IONISATION ENTHALPY-RECAP

The magnitude of ionization energy depends on

• Spin-spin repulsion

• Number of positive charges

• shielding effect increases

• All of the above

Ionization energy between last element of one period and first element of next period receives a rapid

• increase

• decrease

• constancy

• Neutral

Nuclear charge increases in periodic table

• Across a period

• Down a group

• d-Block

• s-Block

The electronic configuration is evident by the successive

• Ionization energies

• Polarity

• Electronegativity

• Shielding effect

The force of attraction between nucleus and electrons increases across a period because

• nuclear charge increases

• distance remains constant

• Shielding effect remains constant

• All of the above

The electron configuration of elements A, B and C are [He]2s1, [Ne]3s1 and [Ar]4s1 respectively. Which one of the following order is correct for the first ionization potentials (in kJ mol–1) of A, B and C?

• A > B > C

• C > B > A

• B > C >A

• C > A > C

The correct order of second ionization energies of C, N, O and F is:

• C > N > O > F

• O > N > F > C

• O > F > N > C

• F > O > N > C

Which of the following species has the highest ionization potential?

• Li⁺

• Mg⁺

• Al⁺

• Ne

The electronic configuration with the highest ionization enthalpy is _______

• 1S¹

• 1S²

• 2S²

• 2S²

The set representing correct order of first ionization potential is:

• K > Na > Li

• Be > Mg > Ca

• B > C > N

• Ge > Si > C