{"id":31539,"date":"2026-05-21T16:27:06","date_gmt":"2026-05-21T10:57:06","guid":{"rendered":"https:\/\/mycbseguide.com\/blog\/?p=31539"},"modified":"2026-05-21T16:27:43","modified_gmt":"2026-05-21T10:57:43","slug":"journey-inside-the-atom-ncert-solutions-class-9-science-exploration","status":"publish","type":"post","link":"https:\/\/mycbseguide.com\/blog\/journey-inside-the-atom-ncert-solutions-class-9-science-exploration\/","title":{"rendered":"Journey Inside the Atom – NCERT Solutions Class 9 Science Exploration"},"content":{"rendered":"\n

Journey Inside the Atom – NCERT Solutions Class 9 Science Exploration includes all the questions with solutions given in NCERT Class 9 Science Exploration<\/a> textbook.<\/p>\n\n\n\n

NCERT Solutions Class 9<\/h2>\n\n\nEnglish Kaveri<\/a>\n\n\nHindi Ganga<\/a>\n\n\nSanskrit Sharada<\/a>\n\n\nMaths Ganita Manjari<\/a>\n\n\nScience Exploration<\/a>\n\n\nSocial Understanding Society<\/a>\n\n\n\n

Journey Inside the Atom \u2013 NCERT Solutions<\/h2>\n\n\n\n
\n\n\n\n

Q.1: Are atoms the smallest indivisible particles?<\/strong><\/p>\n\n\n\n

Solution: No, atoms are not the smallest indivisible particles. According to modern atomic theory, atoms are made up of smaller subatomic particles such as electrons, protons, and neutrons.<\/p>\n\n\n\n

Experiments like J.J. Thomson’s cathode ray experiment and Ernest Rutherford’s gold foil experiment proved that atoms can be divided into smaller parts.<\/p>\n\n\n\n

Hence, atoms are divisible and have an internal structure.<\/p>\n\n\n\n

\n\n\n\n

Q.2: Why do electrons not fall into the nucleus even though they are attracted to protons in it?<\/strong><\/p>\n\n\n\n

Solution: Electrons do not fall into the nucleus because they revolve in fixed energy levels (shells) around the nucleus.<\/p>\n\n\n\n

According to Bohr’s Model of the Atom, each electron has a definite amount of energy. While moving in these orbits, electrons do not lose energy, so they do not spiral into the nucleus despite the electrostatic attraction between electrons and protons.<\/p>\n\n\n\n

\n\n\n\n

Q.3: Why did scientists keep modifying atomic models?<\/strong><\/p>\n\n\n\n

Solution: Scientists kept modifying atomic models because new experimental results were not explained by earlier models.<\/p>\n\n\n\n

For example, Thomson’s atomic model could not explain the results of Rutherford’s gold foil experiment. Hence, a new model was proposed.<\/p>\n\n\n\n

Thus, atomic models were revised to better explain observations and experimental evidence.<\/p>\n\n\n\n

\n\n\n\n

Q.4: Suppose you made up your own \u2018atom\u2019, as Thomson described, using clay for the positive charge and small beads for the electrons spread through it. What will happen if<\/strong>:<\/p>\n\n\n\n

    \n
  1. the positive charge on the clay is lesser than the total negative charge of the beads?<\/li>\n\n\n\n
  2. by mistake, the clay itself carries a bit of negative charge? Would your model still represent a neutral atom?<\/li>\n<\/ol>\n\n\n\n

    Solution:<\/p>\n\n\n\n

      \n
    1. If the positive charge on the clay is less than the total negative charge of the beads, then the atom will not be neutral. It will have a net negative charge.<\/li>\n\n\n\n
    2. If the clay itself carries a bit of negative charge, then the total negative charge increases further. Hence, the model will again not represent a neutral atom.<\/li>\n<\/ol>\n\n\n\n

      Thus, in both cases, the atom will not be neutral because the total positive and negative charges are not equal.<\/p>\n\n\n\n

      \n\n\n\n

      Q.5: Could an orange or a lemon, which also contain seeds inside soft pulp, be a good comparison? In what ways does it match Thomson\u2019s idea and where does it fall short?<\/strong><\/p>\n\n\n\n

