Advertisements
Advertisements
Question
State Heisenberg uncertainty principle.
Advertisements
Solution
Heisenberg's uncertainty principle states that “It is impossible to determine simultaneously, the exact position and exact momentum (or velocity) of an electron”.
APPEARS IN
RELATED QUESTIONS
Choose the correct option.
p-orbitals are _________ in shape.
Define the term Electronic configuration.
Explain the anomalous behaviour of copper.
Explain the anomalous behaviour of chromium.
Write orbital notations for the electron in orbitals with the following quantum numbers.
n = 4, l = 2
Write orbital notations for the electron in orbitals with the following quantum numbers.
n = 3, l = 2
Write electronic configurations of \[\ce{Fe, Fe2+, Fe3+}\].
Write condensed orbital notation of electronic configuration of the following element:
Calcium (Z = 20)
Draw shapes of 2s orbitals.
Explain in brief, the significance of the azimuthal quantum number.
Write a note on ‘Principal Quantum number.
Using the concept of quantum numbers, calculate the maximum numbers of electrons present in the ‘M’ shell. Give their distribution in shells, subshells, and orbitals.
The probability density plots of 1s and 2s orbitals are given in Figure:
The density of dots in a region represents the probability density of finding electrons in the region.
On the basis of above diagram which of the following statements is incorrect?
The number of radial nodes for 3p orbital is ______.
Total number of orbitals associated with third shell will be ______.
Orbital angular momentum depends on ______.
The pair of ions having same electronic configuration is ______.
Calculate the total number of angular nodes and radial nodes present in 3p orbital.
The arrangement of orbitals on the basis of energy is based upon their (n + l) value. Lower the value of (n + l), lower is the energy. For orbitals having same values of (n + l), the orbital with lower value of n will have lower energy.
Based upon the above information, arrange the following orbitals in the increasing order of energy.
4s, 3s, 3p, 4d
What is the difference between the terms orbit and orbital?
Match species given in Column I with the electronic configuration given in Column II.
| Column I | Column II |
| (i) \[\ce{Cr}\] | (a) [Ar]3d84s0 |
| (ii) \[\ce{Fe^{2+}}\] | (b) [Ar]3d104s1 |
| (iii) \[\ce{Ni^{2+}}\] | (c) [Ar]3d64s0 |
| (iv) \[\ce{Cu}\] | (d) [Ar] 3d54s1 |
| (e) [Ar]3d64s2 |
Choose the INCORRECT statement
Which of the following is not the permissible arrangement of electrons in an atom?
