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1. Inorganic Chemistry
Representative Elements
Lecture (1): Periodic Table and Periodicity
Part 1
Dr Abbas Mamdoh

2. • Know the mean of inorganic chemistry.
• Study the atomic structure.
• State the periodic law and explain the organization of elements
• Predict the general properties of elements based on their location.
• Identify metals, nonmetals, and metalloids
• Type of chemical bonding.
• Chemistry of s-block elements
• Chemistry of p-block elements
CourseAim

3. Course Contents
1. Periodic Table and Periodic Properties
2. Chemical Bonding
3. Hydrogen and its Compounds
4. Chemistry of Group 1 Elements
5. Chemistry of Group 2 Elements
6. Chemistry of Group 13 Elements
7. Chemistry of Group 14 Elements
8. Chemistry of Group 15 Elements
9. Chemistry of Group 16 Elements
10. Chemistry of Group 17 Elements
11. Chemistry of Group 18 Elements

4. 1. Cotton, F.A.; Wilkinson, G. (1988). Advanced Inorganic Chemistry (5th
Edn). New York: Wiley. ISBN 0-471-84997p. 1385.
2. Hutchinson, John. "Journal of Chemical Education." Concept
Development Studies in Chemistry (2007). Print. Outside Links
3. Jolly, William L. (1991). Modern Inorganic Chemistry (2nd Edn.). New
York: McGraw-Hill. ISBN 0-07-112651-1.Petrucci, Ralph H. General
Chemistry. 9th ed. New Jersey: Pearson Prentice Hall, 2005.
References

5. Assessment Schedule andWeights
Assessment 1: Mid – term examination (15 grades) 10% (7th week )
Assessment 2: Final practical exam (30 grades) 20% (12th week )
Assessment 3: Oral exam (15 grades ) 10%
Assessment 4: Final term exam (90 grades ) 60%

6. • The branch of chemistry concerned with the elements and all their compounds except those
containing carbon and hydrogen. Some simple carbon and hydrogen compounds, such as
oxides, carbonates, etc, are treated as inorganic.
• Inorganic chemistry is concerned with the properties and behavior of inorganic compounds,
which include metals, minerals, and organometallic compounds.
• While organic chemistry is defined as the study of carbon-containing compounds and
inorganic chemistry is the study of the remaining subset of compounds other than organic
compounds,
What is mean by inorganic chemistry?

7. Atomic structure

8. • Atomic number (z).
• Atomic mass (A) or nucleon number or mass number
• Atomic weight.
• Isotopes
• Isotone
• Isobar
• Isoelectronic species
• Allotropes
Some atomic terms

9. Periodic table
❖Law of Triads (1829 Johann Dobereiner )
❖Law of Octaves (1864 John Newlands )

10. Periodic table
❖Lother Meyer’s (1870)
❖Mendeleev's (1868-1870)
▪ Advantages of Mendeleev’s Periodic
o Systematic study of the elements
o Correction of atomic weights
o Predict the properties of undiscovered elements

11. Periodic table
➢ Disadvantages of Mendeleev’s Periodic
▪ Position of hydrogen.
▪ Anomalous pairs. (argon (at.wt. 39.9) and potassium (at.wt. 39.1); cobalt (at.wt. 59.9) and
nickel (at.wt. 58.6) and tellurium (at.wt. 127.6) and iodine (at.wt. 126.9).
▪ Position of isotopes
▪ Similar elements in different groups and dissimilar elements in the same
group
▪ Position of lanthanides and actinides
▪ Elements in VIII group
▪ Cause of periodicity

12. Periodic table
o This led Moseley to conclude that atomic
number and not atomic weight is the
fundamental property of the atoms.
➢ two defects in Mendeleev’s table were
corrected.
o Anomalous pairs were eliminated.
o Isotops
❖ Modern periodic table (Henry Moseley 1942)
This led to the modern periodic law as the physical and chemical properties of the
elements are periodic functions of their atomic numbers

13. Periodic table
The Long Form Periodic Table (extended form )
• The long form periodic table is constructed on the basis of repeating
electronic configuration. (based on increasing of atomic number).

