Courses
Courses for Kids
Free study material
Offline Centres
More
Store Icon
Store

Important Questions for CBSE Class 9 Science Chapter 4 - Structure of the Atom

ffImage
Last updated date: 22nd Mar 2024
Total views: 651.9k
Views today: 10.51k
MVSAT 2024

CBSE Class 9 Science Chapter-4 Important Questions - Free PDF Download

Important Questions for Class 9 Science Chapter 4 the structure of the atom is created by subject matter experts at Vedantu. The main concept behind creating the important questions for the chapter to enable students to prioritize the concepts of chapter introduced in Science Class 9. The important questions of structure of atom Class 9 are prepared to give a better conceptual understanding. With the help of Class 9 Science Chapter 4 important questions, it would be easy to assume the type of questions will be asked in the chapter exam. The language used while preparing the important questions is proficient and understandable by a Class 9 student. Vedantu is a platform that provides free CBSE Solutions (NCERT) and other study materials for students. Maths and Science Students who are looking for the better solutions ,they can download Class 9 Maths NCERT Solutions and Class 9 Science NCERT Solutions to help you to revise complete syllabus and score more marks in your examinations.


Download CBSE Class 9 Science Important Questions 2023-24 PDF

Also, check CBSE Class 9 Science Important Questions for other chapters:

CBSE Class 9 Science Important Questions

Sl.No

Chapter No

Chapter Name

1

Chapter 1

Matter in Our Surroundings

2

Chapter 2

Is Matter Around Us Pure

3

Chapter 3

Atoms and Molecules

4

Chapter 4

Structure of Atom

5

Chapter 5

The Fundamental Unit of Life

6

Chapter 6

Tissues

7

Chapter 7

Diversity in Living Organisms

8

Chapter 8

Motion

9

Chapter 9

Force and Laws of Motion

10

Chapter 10

Gravitation

11

Chapter 11

Work and Energy

12

Chapter 12

Sound

13

Chapter 13

Why Do We Fall ill

14

Chapter 14

Natural Resources

15

Chapter 15

Improvement in Food Resources

 

Important Topics Covered In Class 9 Science Chapter 4 - Structure of the Atom

The following is a list of some of the important topics and subtopics that students will come across while studying Chapter 4 - Structure of the Atom. Students are advised to ensure that they have covered all these topics while preparing for the exam as questions are likely to be asked from them.

  • Introduction

  • Charged Particles In Matter

  • The Structure of An Atom

  • The Thomson's Model of An Atom

  • Rutherford's Model of An Atom

  • Drawbacks of Rutherford's Model of An Atom

  • Bohr’s Model of An Atom

  • Neutrons

  • How Are Electrons Distributed In Different Orbits?

  • Valency

  • Atomic Number And Mass Numbers

  • Isotopes

  • Isobars

Popular Vedantu Learning Centres Near You
centre-image
Mithanpura, Muzaffarpur
location-imgVedantu Learning Centre, 2nd Floor, Ugra Tara Complex, Club Rd, opposite Grand Mall, Mahammadpur Kazi, Mithanpura, Muzaffarpur, Bihar 842002
Visit Centre
centre-image
Anna Nagar, Chennai
location-imgVedantu Learning Centre, Plot No. Y - 217, Plot No 4617, 2nd Ave, Y Block, Anna Nagar, Chennai, Tamil Nadu 600040
Visit Centre
centre-image
Velachery, Chennai
location-imgVedantu Learning Centre, 3rd Floor, ASV Crown Plaza, No.391, Velachery - Tambaram Main Rd, Velachery, Chennai, Tamil Nadu 600042
Visit Centre
centre-image
Tambaram, Chennai
location-imgComing soon in Tambaram, Chennai
Visit Centre
centre-image
Avadi, Chennai
location-imgVedantu Learning Centre, Ayyappa Enterprises - No: 308 / A CTH Road Avadi, Chennai - 600054
Visit Centre
centre-image
Deeksha Vidyanagar, Bangalore
location-imgSri Venkateshwara Pre-University College, NH 7, Vidyanagar, Bengaluru International Airport Road, Bengaluru, Karnataka 562157
Visit Centre
View More
Watch videos on
Important Questions for CBSE Class 9 Science Chapter 4 - Structure of the Atom
icon
Structure of the Atom in One Shot | CBSE Class 9 Science Chapter 4 NCERT Solutions | Vedantu
Vedantu 9&10
Subscribe
iconShare
6.2K likes
239.8K Views
3 years ago
Download Notes

Study Important Questions for Class 9 Science Chapter 4 – Structure of Atoms

Very Short Answer Questions (1 Mark)

1. What are canal rays?

Ans: Positively charged rays discovered by E. Goldstein are called canal rays.


