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Navigating the Periodic Table 1
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Navigating the Periodic Table
1
What is the Periodic Table?
• An organization of Earth's elements arranged according to atomic number, the number of protons each element's nucleus contains
2
• The structure of the periodic table corresponds directly to atomic structure. This makes the table an invaluable tool for determining the property and behavior of elements and predicting how they will interact.
Introduction to the Periodic Table • In the 1860’s a Russian chemistry teacher
named Dmitri Mendeleev was searching for a way to categorize and make sense of the growing number of elements for his students and invented the Periodic Chart.
• He placed the elements in columns (groups or families) according to their similar chemical and physical properties and in rows (periods) by increasing mass.
• The chart is periodic because the chemical and physical properties of the elements repeat again and again. The same way that a calendar is periodic.
• His brilliance came because of his willingness to leave spaces where he expected elements to be in his chart, but where none had yet been discovered. Sure enough is a few years three more undiscovered elements were isolated to fit in the holes in his chart
3
Groups and Periods • Columns aka Groups aka Families • Rows aka Periods • Why is it called the “Periodic” Chart?
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo 4
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
Group (Family) • A column or group of
columns in the periodic table; elements in one group have the same number of electrons in the outermost shell
5
• Elements in each group share similar chemical properties
Period • A row of the periodic
table; each row corresponds to the number of electron shells in an atom of the elements in that row
• The elements in the second period each have two electron shells, and the elements in the sixth period have six electron shells
Metals vs Nonmetals • Nonmetals • Metals
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo 6
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
Metals vs Nonmetals • Metals are elements that
are generally shiny when smooth and clean, solid at room temperature, and good conductors of heat and electricity.
7
• Physical properties include • Efficient conduction of heat
and electricity • Malleability (can be
hammered into thin sheets) • Ductility (can be pulled into
wires) • A lustrous (shiny) appearance
• Nonmetals are elements that are generally gases or brittle, dull-looking solids, and poor conductors of heat and electricity.
• Generally lack those properties that characterize metals and show much more variation in their properties than metals do
Some Metal Families • Alkali Metals (very, very reactive) • Alkaline Earth Metals (quite reactive) • Transition Metals
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
8
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
The Mixed Groups • Families containing both metals and nonmetals • The aluminum family • The the eight metals (and more) under the staircase
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
9
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
Metalloids (Semimetals) • Close to the “stair-step” and often show a mixture
of metallic and nonmetallic properties.
10
Some of the Nonmetals • Halogens • Noble Gases aka Inert Gases (Unreactive)
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo 11
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
Modern Period Table
12
Natural State of Elements • Most elements are reac-ve • We do not o1en find elements in nature in pure form (more o1en combined with other things)
• There are excep-ons of course! ~ Noble Gases ~ Diatomic Molecules (N2, O2, F2, Cl2, Br2, I2, H2)
13
• What types of ion is formed? (i.e. Ca-on (+) OR Anion (-‐)) • Periodic table guides us! • Group 1 form +1 ca-ons, Group 2 form +2, Group 3 form +3…etc, etc • Transi-on metals form various types of ca-ons
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo 14
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
Ions and the Periodic Table
Compounds that contain ions Writing Chemical Formulas • Ionic compounds – compound between a metal and a non-‐metal
• There must be ca-ons (+) and anions (-‐) present • When combining, the overall charge for the compound must be zero (0)
• Metal (ca-on) comes first THEN non-‐metal (anion) comes second
15
Naming Ionic compounds • Metal comes first and keeps its name • Non-‐metal comes second and add -‐ide at the end • Example: combining sodium and chlorine becomes….Sodium Chloride
16
17
Write the chemical formula for sodium chloride
• When combined together Na+ Cl−
• Metals lose e-‐ (+ ion = ca-on) • Nonmetals gain e-‐ (-‐ ion = anion) • NaCl
1A" 2A" 8A"3A" 4A" 5A" 6A" 7A"
1+" 1B" 2B" 3B" 4B" 5B" 6B" 7B" 8B" 9B" 10B" 1-"
18
Write the chemical formula for magnesium =luoride
• Overall charge must equal zero • Mg(2+) + F(1-‐) = 1+ • (1)2+ + 2(1-‐) = 0 Do the “criss cross method” • MgF2 çNo4ce where we put the number 2
1A" 2A" 8A"3A" 4A" 5A" 6A" 7A"
1-"2+" 1B" 2B" 3B" 4B" 5B" 6B" 7B" 8B" 9B"10B"
19
Write the chemical formula for strontium sul=ide
• Sr2+ S2− you might have wriaen Sr2S2
• always write ionic formula in lowest whole number ra-o so….
