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Introduction to Chemistry > chapter 6: Types of chemical reactions > Flashcards

chapter 6: Types of chemical reactions Flashcards

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1
Q

what is dissolution

A

When an ionic substance dissolves in water, the solvent pulls the individual ions from the crystal and solvates them

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2
Q

What is another name for dissolution?

A

dissociation

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3
Q

Why is an ionic salt soluble in water?

A

Because the interactions between ions and water are strong enough to overcome the lattice energy of the crystal

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4
Q

What does (aq) stand for

A

Aqueous solution

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5
Q

What does aqueous solution indicate

A

Hydration of the ions

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6
Q

Example of aqueous solution

A

NaCl —> (H2O) Na+ (aq) + Cl (aq)

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7
Q

What is a soluble compound

A

A substance that dissolves in water

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8
Q

What is insoluble compound

A

It does not dissolve in water

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9
Q

What do the differences in solubility of ionic compounds depend on

A

Attractions of the ions to one another and the attraction of the ions to the water molecules

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10
Q

what is a solution

A

homogenous mixture of 2 or more substances

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11
Q

what is a solvent

A

what does the dissolving

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12
Q

what is an aqueous solvent

A

water is the solvent

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13
Q

what is a solute

A

what is being dissolved

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14
Q

what is an electrolyte

A

dissociates into ions when dissolved in water

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15
Q

what is a nonelectrolyte

A

many dissolve in water but it does not dissociate

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16
Q

what does a material need to conduct electricity

A

charged particles

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17
Q

what is an electrolyte solution

A

all contain ions dissolved in water

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18
Q

what is a nonelectrolyte solution

A

contain whole molecules dissolved in water

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19
Q

what happens when strong electrolytes dissolve in water

A

dissociates completely

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20
Q

what happens when weak electrolytes dissolve in water

A

only partially dissociates

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21
Q

what types dissociate in water

A

strong electrolytes

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22
Q

strong electrolytes =

A

strong acids

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23
Q

what are strong acids

A

undergo ionization reactions to produce H+ ions and anions that are represented in balanced chemical equations

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24
Q

what are the 7 common strong acids

A
  1. ) sulfuric (H2SO4)
  2. ) hydrochloric (HCL)
  3. ) Hydrobromic (HBr)
  4. ) Perchloric (HClO4)
  5. ) Chloric (HClO3)
  6. ) Hydroiodic acid (HI)
  7. ) Nitric Acid (HNO3)
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25
Q

strong acids and bases are

A

soluble

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26
Q

what is a soluble ionic compound

A

strong electrolytes

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27
Q

What is a balanced equation

A

equation for a chemical reaction in which the number of atoms for each element in the reaction and the total charge is the same for both the reactants and the products

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28
Q

what are weak acids

A

only partially dissociate, so they only

produce a low concentration of ions in solution

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29
Q

what equilibrium arrow is used for weak acids and bases

A

the one where it goes in both directions to show that the reaction does not complete

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30
Q

what are weak bases

A

partially dissociate

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31
Q

what categories can electrolytes be in

A

ionic or molecular

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32
Q

what are some examples of ionic strong electrolytes

A

soluble salts and strong bases

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33
Q

what is an example of a ionic nonelectrolyte

A

insoluble salts

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34
Q

what is an example of a molecular strong electrolyte

A

strong acids

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35
Q

what is an example of a weak molecular electrolyte

A

weak acids and weak bases

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36
Q

what is an example of a molecular nonelectrolyte

A

all other compounds

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37
Q

what is concentration

A

designates the amount of solute
dissolved in a given quantity of solvent or quantity of
solution

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38
Q

what is molarity

A

one way to measure the concentration of

a solution

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39
Q

what is the formula for Molarity (M)

A

moles of solute/ volume of solution in liters

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40
Q

what is the first step for making a concentrated solution

A

one weighs out a known
mass (which can be convert to
number of moles) of the solute

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41
Q

what is the 2nd step for making a concentrated solution

A

solute is added to a
volumetric flask, and solvent is
added to the line on the neck of
the flask

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42
Q

what is a stock solution

A

Solutions that are used routinely
in the lab are often prepared (or
purchased)

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43
Q

what is diluted

A

Solutions of lower concentrations

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44
Q

what happens if a dilute solution contains the same volume as a concentration solution

A

the relationship between the amount of solute and solvent must be different

45
Q

how can someone dilute a concentrated solution

A

dilution

46
Q

how does dilution work

A

use a pipet to deliver a specific amount of the concentrated solution to a new volumetric flask
- add solvent until the line on the neck of the flask is reached

47
Q

what is the formula for dilution

A

molc=mold

Mc x Vc = Md x Vd

48
Q

what is a precipitation reaction

A

reactions that result in the formation of an insoluble product

49
Q

what is a precipitate

A

The insoluble

product

50
Q

what is solubility

A

amount of that
substance that dissolves in a given quantity of
solvent at a given temperature

51
Q

what are some soluble ionic compounds

A

Li+, Na+ K+, Cs+, Rb+, NH4+ (No exceptions)

52
Q

what are some soluble ionic compounds

A

NO3-, C2H3O2- (none exceptions)

53
Q

what are some soluble ionic compound

A

Cl-, Br-, I- (exceptions (Ag+, Hg2+2, Pb+2)

