Exam T

1
Exam T Chapters 7 and 8 Review M 5 SL 110
2
(No Transcript)
3
Figure 8.12 A periodic table illustrating the
building-up order.
4
Figure 8.14 Mendeleevs periodic table.
5
Reactivity of the Alkali Metals
Lithium video
2Li(s) 2H2O(l) ? 2LiOH(aq) H2(g)
Sodium video
2Na(s) 2H2O(l) ? 2NaOH(aq) H2(g)
Potassium video
2K(s) 2H2O(l) ? 2KOH(aq) H2(g)
Trend?
6
More Sodium Reaction Videos
2Na(s) 2H2O(l) ? 2NaOH(aq) H2(g)
http//www.theodoregray.com/PeriodicTable/
Prepping Na
150 g Na in small pieces
100 g Na in one piece
7
(No Transcript)
8
Figure 8.17 Representation of atomic radii
(covalent radii) of the main-group elements.
9
Atomic Radii of the Main-Group and Transition
Elements
10
(No Transcript)
11
(No Transcript)
12
Electronic Configuration Ions

• Na 1s 2 2s 2 2p 6 3s 1 Na 1s 2
  2s 2 2p 6
• Mg 1s 2 2s 2 2p 6 3s 2 Mg2 1s 2 2s
  2 2p6
• Al 1s 2 2s 2 2p 6 3s 2 3p 1 Al3 1s 2
  2s 2 2p 6
• O 1s 2 2s 2 2p 4 O- 2 1s
  2 2s 2 2p 6
• F 1s 2 2s 2 2p 5 F- 1
  1s 2 2s 2 2p 6
• N 1s 2 2s 2 2p 3
  N- 3 1s 2 2s 2 2p 6

13
Isoelectronic Atoms and Ions

• H- 1 He Li Be2
• N- 3 O- 2 F- Ne Na Mg2
  Al3
• P- 3 S- 2 Cl- Ar K Ca2
  Sc3 Ti4
• As- 3 Se- 2 Br- Kr Rb Sr2
  Y3 Zr4
• Sb- 3 Te- 2 I- Xe Cs Ba2
  La3 Hf4

