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Gen Chemistry 1 > Gen Chem Exam 3 > Flashcards

Gen Chem Exam 3 Flashcards

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1
Q

What undergoes combustion during the welding of metals?

A

A mixture of acetylene and oxygen

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2
Q

What is more practical and convenient to measure compared to moles?

A

Mass

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3
Q

Limiting Reactant

A
  • The substance that is used up first
  • The substance that limits the amount of product that can form.
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4
Q

Excess Reactant

A

The reactants that do not completely react and are left over at the end of the reaction.

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5
Q

What reactant yields the smallest amount of product?

A

Limiting reactant

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6
Q

Theoretical Yield

A

The maximum amount of product, which is calculated using the balanced equation and the limiting reactant.

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7
Q

Actual Yield

A

The amount of product experimentally obtained or collected during the experiment.

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8
Q

Percent Yield

A

The ratio of actual yield to theoretical yield.

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9
Q

Percent Yield Formula

A

Actual Yield/Theoretical Yield x 100%

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10
Q

During what 3 scenarios does energy change occur?

A
  1. When reactants interact
  2. When bonds break apart
  3. When products form
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11
Q

Heat of Reaction / Enthalpy Change

A

The difference between the enthalpy of the products and enthalpy of the reactants

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12
Q

Exothermic Reaction

A
  • Heat is released
  • The energy of the products is less than the energy of the reactants
  • Heat is a product
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13
Q

Endothermic Reactions

A
  • Heat is absorbed
  • The energy of the products is greater than the energy of the reactants
  • Heat is a reactant
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14
Q

Cold packs being activated are an example of a ___ reaction.

A

endothermic

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15
Q

How many elements in the periodic table exist as gases at room temperature conditions?

A

Only a few

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16
Q

What elements are considered gases at room temperature conditions?

A
  1. All noble gases
  2. Some diatomic molecules (H2, N2, O2, F2, and Cl2)
  3. Oxides of the nonmetals
    (CO, CO2, NO, NO2, SO2, and SO3)
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17
Q

What are the 7 properties of gases?

A
  1. Indefinite shape and volume
  2. Takes the same shape and volume as its container
  3. Particles are far apart
  4. Particles are moving quickly in random directions
  5. Low densities
  6. Compressible
  7. Form homogenous mixtures
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18
Q

Kinetic Molecular Theory of Gases

A
  1. Gases consist of tiny particles moving randomly at high velocities
  2. Most of the volume of a gas is empty space.
  3. There are no attractive or repulsive forces between gas particles
  4. Gas particles are constantly moving in straight paths.
  5. The average kinetic energy of the gas particles is proportional to the kelvin temperature of the sample.
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19
Q

What causes gas pressure to arise?

A

Collisions exerted by gas particles against the container walls.

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20
Q

What four units are used to measure pressure?

A
  1. Pascal (Pa)
  2. mmHg
  3. Torr
  4. Atmosphere (atm)
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21
Q

Atmosphere

A

A mixture of gases that cover the earth

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22
Q

Atmospheric Pressure

A

The pressure exerted by a column of this air mixture towards the surface of the Earth.

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23
Q

When is atmospheric pressure (atm) at 1?

A

Sea level

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24
Q

How many mmHg and Torr are in 1 atm?

A

760

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25
Q

Barometer

A

Measures the pressure exerted by the gases in the atmosphere.

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26
Q

What causes atmospheric pressure to change?

A
  1. Weather
  2. Altitude
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27
Q

What weather causes the atmospheric pressure to increase?

A

Hot and sunny

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28
Q

What weather causes the atmospheric pressure to decrease?

A

Rainy

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29
Q

Atmospheric pressure decreases as ___ increases.

A

Altitude

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30
Q

What are the 4 variables that define the physical properties of a gas?

A
  1. Pressure (P)
  2. Temperature (T)
  3. Volume (V)
  4. Amount of gas moles (n)
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31
Q

What are the 4 gas laws?