• SrS
20
Write the chemical formula for potassium nitride
• K+ N3−
• K3N
21
Write the chemical formula for Beryllium Arsenide
• Be2+ As3− • Be3As2
Naming Ionic compound
• Remember metal THEN non-‐metal with –ide added to non-‐metal
• Write the name for: NaCl • Na = Sodium • Cl = Chlorine • So….Sodium Chloride
22
Write the name for Li2O
• Li = Lithium • O = Oxygen • Lithium Oxide
23
Write the name for CaBr2
• Ca = Calcium • Br = Bromine • Calcium Bromide
24
Write the name for Na2S
• Sodium Sulfide
25
Write the name for LiI
• Lithium Iodide
26
Write the name for KCl
• Potassium Chloride
27
Ionic Compounds Involving Roman #’s and Nomenclature
Transition Metals • Metal with different ionic states • Can use knowledge of what it is combined with to figure out charge on transi-on metal
• Metal comes first THEN non-‐metal (FeO)
29
1A" 2A" 8A"
3A" 4A" 5A" 6A" 7A"
1B" 2B" 3B" 4B" 5B" 6B" 7B" 8B" 9B" 10B"
2+"1+"2+"
Naming Ionic with Roman #’s
30
• Metal comes first and keeps it’s name with a (roman #) indicating the charge
• Example: Iron with a 2+ charge would be
Iron (II) • Non-metal comes second and add -ide at
the end
Example: combining Iron(II) and oxygen becomes….Iron(II) Oxide or FeO
Write the chemical formula for Copper (I) oxide • Roman # (I) gives info for charge on copper so…1+
• Cu1+ O2− use the ‘criss cross method’ • Cu2O
31
32
Write the chemical formula for iron(III) oxide
• Roman # (III) gives info for charge on iron so…3+
• Fe3+ O2− use the ‘criss cross method’ • Fe2O3
33
Write the chemical formula for zinc chloride
• Remember that zinc is one of the transi-on metals that does not require a Roman #, since it’s oxida-on state is always +2.
• Cl-‐ • ZnCl2
1A" 2A" 8A"3A" 4A" 5A" 6A" 7A"
1B" 2B" 3B" 4B" 5B" 6B" 7B" 8B" 9B" 10B"
2+"1+"2+"
34
Write the chemical formula for chromium (VI) sul=ide
• The Roman # tells you the +6 charge on the chromium metal
• Cr6+ S2− • You might have criss-‐crossed to Cr2S6 but then you must reduce it to the lowest whole number ra-o.
• CrS3
35
Write the name for NiSe
• Ni = ?? • Se = 2- charge • There is only 1 element of each in
the compound above so Nickel MUST have a 2+ charge
• nickel(II) selenide
36
Write the name for TiSe
• Ti = ?? • Se = 2-‐ • 1 element of each • Ti MUST be 2+ charge • Titanium (II) Selenide
37
Write the name for Fe2O3 • you can un-‐criss-‐cross • or you can determine the charge on iron by working from the charge on the anion • Fe2? O32−
• 3 x 2− = 6− • so 2 x ? = 6+ so ? must equal 3+
38
Write the name for Ag2S • Ag = Silver (Exception: always
+1 charge) • S = Sulfur (We know this has a
2- charge) • Silver sulfide
39
Write the name for Ag2S • No need for a Roman # since silver is always +1
• (that’ s a memorize, along with Zn and Cd) • Silver Sulfide
1A" 2A" 8A"
3A" 4A" 5A" 6A" 7A"
1B" 2B" 3B" 4B" 5B" 6B" 7B" 8B" 9B" 10B"
2+"1+" 2+"
40
Write the name for CrP2 • you can’t just un-‐criss-‐cross because this is a formula which has been reduced. • work off the non-‐metal’s charge • Cr? P23− • 2 x 3− = 6− • so ? = 6+ • chromium (VI) phosphide
Ionic Compounds using Polyatomic Ions
• Nomenclature
What is a Polyatomic Ion? • A cluster of atoms (usually nonmetals) that use molecular bonding within the cluster, and that require extra electrons to be sa-sfied
• More than one atom covalently bonded (sharing electrons) together carrying a charge (the cluster needs to gain or lose electrons to be sa-sfied).
