For the second-period elements, the correct increasing order of first ionisation enthalpy is:
1. | Li < Be < B < C < O < N < F < Ne |
2. | Li < Be < B < C < N < O < F < Ne |
3. | Li < B < Be < C < O < N < F < Ne |
4. | Li < B < Be < C < N < O < F < Ne |
A configuration with the lowest ionization enthalpy among the following is:
1. \(1 s^2 2 s^2 2 p^5\)
2. \(1 s^2 2 s^2 2 p^3\)
3. \(1 s^2 2 s^2 2 p^6 3 s^1\)
4. \(1 s^2 2 s^2 2 p^6\)
The correct order of the decreasing ionic radii among the following isoelectronic species is:
1.
2.
3.
4.
The correct order of ionic radii is:
1.
2.
3.
4.
Magnesium reacts with an element (X) to form an ionic compound. If the ground state electronic configuration of (X) is , the simplest formula for this compound is:
1.
2.
3.
4.
Element of the third period that is expected to exhibit positive electron gain enthalpy is:
1. | Na | 2. | Al |
3. | Cl | 4. | Ar |
The most non-metallic element among the given elements is
1. | Be | 2. | B |
3. | Mg | 4. | Al |
In alkaline earth metals, the properties, from the following, that will increase from Be to Ba are-
(i) Atomic radius
(ii) Ionisation energy
(iii) Nuclear charge
1. | (i) and (ii) | 2. | (i) and (iii) |
3. | (ii) and (iii) | 4. | (i), (ii), and (iii) |
The following property/ies decrease from left to right across the periodic table and increase from top to bottom:
(i) Atomic radius (ii) Electronegativity (iii) Ionisation energy (iv) Metallic character
1. | (i) only | 2. | (i), (ii), and (iii) |
3. | (i), (iii), and (iv) | 4. | (i), and (iv) |
Consider the following electronic configuration of an element (P) :
The correct statement about element 'P' is :
1. It belongs to the 6th period and the 1st group.
2. It belongs to the 6th period and the 2nd group.
3. It belongs to the 6th period and the 3rd group.
4. None of the above.