As discussed in the previous chapter, according to Dalton’s atomic theory, atoms are the building blocks of matter. In the year 1808, John Dalton proposed the atomic theory saying that the atom is an indivisible particle of matter. By the end of the nineteenth century, experiments proved that atoms comprise three particles viz protons, neutrons, and electrons. Therefore, the discovery of sub-atomic particles gave rise to various atomic models to explain the structure of an atom.
For more information on Discovery of Electrons and Its Charge, watch the below video:
Common terminologies used – Structure of Atom
- Electrons – These subatomic particles orbit around the nucleus. They are negatively charged particles and found in definite energy levels orbiting the nucleus.
- Protons – These subatomic particles are found in the nucleus. They are positively charged particles and belong to the nucleon group.
- Neutrons – These subatomic particles are found in the nucleus. They are neutral particles and belong to the nucleon group.
- Rutherford model – It states that during a chemical reaction, the mass of the products and reactants will always be equal.
- Bohr model – The model states that electrons orbit stable around the nucleus in certain fixed circular orbits at a distinct distance from the nucleus. These orbits are related to specific energies and are also referred to as energy levels or energy shells.
- Heisenberg uncertainty principle – The Heisenberg Uncertainty Principle states that the simultaneous determination of the velocity and position of a particle is impossible.
- Shells – A pathway followed by the electron to move around the nucleus of the atom.
- Subshells – A pathway for the electron to move within a shell.
For more information on Rutherford Atomic Model, watch the below videos
For more information on the Quantum Mechanical Model of the Atom, watch the below videos
| Also Access |
| NCERT Solutions for Class 11 Chemistry Chapter 2 |
| NCERT Exemplar for Class 11 Chemistry Chapter 2 |
Few Important Questions
1. Calculate the wavenumber and frequency for the below:
Yellow light emitted from a sodium lamp has a wavelength (λ) of 580 nm
2. Calculate and provide the number of electrons for the following:
- H+2
- O+2
- H2
3. Calculate the wavelength using the following details:
The mass of an electron is 9.1 × 10–31 kg and K.E. is 3.0 × 10–25 J
For more information on Atomic Structure Solved Questions, watch the below video
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Other Important Links:
| Bohr Model | Rutherford Model |
Frequently Asked Questions on CBSE Class 11 Chemistry Notes Chapter 2 Structure of an Atom
What does the Heisenberg uncertainty principle state?
The Heisenberg Uncertainty Principle states that the simultaneous determination of the velocity and position of a particle is impossible.
Who was Rutherford?
Ernest Rutherford was a New Zealand physicist who came to be known as the father of nuclear physics.
What is wavelength?
The distance between corresponding points of two consecutive waves is known as wavelength. It is usually denoted by the Greek letter lambda.
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