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Bio 20 > Chem 20 - Solutions > Flashcards

Chem 20 - Solutions Flashcards

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1
Q

Electronegativity

A

A atom’s ability to attract electrons, shown on the periodic table, more electronegative at the top right

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2
Q

Polar Molecule

A

A molecule that has a positive side and a negative side and is not symmetrical

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3
Q

What makes water a good solvent

A

Water molecules are polar so they are attracted to other polar molecules and ions. Water has positive and negative end allowing it to break apart (dissolve/dissociate) most ionic compounds

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4
Q

Why can some ionic compounds not be dissolved in water?

A

Some ionic compounds will not dissolve in water because the ionic bonds between the ion solute is too strong

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5
Q

2 major factors that are involved in the dissolving process

A
  1. Molecules tend to become more spread out

2. Energy is lost or gained

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6
Q

Why is dissolving a physical change and not a chemical change?

A

Because no new substance is formed right, and it is therefore reversible. Energy is still transferred because bonds are breaking and forming

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7
Q

Steps for dissolving

A
  1. The forces between the particles in the solute break (endothermic)
  2. Some intermolecular forces in the solvent break
    (endothermic)
  3. The attraction between the particles of solar and the particles of solvent result in the formation of new solute-solvent bonds (exothermic). In aqueous solutions this process is called hydration
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8
Q

How do you know if a solution is endothermic?

A

If more energy is absorbed to break the bonds than amount of energy released when the bonds are formed , the overall change is endothermic

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9
Q

How do you know if a solution is exothermic?

A

If more energy is released when the solute solvent bonds form than is required to dissolve the solvent, then the overall change is exothermic

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10
Q

Liquids that will dissolve in each other in all proportions, no matter how much solute or solvent exists

A

Miscible

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11
Q

Liquids that will not dissolve in other liquids at all

A

Immiscible

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12
Q

Solubility

A

the maximum amount of solute (mass) that will dissolve in a given amount of solvent (volume)

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13
Q

Dilute:

A

has a relatively small amount of solute compared with the amount of solvent (small concentration)

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14
Q

Concentrated:

A

has a relatively large amount of solute compared with the amount of solvent (large concentration)

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15
Q

Saturated solutions:

A

when no more solute cam be dissolved in a specific volume of solvent. you can tell a saturated solution because you will see a solid precipitate on the bottom of the container

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16
Q

factor that affects saturation levels

A

the higher the temperature the more solute can be dissolved in the same volume

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17
Q

is there a sharp dividing line between soluble and insoluble compounds?

A

no, there are degrees of solubility. even “insoluble compounds are slightly soluble in water

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18
Q

What is dynamic equilibrium?

A

it’s what happens when, at saturation, the solution appears not to be changing, but at the molecular level, ions crystallize at the same rate that solid crystals dissolve

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19
Q

Supersaturated solution:

A

when a saturated solution is prepared at high temperatures and cooled quickly, without crystals forming (solute undissolving). this supersaturated solution is unstable and introducing one crystal can easily start the crystallization process

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20
Q

Electrolytes definition

A

Electrolytes are solutions that conduct electricity. They must contain ions. Ex. acids, bases and ionic compounds in solution

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21
Q

Electrolyte (ionic) (salt). Will the lightbulb light up?

A

Yes, it will light up because it contains ions and therefore conducts electricity.

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22
Q

Non-Electrolyte (molecular) (sugar). Will the lightbulb light up?

A

No it will not light up because it doesn’t contain ions and therefore will not conduct electricity.

23
Q

Non-Electrolytes definition

A

solutions that do not conduct electricity because they do not contain ions. ex: molecular compounds and insoluble ionic compounds are non-electrolytes.

24
Q

how is conductivity measured?

A

conductivity is measured with a conductivity apparatus (with a light bulb) or an ohmmeter. If you are using a conductivity apparatus, if the light turns on, it is an electrolyte. If it doesn’t turn on, it is a non-electrolyte.

25
Q

bulb glowing bright=

A

strong electrolytes with lots of ions

26
Q

bulb glowing dim=

A

weak electrolytes with only a few ions

27
Q

most common solvent

A

water

28
Q

how to determine solubility with ionic solute

A

use solubility table to determine solubility in water

29
Q

non-polar substances dissolve in:

A

other non-polar substances

30
Q

polar substances dissolve in:

A

other polar substances

31
Q

solute with hydrogen bonds dissolve in:

A

hydrogen bonded solvents (ex. water)

32
Q

4 factors that affect the rate of dissolving

A
  1. Particle size (also affects the amount of solute that can dissolve)
  2. Temperature
  3. Nature of the particle
  4. Agitation/Stirring
33
Q

Three factors that affect the solubility of substances in a solvent

A
  1. Temperature
  2. Pressure
  3. Miscibility
34
Q

Effect of temperature on solubility of solids vs. liquids vs. gases

A

Solubility of a solid increases when temperature increases, solubility of liquid s unaffected by temperature change, solubility of a gas decreases when temperature increases

35
Q

Effect of pressure on solubility of solids vs. liquids vs. gases

A

Pressure change has little effect on solubility of both solids and liquids. Solubility of gas increases when pressure exerted on gas increases

36
Q

Dissociation

A

When the separation of ions occurs in compounds dissolved in water

37
Q

Dissociation Equation

A

Equation used to show an ionic compound breaking into ions in water. Like other chemical equations, needs to be balanced

38
Q

Strong Base

A

Ionic compound composed of hydroxide (OH) ions

39
Q

High solubility ionic compounds and bases:

A

dissociate into two ions when placed into water. The solvent (water) pulls apart the compound into its ions

40
Q

High Solubility Ionic Compound and Base Dissociation Equation

A

ionic compound (s) –>positive ion (cation) (aq) + negative (anion) (aq)

41
Q

Low solubility ionic compounds and bases:

A

will not dissociate or dissolve (very much) when placed into water and will form a precipitate

42
Q

Low Solubility Ionic Compound and Base Dissociation Equation

A

ionic compound (s) –> ionic compound (s)

43
Q

Strong Acids:

A

Ionize completely to produce hydrogen ions and an anion. This is shown as a hydrogen ions and a negative partner ion.

44
Q

Strong Acid Ionization Equation

A

Strong Acid (aq) –> H+ (aq) + Negative Anion (aq)

45
Q

Weak Acids:

A

Do not ionize completely in water (less than 50%). This is shown as whole molecules in solution even though they do ionize a small amount.

46
Q

Weak acid ionization equation

A

Weak Acid (aq) H+ (aq) + Negative Anion (aq)

47
Q

High solubility molecular compounds and elements:

A

dissolve in water but do not dissociate

48
Q

High solubility molecular compounds are:

A

H bonded compounds and sugars

49
Q

High solubility elements:

A

group 17 elements

50
Q

Low solubility molecular compounds and elements:

A

do not dissolve in water and do not dissociate (no H-bonds)

51
Q

High solubility molecular compounds/elements dissociation equation

A

High solubility molecular compound/element (s) –> high solubility molecular compound/element (aq)

52
Q

Low solubility molecular compounds dissociation equation

A

Low solubility molecular compound/elements (s) –> low solubility molecular compound/elements (s)

53
Q

Elements:

A

Are either atomic or molecular. They are never shown s ions. They may or may not be soluble in water. Some elements are molecular and some are atomic.

54
Q

Glucose

A

C12H606

Bio 20 (4 decks)

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