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Page 1
Chapter 4 Structure of Atom
Atoms – The smallest constituent particles of matter that cannot be broken down further.
Sub atomic particles – Particles that make up an atom
There are three major sub atomic particles –
1. Protons – discovered by E. Goldstein in 1886. They are positively charged (+1). The mass of proton is
taken as 1 unit.
2. Electrons – discovered by J.J. Thomson in 1897. They are negatively charged (-1) but have negligible
mass.
3. Neutrons – Discovered by James Chadwick in 1932. They do not have any charge. The mass of neutrons
is approximately equal to that of protons and hence is taken as 1 unit.
Neutrons and protons are present in the center pf an atom inside the nucleus and the protons revolve around
them.
Thomson’s Model of Atom
He thought of an atom similar to watermelon where the red part was positively charged and the seeds as the
electrons.
Key features –
a. An atom is a positively charged sphere.
b. Electrons are embedded in that positively charged sphere.
c. The negative and the positive charges are equal in magnitude and that is why an atom is neutral as a
whole.
Fig. Thomson’s model of an atom
Drawbacks –
? Thomson’s model of atom could not explain the Rutherford’s a-particles scattering experiment.
? It could not explain the experiment of other scientists as well such as Neil Bohr.
Rutherford’s Model of an Atom
Rutherford’s Experiment
? He selected a very thin gold foil (1000atoms thick)
Electrons
Positive Sphere
Page 2
Chapter 4 Structure of Atom
Atoms – The smallest constituent particles of matter that cannot be broken down further.
Sub atomic particles – Particles that make up an atom
There are three major sub atomic particles –
1. Protons – discovered by E. Goldstein in 1886. They are positively charged (+1). The mass of proton is
taken as 1 unit.
2. Electrons – discovered by J.J. Thomson in 1897. They are negatively charged (-1) but have negligible
mass.
3. Neutrons – Discovered by James Chadwick in 1932. They do not have any charge. The mass of neutrons
is approximately equal to that of protons and hence is taken as 1 unit.
Neutrons and protons are present in the center pf an atom inside the nucleus and the protons revolve around
them.
Thomson’s Model of Atom
He thought of an atom similar to watermelon where the red part was positively charged and the seeds as the
electrons.
Key features –
a. An atom is a positively charged sphere.
b. Electrons are embedded in that positively charged sphere.
c. The negative and the positive charges are equal in magnitude and that is why an atom is neutral as a
whole.
Fig. Thomson’s model of an atom
Drawbacks –
? Thomson’s model of atom could not explain the Rutherford’s a-particles scattering experiment.
? It could not explain the experiment of other scientists as well such as Neil Bohr.
Rutherford’s Model of an Atom
Rutherford’s Experiment
? He selected a very thin gold foil (1000atoms thick)
Electrons
Positive Sphere
? He passed fast moving a-particles through it.
? a-particles are doubly charged Helium atoms (He
2+
). They have a positive charge of two units and a
mass of 4u.
Observations
? Most of the fast moving a-particles passed straight without any deflection.
? Some of the a-particles were deflected by small angles.
? One out of 12000 particles bounced back after hitting the gold foil.
Inference or Conclusion –
? Most of the space in an atom is empty because most of the a-particles passed without deflection.
? Very few a-particles deflected with small angle indicating that the positive charge in an atom occupied
very less space.
? A very a-particles bounced back with an angle of 180
0
indicating that most of the positive charge and
mass of an atom is concentrated in a very small volume within the atom.
Fig. Rutherford’s a-particles scattering experiment.
Structure of Atom according to Rutherford –
? Nearly all the mass is concentrated in a positively charged nucleus which is present in the center of the
atom.
? The electrons revolve around the nucleus in well-defined orbits.
? The size of the nucleus is very small as compared to the size of an atom. Most of the space in an atom is
empty.
Drawback
? A particle in circular motion always undergoes acceleration. During acceleration a charged particle
radiates energy. Hence, an electron revolving around the nucleus will keep on radiating energy, keep
coming closer to the nucleus and finally fall into it
? It will make an atom highly stable.
? However, as we know that atom is quite stable but cannot be explained by Rutherford’s model.
Bohr’s Model of an atom
Postulates of Neil Bohr
? Electrons revolve only on discrete or special fixed orbits around the nucleus, in an atom.