      Solution: An orange or a lemon can be compared to Thomson’s atomic model to some extent. The soft pulp of the fruit may be considered as the positively charged sphere, and the seeds embedded in it can be compared to electrons. In this way, the comparison matches Thomson\u2019s idea that electrons are embedded in a positively charged medium.<\/p>\n\n\n\n

      However, this comparison is not completely accurate. In an atom, the positive charge is uniformly distributed and electrons are spread evenly throughout, whereas in an orange or lemon, the seeds are not uniformly distributed and are present only in limited numbers. Also, the pulp of the fruit does not actually possess positive charge.<\/p>\n\n\n\n

      Thus, the orange or lemon model only partially represents Thomson\u2019s atomic model and falls short in explaining the actual structure of an atom.<\/p>\n\n\n\n

      \n\n\n\n

      Q.6: Why did Thomson conclude that electrons are present in all atoms?<\/strong><\/p>\n\n\n\n

      Solution: J. J. Thomson concluded that electrons are present in all atoms based on his cathode ray experiments. He observed that the nature of cathode rays remained the same regardless of the type of gas taken in the discharge tube or the material of the electrodes.<\/p>\n\n\n\n

      This showed that electrons are common constituents of all atoms. Thus, he concluded that electrons are present in every atom.<\/p>\n\n\n\n

      \n\n\n\n

      Q.7: What do you think would happen if {tex}\\alpha{\/tex}-particles were replaced with negatively charged particles in Rutherford\u2019s gold foil experiment?<\/strong><\/p>\n\n\n\n

      Solution: If \u03b1-particles were replaced with negatively charged particles (electrons) in Rutherford’s gold foil experiment, the results would be different.<\/p>\n\n\n\n

      Since electrons are negatively charged, they would be strongly attracted towards the positively charged nucleus. As a result, they would not pass straight through or be deflected slightly; instead, most of them would be pulled towards the nucleus.<\/p>\n\n\n\n

      Thus, the experiment would not show large-angle deflections as observed with \u03b1-particles, and it would not lead to the same conclusions about the structure of the atom.<\/p>\n\n\n\n

      \n\n\n\n

      Q.8: Rutherford found that a few \u03b1-particles bounced back sharply. How does this single surprising result completely rule out Thomson\u2019s \u02bbplum pudding model\u02bc of the atom?<\/strong><\/p>\n\n\n\n

      Solution: In Rutherford’s gold foil experiment, a few \u03b1-particles were found to bounce back sharply. This showed that a very small region of the atom contains a large amount of positive charge and mass.<\/p>\n\n\n\n

      According to Thomson’s atomic model, the positive charge is spread uniformly throughout the atom. If this were true, \u03b1-particles would only be slightly deflected and none would bounce back.<\/p>\n\n\n\n

      The observation of large-angle deflection (bouncing back) proved that the positive charge is concentrated in a small dense nucleus. Hence, Thomson\u2019s model was completely ruled out.<\/p>\n\n\n\n

      \n\n\n\n

      Q.9: If you could ask Rutherford one question about his work, what would it be?<\/strong><\/p>\n\n\n\n

      Solution: If I could ask Ernest Rutherford one question, it would be:<\/p>\n\n\n\n

      \u201cHow are electrons arranged around the nucleus so that they do not fall into it despite the strong electrostatic attraction?\u201d<\/p>\n\n\n\n

      \n\n\n\n

      Q.10: Assertion (A):<\/strong> Rutherford concluded that most of the mass of an atom is concentrated in a small region at the centre called the nucleus.<\/p>\n\n\n\n

      Reason (R):<\/strong> According to Thomson\u2019s model, electrons are embedded in a uniformly distributed positive charge sphere.<\/p>\n\n\n\n

      Options:
      (1) Both A and R are true and R is the correct explanation of A.
      (2) Both A and R are true but R is not the correct explanation of A. \u2705
      (3) A is true but R is false.
      (4) A is false but R is true.<\/p>\n\n\n\n

      Explanation: Assertion (A)<\/strong> is true. Ernest Rutherford concluded that most of the mass of an atom is concentrated in a small central region called the nucleus.
      Reason (R)<\/strong> is also true. According to Thomson’s atomic model, electrons are embedded in a uniformly distributed positive charge sphere.<\/p>\n\n\n\n

      However, Reason (R) is not the correct explanation of Assertion (A).<\/strong><\/p>\n\n\n\n