2. If an atom contains one electron and one proton, will it carry any charge or not?

Ans: A single electron contains one negative charge and one single proton contains one positive charge so they are neutralized by each other. That atom will not contain any charge.


3. Name the three sub-atomic particles of an atom.

Ans: Three subatomic particles of an atom are Proton, Neutron and Electron.


4. Rutherford’s alpha-particle scattering experiment was responsible for the discovery of

  1.  Atomic Nucleus

  2.  Electron

  3.  Proton 

  4.  Neutron

Ans: (d) Proton


5. Isotopes of an element have

  1.  The same physical properties

  2.  Different chemical properties

  3.  Different number of neutrons

  4.  Different atomic numbers

Ans: (a) The same physical properties.


6. Number of valence electrons in $C{{l}^{-}}$ ion are:

  1.  16

  2.  8

  3.  17

  4.  18

Ans: (b) 8


7. Which one of the following is a correct electronic configuration of sodium?

  1.  2,8

  2.  8,2,1

  3.  2,1,8

  4.  2,8,1

Ans: (b) 2,8


8. Atomic Number of an element is equal to:

  1.  Number of Protons

  2.  Number of electrons

  3.  Number of neutrons

  4.  Both (a) and (b)

Ans: (a) Number of Protons


9. The charge of proton $({{p}^{+}})$ is:

  1. $+1.6\times {{10}^{-19}}C$ 

  2. $-1.6\times {{10}^{-19}}C$

  3. $+1.6\times {{10}^{19}}C$

  4. $-1.6\times {{10}^{19}}C$

Ans: (a) $+1.6\times {{10}^{-19}}C$


 10. ${}_{10}^{20}Ne$ and ${}_{10}^{22}Ne$ are

  1.  Isotopes

  2.  Isobars

  3.  Isotones

  4.  Both (a) and (b)

Ans: (a) Isotopes


 11. Helium $\left( {}_{2}^{4}He \right)$ has:

  1.  $2P+$ and $2n{}^\circ $

  2.  $2P+$ and $4n{}^\circ $

  3.  $4P+$ and $2n{}^\circ $

  4.  $2P+$ and $4n{}^\circ $

Ans: (a) $2P+$ and $2n{}^\circ $


 12. In which form is oxygen available?

  1.  ${{O}^{2-}}$ 

  2.  ${{O}^{2+}}$

  3.  $O$

  4.  Both (a) and (c)

Ans: (a) ${{O}^{2+}}$


 13. How many electrons does $N{{a}^{+}}$ has in its outermost shell?

  1.  10

  2.  11

  3.  18

  4.  8

Ans: (d) 8 


 14. Atomic number of an element during a Chemical reaction.

  1.  Increases

  2.  Remain Constant

  3.  Decreases

  4.  May be (a) or (c)

Ans: (b) Remain constant


 15. The molecular formula for Aluminum chloride is 

  1.  $A{{l}_{3}}Cl$

  2.  $AlC{{l}_{3}}$

  3.  $AlC{{l}_{3}}$ 

  4.  Both (b) and (c)

Ans: (c) $AlC{{l}_{3}}$


 16. Atomicity of fluorine is:

  1.  1

  2.  2

  3.  3

  4.  4

Ans: (b) 2


 17. Molecular formula for calcium fluoride is-

  1. $Ca{{F}_{2}}$ 

  2.  $CaF$

  3.  $C{{a}_{2}}F$

  4.  $2CaF$

Ans: (a) $Ca{{F}_{2}}$


 18. Electronic configuration of calcium is

  1.  2,8,8,2

  2.  2,8,6,4

  3.  2,8,7,1

  4.  2,8,1,7

Ans: (a) 2,8,8,2


 19. Nitrogen is:

  1.  Monatomic

  2.  Diatomic

  3.  Triatomic

  4.  Tetratomic

Ans: (b) Diatomic


Short Answer Question (2 Marks)

1. On the basis of Thomson’s model of an atom, explain how the atom is neutral as a whole.

Ans: As per Thomson’s model of an atom, the number of electrons and the number of protons are equal in an atom. Electrons are positively charged and protons are negatively charged, hence the + and – charges are neutralized by each other that makes atoms neutral as a whole.


2. On the basis of Rutherford’s model of an atom, which subatomic particle is present in the nucleus of an atom?

Ans: The subatomic particle proton is present in the nucleus of an atom according to Rutherford’s model of an atom.


3. Draw a sketch of Bohr’s model of an atom with three shells.

Ans: Bohr’s model of an atom with three shells is as follows:


Sketch of Bohr’s Mode


4. What do you think would be the observation if the $\alpha -$ particle scattering experiment is carried out using a foil of a metal other than gold?

Ans: If the $\alpha -$ particle scattering experiment is carried out using a foil of a metal other than gold we will get a different observation. 


