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CHEM1A > Midterm 1 > Flashcards

Midterm 1 Flashcards

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1
Q

Bicarbonate or Hydrogen Carbonate

A

HCO3–

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2
Q

Bisulfate or Hydrogen Sulfate

A

HSO4–

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3
Q

Bisulfite or Hydrogen Sulfite

A

HSO3–

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4
Q

Dihydrogen Phosphate

A

H2PO4–

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5
Q

Cyanide

A

CN–

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6
Q

Thiocyanate ion

A

SCN–

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7
Q

Hydride (when combined with group 1A and 2A metals)

A

H–

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8
Q

Perchlorate

A

ClO4–

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9
Q

Chlorate

A

ClO3–

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10
Q

Chlorite

A

ClO2–

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11
Q

Hypochlorite

A

ClO–

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12
Q

Bromate

A

BrO3–

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13
Q

Bromite

A

BrO2–

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14
Q

Hypobromite

A

BrO–

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15
Q

Periodate

A

IO4–

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16
Q

Iodate

A

IO3–

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17
Q

Nitrate

A

NO3–

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18
Q

Nitrite

A

NO2–

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19
Q

Hydroxide

A

OH–

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20
Q

Acetate

A

C2H3O2–

(Often written as CH3COO–)

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21
Q

Permanganate

A

MnO4–

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22
Q

Oxide

A

O2–

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23
Q

Sulfide

A

S2–

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24
Q

Carbonate

A

CO32–

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25
Sulfate
SO42–
26
Sulfite
SO32–
27
Chromate
CrO42–
28
Dichromate
Cr2O72–
29
Oxalate
C2O42–
30
Thiosulfate
S2O32–
31
Peroxide
O22–
32
Hydrogen Phosphate
HPO42–
33
Nitride
N3–
34
Phosphide
P3–
35
Phosphate
PO43–
36
Lithium
Li+
37
Sodium
Na+
38
Potassium
K+
39
Rubidium
Rb+
40
Cesium
Cs+
41
Copper
Copper (I): Cu+ Copper (II): Cu2+
42
Silver
Ag+
43
Ammonium
NH4+
44
Beryllium
Be2+
45
Magnesium
Mg2+
46
Calcium
Ca2+
47
Strontium
Sr2+
48
Barium
Ba2+
49
Zinc
Zn2+
50
Cadmium
Cd2+
51
Manganese
Manganese (II): Mn2+ Manganese (III): Mn3+
52
Iron
Iron (II): Fe2+ Iron (III): Fe3+
53
Cobalt
Cobalt (II): Co2+ Cobalt (III): Co3+
54
Nickel
Ni2+
55
Chromium:
Chromium (II): Cr2+ Chromium (III): Cr3+
56
Mercury
Mercury (II): Hg2+ Mercury (I): Hg22+
57
Tin
Tin (II): Sn2+ Tin (IV): Sn4+
58
Lead
Lead (II): Pb2+ Lead (IV): Pb4+
59
Aluminum
Al3+
60
Gallium
Ga3+
61
Titanium
Titanium (III): Ti3+ Titanium (IV): Ti4+
62
Arsenic
Arsenic (III): As3+ Arsenic (V): As5+
63
Solubility Rules: Soluble Ionic Compounds (name all)
