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H.Chemistry final Flashcards

0
Q

Explains the behavior of particles in terms of their motions

A

Kinetic theory

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1
Q

Energy of motion

A

Kinetic energy

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2
Q

4 properties of gases:

A

1-negligible volume
2-move in rapid, constant straight-line motion
3-Collide elastically
4-far apart with no attractive or repulsive force

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3
Q

Collision in which no kinetic energy is lost.

A

Elastic collision

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4
Q

Measure of average kinetic energy

A

Temperature

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5
Q

The _____________ the temperature, the _____ moving particles.

A

Higher

Faster

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6
Q

Temperature at which the motion of the particles theoretically ceases.

A

Absolute zero

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7
Q

Simultaneous collisions of billions of molecules within an object

A

Pressure

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8
Q

Force is created by _____.

A

Collisions

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9
Q

Pressure=?

A

Force
________
Area

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10
Q

Empty space, no collisions

A

Vacuum

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11
Q

Air molecule collisions

A

Atmospheric pressure

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12
Q

Typical sea level pressure

A

ATM

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13
Q

Barometric reading

A

mm Hg

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14
Q

Forces within a compound that hold it together

A

Intramolecular forces

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15
Q

Forces between compounds that hold these compounds together.

A

Intermolecular forces

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16
Q

Which two phases are fluid?

A

Liquids and gases

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17
Q

Why are liquids more dense than gases?

A

Because they have attractive forces

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18
Q

Temperature that a solid turns into a liquid

A

Melting point

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19
Q

The stronger the intermolecular force the _______ the melting point

A

Higher

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20
Q

Temperature at which a solid melts at 1.00 ATM atmosphere(101.3kPa) of pressure.

A

Normal melting point

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21
Q

Process of a liquid changing to a gas or vapor

A

Vaporization

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22
Q

Liquid to gas below boiling point

Happens only on the surface

A

Evaporation

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23
Q

How many particles escape during evaporation to become a gas

A

Only particles moving fast enough

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24
Q

As high speed particles escape this lowers the average kinetic energy and therefore the temperature.

A

Cooling process

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25
Q

Increasing temperature will _______ vapor pressure

A

Increase

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26
Q

The temperature at which the vapor pressure of a liquid is equal to the external pressure on a liquid.

A

Boiling point

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27
Q

Temperature when the vapor pressure equals the atmospheric pressure 1 atm=101.3kPa.

A

Normal boiling point.

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28
Q

Temperature of liquid _____ gets above the boiling point

A

Never

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29
Q

Three properties of solids:

A

1- tightly packed
2-do not flow(they vibrate)
3-incompressible

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30
Q

State the 3 states of a substance from least dense to the most dense

A

Gas liquid solid

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31
Q

The atoms, ions, or molecules are arranged in a very orderly, repeating 3D arrangement of particles known as the crystal lattice

A

Crystal

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32
Q

2 or more different substances of the same element in the same physical state.

A

Allotropes

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33
Q

A solid in which the particles are randomly arranged

A

Amorphous

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34
Q

The process in which a solid changes to a gas without passing through the liquid state

A

Sublimation

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35
Q

Gas or vapor becomes a liquid

A

Condensation

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36
Q

Vapor to a solid

A

Deposition

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37
Q

Liquid to a solid

A

Freezing

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38
Q

Diagram that shows relationship between solid,liquid, and gas states for a substance in a closed container at different temperatures and pressure.

A

Phase diagram

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39
Q

Temperature and pressure where all three common states of matter coexist in equilibrium

A

Triple point

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40
Q

Above this temperature, the substance can only exist as a gas.

A

Critical point

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41
Q

The amount of a substance that contains the same number of particles, 6.2x10^23 particles.

A

Moles

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41
Q

Consists of one element

A

Atom

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42
Q

Consists of two or more nonmetal elements

A

Molecule

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43
Q

Consists of a metal and a nonmetal/ NH4+

A

Formula unit

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44
Q

Unit for molar mass

A

g/mol

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45
Q

Simplest whole number ratio of moles of the atoms in a substance.

A

Empirical formula

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46
Q

Some multiple of the empirical formula.

A

Molecular formula

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47
Q

Equation to convert an empirical formula to a molecular formula.

