Among noble gases, Xe is quite reactive and form a number of fluorides and oxyfluorides. In these compounds the electrons, from 5p orbitals are excited to 5d orbitals. The predicted shapes of xenon fluorides are linear, square planar and distorted octahedron. The shapes of xeon oxyfluorides can be prodicted by VSEPR theory.

The chemical reactivity of noble gases involves the loss of electrons and hence it can form compounds with highly electronegative elements like F and O. Although Xe forms several fluorides, xenone tetrafluoride is the most important among fluorides. The various compounds of xenon involve xenon in first, second or third excited states. The type of hybridisation and shape of XeF_(2) respectively are

The chemical reactivity of noble gases involves the loss of electrons and hence it can form compounds with highly electronegative elements like F and O. Although Xe forms several fluorides, xenone tetrafluoride is the most important among fluorides. The various compounds of xenon involve xenon in first, second or third excited states. The type of hybridisation and number of lone pair (s) of electrons on Xe in XeOF_(2) respectively are

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 :

Statement I : Compared to other noble gases 'Xe' is chemically active. Statement II : 'Xe' has low IP value and vacant 'd' orbitals, available for the excitation of electrons from 'p' orbitals of valence shell.

Give the correct order of initials T or F for following statements. Use T if statement is true and F if it is falese : (I) The order of repulsion between different pair of electron is I_(p)-I_(p)gtI_(p)-b_(p)gtb_(p)-b_(p) (II) In general, as the number o flone pair of electron on central atom increases, value of bond angle from normal bond angle also increases (III) The number of lone pair on O in H_(2)O is 2 while on N in NH_(3) is 1 (IV) The structures of xenon fluorides and xenon oxyfluorides could not be explained on the basis of VSEPR theory

Give the correct order of initials T or F for following statements. Use T if statement is true and F if it is falese : (I) The order of repulsion between different pair of electron is I_(p)-I_(p)gtI_(p)-b_(p)gtb_(p)-b_(p) (II) In general, as the number o flone pair of electron on central atom increases, value of bond angle from normal bond angle also increases (III) The number of lone pair on O in H_(2)O is 2 while on N in NH_(3) is 1 (IV) The structures of xenon fluorides and xenon oxyfluorides could not be explained on the basis of VSEPR theory

Give the correct order of initials T or F for following statements. Use T if statement is true and F if it is falese : (I) The order of repulsion between different pair of electron is I_(p)-I_(p)gtI_(p)-b_(p)gtb_(p)-b_(p) (II) In general, as the number o flone pair of electron on central atom increases, value of bond angle from normal bond angle also increases (III) The number of lone pair on O in H_(2)O is 2 while on N in NH_(3) is 1 (IV) The structures of xenon fluorides and xenon oxyfluorides could not be explained on the basis of VSEPR theory

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

In octahedral complexes having co-ordination number 6, the degeneracy of the d-orbitals of central atom is removed due to ligand electron metal electron repulsions. In the octahedral complex three orbitals have lower energy, t_(2g) set and two orbitals have higher energy, eg set. This phenomenon is formed as crystal field splitting and the energy seperation is denoted by Delta_(0) . Thus the energy of the two eg orbitals will increase by (3//5)Delta_(0) and that of the three t_(2g) will decrease by (2//5)Delta_(0) . The erystal field splitling, Delta_(0) depends upon the field produced by the ligand and charge on the metal ion. Some ligands are able to produce strong field and in these cases, the splitting will be large whereas other produce weak fields and consequently result in small splitting of d-orbitals. Predict the order of Delta_(0) for the following compound i) [Fe(H_(2)O)_(6)]^(+2) ii) [Fe(CN)2(H_(2)O)_(4) iii) [Fe(CN)_(4)(H_(2)O)_(2)]^(2-)