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General Chemistry 111 > Chapter 4 > Flashcards

Chapter 4 Flashcards

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1
Q

what are solutions composed of (2 things)

A
  • solutes

- solvents

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2
Q

solutes

A

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

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3
Q

solvent

A

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

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4
Q

solution

A

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

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5
Q

covalent bond

A

a bond made between atoms that are sharing their electrons

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6
Q

non-polar covalent bond

A

the electrons in the atoms are being evenly distributes

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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

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8
Q

why is water a powerful solvent

A

water is polar, making it a powerful solvent

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9
Q

hydration

A

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

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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
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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
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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
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13
Q

non-electrolyte

A

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

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14
Q

electrolyte

A

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

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15
Q

strong electrolyte

A

100% dissociation

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16
Q

weak electrolyte

A

not completely dissociated

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17
Q

non-electrolyte

A

no cations or anions in the solution

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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
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19
Q

soluble

A

dissolves, aqueous

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20
Q

insoluble

A

does not dissolve, solid

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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

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22
Q

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

A

AgNO3, NaCl, NaNO3

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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

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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

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25
Q

net ionic equation

A

an equation in which spectator ions are omitted. it shows the reaction that actually occurs at the ionic level

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26
Q

brief summary of writing net ionic equations (5 steps)

A
  • 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
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27
Q

the 3 main types of chemical reactions

A
  • precipitation
  • acid-base reactions
  • oxidation-reduction reactions
28
Q

precipitation reactions

A
  • a solid ionic substance forms from the mixture of 2 solutions of ionic substances
  • precipitate (insoluble solid that separates from solution
29
Q

(Acid) base reactions

A
  • 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
Q

acid (base) reactions

A
  • have a bitter taste
  • feel slippery
  • hydroxide (-OH)
31
Q

arrhenius definition of acids and bases

A
  • 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
Q

bronsted and lowry definition of acids and bases

A
  • an acid donates a proton
  • a base accepts a proton
  • an acid must contaon at least 1 ionizable proton
33
Q

properties of ammonia

A

a weak base and a 2 arrow-equillibrium sign is used in equations because it doesn’t fully dissociate

34
Q

strong acid

A

ionizes completely in H2O (strong electrolyte)

35
Q

weak acid

A

partly ionizes in H2O (weak electrolyte)

36
Q

strong acids and strong bases on periodic table

A

group 1 and 2 hydroxides

37
Q

neutralization reaction

A
  • 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
Q

oxidation-reduction reactions

A
  • oxidized=lose e-

- reduction=gain e-

39
Q

Oxidation number

A

the charge of an atom or a hypothetical charge assigned to an atom in a molecule (or an ionic compound) using simple rules

40
Q

free elements

A

the oxidation number of an atom of an element is zero

41
Q

monotomic ions

A

the oxidation number is equal to the charge of the ion

42
Q

oxidation number of oxygen

A

is usually -2, in H2O and O2 it is -1

43
Q

oxidation number of hydrogen

A

in a compound is +1 except when it is bonded to metals in binary compounds, then it is -1

44
Q

oxidation numbers of group 1A and 2A metals

A 
1A= +1
2A= +2
45
Q

oxidation number of flourine

A

-1

46
Q

what is the sum of the oxidation numbers in all atoms equal to?

A

the charge on the molecule/ion

47
Q

what are the 5 common oxidation-reduction reactions

A
  • combination
  • decomposition
  • displacement
  • combustion
  • disproportionation
48
Q

combination reaction

A
  • 2 substances combine to form a third
  • A+B=C
  • 2Na + Cl2 = 2NaCl
49
Q

decomposition reaction

A
  • a single compound reacts to give 2 or more substances
  • C=A+B
  • 2HgO=2Hg + O
50
Q

displacement reactions

A
  • element reacts with a compound, displacing another element from it
  • A+BC=AC+B
  • Sr + 2H2O = Sr(OH2) + H2
51
Q

combustion reaction

A
  • substances react with oxygen and release heat/flame

- M + O2 = MO2

52
Q

Disproportionation reaction

A
  • simultaneously oxidized and reduced

- Cl2 + 2OH- = ClO- + Cl- + H2O

53
Q

how do we describe the concentration of a solution

A

the concentration of a solution is the amount of solute present in a given quantity of solvent or solution

54
Q

equation for molarity

A

molarity = moles of a solute/liter of solution

55
Q

dilution

A

the procedure for preparing a less concentrated solution from a more concentrated solition

56
Q

relationship between volume and molarity

A

as volume increases, molarity decreases

-MiVi=MfVf

57
Q

quantitative analysis

A

involves the determination of the amount of substance or species present in a material

58
Q

graviametric analysis

A

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
Q

what type of reaction is often used in graviametric analysis

A

precipitation reactions

60
Q

general procedure of graviametric analysis

A
  • 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
Q

volumetric analysis

A

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
Q

volumetric analysis is based on

A

titration

63
Q

titration

A

procedure for determining the amount of substance A by adding substance B until the reaction of B and A is complete

64
Q

general procedure for a titration

A

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
Q

equivalence point

A

the point at which the reaction is complete

66
Q

indicator

A

substance that changes color at (or near) the equivalence point

General Chemistry 111 (8 decks)

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