A
  1. Boyle’s Law
  2. Charles’s Law
  3. Gay-Lussac’s Law
  4. Avogadro’s Law
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32
Q

Ideal Gas Law Definition

A

A gas whose behavior follows the 4 gas laws.

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33
Q

Ideal Gas Law Formula

A

PV = nRT

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34
Q

What does the variable R represent in the ideal gas law formula?

A

The gas constant (value is given on sheet)

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35
Q

What type of volumes do cylinders have?

A

A fixed volume (can’t be greater than 1 atm)

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36
Q

What happens to the volume when you blow up a balloon?

A

The volume will expand until the pressure equalizes with the atmospheric pressure.

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37
Q

Combined Gas Law Definition

A

When more than two properties of gas change at once, two laws can be combined to explain its behavior.

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38
Q

Combined Gas Law Equation

A

(P1 x V1)/T1 x (P2 x V2)/T2

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39
Q

Boyle’s Law

A

V decreases as P increases
- n and T are constant

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40
Q

Charles’s Law

A

V changes the same to T
- n and P are constant

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41
Q

Gay- Lussac’s Law

A

P changes the same to T
- n and V are constant

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42
Q

What causes vapor to form?

A

When liquid molecules with enough kinetic energy break away from the surface of a liquid.

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43
Q

What happens when liquid is left in an open container?

A

It will eventually evaporate

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44
Q

What happens when vapor is left in a closed container?

A

The vapor accumulates and creates pressure called vapor pressure.

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45
Q

What is vapor pressure of a liquid dependent on?

A

Temperature

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46
Q

Boiling Point

A

The temperature at which the vapor pressure (inside container) becomes equal to the external pressure.

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47
Q

Water boils at ___ temperatures in the mountains.

A

lower

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48
Q

Avogadro’s Law

A

V changes the same to n
- P and T are constant

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49
Q

What are the standard conditions for the gas formulas?

A

T = Kelvin
V = L
n = Moles
P = atm

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50
Q

Why do the gas formulas need to be converted with the same units?

A

So comparisons can be made among different experiments.

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51
Q

What is the standard volume at 1 mole of gas?

A

22.4 L (molar volume)

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52
Q

What does the molar volume mean?

A

No matter the identity of the gas, the volume is ALWAYS 22.4 L at 1 mole.

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53
Q

Dalton’s Law of Partial Pressures

A

The total pressure exerted by a mixture of gases in a container at constant V and T

The sum of the pressures of each individual gas in the container

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54
Q

Partial Pressure

A

A gases own pressure in comparison to the total pressure of the gas.

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55
Q

Partial Pressure Formula

A

P total = P1 + P2 + P3 + Pn…

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56
Q

What are the different elements within the air we breath?

A
  1. N2 (78%)
  2. O2 (21%)
  3. other gases (1%)
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57
Q

What is the partial pressure exerted by a given gas proportional to?

A

The mole percentage of that gas in the mixture.

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58
Q

What are the 4 IMFs?

A
  1. Ion Dipole
  2. Hydrogen Bonding
  3. Dipole-Dipole
  4. Dispersion
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59
Q

Aqueous Solution (aq)

A

Dissolved in water

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60
Q

Solutions

A

Homogenous (completely mixed) mixtures of 2+ substances

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61
Q

What are the two components of solutions?

A
  1. Solvents
  2. Solutes
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62
Q

Solvent

A

Present in a larger amount
- major component of the slution

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63
Q

Solute

A

Present in a smaller amount
- spread evenly throughout the solution

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64
Q

___ dissolves into ___ to form a solution.

A

Solute, solvent

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65
Q

What physical states can a solute have?

A

Liquid, gas or solid

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66
Q

How can solutes be seperated?

A

Evaporation
- not by filtration

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67
Q

Are solutes visible?

A

No but they can add a color to the solution

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68
Q

What causes the solute to dissolve into the solvent?

A

Molecules within the solvent are capable of forming sufficient attractions with the solute particles to make them dissolve

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69
Q

Water (H2O)

A
  • A polar molecule due to O-H bonds
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70
Q

What is one of the most common solvents in nature?

