chem6a_f11 hol - chapter 2_part b

Handout #2B (Fall 2011) Chem 6A - Prof. John E. Crowell

Chem 6A - Chapter 2 (Part B)

Types of Chemical FormulasTypes of Chemical Formulas

An empirical formula indicates the relative number of atoms of each element in the compound. It is the simplest type of formula.

A molecular formula shows the actual number of atoms of each element in a molecule of the compound.

A structural formula shows the number of atoms and the bonds between them, that is, the relative placement and connections of atoms in the molecule.

A chemical formula is comprised of element symbols and numerical subscripts that show the type and number of each atom present inthe smallest unit of the substance.

The empirical formula for hydrogen peroxide is HO.

The molecular formula for hydrogen peroxide is H2O2.

The structural formula for hydrogen peroxide is H-O-O-H.

90Chap 2: Matter and Nomenclature

Some Common Monatomic Ions of the ElementsSome Common Monatomic Ions of the Elements

Can you see any patterns?



Chap 2: Matter and Nomenclature 93

Nomenclature: BasicsNomenclature: BasicsTwo general classes of inorganic molecules:

1. Those containing a metal cation and a nonmetal anion OR a metal cation and a polyatomic anion (ionic compounds). There are two types of these ionic compounds:

(a). Those whose metal has only one possible positive oxidation state (Type I compounds);

(b). Those whose metal has more than one possible positive oxidation state (Type II compounds)

2. Those containing only nonmetals (molecular compounds; Type III compounds)

The nomenclature scheme reflects the compounds class or type.


““Type IType I”” ElementsElements1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18

IA VIII

A

1 H

1.008

IIA

IIIA

IVA

VA

VIA

VIIA

2 He

4.002

3 Li

6.941

4 Be 9.01

2

5 B

10.81

6 C

12.01

7 N

14.01

8 O

16.00

9 F

19.00

10 Ne

20.18

11 Na 22.9

9

12 Mg

24.30

IIIB IVB VB VIB VIIB VIII VIII VIII IB IIB

13 Al

26.98

14 Si

28.09

15 P

30.97

16 S

32.06

17 Cl

35.45

18 Ar

39.95

19 K

39.10

20 Ca 40.0

8

21 Sc

44.96

22 Ti

47.90

23 V

50.94

24 Cr

52.00

25 Mn 54.9

4

26 Fe

55.85

27 Co 58.9

3

28 Ni

58.70

29 Cu 63.5

5

30 Zn

65.38

31 Ga 69.7

2

32 Ge 72.5

9

33 As 74.9

2

34 Se

78.96

35 Br

79.90

36 Kr

83.80

37 Rb 85.4

7

38 Sr

87.62

39 Y

88.91

40 Zr

91.22

41 Nb 92.9

1

42 Mo 95.9

4

43 Tc

(99)

44 Ru 101.

1

45 Rh 102.

9

46 Pd 106.

4

47 Ag 107.

9

48 Cd 112.

4

49 In

114.8

50 Sn 118.

7

51 Sb 121.

8

52 Te

127.6

53 I

126.9

54 Xe

131.3

55 Cs 132.

9

56 Ba 137.

3

57 La

138.9

72 Hf

178.5

73 Ta

180.9

74 W

183.9

75 Re 186.

2

76 Os 190.

2

77 Ir

192.2

78 Pt

195.1

79 Au 197.

0

80 Hg 200.

6

81 Tl

204.4

82 Pb 207.

2

83 Bi

209.0

84 Po

(209)

85 At

(210)

86 Rn

(222)

87 Fr

(223)

88 Ra 226.

0

89 Ac 227.

0

104 Rf

(261)

105 Db

(262)

106 Sg

(263)

107 Bh

(262)

108 Hs

(265)

109 Mt

(266)

110 Db

(269)

Lanthanide series Actinide series

= Type I Metal

= Type II Metal

= Type III Non-metal

= Does not form compounds

58 Ce 140.

1

59 Pr

140.9

60 Nd 144.

2

61 Pm (147

)

62 Sm 150.

4

63 Eu 152.

0

64 Gd 157.

3

65 Tb 158.

9

66 Dy 162.

5

67 Ho 164.

9

68 Er

167.3

69 Tm 168.

9

70 Yb 173.

0

71 Lu 175.

0 90 Th 232.

