Chemistry Concept Notes for JEE: Inorganic Chemistry Mixed Topics
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Chemical Bonding
| Species | Shape and hybridisation |
|---|---|
| \(\ce{BCl3}\) | trigonal planar, \(sp^2\), \(120^\circ\) |
| \(\ce{NH3}\), \(\ce{NCl3}\), \(\ce{PH3}\) | pyramidal, one lone pair |
| \(\ce{SF4}\) | see-saw, \(sp^3d\), one lone pair |
| \(\ce{ClF3}\) | T-shaped, \(sp^3d\), two lone pairs |
| \(\ce{XeF4}\) | square planar, \(sp^3d^2\), two lone pairs |
| \(\ce{CF4}\), \(\ce{NH4+}\), \(\ce{BF4-}\) | tetrahedral, \(sp^3\) |
1. Bond order \(= \tfrac12(N_b - N_a)\). Higher bond order means a shorter and stronger bond.
2. For \(\ce{B2}\), \(\ce{C2}\), \(\ce{N2}\) the \(\pi 2p\) orbitals lie below \(\sigma 2p_z\). For \(\ce{O2}\) and \(\ce{F2}\) the order is reversed.
3. Hydrogen bonds need H attached to N, O or F. They explain the high boiling point of \(\ce{NH3}\), alcohols and acids, but ethers cannot form them with themselves.
4. The Born-Haber cycle uses Hess's law to find lattice energy.
5. Nitrogen oxides such as \(\ce{N2O5}\) have covalent and coordinate bonds.
Redox and Selected p-Block and s-Block Facts
1. Oxidation number of N is -3 in \(\ce{NH4+}\) and +5 in \(\ce{NO3-}\).
2. \(\ce{H2O2}\) acts as an oxidising agent when its oxygen goes from -1 to -2, and as a reducing agent when \(\ce{O2}\) is released.
3. Heating PbO in air gives red lead, \(\ce{Pb3O4}\).
4. Silicon forms \(\ce{[SiF6]^{2-}}\) but not \(\ce{[SiCl6]^{2-}}\), because six large chlorides cannot fit round the small atom. Boron cannot exceed a covalency of 4, so no \(\ce{BF6^{3-}}\).
5. LiOH decomposes on heating, unlike the other alkali metal hydroxides.
6. Complex ions such as \(\ce{[Fe(CN)6]^{3-}}\) give no free \(\ce{Fe^{3+}}\), so ordinary tests for the metal ion fail.
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Inorganic Chemistry Mixed Topics Concepts and Summary for JEE Chemistry
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