      \n\n\n\n

      Q.11: Imagine you are a scientist who has discovered a new element. Name this element after yourself and justify that the symbol you have chosen follows the IUPAC rules<\/strong>.<\/p>\n\n\n\n

      Solution: Suppose I discover a new element and name it Rudrium<\/strong>. I would assign it the symbol Rd<\/strong>.<\/p>\n\n\n\n

      According to International Union of Pure and Applied Chemistry rules, the symbol of an element is derived from its name, consisting of one or two letters. The first letter is always written in uppercase and the second letter, if any, is written in lowercase.<\/p>\n\n\n\n

      The symbol Rd<\/strong> follows these rules, as it is taken from the name Rudrium, with \u2018R\u2019 in uppercase and \u2018d\u2019 in lowercase. Hence, it is a valid symbol.<\/p>\n\n\n\n

      \n\n\n\n

      Q.12: What problems could arise if every scientist used different symbols for the same element?<\/strong><\/p>\n\n\n\n

      Solution: If every scientist used different symbols for the same element, it would create confusion and misunderstanding in scientific communication. Scientists from different places would not be able to understand each other\u2019s work easily.<\/p>\n\n\n\n

      This would make it difficult to study, write chemical formulas, and share knowledge globally. Therefore, standard symbols given by International Union of Pure and Applied Chemistry are necessary for uniformity and clarity.<\/p>\n\n\n\n

      \n\n\n\n

      Q.13: An atom with an atomic number of 26 has 56 nucleons. Find out its number of electrons, protons and neutrons.<\/strong><\/p>\n\n\n\n

      Solution: Given:
      Atomic number = 26
      Mass number (nucleons) = 56<\/p>\n\n\n\n

      Number of protons = Atomic number = 26
      Number of electrons = 26 (for a neutral atom)
      Number of neutrons = Mass number – Atomic number = 56 – 26 = 30<\/p>\n\n\n\n

      Thus,<\/strong>
      Protons = 26
      Electrons = 26
      Neutrons = 30<\/p>\n\n\n\n

      \n\n\n\n

      Q.14: The nucleus of an atom contains 20 protons. If its mass number is 41, find the number of neutrons in it.<\/strong><\/p>\n\n\n\n

      Solution: Given:
      Number of protons = 20
      Mass number = 41<\/p>\n\n\n\n

      Number of neutrons = Mass number – Number of protons = 41 – 20 = 21<\/p>\n\n\n\n

      Thus, number of neutrons = 21<\/strong><\/p>\n\n\n\n

      \n\n\n\n

      Q.15: An atom has 18 neutrons and an atomic number of 17. What is its mass number?<\/strong><\/p>\n\n\n\n

      Solution: Given:
      Atomic number = 17
      Number of neutrons = 18<\/p>\n\n\n\n

      Mass number = Number of protons + Number of neutrons
      = 17 + 18 = 35<\/p>\n\n\n\n

      Thus, mass number = 35<\/strong><\/p>\n\n\n\n

      \n\n\n\n

      Q.16: An atom 23<\/sup>A has 11 electrons. Find the number of neutrons in it.<\/strong><\/p>\n\n\n\n

      Solution: Given:
      Atom = 23<\/sup>A
      Number of electrons = 11<\/p>\n\n\n\n

      For a neutral atom, number of electrons = number of protons = atomic number = 11<\/p>\n\n\n\n

      Mass number = 23<\/p>\n\n\n\n

      Number of neutrons = Mass number – Atomic number = 23 – 11 = 12<\/p>\n\n\n\n

      Thus, number of neutrons = 12<\/strong><\/p>\n\n\n\n

      \n\n\n\n

      Q.17: Identify the number of electrons in the outermost shell of the following elements:<\/strong><\/p>\n\n\n\n

        \n
      1. {tex}{ }_6^{12} {C}{\/tex}<\/li>\n\n\n\n
      2. {tex}{ }_9^{19} {~F}{\/tex}<\/li>\n\n\n\n
      3. {tex}{ }_{14}^{28} {Si}{\/tex}<\/li>\n<\/ol>\n\n\n\n

