Structure of the Atom Class 9 Notes
Structure of the atom – An atom is a particle of matter that uniquely defines a chemical element.
An atom consists of a nucleus located in the middle that is surrounded by electrons. The nucleus contains relatively heavy particles known as protons and neutrons.
Therefore, protons, neutrons, and electrons are the three fundamental particles found in an atom. Protons and neutrons make up the atom’s nucleus. The electron shell is the outermost area where the electrons are situated.
Electrons are negatively charged particles located inside all kinds of atoms. Electrons were first discovered in an experiment by J. J. Thomson in 1897, who noticed that negatively charged particle discharged from the cathode toward the anode.
In the same chamber, under a different circumstance, Ernest Goldstein found in 1886 that the anode released positively charged particles known as Canal rays or subsequently designated as Protons.
A subatomic particle with no charge and a mass comparable to the protons in the nuclei of all atoms was found by J. Chadwick. Hence, they came to be known as neutrons, meaning those charged neutrally.
Atomic Structure of different elements
The carbon atom has a mass of 12 due to the presence of six protons, six electrons, and six neutrons.
The oxygen atom has a mass of 16, consisting of eight protons, eight electrons, and eight neutrons.
There is just one proton, one electron, and no neutrons in the hydrogen atom (H).
Two protons, two electrons, and two neutrons make up the helium atom, giving it a mass number of two.
Structure of an Atom: Different Models
Many ideas have been developed since the discovery of atoms by several eminent scientists.
The key atomic structure hypotheses are listed below.
According to J. J. Thomson, an atom’s structure is comparable to a Christmas pudding because electrons are entangled in the sphere like currants.
He proposed that:
- An atom’s structure is a positively charged sphere with embedded electrons.
- Because the magnitudes of the protons and electrons in an atom are equal, it is electrically neutral.
Drawbacks of Thomson’s Model
Thomson’s model did not adequately explain the configuration of protons and electrons in an atom’s structure.
Rutherford bombarded a gold foil with alpha ()-particles in an experiment.
He prepared certain postulates for the experiment based on his observations of the alpha ()-particles’ track after passing through an atom, including:
- Since the particles quickly went through the gold foil, the majority of the space in an atom is vacant.
- All of an atom’s mass is located in the nucleus, which is the positively charged center of the atom. One thousand eight hundred particles bombarded the nucleus before deflecting.
- The route on which the electrons orbit the center is known.
- The nucleus is tiny compared to the size of the entire atom.
Rutherford made these hypotheses via an experiment involving the scattering of alpha ()-particles on gold foil.
Drawbacks of the Model
Rutherford offered a brand-new model for the atom’s structure, but it had several flaws that he did not address, including the following:
- The electrons accelerate as they spin in an unsteady direction, emitting energy. The electrons expend energy as they spin. The nucleus would soon contain all of the electrons. While the atom is relatively stable, this inclination would make it exceedingly unstable.
- Rutherford’s theory of the structure of an atom could only account for the existence of protons in the nucleus, not the idea of atomic number.
To address the issues Rutherford’s model presented, Bohr created a model.
So, he stated the following postulates:
- Only a limited number of electron orbitals are allowed in an atom, which is how the atom’s exterior structure is formed.
- The negatively charged particles in these orbitals or energy levels do not lose energy while rotating.
- A shift in magnitude occurs as the electron moves from one energy shell to another.
Bohr’s model addresses the problems that all prior atomic structure models had and provides a detailed description of atomic structure.
Mass Number (A)
The mass number depicts the “Total number of protons and neutrons” in an atom’s nucleus.
The notation (A) depicts the Mass number. The notation (N) depicts the total number of Neutrons.
Or A = Z+N
Mass Number is also referred to as Nucleon number.
Atomic Number (Z)
The number of protons in the nucleus of an atom, which determines its atomic number, is present in every atom of an element. The atom has the same amount of protons and electrons since it is electrically neutral
A = Z+N
The atomic number is represented by the letter Z. For example, since hydrogen only contains one proton, it has an atomic number of one.
You will benefit from understanding these key components of the chapter structure of an atom:
In an atom,
NCERT Solution for Class 9 Science, Chapter 4: Structure of the atom
FAQs (Frequently Asked Questions)
State the limitations of J.J Thomson’s model of the atom.
According to this theory, the positively charged spheres have electrons embedded all over them. However, research has revealed that electrons are dispersed all around an atom’s nucleus while protons are only found in the center of an atom.
State the limitations of Rutherford’s model of the atom.
In accordance with this theory, the electrons circle the nucleus in a circular pattern. Any such particle would experience acceleration and release energy as it swung around the nucleus. The atom would be extremely unstable since the rotating electron would eventually lose all of its energy and fall into the nucleus. The atoms are quite stable, despite this.
State the properties of electrons, protons, and neutrons.
In the case of Electrons,
|Electrons||Negligible mass||Outside Nucleus||Attracts positively charged||Negative (-)|
In the case of Protons,
|Protons||1 a. m. u||Within Nucleus||Attracts negatively charged||Positive (+)|
In the case of Neutrons,
|Neutrons||1 a. m. u||Inside Nucleus||Neither positive nor negative charge||Positive (+)|
Check out Worksheet on Magnetism and Electromagnetism
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