42
-‐ates and -‐ites
43
nitrite NO2
− sulfite SO3
2− phosphite
PO33−
nitrate NO3
− sulfate SO4
2− phosphate
PO43−
What if there’s more than two?
44
hypochlorite ClO−
chlorite ClO2−
chlorate ClO3−
perchlorate ClO4−
Notable Exceptions
45
ammonium a positive polyatomic
NH4+
cyanide CN−
hydroxide OH−
ferricyanide Fe(CN)63−
ferrocyanide Fe(CN)64−
Write the chemical formula for calcium nitrate
46
• Ca2+ NO3−
• Note: Nitrate does not have a -‐3 charge! The 3 subscript notes that the nitrate polyatomic ion contains 3 oxygen
• use the ‘criss cross method’
• Ca(NO3)2 çNo4ce we need parentheses and where we put the number 2
Write the chemical formula for calcium chlorate
• Ca2+ ClO3−
• use the ‘criss cross method’
• Ca(ClO3)2
47
Write the chemical formula for iron (III) dichromate
• Fe3+ Cr2O72− • Fe2(Cr2O7)3
• note that dichromate does not mean two chromates, it is a par-cular ion
• it got its name for the two chromium’s in the ion, not because there will be two of the polyatomic ions in the compound
48
Write the chemical formula for nickel(II) nitrite
• Ni2+ NO2−
• Ni(NO2)2
49
Write the chemical formula for gallium cyanide
• Ga+3 CN-‐
• Ga(CN)3 • not GaCN3 • you need 3 cyanides, not 3 N’s and 1C
50
Write the name for KBrO
51
• K = Potassium • BrO = hypobromite
• Potassium hypobromite
Write the name for Mn(SO4)2
• We know that we need a Roman # for the manganese, so we need to figure out its charge. • Mn? (SO4)2−2 • 2 x 2− = 4− so 1 x ? = 4+ • ? must be 4+ • Manganese(IV) sulfate
52
Write the name for (NH4)3PO4 • ammonium, NH4+ is one of the few posi-ve polyatomic ions
• Phosphate, PO4-‐3
• Ammonium phosphate
53
Write the name for Ca2Fe(CN)6 • How do you know that it is ferrocyanide, not ferricyanide?
• You do know the charge on the calcium ion is 2+ • 2 x 2+ = 4+ • thus the anion must be 4− to match.
• and ferrocyanide is 4− • calcium ferrocyanide
54
Write the name for AuSCN
• SCN is a polyatomic ion 1− • 1 of each element • thus the gold must be 1+ to balance • gold(I) thiocyanate
55
Write the chemical formula for tin(IV) hydroxide
• Sn(OH)4
56
Write the name for CuCO3
• copper(II) carbonate
57
Write the chemical formula for copper(I) ferrocyanide
• Cu2Fe(CN)6 58
Write the name for CoAs
• cobalt(III) arsenide
59
Write the chemical formula for uranium(VI) =luoride • UF6
60
Write the name for cadmium acetate • Cd(C2H3O2)2
61
Write the chemical formula for iron(III) sul=ite • Fe2(SO3)3
62
Write the name for Cr(ClO)3
• chromium(III) hypochlorite
63
Write the chemical formula for ammonium nitrate • NH4NO3
64
Write the name for Mg(OH)2
• magnesium hydroxide
65
Write the chemical formula for K3Fe(CN)6 • potassium ferricyanide
66
Write the name for Pb(Cr2O7)2
• lead(IV) dichromate
67
Acids • Nomenclature
Systematic Method -‐ Naming Acids
69
nitrous"HNO2" HNO3" nitric"sulfurous"H2SO3" H2SO4" sulfuric"
phosphorous"H3PO3" H3PO4" phosphoric"
H2CO3" carbonic"
HC2H3O2" acetic"
HF" hydrofluoric"HCl" hydrochloric"HBr" hydrobromic"HI" hydroiodic"
H2S" hydrosulfuric"HCN" hydrocyanic"
Does the anion contain oxygen?
No hydro-(anion root)-ic
Yes check the ending of the root
-ITE (anion root)-ous
-ATE (anion root)-ic
HClO3" chloric"HClO4" perchloric"
Naming binary molecular compounds
• Nonmetal combined with nonmetal • No charges -‐ do not try to figure out the formula with charges -‐ there are none.