5. Helium atom has an atomic mass of 4 u and two protons in its nucleus. How many neutrons does it have?

Ans: The atomic mass of an atom is the sum of masses of protons and neutrons present in its nucleus.

Given that the mass of the helium atom is 4 u and two protons present in its nucleus.

So the number of neutrons will be

$\text{Number of neutrons = atomic mass }-\text{ number of protons}$ 

$\Rightarrow \text{Number of neutrons = 4}-2$

$\therefore \text{Number of neutrons = }2$

Therefore, the helium atom has 2 neutrons.


6. Write the distribution of electrons in carbon and sodium atoms.

Ans: Atomic number of carbon is 6 and the atomic number of sodium is 11.

So distribution of electrons in carbon atom is 6 = 2,4

Distribution of electrons in the sodium atom is 11 = 2,8,1.


7. If K and L shells of an atom are full, then what would be the total number of electrons in the atom?

Ans: K shell contains total 2 electrons and L shell contains maximum 8 electrons. If K and L shells of an atom are full, then the total number of electrons in the atom will be 10.


8. If number of electrons in an atom is 8 and number of protons is also 8, then

  1. What is the atomic number of the atom? 

Ans: The atomic number of an atom is equal to the number of protons or electrons present in its nucleus. So the atomic number of an atom with 8 electrons and 8 protons is 8.


  1. What is the charge on the atom?

Ans: A single electron contains one negative charge and one single proton contains one positive charge. There are equal numbers of electrons and protons in an atom so they neutralize each other. The atom will be neutral.


9. With the help of Table 4.1, find out the mass number of oxygen and Sulphur atoms.

Ans: The mass number of an atom is equal to the sum of protons and neutrons present in its nucleus. 

\[Mass\text{ }number\text{ }of\text{ }oxygen=8+8\] 

\[Mass\text{ }number\text{ }of\text{ }oxygen=16\] 

\[Mass\text{ }number\text{ }of\text{ Sulphur}=16+16\] 

\[Mass\text{ }number\text{ }of\text{ Sulphur}=32\]


10. What are the limitations of J.J. Thomson’s model of the atom?

Ans: The J.J. Thomson’s atomic model failed to explain the organization of electrons in an atom.


11. $N{{a}^{+}}$ has completely filled K and L shells. Explain.

Ans: Sodium $(Na)$ has atomic number 11, so the electronic configuration of $Na$ is 2,8,1.

It has a single electron in the outermost shell, when it gives away that electron it becomes $N{{a}^{+}}$ and has electronic configuration 2,8. Also the K shell contains a total 2 electrons and the L shell contains a maximum of 8 electrons. So $N{{a}^{+}}$ has completely filled K and L shells.


12. If $z=3$, what would be the valency of the element? Also, name the element.

Ans: $z=3$ represents that element has 3 electrons in its shells. The electronic configuration is 2,1. It means the outermost shell electron has 1 electron, so its valency is 1. The element is Lithium.

 Composition of the nuclei of two atomic species X and Y are given as under


X

Y

Protons

6

6

Neutrons

6

8


13. Give the mass number of X and Y. What is the relation between the two species?

Ans: The mass number of an atom is equal to the sum of protons and neutrons present in its nucleus.

So the mass number of X is $=6+6=12$ 

Mass number of Y is $=6+8=14$ 

Number of protons is the same in X and Y but the atomic numbers are different. X and Y are isotopes.

 For the following statements, write T for True and F for False.

  1.  J.J. Thomson proposed that the nucleus of an atom contains only nucleons.

Ans: False

  1.  A neutron is formed by an electron and a proton combining together. Therefore, it is neutral.

Ans: True

  1. The mass of an electron is about 12000 times that of proton.

Ans: True

  1.  An isotope of iodine is used for making tincture iodine, which is used as a medicine.

Ans: False


14. The nucleus of an atom of Bi – 210 (atomic number = 83) emits $\beta -$ particle and becomes a polonium nuclide. Write as equation for the nuclear change described.

Ans: Whenever a $\beta -$particle emits from the nucleus of an atom, the atomic number of that atom is increased by 1 but the mass number remains the same.

So when a $\beta -$particle emits from Bi – 210 (atomic number = 83) it becomes polonium nuclide. The equation for the nuclear change is as follows:

${}_{83}^{210}Bi\to {}_{84}^{210}Po+{}_{-1}^{0}e$.


16. How can one conclude that electrons are fundamental particles?

Ans: The $\dfrac{e}{m}$ ratio of electrons remains similar irrespective of the nature of gas and electrodes inside the discharge tube. So we can conclude that electrons are fundamental particles.


17. What happens to the nucleus of an atom when it emits a $\gamma -$ ray?

Ans: There is no change in mass or charge of nuclide when it emits $\gamma -$ ray. The energy of the nucleus decreases equal to the energy of photons emitted.


