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430 Discovering Chemistry You Need to Know

Units and Measurement

1 ft 12 in

1 in 2.54 cm

1 min 60 s

1 hr 3600 s

1 quart 0.946 L

2 pints 1 quart

1 pound 454 g

Common Equivalents

Quantity SI Unit What is used to measure?

Mass—the amount of matter in a sample

Kilograms (kg) Balance (not a “scale”)

Volume—the amount of space an object takes up

Milliliter (mL) Graduated cylinder

Temperature—related to the speed with which molecules move

Celsius (°C) orKelvin (K) Thermometer

Length Meters (m) Ruler, meter stick

Time Seconds (s or sec) Stopwatch, clock

Energy Joule (J) Measured indirectly

Quantities Commonly Measured in Chemistry

Metric PrefixesPrefix Symbol Equivalent (Example)

giga- G 1 giga = 1,000,000,000 base units (1 G = 1,000,000,000 g)

mega- M 1 mega = 1,000,000 base units (1 M = 1,000,000 g)

kilo- k 1 kilo = 1000 base units (1 kg = (1000 g)

hecto- h 1 hecto = 100 base units (1 h = 100 g)

deka- da 1 deka = 10 base units (1 dag = 10 g)

deci- d 1 deci = 0.1 base units (1 dg = 0.1 g)

centi- c 1 cent = 0.01 base units (1 cg = 0.01 g)

milli- m 1 milli = 0.001 base units (1 mg = 0.001 g)

micro- µ 1 micro = 1 • 10–6 base units (1 µg = 1 • 10–6 g)

nano- n 1 nano = 1 • 10–9 base units 1 ng = (1 • 10–9 g)

pico- p 1 pico = 1 • 10–12 base units (1 p = 1 • 10–12g)

°C degree Celsius (temperature)

cal calorie (energy)

J joule (energy)

K kelvin (temperature, thermo-dynamic)

mm Hg millimeters of mercury (pressure)

M molarity (concentration)

Pa pascal (pressure)

psi pounds per square inch (pressure)

V volt (electric potential difference)

Unit Abbreviations

Discovering Chemistry You Need to Know 431

Symbols

Symbol Stands for

α helium nucleus (also 42He) emission from radioactive materials

β electron (also 0-1e) emission from radioactive materials

γ high-energy photo emission from radioactive materials

Δ change in a given quantity (e.g., ΔH for change in enthalpy)

c speed of light in vacuum

Cp specific heat capacity (at constant pressure)

D density

Ea activation energy

E o standard electrode potential

E ocell standard potential of an electrochemical cell

H enthalpy

ΔHO standard enthalpy of reaction

ΔHOf standard molar enthalpy of formation

Keq equilibrium constantionization constant

Ksp solubility-product constant disassociation constant enthalpy

m mass

MM molar mass

NA Avogadro’s number

n number of moles

P pressure

pH measure of acidity (–log[H3O+])

