Unit 2 Test

Question 1

combustion reaction

Answer 1

a reaction involving a substance (hydrocarbon) reacting w/ oxygen (O2) to produce (O2 + H2O)

Question 2

alkali metal reaction

Answer 2

alkali metals (group 1) react with water to produce hydrogen gas (H2) and hydroxide (OH-)

Question 3

halogen reactions

Answer 3

halogen (group 17) react w/ metals to form halides

Question 4

molarity (M)

Answer 4

the amount of solute (in moles) divided by the volume of solution (L)

Question 5

strong electrolyte

Answer 5

substances that completely dissociate into ions when they dissolve in water

Question 6

nonelectrolytes

Answer 6

do not dissociate into ions when dissolved in water and do not conduct electricity

Question 7

weak electrolyte

Answer 7

only a few solute dissolve and ions are created, conducts electricity weakly

Question 8

acid

Answer 8

a substance that produces hydrogen ion in water

Question 9

base

Answer 9

a substance that produces hydroxide ion in water

Question 10

what are the weak acids?

Answer 10

CHO2 (Formic acid), HC2H3O2 (Acetic acid), HF (Hydrofluoric acid)

Question 11

what is the weak base?

Answer 11

NH3 (ammonia)

Question 12

sulfide

Answer 12

S^2-

Question 13

In a gas forming reaction, what gas does sulfide (S^2-) evolve?

Answer 13

H_2S

Question 13

In a gas forming reaction, what gas and liquid do carbonates (CO_3^2-) and bicarbonates (HCO_3^1-) give off?

Answer 13

H2O (l), CO2 (g)

Question 14

Bicarbonate

Answer 14

HCO_3^1-

Question 14

bisulfite

Answer 14

HSO3^1-

Question 14

sulfite

Answer 14

SO3^2-

Question 15

Carbonate

Answer 15

CO_3^2-

Question 16

In a gas forming reaction, what gas and liquid do sulfites and bisulfites give off?

Answer 16

H2O (l), SO2 (g)

Question 17

ammonia

Answer 17

NH3^-

Question 18

In a gas forming reaction, what gas and liquid does ammonium give off?

Answer 18

H2O (l), NH3(g)

Question 19

What is the equivalence point in an acid-base titration?

Answer 19

the amount of titrant added is enough to neutralize the analyte solution, moles of base = moles of acid and the solution only contains water and salt

Question 20

What are the five rules for oxidation states?

Answer 20

1. Oxidation state of a free atom is 0.
2. Oxidation state of a monatomic ion is equal to its charge.
3. Sum of the oxidation states of all atoms in: a neutral molecule or formula unit is 0 and an ion is equal to the charge of the ion
4. Group 1A metrals always have a state of +1, Group 2A metals always have an oxidation state of +2
5. Follow the nonmetals chart.

Question 21

Oxidation state of fluorine:

Answer 21

-1

Question 22

Oxidation state of hydrogen:

Answer 22

+1

Question 23

Oxidation state of oxygen:

Answer 23

-2

Question 24

Oxidation state of Group 7A:

Answer 24

-1

Question 25

Oxidation state of 6A:

Answer 25

-2

Question 26

Oxidation state of 5A:

Answer 26

-3

Question 27

Oxidizing agent

Answer 27

a substance that causes the oxidation of another substance (oxidation number lowers between the reactant and product)

Question 28

Reducing agent

Answer 28

a substance that causes the reduction of another substance (oxidation number is higher between the reactant and product)

Question 29

Combination (synthesis) reaction

Answer 29

2 or more substance combine to form a single product

Question 30

Decomposition reaction

Answer 30

A single compound breaks down into 2 or more simpler substances

Question 31

Combustion reaction

Answer 31

A substance reacts with oxygen, producing heat and light

Question 32

Precipitation reaction

Answer 32

2 aqueous solutions form an insoluble solid (precipitate)

Question 33

Acid - Base reaction

Answer 33

An acid reacts with a base to produce salt and water

Question 34

Gas Forming reactions

Answer 34

reactions that produce a gas w one of the products

Question 35

redox

Answer 35

reactions where electrons are transferred between species, resulting a change in oxidation states

