Based on equation E = –2.178 × 10–18J, certain conclusions are written. Which of them is not correct?
1. | Larger the value of n, the larger the orbit radius. |
2. | Equation can be used to calculate the change in energy when the electron changes orbit. |
3. | For n = 1, the electron has a more negative energy than it does for n = 6 which means that the electron is more loosely bound in the smallest allowed orbit. |
4. | The negative sign in the equation simply means that the energy of the electron bound to the nucleus is lower than what it would be if the electrons were at an infinite distance from the nucleus. |
1. 16
2. 32
3. 4
4. 8
The energies E1 and E2 of two radiations are 25 eV and 50 eV respectively. The relation between their wavelengths i.e., and will be:
1.
2.
3.
4.
If the energy of the second Bohr orbit of the hydrogen atom is –328 kJ mol–1, the energy of the fourth Bohr orbit would be:
1. | –1312 kJ mol–1 | 2. | –82 kJ mol–1 |
3. | –41 kJ mol–1 | 4. | –164 kJ mol–1 |
Ionization energy of second orbit of will be:
1. 122.4 eV
2. 40.8 eV
3. 30.6 eV
4. 13.6 eV
The radius of a hydrogen shell is 0.53Å. In its first excited state, radius of the shell will be:
1. 2.12 Å
2. 1.06 Å
3. 8.5 Å
4. 4.24 Å