0

91 Pa

231.0

92 U

238.0

93 Np

(237)

94 Pu

(244)

95 Am (243

)

96 Cm (247

)

97 Bk

(247)

98 Cf

(251)

99 Es

(252)

100 Fm (257

)

101 Md (258

)

102 No

(259)

103 Lr

(260)

+3+2

+1

+2

+1




““Type IIType II”” ElementsElements1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18

IA VIII

A

1 H

1.008

IIA

IIIA

IVA

VA

VIA

VIIA

2 He

4.002

3 Li

6.941

4 Be 9.01

2

5 B

10.81

6 C

12.01

7 N

14.01

8 O

16.00

9 F

19.00

10 Ne

20.18

11 Na 22.9

9

12 Mg

24.30


13 Al

26.98

14 Si

28.09

15 P

30.97

16 S

32.06

17 Cl

35.45

18 Ar

39.95

19 K

39.10

20 Ca 40.0

8

21 Sc

44.96

22 Ti

47.90

23 V

50.94

24 Cr

52.00

25 Mn 54.9

4

26 Fe

55.85

27 Co 58.9

3

28 Ni

58.70

29 Cu 63.5

5

30 Zn

65.38

31 Ga 69.7

2

32 Ge 72.5

9

33 As 74.9

2

34 Se

78.96

35 Br

79.90

36 Kr

83.80

37 Rb 85.4

7

38 Sr

87.62

39 Y

88.91

40 Zr

91.22

41 Nb 92.9

1

42 Mo 95.9

4

43 Tc (99)

44 Ru 101.

1

45 Rh 102.

9

46 Pd 106.

4

47 Ag 107.

9

48 Cd 112.

4

49 In

114.8

50 Sn 118.

7

51 Sb 121.

8

52 Te

127.6

53 I

126.9

54 Xe

131.3

55 Cs 132.

9

56 Ba 137.

3

57 La

138.9

72 Hf

178.5

73 Ta

180.9

74 W

183.9

75 Re 186.

2

76 Os 190.

2

77 Ir

192.2

78 Pt

195.1

79 Au 197.

0

80 Hg 200.

6

81 Tl

204.4

82 Pb 207.

2

83 Bi

209.0

84 Po

(209)

85 At

(210)

86 Rn

(222)

87 Fr

(223)

88 Ra 226.

0

89 Ac 227.

0

104 Rf

(261)

105 Db

(262)

106 Sg

(263)

107 Bh

(262)

108 Hs

(265)

109 Mt

(266)

110 Db (269

)


= Type I Metal

= Type II Metal



58 Ce 140.

1

59 Pr

140.9

60 Nd 144.

2

61 Pm (147

)

62 Sm 150.

4

63 Eu 152.

0

64 Gd 157.

3

65 Tb 158.

9

66 Dy 162.

5

67 Ho 164.

9

68 Er

167.3

69 Tm 168.

9

70 Yb 173.

0

71 Lu 175.

0 90 Th 232.

0

91 Pa 231.

0

92 U

238.0

93 Np

(237)

94 Pu

(244)

95 Am (243

)

96 Cm (247

)

97 Bk

(247)

98 Cf

(251)

99 Es

(252)

100 Fm (257

)

101 Md (258

)

102 No

(259)

103 Lr

(260)


““Type IIIType III”” Elements: NonmetalsElements: Nonmetals1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18

IA VIII

A

1 H

1.008

IIA

IIIA

IVA

VA

VIA

VIIA

2 He

4.002

3 Li

6.941

4 Be 9.01

2

5 B

10.81

6 C

12.01

7 N

14.01

8 O

16.00

9 F

19.00

10 Ne

20.18

11 Na 22.9

9

12 Mg

24.30


13 Al

26.98

14 Si

28.09

15 P

30.97

16 S

32.06

17 Cl

35.45

18 Ar

39.95

19 K

39.10

20 Ca 40.0

8

21 Sc

44.96

22 Ti

47.90

23 V

50.94

24 Cr

52.00

25 Mn 54.9

4

26 Fe

55.85

27 Co 58.9

3

28 Ni

58.70

29 Cu 63.5

5

30 Zn

65.38

31 Ga 69.7

2

32 Ge 72.5

9

33 As 74.9

2

34 Se

78.96

35 Br

79.90

36 Kr

83.80

37 Rb 85.4

7

38 Sr

87.62

39 Y

88.91

40 Zr

91.22

41 Nb 92.9

1

42 Mo 95.9

4

43 Tc

(99)