 18. Write the electronic configuration of following ions:

  1.  $C{{l}^{-}}$ 

Ans: Electronic configuration of $C{{l}^{-}}$ ion is 2,8,8.

  1.  $Mg$

Ans: Electronic configuration of $Mg$ion is 2,8,2.

  1.  $A{{l}^{3+}}$

Ans: Electronic configuration of $A{{l}^{3+}}$ ion is 2,8.

  1.  $O$ 

Ans: Electronic configuration of $O$ is 2,6.


19. State Mendeleev’s periodic law? 

Ans: Mendeleev’s Periodic law states that the properties of elements are periodic functions of their atomic mass. Properties of elements depend on the atomic mass.


20. Define ionization energy and electron affinity?

Ans: Ionization energy of a component is that the amount of energy that has got to be supplied to at least one mole of the element within the gaseous state to get one mole of caters within the gaseous state.

Electron affinity point is that the energy change that accompanies the formation of 1 mole of anions within the gaseous state from one mole of the atoms of the element within the gaseous state.


21. Why is atomic number is more important than atomic weight in predicting the chemical properties of elements?

Ans: Atomic number is that the number of protons in an atom and through a reaction the number of protons remains unchanged. Atomic number also gives number of electrons. Electrons are present in shells which participate in chemical reactions and decide chemical properties. Whereas relative atomic mass is the sum of the number of protons and number of neutrons so the number is more important in predicting the chemical properties of elements.


 22. What are the advantages of the Periodic Table?

Ans: In periodic table elements are arranged in a tabular form. So it is easy to remember the properties of elements if the position is known. Also the compounds formed by the elements are predictable if the position of the element is known. Periodic table made it easy and systematic to study chemistry.


 23. Which of the following electronic configuration are wrong and why?

  1.  2,8,2

  2.  2,8,8,2

  3. 2,8,9,1.

Ans: From the given electronic configuration, 2,8,9,1 is wrong because in the third shell the maximum number of electrons is 8. The correct electronic configuration is 2,8,8,2.


24. What are ions? What are its two types?

Ans: When one or more electrons are detached from a neutral atom, a positively charged particle is formed and called an ion. Ions may be cations and anions.


25. Show diagrammatically the formation of ${{O}^{2-}}$ ion?

Ans: Atomic number of oxygen is 8 and its electronic configuration is 2,6. In the outermost shell oxygen has 6 electrons. To complete its octet and become stable it needs 2 electrons. By gaining 2 electrons it becomes ${{O}^{2-}}$ ion.

Diagrammatic representation of formation of ${{O}^{2-}}$ ion is as follows:


Diagrammatic representation of formation of o2ー


26. Define isotopes and isobars?

Ans: Isotopes are atoms which have identical atomic numbers but different mass numbers. Examples of isotopes are ${}_{6}^{12}C,{}_{6}^{14}C$.

Isobars are atoms that have different atomic numbers but the same mass number. Examples of isobars are ${}_{18}^{40}Ar,{}_{19}^{40}K$.


Short Answer Questions (3 Marks)

27. For the symbol H, D and T tabulate three subatomic particles found in each of them.

Ans: H represents the hydrogen atom, D represents the deuterium atom and T represents the tritium atom. Three subatomic particles present in each of them is represented as follows:

Symbol

Number of electrons

Number of protons

Number of neutrons

H (hydrogen)

1

1

0

D (deuterium)

1

1

1

T (tritium)

1

1

2


28. Write the electronic configuration of any one pair of isotopes and isobars.

Ans: Electronic configuration of pairs of isotopes of carbon is ${}_{6}^{12}C,{}_{6}^{14}C$. Isotopes have the same number of electrons and protons.

Electronic configuration of a pair of isobars of argon and calcium is ${}_{18}^{40}Ar,{}_{20}^{40}Ca$.


29. Compare the properties of electrons, protons and neutrons.

Ans: Comparison of electrons, protons and neutrons is as follows:

Protons

Neutrons

Electrons

Protons are positively charged.

Mass of a proton is equal to one hydrogen atom i.e. 1 a.m.u.

Protons are present in the nucleus of an atom.

Neutrons are neutral (no charge).

Mass of a neutron is equal to a proton.

Neutron is present inside the nucleus of an atom. 

Electrons are negatively charged.

Mass of an electron is equal to \[\dfrac{1}{1838}\] of the mass of a proton.

Electrons are present outside the nucleus of an atom.


30. What are the limitations of Rutherford’s model of the atom?

Ans: Rutherford’s model of atom is failed to explain the stability of atom because as per his model electrons revolve around the nucleus and while moving through orbit should emit energy and this energy loss will shrink the orbit and finally the electron would hit the nucleus and thus atom is unstable but it is not true.


