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Chem 11 > Chapter 7 > Flashcards

Chapter 7 Flashcards

1
Q

def. Any part of a system that is uniform in composition and in properties, making it visually
distinct from the rest of the system

A

Phase

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2
Q

def. Refers to an individual substance and all the particles of that substance

A

Chemical species

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3
Q

def. A substance made up of only one chemical species, having only one type of particle
โ–ช Cannot be separated by physical means like filtration or distillation (i.e. without
breaking chemical bonds

A

Pure substance

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4
Q

Can a pure substance have multiple phases?

A

Yes

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5
Q

def. A substance made up of multiple chemical species, having more than one type of
particle
โ–ช Can be separated by physical means

A

Mixture

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6
Q

def. The simplest pure substance, made up of either:
โ–ช Individual, identical atoms (He, O, C, etc.)
โ–ช * โ€“ Molecules of identical atoms (homonuclear molecules โ€“ H2, O2, etc.)

A

element

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7
Q

def. o Made up of more than one element
o Can be made up of:
โ–ช Molecules (H2O) ๏ƒ  covalent compounds
โ–ช Ion pairs (NaCl) ๏ƒ  ionic compounds

A

compound

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8
Q

def. Describes a system made up of only one phase

โ–ช All parts of the system contain the same substances in the same proportions

A

homogeneous

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9
Q

def. Describes a system made up of more than one phase
โ–ช Different parts of the system contain either different substances or different
proportions

A

heterogeneous

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10
Q

def. A type of homogeneous mixture, having multiple chemical species in a single phase,
where one or more substances dissolve into another

A

solution

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11
Q

def. The part of the solution that exists in the smaller quantity โ€“ the minor component
โ–ช The part that is dissolving

A

solute

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12
Q

def. The part of the solution that exists in the greater quantity โ€“ the major component
โ–ช What the solute dissolves into

A

solvent

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13
Q

def. A type of heterogeneous mixture, containing multiple chemical species in multiple
phases, specifically insoluble solid particles that are large enough to settle out

A

suspension

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14
Q

def. A type of heterogeneous mixture, having microscopic (1 nm to 1000 nm) dispersed
insoluble particles suspended throughout another substance

A

colloid

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15
Q

def. A solution composed of a solute dissolved in water

A

aqueous solution

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16
Q

How are aqueous solutions represented in chemical equations?

A

(aq)

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17
Q

def. The number of moles of a substance contained in one litre of solution
โ–ช Expressed as mol/L or M

A

Molarity/ molar concentration

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18
Q

def. Describes the maximum amount of solute that will dissolve in a given amount of solvent
at a particular temperature
โ–ช Most often expressed as mass per unit of volume (g/L or g/100 mL)

A

solubility

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19
Q

def. Describes a solute that dissolves very poorly in a solvent, displaying low solubility
โ–ช Commonly defined as a solute whose molar solubility is less than 0.1 mol/L at
25 ยฐC

A

insoluble

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20
Q

def. Describes a solute that dissolves well in a solvent
โ–ช Commonly defined as a solute whose molar solubility is greater than 0.1 mol/L
at 25 ยฐC

A

soluble

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21
Q

def. The property of substances to mix and dissolve into each other in any proportion

A

miscibility

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22
Q

def. Refers to substances that arenโ€™t soluble and that do not mix in any proportion
โ–ช Water and oil do not dissolve into each other, producing two separate phases

A

Immiscible

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23
Q

def. Refers to substances that are mutually soluble, that will mix in any proportion
โ–ช Alcohol and water dissolve into each other, producing a single phase

A

Miscible

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24
Q

When does a precipitate form?

A

If the the reaction product is insoluble (low solubility)

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25
Q

def. A solution into which solute can still dissolve, as the solute has not yet reached the
maximum concentration for that solvent at that temperature

A

Unsaturated solution

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26
Q

def. A solution into which no more solute can dissolve, as the solute has reached the
maximum concentration for that solvent at that temperature

A

Saturated solution

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27
Q

def. A solution that contains more dissolved solute than the solvent can at that temperature
under normal circumstances

A

supersaturated solution

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28
Q

def. Describes a materialโ€™s tendency to repel water or to not mix with it

A

hydrophobic

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29
Q

def. Describes a materialโ€™s tendency to attract water or to mix with it

A

Hydrophilic

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30
Q

what three things must occur for a solute to dissolve?

A
  1. The soluteโ€™s particles must separate from one another
  2. The solventโ€™s particles must separate from one another
  3. The solute and solvent particles must mix together and attract each other
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31
Q

what happens when particles separate?

A

ionic solutes must overcome the electrostatic attraction of their ionic bonds, covalent solutes must overcome the intermolecular forces holding them together

32
Q

In order for the soluteโ€™s particles to mix with those of the solvent there must be โ€ฆ.

A

enough space between the solventโ€™s particles

33
Q

If the forces holding the soluteโ€™s particles together are stronger than the other
two, then the solute________ is the most favourable outcome, and the solute _________

A

staying together, the solute wonโ€™t dissolve

34
Q

if the intermolecular forces within the solvent are stronger than the
other two, then the solventโ€™s particles ___________ is the most favourable
outcome, and the solute _______

A

staying together, the solute wonโ€™t dissolve

35
Q

If the forces that attract the soluteโ€™s particles to the solventโ€™s particles are
stronger than the other two, then the two _______ together is the most
favourable outcome and the solute _______

A

Mixing together, solute will dissolve

36
Q

A solute will only dissolve if the attractive forces between its particles and those of
the solvent are _________ than the forces within the solute or the solvent

A

as strong or stronger

37
Q

def. The attractive force that exists between the partial positive charge of one polar
molecule and the partial negative charge of another