? Electrons do not radiate energy while revolving.
Page 3
Chapter 4 Structure of Atom
Atoms – The smallest constituent particles of matter that cannot be broken down further.
Sub atomic particles – Particles that make up an atom
There are three major sub atomic particles –
1. Protons – discovered by E. Goldstein in 1886. They are positively charged (+1). The mass of proton is
taken as 1 unit.
2. Electrons – discovered by J.J. Thomson in 1897. They are negatively charged (-1) but have negligible
mass.
3. Neutrons – Discovered by James Chadwick in 1932. They do not have any charge. The mass of neutrons
is approximately equal to that of protons and hence is taken as 1 unit.
Neutrons and protons are present in the center pf an atom inside the nucleus and the protons revolve around
them.
Thomson’s Model of Atom
He thought of an atom similar to watermelon where the red part was positively charged and the seeds as the
electrons.
Key features –
a. An atom is a positively charged sphere.
b. Electrons are embedded in that positively charged sphere.
c. The negative and the positive charges are equal in magnitude and that is why an atom is neutral as a
whole.
Fig. Thomson’s model of an atom
Drawbacks –
? Thomson’s model of atom could not explain the Rutherford’s a-particles scattering experiment.
? It could not explain the experiment of other scientists as well such as Neil Bohr.
Rutherford’s Model of an Atom
Rutherford’s Experiment
? He selected a very thin gold foil (1000atoms thick)
Electrons
Positive Sphere
? He passed fast moving a-particles through it.
? a-particles are doubly charged Helium atoms (He
2+
). They have a positive charge of two units and a
mass of 4u.
Observations
? Most of the fast moving a-particles passed straight without any deflection.
? Some of the a-particles were deflected by small angles.
? One out of 12000 particles bounced back after hitting the gold foil.
Inference or Conclusion –
? Most of the space in an atom is empty because most of the a-particles passed without deflection.
? Very few a-particles deflected with small angle indicating that the positive charge in an atom occupied
very less space.
? A very a-particles bounced back with an angle of 180
0
indicating that most of the positive charge and
mass of an atom is concentrated in a very small volume within the atom.
Fig. Rutherford’s a-particles scattering experiment.
Structure of Atom according to Rutherford –
? Nearly all the mass is concentrated in a positively charged nucleus which is present in the center of the
atom.
? The electrons revolve around the nucleus in well-defined orbits.
? The size of the nucleus is very small as compared to the size of an atom. Most of the space in an atom is
empty.
Drawback
? A particle in circular motion always undergoes acceleration. During acceleration a charged particle
radiates energy. Hence, an electron revolving around the nucleus will keep on radiating energy, keep
coming closer to the nucleus and finally fall into it
? It will make an atom highly stable.
? However, as we know that atom is quite stable but cannot be explained by Rutherford’s model.
Bohr’s Model of an atom
Postulates of Neil Bohr
? Electrons revolve only on discrete or special fixed orbits around the nucleus, in an atom.
? Electrons do not radiate energy while revolving.
? These orbits are called energy levels and are denoted as K, L, M, N ………. or n = 1,2, 3, 4 . . . . ..
? An electron can lose energy to move into a lower energy level while it can gain energy and move into
higher energy shell.
Fig. Neil Bohr’s model of Atom
Number of Electrons in different shells:
? The maximum number a shell can have is given by a formula 2n
2
.
? The maximum number of electrons that can be accommodated in the last shell is 8.
? Only if the inner shells are filled, electrons can be accommodated in an outer shell.
Example –
Atomic number or carbon is 6
It means carbon has 6 protons and 6 electrons.
No. of electrons in K shell = 2n
2
For K shell n = 1 and hence no. of electrons in K shell = 2*1
2
= 2
Maximum No. of electrons left = 6-2 = 4
Maximum No. of electrons that can be accommodated in L shell = 2*2
2
= 8
Hence, the remaining 4 electrons will come in L shell.
Fig. Structure of Carbon Atom
Page 4
Chapter 4 Structure of Atom
Atoms – The smallest constituent particles of matter that cannot be broken down further.
Sub atomic particles – Particles that make up an atom
There are three major sub atomic particles –
1. Protons – discovered by E. Goldstein in 1886. They are positively charged (+1). The mass of proton is
taken as 1 unit.