31. Define valency by taking examples of silicon and oxygen.

Ans: The valency of electrons is determined by electrons present in the outermost shell of an atom. Electrons present in the outermost shell of an atom are known as the valence electrons. Electrons gain or lose electrons to complete its octet. The valency of silicon is 14 and electronic configuration is 2,8,4. So silicon can gain or lose 4 electrons. So the valency of silicon is +4 or -4.

Atomic number of oxygen is 8 and the electronic configuration is 2,6. To complete its octet oxygen gains 2 electrons hence the valency of oxygen is 2.


32. If bromine atom is available in the form of, say, two isotopes ${}_{35}^{79}Br(49.7%)$ and ${}_{35}^{81}Br(50.3%)$, Calculate the average atomic mass of bromine atom.

Ans: The average atomic mass of bromine is 

$=\dfrac{79\times 49.7+81\times 50.3}{100}$ 

$=\dfrac{3926.3+4074.3}{100}$ 

$=\dfrac{8000.6}{100}$ 

$=80u$ 

Average atomic mass of bromine atoms is 80 u.


33. The average atomic mass of a sample of an element X is 16.2 u. What are the percentages of isotopes ${}_{8}^{16}X$ ${}_{8}^{18}X$ and in the sample?

Ans: Average atomic mass of sample is given as

$\dfrac{16X+18\times \left( 100-X \right)}{100}$ 

We get

 $\Rightarrow 16.2=\dfrac{16X+18\times \left( 100-X \right)}{100}$

$\Rightarrow 1620=-2X+1800$

$\Rightarrow 2X=1800-1620$

$\Rightarrow 2X=180$

$\therefore X=90$ 

The percentage of isotopes is ${}_{8}^{16}X(90%)$ and ${}_{8}^{18}X(10%)$.


34. In a gold – foil experiment:

  1. Why did many $\alpha -$ particles pass through the gold foil undeflected?

Ans: Most of the space within the atom was empty so many $\alpha -$ particles passed through the gold foil undeflected.

  1. Why did few $\alpha -$ particles deflect through small angles.

Ans: In a gold foil at center there is a positive charge so few $\alpha -$ particles deflect through small angles.

  1. Why did few $\alpha -$ particles, after striking the gold foil, retrace their path.

Ans: In a gold foil there is a positively charged nucleus which is very tiny so few $\alpha -$ particles, after striking the gold foil, retrace their path.

  1.  Compare the three major particles in atoms with respect to their mass and charge?

Ans: Comparison of three major particles proton, neutron and electron with respect to their mass and charge is as follows:


Particles

Symbol

Mass

Charge 

1

Proton

${{P}^{+}}$ 

$1836\left( 9.1\times {{10}^{-31}} \right)Kg$ 

$+1.6\times {{10}^{-19}}C$ 

2

Neutron

${{N}^{0}}$ 

$1836\left( 9.1\times {{10}^{-31}} \right)Kg$

$0$ 

3

Electron

${{e}^{-}}$ 

$9.1\times {{10}^{-31}}Kg$

$-1.6\times {{10}^{-19}}C$


Inside an atom electron revolves around the nucleus in a circular path. Protons and neutrons are present inside the nucleus.

35. Write an experiment to show cathode rays are deflected by magnetic fields?

Ans: Experiment to show that cathode rays were deflected by magnetic fields is as follows:

  • First take a discharge tube with fluorescent material inside it.

  • Place a horse – shoe magnet in the center of the discharge tube.

  • When cathode rays are produced and travel through the discharge tube, then cathode rays get deflected by the magnetic field of the magnets in the direction of anode. Also they are negatively charged.

The diagram of experiment is as follows:


Experimental setup to show cathode rays are deflected by magnetic fields


36. Write the postulates of Bohr theory?

Ans: The postulate of Bohr’s theory is as follows:

  • An electron revolves around the nucleus in the orbit of an atom in a definite path known as orbits or shells.

  • Energy of each orbit is fixed.

  • Energy increases from inner shell to the outer shells i.e. energy for orbit nearest the nucleus is lowest.

  • If energy is supplied then the electron moves from lower orbit to higher orbit.


37. Explain the variation of atomic radius along a period and down a group.

Ans: The atomic radius of an atom increases when we move down as an extra shell is added. The atomic radius decreases when we move from left to right as the nuclear charge of an element increases.


38. Why metals are electropositive and non-metals are electronegative in nature?

Ans: Metals are electropositive in nature because all metals give away electrons from their outermost shell in order to complete the octet and become stable. So metals become positively charged. Non-metals are electronegative in nature because all non-metals gain electrons in order to complete the octet and become stable. So non-metals become negatively charged.


