The general electron configuration of the group having the lowest ionization energy is [Noble gas configuration]xs1. In this case, x is the principal quantum number of the valance electron. The noble gas configuration may either be written out in full or denoted by the noble gas' atomic symbol in brackets (ie [Ne]).
noble gases have the maximum ionisation energy. helium has the highest ionisation energy
Argon is a noble gas element. It has a saturated electronic configuration i.e ns2, np6. So it has a octet configuration. It is already attained stable configuration. Also it has high ionisation energy. Small in atomic size. From the above it is confirmed that it exists in atomic state only and not is molecular form. Therefore chemical bond will be zero in an atom of argon.
Their electronic configuration is similar to that of noble gases.
no the same,first ionisation contains a slightly differences in isotopes
The period of an element is determined by electronic configuration.Period is same as the number of energy levels of the element.
noble gases have the maximum ionisation energy. helium has the highest ionisation energy
Because the force of attraction between the nucleus and the outer most electron is less. In addition, most metals (but not all) will gain the stable electronic configuration of the nearest noble gas if they lose electron.
first Ionisation energy is 1681 kJ/mol = 402.15 Kcal/mol it is high because of the F electron configuration will be 1s22s22p5
Argon is a noble gas element. It has a saturated electronic configuration i.e ns2, np6. So it has a octet configuration. It is already attained stable configuration. Also it has high ionisation energy. Small in atomic size. From the above it is confirmed that it exists in atomic state only and not is molecular form. Therefore chemical bond will be zero in an atom of argon.
Their electronic configuration is similar to that of noble gases.
lol energy level... it's ELECTRONIC CONFIGURATION!!the answer is 8
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.
Beacause of electronic configuration (M.O.T)
no the same,first ionisation contains a slightly differences in isotopes
No
Electronic configuration of scandium: [Ar]3d1.4s2