2. Electrons – discovered by J.J. Thomson in 1897. They are negatively charged (-1) but have negligible
mass.
3. Neutrons – Discovered by James Chadwick in 1932. They do not have any charge. The mass of neutrons
is approximately equal to that of protons and hence is taken as 1 unit.
Neutrons and protons are present in the center pf an atom inside the nucleus and the protons revolve around
them.
Thomson’s Model of Atom
He thought of an atom similar to watermelon where the red part was positively charged and the seeds as the
electrons.
Key features –
a. An atom is a positively charged sphere.
b. Electrons are embedded in that positively charged sphere.
c. The negative and the positive charges are equal in magnitude and that is why an atom is neutral as a
whole.
Fig. Thomson’s model of an atom
Drawbacks –
? Thomson’s model of atom could not explain the Rutherford’s a-particles scattering experiment.
? It could not explain the experiment of other scientists as well such as Neil Bohr.
Rutherford’s Model of an Atom
Rutherford’s Experiment
? He selected a very thin gold foil (1000atoms thick)
Electrons
Positive Sphere
? He passed fast moving a-particles through it.
? a-particles are doubly charged Helium atoms (He
2+
). They have a positive charge of two units and a
mass of 4u.
Observations
? Most of the fast moving a-particles passed straight without any deflection.
? Some of the a-particles were deflected by small angles.
? One out of 12000 particles bounced back after hitting the gold foil.
Inference or Conclusion –
? Most of the space in an atom is empty because most of the a-particles passed without deflection.
? Very few a-particles deflected with small angle indicating that the positive charge in an atom occupied
very less space.
? A very a-particles bounced back with an angle of 180
0
indicating that most of the positive charge and
mass of an atom is concentrated in a very small volume within the atom.
Fig. Rutherford’s a-particles scattering experiment.
Structure of Atom according to Rutherford –
? Nearly all the mass is concentrated in a positively charged nucleus which is present in the center of the
atom.
? The electrons revolve around the nucleus in well-defined orbits.
? The size of the nucleus is very small as compared to the size of an atom. Most of the space in an atom is
empty.
Drawback
? A particle in circular motion always undergoes acceleration. During acceleration a charged particle
radiates energy. Hence, an electron revolving around the nucleus will keep on radiating energy, keep
coming closer to the nucleus and finally fall into it
? It will make an atom highly stable.
? However, as we know that atom is quite stable but cannot be explained by Rutherford’s model.
Bohr’s Model of an atom
Postulates of Neil Bohr
? Electrons revolve only on discrete or special fixed orbits around the nucleus, in an atom.
? Electrons do not radiate energy while revolving.
? These orbits are called energy levels and are denoted as K, L, M, N ………. or n = 1,2, 3, 4 . . . . ..
? An electron can lose energy to move into a lower energy level while it can gain energy and move into
higher energy shell.
Fig. Neil Bohr’s model of Atom
Number of Electrons in different shells:
? The maximum number a shell can have is given by a formula 2n
2
.
? The maximum number of electrons that can be accommodated in the last shell is 8.
? Only if the inner shells are filled, electrons can be accommodated in an outer shell.
Example –
Atomic number or carbon is 6
It means carbon has 6 protons and 6 electrons.
No. of electrons in K shell = 2n
2
For K shell n = 1 and hence no. of electrons in K shell = 2*1
2
= 2
Maximum No. of electrons left = 6-2 = 4
Maximum No. of electrons that can be accommodated in L shell = 2*2
2
= 8
Hence, the remaining 4 electrons will come in L shell.
Fig. Structure of Carbon Atom
Valency
The number of electrons required or need to be reduced (whichever is less) to completely fill the outer most shell is called
the valency of an element.
For e.g.
1. Carbon
Atomic number of carbon is 6
There are 2 electrons in K shell and 4 electrons in L shell but L shall can have 8 electrons.
4 electrons can either be added or removed to completely fill the outermost shell.
Hence, the valency of carbon is 4.
2. Sodium
Atomic number of carbon is 11
There are 2 electrons in K shell and 8 electrons in L shell and 1 in M shell.
M is the outer most shell and can have a maximum of 8 electrons.
So, if 1 electron is removed sodium will be left with 8 electrons in the outermost shell that is L and it will be
completely filled.