A

X= molar mass
____________

 Empirical formula
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48
Q

Steps to find the empirical formula

A
  • get mass
  • get moles
  • get whole numbers(divide by small, multiply by 2,3,4 if needed)
49
Q

Compound that has a specific number of water molecules bound to its atoms.

A

Hydrate

50
Q

The study of quantative relationships between amounts of reactants used and products formed by a chemical reaction.

A

Stoichiometry

51
Q

Amount of product that can be formed in a reaction and how much excess reactant is left over

A

Limiting reactant

52
Q

The percentage of a certain product actually produced in a chemical reaction.
+ equation

A

Percent yield= actual yield
————– x 100
Theoretical yield

53
Q

Pressure conversions

A

1.0atm=760.0mmHg=101.3kPa=14.7psi=760.0torr

54
Q

What happens to the temperature of a boiling liquid when heat is added to it?

A

Remains constant

55
Q

What are four variables that effect gas behavior?

A

Pressure, volume, moles, and temperature

56
Q

Relationship between pressure and volume, law name and equation

A

•Inversely proportional, as volume increases, pressure decreases
•Boyle’s law
•P V = P V
1 1 2 2

57
Q

Relationship between pressure and temperature, law name and equation

A 
• directly proportional
• gay-lussac's law
•   P1    P2
    --- = ----
    T1    T2
58
Q

Relationship between pressure and moles, law name and equation

A
  • Directly proportional
  • Ideal gas law
  • PV=nRT
59
Q

Relationship between temperature and volume, law name, and equation.

A 
•directly proportional
•Charles' law
• V1     V2
  ---- = ----
  T1     T2
60
Q

Equation of combined gas law

A

P1V1= P2V2
—— ——-
T1 T2

61
Q

What are the conditions of STP?

A

273.15k & 101.3kPa

62
Q

Standard molar volume

A

22.4 L

63
Q

Equal volumes of gases at the same temperature and pressure contain equal numbers of particles.

A

Avogadro’s principle

64
Q

A gas that follows the assumptions of the kinetic molecular theory

A

Ideal gas

65
Q

What does the R in PV=nRT and PM=DRT represent?

A

Universal gas constant

66
Q

When would a real gas become less ideal

A

In low temperature and high pressure

67
Q

At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the individual( partial ) pressure. + equation

A

Dalton’s law

P(total)=P1+P2+P3…

68
Q

Dalton’s law correction equation

A

P(total)=P(gas)+P(water)

69
Q

Tendency of molecules to move from an area of high concentration to low concentration until uniformly mixed.

A

Diffusion

70
Q

Rate at which gases escape from a small hole in a container

A

Effusion

71
Q

The rate of effusion of a gas is inversely

proportional to the square root of the gases molar mass.+equation.

A

Graham’s law

Rate A Molar mass B
——–=(square root) ———
Rate B Molar mass A

72
Q

Homogenous mixture; solute+solvent

A

Solution

73
Q

Present in greater amount

A

Solvent

74
Q

Substance being dissolved

A

Solute

75
Q

The process of surrounding solute particles to form a solution

A

Solvation

76
Q

Describes liquids that are insoluble in each other

A

Immiscible

77
Q

Two liquids that are soluble in any proportion

A

Miscible

78
Q

Polar solutes dissolve in polar solvents, and Nonpolar solutes dissolve in Nonpolar solvents.

A

Like dissolves like

79
Q

Why are ionic compounds electrolytes?

A

They conduct electricity

80
Q

Three factor that affect the rate of solvation

A
  • Agitation or Stirring
  • increasing the surface area
  • Heating
81
Q

Maximum amount of solute that can be dissolved in a given amount solvent at a given temperature.

A

Solubility

82
Q

Type of solution in which more solute can be dissolved.

A

Unsaturated

83
Q

Type of solution in which no more solute can be dissolved at that temperature.

A

Saturated

84
Q

More is dissolved than should be at that given temperature.

A

Supersaturated

85
Q

How is solid solubility different from gas solubility as it relates to temperature?

A

Solid solubility usually increases with an increase in temperature and gas solubility usually decreases with and increase in temperature.

86
Q

How is gas solubility related to pressure?

A

It’s directly proportional to pressure.

87
Q

What is the colligative property?

A

A property that depends on the number of solute particles, not the nature of the particle.

88
Q

How is vapor pressure affected when you increase the number or solute particles?

