Factors Affecting Ionisation Energy || Trends-along Period and Group Comparison OF IE1/IE2/IE3 OF P-2 and IE1/IE2/IE3/IE4 OF Na,Mg and Al

Ionisation potential (IP) and ionisation (IE) are related a

The correct order of third ionization energies (IE_3) of Na, Mg and Al is

The second ionisation energies are higher than the first ionisation energies. This is mainly due to the fact that after the removal of the first electrons, the atom changes inot mono valent position ion. In the ion, the number of electrons decreases but the nuclear charge remains the same. As a result of this, the remaining electrons are held more tightly by the nucleus and it becomes difficult to remove the second electron . Therefore, the value of second ionisation energy . (IE_(2)) , is greater than that of the first ionisation energy (IE_(1)) . Similarly third ionisation energy (IE_(3)) is greater than that of second IE_(2) . IE_(1) and IE_(2) of Mg metal are 178 and 348 kcal/mol respectively . The energy required for the given reaction is : Mg(g)rarr Mg^(+2)(G)+2e^(-)

Atomic Radius |Variation Of Atomic Radius Along The Period|Variation Of Atomic Radius Along The Group|Radius Of Isoelectronic Species|Ionization Energy|Successive Ionization Energy|Variation Of I.E. In Group|Second I.E. Of Oxygen Is Greater Than Second I.E. Of Nitrogen|Summary

Choose the correct pair regarding ionisation energy (IE_(1))

The energy required to remove an electron from the outermost shell of an isolate gaseous atom is known as IE_(1) of that atom. Similarly, the enrgy required for the removal of the electron from the unipositive ion, diapositive ion and tripositive ion are known as IE_(2),IE_(3) and IE_(4) respectively, and are called successive ionisation energies. The magnitude of the charge depends on the size of the orbital of electron. Electrons in smaller orbitals are on average close with each other and have more repulsion. Thus for Be(2s^(2)) , the IE_(1) and IE_(2) are 9.3 and 18.2 eV "atom"^(1) , whereas for Ca(4s^(2)) , the values are 6.1 and 11.9 eV . The relationship between IE_(4) and IE_(2) of an element is

The second ionisation energies are higher than the first ionisation energies. This is mainly due to the fact the after the removal of the first electron, the atom changes into monovalent positive ion. In the ion, the number of electrons decreases but the nuclear charge remains the same. as a result of this, the remaining electrons are held more tightly by the nucleus and it becomes difficult to remove the second electron. therefore, the value of second ionisation energy. (IE_(2)) , is greater than that of the first ionisatio energy (IE_(1)) . similarly third ionisation energy (IE_(3)) is greater than that of second IE_(2) . Q. IE_(1) and IE_(2) of Mg metal are 178 and 348 kcal/mol respectively. the energy required for the given reaction is: Mg(s) to Mg^(+2)+2e^(-)