`PF_5`
`SF_6`
`H_2SO_4`
All of the above
increase in energy
decrease in energy
neither decrease nor increase in energy
the repulsive forces overcoming the attractive forces
` BCl_3`
`BeH_2`
`LiCH_3`
All of the above
`:O : C : C : : O :`
`:O : C : : C : O :`
`: O :: C :: C :: C ::O :`
`: O : : C C :: O :`
`HF`
`H_2O`
`BF_3`
`NH_3`
`3p^6`
`3p^6, 4s^2`
`3p^6 , 3d^2`
`3d^2, 4s^2`
`CO_2`
`HI`
`H_2O`
`SO_2`
`C Cl_4`
`O_2`
`NF_3`
All of the above
`A_2B`
`AB_2`
`A_2B_3`
`A_3B_2`
`2`
`3`
`4`
`5`
`MCO_3`
`MHCO_3`
`M(HCO_3)_2`
`M(CO_3)_2`
`3p^6`
`3p^6, 4s^2`
`3p^6 , 3d^2`
`3d^2, 4s^2`
`1`
`2`
`3`
`4`
`XY_2`
`X_5Y_2`
`X_2Y_5`
`XY_5`
`XY`
`X_2 Y`
`X_2 Y_3`
`XY_3`
Column I | Column II | ||
---|---|---|---|
(A) | K | (P) | two |
(B) | Zn | (Q) | one |
(C) | Al | (R) | four |
(D) | C | (S) | three |
2 1 4 3
2 3 1 4
3 1 4 2
3 4 1 2
`A_6 B_6`
`A_2 B_3`
`A_3 B_2`
`A_2B`
with identical spins
unequally shared between the two
transferred fully from one atom to another
equally shared between them
` H _{ 3 } O ^{ + }`
`BF _{ 4 }^{ - }`
` HF _{ 2 }^{ - }`
`NH _{ 4 }^{ + }`
high melting point
presence of ions
strong electrostatic force between lens
non-directional nature of electrovalent bond
ionic
covalent
coordinate
metallic
`CH_4`
`KCN`
`H_2`
`KCl`
`C Cl_4`
`AlCl_3`
`CaCl_2`
`NCl_3`
`PbO_2`
`SiO_2`
`NaCl_2`
`AlCl_3`
Covalent
Dative
Ionicbond
Vanderwallsforces
`NH_4Cl`
`HCN`
`H_2O_2`
`CH_4`
`BF_3`
`CuCl_2`
`CuSO_4 · 5H_2O`
`FeCl_3 · H_2O`
`(i),(ii)` and `(iii) `
`(i),(ii)` and `(iv)`
`(ii),(iii) ` and `(iv)`
`(i),(iii) ` and `(iv)`
`PCl_3`
`SF_4`
`NO`
`POCl_3`
Column I | Column II | ||
---|---|---|---|
(A) | Ionic cornpound | (P) | `NH_4Cl` |
(B) | Polar covalent | (Q) | `O_2` |
(C) | Non-polor covalent molecule | (R) | `HCl` |
(D) | Dative bond | (S) | `KCl` |
4 3 2 1
1 3 2 4
4 1 2 3
1 2 4 3
I, II and III
II, III and IV
I, III and IV
All of these
I and II
II and III
I and III
All of these
Assertion : Purely covalent compounds cannot conduct electricity in their aqueous solution or in molten state.
Reason : Purely covalent compounds have lower melting and boiling points.
an ionic bond
a hydrogen bond
a covalent bond
a coordinate bond
exothermic
endothermic
Both (a) and (b)
None of these
water is an amphiprotic solvent
water is high boiling liquid
the process is accompained by positive heat of solution
water decreases the interionic attraction in the crystal lattice due to solvation
`CH_4`
`H_2O_2`
`NH_4Cl`
None of these
`Al_2Cl_6`
`Al_2O_3`
`AlF_3`
All of these
`CH_4`
`NaCl`
`SO_2`
`KOH`
covelent and co-ordinate
electrovalent and co-ordinate
electrovalent and covalent
electrovalent , covalent and co-ordinate
covalent and electrovalent bonds
covalent and coordinate covalent bonds
electrovalent, covalent and dative bonds
electrovalent bond and dative bonds
`CS_2`
`C_2H_5OH`
`C Cl_4`
`CHCl_3`
Assertion : Fluorine exhibits the same oxidation state in all its compounds.
Reason : Fluorine atom has no d-orbital in its valence shell.
I and II
II and III
I and III
All of these
Assertion : Water `(H_2O)` is more polar than hydrogen sulphide `(B_2S)`.
Reason : Oxygen is more electronegative than sulphur.
`CO_2`
`HI`
`H_2O`
`SO_2`
Water is a non-polar molecule in normal conditons
Water is a polar molecule in normal conditions
Water exist in tile form of `H^(+) OH^-` in normal conditions
All of the above are correct
`HF` molecule associate due to hydrogen bonding
`F_2`, is highly reactive
`HF` is the weakest acids of all hydrogen halides
fluorine atoms is the smallest of all halides
`CHCl_3`
`CH_4`
`C Cl_4`
`CO_2`
`CO_2`
`CHCl_3`
`C Cl_4`
`CH_2Cl_2`
`NH_3`
`CHCl_3`
`H_2O`
`C Cl_4`