        Solution:<\/p>\n\n\n\n

          \n
        1. Carbon\u00a0{tex}{ }_6^{12} {C}{\/tex}
          Electronic configuration: 2, 4
          Outermost shell electrons = 4<\/li>\n\n\n\n
        2. Fluorine\u00a0{tex}{ }_9^{19} {~F}{\/tex}
          Electronic configuration: 2, 7
          Outermost shell electrons = 7<\/li>\n\n\n\n
        3. Silicon\u00a0{tex}{ }_{14}^{28} {Si}{\/tex}
          Electronic configuration: 2, 8, 4
          Outermost shell electrons = 4<\/li>\n<\/ol>\n\n\n\n
          \n\n\n\n

          Q.18: Write the electronic configuration of the elements having atomic numbers 12, 16 and 18.<\/strong><\/p>\n\n\n\n

          Solution:<\/p>\n\n\n\n

          Atomic number 12:<\/strong> Electronic configuration = 2, 8, 2<\/p>\n\n\n\n

          Atomic number 16:<\/strong> Electronic configuration = 2, 8, 6<\/p>\n\n\n\n

          Atomic number 18:<\/strong> Electronic configuration = 2, 8, 8<\/p>\n\n\n\n

          \n\n\n\n

          Q.19: Solve this riddle: I am an atom with a mass number of 23 and 11 protons. I am a soft metal and react vigorously with water. Who am I and how many neutrons do I have? You can also create one such ridd<\/strong>le.<\/p>\n\n\n\n

          Solution: Given:
          Mass number = 23
          Number of protons = 11<\/p>\n\n\n\n

          Element with atomic number 11 is Sodium (Na), which is a soft metal and reacts vigorously with water.<\/p>\n\n\n\n

          Number of neutrons = Mass number – Atomic number = 23 – 11 = 12<\/p>\n\n\n\n

          Thus, the element is Sodium (Na) and it has 12 neutrons.<\/p>\n\n\n\n

          Created riddle:<\/strong>
          I am an atom with atomic number 17. I am a pale yellow, highly reactive gas used in disinfectants. Who am I, and what is my electronic configuration?<\/p>\n\n\n\n

          Answer:<\/strong> Chlorine (Cl), electronic configuration = 2, 8, 7<\/p>\n\n\n\n

          \n\n\n\n

          Q.20: Two different atoms have 11 protons each, but one has 12 neutrons, and the other has 13 neutrons. How do their atomic numbers and mass numbers compare? Are they the same element or different elements?<\/strong><\/p>\n\n\n\n

          Solution: Both atoms have 11 protons, so their atomic number is the same, i.e., 11.<\/p>\n\n\n\n

          First atom:
          Mass number = 11 + 12 = 23<\/p>\n\n\n\n

          Second atom:
          Mass number = 11 + 13 = 24<\/p>\n\n\n\n

          Since atomic number is the same, both atoms are of the same element. They are isotopes of the same element (sodium).<\/p>\n\n\n\n

          \n\n\n\n

          Q.21: If a bromine atom is available in the form of, say two isotopes, {tex}{ }_{35}^{79} {Br}(49.7 \\%){\/tex} and {tex}{ }_{35}^{81} {Br}(50.3 \\%){\/tex}, calculate the average atomic mass of the bromine atom.<\/strong><\/p>\n\n\n\n

          Solution: Average atomic mass of bromine {tex}={\/tex}<\/p>\n\n\n\n

          {tex}(79 \\times 49.7 \\%)+(81 \\times 50.3 \\%){\/tex}
          {tex}=79 \\times 0.497+81 \\times 0.503{\/tex}
          {tex}=39.263+40.743{\/tex}
          {tex}=80.006 \\text { u } \\approx 80.01 \\text { u }{\/tex}<\/p>\n\n\n\n

          Thus, the average atomic mass of bromine is 80.01 u.<\/p>\n\n\n\n

          \n\n\n\n

          Q.22: Choose the correct options and explain the reason for the correct and incorrect options in the context of Ernest Rutherford\u2019s gold foil experiment:<\/strong><\/p>\n\n\n\n

            \n
          1. The experiment clearly showed the existence of neutrons in the nucleus.<\/li>\n\n\n\n
          2. The results disproved the plum pudding model and led to the idea of a nucleus at the centre of the atom.<\/li>\n\n\n\n
          3. The large deflection of a few alpha particles indicated that most of the mass of the atom and positive charge are packed into a tiny centre.<\/li>\n\n\n\n
          4. The way alpha particles were deflected showed that electrons move around the nucleus.<\/li>\n<\/ol>\n\n\n\n

