Match the element in column I with that in column II.
Column-I | Column-II |
(a) Copper | (i) Non-metal |
(b) Fluorine | (ii) Transition metal |
(c) Silicon | (iii) Lanthanoid |
(d) Cerium | (iv) Metalloid |
(a) | (b) | (c) | (d) | |
1. | (ii) | (iv) | (i) | (iii) |
2. | (ii) | (i) | (iv) | (iii) |
3. | (iv) | (iii) | (i) | (ii) |
4. | (i) | (ii) | (iii) | (iv) |
Among the elements Ca, Mg, P and Cl, the correct order of increasing atomic radii is:
1. Cl < P < Mg < Ca
2. P < Cl < Ca < Mg
3. Ca < Mg < P < Cl
4. Mg < Ca < Cl < P
The value of electron gain enthalpy of Na+ if IE1 of Na = 5.1 eV ,is
1. + 10.2 eV
2. –5.1 eV
3. –10.2 eV
4. + 2.55 eV
Which one of the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of the given atomic species:
1. F < Cl < O < S
2. S < O < Cl < F
3. O < S < F < Cl
4. Cl < F < S < O
In which of the following molecule, the internuclear distance will be maximum:
1. CsI
2. CsF
3. LiF
4. LiI
The first ionization potential of Be and B will be:
1. 8.8 and 8.8
2. 6.6 and 6.6
3. 6.6 and 8.8
4. 8.8. and 6.6
An electronic configuration that has maximum difference between II and III ionization potential is:
1. 1s2 2s2 2p6 3s1
2. 1s2 2s2 2p6 3s2
3. 1s2 2s2 2p6
4. 1s2 2s2 2p5
Ionic radii are:
1. | Inversely proportional to the square of effective nuclear charge. |
2. | Directly proportional to the effective nuclear charge. |
3. | Directly proportional to the square of effective nuclear charge. |
4. | Inversely proportional to the effective nuclear charge. |
Incorrect order among the following is:
1. NH3 < PH3 < AsH3 – Acidic
2. Li < Be < B < C – Ist Ionization potential
3. Al2O3 < MgO < Na2O < K2O - Basic
4. Li+ < Na+ < K+ < Cs+ - Ionic radius
If an atom has electronic configuration 1s22s22p63s23p63d34s2, we will place it in group number:
1. | Fifth | 2. | Fifteenth |
3. | Second | 4. | Third |