R ideal gas law constant

T temperature

V volume

State symbols

(aq) substance is dissolved in water

(s) substance in the solid state

(l ) substance in the liquid state

(g) substance in the gaseous state


Common Polyatomic Ions

Writing and Naming Formulas

Acetate, CH3COO –1 or C2H3O2

–1

Ammonium, NH4+1

Bromate, BrO3–1

Bromide, Br–

Bromite, BrO2–1

Carbonate, CO3–2

Chlorate, ClO3–1

Chloride, Cl–

Chlorite, ClO2–1

Chromate, CrO4–2

Cyanide, CN–1

Dichromate, Cr2O7–2

Dihydrogen phosphate, H2PO4–1

Fluoride, F–

Hydride, H–

Hydrogen carbonate or bicarbonate, HCO–1

Hydrogen phosphate or biphosphate, HPO4–2

Hydrogen sulfate or bisulfate, HSO4–1

Hydronium, H3O+

Hydroxide, OH–1

Hypochlorite, ClO–1

Iodate, IO3–1

Iodide, I–

Iodite, IO2–1

Nitrate, NO3–1

Nitrite, NO2–1

Oxalate, C2O4–2

Oxide, O–2

Perchlorate, ClO4–1

Permanganate, MnO4–1

Peroxide, O2–2

Phosphate, PO4–3

Phosphite, PO3–3

Silicate, SiO3–1

Sulfate, SO4–2

Sulfide, S2–

Sulfite, SO3–2


Common Multivalent Metals and Their ChargesType of metal

Chromium Cr2+ Cr+3

Cobalt Co+2 Co+3

Copper Cu+1 Cu+2

Iron Fe+2 Fe+3

Lead Pb+2 Pb+4

Manganese Mn+2 Mn+3

Mercury Hg2+2 Hg+2

Tin Sn+2 Sn+4

Titanium Ti3+ Ti+3

Prefixes Used in Molecular Compounds

1. mono- 2. di- 3. tri- 4. tetra- 5. penta- 6. hexa- 7. hepta- 8. octa- 9. nona- 10. deca-

Organic Nomenclature Prefixes

Number of atoms Prefix for carbon atoms in an organic molecule

1 Meth-

2 Eth-

3 Prop-

4 But-

5 Pent-

6 Hex-

7 Hept-

8 Oct-

9 Non-

10 Dec-

Diatomic Elements and Formulas**

Hydrogen H2

Oxygen O2

Fluorine F2

Bromine Br2

Iodine I2

Nitrogen N2

Chlorine Cl2

**Their chemical symbols can be placed in a word to remember: HOFBrINCl, pronounced “Hoffbrinkle.”


Solubility Rules

Solubility

These anions Form soluble compounds with these cations Form insoluble compounds with these cations

NO3– nitrate Most cations No common cations

CH3COO– acetate Most cations Ag+

Cl– chloride Most cations Ag+, Pb2+, Hg22+, Tl+1

Br– bromide Most cations Ag+, Pb2+, Hg22+, Tl+1

I– iodide Most cations Ag+, Pb2+, Hg22+, Tl+1

SO42– sulfate Most cations Ba2+, Sr2+, Pb2+, Ag+, Ca2+

CrO42– chromate Most cations Ba2+, Sr2+, Pb2+, Ag+

S2– sulfide NH4+, cations of column 1, cations of column 2 Most other cations

OH– hydroxide NH4+, cations of column 1, and Ba2+ and Sr2+ Most other cations

CO32– carbonate NH4

+, cations of column 1 except Li+ Most other cations

PO43– phosphate NH4

+, cations of column 1 except Li+ Most other cations

Solubility Product Constants (25°C)Salt Ksp

Ag2CO3 8.4 × 10–12

AgCl 1.8 × 10–10

Ag2CrO4 1.1 × 10–12

Ag2S 1.1 × 10–49

AgBr 5.4 × 10–13

AgI 8.5 × 10–17

AlPO4 9.8 × 10–21

BaSO4 1.1 × 10–10

CaCO3 5.0 × 10–9

Ca(OH)2 4.7 × 10–7

Ca3(PO4)2 2.1 × 10–33

CaSO4 7.1 × 10–5

CuS 1.3 × 10–36

FeCO3 3.1 × 10–11

Solubility Product Constants (25°C) (cont’d.)Salt Ksp

Fe(OH)2 4.9 × 10–17

Fe(OH)3 2.6 × 10–39

FeS 1.6 × 10–19

MgCO3 6.8 × 10–6

Mg(OH)2 5.6 × 10–12

Mg3(PO4)2 9.9 × 10–25

MnCO3 2.2 × 10–11

Pb(OH)2 1.4 × 10–20

PbS 9.0 × 10–29

PbSO4 1.8 × 10–8

SrSO4 3.4 × 10–7

ZnCO3 1.2 × 10–10

ZnS 2.9 × 10–25


Compound Solubility

Solubility

In grams of solute that can be dissolved at these temperatures in 100 g of water.

