Due to \({\text{ + I}}\) effect, an electron-releasing group increases electron density on oxygen tending to decrease the polarity of \(\mathrm{O}-\mathrm{H}\) bond. This decreases the hydrogen bond strength.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313628
The typical range of molar enthalpies for the strongest intermolecular (hydrogen) bond is
1 \(200-300 \mathrm{~kJ}\)
2 \(300-500 \mathrm{~kJ}\)
3 \(4-25 \mathrm{~kJ}\)
4 \(4-25 \mathrm{~J}\)
Explanation:
The typical range of molar enthalpies for the strongest intermolecular (hydrogen) bond is\(4-25 \mathrm{~kJ}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313629
The types of bonds present in \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.5}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\) are
1 Electrovalent, covalent and H bonds.
2 Electrovalent and coordinate bonds.
3 Electrovalent, covalent, coordinate covalent and H bonds.
4 Covalent and coordinate covalent bonds.
Explanation:
\({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.5}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\) is represented as \(\left[ {{\rm{Cu}}{{\left( {{{\rm{H}}_{\rm{2}}}{\rm{O}}} \right)}_{\rm{4}}}} \right]{\rm{S}}{{\rm{O}}_{\rm{4}}}{\rm{.}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\)
Due to \({\text{ + I}}\) effect, an electron-releasing group increases electron density on oxygen tending to decrease the polarity of \(\mathrm{O}-\mathrm{H}\) bond. This decreases the hydrogen bond strength.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313628
The typical range of molar enthalpies for the strongest intermolecular (hydrogen) bond is
1 \(200-300 \mathrm{~kJ}\)
2 \(300-500 \mathrm{~kJ}\)
3 \(4-25 \mathrm{~kJ}\)
4 \(4-25 \mathrm{~J}\)
Explanation:
The typical range of molar enthalpies for the strongest intermolecular (hydrogen) bond is\(4-25 \mathrm{~kJ}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313629
The types of bonds present in \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.5}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\) are
1 Electrovalent, covalent and H bonds.
2 Electrovalent and coordinate bonds.
3 Electrovalent, covalent, coordinate covalent and H bonds.
4 Covalent and coordinate covalent bonds.
Explanation:
\({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.5}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\) is represented as \(\left[ {{\rm{Cu}}{{\left( {{{\rm{H}}_{\rm{2}}}{\rm{O}}} \right)}_{\rm{4}}}} \right]{\rm{S}}{{\rm{O}}_{\rm{4}}}{\rm{.}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\)
Due to \({\text{ + I}}\) effect, an electron-releasing group increases electron density on oxygen tending to decrease the polarity of \(\mathrm{O}-\mathrm{H}\) bond. This decreases the hydrogen bond strength.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313628
The typical range of molar enthalpies for the strongest intermolecular (hydrogen) bond is
1 \(200-300 \mathrm{~kJ}\)
2 \(300-500 \mathrm{~kJ}\)
3 \(4-25 \mathrm{~kJ}\)
4 \(4-25 \mathrm{~J}\)
Explanation:
The typical range of molar enthalpies for the strongest intermolecular (hydrogen) bond is\(4-25 \mathrm{~kJ}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313629
The types of bonds present in \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.5}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\) are
1 Electrovalent, covalent and H bonds.
2 Electrovalent and coordinate bonds.
3 Electrovalent, covalent, coordinate covalent and H bonds.
4 Covalent and coordinate covalent bonds.
Explanation:
\({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.5}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\) is represented as \(\left[ {{\rm{Cu}}{{\left( {{{\rm{H}}_{\rm{2}}}{\rm{O}}} \right)}_{\rm{4}}}} \right]{\rm{S}}{{\rm{O}}_{\rm{4}}}{\rm{.}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\)
Due to \({\text{ + I}}\) effect, an electron-releasing group increases electron density on oxygen tending to decrease the polarity of \(\mathrm{O}-\mathrm{H}\) bond. This decreases the hydrogen bond strength.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313628
The typical range of molar enthalpies for the strongest intermolecular (hydrogen) bond is
1 \(200-300 \mathrm{~kJ}\)
2 \(300-500 \mathrm{~kJ}\)
3 \(4-25 \mathrm{~kJ}\)
4 \(4-25 \mathrm{~J}\)
Explanation:
The typical range of molar enthalpies for the strongest intermolecular (hydrogen) bond is\(4-25 \mathrm{~kJ}\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313629
The types of bonds present in \({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.5}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\) are
1 Electrovalent, covalent and H bonds.
2 Electrovalent and coordinate bonds.
3 Electrovalent, covalent, coordinate covalent and H bonds.
4 Covalent and coordinate covalent bonds.
Explanation:
\({\rm{CuS}}{{\rm{O}}_{\rm{4}}}{\rm{.5}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\) is represented as \(\left[ {{\rm{Cu}}{{\left( {{{\rm{H}}_{\rm{2}}}{\rm{O}}} \right)}_{\rm{4}}}} \right]{\rm{S}}{{\rm{O}}_{\rm{4}}}{\rm{.}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\)