• The name must tell us the formula • Prefixes will tell us the number of each atom. • The second element listed: -‐ide • mono is op-onal • di-‐, tri-‐, tetra-‐, penta-‐, hexa-‐, septa-‐, octo-‐, nono-‐, deca-‐
70
It’s all in the name....
71
Review • Nomenclature
Naming binary molecular compounds
• Nonmetal combined with nonmetal • No charges -‐ do not try to figure out the formula with charges -‐ there are none.
• The name must tell us the formula • Prefixes will tell us the number of each atom. • The second element listed: -‐ide • mono is op-onal • di-‐, tri-‐, tetra-‐, penta-‐, hexa-‐, septa-‐, octo-‐, nono-‐, deca-‐
73
How to remember the polyatomic acids?? • It’s alphabe-cal! • −ate is an −ic acid
• sulfate = sulfuric acid • nitrate = nitric acid • acetate = ace-c acid
• −ite is an −ous acid (−ous acids are always weak acids) • sulfite = sulfurous acid • nitrite = nitrous acid • phosphite = phosphorous
74
Types of Bonding • Elements can be classified as metal or nonmetal. • These two categories gives rise to three types of bonding:
• Ionic: metal & nonmetal • Molecular: nonmetal & nonmetal • Metallic: metal & metal Electron Sea Model
• Valence electrons are uniformly distributed around the remaining ca-ons of each atom.
• Electrons are loose and able to move.
75
Binary Molecular Compounds • Prefixes (they should be memorized) used to indicate the number of atoms of each element. • mono, di, tri, tetra, penta, hexa, hepta, octo, nono, deca, (11), dodeca
• Less electronega-ve element usually listed first
• Second element listed ends in -‐ide • For most compounds with more than two elements we will use their common names, not the IUPAC naming system except for some simple organic compounds
76
Ionic vs Molecular
77
Metal + Nonmetal" Nonmetal + Nonmetal"Particles called formula units" Particles called molecules"
Electrons transferred" Electrons are shared"
Metals lose e− and become a + ion (cation)" No ions are formed"
Nonmetal gain e− and become a − ion (anion)" No ions are formed"
Formula is always written in lowest whole number ratio"
Formula may not always be in lowest whole number ratio"
Some metals require roman # to indicate charge" No Roman Numerals"
No prefixes unless part of the polyatomic name"
Prefixes are used to indicate the number of atoms in formula"
Ionic Compounds • Ca-on (+) ion (usually metals) listed first
• metals retain the same name • Ammonium: the + polyatomic ion
• Anion (−) ion listed second • Nonmetal (some polyatomic contain metals)
• Binary compounds (only two different elements) end in -‐ide • Polyatomic compounds end in −ite or −ate
• A few excep-ons end in −ide • Most of the table should be memorized
• Certain metals require Roman # to indicate their charge.
78
Bonding between Metal Atoms Sea of Electrons Model • The small yellow spheres represent the valence electrons that move freely about.
• The large white spheres represent the remainder of the atom, a posi-ve ion made of the inner core electrons + nucleus.
79
Sea of Electrons Model to explain metallic properties • easily excitable electrons = colored flames • good electrical conductor • shiny • good thermal conductor • malleable • duc-le
80
Descriptive Symbolism • Single atom • Two atoms stuck together, diatomic molecule
• Two atoms not stuck together • A single ion with a 1-‐ charge, having gained 1e-‐
• An atom showing its atomic number • A nuclide, a par-cular isotope showing its mass number
• A nuclide with its mass number
81
F" F2"2F"
F-1"
21F"9F"Fluorine-19
Using the Chart to Predict Charges • Group 1: Alkali Metals, lose 1 e− = 1+ • Group 2: Alkaline Earth Metals, lose 2 e− = 2+ • Group 3 (metals): Aluminum Group, lose 3 e− = 3+ • Group 7: Halogens, gain 1 e− = 1− • Group 6: Oxygen group, gain 2 e− = 2− • Group 5: Nitrogen group, gain 3 e− = 3− • Don’t forget about the 3 transi-on metals to memorize
82
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
1H
2He
3Li
4Be
5B
6C
7N
8O
9F
10Ne
11Na
12Mg
13Al
14Si
15P
16S
17Cl
18Ar
19K
20Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
71Lu
72Hf
73Ta
73W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
103Lr
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111Uuu
112Uub
113Uut
114Uuq
116Uuh
118Uuo
+2
+2 +1
