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Chemistry R120 > Chapter 4 > Flashcards

Chapter 4 Flashcards

1
Q

What is an aqueous solution?

A

water is the solvent in the solution

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2
Q

What is a solution?

A

homogenous mixture of 2 or more substances

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3
Q

What is a solvent?

A

the substance that is present in the greatest amount in the solution

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4
Q

What is a solute?

A

all other substances in the solution that is dissolved by the solvent

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5
Q

What is an electrolyte?

A

substance that dissociates into ions when dissolved in water (solvent)

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6
Q

What is a non electrolyte?

A

substance that does NOT dissociate into ions when dissolved in water (solvent)

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7
Q

What is dissociation?

A

where water surrounds the separated ions

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8
Q

What is solvation?

A

when water molecules are solvating the ions to help stabilize them in solution and prevent them from recombining

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9
Q

What is a strong electrolyte?

A

one that dissociates COMPLETELY when dissolved in water (ie:NaCl)

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10
Q

What is a weak electrolyte?

A

one that dissociates PARTIALLY when dissolved in water (ie: acetic acid)

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11
Q

What is a precipitation reaction?

A

when 2 solutions containing soluble salts are mixed and produces a water-insoluble salt

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12
Q

What is a precipitation reaction also called?

A

“salting out”

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13
Q

What is a precipitate?

A

insoluble solid formed by a reaction in solution

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14
Q

What is solubility of a substance at a given temperature?

A

the amount of substance that can be dissolved in a given quantity of solvent

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15
Q

What is metathesis?

A

to transpose (exchange) the ions in the reactants compounds with each other

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16
Q

What is a metathesis reaction also called?

A

double replacement

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17
Q

What are the 6 ions that soluble ionic compounds must contain?

A

NO3- | CH3COO- | Cl- | Br- | I- | (SO4)2-

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18
Q

When are Cl-, Br-, and I- not soluble? When paired with which 3 cations?

A

Ag+ | Pb2+ | Hg2+

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19
Q

When is (SO4)2- not soluble? When paired with which 4 cations?

A

Sr2+ | Ba2+ | Hg2+ Pb2+

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20
Q

What are the 4 aniona that insoluble compounds contain?

A

S2- | OH- | (CO3)2- | (PO4)3-

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21
Q

When are S2- and OH- soluble? When paired with which 4 cations and which group?

A

NH4+ | Ca2+ | Ba2+ | Sr2+ | Group 1A cations

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22
Q

When are (CO3)2- and (PO4)3- soluble? When paired with which cation and which group?

A

NH4+ | Group 1A

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23
Q

What are the 3 ways to write a metathesis reaction?

A

molecular euqation | complete ionic equation | net ionic equation

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24
Q

What are the 3 steps to predicting whether or not a precipitate will form when electrolytes mix?

A

1) note the ions present | 2) consider the possible ionic combinations | 3) refer to the solubility guidelines

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25
Q

What is a molecular equation?

A

showing the complete chemical formulas of reactants and products

26
Q

What is a complete ionic equation?

A

all soluble strong electrolytes shown as ions

27
Q

What is a net ionic equation?

A

shows only the ions molecules directly involved in the reaction after spectator ions are cancelled

28
Q

What is an Arrhenius acid?

A

substances that increase the H+ concentration when dissolved in water

29
Q

What is an Arrhenius base?

A

substances that increase the OH- concentration when dissolved in water

30
Q

What is a Bronsted-Lowry acid?

A

proton DONORS

31
Q

What is a Bronsted-Lowry base?

A

proton ACCEPTORS

32
Q

What are mono-protic acids?

A

yields only 1 H+ per acid molecule

33
Q

What are diprotic acids?

A

yields 2 H+ per acid molecule

34
Q

What are the 7 strong acids?

A

HCl | HBr | HI | HNO3 | H2SO4 | HClO3 | HClO4

35
Q

What are the 3 strong bases and which group can strong bases come from?

A

Ca(OH)2 | Ba(OH)2 | Sr(OH)2 | Group 1A hydroxides

36
Q

What is a neutralization reaction?

A

reactions between an acid and a metal hydroxide produce a salt (ionic compound)

37
Q

What are RedOx reactions?

A

electrons transferred from one reactant to another

38
Q

What is oxidation? OIL

A

Loss of electrons

39
Q

What is reduction? RIG

A

Gain of electrons

40
Q

What are oxidation numbers?

A

oxidation states

41
Q

What oxidation numbers do atoms in their elemental form have (ie: H2)?

A

always 0 (neutral state)

42
Q

What oxidation numbers do monoatomic ions have (ie: Na+)?

A

its ionic charge (Na+ = +1)

43
Q

What oxidation number do nonmetals have?

A

usually negative, based on their valence electrons

44
Q

What oxidation number does oxygen have?

A

usually -2 | in peroxides = -1

45
Q

What oxidation number does hydrogen have?

A

usuallt +1 | bonded to metals = -1

46
Q

What oxidation number does fluorine have?

A

always -1

47
Q

What oxidation number do all other halogens have?

A

usually -1 | in oxyanions can be (+)

48
Q

What does the sum of oxidation numbers in a neutral compound must be?

A

0

49
Q

What does the sum of oxidation numbers in a polyatomic ion must be?

A

the charge of the ion

50
Q

What are displacement reactions?

A

ions oxidize an element, the ion in solution is being replaced (one is oxidized, other is reduced)

51
Q

What is a displacement reaction also called?

A

single displacement reaction

52
Q

What is teh activity series?

A

list of metals arranged from most easily oxidized to least

53
Q

What are active metals? Which groups are most reactive?

A

metals that react readily to form compounds | Group 1A and 2A metals

54
Q

What are noble metals? Which groups are noble metals?

A

very stable metals used to make jewelry and coins | Group 8B and 1B

55
Q

What is concentration?

A

amoubnt of solute dissolved in a given quantity of solvent or solution

56
Q

What is the equation for Molarity (M)?

A

moles of solute / L solution

57
Q

What are dilutions?

A

process where the concentrations of gaseous solutions are lowered by adding water into the solution

58
Q

What can the molarity of the diluted solution be determined by?

A

McVc = MdVd

59
Q

What is titration?

A

analytical technique in which one can calculate the concentration of a solute in a solution

60
Q

What is a standard solution?

A

solution of a known concentration

61
Q

What is a standard solution used for?

A

to determine the unknown concentration of another solution

62
Q

What is the equivalence point?

A

point at which stoichiometrically equivalent quantities are achieved and the reaction is complete

Chemistry R120 (18 decks)

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