Chemistry I Second Exam

Front 1

Oxidation

Back 1

loss of electrons by one reactant

Front 2

Reduction

Back 2

gain of electrons by one reactant

Front 3

In oxidation the electrons appear as...

Back 3

a product

Front 4

In reduction the electrons appear as...

Back 4

a reactant

Front 5

Oxidizing Agent

Back 5

accepts the electrons, is reduced.

Front 6

Reducing Agent

Back 6

substance that supplies the electrons, is oxidized

Front 7

Rules for Oxidation Numbers

Back 7

1. any free element is zero
2. any simple monatomic ion is equal to the charge on that ion
3. the sum of all the O numbers of the atoms must equal the charge
4. F = -1
5. H = +1
6. O = -2

Front 8

If the oxidation number is +3, what is the oxidation state?

Back 8

+3

Front 9

When a conflict in oxidation numbers appears...

Back 9

go with the lower numbered rule

Front 10

Oxidation

Back 10

is an increase in oxidation number

Front 11

Reduction

Back 11

is a decrease in oxidation number

Front 12

Ion-Electron Method

Back 12

1. divide into two half reactions
2. balance atoms other than H & O
3. balance O by adding H2O
4. balance H by adding H+
5. balance net charge by adding e-
6. make e- gain = e- loss, add 'em
7. cancel anything you can

Front 13

Additional Steps for Basic Solution

Back 13

8. add OH- to both sides so OH- = H+
9. combine H+ and OH-
10. cancel any H2O you can

Front 14

Non-oxidizing Acid

Back 14

acid in which the anion of the acid is a weaker oxidizing agent than H+ and is more difficult to reduce than H+ (example - HCl, H2SO4, H3PO4)

Front 15

Oxidizing Acid

Back 15

acid in which the anion of the acid is a stronger oxidizing agent than H+ (example - HNO3, hot, conc. H2SO4)

Front 16

The strongest oxidizing agent in a solution of a non-oxidizing acid is...

Back 16

H+

Front 17

Metal + Acid =

Back 17

hydrogen gas

Front 18

Kinetic Energy

Back 18

the energy an object has when it is moving. KE=1/2MV^2

Front 19

Potential Energy

Back 19

energy an object has that can be changed into kinetic energy, stored energy

Front 20

Chemical Energy

Back 20

the potential energy of a chemical. when a chem. reaction occurs, the chemical energy possessed by the substances involved changes, resulting in either an absorption or release of energy (heat or light)

Front 21

Factors that affect Potential Energy

Back 21

potential energy increases when objects that attract move apart, and decreases when they move toward each other. potential energy increases when objects that repel move toward each other, it decreases when they move apart.

Front 22

Law of Conservation of Energy

Back 22

energy cannot be created nor destroyed, it can only be changed from one form to another.

Front 23

Temperature

Back 23

of an object is proportional to the average kinetic energy of its particles. the higher the average KE the higher the temperature.

Front 24

Heat

Back 24

is energy that is transferred between objects caused by differences in their temperatures, also called thermal energy. always moves from high to low.

Front 25

One calorie =

Back 25

4.187 Joules (exactly)

Front 26

Internal Energy

Back 26

the sum of the energies for all the individual particles in a sample of matter

Front 27

Open System

Back 27

can gain or lose mass and energy across its boundary, the human body is an example.

Front 28

Closed System

Back 28

can absorb or release energy, but not mass, across its boundary. the mass of a closed system is constant, no matter what happens inside.

Front 29

Isolated System

Back 29

cannot exchange matter or energy with its surroundings.

Front 30

Adiabatic Processes

Back 30

processes that occur within an isolated system

Front 31

q=

Back 31

heat

Front 32

+q=

Back 32

heat gained

Front 33

-q=

Back 33

heat lost

Front 34

Exothermic

Back 34

reaction in which heat is a product

Front 35

Endothermic

Back 35

reactions that consume energy

Front 36

Heat of Reaction

Back 36

amount of heat absorbed or released in a chemical reaction

Front 37

Calorimeter

Back 37

device used to measure heat of reaction

Front 38

Pressure

Back 38

amount of force acting on a unit of area. pressure = force/area

Front 39

Atmospheric Pressure

Back 39

pressure exerted by the mixture of gases in our atmosphere

Front 40

1 atm

Back 40

= 14.696 lb/in.^-2 or 1.0133 bar

Front 41

First Law of Thermodynamics

Back 41

energy can neither be created nor destroyed. It can only change forms. in any process in an isolated system, the total energy remains the same. for a thermodynamic cycle the net heat supplied to the system equals the net work done by the system

Front 42

Second Law of Thermodynamics

Back 42

the entropy of an isolated system consisting of two regions of space, isolated from one another, each in thermodynamic equilibrium in itself, but not in equilibrium with each other, will, when the isolation that separates the two regions is broken, so that the two regions become able to exchange matter or energy, tend to increase over time, approaching a maximum value when the jointly communicating system reaches thermodynamic equilibrium.