Formula 0°C 20°C 60°C 100°C

Al2(SO4)3 31.2 36.4 59.2 89.0

NH4Cl 29.4 37.2 55.3 77.3

NH4NO3 118.0 192.0 421.0 871.0

(NH4)2SO4 70.6 75.4 88.0 103.0

BaCl2•2H2O 31.2 35.8 46.2 59.4

Ba(OH)2 1.67 3.89 20.94 101.4080°

Ba(NO3)2 4.95 9.02 20.4 34.4

Ca(HCO3)2 16.15 16.60 17.50 18.40

Ca(OH)2 0.189 0.173 0.121 0.076

CuCl2 68.6 73.0 96.5 120.0

CuSO4•5H2O 23.1 32.0 61.8 114.0

PbCl2 0.67 1.00 1.94 3.20

Pb(NO3)2 37.5 54.3 91.6 133.0

LiCl 69.2 83.5 98.4 128.0

Li2SO4 36.1 34.8 32.6 30.990°

MgSO4 22.0 33.7 54.6 68.3

HgCl2 3.63 6.57 16.3 61.3

KBr 53.6 65.3 85.5 104.0

KClO3 3.3 7.3 23.8 56.3

KCl 28.0 34.2 45.8 56.3

K2CrO4 56.3 63.7 70.1 74.590°

KI 128.0 144.0 176.0 206.0

KNO3 13.9 31.6 106.0 245.0

K2SO4 7.4 11.1 18.2 24.1

AgC2H3O2 0.73 1.05 1.93 2.5980°

AgNO3 122.0 216.0 440.0 733.0

NaC2H3O2 36.2 46.4 139.0 170.0

NaClO3 79.6 95.9 137.0 204.0

NaCl 35.7 35.9 37.1 39.2

NaNO3 73.0 87.6 122.0 180.0

C12H22O11 179.2 203.9 287.3 487.2


Useful Constants

EquilibriumAtomic mass unit (amu) 1.6605402 × 10–27kg

Avogadro’s number (NÂ) 6.022137 × 1023/mol

Electron rest mass (mê) 9.1093897 × 10–31 kg

5.4858 × 10–4amu

Gas law constant, R, with atm pressure unit 0.0821 L × atm mole × K

Gas law constant, R, with kPa pressure units 8.31 L × kPa mole × K

Enthalpy of fusion of water (Hfus) 80.87 cal/g

Enthalpy of vaporization of water (Hvap) 547.2 cal/g

Volume of one mole of a gase at STP 22.41410 L/mol

Mass of a neutron 1.6749286 × 10–27 kg 1.008665 amu

Normal boiling point of water (Tb) 373.15 K = 100.0°C

Normal freezing point of water (Tf) 273.15 K = 0.00°C

Planck’s constant (h) 6.626076 × 10–34

J × s

Mass of a proton 1.6726231 × 10–27kg 1.007276 amu

Specific heat capacity of liquid water (Cp) 1.00 cal/g°C

Specific heat capacity of ice (Cp) 0.51 cal/g°C

Specific heat capacity of steam (Cp) 0.48 cal/g°C

Speed of light in a vacuum (c) 2.997924 58 × 108 m/s

Temperature of triple point of water 273.16 K = 0.01°C


ReductionActivity Series Reduction

Useful Constants Electrochemistry

Li Most reactive

Least reactive

K

Ba

Sr

Ca

Na

Mg

Al

Mn

Zn

Cr

Fe

Cd

Co

Ni

Sn

Pb

H

Cu

Hg

Ag

Pt

Au

Reductionhalf-reaction

Standard reduction

potential (volts)

F2 (g) + 2 e–1 → 2 F–1 2.87

Co+3 + e–1 → Co+2 1.82

Au+3 + 3 e–1 → Au (s) 1.50

Cl2 (g) + 2e– → 2 Cl–1 1.36

O2 (g) + 4 H+ → 2 H2O (l) 1.23

Br2 (l) + 2 e–1 → 2 Br–1 1.07

2 Hg+2 + 2 e–1 → Hg2+2 0.92

Hg+2 + 2 e–1 → Hg (l) 0.85

Ag+1 + e–1 → Ag (s) 0.80

Hg2+2 + 2 e–1 → 2 Hg (l) 0.79

Fe+3 + e–1 → Fe+2 0.77

I2 (s) + 2 e–1 → 2 I–1 0.53

Cu+ + e–1 → Cu (s) 0.52

Cu+2 + 2 e–1 → Cu (s) 0.34

Cu+2 + e–1 → Cu+1 0.15

Sn+4 + 2 e–1 → Sn+2 0.15

S (s) + 2 H+ + 2 e–1 → H2S (g) 0.14

2 H+ + 2 e–1 → H2 (g) 0.00

Pb+2 + 2 e–1 → Pb (s) –0.13

Sn+2 + 2 e–1 → Sn(s) –0.14

Reductionhalf-reaction

Standard reduction

potential (volts)

