A Chemical Rebus
networks
interconnected
-s
The interconnected network of ideas for (4) understanding
HIO4, periodic acid – H+ (acid) = the periodic table.
The Interconnected Network of
Ideas for Understanding the
Periodic Table
•
•
•
•
•
•
Periodic Law
Uniqueness Principle
Diagonal Effect
Inert Pair Effect
Metal/Non-Metal Line
Acid-Base Properties of
Oxides
• Standard Reduction
Potentials
• p-d Interactions
The First Five Components of the Network of Ideas
Periodic Law
Uniqueness Principle
Diagonal
Effect
Inert
Pair
Effect
Metal
NonMetal
Line
Zeff inc left to right ; const vertically
Radii decrease up and to the right
Periodic Law
IE, EA, EN increase up and to the
right
A periodic repetition of physical and chemical
properties occurs when the elements are arranged in
order of increasing atomic number.
Figure 9.9 A Summary of the General Vertical and
Horizontal Periodic Trends in Effective Nuclear Charge
(Zeff), Atomic Radii (r), Ionization Energy (IE), Electron
Affinities (EA), and Electronegativities (EN). This
Representation of the Periodic Law Is the First Component
of the Interconnected Network of Ideas for Understanding
the Periodic Table.
Figure 9.16
Figure 9.6
Uniqueness Principle
(a) The small size of the elements
leading to a high degree of polarizing
power and a high degree of covalent
character in their compounds.
(b) The greater probability of pi bonds.
(c) The lack of availability of d
orbitals.
The chemistry of the second period elements (Li, Be, B, C, N, O, F,
Ne) is quite often significantly different from that of the other
elements in their respective groups.
Figure 9.13 A summary of three reasons for the uniqueness
principle.
Figure 9.5
Notice the small size of the Period 2 elements
Figure
9.10
(*) Charge density: the
charge-to-radius ratio of a
cation or anion; taken to be
directly proportional to
polarizing power (the
ability to produce an
induced dipole) of that ion.
The high charge density of
the lithium ion polarizes the
chloride ion and enhances
the covalent character of the
Li-Cl bond
Figure 9.11
Due to the small size of the period 2 elements, π-bonds
(specifically so-called pπ-pπ bonds) are more likely to form.
Figure 9.12
Figure 9.13
A summary of the three
reasons for the uniqueness
principle
Diagonal
Effect
A diagonal relationship exists between the chemistry of the first
member of a group and that of the second member of the next group
Figure 9.15 The elements of the diagonal effect. Lithium and
magnesium, beryllium and aluminum, and boron and silicon,
each pair diagonally located, have similar properties.
Fig 9.14 Four Relevant Properties of elements related to the
diagonal effect
Inert
Pair
Effect
The valence ns2 electronic of metallic elements, particularly
those 5s2 and 6s2 pairs that follow the second- and third-row
transition metals, are less reactive than we would expect on
the basis of trensds in effective nuclear charge, atomic sizes,
and ionization energies.
Metal
NonMetal
Line
The stepwise diagonal metal/nonmetal line divides the metals
(to the bottom left of the line) from the nonmetals (to the top
right of the line. The semi-metals (B, Si, Ge, As, Sb, Te, and At)
are pictured along the line.
Figure 9.18 The metal-nonmetal line
The First Five Components of the
Interconnected Network of Ideas
Figure
9.18,
Front
Left
Cover
& p.227
Periodic trends in Zeff,
IE, EA, EN and r
(a) Uniqueness Principle
(b) Diagonal Effect
(c) Inert Pair Effect
(d) Metal-Nonmetal Line
The Sixth Component
The Acid-Base Character of Oxides
Figure 11.16
Front Right
Cover (color)
& p. 284
(B/W)
MO
=H2O=>
M+ + OH-
NMO
=H2O=>
H3O+ +
NMO-
The Seventh Component
Trends in Standard Reduction Potentials
Figure 12.5,
Back Left
Cover (color)
& p 318
(B/W)
Good
Reducing
Agents
Eo = Standard
Reduction Potential
Good
Oxidizing
Agents
The Eighth Component
The p-d bonding involving the elements
of the second and third periods
Figure 15.5
Back Right
Cover (color)
& p 398
(B/W)