39. Explain the formation of $A{{l}^{3+}}$ ion and why is it formed?

Ans: Aluminum has an atomic number of 13. The electronic configuration of Al is 2,8,3. It has 3 electrons in the outermost shell and to become stable it needs to complete its octet. In the outermost shell, the maximum number of electrons must be 8. So it is easy to lose 3 electrons and complete the octet. By giving away the 3 outermost electrons it becomes  $A{{l}^{3+}}$ ion.


Formation of Al3+


40. Find the percentage composition of sucrose $\left( {{C}_{12}}{{H}_{22}}{{O}_{11}} \right)$.

Ans: The molecular mass of sucrose $\left( {{C}_{12}}{{H}_{22}}{{O}_{11}} \right)$ is

$\left( {{C}_{12}}{{H}_{22}}{{O}_{11}} \right)=12\times 12+22+11\times 16$

$\left( {{C}_{12}}{{H}_{22}}{{O}_{11}} \right)=144+22+176$

$\left( {{C}_{12}}{{H}_{22}}{{O}_{11}} \right)=342g/mol$

342 g of sucrose contains 144g Carbon, 22 g Hydrogen and 176 g Oxygen.

So 100 g sucrose contains:

$C=\dfrac{100\times 144}{342}=42.11g$ 

\[H=\dfrac{100\times 22}{342}=6.43g\]

$O=\dfrac{100\times 176}{342}=51.46g$

So the percentage composition of sucrose is

$C=42.11%$ 

$H=6.43%$ 

$O=51.46%$.


41. Complete the following table:


Ion

Number of electrons

Z

N

A


${}^{86}R{{b}^{+}}_{37}$ 






${}^{24}M{{g}^{2+}}_{12}$






${}^{80}B{{r}^{-}}_{35}$






Ans: In the given table element is represented as ${}_{Z}^{A}X$.

Here, X is the symbol of element,

Z is the symbol of atomic number which is equal to number of protons,

A is the symbol of mass number which is equal to the sum of the number of protons and the number of neutrons.

By using above information we get the complete table as:


Ion

Number of electrons

Z

N

A


${}^{86}R{{b}^{+}}_{37}$ 

36

37

49

86


${}^{24}M{{g}^{2+}}_{12}$

10

12

12

24


${}^{80}B{{r}^{-}}_{35}$

36

35

45

80


  1.  Calculate the following:

  1.  The number of gram – atoms of oxygen

Ans: Oxygen atoms are represented as ${{O}_{2}}$.  In oxygen 2 gram atoms are present.


  1.  The number of atom of oxygen

Ans: Gram atomic mass of oxygen is $6.023\times {{10}^{23}}atoms$.

16 g of oxygen has $6.023\times {{10}^{23}}atoms$.

So 32 g of oxygen has $\dfrac{6.023\times {{10}^{23}}\times 32}{16}=1.205\times {{10}^{24}}atoms$. 


  1. The number of molecules in 32 g of ozone $\left[ {{O}_{3}} \right]$.

Ans: We know that 48 g of ozone contains $6.023\times {{10}^{23}}molecules$.

So 1 g of ozone contains \[\dfrac{6.023\times {{10}^{23}}}{48}\] molecules.

Thus 32 g of ozone has \[\dfrac{6.023\times {{10}^{23}}\times 32}{48}=4.015\times {{10}^{23}}molecules.\]


  1.  What mass of water will contain the same number of molecules as 8.0 g of ferrous oxide [FeO]?

Ans: We know that the atomic mass of 18 g of water is $6.023\times {{10}^{23}}atoms$.

Ferrous oxide is $56+16=72g$ 

So the atomic mass of 72 g of FeO is $6.023\times {{10}^{23}}atoms$.

Now, 1 g of FeO is \[=\dfrac{6.023\times {{10}^{23}}}{72}\] 

Also, 8 g of FeO is \[=\dfrac{6.023\times {{10}^{23}}\times 8}{72}\].

8 g of FeO is \[=0.669\times {{10}^{23}}\].

Now, 18 g of water is $6.023\times {{10}^{23}}atoms$.

So we get

$\dfrac{18}{6.023\times {{10}^{23}}}gms=1\text{ }atom$ 

$\Rightarrow \dfrac{18\times 0.669\times {{10}^{23}}}{6.023\times {{10}^{23}}}gms=0.669\times {{10}^{23}}\text{ }atoms$

Therefore, 2g of water contains \[=0.669\times {{10}^{23}}\].

So 2g of water will contain the same number of molecules as 8 g of ferrous oxide.


Long Answer Questions (5 Marks)

42. How will you find the valency of chlorine, Sulphur and magnesium?

Ans: The valency of electrons is determined by electrons present in the outermost shell of an atom. Electrons present in the outermost shell of an atom are known as the valence electrons. Those electrons determine the valency of that atom.

