Exam 2

Front 1

You can determine the weight in grams of a mole of atoms by using this.

Back 1

Molar Mass

Front 2

You can determine the weight in grams of a mole of atoms by using this.

Back 2

A Mole

Front 3

This is the unit used for molar mass.

Back 3

Grams/Mole

Front 4

We can use this to convert between grams and moles of any material.

Back 4

Molar Mass

Front 5

We can use this to convert between grams and moles of any material.

Back 5

Molar Mass

Front 6

This is the molar mass of carbon dioxide, CO2.

Back 6

44 g/mol

Front 7

Balancing a chemical equation is used to show that this is conserved.

Back 7

Mass

Front 8

These materials are used to speed up reactions, but are not altered by the reaction.

Back 8

Catalysts

Front 9

Heat is measured in these units.

Back 9

Calories

Front 10

The energy content of food is measured in these units.

Back 10

Calories

Front 11

This is the study of reaction rates.

Back 11

Kinetics

Front 12

In addition to mass, this is also conserved in a chemical reaction.

Back 12

Energy

Front 13

In order to break a bond in a chemical reaction, this must be added.

Back 13

Energy

Front 14

A reaction may be slow because the value of this is quite high.

Back 14

EsubA

Front 15

A catalyst works by reducing this.

Back 15

EsubA

Front 16

This is a biological catalyst.

Back 16

Enzyme

Front 17

The symbol ΔH is used to indicate this about a reaction.

Back 17

Changes in enthalpy, or heat released

Front 18

These types of reactions release heat to the environment.

Back 18

Exothermic

Front 19

These reactions absorb heat from the environment.

Back 19

Endothermic

Front 20

This tells us on an energy diagram that a reaction is exothermic.

Back 20

Products lower than reactants

Front 21

ATP is mostly used by our bodies for this purpose.

Back 21

Energy transfers

Front 22

An increase in temperature usually has this effect on a reaction.

Back 22

Speeds up

Front 23

This happens to reactions with higher reactant concentrations.

Back 23

Speeds up

Front 24

This set of biochemical pathways has negative changes in enthalpy.

Back 24

Exothermic

Front 25

This is a chemical reaction in which the rate of the forwards and backwards reactions are equal and balanced.

Back 25

Equilibrium

Front 26

This is the rule determining how reactions reach equilibrium.

Back 26

Le Châtelier’s rule

Front 27

There is considerable space between molecules in this state of matter.

Back 27

Gas

Front 28

In this state of matter, molecules are locked in place, and their only motion is vibrational.

Back 28

Solid

Front 29

This represents energy that flows from a high temperature object to a lower temperature object.

Back 29

Heat

Front 30

This is a hidden energy, which may be converted to motion or work at a later time.

Back 30

Potential energy

Front 31

This type of energy is obvious in the motion of things around us.

Back 31

Kinetic energy

Front 32

A heating curve shows that adding heat to something at its boiling point or melting point has this effect on its temperature.

Back 32

No change

Front 33

Since melting something draws heat out of nearby objects, this is the result of freezing something.

Back 33

Heat flows into the object

Front 34

This is true of the vapor pressure of a liquid at its boiling point.

Back 34

It equals atmospheric pressure

Front 35

This increases if the temperature of a gas increases when the pressure stays constant.

Back 35

Volume

Front 36

This increases if the temperature of a gas decreases if the volume decreases.

Back 36

Pressure

Front 37

If a gas is forced into a smaller volume, then this property increases.

Back 37

Pressure

Front 38

This occurs more frequently at the walls of a container when the pressure of a gas inside it increases.

Back 38

Collisons

Front 39

This theory connects particle motion with some bulk properties of materials.

Back 39

Kinetic Molecular Theory

Front 40

If a gas consists of many components, its total pressure is the sum of these.

Back 40

Partial pressure

Front 41

The solubility of a gas in water is proportional to this.

Back 41

Partial pressure

Front 42

Hydrocarbons contain only these elements.

Back 42

Hydrogen and carbon

Front 43

These hydrocarbon compounds contain some carbon-carbon double bonds.

Back 43

Alkenes

Front 44

Because hydrocarbons have this property, they are insoluble in water.

Back 44

Non-polar

Front 45

These result when a chain of carbons is joined at its ends.

Back 45

Cyclic Hydrocarbons

Front 46

It is common to draw cyclic hydrocarbons using these geometric figures.

Back 46

Polygons

Front 47

These are the simplest way to draw hydrocarbons and other organic molecules.

Back 47

Skeletal Line Drawings

Front 48

This is the name for a hydrocarbon with a continuous chain of 4 carbons.

Back 48

Butane

Front 49

These cyclic hydrocarbons may be drawn with double bonds, but are much more stable than alkenes.

Back 49

Aromatic hydrocarbons

Front 50

This is the simplest of all the aromatic compounds.

Back 50

Benzene

Front 51

Generally, aromatic compounds contain this structure.

Back 51

The benzene ring

Front 52

This structure results when an O is joined to an H and an R-group.

Back 52

Alcohols

Front 53

Alcohols are soluble in water due to this property.

Back 53

Polarity

Front 54

These bonds may form between adjacent alcohols or to water from an alcohol.

Back 54

H-bonds

Front 55

This is a compound consisting of an alcohol joined to a benzene ring.

Back 55

Phenol

Front 56

These compounds consist of an O suspended between two R-groups.

Back 56

Ethers

Front 57

This cluster of atoms consists of a carbon double bonded to an oxygen.

Back 57

Carbonyl

Front 58

Aldehydes consist of these bonded to a carbonyl group.

Back 58

An R and an H group

Front 59

Ketones are different from aldehydes due to this feature.

Back 59

They have two R groups

Front 60

This feature of carbonyl-containing compounds aids their solubility in water.

Back 60

Polarity

Front 61

This consists of a carbonyl group joined to an alcohol.

Back 61

Carboxylic acids

Front 62

When carboxylic acids dissolve in water, they form these polyatomic ions.

Back 62

Carboxylate ions

Front 63

This is the common name for the two-carbon carboxylic acid.

Back 63

Acetic acid

Front 64

This is the common name for the one-carbon aldehyde.

Back 64

Formaldehyde

Front 65

This is the common name for the simplest of all the ketones.

Back 65

Acetone

Front 66

These are like carboxylic acids, except the OH is replaced by an N, and other atoms.

Back 66

Amides

Front 67

These compounds have fruity flavors and are derivatives of carboxylic acids.

Back 67

Esters

Front 68

This is the only important thioester in biological systems.

Back 68

Coenzyme A

Front 69

If the carboxylic acid group is joined to a very long R chain, these compounds result.

Back 69

Fatty acids

Front 70

Soaps are examples of these compounds

Back 70

Fatty acids and carboxylate salts

Front 71

These are compounds consisting of an N joined to a hydrocarbon.

Back 71

Amines

Front 72

These ions result when an amine gains a fourth bond.

Back 72

Ammonium ions

Front 73

These important compounds contain both a carboxylic acid group and an amine.

Back 73

Amides

Front 74

Many biological compounds have this group in which a phosphorus atom is surrounded by oxygens.

Back 74

Phosphates

Front 75

Energy transfer may occur in biological systems due to the properties of these functionalgroups.

Back 75

Phosphoanhydrides