A

dipole-dipole

38
Q

def. An electrostatic attraction that forms between
the partially positive hydrogen in a highly
polarized bond (usually Hโ€“N, Hโ€“O and Hโ€“F) and
the negative lone pair on a nearby atom

A

hydrogen bond

39
Q

def. A weakly attractive force that forms when nonpolar molecules gain temporary dipole
moments

A

london dispersion forcesq

40
Q

def. The separation of the component ions of an ionic compound when it dissolves in water

A

Dissociation

41
Q

def. A molecule that has an overall, or net dipole moment, because of its bond polarities and
its molecular geometry

A

Polar molecule

42
Q

def. An attractive force that forms between the partial charge of a molecular dipole moment
and an oppositely charged ion

A

ion-dipole force

43
Q

Polar solvents dissolve ionic and polar solutes because of either favourable _________
forces, favourable ________ bonding or favourable ________ forces

A

ion-dipole, hydrogen, dipole-dipole

44
Q

Nonpolar covalent solutes are only soluble in nonpolar covalent
solvents because of favourable __________ forces

A

London dispersion forces

45
Q

Why do soaps help clean?

A

One side is hydrophilic (polar) and the other is hydrophobic (non-polar)

46
Q

def. A solution of relatively high concentration

โ–ช A large amount of solute dissolved in the solvent

A

concentrated

47
Q

def. A solution of relatively low concentration

โ–ช A very small amount of solute dissolved in the solvent

A

dilute

48
Q

whats the formula for finding final concentration?

A

[๐Ÿ๐ข๐ง๐š๐ฅ] =
๐ฆ๐จ๐ฅ๐ž๐ฌ๐ญ๐จ๐ญ๐š๐ฅ/
๐ฏ๐จ๐ฅ๐ฎ๐ฆ๐ž๐ญ๐จ๐ญ๐šl

49
Q

def. The process of solvent molecules surrounding solute ions or molecules, in order to form
favourable ion-dipole or intermolecular forces

A

Solvation

50
Q

def. Refers to the process of solvation when the solvent is water

A

hydration

51
Q

def. An equation similar to a chemical equation that shows the separation of an ionic
compound into its component ions

A

Dissociation equation

52
Q

what do we use to describe the dissocation of ionic solutes?

A

dissociation equations

53
Q

def. An equation similar to a chemical equation that shows the breakup of a neutral
molecule into charged pieces

A

ionization equation

54
Q

whatโ€™s the difference between an ionization equation and a dissociation equation?

A

Dissociation equations start with ionic compounds, ionization equations start with covalent compounds

55
Q

the following is an example of what kind of equation?
NaCl(aq) โ€“> Na+
(aq) + Clโ€“
(aq)

A

Dissociation

56
Q 
the following is an example of what kind of equation? 
HCl(aq) --> H
\+
(aq) + Clโ€“
(aq)
A

Ionization equation

57
Q

_________ equations represent the separation of ionic compounds into ions that already
exist, while _________ equations represent covalent compounds that breakup to form ions

A

Dissociation, ionization

58
Q

def. A quantitative measure of a solutionโ€™s ability to conduct electricity, thanks to its ionic
content

A

conductivity

59
Q

___________ though most often referring to the flow of electrons,
actually refers to a flow of any charged particles, including ions

A

electrical current

60
Q

def. A substance that only partially dissociates or ionizes in solution, producing a solution
that conducts electricity, but only weakly

A

weak electrolyte

61
Q

def. A substance that completely, or almost completely, dissociates or ionizes in solution,
producing a solution that conducts electricity very well

A

strong electrolyte

62
Q

def. A substance that dissolves, but that doesnโ€™t dissociate or ionize, producing a solution
that does not conduct electricity

A

non-electrolyte

63
Q

what two mechanisms produce conductive solutions?

A

Ionization, dissociation

64
Q

def. A common laboratory technique that allows you to determine the unknown
concentration of a solution, by reacting it with a second solution whose concentration
you do know

A

titration

65
Q

def. The solution whose concentration you know

โ–ช Ends in โ€œtโ€ because you put it in the tube rather than in the flask

A

titrant

66
Q

def. The solution whose concentration you want to figure out

โ–ช Ends in โ€œdโ€ because you donโ€™t know its concentration and want to determine it

A

titrand

67
Q

def. A solution whose concentration you know relatively precisely

A

standardized solution

68
Q

def. An exothermic double replacement reaction between an acid and a base that always
produces a salt and water

A

neutralization

69
Q

what is this an example of?

HX(aq) + MOH(aq) โ€“> MX(aq) + H2O(l) + heat

A

neutralization

70
Q

What four things do we need to complete titration calculations?

A
  • stoichiometric mole ratio between the acid and the base
  • volume of the titrand
  • concentration of the titrant
  • the volume of your titrant
71
Q

What is the purpose of a titration?

A

to figure out how much titrant is needed to neutralise the titrand

72
Q

def. A piece of laboratory equipment designed for very accurate (four significant figures)
measuring and dispensing of a specific volume of solution

A

volumetric pipette

73
Q

def. A piece of laboratory equipment designed for very accurate (four significant
figures) measuring and dispensing of a variable volume of solution

A

burette

74
Q

def. The point in a titration at which the ratio of the moles of titrant to those of titrand is
identical to the ratio of their coefficients in the balanced chemical equation

A

equivalence point

75
Q

At the equivalence point, the contents of the flask have pH = ?

A

7

76
Q

def. A group of chemical compounds that change colour based on pH, when added in small
amounts to a solution

A

pH indicators

77
Q

def. The point in a titration at which the pH indicator changes colour, signaling the
titrationโ€™s end and the titrant volume you record

A

endpoint

Chem 11 (6 decks)

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