A

Water

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71
Q

What do solute molecules form with water?

A

Intermolecular forces

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72
Q

What takes place in water media?

A

The vast majority of chemical reactions (biological reactions)

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73
Q

Aqueous Reactions

A

Reactions that take place in water media

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74
Q

What combinations causes solutions to form?

A

Polar - Polar
Nonpolar - Nonpolar

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75
Q

What are the 3 common nonpolar solvents?

A
  1. Hexane (C6H12)
  2. Toluene (C7H8)
  3. Carbon Tetrachloride (CCL4)
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76
Q

Do nonpolar solutes dissolve in polar solvents?

A

NO
- Nonpolar outweighs the polar

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77
Q

What are the 2 examples of nonpolar solutes?

A
  1. Hydrocarbons, oils, and fats
  2. Compounds that can only form dispersion forces (cancel out)
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78
Q

Hydrocarbons

A

Compounds with only hydrogen and carbon

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79
Q

What happens when there is an absence of attractions?

A

A solution cannot form due to insufficient energy levels.

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80
Q

Nonpolar molecular compounds do not dissolve in….

A

Water

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81
Q

What are the 3 most common polar solvents?

A
  1. Water (H2O)
  2. Acetone ((CH3)2C=O)
  3. Ethanol (CH3CH2OH)
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82
Q

What are examples of polar solutes?

A
  1. Ionic compounds or salts
  2. Compounds that can form dipole-dipole interactions and/or Hydrogen Bonding
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83
Q

Within a lewis structure, hydrogen bonds are shown as…

A

dashed lines

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84
Q

Are polar molecular compounds, such as menthol, soluble in water?

A

Yes
- There is a polar OH- group present to form H bonds in water

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85
Q

What are 2 examples of polar molecular compounds?

A
  1. Small polar molecules
  2. Water soluble vitamins
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86
Q

Ionic Solutes

A

Form ion dipole interactions with water molecules.

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87
Q

What is an example of an ionic solute?

A

NaCl crystals

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88
Q

What happens during the ionic solute of NaCl crystals?

A
  1. Na+ and Cl- ions are pulled out into the solution and get dissolved
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89
Q

What does hydrated mean?

A

Surrounded by water
(water molecules surround themselves around the positive and negative ions)

90
Q

Dissociate

A

A solid dissolves in water
- becoming hydrated as an ion

91
Q

How are solutes in a solution classified?

A
  1. Electrolytes
  2. Non-electrolytes
92
Q

Dissolved ions play an important role in…

A

Maintaining the proper function of the nervous system, cells, and organs.

93
Q

How can dissolved ions such as K, Cl, and bicarbonate be measured?

A

In a blood test

94
Q

Electrolytes

A

Compounds that dissociate to produce ions when dissolved in water.

95
Q

What do electrolytes conduct?

A

Electricity due to the presence of ions

96
Q

What are examples of electrolytes?

A
  1. Water soluble ionic compounds
    Ex) NaCl, KBr, Ca(NO3)2, LiOH, CuSO4
  2. Molecular compounds that are acids
    Ex) HCl, H2SO4, COOH
97
Q

How are electrolytes classified?

A
  1. Strong
  2. Weak
98
Q

Strong Electrolytes

A

Completely dissolve in water to produce ions.
- Distinguished by a forward pointing arrow

99
Q

What are examples of strong electrolytes?

A
  1. Water soluble ionic compounds
    Ex) NaCl, KBr, Ca(NO3)2, LiOH, CuSO4
  2. Molecular compounds that are STRONG acids
    Ex) HCL, H2SO4
100
Q

Weak Electrolytes

A

Dissolve only slightly in water to produce few ions.
- Mixture of ions and intact molecules

101
Q

A formula with weak electrolytes is displayed by…

A

A double arrow
= does not completely dissolve

102
Q

Nonelectrolytes

A

Compounds that do not dissolve in water to produce ions.
- only intact molecules are found

103
Q

Non electrolytes do not…

A

conduct electricity due to the absence of ions

104
Q

What are examples of nonelectrolytes?

