11865
When \(NaCl\) is dissolved in water the sodium ion becomes
1 Oxidized
2 Reduced
3 Hydrolysed
4 Hydrated
Explanation:
(d) When sodium chloride is dissolved in water, the sodium ion is hydrated.
Chemical Bonding and Molecular Structure
11866
Solid \(NaCl\) is a bad conductor of electricity since
1 In solid \(NaCl\) there are no ions
2 Solid \(NaCl\) is covalent
3 In solid \(NaCl\) there is no motion of ions
4 In solid \(NaCl\) there are no electrons
Explanation:
A substance can only conduct electricity if it contains charged particles (electrons or ions) that are free to move around. In solid sodium chloride, there are ions but these ions are locked into the ionic lattice and are unable to move. \(NaCl\) (common salt) is solid in state and solid ions or compounds don't conduct electricity. It needs to be either melted, molten or dissolved in a solution (i.e. water) first. Only then will the electrons be free to move to either the Cathode \((-ve)\) or to the Anode \((+ve)\). In a liquid state the electrons are free enough to move. Hence, solid \(NaCl\) is a bad conductor of electricity because its ions cannot move freely.
Chemical Bonding and Molecular Structure
11867
Favourable conditions for electrovalency are
1 Low charge on ions, large cation, small anion
2 High charge on ions, small cation, large anion
3 High charge on ions, large cation, small anion
4 Low charge on ions, small cation, large anion
Explanation:
Electrovalency is calculated for ionic compounds. Greater the size of metal atom, easier is the formation of cation. Smaller the size of the non-metal, easier is the formation of the anion. Lower charge is another favourable factor in the formation of ionic compounds. It is easier to remove smaller number of electrons to form a positively charged cation as a lesser amount of ionization energy has to be supplied. Same is the case for anion formation.
Chemical Bonding and Molecular Structure
11868
The sulphate of a metal has the formula \({M_2}{\left( {S{O_4}} \right)_3}.\) The formula for its phosphate will be
1 \(M{\left( {HP{O_4}} \right)_2}\)
2 \({M_3}{\left( {P{O_4}} \right)_2}\)
3 \({M_2}{\left( {P{O_4}} \right)_3}\)
4 \(MP{O_4}\)
Explanation:
(d) Yet the formula of sulphate of a metal \((M)\) is \({M_2}{(S{O_4})_3}\), it is \({M^{3 + }}\) ion so formula of its phosphate would be \(MP{O_4}\).
11865
When \(NaCl\) is dissolved in water the sodium ion becomes
1 Oxidized
2 Reduced
3 Hydrolysed
4 Hydrated
Explanation:
(d) When sodium chloride is dissolved in water, the sodium ion is hydrated.
Chemical Bonding and Molecular Structure
11866
Solid \(NaCl\) is a bad conductor of electricity since
1 In solid \(NaCl\) there are no ions
2 Solid \(NaCl\) is covalent
3 In solid \(NaCl\) there is no motion of ions
4 In solid \(NaCl\) there are no electrons
Explanation:
A substance can only conduct electricity if it contains charged particles (electrons or ions) that are free to move around. In solid sodium chloride, there are ions but these ions are locked into the ionic lattice and are unable to move. \(NaCl\) (common salt) is solid in state and solid ions or compounds don't conduct electricity. It needs to be either melted, molten or dissolved in a solution (i.e. water) first. Only then will the electrons be free to move to either the Cathode \((-ve)\) or to the Anode \((+ve)\). In a liquid state the electrons are free enough to move. Hence, solid \(NaCl\) is a bad conductor of electricity because its ions cannot move freely.
Chemical Bonding and Molecular Structure
11867
Favourable conditions for electrovalency are
1 Low charge on ions, large cation, small anion
2 High charge on ions, small cation, large anion
3 High charge on ions, large cation, small anion
4 Low charge on ions, small cation, large anion
Explanation:
Electrovalency is calculated for ionic compounds. Greater the size of metal atom, easier is the formation of cation. Smaller the size of the non-metal, easier is the formation of the anion. Lower charge is another favourable factor in the formation of ionic compounds. It is easier to remove smaller number of electrons to form a positively charged cation as a lesser amount of ionization energy has to be supplied. Same is the case for anion formation.
Chemical Bonding and Molecular Structure
11868
The sulphate of a metal has the formula \({M_2}{\left( {S{O_4}} \right)_3}.\) The formula for its phosphate will be
1 \(M{\left( {HP{O_4}} \right)_2}\)
2 \({M_3}{\left( {P{O_4}} \right)_2}\)
3 \({M_2}{\left( {P{O_4}} \right)_3}\)
4 \(MP{O_4}\)
Explanation:
(d) Yet the formula of sulphate of a metal \((M)\) is \({M_2}{(S{O_4})_3}\), it is \({M^{3 + }}\) ion so formula of its phosphate would be \(MP{O_4}\).
