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Q. No.Among the following compounds, how many contain two lone pairs on the central atom?
XeF4, H2O, SF4, CF4
1. 4
2. 1
3. 2
4. 0
Subtopic: V.S.E.P.R & V.B.T |
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Subtopic: Octate, Isoelectronic Species, Lewis Structure & Formal Charge |
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How many molecules among the following exhibit a non-zero dipole moment?
\(BeF_2 , BF_3 , H_2O , NH_3 , HCl , CCl_4 \)
1. 4
2. 6
3. 0
4. 3
\(BeF_2 , BF_3 , H_2O , NH_3 , HCl , CCl_4 \)
1. 4
2. 6
3. 0
4. 3
Subtopic: Polarity |
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Species among the following that experience an increase in bond strength upon the removal of an electron are:
(a) B2
(b) NO
(c) N2
(d) O2
(e) C2
1. b,d
2. a,b,d
3. b,e
4. b,c
(a) B2
(b) NO
(c) N2
(d) O2
(e) C2
1. b,d
2. a,b,d
3. b,e
4. b,c
Subtopic: M.O.T |
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The pair of ions that is isoelectronic with \(\text{Al}^{3+}\) ion is:
1. \(\mathrm{Mg}^{2+}, \mathrm{O}^{2-} \)
2. \(\mathrm{Na}^{+}, \mathrm{N}^{2-} \)
3. \(\mathrm{C}^{4-}, \mathrm{Cl}^{-} \)
4. \(\mathrm{F}^{-}, \mathrm{Mg}^{+} \)
1. \(\mathrm{Mg}^{2+}, \mathrm{O}^{2-} \)
2. \(\mathrm{Na}^{+}, \mathrm{N}^{2-} \)
3. \(\mathrm{C}^{4-}, \mathrm{Cl}^{-} \)
4. \(\mathrm{F}^{-}, \mathrm{Mg}^{+} \)
Subtopic: Octate, Isoelectronic Species, Lewis Structure & Formal Charge |
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Identify the correct statement regarding SF4:
| 1. | It has one lone pair at the equatorial position with two lone pair-bond pair repulsion at 90°. |
| 2. | It has one lone pair at the axial position with two lone pair-bond pair repulsion at 90°. |
| 3. | It has one lone pair at the equatorial position with three lone pair-bond pair repulsion at 90°. |
| 4. | It has one lone pair at the axial position with three lone pair-bond pair repulsion at 90°. |
Subtopic: Hybridisation |
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Match the compounds given in Column-I with their respective hybridisation which is given in Column-II.
Correct matching is:
| Column-I (Compound) | Column-II Hybridisation | ||
| (i) | \(PCl_5 \) | (a) | \(sp^3d^2 \) |
| (ii) | \([Pt(CN)_4]^{-2} \) | (b) | \(sp^3d \) |
| (iii) | \([Co(NH_3)_6]^{3+} \) | (c) | \(d^2sp^3 \) |
| (iv) | \(BrF_5 \) | (d) | \(dsp^2 \) |
| I | II | III | IV | |
| 1. | b | d | c | a |
| 2. | a | b | c | d |
| 3. | b | d | a | c |
| 4. | d | b | a | c |
Subtopic: Hybridisation | V.S.E.P.R & V.B.T |
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Identify the correct increasing strength of intermolecular H-bonding.
1. \(\mathrm{HCN}<\mathrm{H}_2 \mathrm{O}<\mathrm{NH}_3\)
2. \(\mathrm{HCN}<\mathrm{CH}_4<\mathrm{NH}_3\)
3. \(\mathrm{CH}_4<\mathrm{HCN}<\mathrm{NH}_3\)
4. \(\mathrm{CH}_4<\mathrm{NH}_3<\mathrm{HCN}\)
1. \(\mathrm{HCN}<\mathrm{H}_2 \mathrm{O}<\mathrm{NH}_3\)
2. \(\mathrm{HCN}<\mathrm{CH}_4<\mathrm{NH}_3\)
3. \(\mathrm{CH}_4<\mathrm{HCN}<\mathrm{NH}_3\)
4. \(\mathrm{CH}_4<\mathrm{NH}_3<\mathrm{HCN}\)
Subtopic: van der Waal Force & Hydrogen Bonding |
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Which of the following statement is incorrect regarding PCl5?
1. In PCl5, axial bonds are longer than equatorial bonds.
2. It has a trigonal bipyramidal structure.
3. 3 chlorine atoms are in the same plane.
4. Hybridisation of 'P' is sp3d2.
1. In PCl5, axial bonds are longer than equatorial bonds.
2. It has a trigonal bipyramidal structure.
3. 3 chlorine atoms are in the same plane.
4. Hybridisation of 'P' is sp3d2.
Subtopic: Hybridisation |
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Match the molecules in Column-I with their corresponding molecular shapes in Column-II.
Choose the correct matching sequence:
| Column-I (Molecule) |
Column-II (Shape) |
||
| (i) | BF3 | (a) | T-shape |
| (ii) | SF4 | (b) | Square planar |
| (iii) | XeF4 | (c) | See-saw |
| (iv) | ClF3 | (d) | Trigonal planar |
| (i) | (ii) | (iii) | (iv) | |
| 1. | d | c | b | a |
| 2. | a | b | c | d |
| 3. | d | a | c | d |
| 4. | b | c | d | a |
Subtopic: V.S.E.P.R & V.B.T |
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