Ni+2 + 2 e–1 → Ni (s) –0.25

Co+2 + 2 e–1 → Co (s) –0.28

Tl+1 + e–1 → Tl (s) –0.34

Cd+2 + 2 e–1 → Cd (s) –0.40

Cr+3 + e–1 → Cr+2 –0.41

Fe+2 + 2 e–1 → Fe (s) –0.44

Cr+3 + 3 e–1 → Cr (s) –0.74

Zn+2 + 2 e–1 → Zn (s) –0.76

Mn+2 + 2 e–1 → Mn (s) –1.18

Al+3 + 3 e–1 → Al (s) –1.66

Be+2 + 2 e–1 → Be (s) –1.70

Mg+2 + 2 e–1 → Mg (s) –2.37

Na+1 + e–1 → Na (s) –2.71

Ca+2 + 2 e–1 → Ca (s) –2.87

Sr+2 + 2 e–1 → Sr (s) –2.89

Ba+2 + 2 e–1 → Ba (s) –2.90

Rb+1 + e–1 → Rb (s) –2.92

K+1 + e–1 → K (s) –2.92

Cs+1 + e–1 → Cs (s) –2.92

Li+1 + e–1 → Li (s) –3.05


Enthalpies of Formation (Hf) kJ/mole

Enthalpies of Formation (Hf) kJ/moleAluminum

Al(s) 0

AlCl3(s) –704.2

Al2O3(s) –1675.7

Barium

BaCl2(s) –858.6

BaO(s) –553.5

BaSO4(s) –1473.2

Beryllium

Be(s) 0

Be(OH)2 –902.5

Bromine

Br(g) 111.9

Br2(l) 0

Br2(g) –30.9

BrF3(g) –255.6

Calcium

Ca(s) 0

Ca(g) 178.2

Ca+2(g) 1925.9

CaC2(s) –59.8

CaCO3(s; calcite) –1206.9

CaCl2(s) –795.8

CaF2(s) –1219.6

CaH2(s) –186.2

CaO(s) –635.1

CaS(s) –482.4

Ca(OH)2(s) –986.1

Ca(OH)2(aq) –1002.8

CaSO4(s) –1434.1

Carbon

C(s; graphite) 0

C(s; diamond) 1.9

C(g) 716.7

CCl4(l) –135.4

CCl4(g) –102.9

CHCl3(l) –134.5

CHCl3(g) –103.1

HgCl2(s) –224.3

HgO(s) –90.8

CH4(g; methane) –74.81

C2H2(g; ethyne) 226.7

C2H4(g; ethene) 52.3

C2H6(g; ethane) –84.7

C3H8(g; propane) –103.8

C6H6(l; benzene) 49.0

CH3OH(l; methanol) –238.7

CH3OH(g; methanol) –200.7

C2H5OH(l; ethanol) –277.7

C2H5OH(g; ethanol) –235.1

CO(g) –110.5

CO2(g) –393.5

CS2(g) 117.36

COCl2(g) –218.8

Cesium

Cs(s) 0

Cs+1(g) 458.0

CsCl(s) –443.0

Chlorine

Cl(g) 121.7

Cl–1(g) –233.1

Cl2(g) 0

Chromium

Cr(s) 0

Cr2O3(s) –1139.7

CrCl2(s) –556.5

Copper

Cu(s) 0

CuO(s) –157.3

CuCl2(s) –220.1

Fluorine

F2(g) 0

F(g) 79

F–1(g) –255.4

F–1(aq) –332.6

Hydrogen

H2(g) 0

H(g) 218

H+1(g) 1536.2

H2O(l) –285.8

H2O(g) –241.8

H2O2(l) –187.8

Iodine

I2(s) 0

I2(g) 62.4

I(g) 106.8

I–1(g) –197.0

ICl(g) 17.78

Iron

Fe(s) 0

FeO(s) –272

Fe2O3 (s; hematite) –824.2