Question 36

Nitrate

Answer 36

NO3^1-

Question 37

Sulfate

Answer 37

SO4^2-

Question 38

Phosphate

Answer 38

PO4^3-

Question 39

Acetate

Answer 39

C2H3O2^1-

Question 40

Carbonate

Answer 40

CO3^2-

Question 41

energy

Answer 41

the capacity to do work

Question 42

work

Answer 42

the result of a force acting through a distance

Question 43

heat

Answer 43

the flow of energy caused by a temperature difference

Question 44

kinetic energy

Answer 44

the energy associated with the motion of an object

Question 45

thermal energy

Answer 45

the energy associated with the temperature of an object

Question 46

potential energy

Answer 46

the energy associated with the position or composition of an object

Question 47

chemical energy

Answer 47

the energy associated with the relative positions of electrons and nuclei in atoms and molecules

Question 48

law of conservation of energy

Answer 48

energy can neither be destroyed nor created

Question 49

1st law of theromynamics

Answer 49

total energy of the universe is constant

Question 50

internal energy

Answer 50

the sum of the kinetic energy and potential energy of al the particles that compose the system

Question 51

state function

Answer 51

a quantity, such as internal energy, whose value depends only on the state of the system, not on how it got there

Question 52

how many Joules in a cal?

Answer 52

1 cal = 4.184 J

Question 53

how many joules in a Cal?

Answer 53

1 Cal = 4184 J

Question 54

how many joules in a kwh?

Answer 54

3.60 * 10^6 J

Question 55

extensive property

Answer 55

a property that depends on the amount of a given substance

Question 56

intensive property

Answer 56

a property that is independent of an amount of a given substance

Question 57

when heat (q) is greater than 0 ...

Answer 57

heat absorbed (endothermic)

Question 58

when heat (q) is less than 0 ...

Answer 58

heat released (exothermic)

Question 59

when work (w) is greater than 0 ...

Answer 59

work done on the system

Question 60

when work (w) is less than 0 ...

Answer 60

work done by the system

Question 61

specific heat capacity

Answer 61

the amount of heat required to raise the temp of 1g of a substance by 1 C or 1K (J/g C)

Question 62

molar heat capacity

Answer 62

the amount of heat required to raise the temperature of 1 mole by 1 degrees Celsius

Question 63

in calorimetry, how do you find qcal?

Answer 63

qcal =Ccal * change in temp

Question 64

in calorimetry, how do you find qrxn

Answer 64

qrxn = -qcal

Question 65

enthalpy

Answer 65

a thermodynamic property that represent the total heat content of a system the sum of the internal energy and product of pressure and volume

Question 66

what should you know about enthalpy and its relationship with heat at constant pressure?

Answer 66

The heat given off or absorbed when a reaction is run at constant pressure is equal to the change in the enthalpy of the system.

Question 67

exothermic reaction

Answer 67

a reaction that released heat, q is neg, change in enthalpy is neg

Question 68

endothermic reaction

Answer 68

a reaction that absorbs heat, q is pos, change in enthalpy is pos

Question 69

standard enthalpy (delta H)

Answer 69

enthalpy change under standard condition

Question 70

standard enthalpy of formation(delta H_f)

Answer 70

enthalpy change for forming one mole of a compound from its elements in their standard states

Question 71

how do you find delta H reaction

Answer 71

sum of delta Hf (products) - sum of delta H_f (reactants)

Question 72

Hess's law

Answer 72

the total enthalpy change for a chemical reaction is the same regardless of the pathway by which the reaction occurs

Question 73

what are the monoprotic acids?

Answer 73

Hydrochloric acid (HCl) Nitric acid (HNO₃) Acetic acid (CH₃COOH) Hydrobromic acid (HBr) Hydroiodic acid (HI)

Question 74

what are the diprotic acids?

Answer 74

Sulfuric acid (H₂SO₄) Carbonic acid (H₂CO₃) Oxalic acid (H₂C₂O₄)

Question 75

what are the tripotic acids?

Answer 75

Phosphoric acid (H₃PO₄) Citric acid (C₆H₈O₇) Arsenic acid (H₃AsO₄)

Question 76

nitrite

Answer 76

NO2—