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Chem U2 Atomic Structure and Properties > Unit 4 > Flashcards

Unit 4 Flashcards

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1
Q

What is a solution?

A

A homogenous mixture of two or more substances

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2
Q

What is an aqueous solution?

A

A solution that contains water as the solvent

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3
Q

What is a heterogenous mixture?

A

A mixture that contains two or more phases, for example oil and water

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4
Q

What is a solute?

A

A substance that is dissolved in a solvent and is present in lower amount

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5
Q

What is a solvent?

A

The component of a solution that is present in the greatest amount

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6
Q

What is concentration?

A

The ratio of quantity of solute to solvent in a solution

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7
Q

What is a concentrated solution?

A

A high ratio of solute to solution

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8
Q

What is a dilute solution?

A

A low ratio of solute to solution

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9
Q

What is an alloy?

A

A solution of two or more metals

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10
Q

What is an amalgam?

A

An alloy of mercury and other metals

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11
Q

The formation of most solutions depends on the strength of 3 types of interactions. What are they?

A

Solute-solute particles, solute and solvent particles, solvent-solvent particles

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12
Q

When a solution forms, which particles are attracted to which?

A

The particles of solute are attracted to the particles of solvent

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13
Q

Which interactions must be disrupted when a solution forms?

A

Solvent-solvent and solute-solute interactions

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14
Q

What is the process of dissolving?

A

1) Forces between solute particles are disrupted (this step requires energy)
2) Forces between solvent particles are disrupted (this step requires energy)
3) There is interaction between solute and solvent particles (this step gives off energy)

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15
Q

What is known as a universal solvent? Why is it called this?

A

Water; it is a polar molecule, with two dipoles, which allows it to dissolve many things; it undergoes hydrogen bonding with itself

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16
Q

What is hydration?

A

The process in which water molecules surround ions

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17
Q

What is dissociation?

A

The separation of individual ions from an ionic compound as it dissolves in water

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18
Q

Do all ionic compounds dissolve in water?

A

No, if the attraction between both ions in the compound is too strong, the compound won’t dissolve and the crystal stays together

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19
Q

Finish the sentence:

The greater the charge on each ion…

A

The less soluble the compound will be

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20
Q

What does miscible mean?

A

Liquids that mix with each other to form a solution

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21
Q

What does immiscible mean?

A

Liquids that do not readily mix to form a solution

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22
Q

What is a surfactant?

A

A compound with a non-polar hydrophobic part and also a polar hydrophilic part

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23
Q

What is electrical conductivity?

A

The ability to conduct electrical current

24
Q

What are strong, weak and nonelectrolytes?

A

Strong: many ions, great conductors
Weak: few ions, weak conductors
Nonelectronlytes: no ions, do not conduct at all

25
Q

What are strong bases?

A

They completely ionize in water to produce a metal cation (Na+) and a hydroxide anion (OH-)

26
Q

What is solubility?

A

The maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature

27
Q

What is an unsaturated solution?

A

A solution in which more solute can dissolve

28
Q

What is a saturated solution?

A

A solution that contains the maximum quantity of solute

29
Q

What is a supersaturated solution?

A

A solution that contains more than the maximum quantity of solute it should contain

30
Q

What does like dissolves like mean?

A

Solubility is favored when solute and solvent have similar properties

31
Q

What is Henry’s law?

A

The amount of gas dissolved in a solution is directly proportional to the pressure of the gas above the solution

32
Q

What is a solubility curve?

A

A graph of the solubility of a substance over a range of temperatures

33
Q

What is the rate of dissolving?

A

A measure of how quickly a solute dissolves in a solvent

34
Q

What is vapor pressure?

A

The pressure exerted by the vapor given off by a liquid

35
Q

What is Raoult’s Law?

A

It allows us to calculate the vapor pressure of solutions

36
Q

What do we call a solution that obeys Raoult’s Law?

A

An ideal solution

37
Q

What is a stock solution?

A

A concentrated solution that is used to prepare dilute solutions for actual use

38
Q

What is molar/amount concentration (c)?

A

The amount in moles of solute dissolved in 1 L of solution

39
Q

What is the equation for molar concentration?

A

Molar concentration = amount of solute in moles/volume of solution in litres

40
Q

What is a standard solution?

A

A solution for which the precise concentration is known

41
Q

What is percent (V/V)?

A

A ratio of the volume of solute to the volume of solution expressed as a percent

42
Q

What is percent (W/V)?

A

A ratio of the mass of solute (in grams) to the volume of solution (in mL) expressed as a percent

43
Q

What is percent (W/W) or mass percent?

A

A ratio of the mass of solute to the mass of solution expressed as a percent

44
Q

What is a mole fraction?

A

The ratio of the number of moles of a component divided by the total moles of solution

45
Q

What is molarity?

A

The number of moles of solute per kilogram of solvent

46
Q

What is normality?

A

The number of equivalents per liter of solution

47
Q

What is the dilution equation?

A

C1V1 = C2V2

48
Q

What are the steps to make a standard solution from a solid solute?

A

1) measure the amount of solid solute using a balance
2) dissolve the solute in water in a volumetric flask
3) add more water to the desired final volume
4) mix the solution
5) transfer solution to a WHMIS labeled container

49
Q

What is a strong acid?

A

An acid that ionizes completely in water to form hydrogen ions

50
Q

What is a weak acid?

A

An acid that partially ionizes in a water solution

51
Q

What is a strong base?

A

An ionic substance that (according to Arrhenius) dissociates completely in water releasing hydroxide ions

52
Q

What is a weak base?

A

A base that produces few hydroxide ions in water

53
Q

What are acidic oxides?

A

Non-metal oxides form acids in water; their covalent bonds do not break apart in water

54
Q

What are basic oxides?

A

Metal oxides form bases in water; their ionic bonds that dissociate in water

55
Q

What is a Lewis acid?

A

An electron pair acceptor

56
Q

What is a Lewis base?

A

An electron pair donor

57
Q

What is a pH scale?

A

A scale named after the “potency of Hydrogen” used to describe the acidity or basicity of a solution

Chem U2 Atomic Structure and Properties (4 decks)

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