Fe3O4(s; magnetite) –1118.4

FeCl2(s) –341.8

FeCl3(s) –399.5

FeS2(s; pyrite) –178.2

Fe(CO)5(l) –774


Enthalpies of Formation (Hf) kJ/moleLead

Pb(s) 0

PbCl2(s) –359.4

PbO(s) –217.3

PbS(s) –100.4

Lithium

Li(s) 0

Li+1(g) 685.8

LiOH(s) –484.9

LiOH(aq) –508.5

LiCl(s) –408.7

Magnesium

Mg(s) 0

MgCl2(s) –641.3

MgO(s) –601.7

Mg(OH)2(s) –924.5

MgS(s) –346

Mercury

Hg(l) 0

HgCl2(s) –224.3

HgO(s) –90.8

HgS(s) –58.2

Nickel

Ni(s) 0

NiO(s) –239.7

NiCl(s) –305.3

Nitrogen

N2(g) 0

N(g) 472.7

NH3(g) –46.11

N2H4(l) 50.6

NH4Cl(s) –314.4

NH4Cl(aq) –299.7

NH4NO3(s) –365.6

NH4NO3(aq) –339.9

NO(g) 90.3

NO2(g) 33.2

N2O(g) 82.1

N2O4(g) 9.16

NOCl(g) 51.7

Oxygen

O2(g) 0

O(g) 249.17

O3(g) 142.7

Phosphorus

P(g) 314.6

PH3(g) 5.4

PCl3(g) –287.0

P4O10(s) –2984.0

Potassium

K(s) 0

KCl(s) –436.7

KClO3(s) –397.7

KI(s) –327.9

KOH(s) –424.8

KOH(aq) –482.4

Silicon

Si(s) 0

SiBr4(l) –457.3

SiC(s) –65.3

SiCl4(g) –657

SiH4(g) 34.3

SiF4(g) –1614.9

SiO2(s; quartz) –910.9

Silver

Ag(s) 0

Ag2O(s) –31.1

AgCl(s) –127.1

AgNO3(s) –124.4

Sodium

Na(s) 0

Na(g) 107.3

Na+1(g) 609.4

NaBr(s) –361.1

NaCl(s) –411.2

NaCl(g) –176.65

NaCl(aq) –407.3

NaOH(s) –425.6

NaOH(aq) –470.1

Na2CO3(s) –1130.7

Na2SO4(aq) –1387.1

Sulfur

S(s; rhombic) 0

S(g) 278.8

S2Cl2(g) –18.4

SF6(g) 1209

SO2(g) –296.8

SO3(g) –395.7

SOCl2(g) –212.5

Tin

Sn(s; white) 0

Sn(s; gray) –2.09

SnCl4(l) –511.3

SnCl4(g) –471.5

SnO2(g) –580.7

Titanium

Ti(s) 0

TiCFl4(l) –804.2

TiCl4(g) –763.2

TiO2 –939.7

Zinc

Zn(s) 0

ZnCl2(s) –415.1

ZnO(s) –348.3

ZnS(s; sphalerite) –205.98

Acids

HBr(g) –36.4

HCl(g) –92.3

HCl(aq) –167.2

HF(g) –271.1

HF(aq) –332.6

HNO3(l) –174.1

HNO3(g) –135.1

HNO3(aq) –207.0

H3PO4(s) –1279.0

H2S(g) –20.6

H2SO4(l) –814.0

H2SO4(aq) –909.3


The Elements

Name Symbol Atomic Number Atomic Mass

Actinium Ac 89 (227)

Aluminum Al 13 26.08

Americium Am 95 (243)

Antimony Sb 51 121.8

Argon Ar 18 39.95

Arsenic As 33 74.92

Astatine At 85 (210)