44 Ru 101.

1

45 Rh 102.

9

46 Pd 106.

4

47 Ag 107.

9

48 Cd 112.

4

49 In

114.8

50 Sn 118.

7

51 Sb 121.

8

52 Te

127.6

53 I

126.9

54 Xe

131.3

55 Cs 132.

9

56 Ba 137.

3

57 La

138.9

72 Hf

178.5

73 Ta

180.9

74 W

183.9

75 Re 186.

2

76 Os 190.

2

77 Ir

192.2

78 Pt

195.1

79 Au 197.

0

80 Hg 200.

6

81 Tl

204.4

82 Pb 207.

2

83 Bi

209.0

84 Po

(209)

85 At

(210)

86 Rn

(222)

87 Fr

(223)

88 Ra 226.

0

89 Ac 227.

0

104 Rf

(261)

105 Db

(262)

106 Sg

(263)

107 Bh

(262)

108 Hs

(265)

109 Mt

(266)

110 Db

(269)


= Type I Metal

= Type II Metal



58 Ce 140.

1

59 Pr

140.9

60 Nd 144.

2

61 Pm (147

)

62 Sm 150.

4

63 Eu 152.

0

64 Gd 157.

3

65 Tb 158.

9

66 Dy 162.

5

67 Ho 164.

9

68 Er

167.3

69 Tm 168.

9

70 Yb 173.

0

71 Lu 175.

0 90 Th 232.

0

91 Pa

231.0

92 U

238.0

93 Np

(237)

94 Pu

(244)

95 Am (243

)

96 Cm (247

)

97 Bk

(247)

98 Cf

(251)

99 Es

(252)

100 Fm (257

)

101 Md (258

)

102 No

(259)

103 Lr

(260)




Nomenclature Periodic TableNomenclature Periodic Table1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18

IA VIII

A

1 H

1.008

IIA

IIIA

IVA

VA

VIA

VIIA

2 He

4.002

3 Li

6.941

4 Be 9.01

2

5 B

10.81

6 C

12.01

7 N

14.01

8 O

16.00

9 F

19.00

10 Ne

20.18

11 Na 22.9

9

12 Mg

24.30


13 Al

26.98

14 Si

28.09

15 P

30.97

16 S

32.06

17 Cl

35.45

18 Ar

39.95

19 K

39.10

20 Ca 40.0

8

21 Sc

44.96

22 Ti

47.90

23 V

50.94

24 Cr

52.00

25 Mn 54.9

4

26 Fe

55.85

27 Co 58.9

3

28 Ni

58.70

29 Cu 63.5

5

30 Zn

65.38

31 Ga 69.7

2

32 Ge 72.5

9

33 As 74.9

2

34 Se

78.96

35 Br

79.90

36 Kr

83.80

37 Rb 85.4

7

38 Sr

87.62

39 Y

88.91

40 Zr

91.22

41 Nb 92.9

1

42 Mo 95.9

4

43 Tc (99)

44 Ru 101.

1

45 Rh 102.

9

46 Pd 106.

4

47 Ag 107.

9

48 Cd 112.

4

49 In

114.8

50 Sn 118.

7

51 Sb 121.

8

52 Te

127.6

53 I

126.9

54 Xe

131.3

55 Cs 132.

9

56 Ba 137.

3

57 La

138.9

72 Hf

178.5

73 Ta

180.9

74 W

183.9

75 Re 186.

2

76 Os 190.

2

77 Ir

192.2

78 Pt

195.1

79 Au 197.

0

80 Hg 200.

6

81 Tl

204.4

82 Pb 207.

2

83 Bi

209.0

84 Po

(209)

85 At

(210)

86 Rn

(222)

87 Fr

(223)

88 Ra 226.

0

89 Ac 227.

0

104 Rf

(261)

105 Db

(262)

106 Sg

(263)

107 Bh (262

)

108 Hs

(265)

109 Mt

(266)

110 Db

(269)


= Type I Metal

= Type II Metal



58 Ce 140.

1

59 Pr

140.9

60 Nd 144.

2

61 Pm (147

)

62 Sm 150.

4

63 Eu 152.

0

64 Gd 157.

3

65 Tb 158.

9

66 Dy 162.

5

67 Ho 164.

9

68 Er

167.3

69 Tm 168.

9

70 Yb 173.

0

71 Lu 175.

0 90 Th 232.