A

Molecular compounds that are not acids like carbon containing compounds.
- Ethanol, sucrose, urea

105
Q

Solubility

A

The maximum amount of solute that dissolved in a specific amount of solvent at a specific heat.

106
Q

How is solubility expressed?

A

As grams of solute in 100 grams of solvent (water)
- (g solute)/(100 g water)

107
Q

What is the solubility of a given solute dependent on?

A

Temperature

108
Q

Unsaturated Solutions

A

Contain less than the maximum amount of solute (solubility)

109
Q

What are two characteristics of unsaturated solutions?

A
  1. No undissolved solute found at the bottom of the container.
  2. If more solute is added, it will dissolve.
    - No noticeable materials within the solution.
110
Q

Saturated Solutions

A

Contains the maximum amount of solute that can dissolve at a specific temperature

111
Q

What are 3 characteristics of saturated solutions?

A
  1. Have undissolved solute at the bottom of the container
  2. If more solute is added, it will NOT dissolve
  3. Contain solute that dissolves as well as solute that recrystallizes in an equilibrium process.
    - displayed with double arrow (not fully dissolved)
112
Q

What is the relationship between temperature and solubility in solids?

A

As the temperature increases, the solubility increase

113
Q

What physical state usually becomes more soluble in water when the solution is heated up?

A

Solids

114
Q

What is the relationship between temperature and solubility in gases?

A

As the temperature increases, the solubility level decreases

115
Q

Henry’s Law

A

The solubility of a gas in a liquid is directly related to the pressure of the gas above the liquid.

116
Q

What is the relationship between pressure and gas molecules?

A

As the pressure level increases, more gas molecules dissolve in the liquid.

117
Q

Insoluble Ionic Compound

A

Will form when the ionic bonds are too strong for the polar molecules to break

visually separation within the solution (precipitate)

118
Q

Solubility Guidelines

A

A set of rules that help determine whether a compound is soluble or not.
(given on exam sheet)

119
Q

Precipitation Reactions

A

A chemical reaction in which soluble reactants yield an insoluble product that precipitates out of a solution

120
Q

Precipitate

A

A solid

121
Q

What happens when two soluble solutions are mixed together?

A

An insoluble solution is created.

122
Q

What type of reactions do precipitation reactions undergo?

A

Double Reaction

  • the cation of one compound partners with the anion of the other compound.
123
Q

Complete Ionic Equation

A

All soluble reactants (aq) and products are written as dissociated ions.

124
Q

How are solids written in an ionic equation?

A

Intact since they are no longer dissolved in the solution

125
Q

Net Ionic Equation

A

Remove the spectator ions from the complete ionic equation.

126
Q

Spectator Ions

A

Ions that remain unchanged from the reactant to product side
(stays the same)

127
Q

Concentration

A

How much of a solute is dissolved in a solution

128
Q

Concentration of a solution =

A

(amount of solute)/
(amount of solution)

129
Q

What units can solute be expressed in?

A

-grams
-millimeters
-moles

130
Q

What units can a solution be measured in?

A
  • grams
  • millimeters
  • liters
131
Q

Mass/Volume Percent of a Solute

A

mass/volume percent

(mass of solute)/(volume of solution) X 100

132
Q

Mass Percent of a Solute

A

mass percent

(mass of a solute)/(mass of a solution) X 100

133
Q

Volume Percent of a Solute

A

Volume percent

(volume of solute)/(volume of solution) X 100

134
Q

Molarity of a Solute

A

Molarity (M)

(moles of solute)/(volume of solution)

135
Q

What happens to concentrated solutions before use?

A

It is diluted

136
Q

What happens to the volume/concentration ratio when a chemical is diluted?

A
  • Volume increases
  • Concentration decreases
137
Q

What happens to the Molarity (M) when a solution is diluted?