54
Q

what are some soluble ionic compounds

A

SO4-2 ( Ca+2, Sr+2, Ba+2, Ag+2, Hg+2, Pb+2,

55
Q

what are some insoluble ionic compoinds

A

S-2, OH-

56
Q

what are some insoluble ionic compounds

A

CO3-2, CrO4-2, PO4-3

57
Q

what is a molecular equation

A

shows the complete neutral
formulas and phases for each compound in the
aqueous reaction

58
Q

what is a complete ionic equation

A

all strong
electrolytes (strong acids, strong bases, and
soluble ionic salts) are dissociated into their ions

59
Q

what is another name for complete ionic equation

A

ionic equation

60
Q

what does an ionic equation show

A

accurately reflects the species that are found in the reaction mixture

61
Q

what is the net ionic equation

A

cross out anything
that does not change from the left side of the
equation to the right

62
Q

what are spectator ions

A

those that didn’t change (deleted from the net ionic equation)

63
Q

what is the other type of stoichiometry problem

A

molarity-molarity

64
Q

what are some characteristics of acids

A

have a sour taste.
−Can dissolve many metals
−Ability to neutralize bases

65
Q

what does the Latin word acidus mean

A

sour or tart

66
Q

what are some characteristics of bases

A

have a bitter taste

  • feel slipper to the touch
  • ability to neutralize acids
67
Q

where does the word base come from

A

english word which means to bring low

68
Q

who was svante arrhenius

A

(`1880)

- swedish chemist

69
Q

what was the arrhenius theory

A

acids are substances that increase the concentration of H+

bases are substances that increase the concentration of OH- when dissolved in water

70
Q

what are some problems with arrhenius theory

A

1.) does not explain why molecular substances like NH3 and Na2CO3, Na2O dissolve in water
(bc they do not contain OH-ions)
2.) does not explain why molecular substances like CO2 dissolve in water
(they do not contain H+ ions)
3.) it does not explain acid-base reactions that take place outside aqeuous solutions

71
Q

who were bronsted and lowry and what did they do

A

(1923)
- Johannes Bronsted was a danish chemist
-Thomas lowry was an English Chemist
they proposed a general definition of acids and bases

72
Q

what was the bronsted-lowry theory

A

acids are proton donors
(must have a removable proton)
bases are proton acceptors
(must have a pair of nonbonding electrons)

73
Q

what is a neutralization reaction

A

a solution of an acid and a solution of a base

are mixed

74
Q

what does a neutralization reaction between acid and metal hydroxide produce

A

water and a salt

75
Q

what is a salt

A

ionic compound whose cation comes from a base and the anion comes from an acid

76
Q

what does cation mean

A

to lose an electron

77
Q

what does anion mean

A

to gain electron

78
Q

what is a titration

A

analytical technique in which one can

calculate the concentration of a solute in a solution.

79
Q

what is standard solution

A

solution of a known concentration

80
Q

what does titration involve

A

combing sample of unknown w/ standard solution

81
Q

what is the equivalence point

A 
point at which the two 
different solutions (known and unknown) are at 
stoichiometrically equivalent quantities.
82
Q

what is used in acid-base titrations

A

indicators or dyes

83
Q

why is equivalence point never found

A

acid-base titrations dyes and instead the end point is found

84
Q

what reaction does precipitation, acid base, gas evolution rections involve

A

oxidation-reduction reaction

85
Q

what is an oxidation-reduction

A

Reactions that involve transferring electrons from one

atom to another

86
Q

what is oxidation

A

occurs when an

atom or ion loses electrons

87
Q

what is reduction

A

an

atom or ion gains electrons.

88
Q

when do redox reactions occur

A

in and out of solution

89
Q

what is an example of redox reaction

A

rusting iron, bleaching hair, producing electricity

90
Q

how can you determine if an oxidation-reduction reaction has occured

A

we assign an oxidation number

91
Q

what can oxidation number help us with

A

determine the electron flow in the reaction

92
Q

what are oxidations not

A

ion charges

93
Q

what is the first rule of oxidation numbers

A

free elements = 0

Na, Be, K, Pb

94
Q

in monatomic ions the oxidation number is equal to what

A

the charge on the ion
Li+ = +1
Fe+3 = +3

95
Q

Group IA metals have a charge of

A

+1

96
Q

Group 2A have a charge of

A

+2

97
Q

aluminum is always

A

+3

98
Q

what oxidation number do nonmetals have

A

negative

99
Q

what is the oxidation number of hydrogen

A

+1 but -1 when bonded to metals

100
Q

what is the oxidation number of O

A

-2

101
Q

what is exception for oxygen

A

H2O2 bc it is -1

102
Q

what oxidation numbers do halogens

A

-1

103
Q

what is the sum of the oxidation numbers in a neutral compound

A

0

example:NaCl

104
Q

what is the sum of the oxidation numbers on a polyatmic

A

The sum of the oxidation numbers in a polyatomic

ion is the charge on the ion

105
Q

when does oxidation occur

A

atoms oxidation increases during reaction

106
Q

when does a reduction occur

A

atoms oxidation state decreases during reaction

107
Q

oxidation and reduction must occur…

A

simultaneously

108
Q

what is a reducing agent

A

reduces an element in another
reactant is called the reducing agent.
- contains the element that is oxidized

109
Q

what is an oxidizing agent

A

The reactant that oxidizes an element in another
reactant
-contains the element is reduced

Introduction to Chemistry (12 decks)

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