Hence, its valency is 1
Electronic configuration
It is the method of representation of the number of electrons in each shell of an atom
E.g. Atomic number of Sodium is 11
Electronic configuration = 2, 8, 1 (Because there are 2, 8 and 1 electrons in K, L and M shell respectively)
Atomic number of Oxygen is 8
Electronic configuration = 2, 6
Atomic Number
Number of protons present in the nucleus of an atom is known as its atomic number.
It is denoted by ‘Z’.
Atomic Mass
Total number protons and neutrons in an atom is known as atomic mass.
It is denoted by ‘A’
Notation or representing atomic mass and number of an element
Page 5
Chapter 4 Structure of Atom
Atoms – The smallest constituent particles of matter that cannot be broken down further.
Sub atomic particles – Particles that make up an atom
There are three major sub atomic particles –
1. Protons – discovered by E. Goldstein in 1886. They are positively charged (+1). The mass of proton is
taken as 1 unit.
2. Electrons – discovered by J.J. Thomson in 1897. They are negatively charged (-1) but have negligible
mass.
3. Neutrons – Discovered by James Chadwick in 1932. They do not have any charge. The mass of neutrons
is approximately equal to that of protons and hence is taken as 1 unit.
Neutrons and protons are present in the center pf an atom inside the nucleus and the protons revolve around
them.
Thomson’s Model of Atom
He thought of an atom similar to watermelon where the red part was positively charged and the seeds as the
electrons.
Key features –
a. An atom is a positively charged sphere.
b. Electrons are embedded in that positively charged sphere.
c. The negative and the positive charges are equal in magnitude and that is why an atom is neutral as a
whole.
Fig. Thomson’s model of an atom
Drawbacks –
? Thomson’s model of atom could not explain the Rutherford’s a-particles scattering experiment.
? It could not explain the experiment of other scientists as well such as Neil Bohr.
Rutherford’s Model of an Atom
Rutherford’s Experiment
? He selected a very thin gold foil (1000atoms thick)
Electrons
Positive Sphere
? He passed fast moving a-particles through it.
? a-particles are doubly charged Helium atoms (He
2+
). They have a positive charge of two units and a
mass of 4u.
Observations
? Most of the fast moving a-particles passed straight without any deflection.
? Some of the a-particles were deflected by small angles.
? One out of 12000 particles bounced back after hitting the gold foil.
Inference or Conclusion –
? Most of the space in an atom is empty because most of the a-particles passed without deflection.
? Very few a-particles deflected with small angle indicating that the positive charge in an atom occupied
very less space.
? A very a-particles bounced back with an angle of 180
0
indicating that most of the positive charge and
mass of an atom is concentrated in a very small volume within the atom.
Fig. Rutherford’s a-particles scattering experiment.
Structure of Atom according to Rutherford –
? Nearly all the mass is concentrated in a positively charged nucleus which is present in the center of the
atom.
? The electrons revolve around the nucleus in well-defined orbits.
? The size of the nucleus is very small as compared to the size of an atom. Most of the space in an atom is
empty.
Drawback
? A particle in circular motion always undergoes acceleration. During acceleration a charged particle
radiates energy. Hence, an electron revolving around the nucleus will keep on radiating energy, keep
coming closer to the nucleus and finally fall into it
? It will make an atom highly stable.
? However, as we know that atom is quite stable but cannot be explained by Rutherford’s model.
Bohr’s Model of an atom
Postulates of Neil Bohr
? Electrons revolve only on discrete or special fixed orbits around the nucleus, in an atom.
? Electrons do not radiate energy while revolving.
? These orbits are called energy levels and are denoted as K, L, M, N ………. or n = 1,2, 3, 4 . . . . ..
? An electron can lose energy to move into a lower energy level while it can gain energy and move into
higher energy shell.
Fig. Neil Bohr’s model of Atom
Number of Electrons in different shells:
? The maximum number a shell can have is given by a formula 2n
2
.
? The maximum number of electrons that can be accommodated in the last shell is 8.
? Only if the inner shells are filled, electrons can be accommodated in an outer shell.
Example –
Atomic number or carbon is 6
It means carbon has 6 protons and 6 electrons.
