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Gen Chem > Unit 2 Test > Flashcards

Unit 2 Test Flashcards

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1
Q

combustion reaction

A

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

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2
Q

alkali metal reaction

A

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

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3
Q

halogen reactions

A

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

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4
Q

molarity (M)

A

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

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5
Q

strong electrolyte

A

substances that completely dissociate into ions when they dissolve in water

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6
Q

nonelectrolytes

A

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

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7
Q

weak electrolyte

A

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

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8
Q

acid

A

a substance that produces hydrogen ion in water

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9
Q

base

A

a substance that produces hydroxide ion in water

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10
Q

what are the weak acids?

A

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

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11
Q

what is the weak base?

A

NH3 (ammonia)

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12
Q

sulfide

A

S^2-

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13
Q

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

A

H_2S

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13
Q

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

A

H2O (l), CO2 (g)

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14
Q

Bicarbonate

A

HCO_3^1-

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14
Q

bisulfite

A

HSO3^1-

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14
Q

sulfite

A

SO3^2-

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15
Q

Carbonate

A

CO_3^2-

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16
Q

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

A

H2O (l), SO2 (g)

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17
Q

ammonia

A

NH3^-

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18
Q

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

A

H2O (l), NH3(g)

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19
Q

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

A

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

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20
Q

What are the five rules for oxidation states?

A
  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.
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21
Q

Oxidation state of fluorine:

A

-1

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22
Q

Oxidation state of hydrogen:

A

+1

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23
Q

Oxidation state of oxygen:

A

-2

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24
Q

Oxidation state of Group 7A:

A

-1

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25
Q

Oxidation state of 6A:

A

-2

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26
Q

Oxidation state of 5A:

A

-3

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27
Q

Oxidizing agent

A

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

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28
Q

Reducing agent

A

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

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29
Q

Combination (synthesis) reaction

A

2 or more substance combine to form a single product

30
Q

Decomposition reaction

A

A single compound breaks down into 2 or more simpler substances

31
Q

Combustion reaction

A

A substance reacts with oxygen, producing heat and light

32
Q

Precipitation reaction

A

2 aqueous solutions form an insoluble solid (precipitate)

33
Q

Acid - Base reaction

A

An acid reacts with a base to produce salt and water

34
Q

Gas Forming reactions

A

reactions that produce a gas w one of the products

35
Q

redox

A

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

36
Q

Nitrate

A

NO3^1-

37
Q

Sulfate

A

SO4^2-

38
Q

Phosphate

A

PO4^3-

39
Q

Acetate

A

C2H3O2^1-

40
Q

Carbonate

A

CO3^2-

41
Q

energy

A

the capacity to do work

42
Q

work

A

the result of a force acting through a distance

43
Q

heat

A

the flow of energy caused by a temperature difference

44
Q

kinetic energy

A

the energy associated with the motion of an object

45
Q

thermal energy

A

the energy associated with the temperature of an object

46
Q

potential energy

A

the energy associated with the position or composition of an object

47
Q

chemical energy

A

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

48
Q

law of conservation of energy

A

energy can neither be destroyed nor created

49
Q

1st law of theromynamics

A

total energy of the universe is constant

50
Q

internal energy

A

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

51
Q

state function

A

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

52
Q

how many Joules in a cal?

A

1 cal = 4.184 J

53
Q

how many joules in a Cal?

A

1 Cal = 4184 J

54
Q

how many joules in a kwh?

A

3.60 * 10^6 J

55
Q

extensive property

A

a property that depends on the amount of a given substance

56
Q

intensive property

A

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

57
Q

when heat (q) is greater than 0 …

A

heat absorbed (endothermic)

58
Q

when heat (q) is less than 0 …

A

heat released (exothermic)

59
Q

when work (w) is greater than 0 …

A

work done on the system

60
Q

when work (w) is less than 0 …

A

work done by the system

61
Q

specific heat capacity

A

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

62
Q

molar heat capacity

A

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

63
Q

in calorimetry, how do you find qcal?

A

qcal =Ccal * change in temp

64
Q

in calorimetry, how do you find qrxn

A

qrxn = -qcal

65
Q

enthalpy

A

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

66
Q

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

A

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.

67
Q

exothermic reaction

A

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

68
Q

endothermic reaction

A

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

69
Q

standard enthalpy (delta H)

A

enthalpy change under standard condition

70
Q

standard enthalpy of formation(delta H_f)

A

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

71
Q

how do you find delta H reaction

A

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

72
Q

Hess’s law

A

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

73
Q

what are the monoprotic acids?

A

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

74
Q

what are the diprotic acids?

A

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

75
Q

what are the tripotic acids?

A

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

76
Q

nitrite

A

NO2—

Gen Chem (4 decks)

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