A

Decreases

89
Q

How is the boiling point affected when you increase the number or solute particles?

A

Increases

90
Q

How is the freezing point affected when you increase the number or solute particles?

A

Decreases

91
Q

% mass equation

A

= mass of solute
—————– X 100
Mass of solute+ Mass of solvent

92
Q

% volume equation

A

Volume of solute
——————- X 100
Volume of solution

93
Q

% mass/ volume equation

A

Mass solute(g)
—————- X 100
Volume of solution(ml)

94
Q

The amount of solute in a solution

A

Concentration

95
Q

Molarity equation

A

M = moles of solute / Liters of solution

96
Q

When diluting you use this equation:

A

M1V1=M2V2

97
Q

Molality equation

A

m= moles of solute / mass of solvent(kg)

98
Q

Visible scattering of light caused by the reflection off particles

A

Tyndall effect

99
Q
  • Mixture with particles so large, they settle out.
  • Positive or negative Tyndall affect?
  • type of mixture?
A
  • Suspension
  • positive
  • heterogeneous
100
Q
  • Mixture with intermediate sized particles small enough that the moving water molecules keep them stirred up.
  • type of mixture?
  • do they settle out?
  • positive or negative Tyndall effect?
A
  • Colloid
  • heterogeneous
  • no, don’t settle out
  • positive
101
Q
  • particles are uniformly mixed throughout.
  • do they settle out?
  • particle size?
  • Tyndall effect?
  • type of mixture?
A
  • solution
  • no,don’t settle out
  • small particles
  • negative Tyndall effect
  • homogeneous
102
Q

Mole fraction equation

A

Xa= na Xb= nb
——— ———
na+nb na+nb

103
Q

Boiling point elevation equation

A

Tb= kb x m x i

104
Q

Freezing point depression equation

A

Tf= kf x m x i

105
Q

What are the three main parts of collision theory?

A
  • reacting substances must collide
  • reacting substances must collide with correct orientation.
  • reacting substances must collide with sufficient kinetic energy to form the activated complex.
106
Q

An unstable arrangement of atoms that forms for a moment at the peak of the activation-energy barrier.

A

Activated complex

107
Q

Minimum energy needed for a successful reaction.

A

Activation energy

108
Q

Increases reaction rate, lowers the energy of activation.

A

Catalyst

109
Q

Decreases reaction rate, lowers the energy of activation.

A

Intermediate

110
Q

4 factors that affect the reaction rate and how do they affect them?

A
  • Temperature-increasing it usually increases reaction rate.
  • Catalyst- increases reaction rate
  • Concentration- more collision increases the reaction rate
  • Particle size- decreasing particle size, increases surface area, and makes the reaction rate faster.
111
Q

Average reaction rate equation

A

R= -[ change in reactant concentration ]
—————————————–
change in time

112
Q

In order for a reaction system to be in equilibrium,

A
  • The reaction must be reversible
  • the forward and reverse rates must be equal
  • the concentrations of the reactants and products must be constant, but not necessarily equal
  • if a reaction shifts to the right, the forward rate is larger than the reverse rate.
113
Q

At a given temperature, a chemical system may reach a state in which a particular ratio of reactant and product concentration is constant

A

Equilibrium constant expression

114
Q

What does K(eq)>1 mean?

A

More products than reactants at equilibrium.

115
Q

What does K(eq)<1 mean?

A

More reactants than products at equilibrium

116
Q

If a system at equilibrium is stressed, the equilibrium will shift until the stress is relieved.

A

Le Chatelier’s principle

117
Q

How does temperature affect equilibrium ?

A

If the reaction is endothermic it will shift to the right and if it’s exothermic, it will shift to the left.

118
Q

How does pressure and volume affect equilibrium ?

A

Increasing the pressure/ decreasing volume favors the side with the fewer gas particles

119
Q

Acid, hydrogen ion or proton that ionizes to make H+ protons.
Base, hydrogen ion or proton that ionizes to make OH-.

A

Arrhenius model Acid

120
Q

Acid, proton or hydrogen-ion donor

Base, proton or hydrogen-ion acceptor

A

Bronsted-Lowry model

121
Q

Difference between a strong and a weak acid/base?

A

Strong acids/bases completely ionize and weak acids/bases only partially ionize.

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