32 INNER TRANSITION ELEMENTS and 33 INERT GASES

32 and 33

CHAPTER 32 INNER TRANSITION ELEMENTS (8 pages) and CHAPTER 33 INERT GASES(2 pages) are complementary but useful chapters.

All chapters are complementary to one another. All important references are duly acknowledged.

31. ELEMENTS OF GROUP IIB

31

ELEMENTS OF GROUP IIB

CHAPTER 31 -ELEMENTS OF GROUP IIB (9 pages) - answers questions such as:

Why does Hg, an otherwise inert element, react with S and I₂ even at room temperature?

Why does Hg remain as a liquid?

Why the hypothetical next element of the IIB group with atomic number 112 would be a gas with metallic properties, are mentioned.

30. THE ELEMENTS OF GROUP IB

30

ELEMENTS OF GROUP !B

In CHAPTER 30 (9 pages) the dissociation energies of Cu₂, Ag₂, and Au₂ molecules,
 the relative stabilities of Cu⁺ and Cu²⁺ in different environments and 
the stability of the oxidation states of Cu, Ag and Au are theoretically interpreted at great depth.

29 TRANSITION ELEMENTS

29

TRANSITION ELEMENTS

CHAPTER 29 - TRANSITION ELEMENTS (20 pages). In this chapter, the colour of the transition metals and their salts are discussed.

 Reason for the ferromagnetism of Fe, Co and Ni explained. 

Further, the variations in the melting points, boiling points, binding energies and densities of the transition metals are interpreted. 

The variations in the valency of these metals are also interpreted. 

The treatment has great depth.

27 VBT, CFT AND MOT, 28 TRANSITION ELEMENTS - REACTIONS, KINETICS AND MECHANISM

2 7 and 28

CHAPTER 27-VBT, CFT AND MOT (13 pages) and CHAPTER 28 TRANSITION ELEMENTS- REACTIONS, KENETICS AND MECHANISM(4 pages)- are useful but conventional chapters.

26. SECOND AND THIRD PERIODS

26

SECOND AND THIRD PERIODS

CHAPTER 26- SECOND AND THIRD PERIODS (9 pages) - answers many questions such as:

 Why is the formula of nitric acid HNO₃ and not (HO)₅N or H₃NO_4.

Why are SO₂ and CO₂ monomers rather than polymers like SiO₂.

25. SILICON

25

SILICON

CHAPTER 25 - SILICON 5 pages- deals with silicon. In this chapter, the relative strengths of Si-X bond and Si-H bond, C-C bond and Si-Si bond are discussed. 

Reason for the non-polymerization of CO₂, SiX₄ and SiH₄ unlike SiO₂ is given.

 Notes on silicon chip and silicone rubber are also given.

24. OXYGEN AND FLUORINE

24

OXYGEN AND FLUORINE

CHAPTER 24 - OXYGEN AND FLUORINE (9 pages)- is one of the important chapters. The relative oxidizing powers of oxygen and fluorine are interpreted in this chapter. 

This kind of interpretation is not found in other books. 

The fact that the +4 and +6 oxidation states for chlorine are stabilized by oxygen and not by fluorine is clearly discussed. 

In this chapter also a new generalization regarding the stability of oxides, fluorides, oxychloride and oxyflouride has been given.

23. OXYGEN

23

OXYGEN

CHAPTER 23 -OXYGEN (3 pages)- explains why the b.p. of oxygen is higher than either of its neighbours – nitrogen and fluorine. 

Moreover, the magnetic properties of oxygen, 

the instability of O^2- ion,

 the importance of partial negative charge on oxygen,

 reason for the skew structure of H₂O₂ and 

the maximum co-ordination number of oxygen are discussed.

22 NITROGEN

22

NITROGEN

In CHAPTER 22 - NITROGEN  (6 pages)- why does the nature of bonding in the N₂ molecule remain as a challenge to all theories of bonding, 

why is there a sudden drop in melting point from carbon to nitrogen, 

why is solid NO diamagnetic and 

why are certain N III molecules planar are discussed.

CHAPTER 21

CHAPTER 21(6 pages) emphasizes the importance of carbon in organic chemistry. Further, it explains why graphite is more stable than diamond. The reason why CO does not form a complex with any halide of boron is mentioned.

20 BORON

20

BORON

CHAPTER 20 - BORON (4 pages)- gives various definitions for metals and non-metals (metals exhibit only positive oxidation state with the exception of As, Re and Au, but non-metals exhibit +ve and –ve oxidation states). 

Reason for the sudden change from metallic (Be) to non-metallic (B) properties explained.

 Reason for the stability of B₂H₅I, and instability of B₂H₅Cl is mentioned.

19. BERYLLIUM

19

BERYLLIUM

CHAPTER 19 - BERYLLIUM (4 Pages) - is a small chapter. But it explains the reason for the steep increase in the melting point from lithium to beryllium, and then beryllium to carbon. 

It explains why Be, (1s²2s²), is not remaining as a mono-atomic gas just like He(1s²). 

It also explains the greater reactivity of Be compared to He, which has an electronic configuration similar to that of Be.

