Q. No.Boron has lesser ionization enthalpy than Beryllium, because -
1.
It is easier to remove electrons from p - a subshell than a filled s - subshell.
2.
The s-electron can be removed easier than the p-electron.
3.
Ionization enthalpy decreases with an increase in atomic number.
4.
Ionization enthalpy increases along the period.
Difference between electron gain enthalphy and electronegativity is described by :
1) Valence electrons
2) Atomic size
3) Atomic radii
3) Atomic number
Incorrect statement about metal is:
1. Metals can donate electrons.
2. Metals form ionic compounds.
3. Metals are more electronegative.
4. Metals have less ionization energy.
The group number that has non-metal, liquid as well as gas at room temperature, is -
| 1. | 15 | 2. | 14 |
| 3. | 18 | 4. | 17 |
| Elements | |||
| I | 520 | 7300 | -60 |
| II | 419 | 3051 | -48 |
| III | 1681 | 3374 | -328 |
| IV | 1008 | 1846 | -295 |
| V | 2372 | 5251 | +48 |
| VI | 738 | 1451 | -40 |
1. III
2. IV
3. II
4. V
Incorrect statement among the following is :
| 1. | The p-block has 6 columns because a maximum of 6 electrons can occupy all the orbitals in a p-shell. |
| 2. | The d-block has 8 columns because a maximum of 8 electrons can occupy all the orbitals in a d-subshell. |
| 3. | Each block contains a number of columns equal to the number of electrons that can occupy that subshell. |
| 4. | The s- block contains mainly reactive metals. |
Among the following elements, the one that is not an actinoid is:
| 1. | Curium (Z=96) | 2. | Californium (Z=98) |
| 3. | Uranium (Z=92) | 4. | Terbium (Z=65) |
The order of screening effect of electrons of s, p, d and f orbitals of a given shell of an atom on electrons in its outer shell is :
1. s > p > d > f
2. f > d > p > s
3. p < d < f < s
4. f > p > s > d
Among halogens, the correct order of amount of energy released in electron gain (electron gain enthalpy) is-
| 1. | F > Cl > Br > I | 2. | F < Cl < Br < I |
| 3. | F < Cl > Br > I | 4. | F < Cl < Br > I |
The period number in the long form of the periodic table is equal to :
| 1. | Magnetic quantum number of any element of the period. |
| 2. | Atomic number of any element of the period. |
| 3. | Maximum principal quantum number of any element of the period. |
| 4. | Maximum azimuthal quantum number of any element of the period. |
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