrochemical Series

A

The order of splitting by ligands

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13
Q

Heat (q)

A

Energy transferred from a hotter to a cooler body

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14
Q

Work (w)

A

The product of force and distance

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15
Q

Energy

A

The capacity to do work

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16
Q

Kinetic Energy

A

The energy of motion

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17
Q

Potential Energy

A

The capability to do work as a result of position, condition or composition

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18
Q

Standard Reaction Conditions

A

Exist when reactions occur during pure substances, 1 mol/L substances, approx 1 bar partial pressure

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19
Q

State

A

The specific conditions relating to a system: temperature, pressure, concentration etc.

20
Q

State Function

A

Any property that has a unique value at a specific state

- a property of a system that is independent of the path taken to arrive at a specified state

21
Q

Internal Energy (U or E)

A

The total kinetic and potential energy within an entity

22
Q

Heat Capacity (C)

A

The heat required to change the temperature of one gram/mole of an entity by one kelvin.

23
Q

Enthalpy (H)

A

The heat evolved from a reaction at a constant external pressure

24
Q

Hess’s Law

A

States that the change in reaction enthalpy is independent of the path taken between reactants and products

25
Q

Standard Formation Enthalpy

A

The enthalpy for the creation of one mole of an entity from elements in their standard state

26
Q

Calorimeter

A

Measures the heat of reaction

27
Q

Spontaneous Process

A

A process that occurs if left to itself

28
Q

Non-spontaneous Process

A

Process that will not occur unless external energy is input

29
Q

Second Law of Thermodynamics

A

All spontaneous processes increase the entropy of the universe

30
Q

Gibbs Free Energy

A

The maximum work that can be extracted from a system and still have a spontaneous process at a constant pressure and temperature.

31
Q

Formation Gibbs Free Energy

A

The change in free energy involved in the creation of one mole of an entity from elements in their standard state

32
Q

Phase Transitions

A

A class of chemical reaction where the enthalpy and entropy of the products and reactants are tabulated at 298K, yet the reaction occurs far from 298K.

33
Q

Galvanic/voltaic cells

A

Proceed spontaneously; Largest Ecell tends to occur

34
Q

Electrolytic cell

A

Does not proceed spontaneously; smallest Ecell tends to occur

35
Q

Cell Diagram

A

A convenient way to represent the chemistry occurring in an electrochemical cell

36
Q

Active electrodes

A

Take part in the chemistry

37
Q

Inert electrodes

A

Provide electrical connectivity but do not take part in the chemistry

38
Q

Primary Cells

A

Produce electricity from chemical reactions that cannot be reversed; are not rechargeable

39
Q

Secondary Cells

A

Produce electricity from chemical reactions that can be reversed by putting electricity into the cell; Rechargeable

40
Q

Fuel Cells

A

Produce energy - electricity or heat - when reactants are available; Not batteries, do not store electricity

41
Q

Chemical equilibrium

A

Exists when the forward and reverse kinetic reaction rates are equal

42
Q

Activity

A

The effective concentration of an entity

43
Q

Fugacity

A

The effective pressure of a gaseous entity

44
Q

Thermodynamic equilibrium constant

A

Retains the normal reporting state of the reagants

45
Q

Levelling Effect

A

Strong acids and bases are strong because they react with the solvent, leaving the acid/base of the solvent

46
Q

Buffered System

A

Resists changes in pH with the addition of other acids or bases; contains a mixture of a weak conjugate acid-base pair.

47
Q

Solubility Equilibrium

A

Exists when a sparingly soluble entity is put or forms in solution

Chem 102 (1 decks)

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