            Options:
            (1) Statements a and b are correct.
            (2) Statements b and c are correct. \u2705
            (3) Statements c and d are correct.
            (4) Statements d and a are correct.<\/p>\n\n\n\n

            Explanation:<\/p>\n\n\n\n

              \n
            1. Incorrect – Rutherford’s gold foil experiment did not show the existence of neutrons. Neutrons were discovered later by Chadwick.<\/li>\n\n\n\n
            2. Correct – The results disproved Thomson’s atomic model and led to the conclusion that most of the atom is empty space with a small, dense, positively charged nucleus at the centre.<\/li>\n\n\n\n
            3. Correct – The large deflection of a few alpha particles showed that most of the mass and all positive charge of the atom are concentrated in a very small central nucleus.<\/li>\n\n\n\n
            4. Incorrect – The experiment did not provide direct evidence for electrons moving around the nucleus; this idea was developed later in Bohr\u2019s model.<\/li>\n<\/ol>\n\n\n\n
              \n\n\n\n

              Q.23: Which of the following statements are correct or incorrect according to the Bohr\u2019s atomic model? Give a reason for each statement<\/strong>.<\/p>\n\n\n\n

                \n
              1. Electrons lose energy while moving in fixed orbits and slowly fall into the nucleus.<\/li>\n\n\n\n
              2. Electrons can exist anywhere around the nucleus with no fixed energy.<\/li>\n\n\n\n
              3. Electrons revolve around the nucleus in orbits of fixed energy without losing energy.<\/li>\n\n\n\n
              4. Electrons can be found between energy levels as they move around the nucleus.<\/li>\n<\/ol>\n\n\n\n

                Solution:<\/p>\n\n\n\n

                  \n
                1. Electrons lose energy while moving in fixed orbits and slowly fall into the nucleus.
                  Incorrect – Electrons in fixed orbits do not lose energy; hence they do not fall into the nucleus.<\/li>\n\n\n\n
                2. Electrons can exist anywhere around the nucleus with no fixed energy.
                  Incorrect – Electrons occupy only fixed energy levels and cannot exist anywhere randomly.<\/li>\n\n\n\n
                3. Electrons revolve around the nucleus in orbits of fixed energy without losing energy.
                  Correct – This is a postulate of Bohr\u2019s model.<\/li>\n\n\n\n
                4. Electrons can be found between energy levels as they move around the nucleus.
                  Incorrect – Electrons cannot exist between energy levels; they jump between fixed orbits only by absorbing or emitting energy.<\/li>\n<\/ol>\n\n\n\n
                  \n\n\n\n

                  Q.24: The composition of the nuclei of three atomic species X, Y, and Z are given as follows<\/strong>.<\/p>\n\n\n\n

                   <\/td>{tex}{X}{\/tex}<\/td>{tex}{Y}{\/tex}<\/td>{tex}{Z}{\/tex}<\/td><\/tr>
                  Number of protons<\/td>18<\/td>17<\/td>17<\/td><\/tr>
                  Number of neutrons<\/td>19<\/td>18<\/td>20<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

                  Explain the relation between the following:<\/p>\n\n\n\n

                    \n
                  1. Y and Z<\/li>\n\n\n\n
                  2. Z and X<\/li>\n<\/ol>\n\n\n\n

                    Solution:<\/p>\n\n\n\n

                      \n
                    1. Y and Z Both Y and Z have the same number of protons (17), but different number of neutrons (18 and 20). Therefore, they have the same atomic number but different mass numbers. Hence, Y and Z are isotopes of the same element (chlorine).<\/li>\n\n\n\n
                    2. Z and X
                      Z has 17 protons while X has 18 protons. Since their atomic numbers are different, they are atoms of different elements. Therefore, Z and X are different elements.<\/li>\n<\/ol>\n\n\n\n
                      \n\n\n\n

                      Q.25: What conclusion did Rutherford draw about the position and characteristics of the atom\u2019s positively charged part based on the few alpha particles that bounced back or were deflected at large angles in the gold foil experiment?<\/strong><\/p>\n\n\n\n

                      Solution: Based on the Rutherford’s gold foil experiment, Ernest Rutherford concluded that the positively charged part of the atom is located at the centre of the atom in a very small, dense region called the nucleus.<\/p>\n\n\n\n

