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Intro to Chem > Unit 7-9? > Flashcards

Unit 7-9? Flashcards

1
Q

Kinetic energy is associated with _____.

A

Motion

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2
Q

Potential energy is associated with ____ or _____.

A

Position or composition.

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3
Q

Chemical energy is a form of _____ energy.

A

Potential

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4
Q

Thermal energy is a form of _____ energy.

A

Kinetic

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5
Q

Chemical energy is associated with:

A

Relative positions of electrons and nuclei in atoms and molecules

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6
Q

Heat is the _____ of thermal energy.

A

Transfer

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7
Q

Breaking bonds _____ energy.

A

Consumes or absorbs (+)

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8
Q

Forming bonds _____ energy.

A

Releases (-)

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9
Q

Heat is absorbed (+ delta H) in ______ reactions.

A

Endothermic

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10
Q

Heat is released (- Delta H) in _____ reactions.

A

Exothermic

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11
Q

Bonds broken in reactants are stronger than bonds formed in products. What is the reaction?

A

Endothermic

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12
Q

Products are higher in energy than reactants. What is the reaction?

A

Endothermic

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13
Q

Bonds formed in products are stronger than bonds broken in reactants. What is the reaction?

A

Exothermic

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14
Q

Products lower in energy than reactants. What is the reaction?

A

Exothermic

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15
Q

Delta H reaction is the difference between energy needed to ______ in the reactants and the energy needed to _____ in the products.

A

Break bonds, form bonds.

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16
Q

Increase [_____] leads to an increase in the _____ of _____ leads to increase _____.

A

Reactants, number of collisions, reaction rate.

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17
Q

Increasing temperature drives a chemical rxn by increasing the _____ of each molecule, leading to more _____ _____, and increasing the overall _____ _____.

A

Energy, successful collisions, reaction rate.

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18
Q

Catalysts effects the _____, and not the _____.

A

Reaction rate (fast or slow), not delta H.

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19
Q

Catalysts do not appear in the _____.

A

Product.

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20
Q

Catalysts speed up the rxn rate by _____ the activation energy.

A

Lowering

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21
Q

Equilibrium is the point in which the rate of the forward reaction ______ the rate of the reverse reaction.

A

Equals

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22
Q

Molarity ( __ ) equals x/x

A

Capitol M, moles / liters.

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23
Q

K = [ _____ ] / [ _____ ]

A

K (equilibrium constant) = concentration of products / concentration of reactants

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24
Q

K>1, equilibrium favors _____.

A

Products

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25
Q

K<1, equilibrium favors _____.

A

Reactants

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26
Q

K~1, _____ and _____ are present.

A

Reactants and products

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27
Q

Le Chatelier’s Principle basically states that:

A

If a chemical system is stressed, it will react in the direction that relieves the stress. It finds balance!

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28
Q

Delta H is always written for the _____ direction.

A

Forward

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29
Q

Gasses have a(n) _____ volume and a(n) _____ shape.

A

Indefinite, indefinite.

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30
Q

Liquids have a(n) _____ volume and a(n) _____ shape.

A

Definite, indefinite.

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31
Q

Solids have a(n) _____ volume and a(n) _____ shape.

A

Definite, definite.

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32
Q

Unit of pressure:

Atmospheres = ( _____ )

A

atm

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33
Q

Unit of pressure:

psi =

A

Pounds per square inch

34
Q

Unit of pressure:

(Pa) =

A

Pascals

35
Q

How many mmHg are in one atm?

A

760.

36
Q

How many torr in one atm?

A

760.

37
Q

STP stands for:

A

Standard temperature (273 K), and pressure (1 atm)

38
Q

At STP, the molar volume of any ideal gas is _____ Liters.

A

22.4

39
Q

A rxn with a lower activation energy is (more/less) likely to occur than a rxn with a higher activation energy.

A

More likely

40
Q

A higher activation energy is typically associated with (slower/faster) rxn rates.

A

Slower, because fewer particles has sufficient energy to overcome the E of a (activation energy) and form products.

41
Q

Catalysts (are/ are not) consumed in an overall reaction.

A

Are not.

42
Q

1 calorie = (x) Joules

A

4.184 joules

43
Q

1 Pa = x PSI

A

1.45 x 10^-4

44
Q

What affects rate of chem rxn?