No. of electrons in K shell = 2n
2
For K shell n = 1 and hence no. of electrons in K shell = 2*1
2
= 2
Maximum No. of electrons left = 6-2 = 4
Maximum No. of electrons that can be accommodated in L shell = 2*2
2
= 8
Hence, the remaining 4 electrons will come in L shell.
Fig. Structure of Carbon Atom
Valency
The number of electrons required or need to be reduced (whichever is less) to completely fill the outer most shell is called
the valency of an element.
For e.g.
1. Carbon
Atomic number of carbon is 6
There are 2 electrons in K shell and 4 electrons in L shell but L shall can have 8 electrons.
4 electrons can either be added or removed to completely fill the outermost shell.
Hence, the valency of carbon is 4.
2. Sodium
Atomic number of carbon is 11
There are 2 electrons in K shell and 8 electrons in L shell and 1 in M shell.
M is the outer most shell and can have a maximum of 8 electrons.
So, if 1 electron is removed sodium will be left with 8 electrons in the outermost shell that is L and it will be
completely filled.
Hence, its valency is 1
Electronic configuration
It is the method of representation of the number of electrons in each shell of an atom
E.g. Atomic number of Sodium is 11
Electronic configuration = 2, 8, 1 (Because there are 2, 8 and 1 electrons in K, L and M shell respectively)
Atomic number of Oxygen is 8
Electronic configuration = 2, 6
Atomic Number
Number of protons present in the nucleus of an atom is known as its atomic number.
It is denoted by ‘Z’.
Atomic Mass
Total number protons and neutrons in an atom is known as atomic mass.
It is denoted by ‘A’
Notation or representing atomic mass and number of an element
O
H Atomic no. 1; mass no 1
H Atomic no. 1 mass no. 3
H Atomic no. 1 mass no. 2
Cl Atomic no. 17; mass no 35
Cl Atomic no. 17; mass no 37
Mass number
Symbol of Element
Atomic Number
A
Element
Z
For example:
16
8
Isotopes
Atoms of an element having same atomic number but different mass number are known as isotopes.
E.g.
1. There are 3 isotopes of hydrogen
Protium –
1
1
Deutrium
2
1
Tritium
3
1
There are two isotopes of Chlorine
35
And
37
17 17
Calculating the Mass number of elements with isotopes:
It is calculated using the average percentage of those isotopes present on Earth:
For example – 75% of the chlorine present is Isotope 35 and 25% is isotope 37
Average atomic mass of chlorine = 35*75 + 37*25
100 100
= 105 + 37
4 4
= 35.5u
Applications of Isotopes:
? An isotope of uranium is used as nuclear fuel.
? An isotope of cobalt is used to treat cancer.
? An isotope of iodine is used to treat goiter.
? Radioactive isotopes of an element are used are markers in molecular biology experiments.
Isobars
Elements have different atomic number but different atomic mass are known as isobars.
E.g. Calcium and Argon both have the atomic mass of 40. The atomic number of Calcium is 20 while that of Argon is 18.
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FAQs on Chapter 4 Structure of Atom - Class 9
| 1. What is the structure of an atom? |  |
Ans. The structure of an atom consists of a positively charged nucleus at the center, which contains protons and neutrons, surrounded by negatively charged electrons in different energy levels or shells.
| 2. How are electrons arranged in an atom? | |
Ans. Electrons are arranged in different energy levels or shells around the nucleus of an atom. The first shell can hold a maximum of 2 electrons, the second shell can hold a maximum of 8 electrons, and so on. Electrons occupy the shells based on their energy levels, with the innermost shell being filled first.
| 3. What are the subatomic particles present in an atom? | |
Ans. The subatomic particles present in an atom are protons, neutrons, and electrons. Protons carry a positive charge, neutrons carry no charge (neutral), and electrons carry a negative charge.
| 4. How do protons, neutrons, and electrons contribute to the overall charge of an atom? | |
Ans. Protons carry a positive charge, and electrons carry a negative charge. Neutrons, on the other hand, are neutral and do not contribute to the overall charge of an atom. The number of protons and electrons in an atom is usually equal, resulting in a neutral overall charge.
| 5. What is the significance of the structure of an atom? | |
Ans. The structure of an atom is significant because it determines the chemical properties and behavior of an element. The arrangement of electrons in different energy levels influences how atoms bond with each other to form molecules and compounds. Understanding the structure of an atom is crucial for understanding the behavior of matter at the atomic level.
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