Home
Class 12
CHEMISTRY
Account for the follwing : (i) Bi(v) ...

Account for the follwing :
(i) `Bi(v)` is a stronger oxidizing agent then Sb(v).
(ii) N-N single bond is weaker then P - P Single bond.
(iii) Noble gases have very low boiling points.

Text Solution

Verified by Experts

(i) Because in inert pair effect + 5 oxidation state is less in Bi then in Sb. So the bi in + 5
state will immediately get reducced to its +3 state and thus will be a better oxidizing agent than + 5 state of Sb
(ii) N-N single bond is weaker then P-P bond due to smaller size of N as compared to P.
Smaller size of N leads to the lone pair of electons on the both the N atoms repal each
other leading to unstability or weakening of N-N bond.
(iii) Noble gases have weak interatomic forces between them and thus have a very low boiling point.
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • XII BOARDS

    XII BOARDS PREVIOUS YEAR|Exercise SET - II|13 Videos

  • XII BOARDS

    XII BOARDS PREVIOUS YEAR|Exercise SET- III|10 Videos

  • SAMPLE PAPER 2019

    XII BOARDS PREVIOUS YEAR|Exercise SECTION: D|1 Videos

Similar Questions

Explore conceptually related problems

Account for the statement : Noble gases have very low boiling points.

(a) Give reasons for the following: (i) Sulphurin vapour state shows paramagnetic behaviour. (ii) N-N bond is weaker than P-P bond. (iii) Ozone is thermodynamically less stable than oxygen. (b) Write the name of gas released when Cu is added to: (i) dilute HNO_(3) and, (ii) conc. HNO_(3)

Knowledge Check

  • Single N-N bond is weaker than the single P-P bond. This is because of :

    A
    larger `N-N` bodn length in comparison to `P-P` bond length.
    B
    high interelectronic repulsion of the non`-` bondioni electrons, owing to the small `N-N` bond length in comparison to that in that in `P-P` single bond.
    C
    Higher electronegativity of N in comparison to P.
    D
    smaller atomic size of N as compared to that of P.

  • All the noble gases are colourless and tasteless monoatomic gases. In general, noble gases are least reactive and their inertness to chemical reactivity is attributed to the following reasons. Reactive and their inertness to chemical reactivity is attributed to the following reasons. (i)Except helium, all have completely filled ns^(2)np^(6) electronic configuration in their valence shells. (ii)All have high ionisation enthalpy and more positive electron gain enthalpy. However, a number of xenon compounds mainly with most electronegative elements like fluorine and oxygen have been synthesized under different conditions and fluorides of xenon have been used as an oxidising agent and a fluorinating agent in many of the chemical reactions Noble gases have very low melting and boiling points because.

    A
    they have high ionisation enthalpy
    B
    they have more positive electron gain enthalpy
    C
    the type of interatomic interaction is weak metallic bonds.
    D
    the type of interaction is weak dispersion forces.

  • Assertion : P_(4) is more reactive than N_(2) Reason: P-P single bond in P_(4) is much weaker than N-=N triple bond in N_(2)

    A
    Both A and R are true and R is the correct explanation of A
    B
    Both A and R are true but R is false
    C
    A is true but R is false
    D
    A is false but R is true

    • Similar Questions

    Explore conceptually related problems

    Account for the following : (i) NH_(3) has a higherboiling point than PH_(3) (ii) HF is a weaker acid than HI (iii) Of noble gases, only xenon forms real compounds (iv) H_(3)PO_(3) is a diprotic acid.

    Account for the following : (i) NH_(3) is a stronger base than PH_(3) (ii) Sulphur has a greater tendency for catention than oxygen. (iii) Bond dissociation energy of F_(2) is less than that of Cl_(2) . (OR) Explain the following situations : (i) In the structure of HNO_(3) moleucle, the N-O bond (121 pm) is shorter than the N-OH bond (140 pm). (ii) SF_(4) is easily hydrolysed whereas SF_(6) is not easily hydrolysed. (iii) XeF_(2) has a straight linear structure and not a bent angular structure.

    Give reasons for the following observations : (i) Halogens are strong oxidising agents. (ii) Noble gases have very low boiling points. (iii) O and Cl have nearly same electronegativity, yet oxygen forms H bond while Cl doesn't.

    Account for the following statements: (i) Ethene is a covalent compound. (ii) Carbon atoms from a strong bond. (iii) Carbon shows catenation property. (iv) Pentane has higher boiling point than methane. (v) Alkenes have double bonds.

    (a) what happens when (i) Chlorine gas is passed though a hot concentrated solution of NaOH? (ii) sulphure dioxide gas is passed through an aqueses solution of Fe (III) salt? (b) Answer the following : (i) what is the basicity of H_(3) PO_(3) and why?. (ii) why does fluorine not pay the role of a central atom in interhalogen compounds ? (iii) Why do noble gases have very low boiling points ?

    Home
    Profile