1) All common compounds of Group 1A(1) ions (Li+, Na+, K+, etc.) - No exceptions 2) All common compounds of ammonium ion (NH4+) -- No exceptions 3) All common Nitrates (NO3-), acetates (CH3COO- or C2H3O2-) and perchlorates (ClO4-) -- No exceptions 4) All common chlorides (Cl-), bromides (Br-), and Iodides (I-) -- exceptions: Ag+, Pb2+, Cu+, Hg22+ 5) All common Flurides (F-) -- exceptions: PbF2 and fluorides of Group 2A(2) 6) All common sulfates (SO42-) -- exceptions: CaSO4, SrSO4, BaSO4, Ag2SO4,PbSO4
64
Solubility Rule Exceptions: All common compounds of Group 1A(1) ions (Li+, Na+, K+, etc.) are **SOLUBLE**, except:
No exceptions
65
Solubility Rule Exceptions: All common compounds of ammonium ion (NH4+) are **SOLUBLE**, except:
No exceptions
66
Solubility Rule Exceptions: All common Nitrates (NO3-), acetates (CH3COO- or C2H3O2-) and perchlorates (ClO4-) are **SOLUBLE**, except:
No exceptions
67
Solubility Rule Exceptions: All common chlorides (Cl-), bromides (Br-), and Iodides (I-) are **SOLUBLE**, except:
All common chlorides (Cl-), bromides (Br-), and Iodides (I-) are **SOLUBLE**, except: Ag+, Pb2+, Cu+, Hg22+
68
Solubility Rule Exceptions: All common Flurides (F-) are **SOLUBLE**, except:
All common Flurides (F-) are **SOLUBLE**, except: PbF2 and fluorides of Group 2A(2)
69
Solubility Rule Exceptions: All common sulfates (SO42-) are **SOLUBLE**, except:
All common sulfates (SO42-) are **SOLUBLE**, except: CaSO4, SrSO4, BaSO4, Ag2SO4,PbSO4
70
Solubility Rules: Insoluble Ionic Compounds
1) All common metal hydroxides -- Exceptions: Group 1(A) hydroxides and Ca(OH)2, Sr(OH)2 and Ba(OH)2 2) All common carbonates (CO32-) and phosphates (PO43-) -- Exceptions: Carbonates and Phosphates of Group 1A(1) and NH4+ 3) All common sulfides -- Exceptions: Sulfides of Group 1A(1), Group 2A(2), and NH4+
71
Solubility Rules Exceptions: All common metal hydroxides are **INSOLUBLE**, except:
All common metal hydroxides are **INSOLUBLE**, except: -- Exceptions: Group 1(A) hydroxides and Ca(OH)2, Sr(OH)2 and Ba(OH)2
72
Solubility Rules Exceptions: All common carbonates (CO32-) and phosphates (PO43-) are **INSOLUBLE** except:
All common carbonates (CO32-) and phosphates (PO43-) are **INSOLUBLE** except: Carbonates and Phosphates of Group 1A(1) and NH4+
73
Solubility Rules Exceptions: All common sulfides are **INSOLUBLE**, except:
All common sulfides are **INSOLUBLE**, except: Sulfides of Group 1A(1), Group 2A(2), and NH4+
74
Name the Strong Acids:
1) Hydrochloric Acid, HCl 2) Hydrobromic Acid, HBr 3) Hydriodic Acid, HI 4) Nitric Acid, HNO3 5) Sulfuric Acid, H2SO4 6) Perchloric Acid, HClO4
75
Name the Strong Bases:
Group 1A(1) Hydroxides: 1) Lithium Hydroxide: LiOH 2) Sodium Hydroxide: NaOH 3) Potassium Hydroxide: KOH 4) Rubidium Hydroxide: RbOH 5) Cesium Hydroxide: CsOH Heavy Group 2A(2) Hydroxides: 6) Calcium Hydroxide: Ca(OH)2 7) Strontium Hydroxide: Sr(OH)2 8) Barium Hydroxide: Ba(OH)2
76
Metric System Prefix, name and value: P
Peta, 1015
77
Metric System Prefix, name and value: T
Tera, 1012
78
Metric System Prefix, name and value: G
Giga, 109
79
Metric System Prefix, name and value: M
Mega, 106
80
Metric System Prefix, name and value: k
Kilo, 103
81
Metric System Prefix, name and value: h
hecto, 102
82
Metric System Prefix, name and value: da
deca, 101
83
Metric System Prefix, name and value: d
deci, 10-1
84
Metric System Prefix, name and value: c
Centi, 10-2
85
Metric System Prefix, name and value: m
Milli, 10-3
86
Metric System Prefix, name and value: µ
micro, 10-6
87
Metric System Prefix, name and value: n
Nano, 10-9
88
Metric System Prefix, name and value: p
Pico, 10-12
89
Metric System Prefix, name and value: f
