Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

General Chemistry 111 > Chapter 4 > Flashcards

Chapter 4 Flashcards

1
Q

what are solutions composed of (2 things)

A
  • solutes

- solvents

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

solutes

A

the substances present in smaller amounts, and the component that is dissolved

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

solvent

A

the substance present in a larger amount, and the component that is able to dissolve things

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

solution

A

a homogenous mixture of 2 or more substances, composed of a solvent and solutes

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

covalent bond

A

a bond made between atoms that are sharing their electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

non-polar covalent bond

A

the electrons in the atoms are being evenly distributes

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

polar covalent bond

A

when the pulling power of one atom is stronger, and the electrons are displaced closer to that atom than the other

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

why is water a powerful solvent

A

water is polar, making it a powerful solvent

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

hydration

A

the process by which an ion is surrounded by H2O molecules arranged in a specific manner

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

ionic theory of solutions (Arrhenius)

A 
certain substances (electrolytes and non-electrolytes) produce freely moving ions when they dissolve in water, and these ions conduct an electric
current in solution
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

theoretically, if an electric wire is dipped into a solution of NaCl, how will electricity be conducted

A
  • Na+ ions are attracted to the negative wire
  • Cl- ions are attracted to the positive wire
  • opposite charges allow an electrical current to flow through
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

what was the most important idea of Arrhenius’s ionic theory of solutions

A
  • salt and pure water do not conduct electricity BUT
  • once salts are dissolved in water, they are conductors
  • salt contains ions even in the absence of an electric current
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

non-electrolyte

A

a substance that, when dissolved, results in a solution that does not conduct electricity

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

electrolyte

A

a substance that, when dissolved in water, results in a solution that can conduct electricity

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

strong electrolyte

A

100% dissociation

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

weak electrolyte

A

not completely dissociated

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

non-electrolyte

A

no cations or anions in the solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

basics of solubility rules

A
  • substances vary in their solubility
  • compounds that dissolve readily are said to be soluble
  • compounds that dissolve very little are said to be insoluble
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

soluble

A

dissolves, aqueous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

insoluble

A

does not dissolve, solid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

molecular equation

A

a chemical equation in which the reactants and products are written as if they were molecular substances, even though they may actually exist in a solution as ions

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

examples of aqueous solutions that are written as compounds in molecular equations

A

AgNO3, NaCl, NaNO3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

molecular and ionic equations

A

a chemical equation in which strong electrolytes are written as separate ions in a solution is a complete ionic equation. other reactants and products are written in molecular form

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

spectator ion

A

an ion in an ionic equation that does not take part in the reaction. it appears as both a reactant and a product

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
net ionic equation
an equation in which spectator ions are omitted. it shows the reaction that actually occurs at the ionic level
26
brief summary of writing net ionic equations (5 steps)
- write balanced molecular equation - write the complete ionic equation showing the strong electrolytes - determine precipitate from solubility rules - cancel the spectator ions on both sides - write the net ionic form
27
the 3 main types of chemical reactions
- precipitation - acid-base reactions - oxidation-reduction reactions
28
precipitation reactions
- a solid ionic substance forms from the mixture of 2 solutions of ionic substances - precipitate (insoluble solid that separates from solution
29
(Acid) base reactions
- have a sour taste - react with certain metals to produce hydrogen gas - redox reactions (react with carbonates an bicarbonates to produce carbon dioxide gas
30
acid (base) reactions
- have a bitter taste - feel slippery - hydroxide (-OH)
31
arrhenius definition of acids and bases
- an acid is a substance that increases hydrogen ion concentration in water - a base is a substance that increases hydroxide ion concentration in water
32
bronsted and lowry definition of acids and bases
- an acid donates a proton - a base accepts a proton - an acid must contaon at least 1 ionizable proton
33
properties of ammonia
a weak base and a 2 arrow-equillibrium sign is used in equations because it doesn't fully dissociate
34
strong acid
ionizes completely in H2O (strong electrolyte)
35
weak acid
partly ionizes in H2O (weak electrolyte)
36
strong acids and strong bases on periodic table
group 1 and 2 hydroxides
37
neutralization reaction
- the chemical properties of acids and bases neutralize one another - a reaction of an acid and a base that results in an ionic compound (a salt) and water
38
oxidation-reduction reactions
- oxidized=lose e- | - reduction=gain e-
39
Oxidation number
the charge of an atom or a hypothetical charge assigned to an atom in a molecule (or an ionic compound) using simple rules
40
free elements
the oxidation number of an atom of an element is zero
41
monotomic ions
the oxidation number is equal to the charge of the ion
42
oxidation number of oxygen
is usually -2, in H2O and O2 it is -1
43
oxidation number of hydrogen
in a compound is +1 except when it is bonded to metals in binary compounds, then it is -1
44
oxidation numbers of group 1A and 2A metals
``` 1A= +1 2A= +2 ```
45
oxidation number of flourine
-1
46
what is the sum of the oxidation numbers in all atoms equal to?
the charge on the molecule/ion
47
what are the 5 common oxidation-reduction reactions
- combination - decomposition - displacement - combustion - disproportionation
48
combination reaction
- 2 substances combine to form a third - A+B=C - 2Na + Cl2 = 2NaCl
49
decomposition reaction
- a single compound reacts to give 2 or more substances - C=A+B - 2HgO=2Hg + O
50
displacement reactions
- element reacts with a compound, displacing another element from it - A+BC=AC+B - Sr + 2H2O = Sr(OH2) + H2
51
combustion reaction
- substances react with oxygen and release heat/flame | - M + O2 = MO2
52
Disproportionation reaction
- simultaneously oxidized and reduced | - Cl2 + 2OH- = ClO- + Cl- + H2O
53
how do we describe the concentration of a solution
the concentration of a solution is the amount of solute present in a given quantity of solvent or solution
54
equation for molarity
molarity = moles of a solute/liter of solution
55
dilution
the procedure for preparing a less concentrated solution from a more concentrated solition
56
relationship between volume and molarity
as volume increases, molarity decreases | -MiVi=MfVf
57
quantitative analysis
involves the determination of the amount of substance or species present in a material
58
graviametric analysis
a type of quantitative analysis in which the amount of a species in a material is determined by converting it into a product that can be isolated and weighed
59
what type of reaction is often used in graviametric analysis
precipitation reactions
60
general procedure of graviametric analysis
- dissolve unknown substance in water - react the unknown substance with a known substance that is a precipitate - filter and dry the precipitate - weigh precipitate - use the chemical formula and mass of precipitate to determine the amount of unknown ion
61
volumetric analysis
method for determining the amount of a particular substance based on measuring the volume of a solution of known concentration that is required to achieve a complete reaction
62
volumetric analysis is based on
titration
63
titration
procedure for determining the amount of substance A by adding substance B until the reaction of B and A is complete
64
general procedure for a titration
a solution of accuratley known concentration is added gradually to another solution of unknown concentration until the chemical reaction between the 2 solutions is complete
65
equivalence point
the point at which the reaction is complete
66
indicator
substance that changes color at (or near) the equivalence point

General Chemistry 111 (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions