316589
Which one of the following halogens has the highest bond dissociation energy?
1 \(\mathrm{F}_{2}\)
2 \(\mathrm{Cl}_{2}\)
3 \(\mathrm{Br}_{2}\)
4 \(\mathrm{I}_{2}\)
Explanation:
As the size of atom increases, bond length increases, thus bond dissociation energy decreases. However, the dissociation energy of fluorine is lesser than that of chlorine because of its small size. {Hence, \(\mathrm{Cl}_{2}\) has the highest bond dissociation energy.}
CHXI11:THE P-BLOCK ELEMENTS
316590
The electron gain enthalpy (in \(\mathrm{kJ} / \mathrm{mol}\) ) of fluorine, chlorine, bromine and iodine, respectively, are :
Chlorine has higher electron gain enthalpy than fluorine (exception). Order of electron gain enthalpy of halogens is \({\rm{Cl > F > Br > I}}{\rm{.}}\)
JEE - 2020
CHXI11:THE P-BLOCK ELEMENTS
316591
Halogens have maximum negative electron gain enthalpy in the respective periods of the periodic table. Why?
1 \({{\rm{Z}}_{{\rm{eff }}}}\) is high and require one electron for octet
2 Due to large size
3 Energy of halogen increases by accepting electron
4 They are non metals
Explanation:
Halogens have the smallest size in their respective periods and therefore high effective nuclear charge. As a consequence, they readily accept one electron to acquire noble gas electronic configuration.
CHXI11:THE P-BLOCK ELEMENTS
316592
Among the following, the one that is relatively most electropositive is
1 \(\mathrm{F}\)
2 \(\mathrm{Cl}\)
3 \(\mathrm{Br}\)
4 \({\rm{I}}\)
Explanation:
On moving down the group \({\rm{F}}\,\,{\rm{to}}\,\,{\rm{I}}\) electronegativity decreases and electropositive nature increases.
NEET Test Series from KOTA - 10 Papers In MS WORD
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CHXI11:THE P-BLOCK ELEMENTS
316589
Which one of the following halogens has the highest bond dissociation energy?
1 \(\mathrm{F}_{2}\)
2 \(\mathrm{Cl}_{2}\)
3 \(\mathrm{Br}_{2}\)
4 \(\mathrm{I}_{2}\)
Explanation:
As the size of atom increases, bond length increases, thus bond dissociation energy decreases. However, the dissociation energy of fluorine is lesser than that of chlorine because of its small size. {Hence, \(\mathrm{Cl}_{2}\) has the highest bond dissociation energy.}
CHXI11:THE P-BLOCK ELEMENTS
316590
The electron gain enthalpy (in \(\mathrm{kJ} / \mathrm{mol}\) ) of fluorine, chlorine, bromine and iodine, respectively, are :
Chlorine has higher electron gain enthalpy than fluorine (exception). Order of electron gain enthalpy of halogens is \({\rm{Cl > F > Br > I}}{\rm{.}}\)
JEE - 2020
CHXI11:THE P-BLOCK ELEMENTS
316591
Halogens have maximum negative electron gain enthalpy in the respective periods of the periodic table. Why?
1 \({{\rm{Z}}_{{\rm{eff }}}}\) is high and require one electron for octet
2 Due to large size
3 Energy of halogen increases by accepting electron
4 They are non metals
Explanation:
Halogens have the smallest size in their respective periods and therefore high effective nuclear charge. As a consequence, they readily accept one electron to acquire noble gas electronic configuration.
CHXI11:THE P-BLOCK ELEMENTS
316592
Among the following, the one that is relatively most electropositive is
1 \(\mathrm{F}\)
2 \(\mathrm{Cl}\)
3 \(\mathrm{Br}\)
4 \({\rm{I}}\)
Explanation:
On moving down the group \({\rm{F}}\,\,{\rm{to}}\,\,{\rm{I}}\) electronegativity decreases and electropositive nature increases.
316589
Which one of the following halogens has the highest bond dissociation energy?
1 \(\mathrm{F}_{2}\)
2 \(\mathrm{Cl}_{2}\)
3 \(\mathrm{Br}_{2}\)
4 \(\mathrm{I}_{2}\)
Explanation:
As the size of atom increases, bond length increases, thus bond dissociation energy decreases. However, the dissociation energy of fluorine is lesser than that of chlorine because of its small size. {Hence, \(\mathrm{Cl}_{2}\) has the highest bond dissociation energy.}
CHXI11:THE P-BLOCK ELEMENTS
316590
The electron gain enthalpy (in \(\mathrm{kJ} / \mathrm{mol}\) ) of fluorine, chlorine, bromine and iodine, respectively, are :
Chlorine has higher electron gain enthalpy than fluorine (exception). Order of electron gain enthalpy of halogens is \({\rm{Cl > F > Br > I}}{\rm{.}}\)
JEE - 2020
CHXI11:THE P-BLOCK ELEMENTS
316591
Halogens have maximum negative electron gain enthalpy in the respective periods of the periodic table. Why?
1 \({{\rm{Z}}_{{\rm{eff }}}}\) is high and require one electron for octet
2 Due to large size
3 Energy of halogen increases by accepting electron
4 They are non metals
Explanation:
Halogens have the smallest size in their respective periods and therefore high effective nuclear charge. As a consequence, they readily accept one electron to acquire noble gas electronic configuration.
CHXI11:THE P-BLOCK ELEMENTS
316592
Among the following, the one that is relatively most electropositive is
1 \(\mathrm{F}\)
2 \(\mathrm{Cl}\)
3 \(\mathrm{Br}\)
4 \({\rm{I}}\)
Explanation:
On moving down the group \({\rm{F}}\,\,{\rm{to}}\,\,{\rm{I}}\) electronegativity decreases and electropositive nature increases.
316589
Which one of the following halogens has the highest bond dissociation energy?
1 \(\mathrm{F}_{2}\)
2 \(\mathrm{Cl}_{2}\)
3 \(\mathrm{Br}_{2}\)
4 \(\mathrm{I}_{2}\)
Explanation:
As the size of atom increases, bond length increases, thus bond dissociation energy decreases. However, the dissociation energy of fluorine is lesser than that of chlorine because of its small size. {Hence, \(\mathrm{Cl}_{2}\) has the highest bond dissociation energy.}
CHXI11:THE P-BLOCK ELEMENTS
316590
The electron gain enthalpy (in \(\mathrm{kJ} / \mathrm{mol}\) ) of fluorine, chlorine, bromine and iodine, respectively, are :
Chlorine has higher electron gain enthalpy than fluorine (exception). Order of electron gain enthalpy of halogens is \({\rm{Cl > F > Br > I}}{\rm{.}}\)
JEE - 2020
CHXI11:THE P-BLOCK ELEMENTS
316591
Halogens have maximum negative electron gain enthalpy in the respective periods of the periodic table. Why?
1 \({{\rm{Z}}_{{\rm{eff }}}}\) is high and require one electron for octet
2 Due to large size
3 Energy of halogen increases by accepting electron
4 They are non metals
Explanation:
Halogens have the smallest size in their respective periods and therefore high effective nuclear charge. As a consequence, they readily accept one electron to acquire noble gas electronic configuration.
CHXI11:THE P-BLOCK ELEMENTS
316592
Among the following, the one that is relatively most electropositive is
1 \(\mathrm{F}\)
2 \(\mathrm{Cl}\)
3 \(\mathrm{Br}\)
4 \({\rm{I}}\)
Explanation:
On moving down the group \({\rm{F}}\,\,{\rm{to}}\,\,{\rm{I}}\) electronegativity decreases and electropositive nature increases.
