Which of the following sets of atomic numbers corresponds to elements of group 16?

1. 8,16, 32, 54

2. 16, 34, 54, 86

3. 8,16, 34, 52

4. 10,16, 32, 50

Sodium generally does not show oxidation state of +2, because of its: 

 

1. High first ionization potential

2. High second ionization potential 

3. Large ionic radius

4. High electronegativity

Assuming that elements are formed to complete the seventh period, the atomic number of alkaline earth metal of the eighth period would be:

1. 113

2. 120

3. 119

4. 106

Which of the following is not representative element?

1. Tellurium

2. Tantalum

3. Thallium

4. Astatine

Largest in size out of Na⁺, Ne and F^- is:

1. Na⁺

2. Ne

3. F^-

4. All are equal

Incorrect order of radius is:

1. Sr²⁺<Rb⁺<Br^-<Se^2-

2. Nb⁵⁺<Zr⁴⁺<Y³⁺

3. Co>Co²⁺>Co³⁺>Co⁴⁺

4. Ba²⁺<Cs⁺<Se2^-<As^3-

The electronic configuration of four elements are :
(I)   [Kr]5s¹
(II)  [Rn]5f¹⁴6d¹7s²
(III) [Ar]3d¹⁰4s²4p⁵
(IV) [Ar]3d⁶4s²

Consider the following statements :
(i) I Shows variable oxidation state
(ii) II is a d-block element
(iii) The compound formed between I and III is covalent
(iv) IV shows single oxidation state

Which statement is True (T) or False (F)?

1. FTFF
2. FTFT
3. FFTF
4. FFFF

If the ionic radii of K⁺ and F^- are nearly the same (i.e., 1.34 Å), what are the atomic radii of K and F respectively?

X_(g)→ X⁺_(g) + e^- , ∆H = +720 KJ mol^-1

Calculate the amount of energy required to convert 110 mg of ‘X’ atom in gaseous state into X⁺ion. (Atomic wt. for X = 7 g/mol)

Which is the correct order of ionization energies?