NEW
Font size
Worksheetsp block
Total questions: 30
Worksheet time: 36mins
Which of the following elements can be involved in pπ–dπ bonding?
Carbon
Nitrogen
Boran
Phosphorous
Which of the following pairs of ions are isoelectronic and isostructural?
CO32–, NO3–
ClO3– , CO32–
SO32–, NO3–
ClO3– , SO32–
Bond dissociation enthalpy of E—H (E = element) bonds is given below. Which of the compounds will act as strongest reducing agent?
Compound NH3 PH3 AsH3 SbH3
Δdiss (E—H)/kJ mol–1 389 322 297 255
NH3
PH3
AsH3
SbH3
Which of the following acids forms three series of salts?
H3PO2
H3BO3
H3PO4
H3PO3
Strong reducing behaviour of H3PO2 is due to
Low oxidation state of phosphorus
Presence of two –OH groups and one P–H bond
Presence of one –OH group and two P–H bonds
High electron gain enthalpy of phosphorus
On heating lead nitrate forms oxides of nitrogen and lead. The oxides formed are ______.
N2O, PbO
NO2, PbO
NO, PbO
NO, PbO2
Which of the following elements does not show allotropy?
Nitrogen
Bismuth
Antimony
Arsenic
Maximum covalency of nitrogen is ______________.
3
4
5
6
Which of the following statements is wrong?
Single N–N bond is stronger than the single P–P bond.
PH3 can act as a ligand in the formation of coordination compound with transition elements.
NO2 is paramagnetic in nature.
Covalency of nitrogen in N2O5 is four
A brown ring is formed in the ring test for NO3– ion. It is due to the formation of
[Fe(H2O)5 (NO)]2+
FeSO4.NO2
[Fe(H2O)4(NO)2]2+
FeSO4.HNO3
Elements of group-15 form compounds in +5 oxidation state. However, bismuth forms only one well characterised compound in +5 oxidation state. The compound is
(i) Bi2O5
(ii) BiF5
(iii) BiCl5
Bi2S5
The oxidation state of central atom in the anion of compound NaH2PO2 will
be ______.
+3
+5
+1
–3
Which of the following is not tetrahedral in shape?
NH4+
SiCl4
SF4
SO42–
Which of the following are peroxoacids of sulphur?
H2SO5 and H2S2O8
H2SO5 and H2S2O7
H2SO5 and H2S2O8
H2S2O6 and H2S2O7
In solid state PCl5 is a _________.
covalent solid
octahedral structure
ionic solid with [PCl6]+ octahedral and [PCl4]– tetrahedra
ionic solid with [PCl4]+ tetrahedral and [PCl6]– octahedra
Which of the following statements are correct for SO2 gas?
It’s have one sigma σ. and two Pπ -dπ
It’s molecule has linear geometry.
It’s have one sigma σ. and one Pπ -dπ
It can be prepared by the reaction of dilute H2SO4 with metal sulphide.
Which of the following statements are correct?
All the three N—O bond lengths in HNO3 are equal.
All P—Cl bond lengths in PCl5 molecule in gaseous state are equal.
P4 molecule in white phohsphorus have angular strain therefore white phosphorus is very reactive.
In case of PCl5 two P—Cl bond shorter then three P—Cl bond
Which of the following orders are correct as per the properties mentioned against each?
(i) N2O4< N2O3 < NO < N2O (Acid strength)
(ii) AsH3 < PH3 < NH3 (Enthalpy of vapourisation)
(iii) S < O < Cl < F (More negative electron gain enthalpy)
(iv) H2O > H2S > H2Se > H2Te ( Thermal stability)
Which of the following statements are correct?
S–S bond is present in H2S2O6.
In peroxosulphuric acid (H2SO5) sulphur is in +8 oxidation state.
Sulphur exist in S2 in nature like O2
Change in enthalpy is positive for the preparation of SO3 by catalytic oxidation of SO2.
SF6 is known but SCl6 is not________
Due to small size of fluorine six F – ion can be accomodated around sulphur whereas chloride ion is comparatively larger in size, therefore, there will be interionic repulsion
Due to absence of vacant d orbital
Chlorine have more electron gain enthalpy than
none of these
PH3 exist but PH5 does not exist?
becouse phosphorous have large size
becouse hydrogen have small size and less electronegativity hence can't promote electron 3p to 3d orbital
both are correct
none of these
Match the correct option
Column I Column II
(A) Pb3O4 (1) Neutral oxide
(B) N2O (2) Acidic oxide
(C) Mn2O7 (3) Basic oxide
(D) Bi2O3 (4) Mixed oxide
A (1) B (2) C (3) D (4)
A (4) B (1) C (2) D (3)
A (3) B (2) C (4) D (1)
A (4) B (3) C (1) D (2)
Match the following
(A) H2SO4 (1) Highest electron gain enthalpy
(B) CCl3NO2 (2) Chalcogen
(C) Cl2 (3) Tear gas
(D) Sulphur (4) Storage batteries
A (4) B (3) C (1) D (2)
A (3) B (4) C (1) D (2)
A (4) B (1) C (2) D (3)
A (2) B (1) C (3) D (4)
Assertion : N2 is less reactive than P4.
Reason : Nitrogen has more electron gain enthalpy than phosphorus
Both assertion and reason are correct statements, and reason is the correct explanation of the assertion.
Both assertion and reason are correct statements, but reason is not the correct explanation of the assertion.
Assertion is correct, but reason is wrong statement.
Assertion is wrong but reason is correct statement.
Both assertion and reason are wrong statement
Assertion : Both rhombic and monoclinic sulphur exist as S8 but oxygen exists as O2.
Reason : Oxygen forms pπ – pπ multiple bond due to small size and small bond length but pπ – pπ bonding is not possible in sulphur
Both assertion and reason are correct statements, and reason is the correct explanation of the assertion.
Both assertion and reason are correct statements, but reason is not the correct explanation of the assertion.
Assertion is correct, but reason is wrong statement.
Assertion is wrong but reason is correct statement.
Both assertion and reason are wrong statement
Bond angle in PH4+ is higher than that in PH3
becouse PH4+ sp3d and trigonal bi pyramidal
becouse PH4+ sp3 tetrahedral
becouse PH4+ sp2 trigonal planner
none of these
Among the following hydride which have more basic
NH3, PH3, AsH3, SbH3, BiH3
BiH3
SbH3
AsH3
PH3
NH3
Three P–OH groups are present in the molecule of H3PO4. Therefore, its basicity is three
2
3
4
1
Why does R3P = O exist but R3N = O does not (R = alkyl group)
Nitrogen have vacant orbital
Nitrogen have absence vacant orbital
Nitrogen is small size
P is small size
Which of the following options are not in accordance with the property
mentioned against them?
(i) F2 > Cl2 > Br2 > I2 Oxidising power.
(ii) MI < MBr < MCl < MF Ionic character of metal halide.
(iii) F2 > Cl2 > Br2 > I2 Bond dissociation enthalpy.
(iv) HI < HBr < HCl < HF Bond dissociation enthalpy.