The atomic number of chlorine is 17 and the electronic configuration is 2,8,7.

Thus chlorine has 7 electrons in the outermost shell and to complete its octet it needs 1 more electron. So the valency of chlorine is one.

The atomic number of Sulphur is 16 and the electronic configuration is 2,8,6.

Thus Sulphur has 6 electrons in the outermost shell and to complete its octet it needs 2 more electrons. So the valency of Sulphur is two.

The atomic number of Magnesium is 12 and the electronic configuration is 2,8,2.

Thus Magnesium has 2 electrons in the outermost shell. It is easy to give away two valence electrons. So the valency of Magnesium is two.


43. Describe Bohr’s model of the atom.

Ans: There are some drawbacks in Rutherford’s atomic model. So to overcome this and to explain the structure of atoms in detail Neil Bohr in 1912 proposed a model of atoms. The postulates of Bohr’s model are given below:

  • An electron revolves around the nucleus in the orbit of an atom with fixed energy.

  • Energy of orbits increases from inner shell to the outer shells i.e. energy for orbit nearest the nucleus is lowest.

  • If energy is supplied then the electron moves from lower orbit to the higher orbit and if an electron jumps from higher orbit (energy level) to the lower orbit (energy level) then energy is emitted as electromagnetic waves.

  • Each orbit or shell represents an energy level by an integer number as n=1,2,3,….  Such orbits are characterized as K,L,M,N……….. and titled from nucleus side to outwards.


44. Compare all the proposed models of an atom given in this chapter.

Ans: There are three proposed models of an atom are discussed in detail i.e. Thomson’s model, Rutherford’s model and Bohr’s model.

The comparison between the three is given below:

Thomson’s model

Rutherford’s model

Bohr’s model

According to Thomson's model, an atom has negatively charged electrons in a positively charged sphere. So the atom as a whole is neutral as negative and positive charges are equal in magnitude.

This model fails to explain the stability of an atom.

This model explains that there is a nucleus in the center of an atom and electrons revolve around that nucleus.

The arrangement of electrons is not explained in this model thus it seems to be incomplete.

According to Bohr’s model electrons revolve around the nucleus in a specific path known as orbits or shells with a fixed energy.

An electron has complete atomic shells thus the atom becomes more stable.


45. Summarize the rules for writing of distribution of electrons in various shells for the first eighteen elements.

Ans: The following rules are followed for writing the number of electrons in different energy levels or shells:

  • The maximum number of electrons existing in a shell is given by the formula $2{{n}^{2}}$, where ‘n’ is the orbit number or energy level and is equal to 1,2,3,…

  • Hence the maximum number of electrons in different shells are as follows:

In the first orbit or also known as K-shell it will be $2\times {{1}^{2}}=2$ (n=1).

In the second orbit or also known as L-shell will be $2\times {{2}^{2}}=8$ (n=2).

In the third orbit or also known as M-shell will be $2\times {{3}^{2}}=18$ (n=3) and so on.

  • In the outermost shell the maximum number of electrons can be 8.

  • First inner shells are filled then outer shells are filled. Electrons are not put up in a given shell, unless the inner shells are filled. That


46. Explain following with examples and Give any two uses of isotopes.

  1. Atomic number

Ans: Atomic number of an atom is equal to the number of protons present inside the nucleus of that atom. It is represented by Z.

  1. Mass number

Ans: The atomic mass of an atom is the sum of masses of protons and neutrons present in its nucleus. It is represented by A. For example, the mass number of Carbon is 12 u because it has 6 protons and 6 neutrons in its nucleus.

  1. Isotopes

Ans: Isotopes are atoms which have identical atomic numbers but different mass numbers. Examples of isotopes are ${}_{6}^{12}C,{}_{6}^{14}C$.

  1. Isobars

Ans: Isobars are atoms that have different atomic numbers but the same mass number. Examples of isobars are ${}_{18}^{40}Ar,{}_{19}^{40}K$. Total number of neutrons is the same in the atoms.

Two uses of isotopes are as follows:

  • An isotope of uranium is used in nuclear reactors as a fuel.

  • An isotope of cobalt is used in the treatment of cancer.


47. Complete the following table.

Atomic number

Mass number

Number of neutrons

Number of protons

Number of electrons

Name of the atomic species

9

-

10

-

-

-

16

32

-

-

-

Sulphur

-

24

-

12

-

-

-

2

-

1

-

-

-

1

0

1

0

-


Ans: The complete table is as follows:

Atomic number

Mass number

Number of neutrons

Number of protons

Number of electrons

Name of the atomic species

9

19

10

9

9

Fluorine

16

32

16

16

16

Sulphur

12

24

12

12

12

Magnesium

1

2

1

1

1

Deuterium 

1

1

0

1

0

Hydrogen ion


Chapter 4 Science Class 9 Important Questions

Chapter 4 structure of the atom is the part of atomic physics. Some of the scientists who have greatly contributed to modern atomic theory by finding actual evidence are John Dalton, J.J. Thompson, Ernest Rutherford, Niels Bohr, James Chadwick and Ernest Schrodinger.