                      Since only a few alpha particles were deflected or bounced back, it showed that the nucleus is extremely small compared to the size of the atom, but it contains most of the positive charge and mass of the atom.<\/p>\n\n\n\n

                      \n\n\n\n

                      Q.26: Explain and arrange the following statements in the correct chronological order to show how atomic models have evolved over time.<\/strong><\/p>\n\n\n\n

                        \n
                      1. Bohr\u2019s model proposed that electrons move in fixed orbits around the nucleus, each with a definite energy.<\/li>\n\n\n\n
                      2. Thomson\u2019s model depicted the atom as a \u02bbplum pudding\u02bc with electrons embedded in a sphere of positive charge.<\/li>\n\n\n\n
                      3. Rutherford\u2019s model proposed that atoms have a dense central nucleus.<\/li>\n\n\n\n
                      4. Dalton\u2019s model described atoms as indivisible particles.<\/li>\n<\/ol>\n\n\n\n

                        Solution: Dalton \u2192 Thomson \u2192 Rutherford \u2192 Bohr<\/p>\n\n\n\n

                          \n
                        1. John Dalton described atoms as indivisible particles.<\/li>\n\n\n\n
                        2. J. J. Thomson proposed the \u2018plum pudding\u2019 model in which electrons are embedded in a positively charged sphere.<\/li>\n\n\n\n
                        3. Ernest Rutherford proposed that atoms have a small, dense, positively charged nucleus at the centre.<\/li>\n\n\n\n
                        4. Bohr’s Model of the Atom stated that electrons move in fixed orbits around the nucleus, each with definite energy.<\/li>\n<\/ol>\n\n\n\n
                          \n\n\n\n

                          Q.27: Electrons move around the nucleus in orbits. Why do they not fly away from the atom? Explain what keeps them attracted to the nucleus<\/strong>.<\/p>\n\n\n\n

                          Solution: Electrons do not fly away from the atom because they are held by the strong electrostatic force of attraction between the negatively charged electrons and the positively charged nucleus.<\/p>\n\n\n\n

                          According to Bohr’s Model of the Atom, electrons revolve around the nucleus in fixed energy levels, and the attraction between opposite charges keeps them bound to the nucleus, preventing them from escaping the atom.<\/p>\n\n\n\n

                          \n\n\n\n

                          Q.28: Assertion\u2009(A):\u2009<\/strong>\u2009The discovery of subatomic particles helped in understanding the atomic structure.
                          Reason (R): <\/strong>The number of electrons is equal to the number of protons in an atom.<\/p>\n\n\n\n

                          Options:
                          (1) Both A and R are true and R is the correct explanation of A.
                          (2) Both A and R are true but R is not the correct explanation of A. \u2705
                          (3) A is true but R is false.
                          (4) A is false but R is true.<\/p>\n\n\n\n

                          Explanation:<\/p>\n\n\n\n

                          Assertion (A)<\/strong> is true because the discovery of subatomic particles like electrons, protons, and neutrons helped scientists understand the internal structure of the atom.<\/p>\n\n\n\n

                          Reason (R) <\/strong>is also true because in a neutral atom, the number of electrons is equal to the number of protons. However, this statement does not explain how the discovery of subatomic particles helped in understanding atomic structure.<\/p>\n\n\n\n

                          \n\n\n\n

                          Q.29: Magnesium is essential for many biological processes, including muscle contraction. For an atom of magnesium with a mass number of 24 and atomic number 12, determine the number of (i) protons, (ii) neutrons, (iii) electrons, and also illustrate the arrangement of electrons in a magnesium atom.<\/strong><\/p>\n\n\n\n

                          Solution: Given:
                          Mass number = 24
                          Atomic number = 12<\/p>\n\n\n\n

                            \n
                          1. Number of protons = Atomic number = 12<\/strong><\/li>\n\n\n\n
                          2. Number of neutrons = Mass number – Atomic number = 24 – 12 = 12<\/strong><\/li>\n\n\n\n
                          3. Number of electrons = 12 (for a neutral atom) = 12<\/strong><\/li>\n<\/ol>\n\n\n\n

                            Electronic arrangement:
                            Electrons are arranged as 2, 8, 2<\/p>\n\n\n\n

                            Thus, magnesium atom has 12 protons, 12 neutrons, 12 electrons and electronic configuration 2, 8, 2.<\/p>\n\n\n\n