A

Molarity (M) decreases because the volume increases

138
Q

What MUST stay the same throughout the dilution process?

A

Number of moles of solute

139
Q

How are chemicals stored or prepared?

A

As concentrated solutions

140
Q

What has to be done to concentrated solutions before they are used?

A

They must be diluted

141
Q

What are common examples of concentrated solutions?

A

Acids

142
Q

What happens to the amount of concentrated solution when it is diluted?

A

It is now spread out in a larger volume of water.

143
Q

What is the formula of dilution?

A

M1 X V1 = M2 X V2

144
Q

What does 1 and 2 represent in the dilution formula?

A

Initial (1) and Final (2)

145
Q

What are the 3 types of mixtures?

A
  1. Solution
  2. Colloid
  3. Suspension
146
Q

What do the properties of solutions measure?

A

Size vs quanitity

147
Q

What type of particles are solutions?

A

Small particles
(atoms, ions, or small molecules)

148
Q

How do particles settle in a solution?

A

The particles DO NOT settle

149
Q

How can particles be separated in a solution?

A

They cannot be separated.

150
Q

What types of particles make up a colloid?

A

Larger molecules or groups of molecules/ions

151
Q

How do particles settle in a colloid?

A

The particles DO NOT settle

152
Q

How can particles be separated in a colloid?

A

By semipermeable membranes.

153
Q

What types of particles are in a suspension?

A

VERY large particles
- may be visible

154
Q

How do particles in a suspension settle?

A

Settle rapidly

155
Q

How can particles in a suspension be separated?

A

By filters

156
Q

What are the two ways to separate mixtures?

A
  • Filters
  • Semipermeable Membranes
157
Q

What are examples of suspensions?

A
  • Blood platelets
  • Muddy water
  • Calamine lotion
  • Flour in water

(separates on standing)

158
Q

What type of mixture is heterogenous?

A

Suspensions

159
Q

What type of mixture is transparent?

A

Solutions

160
Q

What is osmotic pressure?

A

A colligative property

161
Q

Colligative Properties

A

Depends only on the NUMBER of solute particles in the solution.

  • Not focused on concentration/identity (amount)
162
Q

What do semipermeable membranes allow to pass through?

A

Solvent molecules

163
Q

What do semipermeable membranes NOT allow to pass through?

A

Solute molecules/ions

164
Q

Osmosis

A

Solvent molecules (water) flow from the lower solute concentration to the higher solute concentration via a semipermeable membrane.

165
Q

What happens to the flow of water in osmosis?

A

It becomes equal in both directions

166
Q

What happens to the water level of the solutions in osmosis?

A

The one with the higher level concentration rises.

167
Q

Osmotic Pressure

A

The pressure that would prevent the flow of additional water into the more concentrated solution.

168
Q

What causes osmotic pressure to increase?

A

An increase in amount of dissolved molecules in a solution.

169
Q

Reverse Osmosis

A

An external pressure that is greater than osmotic pressure is applied to a solution, forcing it through the opposite way of the membrane.

170
Q

What happens to the flow of water in reverse osmosis?

A

It is reversed
- High to low solute concentration

171
Q

What does reverse osmosis leave behind?

A

The molecules and ions in the solution.

172
Q

What is one example of reverse osmosis?

A

It is used in removing the salt water from plants in order to obtain pure water.

173
Q

What is the problem with osmosis?

A

It requires a large amount of energy

174
Q

What causes osmosis to continuously occur in biological systems?

A

The cell membranes are semi permeable

175
Q
A
176
Q

What are examples of solutes in the body?

A
  • Blood
  • Tissue fluids
  • Lymph
  • Plasma
177
Q

What do all solutes in the body do?

A

Exert osmotic pressure

178
Q

What is an example of isotonic solutions in hospitals?

A

IV solutions

179
Q

What are the 3 types of solutions?

A
  1. Isotonic
  2. Hypotonic
  3. Hypertonic
180
Q

Isotonic Solutions

A

Exert the same osmotic pressure as the solute concentration.