Topics covered under the structure of atom Class 9 important questions are charged particles in matter, the structure of an atom, Thomson’s model of an atom, rutherford model of an atom, Bohr’s model of an atom, neutrons, distribution of electrons in different orbits, valency, atomic number,  mass number, isotopes and isobars. In this chapter, we also get to know about the discovery of electrons and protons  J.J. Thomson and E.Goldstein, respectively. From the mentioned topics many different questions can be framed in Class 9 Science Chapter 4 important questions.


Structure of Atom

It consists of three main particles: protons, electrons, and neutrons. The nucleus of the atom contains protons which are positively charged and neutrons with no charge.  The outermost region of the atoms is called an electron shell and contains an electron, which is a negatively charged particle.


Key Benefits of CBSE Class 9 Science Chapter 4 Important Questions

Here are some of the benefits of referring to Class 9 Science Chapter 4 Important Questions:


  1. Awareness of Key Topics: Practising important questions provides a clear understanding of the crucial topics covered in the chapter.


  1. Skill Development: Solving these questions enhances time management and problem-solving skills across all vital topics.


  1. Understanding Question Formats: Students gain insights into the difficulty levels and various question formats that may appear in exams.


  1. Confidence Boost: Repeated practice instills confidence in students, making them more assured in tackling exam questions.


  1. Versatility in Exam Preparation: Students become well-prepared to handle any type of questions that may arise in the exam.

 

Conclusion

Students can find the important question of structure of atom Class 9 on Vedantu, which has been prepared by experts to help students with their annual exam preparation. The correct solution to the important questions is given in the PDF. By this, students can save a lot of time in finding the correct answer for the respective question. To know more about this chapter, download the solution of Class 9 Chapter 4 from our site. Chapter 4 has a good weightage in the final exam. By revising the concepts of Chapter 4, you can achieve almost 10 marks from this chapter.


Important Related Links for CBSE Class 9 

FAQs on Important Questions for CBSE Class 9 Science Chapter 4 - Structure of the Atom

1. What is the structure of an atom according to Chapter 4 of Class 9 Science?

We learned in Chapter 4 of Class 9 Science that an atom is made up of a nucleus surrounded by electrons and a nucleus made up of protons and neutrons. Electrons have a negative charge, while protons have a positive charge, and neutrons have no charge. The electrons are thought to travel in circular orbits of specified radii corresponding to discrete energy states with the nucleus at the centre in a simplified description of the atomic structure based on the Bohr model. The atom may thus be thought of as being made up of circular shells of electrons, with the lowest shell corresponding to the lowest energy state and the higher level shells having more energy.

2. Why are NCERT Solutions of Chapter 4 of Class 9 Science important?

The NCERT Solutions are a must before every examination and they cumulatively cover all the important concepts. All the NCERT based questions follow a certain pattern and they are extremely essential as this pattern is also adhered to in the examination. Make sure you practice all the NCERT Solutions numerous times to get a good understanding of the concept and further, to leave no scope for error in your exams.

3. What is inside the atom according to Chapter 4 of Class 9 Science notes?

There are a couple of components inside an atom according to Chapter 4 of Class 9 Science. Atoms are the fundamental components of matter. The proton, neutron, and electron are the three subatomic particles that make up the smallest unit of matter. Protons, neutrons, and electrons make up the basic structure of an atom. The mass and charge of the atoms are provided by these fundamental components. The proton and neutron make up the nucleus, with the electron circling around it. Students can learn more about this topic from Vedantu and the study material is absolutely free of cost.

4. What is Z in chemistry according to Chapter 4 of Class 9 Science?

The number of protons in the nucleus of every atom of a chemical element is known as the atomic number or proton number which has the symbol Z. A chemical element's atomic number is the only way to identify it and it makes an element unique. It is the same as the nucleus' charge number. The atomic number is also equivalent to the number of electrons in an uncharged atom.

5. What are neutrons in accordance with Chapter 4 of Class 9 Science?

Chadwick found another subatomic particle with a mass almost equal to that of a proton but no charge. It was given the name neutron later on. Except for hydrogen, all atoms have neutrons in their nuclei. In general, a neutron is denoted by the letter ‘n’. The total of the masses of the protons and neutrons in the nucleus determines the mass of an atom. Neutrons are introduced in the Chapter 4 of Class 9 Science and they are explained thoroughly in the NCERT notes.