                            \n\n\n\n

                            Q.30: Find the following information for the elements shown in the figure:<\/strong>
                            <\/p>\n\n\n\n

                              \n
                            1. Name of the element<\/li>\n\n\n\n
                            2. Symbol<\/li>\n\n\n\n
                            3. Total number of electrons<\/li>\n\n\n\n
                            4. Number of valence electrons<\/li>\n\n\n\n
                            5. Valency of the element<\/li>\n\n\n\n
                            6. Number of protons<\/li>\n\n\n\n
                            7. Atomic number<\/li>\n<\/ol>\n\n\n\n

                              Solution:<\/p>\n\n\n\n

                                \n
                                1. Name of element: Lithium<\/strong><\/li>
                                2. Symbol: Li<\/strong><\/li>
                                3. Total electrons: 3<\/strong><\/li>
                                4. Valence electrons: 1<\/strong><\/li>
                                5. Valency: 1<\/strong><\/li>
                                6. Number of protons: 3<\/strong><\/li>
                                7. Atomic number: 3<\/strong><\/li><\/ol>
                                  1. Name of element: Carbon<\/strong><\/li>
                                  2. Symbol: C<\/strong><\/li>
                                  3. Total electrons: 6<\/strong><\/li>
                                  4. Valence electrons: 4<\/strong><\/li>
                                  5. Valency: 4<\/strong><\/li>
                                  6. Number of protons: 6<\/strong><\/li>
                                  7. Atomic number: 6<\/strong><\/li><\/ol>
                                    1. Name of element: Magnesium<\/strong><\/li>
                                    2. Symbol: Mg<\/strong><\/li>
                                    3. Total electrons: 12<\/strong><\/li>
                                    4. Valence electrons: 2<\/strong><\/li>
                                    5. Valency: 2<\/strong><\/li>
                                    6. Number of protons: 12<\/strong><\/li>
                                    7. Atomic number: 12<\/strong><\/li><\/ol>\n
                                        \n
                                      1. Name of element: Fluorine<\/strong><\/li>\n\n\n\n
                                      2. Symbol: F<\/strong><\/li>\n\n\n\n
                                      3. Total electrons: 9<\/strong><\/li>\n\n\n\n
                                      4. Valence electrons: 7<\/strong><\/li>\n\n\n\n
                                      5. Valency: 1<\/strong><\/li>\n\n\n\n
                                      6. Number of protons: 9<\/strong><\/li>\n\n\n\n
                                      7. Atomic number: 9<\/strong><\/li>\n<\/ol>\n<\/li>\n<\/ol>\n\n\n\n
                                        \n\n\n\n

                                        Q.31: Both Rutherford\u2019s and Bohr\u2019s models have electrons orbiting the nucleus. Why did Rutherford\u2019s model fail to explain atomic stability, while Bohr\u2019s model succeeded?<\/strong><\/p>\n\n\n\n

                                        Solution: Rutherford\u2019s model failed to explain atomic stability because, according to classical physics, an electron moving in a circular orbit around the nucleus should continuously radiate energy. As a result, it would lose energy, slow down, and eventually spiral into the nucleus. This would make the atom unstable, which contradicts the fact that atoms are stable.<\/p>\n\n\n\n

                                        Bohr improved this model by proposing that electrons revolve in fixed energy levels (stationary orbits) where they do not radiate energy. Radiation is emitted or absorbed only when an electron jumps between these fixed orbits. Hence, Bohr\u2019s model successfully explained atomic stability.<\/p>\n\n\n\n

                                        \n\n\n\n

                                        Q.32: An atom 70<\/sup>\u2009X has 31 electrons. How many neutrons are there in its nucleus?<\/strong><\/p>\n\n\n\n

                                        Solution: Given:
                                        Mass number (A) = 70
                                        Number of electrons = 31<\/p>\n\n\n\n

                                        For a neutral atom:
                                        Number of protons = Number of electrons = 31<\/p>\n\n\n\n

                                        Now,
                                        Mass number = Protons + Neutrons<\/p>\n\n\n\n

                                        So,
                                        Neutrons = 70 – 31 = 39<\/strong><\/p>\n\n\n\n

                                        \n\n\n\n

                                        Q.33: An atom has 79 protons and a mass number of 197. Calculate (i) the number of neutrons, and (ii) the number of electrons.<\/strong><\/p>\n\n\n\n

