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Chemistry 101 > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

Coefficient

A

used to describe the quantity relationships between substances involved in a chemical equation

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2
Q

Mole ratio or mole bridge

A

Relationship between two component sin a balanced chemical equation

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3
Q

A+B —> C + D

How many grams of D made from Xg of A

A

Mass in g of A–>moles of a—>moles of D—->mass in g of D

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4
Q

how to find out if and how much of access there is

A

count out on dot diagram, must obey law of conservation by showing access

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5
Q

Theoretical yield

A

theoretical yield: stoichiometry

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6
Q

solution defintion

A

homogeneous mixture of 2+ solutions

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7
Q

2 different components of a solution

A

solvent- major component: water

Solute-minor component

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8
Q

aqueous solution

A

dissolved in water

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9
Q

color of CuSO4(s) vs color of CuSO4(aq)

A

blue-intensive

blue-extensive (depends on amount of waterCuSO4)

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10
Q

electrolyte

A

substance who’s solution (substance (aq)) contains ions and has the ability to conduct electricity

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11
Q

how to identify an electrolyte

A

look for ionic compounds (metal and non metal)

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12
Q

non elctrolyte

A

a substance who’s aqueous solution does not contain ions and therefore doesn’t conduct electrocution (coval

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13
Q

non elctrolyte

A

a substance who’s aqueous solution does not contain ions and therefore doesn’t conduct electrocution

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14
Q

how to identify a non electrolyte

A

covalent bond: 2 non metals

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15
Q

what happens to ions in a solution

A

solvent forms a cane around an ion because solvent (water) has partially polar ends and ions have charged ends

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16
Q

What happens in a solution with polyatomic ions

A

never break apart when in solution

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17
Q

what happens when you put a covalent compound in H2O

A
  1. solid dissolve in water: tend to have N,O, Halogen
  2. solids don’t dissolve (only C,H)
  3. Liquids that are Miscible: will mix
  4. Liquids that are immiscible (lots of C,H)
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18
Q

Miscible/immiscible

A

able to mix/unable to mix

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19
Q

electrolytes in Ionic compounds

A

Strong electrolytes: All, strong bases and salts, lots of ions in solution
Weak electrolyte: none, few ions in solution
Non electrolytes: none

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20
Q

electrolytes in Covalent compounds

A

Strong electrolytes: strong acids, lots of ions in solution
Weak electrolytes: weak acids, weak bases, few ions in solution
No electrolytes: almost all (every covalent molecule)

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21
Q

what certain types of molecules compounds don’t disassociate when mix with water

A

most important acid

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22
Q

Strong acids

A

strong electrolytes

  • only move one way through he reaction (one arrow)
  • completely dissociates
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23
Q

Weak acids

A

Weak electrolytes

  • moves both ways through equation, double arrow
  • partially disassociate
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24
Q

Strong acids

A
  1. HCl
  2. HBr
  3. HI
  4. HNO3
  5. H2SO4
  6. HClO4
  7. HClO3
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25
Q

Weak acids

A

H and anything else lol

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26
Q

Solubility of NO3-,CLO4-,Na+,K+,NH$+

A

Soluable

no exceptions

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27
Q

Solubility of Cl- and I-

A

Soluble except with Ag+, Hg22+,Pb2+

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28
Q

Solubility of SO42-

A

Soluble except with Ca2+,Ba2+,Sr2+,Hg,2+,Pb2+,Ag+

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29
Q

CO32- and PO43- solubility

A

insoluble except with Group 1A and NH4+

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30
Q

OH- solubility

A

Insoluble except with Group 1A, Ca2+,Ba2+,Sr2+

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31
Q

S2- solubility

A

insoluble except with Group 1A, 2A, and NH4+

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32
Q

Strong acids vs strong bases in terms of compounds and dissacociation

A

Strong acids: Covalent compounds fully dissacociate

Strong bases: Ionic compounds and always include NH-

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33
Q

Are Molecular (covalent) compounds) with OH

A

Pb2+ and Ca2+

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34
Q

exchange reaction

A

reaction in which cation from one reactant and the anion from the other reactant form a product

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35
Q

Two ionic compounds as reactants making two ionic compouns

A

make aqueous solution of ionic reactants

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36
Q

common strong acids

A 
Hydrochloric acid HCl
Hydrobromic acid HBr
Hydroiodic acid HI
Chloric acid HClO3
Perchloric acid HClO4
Nitric acid HNO3
Sulfuric acid (first proton) H2SO4
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37
Q

Strong bases

A

Group 1A metal hydroxides
(LiOH,naOH,kOH,RbOH,CsOH)
Heavy group 2A metal hydroxides
(Ca(OH)2,Sr(OH)2,Ba(OH)2

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38
Q

Precipitation reactions

A
  1. use reaction formulas to determine available ions
  2. switch partners; propose products
  3. check solubility rules
  4. balance equation
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39
Q

Molecular equation

A

balanced reaction shown without charges

AgNO3(aq)+NaCl(aq)–>AgCl(s)+NaNO3(aq)

40
Q

Complete ionic equations

A

balanced reactions shown with all aqueous solutions as ions

Ag+(aq) + NO3- (aq) +Na+ (aq) + Cl- (aq) –> AgCl(s) + Na+(aq) + NO2-(aq)