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Chemical Bonding and Molecular Structure
11865
When \(NaCl\) is dissolved in water the sodium ion becomes
1 Oxidized
2 Reduced
3 Hydrolysed
4 Hydrated
Explanation:
(d) When sodium chloride is dissolved in water, the sodium ion is hydrated.
Chemical Bonding and Molecular Structure
11866
Solid \(NaCl\) is a bad conductor of electricity since
1 In solid \(NaCl\) there are no ions
2 Solid \(NaCl\) is covalent
3 In solid \(NaCl\) there is no motion of ions
4 In solid \(NaCl\) there are no electrons
Explanation:
A substance can only conduct electricity if it contains charged particles (electrons or ions) that are free to move around. In solid sodium chloride, there are ions but these ions are locked into the ionic lattice and are unable to move. \(NaCl\) (common salt) is solid in state and solid ions or compounds don't conduct electricity. It needs to be either melted, molten or dissolved in a solution (i.e. water) first. Only then will the electrons be free to move to either the Cathode \((-ve)\) or to the Anode \((+ve)\). In a liquid state the electrons are free enough to move. Hence, solid \(NaCl\) is a bad conductor of electricity because its ions cannot move freely.
Chemical Bonding and Molecular Structure
11867
Favourable conditions for electrovalency are
1 Low charge on ions, large cation, small anion
2 High charge on ions, small cation, large anion
3 High charge on ions, large cation, small anion
4 Low charge on ions, small cation, large anion
Explanation:
Electrovalency is calculated for ionic compounds. Greater the size of metal atom, easier is the formation of cation. Smaller the size of the non-metal, easier is the formation of the anion. Lower charge is another favourable factor in the formation of ionic compounds. It is easier to remove smaller number of electrons to form a positively charged cation as a lesser amount of ionization energy has to be supplied. Same is the case for anion formation.
Chemical Bonding and Molecular Structure
11868
The sulphate of a metal has the formula \({M_2}{\left( {S{O_4}} \right)_3}.\) The formula for its phosphate will be
1 \(M{\left( {HP{O_4}} \right)_2}\)
2 \({M_3}{\left( {P{O_4}} \right)_2}\)
3 \({M_2}{\left( {P{O_4}} \right)_3}\)
4 \(MP{O_4}\)
Explanation:
(d) Yet the formula of sulphate of a metal \((M)\) is \({M_2}{(S{O_4})_3}\), it is \({M^{3 + }}\) ion so formula of its phosphate would be \(MP{O_4}\).
11865
When \(NaCl\) is dissolved in water the sodium ion becomes
1 Oxidized
2 Reduced
3 Hydrolysed
4 Hydrated
Explanation:
(d) When sodium chloride is dissolved in water, the sodium ion is hydrated.
Chemical Bonding and Molecular Structure
11866
Solid \(NaCl\) is a bad conductor of electricity since
1 In solid \(NaCl\) there are no ions
2 Solid \(NaCl\) is covalent
3 In solid \(NaCl\) there is no motion of ions
4 In solid \(NaCl\) there are no electrons
Explanation:
A substance can only conduct electricity if it contains charged particles (electrons or ions) that are free to move around. In solid sodium chloride, there are ions but these ions are locked into the ionic lattice and are unable to move. \(NaCl\) (common salt) is solid in state and solid ions or compounds don't conduct electricity. It needs to be either melted, molten or dissolved in a solution (i.e. water) first. Only then will the electrons be free to move to either the Cathode \((-ve)\) or to the Anode \((+ve)\). In a liquid state the electrons are free enough to move. Hence, solid \(NaCl\) is a bad conductor of electricity because its ions cannot move freely.
Chemical Bonding and Molecular Structure
11867
Favourable conditions for electrovalency are
1 Low charge on ions, large cation, small anion
2 High charge on ions, small cation, large anion
3 High charge on ions, large cation, small anion
4 Low charge on ions, small cation, large anion
Explanation:
Electrovalency is calculated for ionic compounds. Greater the size of metal atom, easier is the formation of cation. Smaller the size of the non-metal, easier is the formation of the anion. Lower charge is another favourable factor in the formation of ionic compounds. It is easier to remove smaller number of electrons to form a positively charged cation as a lesser amount of ionization energy has to be supplied. Same is the case for anion formation.
Chemical Bonding and Molecular Structure
11868
The sulphate of a metal has the formula \({M_2}{\left( {S{O_4}} \right)_3}.\) The formula for its phosphate will be
1 \(M{\left( {HP{O_4}} \right)_2}\)
2 \({M_3}{\left( {P{O_4}} \right)_2}\)
3 \({M_2}{\left( {P{O_4}} \right)_3}\)
4 \(MP{O_4}\)
Explanation:
(d) Yet the formula of sulphate of a metal \((M)\) is \({M_2}{(S{O_4})_3}\), it is \({M^{3 + }}\) ion so formula of its phosphate would be \(MP{O_4}\).