Which element will have the following property in the periodic table 1) Largest atomic size 2) Highest electron affinity 3) lowest ionisation enthalpy in group II 4) gaseous form at room temperature

1) Largest atomic size, Francium Fr

2) Highest electron affinity, Fluorine F

3) lowest ionisation enthalpy in group II, radio Ra

4) gaseous form at room temperature, The elements that are in a gaseous state are the noble gases (He, Ne, Ar, Kr, Xe and Rn) hydrogen, nitrogen, oxygen.

Explanation:

1) Atomic size increases on the periodic table from top to bottom and from right to left.

2) The electronic affinity increases from left to right, and from bottom to top, as does electronegativity.

3) In the elements of the same group, the ionization energy decreases as the atomic number increases, that is, from top to bottom.

1) Francium

2) Chlorine

3) Barium

4) Rn, Xe, Kr, Ar, Ne, He, F, Cl, O, N and H

Explanation:

1) The atomic radius increases from the top to the bottom of a given group and decreases from the left hand side of a given period to the right of the period. Therefore looking at the bottom left of the periodic table, the atom with the largest atomic radii is Francium

2) Elements with the highest electron are located at the top right corner of the periodic table, opposite to the location of the elements with the highest atomic radius, however, although Fluorine has the highest electronegativity, Chlorine has the highest electron affinity, due to the repulsion present in the 2-p sub-shell of Fluorine

3) Ionization energies increases from bottom to top of given group, therefore, the element with the lowest ioniztion energy in group II is the element at the bottom of the group which is Ba or barium

4) The gaseous elements are located at the top and extreme right of the periodic table and includes the elements of group 8A (radon (Rn), xenon (Xe), krypton (Kr), Argon (Ar), Neon (Ne) as well as Fluorine (F), Chlorine (Cl), Oxygen (O), Nitrogen (N), Helium (He) and Hydrogen (H).