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CHEM 119 > Unit 6: Aqueous Reactions > Flashcards

Unit 6: Aqueous Reactions Flashcards

1
Q

define solution

A

homogenous mixture of two or more substances

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2
Q

what phases can solutions be in

A
  • liquid
  • solid
  • gas
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3
Q

what is an example of a liquid solution

A

alloys

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4
Q

define solvent

A

substance present in the greatest quantity

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5
Q

define solute

A
  • substances other than the solvent
  • solutes are said to be dissolved in the solvent
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6
Q

define aqueous solution

A

liquid solution in which the solvent is water

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7
Q

what are molecular compounds composed of

A

nonmetals

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8
Q

what happens to molecular compounds when dissolved in water

A

the molecules remain intact in the solution

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9
Q

what are ionic compounds composed of

A

a metal and a nonmetal

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10
Q

what happens to ionic compounds when dissolved in water

A

the atoms dissociate to form ions

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11
Q

what does the molecular interpretation of a solution look like; use the example of NaCl

A
  • the molecule in solid form –> the molecule in a solution (aqueous)
  • ions are NOT shown
  • NaCl (s) –> NaCl (aq)
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12
Q

what does the ionic interpretation of a solution look like; use the example of NaCl

A
  • the molecule in solid form –> the ions that have dissociated and their charges
  • ions are shown
  • NaCl (s) –> Na+ (aq) + Cl- (aq)
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13
Q

which interpretation is a more accurate/better interpretation of a solution: molecular or ionic

A

ionic interpretation

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14
Q

which salts are always soluble

A

sodium salts are always soluble

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15
Q

define electrolyte

A

a substance that conducts electricity when dissolved in water

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16
Q

define non-electrolyte

A

a substance that does not conduct electricity when dissolved in water

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17
Q

define strong electrolytes

A
  • exist completely or nearly completely as ions in a solution
  • completely dissociate into ions when dissolved in water
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18
Q

what are the strong electrolytes

A
  • all soluble salts
  • all strong acids
  • all strong bases
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19
Q

define weak electrolytes

A
  • solutes that exist in solution mostly in the form of molecules
  • only slightly dissociate into ions when dissolved in water
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20
Q

what are the weak electrolytes

A
  • all weak acids
  • all weak bases
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21
Q

would strong electrolytes be considered soluble or insoluble

A

soluble

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22
Q

define precipitate

A

insoluble compound that forms during a reaction

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23
Q

describe what happens molecularly in a precipitation reaction

A
  • the ions in the reactant compounds exchange
  • the ions in both compounds “switch partners”
  • AgNO3 + KCl –> AgCl + KNO3
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24
Q

describe how to write molecular equations

A
  • determine the products of the reaction
  • balance the equation
  • determine the phase states of each compound by checking the solubility chart (soluble = aq, insoluble = s)
25
define spectator ions
- ions that do not participate in a reaction - exist in the same form before and after the reaction
26
are spectator ions included in total ionic equations
yes
27
are spectator ions included in net ionic equations
no
28
describe how to write total ionic equations
- start with molecular equation - rewrite all aqueous (soluble) compounds into their ion form - solid compounds stay as solid compounds
29
describe how to write net ionic equations
- start with total ionic equation - determine which ions are spectator ions (appear both before and after reaction) - remove the spectator ions from the equation
30
which type of equation best describes a precipitation reaction
net ionic equation
31
how do you determine if a precipitate has formed
- write the molecular equation - if an insoluble (s) product is formed, that is the precipitate - if all products are aqueous (aq), there is no precipitate
32
can you write a net ionic equation for a reaction where no precipitate forms (all compounds are soluble)
- not really - the total ionic equation would be written and all ions would be spectator ions - no reaction has occurred
33
what are the 7 strong acids
- HCl - HBr - HI - HNO3 - HClO4 - H2SO4
34
what are the 3 soluble strong bases
- LiOH - NaOH - KOH
35
define acid
substance that produces H+ when dissolved in water
36
define strong acids
- dissociate completely in solution - strong electrolytes
37
define weak acids
- barely dissociates in solution - weak electrolytes
38
define base
substance that produces OH- when dissolved in water
39
define strong bases
- dissociate completely in solution - strong electrolytes
40
define weak bases
- produce very little OH- in solution (barely dissociate) - weak electrolytes
41
what is the general equation for acid-base reactions
strong acid + strong base --> water + soluble ionic compound
42
what is the difference between dissolving and dissociating
- dissolving is when molecules are still bonded and are just dispersed through water molecules - dissociating is when molecules separate and form ions
43
what is the oxidation state of atoms in their elemental form (H2, Fe)
0
44
what is the oxidation state of monoatomic ions (H+, S2-)
equal to the charges of the ions
45
describe the relationship between atoms oxidation states in a neutral molecule (H2O)
the sum of the oxidation states of all atoms in a neutral molecule is 0
46
describe the relationship between atoms oxidation states in a polyatomic ion (NO3-)
the sum of the oxidation states of all atoms in an ion is equal to the charge of the ion
47
what is the oxidation state of all atoms in group 1
1+
48
what is the oxidation state of all atoms in group 2
2+
49
what is the oxidation state of all atoms in group 6
2-
50
what is the oxidation state of all atoms in group 7
1-
51
which atoms should you assign oxidation states to first
- H+ and O2- - if neither are present, look for any group 1, 2, 6, or 7 atom
52
define oxidation-reduction reactions
- reactions in which electrons are transferred from one reactant to another - the same atom has different oxidation states on the reactant and product side
53
define oxidation
- loss of electrons - increase in charge
54
define reduction
- gain of electrons - decrease (reduction) in charge
55
what referring to which atom/molecule is being oxidized or reduced, which side of the chemical equation are you looking at
- look at both sides to determine whether charges changes and electrons were transferred - the atom/molecule being reduced will be named as the one on the reactant side of the equation
56
define oxidizing agent
- the species that is reduced - gaining electrons/reducing charge
57
define reducing agent
- the species that is oxidized - losing electrons/increasing charge
58
how do you determine moles from volume and molarity
volume (L) * M(mol/L) = mol

CHEM 119 (8 decks)

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