0

91 Pa

231.0

92 U

238.0

93 Np

(237)

94 Pu

(244)

95 Am (243

)

96 Cm (247

)

97 Bk

(247)

98 Cf

(251)

99 Es

(252)

100 Fm (257

)

101 Md (258

)

102 No

(259)

103 Lr

(260)

Common Common MonoatomicMonoatomic IonsIons

H- hydride

Na+ sodium

H+ hydrogen

Li+ lithium fluorideF-

Cs+ cesium

K+ potassium

Ag+ silver

chlorideCl-

bromideBr-

iodideI-

Mg2+ magnesium

Sr2+ strontium

Ca2+ calcium

Zn2+ zinc

Ba2+ barium

Cd2+ cadmium

Al3+ aluminum

1+

2+

3+

CationsCharge Formula Name

AnionsCharge Formula Name

1-

2-

3-

oxideO2-

sulfideS2-

nitrideN3-

Common anions are in blue.




Nomenclature: Nomenclature: CationCation BasicsBasicsTo name a cation (or the first element in a Type III

compound): Type I: Use the name of the element; if you are talking

about an ion by itself put ‘ion’ after the name: Na+ = sodium ion; Mg+2 = magnesium ion Special cations: NH4

+ = ammonium ion; H3O+ = hydronium ion

Type II: Use the name of the element AND its oxidation state (or charge); use roman numerals in parentheses to denote this; if you are talking about an ion by itself put ‘ion’ after the name:

Cu+2 = copper (II) ion; Cr+6 = chromium (VI) ion

Type III : Use the name; denote number of that element present using greek prefixes (more later).


Nomenclature: Anion BasicsNomenclature: Anion BasicsTo name a monatomic anion (OR the second element in a

binary Type III compound):

For ALL: Take the root name of the element and add -ide to the end: if you are talking about an ion by itselfput ‘ion’ after the name:

Cl- = chloride ion; S-2 = sulfide ion; P-3 = phosphide ion

Type III Compounds ONLY: Add to the name of the second element a prefix denoting how many of that element there are:

XO2 would be “X dioxide”, e.g. titanium dioxide

POLYATOMIC ANIONS: These have their own nomenclature you need to know




Nomenclature: Polyatomic AnionsNomenclature: Polyatomic AnionsLearn these polyatomic anions names:

HCO3- Hydrogen carbonate

HS- Hydrogen sulfide

HSO4- Hydrogen sulfate

HSO3- Hydrogen sulfite

H2PO4- Dihydrogen phosphate

ClO4- Perchlorate

ClO3- Chlorate

ClO2- Chlorite

ClO- Hypochlorite

BrO3- Bromate

BrO2- Bromite

BrO- Hypobromite

IO4- Periodate

IO3- Iodate

C2H3O2- Acetate

NO3- Nitrate

NO2- Nitrite

OH- Hydroxide

MnO4- Permanganate

CO3-2 Carbonate

SO4-2 Sulfate

SO3-2 Sulfite

C2O4-2 Oxalate

CrO4-2 Chromate

Cr2O7-2 Dichromate

SCN- Thiocyanate

CN- Cyanide

HPO4-2 Hydrogen Phosphate

PO4-3 Phosphate


Nomenclature: Polyatomic AnionsNomenclature: Polyatomic AnionsLearn these “-ate” polyatomic anions names:

HCO3- Hydrogen carbonate

HS- Hydrogen sulfide

HSO4- Hydrogen sulfate

HSO3- Hydrogen sulfite

H2PO4- Dihydrogen phosphate

ClO4- Perchlorate

ClO3- Chlorate

ClO2- Chlorite

ClO- Hypochlorite

BrO3- Bromate

BrO2- Bromite

BrO- Hypobromite

IO4- Periodate

IO3- Iodate

C2H3O2- Acetate

NO3- Nitrate

NO2- Nitrite

OH- Hydroxide

MnO4- Permanganate

CO3-2 Carbonate

SO4-2 Sulfate

SO3-2 Sulfite

C2O4-2 Oxalate

CrO4-2 Chromate

Cr2O7-2 Dichromate

SCN- Thiocyanate

CN- Cyanide

HPO4-2 Hydrogen Phosphate

PO4-3 Phosphate




Nomenclature: Nomenclature: OxyanionsOxyanionsSystematic nomenclature based on oxoacids of origin;End in -ate or -ite; may have per- or hypo- as prefixes;Learn name, formula, and charge of all -ate ions, then:

a) If an ion has ONE LESS oxygen than the -ate ion, change -ate to -ite (charge does not change!);

b) If an ion has TWO LESS oxygens than the -ate ion, change -ate to -ite and add hypo- as a prefix (charge does not change!);

c) If an ion has ONE MORE oxygen than the -ate ion, add per-as a prefix (charge does not change!).

ClO3 ClO2 ClOClO4

Onemore O

Oneless O

Oneless O

chlorateperchlorate chlorite hypochlorite

Two less O's


Nomenclature: Type I and II CompoundsNomenclature: Type I and II Compounds

Simple: take name of cation and anion and combine:

CaCl2 = calcium chloride

ZnS = zinc sulfide

Ba3(PO4)2 = barium phosphate

CrO3 = chromium (VI) oxide

PbI4 = lead (IV) iodide

Fe2O3 = iron (III) oxide




Determining Determining cationcation charge for Type II ionscharge for Type II ions

Based on knowing your anions and their charges!

A compound is neutral and has a charge of zero.

The sum of all the oxidation states in a compound must equal the overall charge on the ion or molecule.

Set up and solve for the unknown algebraically; so for Fe2O3:

2 3

×

×

# irons charge of iron +

# oxygens charge of oxygen

62x + 3 -2 = 0; solve to get x = =

= charge

+

of

2

e

3

F O

1. START by naming as if it were a Type I compound:

N2F4: nitrogen fluoride

2. THEN add a greek prefix to tell how MANY of each element there are:

N2F4: dinitrogen tetrafluoride

* Note: if there is only one of the first element, the prefix mono is NOT used:

SO2 is sulfur dioxide NOT monosulfur dioxide


Nomenclature: Type III CompoundsNomenclature: Type III Compounds

1 = mono 2 = di 3 = tri 4 = tetra 5 = penta

6 = hexa 7 = hepta 8 = octa 9 = nona 10 = deca



Chap 2: Matter and Nomenclature110

Nomenclature: PracticeNomenclature: PracticeTry the following:

C2O4

Na2SO3

MgO

CrO2

P5O10

AsO3

SeO4

Al2Cr2O7

Mo(CO3)2

Rh(NO3)5

H2O

N2O

Give yourself five minutes


Nomenclature: PracticeNomenclature: PracticeAnswers:

C2O4 dicarbon tetroxide

Na2SO3 sodium sulfite

MgO magnesium oxide

CrS2 chromium (IV) sulfide

P5O10 pentaphosphorus decoxide

AsO3 arsenic trioxide




Nomenclature: PracticeNomenclature: PracticeAnswers:

SeO4 selenium tetroxide

Al2Cr2O7 aluminum dichromate

Mo(CO3)2 molybdenum (IV) carbonate

Rh(NO3)5 rhodium (V) nitrate

H2O dihydrogen monoxide

N2O dinitrogen monoxide


Nomenclature: Exceptions (1)Nomenclature: Exceptions (1)1. Some compounds have been known and used for so

long that their trivial (or common names) have become accepted by the IUPAC as official:

H2O = water CH4 = methane PH3 = phosphine

NH3 = ammonia SiH4 = silane N2H4 = hydrazine

2. Oxides of some nonmetals will sometimes be named as if they were Type II compounds:

P2O5 = phosphorus (V) oxide; SeO3 = selenium (VI) oxide

Note: this is an older nomenclature system that is slowly being phased out.