A

Temperature, concentration of reactants, and presence of a catalyst.

45
Q

Potential energy is stored in _____ or _____ bonds.

A

Ionic or covalent

46
Q

Bond dissociation energies are (+-) and bond formation energies are (+-).

A

Positive, negative.

47
Q

The higher + delta H, the more energy required to _____ the bond. Decreasing dissociation energy as you move _____ a group, and as atomic size _____.

A

Break. Down. Increases.

48
Q

Electrostatic interactions exist WITHIN _____ compounds.

A

Ionic

49
Q

INTRAmolecular forces) are:

A

Forces that hold molecules together (form bonds).

50
Q

INTERmolecular forces (IMF) are:

A

Attractive forces between molecules or ions that hold them near each other.

51
Q

What is the weakest force of all three intrOmolecular forces? What kind of line is used to represent these forces?

A

IntERmolecular forces, - - - - - line.

52
Q

List the three types of intERmolecular interactions between molecules?

A

London dispersion forces, dipole-dipole, and hydrogen bonding.

53
Q

What is a temporary dipole?

A

A momentary change in the e- density of a molecule. They can shift back and forth from non-polar to polar. & they create temporary dipoles in neighboring molecules.

54
Q

All covalent compounds have what type of intermolecular interactions?

A

London dispersion forces.

55
Q

Non-polar covalent compounds have only what type of intermolecular interactions?

A

London dispersion forces

56
Q

The larger the (mass of a) molecule, the _____ the forces between two molecules.

A

Stronger

57
Q

Dipole-dipole interactions are:

A

Attractive forces between permanent dipoles of two POLAR molecules.

58
Q

Hydrogen bonding occurs when ___ atom is bound to: ___, ___, or ___. And can be broken apart using _____ means.

A

H bound to O,N, or F. Physical.

59
Q

Boiling point is defined as:

A

The temperature in which a liquid becomes a gas.

60
Q

Melting point is defined as:

A

The temperature in which a solid becomes a liquid.

61
Q

The strength of the intermolecular force is proportionally related to:

A

Boiling point, melting point, and surface tension.

62
Q

The strength of the intermolecular force is inversely related to:

A

Vapor pressure.

63
Q

Surface tension is defined as:

A

The measure of resistance of a liquid spread out.

64
Q

Sublimation, vaporization, and melting, are all processes in which energy is _____.

A

Absorbed.

65
Q

Deposition, condensation, and freezing are processes in which energy is _____.

A

Released

66
Q

Sublimation is when you go from a _____ to a _____ and skip the _____ phase altogether.

A

Solid to a gas and skip the liquid phase. (Dependent on atm pressure)

67
Q

What is not included in the K expression?

A

Pure solids and liquids because they have constant concentrations.

68
Q

_____molecular forces/attractions influence the chemical properties of a substance, and _____molecular forces/attractions influence the physical properties of a substance.

A

Intramolecular forces, intermolecular attractions.

69
Q

Vaporization is the phase of ____ becoming _____.

A

Liquid becoming a gas

70
Q

Condensation is the phase of _____ becoming _____.

A

Gas to a liquid

71
Q

Sublimation is the phase of _____ becoming _____.

A

Solid to a gas

72
Q

Deposition is the phase of _____ becoming _____.

A

Gas to solid

73
Q

Any time particles are close together and need to be pulled apart, energy needs to be _____.

A

Absorbed

74
Q

Any time particles are going from less compact to more compact, energy will be _____.

A

Released

75
Q

What is solute?

A

The substance present in smaller amount.

76
Q

What is solvent?

A

Substance present in larger amount

77
Q

What is solubility?

A

Max amount of solute that dissolves in a given amount of solvent under a given set of conditions

78
Q

List the three mixtures in order of particle size (smallest to largest)

A

Solution, collid, and suspension.

79
Q

When a solute is added, vapor pressure _____.

A

Decreases

80
Q

When a solute is added, the freezing point _____.

A

Decreases

81
Q

When a solute is added, the boiling point _____.

A

Increases

82
Q

Freezing-point depression is directly proportional to the _____ per formula unit.

A

Ions

Intro to Chem (10 decks)

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