181
Q

Hypotonic Solutions

A

Exert lower pressure than the solute concentration.

182
Q

Hypertonic Solution

A

Exert higher osmotic pressure than the solute concentration.

183
Q

What can solute concentrations be compared to when examining solution types?

A

Red blood cells in the body

184
Q

Hemolysis

A

Water flows into red blood cells, causing the to swell/burst

185
Q

What type of solution does hemolysis include?

A

Hypotonic

186
Q

Crenation

A

Water flows out of the red blood cells, causing them to shrink.

187
Q

What type of solution does crenation involve?

A

Hypertonic

188
Q

Do products or reactants have more energy in Exothermic Reactions?

A

Reactants (negative energy level)\

189
Q

Do products or reactants have more energy in Endothermic Reactions?

A

Products (positive energy level)

190
Q

Energy for Chemical Reactions Formula

A

(Energy of Products) - (Energy of Reactants)

191
Q

Rate of Reaction Formula

A

(change in concentration of reactant/product)/
(change in time)

192
Q

Collision Theory

A

Chemical reactions occur through collisions between molecules/atoms

193
Q

What 3 conditions must be met for a chemical reaction to occur?

A
  1. The reactants must collide
  2. The reactants must properly align to break and form bonds
  3. The collision must provide sufficient energy of activation
194
Q

Activation Energy (Ea)

A

The minimum amount of energy required to break the bonds between atoms of the reactants

195
Q

What must be overcome for the reactants to turn to products?

A

Activation energy barrier

196
Q

What 3 factors influence the rate of a chemical reaction?

A
  1. Changes in temperature
  2. Changes in reactant amount (concentration)
  3. Presence of a catalyst
197
Q

How does increasing the temperature increase reaction rate?

A

More collisions occur

198
Q

How does increasing the reactant concentration increase reaction rate?

A

More collisions occur

199
Q

How does adding a catalyst increase reaction rate?

A

Lowers the energy of activation

200
Q

What increases as temperature increases?

A

Kinetic energy of the reactant molecules

201
Q

What happens to reaction rates as the reaction proceeds?

A

It decreases due to reactants getting converted to products

202
Q

How does adding a catalyst speed up rate of reaction?

A

Provides an alternate pathway that has a lower activation energy.
- More collisions provide sufficient energy for the reactants to form products

203
Q

What does not happen to the catalyst during a chemical reaction

A

It is not changed or consumed during the reaction

204
Q

Do reactions with a lower or higher activation energy level have faster reaction rates?

A

Lower

205
Q

Forward Reaction

A

Reactants to products
- produced until limiting

206
Q

Reverse Reaction

A

Products to reactants

207
Q

What two reactions occur at the same time?

A

Forward and Reverse reactions

208
Q

Reversible Reactions

A

Reactions that occur in both the forward and reverse direction at the same time

209
Q

Are all reactions reversible?

A

MOST but not all

210
Q

What is a sign that a reaction is reversible?

A

Two arrows pointing in opposite directions

211
Q

What is the relationship between the rate of forward reaction and rate of reverse reaction?

A

Rate of Forward Reaction decreases
as
Rate of Reverse Reaction increases
(as time goes on)

212
Q

Equilibrium

A

Rate of forward reaction

Rate of reverse reaction

213
Q

What is the relationship between the concentration of reactants and the concentration of products?

A

The concentration of reactants decreases
as
the concentration of products increases

214
Q

What happens to the concentrations of reactants at equilibrium?

A

No longer change with time
- Reactants and products are being used up at the same rate at which they are being formed

215
Q

What is produced at equilibrium?

A

The same mixture is formed from the reactants and products.

216
Q

Equilibrium Constant

A

(Concentration of Products)/
(Concentration of Reactants)

217
Q

What do the coefficients represent in the equilibrium constant formula?

A

Exponents

218
Q

Does the equilibrium constant have units?

A

No

219
Q

What unit are concentrations given in?

A

Molarity units (mol/L)

220
Q
A

Gen Chemistry 1 (10 decks)

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