Barium Ba 56 137.3

Berkelium Bk 97 (247)

Beryllium Be 4 9.01

Bismuth Bi 83 209.0

Boron B 5 10.81

Bromine Br 35 79.90

Cadmium Cd 48 112.4

Calcium Ca 20 40.08

Californium Cf 98 (251)

Carbon C 6 12.01

Cerium Ce 58 140.1

Cesium Cs 55 132.9

Chlorine Cl 17 35.45

Chromium Cr 24 52.00

Cobalt Co 27 58.93

Copper Cu 29 63.55

Curium Cm 96 (247)

Dysprosium Dy 66 162.5

Einsteinium Es 99 (252)

Erbium Er 68 167.3

Europium Eu 63 152.0

Fermium Fm 100 (257)

Fluorine F 9 19.00

Francium Fr 87 (223)

Gadolinium Gd 64 157.3

Gallium Ga 31 69.72

Germanium Ge 32 72.59

The Elements


The Elements (cont’d.)


Gold Au 79 197.0

Hafnium Hf 72 178.5

Helium He 2 4.00

Holmium Ho 67 164.9

Hydrogen H 1 1.01

Indium In 49 114.8

Iodine I 53 126.9

Iridium Ir 77 192.2

Iron Fe 26 55.85

Krypton Kr 36 83.80

Lanthanum La 57 138.9

Lawrencium Lr 103 (260)

Lead Pb 82 207.2

Lithium Li 3 6.94

Lutetium Lu 71 175.0

Magnesium Mg 12 24.31

Manganese Mn 25 54.94

Mendelevium Md 101 (258)

Mercury Hg 80 200.6

Molybdenum Mo 42 95.94

Neodymium Nd 60 144.2

Neon Ne 10 20.18

Neptunium Np 93 (237)

Nickel Ni 28 58.70

Niobium Nb 41 92.91

Nitrogen N 7 14.01

Nobelium No 102 (259)

Osmium Os 76 190.2

Oxygen O 8 16.00

Palladium Pd 46 106.4

Phosphorus P 15 30.97

Platinum Pt 78 195.1

Plutonium Pu 94 (244)

Polonium Po 84 (209)

Potassium K 19 39.10

(continues)


The Elements (cont’d.)


Praseodymium Pr 59 140.9

Promethium Pm 61 (145)

Protactinium Pa 91 (231)

Radium Ra 88 226.0

Radon Rn 86 (222)

Rhenium Re 75 186.2

Rhodium Rh 45 102.9

Rubidium Rb 37 85.47

Ruthenium Ru 44 101.1

Samarium Sm 62 150.4

Scandium Sc 21 44.96

Selenium Se 34 78.96

Silicon Si 14 28.09

Silver Ag 47 107.9

Sodium Na 11 22.99

Strontium Sr 38 87.62

Sulfur S 16 32.06

Tantalum Ta 73 180.9

Technetium Tc 43 (98)

Tellurium Te 52 127.6

Terbium Tb 65 158.9

Thallium Tl 81 204.4

Thorium Th 90 232.0

Thulium Tm 69 168.9

Tin Sn 50 118.7

Titanium Ti 22 47.90

Tungsten W 74 183.9

Uranium U 92 238.0

Vanadium V 23 50.94

Xenon Xe 54 131.3

Ytterbium Yb 70 173.0

Yttrium Y 39 88.91

Zinc Zn 30 65.38

Zirconium Zr 40 91.22


Element Properties

Name

Form/colorCommon oxidation

statesDensity (g/cm3)

BoilingPoint (°C)

Melting point (°C)

Aluminum Silver metal 3+ 2.702 2467 660.37

Arsenic Gray metalloid 3–, 3+, 5+ 5.72714 613 (sublimes) 817 (28 atm)

Barium Bluish white metal 2+ 3.51 1640 725

Bromine Red-brown liquid 1–, 1+, 3+, 5+, 7+ 3.119 58.78 27.2

Calcium Silver metal 2+ 1.54 1484 839 ± 2

Carbon Diamond 2+, 4+ 3.51 3930 3500 (63.5 atm)

Graphite — 2.25 — 3652 (sublimes)

