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What will be the spatial distribution of...

What will be the spatial distribution of (i) `sp^(3)`,
(ii) `sp^(2)`
and (iii) sp hybrid orbitals?

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(i) `sp^(3)`-In this case, each of the hybrid orbitals are directed towards the four corners of tetrahedron.
(ii) `sp^(2)`- in this case, each of the hybrid orbitals are directed towards the three corners of a triangle.
(iii) sp-In this case, the two hybrid orbitals linearly arranged.
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Quantum mechanical calcuations show that mathematical mixing of certain combinaaation of orbitals in a given atom forms hybrid orbitals. The spatial orientations of these new orbitals lead to more stable bonds and are consistent with the observed molecular shapes . The process of orbital mixing is called hybridization and the new atomic orbitals are called hybrid orbitals.- Conditions (i) The no. of hybrid orbitals equal the number of atomic orbitalsmixed. (ii)The type of hybrid orbitals obtained varies with the type of atomic orbitals mixed. Rules to determine hybrid orbitals. Method i:Count no .of atoms directiy attached to central atom + lone pairs+single electrons. Method II: Count sigma - bonds+co-ordinate bonds+ lone pair+single electrons. If the number comes one to be 2 implies sp 5 implies sp^3d/dsp^3 3 implies sp^2 6 implies sp^3d^2/d^2sp^3 4 implies sp^3/dsp^2 7 implies sp^3d^3 Answer the following questions based on above passage : Phosphorous pentachloride in gaseous state exists as a momomer. In solid state, it exists as PCl_5^+. PCl_6^- ions. The hybrid state of P atom in PCl_5 is sp^3d . The hybrid state of P atoms in PCl_4^+ and PCl_6^- will be respectively

Quantum mechanical calcuations show that mathematical mixing of certain combinaaation of orbitals in a given atom forms hybrid orbitals. The spatial orientations of these new orbitals lead to more stable bonds and are consistent with the observed molecular shapes . The process of orbital mixing is called hybridization and the new atomic orbitals are called hybrid orbitals.- Conditions (i) The no. of hybrid orbitals equal the number of atomic orbitalsmixed. (ii)The type of hybrid orbitals obtained varies with the type of atomic orbitals mixed. Rules to determine hybrid orbitals. Method i:Count no .of atoms directiy attached to central atom + lone pairs+single electrons. Method II: Count sigma - bonds+co-ordinate bonds+ lone pair+single electrons. If the number comes one to be 2 implies sp 5 implies sp^3d/dsp^3 3 implies sp^2 6 implies sp^3d^2/d^2sp^3 4 implies sp^3/dsp^2 7 implies sp^3d^3 Answer the following questions based on above passage : Hybrid states of Xe in XeF_2, XeF_4 and XeF_6 respectively are :

Which of the following molecules represents the order of hybridisation sp^(2) , sp^(2) , sp , sp from left to right atoms ?

The posatively charged carbon atom in structure (I) is sp^(2) - hybridised while the negatively charged carbon atom in (II) is sp^(3) - hybridised - Explain.

CHHAYA PUBLICATION-CHEMICAL BONDING AND MOLECULAR STRUCTURE-WARM UP EXERCISE
  1. Which symmetry element is present in a pi-bond?

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  2. What is meant by hybridisation of atomic orbitals?

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  3. What will be the spatial distribution of (i) sp^(3), (ii) sp^(2) a...

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  4. Is hybridisation possible in an isolated atom?

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  5. The state of hybridisation of the central atom of which of the followi...

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  6. Name the type of hybridisation of the central atom which leads to eaac...

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  7. Identify the state of hybridisation of each carbon in: (i) CH(2)=CH-...

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  8. The four C-H bonds in methane are equivalent though carbon was differe...

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  9. Arrange ehthane, ethylene and acetylene in order of their decreasing C...

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  10. Total number of lone pair of electrons in I(3)^(-) ion is -

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  11. Why are the P-Cl bonds in PC l(5) not of same length?

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  12. Which of the molecules or ions are iso-structural and why? BF(3),NH(...

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  13. All the C-O bond lengths in CO(3)^(2-) are equal-explain.

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  14. Give reasons for the extra stability of benzene.

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  15. Write the canonical structures for sulphite ion and phosphate ion.

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  16. All the C-O bond lengths in CO(3)^(2-) are equal-explain.

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  17. Define electronegativity of an element.

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  18. Explain Pauling's scale of electronegativity.

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  19. Which is the most electronegative element according to the pauling's s...

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  20. Which one among the following pairs is more electronegative and why? ...

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