313989
\({\rm{C}}{{\rm{O}}_{\rm{2}}}\) is not iso-structural with
1 \({\rm{HgC}}{{\rm{l}}_{\rm{2}}}\)
2 \({\rm{SnC}}{{\rm{l}}_{\rm{2}}}\)
3 \({{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{2}}}\)
4 \({\rm{BeC}}{{\rm{l}}_{\rm{2}}}\)
Explanation:
\({\rm{SnC}}{{\rm{l}}_{\rm{2}}}\) has angular shape
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313908
Predict the correct order of repulsion forces among the following
1 lone pair - bond pair > bond pair - bond pair > lone pair - lone pair
2 lone pair - lone pair > lone pair - bond pair > bond pair - bond pair
3 lone pair - lone pair > bond pair - bond pair > lone pair - bond pair
4 bond pair - bond pair > lone pair - bond pair > lone pair - lone pair
Explanation:
The order of repulsion forces according to VSEPR theory: lone pair - lone pair > lone pair - bond pair > bond pair - bond pair.
NEET - 2016
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313909
The geometry of ammonia molecule can be best described as
1 Nitrogen at one vertex of a regular tetrahedron, the other three vertices being occupied by the three hydrogens
2 Nitrogen at the centre of the tetrahedron, three of the vertices being occupied by three hydrogens
3 Nitrogen at the centre of an equilateral triangle, three corners being occupied by three hydrogens
4 Nitrogen at the junction of a T, three open ends being occupied by three hydrogens
Explanation:
In \(\mathop {\text{N}}\limits^{ \cdot \,\, \cdot } {{\text{H}}_3}\), central atom nitrogen is \(\mathrm{sp}^{3}\) hybridized hence it will be at the centre of tetrahedron with \(\mathrm{H}\)-atoms at three vertices.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313910
Statement A : Lone pair-lone pair repulsive interactions are greater than lone pair-bond pair and bond pair-bond pair interactions. Statement B : The space occupied by lone pair electrons is more as compared to bond pair electrons.
1 Statement A is correct but Statement B is incorrect
2 Statement A is incorrect but Statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
While the lone pairs are localised on the central atom, each bonded pair is shared between two atoms. As a result, the lone pair electrons in a molecule occupy more space as compared to the bonding pairs of electrons. This results in greater repulsion between lone pairs of electrons as compared to the lone pair-bond pair, bond pair and bond pair - repulsions. So, the option (3) is correct.
313989
\({\rm{C}}{{\rm{O}}_{\rm{2}}}\) is not iso-structural with
1 \({\rm{HgC}}{{\rm{l}}_{\rm{2}}}\)
2 \({\rm{SnC}}{{\rm{l}}_{\rm{2}}}\)
3 \({{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{2}}}\)
4 \({\rm{BeC}}{{\rm{l}}_{\rm{2}}}\)
Explanation:
\({\rm{SnC}}{{\rm{l}}_{\rm{2}}}\) has angular shape
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313908
Predict the correct order of repulsion forces among the following
1 lone pair - bond pair > bond pair - bond pair > lone pair - lone pair
2 lone pair - lone pair > lone pair - bond pair > bond pair - bond pair
3 lone pair - lone pair > bond pair - bond pair > lone pair - bond pair
4 bond pair - bond pair > lone pair - bond pair > lone pair - lone pair
Explanation:
The order of repulsion forces according to VSEPR theory: lone pair - lone pair > lone pair - bond pair > bond pair - bond pair.
NEET - 2016
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313909
The geometry of ammonia molecule can be best described as
1 Nitrogen at one vertex of a regular tetrahedron, the other three vertices being occupied by the three hydrogens
2 Nitrogen at the centre of the tetrahedron, three of the vertices being occupied by three hydrogens
3 Nitrogen at the centre of an equilateral triangle, three corners being occupied by three hydrogens
4 Nitrogen at the junction of a T, three open ends being occupied by three hydrogens
Explanation:
In \(\mathop {\text{N}}\limits^{ \cdot \,\, \cdot } {{\text{H}}_3}\), central atom nitrogen is \(\mathrm{sp}^{3}\) hybridized hence it will be at the centre of tetrahedron with \(\mathrm{H}\)-atoms at three vertices.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313910
Statement A : Lone pair-lone pair repulsive interactions are greater than lone pair-bond pair and bond pair-bond pair interactions. Statement B : The space occupied by lone pair electrons is more as compared to bond pair electrons.
1 Statement A is correct but Statement B is incorrect
2 Statement A is incorrect but Statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
While the lone pairs are localised on the central atom, each bonded pair is shared between two atoms. As a result, the lone pair electrons in a molecule occupy more space as compared to the bonding pairs of electrons. This results in greater repulsion between lone pairs of electrons as compared to the lone pair-bond pair, bond pair and bond pair - repulsions. So, the option (3) is correct.