14. Periodic table
▪ Nomenclature of Elements with Atomic Number Above 100

15. Periodic table
The Long Form Periodic Table
I. Periods:
II.Groups:

16. Periodic table
▪ Classification of Elements
into s, p, d and f block
Elements
Be 1s22s2
B 1s22s2 2p1
The Long Form Periodic Table

17. Periodic table
▪ Classification of Elements into s, p, d and f block Elements
▪ s-Block elements (ns1or2)
I. except hydrogen all these elements are metals
II. they are soft metals with low melting and boiling points
III.their ionization energies are low.
IV.alkali metals exhibit +I and alkaline earth metals exhibit +II oxidation states
V. they form ionic compounds
VI.they are strong reducing agents
The Long Form Periodic Table

18. Periodic table
▪ Classification of Elements into s, p, d and f block Elements
2. p-Block elements (ns2np1-6)
I. consists of metals, non-metals and metalloids.
II. Their ionization energies are relatively high as compared to s-block
elements.
III. Generally they form covalent compounds (mostly).
IV. Most of these elements exhibit variable valence
V. Gradually the reduction power decreases and oxidation power increases
from left to right
The Long Form Periodic Table

19. Periodic table
▪ Classification of Elements into s, p, d and f block Elements
3. d-Block elements (n–1)d1–10 ns1 or 2)
I. all metals having high melting and boiling points
II. they are good conductors of electricity
III. they form colored compounds
IV.they form complex compounds
V. their compounds are generally paramagnetic
VI.the metals and their compounds have catalytic activity
VII.they exhibit variable valency
The Long Form Periodic Table

20. Periodic table
▪ Classification of Elements into s, p, d and f block Elements
4. f-Block elements (n–2) f1–14 (n–1) d0 or 1 ns2)
I. they are heavy metals
II. they generally have high melting and boiling points
III. they exhibit variable valence
IV.they form colored compounds and their compounds are paramagnetic
V. they have a tendency to form complex compounds
VI.Actinides are radioactive in nature
The Long Form Periodic Table

21. Periodic table
▪ Classification of the Elements Based on Properties
1. Noble gases
2. Representative elements
3. Transition elements
4. (Inner transition elements
▪ Classification of Elements into Metals, Non-metals and Metalloids
The Long Form Periodic Table

22. Periodic table
▪ Prediction of period, group and block of an element:
1. The period number of an element is equal to the principal quantum number
value of the valence shell.
2. Block of the element corresponds to the subshell into which the
differentiating electron enters.
3. Group number of an element is equal to the number of electrons present in
the valence shell or penultimate shell as follows.
o For s-block elements group number is equal to number of valence
electrons (ns electrons)
o For p-block elements group number is equal to 10 + number of valence
electrons (ns + np)
o For d-block elements group number is equal to number of electrons in
(n–1)d and ns subshells.

23. ▪ Prediction of period, group and block of an element:
▪ Write the electronic configuration of the elements with atomic numbers (29,
33, 55, 63, 86). Predict the period, group and the block to which it belong.
Periodic table

24. ➢ Periodic Trends in properties of elements.
➢ Periodicity
▪ The repetition of similar properties of the elements after certain regular
intervals when they are arranged in the order of increasing atomic
numbers.
➢ Cause of periodicity.
▪ The repetition of similar electronic configuration of their atoms in the
outermost shell (or valence shell) after certain regular intervals.
Periodic table

25. ➢ Periodic Trends in properties of elements.
Periodic table

26. ➢ Effective Nuclear Charge
Effective nuclear charge is the charge felt by the valence electrons
after you have considered the number of shielding electrons that
surround the nucleus.
Periodic table
Zeff = Z – S
Z is the atomic number
S shielding constant or Screening constant

27. ➢ Effective Nuclear Charge
❖ Slater's rules for effective nuclear charge
1. Write the electronic configuration for the atom using the following grouping, called
Slater electron configuration: (1s) (2s,2p) (3s,3p) (3d) (4s,4p) (4d) (4f) (5s,5p) ... ,
2. Any electron to the right of the considered electron of interest do not contribute to
shielding,
3. All other electrons in the same group of the considered electron shield by 0.35 nuclear
charge units each; except for 1s, the screening is reduced to 0.30,
Periodic table

28. ➢ Effective Nuclear Charge
❖ Slater's rules for effective nuclear charge
4. All the electrons in the n–1 shell (penultimate shell) shield (ns,np)
electrons to an extent of 0.85 each.
5. All the electrons in n–2 shell or lower, shield completely that is their
contribution is 1.00 each.
6. All the electrons in groups lying to the left of ‘nd’ or ‘nf ’ group
contribute 1.00.
Periodic table

29. ➢ Effective Nuclear Charge
What is the effective nuclear charge experienced by a valence p-
electron in boron?
1s2 2s22p1
(1s2)(2s2,2p1)
S [2p] = 0.85(2) + 0.35(2) = 2.40
Z = 5
Zeff=2.60
Periodic table

30. ➢ Effective Nuclear Charge
What is the shielding constant experienced by a 3d electron in the
bromine atom?
Br: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
Br: (1s2)(2s2,2p6)(3s2,3p6)(3d10)(4s2,4p5)
S [3d] = 1.00(18) + 0.35(9) = 21.15
Periodic table

31. ➢ Effective Nuclear Charge
▪ Calculate the effective nuclear charge for the following
1. Nitrogen (7N):
2. Zinc (30 Zn).
3. Screening constant for 3d electron in zinc.
Periodic table