Chlorine Green-yellow gas 1– 1+, 3+, 5+, 7+ 3.214* 234.6 2100.98

Chromium Gray metal 2+, 3+, 6+ 7.2028 2672 1857 ± 20

Cobalt Gray metal 2+, 3+ 8.9 2870 1495

Copper Red metal 1+, 2+ 8.92 2567 1083.4 ± 0.2

Fluorine Yellow gas 1– 1.69‡ 2188.14 2219.62

Germanium Gray metalloid 4+ 5.32325 2830 937.4

Gold Yellow metal 1+, 3+ 19.31 2808±2 1064.43

Helium Colorless gas 0 0.1785* 2268.9 2272.2 (26 atm)

Hydrogen Colorless gas 1–, 1+ 0.0899* 2252.8 2259.34

Iodine Blue-black solid 1–, 1+, 3+, 5+ 7+ 4.93 184.35 113.5

Iron Silver metal 2+, 3+ 7.86 2750 1535

Lead Bluish white metal 2+, 4+ 11.343716 1740 327.502

Lithium Silver metal 1+ 0.534 1342 180.54

Magnesium Silver metal 2+ 1.745 1107 648.8

Manganese Gray-white metal 2+, 3+, 4+, 6+, 7+ 7.20 1962 1244 ± 3

Mercury Silver liquid metal 1+, 2+ 13.5462 356.58 238.87

Neon Colorless gas 0 0.9002* 2245.9 2248.67

Nickel Silver metal 2+, 3+ 8.90 2730 1455

Nitrogen Colorless gas 3–, 3+, 5+ 1.2506* 2195.8 2209.86

Oxygen Colorless gas 2– 1.429* 2182.962 2218.4

Phosphorus Yellow solid 3–, 3+, 5+ 1.82 280 44.1

Platinum Silver metal 2+, 4+ 21.45 3827 ± 100 1772

Potassium Silver metal 1+ 0.86 760 63.25

Silicon Gray metalloid 2+, 4+ 2.33 ± 0.01 2355 1410

Silver White metal 1+ 10.5 2212 961.93

Sodium Silver metal 1+ 0.97 882.9 97.8

Strontium Silver metal 2+ 2.6 1384 769

Sulfur Yellow solid 2–, 4+, 6+ 1.96 444.674 119.0

Tin White metal 2+, 4+ 7.28 2260 231.88

Titanium White metal 2+, 3+, 4+ 4.5 3287 1660 ± 10

Uranium Silver metal 3+, 4+, 6+ 19.05 ± 0.0225 3818 1132.3 ± 0.8

Zinc Blue-white metal 2+ 7.14 907 419.58

*Densities of gases given in g/L at STP †Densities obtained at 20°C unless otherwise noted (superscript)‡ Density of fluorine given in g/L at 1 atm and 15°C


Figure 4-7

Transition metalsAlk

alin

eea

rth

met

als

Alk

ali m

etal

s

Cha

lco

gen

s

Hal

og

ens

No

ble

gas

es

Lanthanide seriesActinide series

Group names on the periodic table

Figure 4-8

H

Li

Na

K

Rb

Cs

Fr

Be

Mg

Ca

Sr

Ba

Ra

La

Ac

Ce

Th

Pr

Pa

Nd

U

Pm

Np

Sm

Pu

Eu

Am

Gd

Cm

Tb

Bk

Dy

Cf

Ho

Es

Er

Fm

Tm

Md

Yb

No

Lu

Lr

Hf

Rf

Ta

Db

W

Sg

Re

Bh

Os

Hs

Ir

Mt

Pt

Uun

Au

Uuu

Hg

Uub

Tl

Uut

Sc

Y

Ti

Zr

V

Nb

Cr

Mo

Mn

Tc

Fe

Ru

Co

Rh

Ni

Pd

Cu

Ag

Zn

Cd

Ga

In

Pb

Ge

Sn

Bi

As

Sb

Po

Se

Te

At

Br

I

Rn

Kr

Al Si P S Cl Ar

B C N O F Ne

He

Xe

The periodic table

The Periodic Table

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