Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

CHEM 119 > Unit 6: Aqueous Reactions > Flashcards

Unit 6: Aqueous Reactions Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

define solution

A

homogenous mixture of two or more substances

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what phases can solutions be in

A
  • liquid
  • solid
  • gas
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what is an example of a liquid solution

A

alloys

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

define solvent

A

substance present in the greatest quantity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

define solute

A
  • substances other than the solvent
  • solutes are said to be dissolved in the solvent
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

define aqueous solution

A

liquid solution in which the solvent is water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

what are molecular compounds composed of

A

nonmetals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

what happens to molecular compounds when dissolved in water

A

the molecules remain intact in the solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

what are ionic compounds composed of

A

a metal and a nonmetal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what happens to ionic compounds when dissolved in water

A

the atoms dissociate to form ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

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

A

ionic interpretation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

which salts are always soluble

A

sodium salts are always soluble

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

define electrolyte

A

a substance that conducts electricity when dissolved in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

define non-electrolyte

A

a substance that does not conduct electricity when dissolved in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

define strong electrolytes

A
  • exist completely or nearly completely as ions in a solution
  • completely dissociate into ions when dissolved in water
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what are the strong electrolytes

A
  • all soluble salts
  • all strong acids
  • all strong bases
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what are the weak electrolytes

A
  • all weak acids
  • all weak bases
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

would strong electrolytes be considered soluble or insoluble

A

soluble

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

define precipitate

A

insoluble compound that forms during a reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
Q

define spectator ions

A
  • ions that do not participate in a reaction
  • exist in the same form before and after the reaction
26
Q

are spectator ions included in total ionic equations

A

yes

27
Q

are spectator ions included in net ionic equations

A

no

28
Q

describe how to write total ionic equations

A
  • start with molecular equation
  • rewrite all aqueous (soluble) compounds into their ion form
  • solid compounds stay as solid compounds
29
Q

describe how to write net ionic equations

A
  • 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
Q

which type of equation best describes a precipitation reaction

A

net ionic equation

31
Q

how do you determine if a precipitate has formed

A
  • 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
Q

can you write a net ionic equation for a reaction where no precipitate forms (all compounds are soluble)

A
  • not really
  • the total ionic equation would be written and all ions would be spectator ions
  • no reaction has occurred
33
Q

what are the 7 strong acids

A
  • HCl
  • HBr
  • HI
  • HNO3
  • HClO4
  • H2SO4
34
Q

what are the 3 soluble strong bases

A
  • LiOH
  • NaOH
  • KOH
35
Q

define acid

A

substance that produces H+ when dissolved in water

36
Q

define strong acids

A
  • dissociate completely in solution
  • strong electrolytes
37
Q

define weak acids

A
  • barely dissociates in solution
  • weak electrolytes
38
Q

define base

A

substance that produces OH- when dissolved in water

39
Q

define strong bases

A
  • dissociate completely in solution
  • strong electrolytes
40
Q

define weak bases

A
  • produce very little OH- in solution (barely dissociate)
  • weak electrolytes
41
Q

what is the general equation for acid-base reactions

A

strong acid + strong base –> water + soluble ionic compound

42
Q

what is the difference between dissolving and dissociating

A
  • dissolving is when molecules are still bonded and are just dispersed through water molecules
  • dissociating is when molecules separate and form ions
43
Q

what is the oxidation state of atoms in their elemental form (H2, Fe)

A

0

44
Q

what is the oxidation state of monoatomic ions (H+, S2-)

A

equal to the charges of the ions

45
Q

describe the relationship between atoms oxidation states in a neutral molecule (H2O)

A

the sum of the oxidation states of all atoms in a neutral molecule is 0

46
Q

describe the relationship between atoms oxidation states in a polyatomic ion (NO3-)

A

the sum of the oxidation states of all atoms in an ion is equal to the charge of the ion

47
Q

what is the oxidation state of all atoms in group 1

A

1+

48
Q

what is the oxidation state of all atoms in group 2

A

2+

49
Q

what is the oxidation state of all atoms in group 6

A

2-

50
Q

what is the oxidation state of all atoms in group 7

A

1-

51
Q

which atoms should you assign oxidation states to first

A
  • H+ and O2-
  • if neither are present, look for any group 1, 2, 6, or 7 atom
52
Q

define oxidation-reduction reactions

A
  • 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
Q

define oxidation

A
  • loss of electrons
  • increase in charge
54
Q

define reduction

A
  • gain of electrons
  • decrease (reduction) in charge
55
Q

what referring to which atom/molecule is being oxidized or reduced, which side of the chemical equation are you looking at

A
  • 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
Q

define oxidizing agent

A
  • the species that is reduced
  • gaining electrons/reducing charge
57
Q

define reducing agent

A
  • the species that is oxidized
  • losing electrons/increasing charge
58
Q

how do you determine moles from volume and molarity

A

volume (L) * M(mol/L) = mol

CHEM 119 (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions