periodic table of the elements (used for grade 8 and high … › 2020 › 04 › ... ·...
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Periodic Table of the Elements (Used for Grade 8 and High School) California Science Test
Sodium 22.99
Na 11
Element symbol
* Element name
Hydrogen 1.01
H 1
Lithium 6.94
Li 3
Sodium 22.99
Na 11
39.10
19
K 58.69
Ni 28
Rubidium 85.47
Rb 37
140.91
Pr 59
(261)
Rf 104
95.94
Mo 42
(258)
Md 101
72.61
Ge 32
1 1A
2 2A
1
2
3
4
7 7B
11 1B
12 2B
13 3A
16 6A
8
5
6
7
9 8B
10
14 4A
15 5A
17 7A
18 8A
3 3B
4 4B
5 5B
6 6B
Copper 63.55
Cu 29
Cobalt 58.93
Co 27
Helium 4.00
He 2
Boron 10.81
B 5
Carbon 12.01
C 6
Nitrogen 14.01
N 7
Oxygen 16.00
O 8
19.00
F 9
Neon 20.18
Ne 10
26.98
Al 13
Silicon 28.09
Si 14
30.97
P 15
Sulfur 32.07
S 16
35.45
Cl 17
Argon 39.95
Ar 18
Calcium 40.08
Ca 20
Scandium 44.96
Sc 21
Titanium 47.87
Ti 22
Chromium 52.00
Cr 24
Iron 55.85
Fe 26
Zinc 65.39
Zn 30
Gallium 69.72
Ga 31
Arsenic 74.92
As 33
Selenium 78.96
Se 34
Bromine 79.90
Br 35
83.80
Kr 36
Strontium 87.62
Sr 38
88.91
Y 39
Zirconium 91.22
Zr 40
Niobium 92.91
Nb 41
(98)
Tc 43
Ruthenium 101.07
Ru 44
Rhodium 102.91
Rh 45
106.42
46
107.87
Ag 47
Cadmium 112.41
Cd 48
Indium 114.82
In 49
Tin 118.71
Sn 50
121.76
Sb 51
127.60
52
Iodine 126.90
I 53
Xenon 131.29
Xe 54
Cesium 132.91
Cs 55
137.33
Ba 56
138.91
La 57
Hafnium 178.49
Hf 72
180.95
73
183.84
W 74
Rhenium 186.21
Re 75
Osmium 190.23
Os 76
192.22
Ir 77
195.08
Pt 78
Gold 19 7
79
200.59
Hg 80
Thallium 204.38
Tl 81
Lead 207.2
Pb 82
208.98
Bi 83
(209)
84
Astatine (210)
At 85
Pd
Radon (222)
Rn 86
(223)
Fr 87
Radium (226)
Ra 88
Actinium (227)
Ac 89
Dubnium (262)
Db 105
Seaborgium (266)
Sg 106
(264)
Bh 107
Hassium (269)
Hs 108
(268)
Mt 109
140.12
Ce 58
Neodymium 144.24
Nd 60
Promethium (145)
Pm 61
150.36
Sm 62
Europium 151.96
Eu 63
Gadolinium 157.25
Gd 64
158.93
Tb 65
Dysprosium 162.50
Dy 66
Holmium 164.93
Ho 67
Erbium 167.26
Er 68
Thulium 168.93
Tm 69
Ytterbium 173.04
Yb 70
Lutetium 174.97
Lu 71
232.04
Th 90
Protactinium 231.04
91
238.03
U 92
Neptunium (237)
Np 93
Plutonium (244)
Pu 94
(243)
Am 95
(247)
Cm 96
(247)
Bk 97
(251)
Cf 98
Einsteinium (252)
Es 99
(257)
Fm 100
Nobelium (259)
No 102
(262)
Lr 103
Magnesium 24.31
Mg 12
9.01
Be 4
50.94
V 23
Manganese 54.94
Mn 25
*
Atomic number
Average atomic mass
Potassium Nickel
Praseodymium
Rutherfordium
Molybdenum
Mendelevium
Germanium
Key
Fluorine
Aluminum Phosphorus Chlorine
Krypton
Yttrium Technetium Palladium Silver Antimony Tellurium Te
Barium Lanthanum Tantalum Ta
Tungsten Iridium Platinum 6.9
Au Mercury Bismuth Polonium
Po
Francium Bohrium Meitnerium (281)
Ds110
Darmstadtium
(280)
Rg111
Roentgenium
(285)
Cn112
Copernicium(284)
Nh113
Nihonium(289)
Fl114
Flerovium(288)
Mc115
Moscovium(293)
Lv116
Livermorium(294)
Ts117
Tennessine(294)
Og118
Oganesson
Cerium Samarium Terbium
Thorium Pa
Uranium Americium Curium Berkelium Californium Fermium Lawrencium
Beryllium
Vanadium
If this number is in parentheses, then it refers to the atomic mass of the most stable isotope.
Copyright © 2017 California Department of Education
Names, Formulas, and Charges of Common Ions
POSITIVE IONS (CATIONS) Name Symbol Name Symbol aluminum Al3+ lithium Li+ ammonium NH4
+ magnesium Mg2+
barium Ba2+ manganese(II) Mn2+ cadmium Cd2+ manganese(IV) Mn4+ calcium Ca2+ mercury(I) Hg2
2+ chromium(II) Cr2+ mercury(II) Hg2+ chromium(III) Cr3+ nickel(II) Ni2+ copper(I) Cu+ potassium K+ copper(II) Cu2+ silver Ag+ hydrogen, H+ sodium Na+ iron(II) Fe2+ strontium Sr2+ iron(III) Fe3+ tin(II) Sn2+
lead(II) Pb2+ tin(IV) Sn4+ lead(IV) Pb4+ zinc Zn2+
NEGATIVE IONS (ANIONS) Name Symbol Name Symbol acetate C2H3O2
– (CH3COO–) nitrate NO3–
azide N3– nitride N3–
bromide Br– nitrite NO2–
bromate BrO3– oxalate C2O4
2–
carbonate CO32– hydrogen oxalate H C2O4
– hydride H– oxide O2–
hydrogen carbonate HCO3– perchlorate ClO4
–
chlorate ClO3– permanganate MnO4
–
chloride Cl– phosphate PO43–
chlorite ClO2– monohydrogen phosphate HPO4
2–
chromate CrO42– dihydrogen phosphate H2PO4
–
citrate C6H5O73– silicate SiO3
2–
cyanide CN– sulfate (sulphate) SO42–
dichromate Cr2O72– hydrogen sulfate (sulphate) HSO4
–
fluoride F– sulfide (sulphide) S2– hydroxide OH– hydrogen sulfide (sulphide) HS–
hypochlorite ClO– sulfite (sulphite) SO32–
iodide I– hydrogen sulfite (sulphite) HSO3–
iodate IO3– thiocyanate SCN–
G r a d e 1 2 C h e m i s t r y24 of 32
Relative Strengths of Acids Table
Acid Reaction Ka
Perchloric acid HClO4 + H2O H3O+ + ClO4� very large
Hydriodic acid Hl + H2O H3O+ + I� very large
Hydrobromic acid HBr + H2O H3O+ + Br� very large
Hydrochloric acid HCl + H2O H3O+ + Cl� very large
Nitric acid HNO3 + H2O H3O+ + NO3� very large
Sulfuric acid H2SO4 + H2O H3O+ + HSO4� very large
Oxalic acid H2C2O4 + H2O H3O+ + HC2O4� 5.4 x 10�2
Sulfurous acid H2SO3 + H2O H3O+ + HSO3� 1.7 x 10�2
Hydrogen sulfate ion HSO4� + H2O H3O+ + SO4
2� 1.3 x 10�2
Phosphoric acid H3PO4 + H2O H3O+ + H2PO4� 7.1 x 10�3
Ferric ion Fe(H2O)63+ + H2O H3O+ + Fe(H2O)5(OH)2+ 6.0 x 10�3
Hydrogen telluride H2Te + H2O H3O+ + HTe� 2.3 x 10�3
Hydrofluoric acid HF + H2O H3O+ + F� 6.7 x 10�4
Nitrous acid HNO2 + H2O H3O+ + NO2� 5.1 x 10�4
Hydrogen selenide H2Se + H2O H3O+ + HSe� 1.7 x 10�4
Chromic ion Cr(H2O)63+ + H2O H3O+ + Cr(H2O)5(OH)2+ 1.5 x 10�4
Benzoic acid C6H5COOH + H2O H3O+ + C6H5COO� 6.6 x 10�5
Hydrogen oxalate ion HC2O4� + H2O H3O+ + C2O4
2� 5.4 x 10�5
Acetic acid HC2H3O2 + H2O H3O+ + C2H3O2� 1.8 x 10�5
Aluminum ion Al(H2O)63+ + H2O H3O+ + Al(H2O)5(OH)2+ 1.4 x 10�5
Carbonic acid H2CO3 + H2O H3O+ + HCO3� 4.4 x 10�7
Hydrogen sulfide H2S + H2O H3O+ + HS� 1.0 x 10�7
Dihydrogen phosphate ion H2PO4� + H2O H3O+ + HPO4
2� 6.3 x 10�8
Hydrogen sulfite ion HSO3� + H2O H3O+ + SO3
2� 6.2 x 10�8
Ammonium ion NH4+ + H2O H3O+ + NH3 5.7 x 10�10
Hydrogen carbonate ion HCO3� + H2O H3O+ + CO3
2� 4.7 x 10�11
Hydrogen telluride ion HTe� + H2O H3O+ + Te2� 1.0 x 10�11
Hydrogen peroxide H2O2 + H2O H3O+ + HO2� 2.4 x 10�12
Monohydrogen phosphate HPO42� + H2O H3O+ + PO4
3� 4.4 x 10�13
Hydrogen sulfide ion HS� + H2O H3O+ + S2� 1.2 x 10�15
Water H2O + H2O H3O+ + OH� 1.8 x 10�16
Hydroxide ion OH� + H2O H3O+ + O2� < 10�36
Ammonia NH3 + H2O H3O+ + NH2� very small
F i n a l P r a c t i s e E x a m i n a t i o n A n s w e r K e y 25 of 32
Name: ___________________________________________
Solubility Chart
Negative Ions Positive Ions Solubility
essentially all alkali ions (Li+, Na+, K+, Rb+, Cs+) soluble
essentially all hydrogen ion H+(aq) soluble
essentially all ammonium ion (NH4+) soluble
nitrate, NO3� essentially all soluble
acetate, CH3COO� essentially all (except Ag+) soluble
chloride, Cl� bromide, Br� iodide, I�
Ag+, Pb2+, Hg22+, Cu+, Tl+ low solubility
all others soluble
sulfate, SO42�
Ca2+, Sr2+, Ba2+, Pb2+, Ra2+ low solubility
all others soluble
sulfide, S2�
alkali ions, H+(aq), NH4
+, Be2+, Mg2+, Ca2+,
Sr2+, Ba2+, Ra2+soluble
all others low solubility
hydroxide, OH�
alkali ions, H+(aq), NH4
+, Sr2+, Ba2+, Ra2+, Tl+ soluble
all others low solubility
phosphate, PO43�
carbonate, CO32�
sulfite, SO32�
alkali ions, H+(aq), NH4
+ soluble
all others low solubility
chromate, CrO42�
Ba2+, Sr2+, Pb2+, Ag+ low solubility
all others soluble
G r a d e 1 2 C h e m i s t r y26 of 32
Table of Standard Reduction Potentials with Values
Oxidized species Reduced Species E°/V
Li+(aq) + e� Li(s) �3.04
K+(aq) + e� K(s) �2.93
Ca2+(aq) + 2e� Ca(s) �2.87
Na+(aq) + e� Na(s) �2.71
Mg2+(aq) + 2e� Mg(s) �2.37
Al3+(aq) + 3e� Al(s) �1.66
Mn2+(aq) + 2e� Mn(s) �1.19
H2O(l) + e� ½H2(g) + OH�
(aq) �0.83
Zn2+(aq) + 2e� Zn(s) �0.76
Fe2+(aq) + 2e� Fe(s) �0.45
Ni2+(aq) + 2e� Ni(s) �0.26
Sn2+(aq) + 2e� Sn(s) �0.14
Pb2+(aq) + 2e� Pb(s) �0.13
H+(aq) + e� ½H2(g) 0.00
Cu2+(aq) + e� Cu+
(aq) +0.15
SO42�
(aq) + 4 H+(aq) + 2e� H2SO3(aq) + H2O(l) +0.17
Cu2+(aq) + 2e� Cu(s) +0.34
½O2(g) + H2O(l) + 2e� 2OH�(aq) +0.40
Cu+(aq) + e� Cu(s) +0.52
½I2(s) + e� I�(aq) +0.54
Fe3+(aq) + e� Fe2+
(aq) +0.77
Ag+(aq) + e� Ag(s) +0.80
½Br2(l) + e� Br�(aq) +1.07
½O2(g) + 2H+(aq) + 2e� H2O(l) +1.23
Cr2O72�
(aq) + 14H+(aq) + 6e� 2Cr3+
(aq) + 7H2O(l) +1.33
½Cl2(g) + e� Cl�(aq) +1.36
MnO4�(aq) + 8H+
(aq) + 5e� Mn2+(aq)+ 4H2O(l) +1.51
½F2(g) + e� F�(aq) +2.87
F i n a l P r a c t i s e E x a m i n a t i o n A n s w e r K e y 27 of 32
Name: ___________________________________________
Names, Formulas, and Charges of Common Ions
Positive Ions (Cations)
Name Symbol Name Symbol
aluminum Al3+ magnesium Mg2+
ammonium NH4+ manganese(II) Mn2+
barium Ba2+ manganese(IV) Mn4+
cadmium Cd2+ mercury(I) Hg22+
calcium Ca2+ mercury(II) Hg2+
chromium(II) Cr2+ nickel(II) Ni2+
chromium(III) Cr3+ nickel(III) Ni3+
copper(I) Cu+ potassium K+
copper(II) Cu2+ silver Ag+
hydrogen H+ sodium Na+
iron(II) Fe2+ strontium Sr2+
iron(III) Fe3+ tin(II) Sn2+
lead(II) Pb2+ tin(IV) Sn4+
lead(IV) Pb4+ zinc Zn2+
lithium Li+
G r a d e 1 2 C h e m i s t r y28 of 32
Names, Formulas, and Charges of Common Ions (continued)
Negative Ions (Anions)
Name Symbol Name Symbol
acetate C2H3O2�(CH3COO�) nitrate NO3
�
azide N3� nitride N3�
bromide Br� nitrite NO2�
bromate BrO3� oxalate C2O4
2�
carbonate CO32� hydrogen oxalate HC2O4
�
hydride H� oxide O2�
hydrogen carbonate
or bicarbonateHCO3
� perchlorate ClO4�
chlorate ClO3� permanganate MnO4
�
chloride Cl� phosphate PO43�
chlorite ClO2� monohydrogen phosphate HPO4
2�
chromate CrO42� dihydrogen phosphate H2PO4
�
citrate C6H5O73� silicate SiO3
2�
cyanide CN� sulfate SO42�
dichromate Cr2O72� hydrogen sulfate HSO4
�
fluoride F� sulfide S2�
hydroxide OH� hydrogen sulfide HS�
hypochlorite ClO� sulfite SO32�
iodide I� hydrogen sulfite HSO3�
iodate IO3� thiocyanate SCN�
F i n a l P r a c t i s e E x a m i n a t i o n A n s w e r K e y 29 of 32
Name: ___________________________________________
Common Ions
Cations (Positive Ions)
1+ charge 2+ charge 3+ charge
NH4+ Ammonium Ba2+ Barium Al3+ Aluminum
Cs+ Cesium Be2+ Beryllium Cr3+ Chromium(III)
Cu+ Copper(I) Cd2+ Cadmium Co3+ Cobalt(III)
Au+ Gold(I) Ca2+ Calcium Ga3+ Gallium
H+ Hydrogen Cr2+ Chromium(II) Au3+ Gold(III)
Li+ Lithium Co2+ Cobalt(II) Fe3+ Iron(III)
K+ Potassium Cu2+ Copper(II) Mn3+ Manganese
Rb+ Rubidium Fe2+ Iron(II) Ni3+ Nickel(III)
Ag+ Silver Pb2+ Lead(II)
Na+ Sodium Mg2+ Magnesium 4+ charge
Mn2+ Manganese(II) Pb4+ Lead(IV)
Hg22+ Mercury(I) Mn4+ Manganese(IV)
Hg2+ Mercury(II) Sn4+ Tin(IV)
Ni2+ Nickel(II)
Sr2+ Strontium
Sn2+ Tin(II)
Zn2+ Zinc
G r a d e 1 2 C h e m i s t r y30 of 32
Common Ions (continued)
Anions (Negative Ions)
1� charge 1� charge 2� charge
CH3COO�
(C2H3O2�)
Acetate (or
ethanoate)
HS�Hydrogen
sulfide
CO32� Carbonate
CrO42� Chromate
BrO3� Bromate OH� Hydroxide Cr2O7
2� Dichromate
Br� Bromide IO3� Iodate O2� Oxide
ClO3� Chlorate I� Iodide O2
2� Peroxide
Cl� Chloride NO3� Nitrate SO4
2� Sulfate
ClO2� Chlorite NO2
� Nitrite S2� Sulfide
CN� Cyanide ClO4� Perchlorate SO3
2� Sulfite
F� Fluoride IO4� Periodate S2O3
2� Thiosulfate
H� Hydride MnO4� Permanganate
HCO3� Hydrogen
carbonate (or
bicarbonate)
SCN� Thiocynate 3� charge
N3� Nitride
ClO� Hypochlorite PO43� Phosphate
HSO4�
Hydrogen
sulfate
P3� Phosphide
PO33� Phosphite
Chemistry 40S Constants and Equations
Atomic Structure Chemical Kinetics
E = h × c
λ c = λ × ν Average Rate =
∆[ ]
∆t
E = h × ν λ = h
mv Rate = k[A]x[B]y
Chemical Equilibrium
Keq = [C]c[D]d
[A]a[B]b aA + bB cC + dD
Ksp = [A+]a[B-]b AaBb (s) aA+ (aq) + bB- (aq)
c=𝑛
𝑣
c1 × v1 = c2 × v2
Acid-Base Equilibrium
Kw = [H3O+][OH-]= 1.0 X 10-14
Ka = [H3O+][A−]
[HA] HA + H2O H3O+ + A-
Kb = [OH−][HB+]
[B] B + H2O BH+ + OH-
Percent dissociation = [H3O+]
[HA] × 100%
Percent dissociation = [OH−]
[B] × 100%
CA × VA= CB × VB
pH = -log[H+]
pOH = -log[OH-]
pH + pOH = 14
Electrochemistry
Ecell = E
red +Eox
Number of moles electrons = I∆t
F
Constants
h = 6.63 × 10-34 Js
c = 3.0 × 108 m/s
Kw = 1.0 × 10-14
F ≈ 96 500 C/mol of e-