14
Pseudo - Noble Gas Electron Configurations
Elements in groups 3A, 4A, and 5A can form
cations by losing enough electrons to leave a
pseudo noble gas configuration. By losing
electrons and leaving a filled d orbital, which
is quite stable!
Sn Kr 5s24d105p2
Sn4 Kr 4d10 4 e - Sn Kr 5s24d105p2
Sn2 Kr 5s24d10
2 e - Pb Xe 4f145d106s26p2
Pb2 Xe 4f145d106s2 2 e- Pb Xe
4f145d106s26p2 Pb4 Xe
4f145d10 4 e- As Ar 3d104s24p3
As3 Ar 3d104s2 3
e- As Ar 3d104s24p3
As5 Ar 3d10 5 e- Sb Kr 4d105s25p3
Sb3 Kr
4d105s2 3 e- Sb Kr 4d105s25p3
Sb5 Kr 4d10 5 e-
15
(No Transcript)
16
Ranking Ions According to Size
Problem Rank each set of Ions in order of
increasing size. a) K, Rb, Na b) Na,
O2-, F - c) Fe2, Fe3 Plan We find the
position of each element in the periodic table
and apply the ideas of size i) size increases
down a group, ii) size decreases across a period
but increases from cation to anion. iii) size
decreases with increasing positive (or
decreasing negative) charge in an isoelectronic
series. iv) cations of the same element decreases
in size as the charge increases. Solution a)
since K, Rb, and Na are from the same group
(1A), they increase in size down the
group Na lt K lt Rb b) the ions Na, O2-,
and F- are isoelectronic. O2- has lower Zeff than
F-, so it is larger. Na is a cation, and
has the highest Zeff, so it is smaller
Na lt F- lt O2- c) Fe2 has a lower charge than
Fe3, so it is larger Fe3 lt Fe2
17
Ranking Ions According to Size
Problem Rank each set of Ions in order of
increasing size. a) K, Rb, Na b) Na,
O2-, F - c) Fe2, Fe3 Plan We find the
position of each element in the periodic table
and apply the ideas of size i) size increases
down a group, ii) size decreases across a period
but increases from cation to anion. iii) size
decreases with increasing positive (or
decreasing negative) charge in an isoelectronic
series. iv) cations of the same element decreases
in size as the charge increases. Solution a)
since K, Rb, and Na are from the same group
(1A), they increase in size down the
group Na lt K lt Rb b) the ions Na, O2-,
and F- are isoelectronic. O2- has lower Zeff than
F-, so it is larger. Na is a cation, and
has the highest Zeff, so it is smaller
Na lt F- lt O2- c) Fe2 has a lower charge than
Fe3, so it is larger Fe3 lt Fe2
18
Periodicity of First Ionization Energy (IE1)
Like Figure 8-18
19
Fig. 8.15
20
(No Transcript)
21
Identifying Elements by Its Successive
Ionization Energies
Problem Given the following series of
ionization energies (in kJ/mol)
for an element in period 3, name the element and
write its electron
configuration
IE1 IE2 IE3
IE4 580
1,815 2,740
11,600 Plan Examine the values to find the
largest jump in ionization energy,
which occurs after all valence electrons have
been removed. Use the periodic
table! Solution
22
Identifying Elements by Its Successive
Ionization Energies
Problem Given the following series of
ionization energies (in kJ/mol)
for an element in period 3, name the element and
write its electron
configuration
IE1 IE2 IE3
IE4 580
1,815 2,740
11,600 Plan Examine the values to find the
largest jump in ionization energy,
which occurs after all valence electrons have
been removed. Use the periodic
table! Solution
The largest jump in IE occurs after IE3 so the
element has 3 valence electrons thus it is
Aluminum ( Al, Z13), its electron configuration
is
1s2 2s2 2p6 3s2 3p1
23
Fig. 8.16
24
Ranking Elements by First Ionization Energy
Problem Using the Periodic table only, rank the
following elements in each
of the following sets in order of increasing
IE! a) Ar, Ne, Rn b) At, Bi, Po c)
Be, Na, Mg d) Cl, K, Ar Plan Find their
relative positions in the periodic table and
apply trends! Solution
25
Ranking Elements by First Ionization Energy
Problem Using the Periodic table only, rank the
following elements in each
of the following sets in order of increasing
IE! a) Ar, Ne, Rn b) At, Bi, Po c)
Be, Na, Mg d) Cl, K, Ar Plan Find their
relative positions in the periodic table and
apply trends! Solution
a) Rn, Ar,Ne These elements are all noble
gases and their IE
decreases as you go down the group.
26
Suggested problems for Chapter 9
19, 20, 21, 22, 23, 25, 27, 29, 35, 37, 39, 43,
47, 49, 51, 53, 55, 56, 60, 62, 65, 79, 85, 93,
95, 96, 97 103, 105, 107
27
Chapter 9 - Models of Chemical Bonding
9.1) Atomic Properties and Chemical Bonds 9.2)
The Ionic Bonding Model 9.3) The Covalent
Bonding Model 9.4) Between the Extremes
Electronegativity and Bond Polarity 9.5) An
Introduction to Metallic Bonding
28
(No Transcript)
29
Sodium Chloride
30
Depicting Ion Formation with Orbital Diagrams and
Electron Dot Symbols - I
Problem Use orbital diagrams and Lewis
structures to show the formation of magnesium
and chloride ions from the atoms, and determine
the formula of the compound. Plan Draw the
orbital diagrams for Mg and Cl. To reach filled
outer levels Mg loses 2 electrons, and Cl will
gain 1 electron. Therefore we need two Cl atoms
for every Mg atom. Solution
Mg
Mg2 2 Cl-

..
2 Cl
.
..
..
..
.
Cl Cl
.
..
..
..
..
Mg
Mg2 2 Cl
.
..
..
31
Depicting Ion Formation from Orbital Diagrams and
Electron Dot Symbols - II
Problem Use Lewis structures and orbital
diagrams to show the formation of potassium and
sulfide ions from the atoms, and determine the
formula of the compound. Plan Draw orbital
diagrams for K and S. To reach filled outer
orbitals, sulfur must gain two electrons, and
potassium must lose one electron. Solution
2 K

2 K S - 2
S
..
.
.
2 -
.
..
..
..
..
..
K
.

S
2 K S
K
32
Three Ways of Showing the Formation ofLi and F
- through Electron Transfer
33
Lewis Electron-Dot Symbols for Elements in
Periods 2 3
34
The Reaction between Na and Br to Form NaBr
The Elements
The Reaction!