boron
electros removed from 2p orbitals
more shielded from the + nucleus so easily lost
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
krypton because it is an inert/noble gas, which means it has a complete outer shell and takes a lot of energy to remove an electron.
Na(g) --> Na+(g) + e- First ionisation energy is always: X(g) --> X+(g) + e- with X being an element
No
Element 115 on most modern periodic charts.
noble gases have the maximum ionisation energy. helium has the highest ionisation energy
ionisation energy order for gr 14 is c>si>ge>sn<pb
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
ionisation energy order for gr 14 is c>si>ge>sn<pb
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
Ionisation energies GENERALLY increase across a period. As a result, the noble elements (i.e. Group 0 elements) usually have the highest ionisation energies, as they are highly stable.
Ionisation energy decreases down the group. It is easy to remove an electron.
The first ionization energy of an atom or molecule describes the amount of energy required to remove an electron from the atom or molecule in the gaseous state.
1.A small atomic/ionic radius 2.therefore less number of protons 3. more net nuclear attraction between the positively charged nucleus 4. higher energy is needed to break those bonds. 5. therefore an element has high ionisation energy
no the same,first ionisation contains a slightly differences in isotopes
krypton because it is an inert/noble gas, which means it has a complete outer shell and takes a lot of energy to remove an electron.
Na(g) --> Na+(g) + e- First ionisation energy is always: X(g) --> X+(g) + e- with X being an element