Q. No.How many elements are present in the sixth period of the periodic table?
1. 32
2. 36
3. 35
4. 33
The period and group number of the element with Z =114 are:
| 1. | 8th period and 16th group | 2. | 7th period and 14th group |
| 3. | 14th period and 7th group | 4. | 9th group and 14th period |
The atomic number of the element present in the 3rd period and 17th group of the periodic table would be:
| 1. | 18 | 2. | 23
|
| 3. | 24
|
4. | 17 |
The resemblance in physical and chemical properties within a group of the periodic table is a result of:
1. Same atomic number
2. Same number of valence electrons
3. Same atomic mass
4. Same number of isotopes
What does the ionic radius represent?
1. The distance from the nucleus to the outermost shell of an atom2. The distance from the nucleus to the outermost shell of an ion
3. The distance from the nucleus to the outermost shell of a cation only
4. The distance from the nucleus to the outermost shell of an anion only
The trend of atomic radius in a period and a group is :
| 1. | Generally decreases from right to left across a period and increases down a group. |
| 2. | Generally increases from left to right across a period and decreases down a group. |
| 3. | Generally decreases from left to right across a period and increases down a group. |
| 4. | Generally remains same from left to right across a period and increases down a group. |
Anions generally possess larger atomic radii than their corresponding neutral atoms. This is primarily due to:
| 1. | An anion has a fewer number of electrons than its parent atom |
| 2. | An anion has the same number of electrons as its parent atom. |
| 3. | An anion has a higher effective nuclear charge. |
| 4. | An anion has more electrons than its parent atom |
The energy of an electron in the ground state of a hydrogen atom is −2.18 × 10⁻¹⁸ J per atom. Find the ionization enthalpy of atomic hydrogen in J mol⁻¹.
1. 2.81 × 106 J mol
2. 1.31 × 106 J mol
3. 2.31 × 106 J mol
4. 1.81 × 106 J mol
The explanation for the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium would be :
| 1. | Pressure and volume |
| 2. | Lustre and brightness |
| 3. | Atomic size and effective nuclear charge |
| 4. | Availability in nature |
The ionization enthalpy of the main group elements tends to decrease down a group due to,
1) Increase in the atomic size of elements and increase in the shielding effect
2) Decrease in the atomic size of elements and increase in the shielding effect
3) Increase in the atomic size of elements and decrease in the shielding effect
4) Decrease in the atomic size of elements and decrease in the shielding effect
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