Explain why there is a phenomenal decrease in ionisation enthalpy from carbon to silicon?
(N/A) The ionisation enthalpy of carbon (the first element of group $14$) is very high $(1086 \, kJ/mol)$.
This is expected due to its small atomic size.
However,on moving down the group to silicon,there is a sharp decrease in the ionisation enthalpy $(786 \, kJ/mol)$.
This is because of an appreciable increase in the atomic size of elements when moving down the group,which reduces the effective nuclear attraction on the valence electrons.
This is expected due to its small atomic size.
However,on moving down the group to silicon,there is a sharp decrease in the ionisation enthalpy $(786 \, kJ/mol)$.
This is because of an appreciable increase in the atomic size of elements when moving down the group,which reduces the effective nuclear attraction on the valence electrons.
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View Solution$B$ has a smaller first ionization enthalpy than $Be$. Consider the following statements:
$(I)$ It is easier to remove a $2p$ electron than a $2s$ electron.
$(II)$ The $2p$ electron of $B$ is more shielded from the nucleus by the inner core of electrons than the $2s$ electrons of $Be$.
$(III)$ The $2s$ electron has more penetration power than the $2p$ electron.
$(IV)$ The atomic radius of $B$ is more than $Be$.
(Atomic number: $B=5, Be=4$)
The correct statements are:
$(I)$ It is easier to remove a $2p$ electron than a $2s$ electron.
$(II)$ The $2p$ electron of $B$ is more shielded from the nucleus by the inner core of electrons than the $2s$ electrons of $Be$.
$(III)$ The $2s$ electron has more penetration power than the $2p$ electron.
$(IV)$ The atomic radius of $B$ is more than $Be$.
(Atomic number: $B=5, Be=4$)
The correct statements are:
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