41
Q

Net ionic equation

A

balanced equation that does not predicate in product formation (without spectator ions)
Ag+(aq)+Cl-(aq)–>AgCL(s)

42
Q

Spectator ions

A

The ions which do not change state

43
Q

acids are

A

molecular compounds that ionize in water, produce H+ (hydrogen cation) proton donors

  1. strong acid completely disassociates h+ grabbed by H2O
  2. Weak acids partially disassociate H3O+ hydronium
44
Q

Basics reacting with water

A
  1. Ionic solids that dissolve in water, result of OH- in solution STRONG
  2. Molecular compounds react with water, result of reaction is OH- in solution, WEAK
45
Q

Note to remember about bases

A
  1. NaOH(s) –>(in H2O) –>Na+(aq) + OH- (aq)

2. NH3(l) –>in H2O

46
Q

monoprotic acids

A

1 reactant:1 H+ mole ratio

47
Q

Polyprotic

A

1 reactant: X H+ mole ratio

48
Q

Strong acids

A

Only one way, will not see any reactions in solution

49
Q

Weak acids

A

Both ways, see reactants and products in solution

-not all equally weak; more H+ you see the stronger the weak acid

50
Q

Strong Base

A

mOH,m(OH)2 heavy metal

51
Q

Weak bases

A

Look for “n” in molecular formulas

52
Q

Neutralization reaction

A

exchange reaction between acid and base

*note: some will relate gas if base contains CO32- carbonate

53
Q

Molarity (M)

A

describes solution concentrations

54
Q

M=

A

Moles/Liters

55
Q

Dilution

A

M1V1=M2V2

-Number of moles removed from concentrated solution is equal to number of moles put into dilute solution

56
Q

Solution stychiometry

A
  1. in solution you will be given volume, go to moles and use the mole bridge
  2. build a chemical reaction any time two different compounds are being discussed
57
Q

Neutral pH

A

H+=OH-

58
Q

Acid pH

A

H+>OH-

59
Q

Basic pH

A

H+

60
Q

[H+][OH-]=

A

1.0x10^-14

61
Q

pH=

A

-Log[H+]

62
Q

pH+pOH

A

14

63
Q

pOH=

A

-log[OH-]

64
Q

[OH-]=

A

10^-pOH

65
Q

H+=

A

10^-pH

66
Q

What is one of the most important properties of water

A

it has the ability to act as either an acid or a base

67
Q

K>1

A

Reaction is product forward

68
Q

K<1

A

Reaction is reaction forward

69
Q

Kw=

A

1.0x10^-14

70
Q

How to solve pH

A
  1. identify acid or base
  2. write what you expect
  3. what I the dissacoication of the chemical being discussed?
71
Q

Thermochemistry

A

energy chains accompanying chemical reactions

72
Q

Energy

A

capacity to do work or to transfer heat

73
Q

Work (w)

A

ability to move something

74
Q

Heat (q)

A

cause a temp change

  • remove heat: object cools
  • add heat: object warms
75
Q

Kinetic energy

A

energy of motion despite small size, atoms, and molecules have mass and motion. therefor they have kinetic energy

76
Q

Ek=

A

1/2mv^2 unites of Jules (j)

77
Q

potential energy

A

energy an objet has due to it’s position relative to other objects

78
Q

two types of potential energy

A
  1. Gravitational potential E: macro scale items

2. Elecrostatic potential E: Due to interactions between 2 charges particles

79
Q

Ee1=

A

(KQ1Q2)/d

Q1-charge 1
Q2-charge 2

80
Q

relationship between attraction and distance between particles

A

Opposites attracts as the distance between decreases, the attraction increases

81
Q

System

A

part you’re interested in: a chemical reaction that’ll take place (phase change or rxns)

82
Q

surroundings

A

literally everything else in the universe

83
Q

Three kinds of systems

A
  1. open-energy and matter can be transferred (coffee cup w no top)
  2. closed-Energy can be transferred matter not transfereed (cardboard cup with lid and sleeve)
    - -since matter not transferred just worry about energy
  3. isolated-energy nor matter can’t be transferred(yeti)
84
Q

transferring heat

A
  • cause temperature change
  • heat can be transferred from system to surrounding or from surrounding to system
  • if heat enters: endothermic
  • if heat leaves: exothermic
85
Q

Transferring work

A

when force moves an object

-work can be preformed on or by system

86
Q

first law of thermodynamics

A

-energy conserved
-E can be transferred in and out of a system, but the total E of the universe is constant
Euniverse=Esys+Esur

87
Q

The internal energy, E, of a system

A

add up every component of all kinetic and potential E of every piece of mater in system

  • motion of molecules; interactions b/t molecules
  • in any given atom you have motions and interactions b/t nuclei and electrons
88
Q

Change in E

A

Ef-Ei

89
Q

state of function=

A

delta E

90
Q

Delta E>0

A

system must gain energy from surroundings

91
Q

Delta E<0 system

A

must lose heat to surroundings

92
Q

what is so special about only having to quantify chang

A

Energy is both heat and work delta E=q+w

93
Q

loss of E of battery

A

W/coil: energy lost only as heat

w/fan: energy lost w heat and work

94
Q

Exothermic feels

A

warm to touch

95
Q

endothermic feels

A

cold to touch

96
Q

First law of thermodynamics

A

Reactants to products delta E<0 loss of E

Products to reactants delta E>0 gain of E

Chemistry 101 (4 decks)

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