The period and group number of the element with Z =114 are:

1.	8th period and 16th group	2.	7th period and 14th group
3.	14th period and 7th group	4.	9th group and 14th period

The atomic number of the element present in the 3rd period and 17th group of the periodic table would be:

The resemblance in physical and chemical properties within a group of the periodic table is a result of:

1. Same atomic number

2. Same number of valence electrons

3. Same atomic mass

4. Same number of isotopes

What does the ionic radius represent?

 The trend of atomic radius in a period and a group is :

Anions generally possess larger atomic radii than their corresponding neutral atoms. This is primarily due to:

The energy of an electron in the ground state of a hydrogen atom is −2.18 × 10⁻¹⁸ J per atom. Find the ionization enthalpy of atomic hydrogen in J mol⁻¹.

1. 2.81 × 10⁶ J mol${}^{-1}$

2. 1.31 × 10⁶ J mol${}^{-1}$

3. 2.31 × 10⁶ J mol${}^{-1}$

4. 1.81 × 10⁶ J mol${}^{-1}$

The explanation for the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium would be :

The first ionization enthalpy values (in kJ mol^–1) of group 13 elements are :

The explanation for the deviation from the general trend can be:

1. B has filled subshells, giving it unusually high ionization energy

2. Ga has a filled 3d¹⁰ subshell, increasing the effective nuclear charge

3. Indium has a very small atomic size, lowering its ionization energy

4. Tl has an unusually low nuclear charge, decreasing ionization energy

Which of the following pairs correctly identifies the element with the more negative electron gain enthalpy in each set?
(i) O or F  (ii) F or Cl

1. O, Cl
2. F, F
3. O, F
4. F, Cl