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General Chem I > Chapter 6 > Flashcards

Chapter 6 Flashcards

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1
Q

Is water polar or nonpolar?

A

polar molecule

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2
Q

What is the shape of water?

A

bent

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3
Q

What can water do that makes it so unique?

A

it can dissolve more substances than any other liquid

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4
Q

What happens when salts dissolve in water?

A

a hydration shell forms around the ions of a salt

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5
Q

What is the hydration process?

A

interaction between water molecules and charged ions

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6
Q

How do you write the chemical equation for hydration?

A 
H2O (l)
ionic compound (s/l/g) ----> + ion (aq)   + - ion (aq)
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7
Q

What is solubility?

A

amount of substance that can be dissolved in a solvent

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8
Q

What is a solute?

A

substance being dissolved

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9
Q

What is a solution?

A

substance doing the dissolving

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10
Q

What does the term “likes dissolves likes” mean?

A

non polar will dissolve with nonpolar and polar will dissolve with polar

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11
Q

What ion does water interact with?

A

hydroxide ions

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12
Q

why don’t oil and water mix?

A

oil is majority non-polar while water is polar

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13
Q

What part of oil can only interact with water?

A

the carboxyl group and the rest of the oil is a hydrocarbon chain that is nonpolar

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14
Q

What are aqueous solutions?

A

the substance is dissolved in liquid water

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15
Q

What is electrical conductivity?

A

the ability of a solution to conduct electricity

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16
Q

Does pure water conduct electricity?

A

no

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17
Q

What has to be added to water for it to conduct electricity?

A

ions and water together

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18
Q

What are electrolytes?

A

substances that produce a conductive solution when dissolved in water

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19
Q

What are strong electrolytes?

A

can completely ionic when dissolved in water

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20
Q

What kinds of bonds are typically found in strong electrolytes?

A

ionic and covalent

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21
Q

What are weak electrolytes?

A

partially dissociate/ionize in water

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22
Q

What is an example of a strong soluble salt?

A

NaCl

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23
Q

What is an example of a strong acid?

A

HCl

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24
Q

What is an example of a strong base?

A

NaOH

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25
Q

What is an example of a weak acid?

A

acetic acid

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26
Q

What is an example of a weak base?

A

ammonia

27
Q

What are nonelectrolytes?

A

do not ionize when dissolved in water

28
Q

What is an example of a nonelectrolyte?

A

ethanol (alchohol) and sucrose

29
Q

What forms around nonelectrolytes?

A

a hydration shell

30
Q

What is molarity?

A

the measure of concentration aka how many moles of a solute per liters of solution

31
Q

What is the formula for molarity

A

M = moles of a solute / L of a solution

32
Q

What are standard solutions?

A

have concentrations that are accurately known

33
Q

What is dilution?

A

process of adding water to a concentrated solution

34
Q

What are stock solutions?

A

concentrated solutions which are used to make less concentrated solutions

35
Q

What is the dilution formula?

A

M1V1 = M2V2 (molarity before diffusion times the volume before dilution equals the molarity after the dilution times the volume after the dilution)

36
Q

Does the amount of moles of solute change when diluting a stock solution?

A

NO

37
Q

How do you determine if a compound is a strong, weak, or nonelectrolyte

A

is it strong acid or base? means it is a strong electrolyte
is the ionic compound completely soluble? it is a strong electrolyte
if the first two criteria are not fulfilled to a certain extent, then it is a nonelectrolyte

38
Q

What is a precipitation reaction?

A

involves the formation of an insoluble substance when two solutions are mixed

39
Q

The solid that is formed during a precipitation reaction is called a what?

A

precipitate

40
Q

For a net ionic equation to happen, what has to be on the product’s side?

A

the insoluble product that forms a solid

41
Q

What are spectator ions?

A

ions that don’t participate in the reaction

42
Q

How do you write a net ionic equation?

A

Formula Equations (include chemical formulas and states)
Complete ionic equations (include all ionic species present)
Net ionic equations (remove spectator ions)

43
Q

In the solution base stoichiometry problems, what do you have to consider when products are formed?

A

the limiting reagent! (convert moles of reactant to moles of product and compare)

44
Q

What are acids?

A

H+ donors

45
Q

What are bases?

A

H+ acceptors

46
Q

In a net ionic equation involving bases, what should you consider?

A

OH making the water as a product

47
Q

What are acid-base reactions also called?

A

neutralization reactions

48
Q

What is titration?

A

adding a volume of known concentration

to the solution being analyzed

49
Q

What are oxidation-reduction reactions also called?

A

redox reactions

50
Q

What do redox reactions involve?

A

transfer of one or more electrons

51
Q

What are oxidation states?

A

(or numbers) allow us to keep track of

electrons during reactions

52
Q

An element alone has what oxidation state?

A

0

53
Q

What is the oxidation state of a monoatomic ion?

A

the same as its charge (ex: NaCl is +1 -1)

54
Q

What is the oxidation number for fluorine in COMPOUNDS always?

A

-1

55
Q

What is the oxygen oxidation state in compounds?

A

-2

56
Q

What is the oxidation state exception for oxygen?

A

-1 when talking about peroxide

57
Q

What is the oxidation state for hydrogen in compounds?

A

+1

58
Q

How do you know if a reaction is a redox reaction?

A

the oxidation numbers changed and the ions changed

59
Q

What is oxidation?

A

loss of electrons

60
Q

What is reduction?

A

gain of electrons

61
Q

What are oxidizing agents?

A

electron accepters

62
Q

What are reducing agents?

A

electron donors

63
Q

What is conserved in a redox reaction?

A

matter and energy

64
Q

How do you balance a redox reaction?

A

1) Write the unbalanced chemical equation (include states)
2) Determine oxidation states for all atoms
3) Show electrons gained/lost using “tie lines”
4) Use coefficients to equalize electrons gained/lost
5) Balance the rest of the equation using inspection

General Chem I (10 decks)

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