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313989
\({\rm{C}}{{\rm{O}}_{\rm{2}}}\) is not iso-structural with
1 \({\rm{HgC}}{{\rm{l}}_{\rm{2}}}\)
2 \({\rm{SnC}}{{\rm{l}}_{\rm{2}}}\)
3 \({{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{2}}}\)
4 \({\rm{BeC}}{{\rm{l}}_{\rm{2}}}\)
Explanation:
\({\rm{SnC}}{{\rm{l}}_{\rm{2}}}\) has angular shape
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313908
Predict the correct order of repulsion forces among the following
1 lone pair - bond pair > bond pair - bond pair > lone pair - lone pair
2 lone pair - lone pair > lone pair - bond pair > bond pair - bond pair
3 lone pair - lone pair > bond pair - bond pair > lone pair - bond pair
4 bond pair - bond pair > lone pair - bond pair > lone pair - lone pair
Explanation:
The order of repulsion forces according to VSEPR theory: lone pair - lone pair > lone pair - bond pair > bond pair - bond pair.
NEET - 2016
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313909
The geometry of ammonia molecule can be best described as
1 Nitrogen at one vertex of a regular tetrahedron, the other three vertices being occupied by the three hydrogens
2 Nitrogen at the centre of the tetrahedron, three of the vertices being occupied by three hydrogens
3 Nitrogen at the centre of an equilateral triangle, three corners being occupied by three hydrogens
4 Nitrogen at the junction of a T, three open ends being occupied by three hydrogens
Explanation:
In \(\mathop {\text{N}}\limits^{ \cdot \,\, \cdot } {{\text{H}}_3}\), central atom nitrogen is \(\mathrm{sp}^{3}\) hybridized hence it will be at the centre of tetrahedron with \(\mathrm{H}\)-atoms at three vertices.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313910
Statement A : Lone pair-lone pair repulsive interactions are greater than lone pair-bond pair and bond pair-bond pair interactions. Statement B : The space occupied by lone pair electrons is more as compared to bond pair electrons.
1 Statement A is correct but Statement B is incorrect
2 Statement A is incorrect but Statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
While the lone pairs are localised on the central atom, each bonded pair is shared between two atoms. As a result, the lone pair electrons in a molecule occupy more space as compared to the bonding pairs of electrons. This results in greater repulsion between lone pairs of electrons as compared to the lone pair-bond pair, bond pair and bond pair - repulsions. So, the option (3) is correct.
313989
\({\rm{C}}{{\rm{O}}_{\rm{2}}}\) is not iso-structural with
1 \({\rm{HgC}}{{\rm{l}}_{\rm{2}}}\)
2 \({\rm{SnC}}{{\rm{l}}_{\rm{2}}}\)
3 \({{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{2}}}\)
4 \({\rm{BeC}}{{\rm{l}}_{\rm{2}}}\)
Explanation:
\({\rm{SnC}}{{\rm{l}}_{\rm{2}}}\) has angular shape
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313908
Predict the correct order of repulsion forces among the following
1 lone pair - bond pair > bond pair - bond pair > lone pair - lone pair
2 lone pair - lone pair > lone pair - bond pair > bond pair - bond pair
3 lone pair - lone pair > bond pair - bond pair > lone pair - bond pair
4 bond pair - bond pair > lone pair - bond pair > lone pair - lone pair
Explanation:
The order of repulsion forces according to VSEPR theory: lone pair - lone pair > lone pair - bond pair > bond pair - bond pair.
NEET - 2016
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313909
The geometry of ammonia molecule can be best described as
1 Nitrogen at one vertex of a regular tetrahedron, the other three vertices being occupied by the three hydrogens
2 Nitrogen at the centre of the tetrahedron, three of the vertices being occupied by three hydrogens
3 Nitrogen at the centre of an equilateral triangle, three corners being occupied by three hydrogens
4 Nitrogen at the junction of a T, three open ends being occupied by three hydrogens
Explanation:
In \(\mathop {\text{N}}\limits^{ \cdot \,\, \cdot } {{\text{H}}_3}\), central atom nitrogen is \(\mathrm{sp}^{3}\) hybridized hence it will be at the centre of tetrahedron with \(\mathrm{H}\)-atoms at three vertices.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313910
Statement A : Lone pair-lone pair repulsive interactions are greater than lone pair-bond pair and bond pair-bond pair interactions. Statement B : The space occupied by lone pair electrons is more as compared to bond pair electrons.
1 Statement A is correct but Statement B is incorrect
2 Statement A is incorrect but Statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
While the lone pairs are localised on the central atom, each bonded pair is shared between two atoms. As a result, the lone pair electrons in a molecule occupy more space as compared to the bonding pairs of electrons. This results in greater repulsion between lone pairs of electrons as compared to the lone pair-bond pair, bond pair and bond pair - repulsions. So, the option (3) is correct.