Femto, 10-15
90
Name the Scientist and Importance: Cathode Rays
Thompson used cathode rays and discovered that atoms can be divided into smaller particles.
91
Name the Scientist and Importance: Gold Foil
Rutherford used the gold-foil experiment to discover the nucleus of the atom.
92
Name the Scientist and Importance: Oil Drops
Millikan used the oil-drop experiement to determine the charge of a single electron.
93
Give the greek numerical prefix 1-10:
**mono- 1 di- 2 tri- 3 tetra- 4 penta- 5 hexa- 6 hepta 7 octa- 8 nona- 9 deca- 10**
94
In the case where a metal ion has multiple charges, the charge on the metal ion (oxidation number) is indicated in the name by using a Roman numeral, inside parentheses, after the name of the metal. The Roman numeral is considered to be part of the name of the ion and is required. Alternatively, we can add the suffix -ic or -ous, how are these divided?
- ous goes to the ion with the lower charge - ic goes to the ion with the higher charge e. g. Fe2+ is ferrous and Fe3+ is ferric
95
Naming Conventions: Binary Acids
These acids are composed of hydrogen and another nonmetal. The name of the acid is derived from the name of the parent anhydrous compound by using the following general rules: a. The word hydrogen is replaced with the prefix hydro-. b. The suffix -ide is replaced with -ic. c. The word acid is added. E.G. HCl is Hydrogen Chloride. HCl(aq) is Hydrochloric Acid. H2S is Hydrogen Sulfide. H2S(aq) is Hydrosulfuric Acid.
96
Oxoanions (sulfate, carbonate, etc.) prefixes, per-ATOM-ate, ATOM-ate, ATOM-ite, HPO-ATOM-ite -- how do these go?
per-ATOM-ate = largest number of oxygens in an oxyanion in 4 verions. ATOM-ate = the second largest in a oxoanion with 4 verions, or largest in an oxyanion with 2 ATOM-ite = second smallest in an oxoanion with 4 versions, or smallest in oxyanion with 2. hypo-ATOM-ite = smallest in an oxoanion with 4 verions.
97
Naming Conventions: Oxo-acids
These are acids that contain oxoanions. The name of the acid is derived from the name of the oxoanion by using the following general rules: a. When the name of the oxoanion ends in -ate, replace the -ate with -ic. When the name of the oxoanion ends in -ite, replace the -ite with -ous. b. The word acid is added. c. Prefixes hypo- and per- are retained. E.G Sulfate (SO42–) --\> H2SO4(aq) is Sulfuric Acid. Sulfite (SO32–) --\> H2SO3(aq) is Sulfurous Acid. Hypochlorite (ClO–) --\> HClO(aq) is Hypochlorous Acid.
98
Naming Convenions: Hydrates
name of anhydrous compound followed by greek number prefix + hydrate E.G. CuCl2•2H2O or CuCl2(H2O)2 = Copper(II) Chloride Dihydrate
99
Rules for Assigning an Oxidation Number
**General Rules:** 1. For an atom in its elemental form (Na, O2, Cl2, etc.) O.N. = 0 2. For a monatomic ion, O.N. = ion charge 3. The sum of O.N. numbers for a compound equals zero. The sum of O.N. values for a polyatomic ion equals the ion's value. **Rules for Specific Atoms:** 1. For Group 1A(1): O.N. = +1 in all compounds 2. For Group 2A(1): O.N. = +2 in all compounds 3. For Hydrogen: O.N. = +1 in combination with nonmetals, -1 in combination with metals 4. For Fluorine: O.N. = -1 in all combinations 5. For Oxygen: O.N. = -1 in peroxides, -2 in all other compounds (except withF) 6. For Group 7A(17): O.N. = -1 in combination with metals, nonmetals (except O), and other halogens lower in the group.

CHEM1A (2 decks)

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