Multiple Choice

The factors that influence the ionisation energies are :

Athe size of the atom
Correct Answer
Bthe charge on the nucleus
Correct Answer
Chow effectively the inner electrons screen the nuclear charge
Correct Answer
Dthe atomic mass

Solution

Factors which influence the ionization energies are:
Concept involved:
Ionization potential : Energy required to remove an electron from outermost orbit of a gaseous neutral atom.
A) Atomic size(atomic radius):As the atomic size increases ionization potential decreases because less energy is required to remove electron when size is more.
B) The charge on the nucleus:As the charge on the nucleus increases ionization potential increases because it requires more energy when the charge is more on nucleus.
C) how effectively the inner electrons screen the nuclear charge(shielding effect): As the shielding effect increases ionization potential increase because it requires more energy to remove electron.
D) Atomic mass do not influences the ionization potential.Because ionization potential is Energy required to remove an electron from outermost orbit not from the entire atom.
Hence option A,B & C are correct.

SIMILAR QUESTIONS

Periodic Classification of Elements

The ionization energy of nitrogen is more than that of oxygen because :

Periodic Classification of Elements

Which of the following elements has the highest ionization energy?

Periodic Classification of Elements

Which one of the following elements has the highest first ionization potential?

Periodic Classification of Elements

Gradual addition of electronic shells in the noble gases causes a decrease in their:

Periodic Classification of Elements

Which one of the following statements is incorrect in relation to ionization enthalpy? (a) Ionization enthalpy increases for each successive electron. (b) The greatest increases in ionization enthalpy is experienced on removal of electron from core noble gas configuration. (c) End of valence electrons is marked by a big jump in ionization enthalpy. (d) Removal of electron from orbitals bearing lower n value is easier than from orbital having higher n value.

Periodic Classification of Elements

The first ($$\Delta H_{1}$$) and second ($$\Delta H_{2}$$) ionisation enthalpies (in $$kJ mol^{-1}$$) and the electron gain enthalpy ($$\Delta_{eg}H$$) (in $$kJ mol^{-1}$$) of the elements I, II, III, IV and V are given below: Element $$\Delta_{1}H_{1}$$ $$\Delta_{1}H_{2}$$ $$\Delta_{eg}H$$ I 520 7300 -60 II 419 3051 -48 II 1681 3374 -328 IV 1008 1846 -295 V 2372 5251 +48 The most reactive metal and the least reactive non-metal of these are respectively.

Periodic Classification of Elements

Nuclear charge increases in a period as well as group. However, periodic properties such as atomic size and IP show a reverse trend. Why?

Periodic Classification of Elements

Gradual addition of electronic shells in the noble gases causes a decrease in their:

Periodic Classification of Elements

Poor shielding of nuclear charge by d or f-orbital electrons is responsible for which of the following facts?

Periodic Classification of Elements

Which of the following element has maximum first ionisation potential?

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