18. LITHIUM

18

 LITHIUM

In CHAPTER 18 -  LITHIUM (10 Pages)- explanations for mainly the following questions are given.

1. Why is Li₂ molecule not as stable as H₂ molecule?

2. Though Li-Li covalent bond is stronger than the bond in the Li metal lattice, Li atoms try to form a metal lattice of lithium. Why?

3. Why are some alkali metal-salts coloured?

4. Why does Li form lithium bonds?

5. With respect to hydration, why does lithium differ from its diagonally related Mg?

6. Why is LiOH  a stronger base than CsOH in water?

7. “Cs₂CO₃ is more soluble in water than Li₂CO₃. But LiClO₃ is more soluble in water than C_SClO₃”. Why?

8. LiF and certain other alkali metal salts are insoluble, or only slightly soluble, in water. Why?

9. What are the entropy effects on the solubility of the alkali metal salts?

10. Why do Li⁺ and Na⁺ ions retain their water of crystallization in the solid state?

11. Why are alkali metals porous?

17. HYDROGEN

17

HYDROGEN

In CHAPTER 17 - HYDROGEN (15 Pages)-  the preferential polarization of hydrogen (not discussed in any other book) is discussed. Why does hydrogen form a three dimensional lattice when it combines with alkali metals (and not when it combines with electronegative elements), why does the stability of the hydrides decrease down the group in contrast to the respective oxides, why do molecules such as HF₃, HCl₃ are not formed and why is there  no intra molecular hydrogen bonding in CH₃COOH are explained.

     Further, the reason for 1:3 ratio for ortho and para hydrogen, the reason for the increase in oxidation potential with decrease in hydrogen ion concentration, the reason why, say, the electron of the hydrogen atom has same energy when it remains in the 3s, 3p, 3d orbitals are also discussed. 

    The effect of squeezing hydrogen under ultra high pressure ( Ho-Kulang Mao and Russel Homley – 1989) is mentioned.

    Present status of cold fusion given.

16. HYDROLYSIS OF CERTAIN HALIDES

16

HYDROLYSIS OF CERTAIN HALIDES

CHAPTER 16(15 Pages) deals with the mechanism of the hydrolysis of the halides of the elements, which lie in the heart of the periodic table such as B, C, Al, Si, P, S. This chapter explains why halides such as CF₄, NF₃, SF₆ are inert, why SiCl₄ undergoes hydrolysis readily in contrast to CCl₄, why NCl₃ and PCl₃ do not yield the same product on hydrolysis and so on.

15 MELTING POINTS OF CERTAIN HALIDES

15

MELTING POINTS OF CERTAIN HALIDES

In CHAPTER 15 (8 Pages) the melting points of halides of C, Si, Ge, B, Sn and Al have been interpreted based on their structures and electronegativities. For example, it explains why the melting and boiling points of the tetrahalides of the elements of the IV A group fall from carbon to silicon and increase from silicon to lead.

14. HARD AND SOFT ACIDS AND BASES

14

HARD AND SOFT ACIDS AND BASES

CHAPTER 14(2 Pages) is a conventional chapter that mentions Hard and Soft Acids and Bases

13. BASES- STRENGTH AND STABILITY

13. 

BASES- STRENGTH AND STABILITY

In CHAPTER 13(4 Pages) the strength and stability of bases have been discussed mainly based on the charge density and electronegativity of cations.

12. REDOX REACTIONS

12

REDOX REACTIONS

CHAPTER 12(5 Pages) is a conventional chapter in which a few redox reactions such as
As₂S₃ + HNO_3-----> H₃AsO₄ + H₂SO₄ + NO are balanced.

11. REDOX PROPERTIES OF ACIDS

11

           REDOX PROPERTIES OF ACIDS

In CHAPTER 11 (7 pages), the redox properties of the acids have been discussed based on the electron configuration and structure. It explains, for instance, why H₂SO₃ is more oxidizing than H₂SO₄.

10. STABILITY OF ACIDS

10

STABILITY OF ACIDS

CHAPTER 10 (10 pages). In this chapter, the acids have been grouped together as in the above chapter. The depth of the treatment could be gauged from the fact that as many as 10 points have been given while interpreting the stability of the acids of the series

H₄SiO₄ – H₃PO₄ – H₂SO₄ – HClO₄

and equal number of points, including alternating effect, while interpreting the stability of the acids of the series

ClO₄^- BrO₄^- IO₆^5-

SO₄^2- SeO₄^2- TeO₆^6-

9 STRENGTHS OF ACIDS

9

STRENGTHS OF ACIDS

CHAPTER 9 (11 pages) Ignoring the leveling effect of water, the relative strengths of acids have been interpreted based on their structures and electron configurations. After going through this chapter, one would write a few sentences about the relative strengths of, say, HNO₃ and HClO₃.

In this chapter, the acids have been grouped together as given below.

IV A V A VI A VII A

(H₂CO₃) HNO₃

(H₂SiO₄) H₃PO₄ H₂SO₄ HClO₄

H₃AsO₄ H₂SeO₄ HBrO₄

H₆TeO₆ H₃IO₅