Nomenclature: Exceptions (2)Nomenclature: Exceptions (2)3. For Type II metals with only two common oxidation

states an older, Latin system was once used; while it is not employed very often it is useful to know some simple rules regarding it. It is sometimes called the “-ous/-ic” system, where the LOWER charged cation will be denoted by the latin root name for that element plus -ous and the HIGHER charged cation will be denoted by the latin root name for that element plus -ic :

Fe2+ = ferrous ion/Fe3+ = ferric ion; Sn2+ = stannous ion/Sn4+ = stannic ion

Not used much but still can be found being employed

4. Compounds containing hydrogen listed as the first element are acids and named differently, as are many carbon compounds.


Acid NomenclatureAcid NomenclatureAn acid is a compound that contains an acidic

hydrogen (an H that ionizes in water) :

Not all hydrogens are ionizable; by convention, to indicate when one IS, we begin the chemical formula with it:

HC2H3O2 (acetic acid) has four hydrogens but only ONE is acidic (underlined for emphasis)

There are two types of acids: binary and oxoacids

HX(aq) H (aq) X – (aq)




Binary Acid NomenclatureBinary Acid NomenclatureFor BINARY acids (HX(aq), where X does NOT

contain oxygen; it MUST be in aqueous solution); Add hydro…ic acid to the root of the element X:

H2S (aq) = hydrosulfuric acid; HI (aq) = hydroiodic acid; HN3 (aq) = hydrazoic acid

Note: if phase is NOT aqueous, name as if it were a Type I compound (even though they are considered to be molecular in nature):

H2S (g) = hydrogen sulfide; HI (g) = hydrogen iodide; HN3 (l) = hydrogen azide


OxoacidOxoacid NomenclatureNomenclatureIf the acid contains oxygen (HOX or HXOn) its name will

be a function of the name of the anion portion (i.e. the portion remaining after all the acidic H’s have been removed: OX- or XOn

-); so:

Determine the anion name;

If the name ends in -ate, replace -ate with -ic acid

If the name ends in -ite, replace -ite with -ous acid

Leave prefixes alone; the root name is sometimes tweaked to aid in pronunciation

H2SO4(aq) anion is SO4-2 (sulfate) acid name is sulfuric acid

HClO(aq) anion is ClO- (hypochlorite) acid name is hypochlorous acid




Acid Nomenclature: PracticeAcid Nomenclature: Practice

Try the following:

H2C2O4

H2SO3

HCN

H2CrO4

H3PO4

H2Se

HIO4

H2CO3

HF

HC2H3O2

HNO3

HNO2

Give yourself five minutes


Acid Nomenclature: PracticeAcid Nomenclature: PracticeAnswers:

H2C2O4 oxalic acid

H2SO3 sulfurous acid

HCN hydrocyanic acid

H2CrO4 chromic acid

H3PO4 phosphoric acid

H2Se hydroselenic acid




Acid Nomenclature: PracticeAcid Nomenclature: PracticeAnswers:

HIO4 periodic acid

H2CO3 carbonic acid

HF hydrofluoric acid

HC2H3O2 acetic acid

HNO3 nitric acid

HNO2 nitrous acid

MixturesHeterogeneous mixtures: have one or more visible boundaries between the components.

Homogeneous mixtures: have no visible boundaries because the components are mixed as individual atoms, ions, and molecules.

Solutions: A homogeneous mixture is also called a solution. Solutions in water are called aqueous solutions, and are very important in chemistry. Although we normally think of solutions as liquids, they can exist in all three physical states.

122Chap 2: Matter and Nomenclature



66

Clicker Problem 3: Atomic Symbols The picture (a) below depicts which atom or ion given

below?

a). 18O 2- b). 18N 2- c). 17N 3-

d). 19F - e). 17O 2-

Clicker Problem 6: Binary Ionic Compounds

Write the molecular formula for the ionic compound formed from the following pairs of elements: magnesium and nitrogen?

a). MgN b). MgN2 c). NMgN

d). Mg3N2 e). Mg2N3

chem6a_f11 hol - chapter 2_part b

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