Periodic Table Questions

The correct order of electron affinity of B, C, N, O is -

The electron affinities of N, O, S and Cl are such that -

Electron affinity is a -

Consider the following changes - A → A⁺ + e⁻ : E₁ and A⁺ → A²⁺ + e⁻ : E₂ The energy required to pull out the two electrons are E₁ and E₂ respectively. The correct relationship between two energies would be -

The correct values of ionization enthalpies (in kJ mol⁻¹) of Si, P, Cl and S respectively are -

I.P. of sodium is 5.14 eV, then I.P. of potassium will be -

M(g) → M⁺(g) + e⁻, ΔH = 100 eV M(g) → M²⁺(g) + 2e⁻, ΔH = 250 eV Which is incorrect statement ?

First, second and third IP values are 100eV, 150eV and 1500eV. Element can be -

The correct order of second ionization potential of C, N, O and F is -

Arrange the elements S, P, As in order of increasing ionization enthalpy -

The order of first ionisation enthalpies of the elements Li, Be, B, Na is -

For the processes K⁺(g) ─I→ K(g) ─II→ K(s)-

The decreasing order of the ionization potential of the following elements is -

The first (IE₁) and second (IE₂) ionization energies (kJ/mol) of a few elements designated by Roman numerals are given below. Which of these would be an alkali metal ? IE₁ IE₂

Element X, Y and Z have atomic numbers 19, 37 and 55 respectively. Which of the following statements is true -

Which of the following transitions involves maximum amount of energy -

The correct order of decreasing first ionisation energy is -

Among the following elements (Whose electronic configuration is given below) the one having the highest ionisation energy is -

Which of the following has 2nd IP < 1st IP -

The ionisation energy of B and Al as compared to Be and Mg are -

Successive ionisation energies of an element ‘X’ are given below (in k.cal) : IP₁ = 165 IP₂ = 195 IP₃ = 556 IP₄ = 595 Electronic configuration of the element 'X' is -

With reference to ionisation potential which one of the following sets is correct -

The IP₁, IP₂, IP₃, IP₄ and IP₅ of an element are 7.1, 14.3, 34.5, 46.8, 162.2 eV respectively. The element is likely to be -

HC≡C–CH=CH–CH₃. Which carbon atom will show minimum electronegativity -

Which one of the following is incorrect ?

Electronegativity of the following elements increases in the order -

Outermost electronic configuration of the most electronegative element is -

Which of the following is affected by stable configuration of an atom : (i) Electronegativity (ii) Ionisation potential (iii) Electron affinity Correct answer is -

Which of the following configuration will have least electron affinity -

The process requiring the absorption of energy is -

The electron affinity values for the halogens shown the following trend -

The element having very high ionization enthalpy but zero electron gain enthalpy is-

Second electron affinity of an element is -

Which of the following process energy is liberated -

In the process Cl(g) + e⁻ → Cl⁻(g), ΔH is -

Electron addition would be easier in -

The correct order of electron affinity is -

In the formation of a chloride ion, from an isolated gaseous chlorine atom, 3.8 eV energy is released, which would be equal to -

In which case the energy released is minimum -

Highest ionisation potential in a period is shown by -

IP₁ and IP₂ of Mg are 178 and 348 K.cal mol⁻¹. The enthalpy required for the reqction Mg → Mg²⁺ + 2e⁻ is -

Ionisation energy increases in the order -

The correct order of stability of Al⁺, Al²⁺, Al³⁺ is-

A sudden large jump between the values of 2nd and 3rd IP of an element would be associated with the electronic configuration-

The second ionisation potentials in electron volts of oxygen and fluorine atoms are respectively given by -

The maximum tendency to form unipositive ion is for the element with the electronic configuration-

Correct orders of 1st I.P. are - (i) Li < B < Be < C (ii) O < N < F (iii) Be < N < Ne

Which of the following is not isoelectronic series-

Consider the isoelectronic series : K⁺, S²⁻, Cl⁻ and Ca²⁺, the radii of the ions decrease as -

Arrange the following in order of increasing atomic radii Na, Si, Al, Ar -