Front 43

Third Law of Thermodynamics

Back 43

as temperature approaches absolute zero, the entropy of a system approaches a constant minimum

Front 44

Heat of Combustion

Back 44

heat produced by a combustion reaction, measured by a bomb calorimeter

Front 45

4.18 Joules

Back 45

amount of energy required to raise the temperature of 1g of H2O, 1 degree C. 4.18 is water's specific heat.

Front 46

q=

Back 46

(C)(∆T) + (S)(M)(∆T)

M*S*∆T

Front 47

∆T

Back 47

=T sub f - T sub i

Front 48

4.18 Joules

Back 48

amount of energy required to raise the temperature of 1g of H2O, 1 degree C. 4.18 is water's specific heat.

Front 49

q=

Back 49

(C)(∆T) + (S)(M)(∆T)

M*S*∆T

Front 50

∆T

Back 50

=T sub f - T sub i

Front 51

Third Law of Thermodynamics

Back 51

as temperature approaches absolute zero, the entropy of a system approaches a constant minimum

Front 52

Heat of Combustion

Back 52

heat produced by a combustion reaction, measured by a bomb calorimeter

Front 53

4.18 Joules

Back 53

amount of energy required to raise the temperature of 1g of H2O, 1 degree C. 4.18 is water's specific heat.

Front 54

Specific Heat

Back 54

amount of energy needed to raise 1g of a substance 1 degree C

Front 55

q=

Back 55

(C)(∆T) + (S)(M)(∆T)

M*S*∆T

Front 56

∆T

Back 56

=T sub f - T sub i

Front 57

Enthalpy

Back 57

a thermodynamic quantity equivalent to the total heat content of a system

Front 58

Manipulation of Thermochemical Equations

Back 58

1) when an equation is reversed—written in the opposite direction—the sign of ΔH° must also be reversed
2) formulas canceled from both sides of an equation must be for the substance in identical physical states
3) if all the coefficients of an equation are multiplied or divided by the same factor, the value of ΔH° must likewise be multiplied or divided by that factor

Front 59

Na + Cl

Back 59

yields NaCl, involves the loss of electrons by sodium (the oxidation of sodium) and the gain of electrons by chlorine (the reduction of chlorine). Chlorine is the oxidizing agent (accepts electrons), Sodium is the reducing agent (gives up electrons)

Front 60

Oxidation and Reduction Agents

Back 60

The oxidizing agent causes oxidation to occur by accepting electrons (it gets reduced). The reducing agent causes reduction by supplying electrons (it gets oxidized).

Front 61

Activity Series

Back 61

Au>Hg>Ag>Cu>H+>Pb>Sn>Co>Cd>Fe>Cr>
Zn>Mn>Al>Mg>Na>Ca>Sr>Ba>K>Rb>Cs

Front 62

Sodium's vigorous reaction with water is due to...

Back 62

it's ability to reduce the hydrogen in water molecules.

Front 63

Hydrocarbons

Back 63

compounds containing only carbon and hydrogen,

Front 64

Hydrocarbon + Plentiful O2

Back 64

yields CO2 and H2O

Front 65

Hydrocarbon + Limited O2

Back 65

yields CO and H2O

Front 66

Hydrocarbon + Extremely Limited O2

Back 66

yields elemental Carbon and H2O

Front 67

Exothermic Reaction

Back 67

any reaction in which heat is a product, or in which heat is emitted.

Front 68

Endothermic Reaction

Back 68

any reaction in which heat is a reactant, or in which heat is consumed.

Front 69

1 joule

Back 69

the amount of energy possessed by a 2kg object moving at 1m/s.

Front 70

Work

Back 70

is done by an object when it causes something to move.

Front 71

Internal Energy (E)

Back 71

sum of the energies for all the individual particles in a sample of matter

Front 72

(C)(∆T) + (S)(M)(∆T) = q

Back 72

the heat capacity times the change in temperature (∆T) plus the specific heat times the mass times the change in temperature equals heat (q)

Front 73

Heat Capacity

Back 73

heat capacity = mass * specific heat
C = MS

Front 74

State Function

Back 74

a property that depends only on an object's current state

Front 75

C (heat capacity) depends on...

Back 75

what the object is made of and the size of the object.

Front 76

Hydrocarbons and Heat

Back 76

Burning a hydrocarbon fuel produces one molecule of carbon dioxide for each carbon atom and one molecule of water for each pair of hydrogen atoms in the fuel. Generally, the more carbon and hydrogen atoms a molecule of the fuel contains, the more strong bonds can form when it burns—and the more heat it will produce, per molecule.

Front 77

∆H Significance

Back 77

if ∆H is positive, the reaction is endothermic.
if ∆H is negative, the reaction is exothermic

Front 78

Cellulose

Back 78

C6H10O5 repeated n times

Front 79

Combustion of Sulfur containing materials...

Back 79

results in SO2 as a product, which is the main contributor of acid rain