                                        Solution: Given:
                                        Number of protons {tex}=79{\/tex}
                                        Mass number {tex}(A)=197{\/tex}<\/p>\n\n\n\n

                                          \n
                                        1. Number of neutrons: Mass number {tex}={\/tex} Protons + Neutrons
                                          Neutrons {tex}=197-79=118{\/tex}<\/li>\n\n\n\n
                                        2. Number of electrons: For a neutral atom:
                                          Electrons {tex}={\/tex} Protons {tex}=79{\/tex}<\/li>\n<\/ol>\n\n\n\n
                                          \n\n\n\n

                                          Q.34: Complete the Table.<\/strong><\/p>\n\n\n\n

                                          Atomic number<\/strong><\/td>Mass number<\/strong><\/td>Number of neutrons<\/strong><\/td>Number of protons<\/strong><\/td>Number of electrons<\/strong><\/td>Name of the elements<\/strong><\/td><\/tr>
                                          5<\/td>____<\/td>6<\/td>____<\/td>____<\/td>____<\/td><\/tr>
                                          ____<\/td>14<\/td>____<\/td>____<\/td>7<\/td>Nitrogen<\/td><\/tr>
                                          ____<\/td>24<\/td>____<\/td>12<\/td>____<\/td>____<\/td><\/tr>
                                          15<\/td>____<\/td>16<\/td>____<\/td>____<\/td>____<\/td><\/tr>
                                          ____<\/td>1<\/td>0<\/td>____<\/td>____<\/td>____<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

                                          Solution:<\/p>\n\n\n\n

                                          Atomic number<\/strong><\/td>Mass number<\/strong><\/td>Number of neutrons<\/strong><\/td>Number of protons<\/strong><\/td>Number of electrons<\/strong><\/td>Name of the elements<\/strong><\/td><\/tr>
                                          5<\/td>11<\/td>6<\/td>5<\/td>5<\/td>Boron<\/td><\/tr>
                                          7<\/td>14<\/td>7<\/td>7<\/td>7<\/td>Nitrogen<\/td><\/tr>
                                          12<\/td>24<\/td>12<\/td>12<\/td>12<\/td>Magnesium<\/td><\/tr>
                                          15<\/td>31<\/td>16<\/td>15<\/td>15<\/td>Phosphorus<\/td><\/tr>
                                          1<\/td>1<\/td>0<\/td>1<\/td>1<\/td>Hydrogen<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n
                                          \n\n\n\n

                                          Q.35: Aman was discussing the structure of atom with his classmates. During the discussion, he learnt that an element X has a mass number of 35 and contains 18 neutrons. Based on this information, answer the following questions:<\/strong><\/p>\n\n\n\n

                                            \n
                                          1. How many electrons and protons does element X have?<\/li>\n\n\n\n
                                          2. What is its atomic number?<\/li>\n\n\n\n
                                          3. Identify the element X.<\/li>\n\n\n\n
                                          4. Write its electronic configuration.<\/li>\n\n\n\n
                                          5. How many valence electrons does it have?<\/li>\n\n\n\n
                                          6. What will be the mass number if two neutrons are added to its nucleus?<\/li>\n\n\n\n
                                          7. What will be the relation of X with the new atom?<\/li>\n<\/ol>\n\n\n\n

                                            Solution: Given:
                                            Mass number {tex}({A})=35{\/tex}
                                            Neutrons {tex}=18{\/tex}<\/p>\n\n\n\n

                                              \n
                                            1. Electrons and protons<\/strong> Protons {tex}={A}-{\/tex} Neutrons {tex}=35-18=17{\/tex}
                                              For a neutral atom:
                                              Electrons = Protons = 17<\/li>\n\n\n\n
                                            2. Atomic number<\/strong> Atomic number = number of protons = 17<\/li>\n\n\n\n
                                            3. Identify element X<\/strong> Element with atomic number 17 = Chlorine (Cl)<\/li>\n\n\n\n
                                            4. Electronic configuration<\/strong>
                                              {tex}{Cl}({Z}=17) \\rightarrow 2,8,7{\/tex}<\/li>\n\n\n\n
                                            5. Valence electrons<\/strong> Valence electrons = 7<\/li>\n\n\n\n
                                            6. New mass number (after adding 2 neutrons)<\/strong> New mass number = 35 + 2 = 37<\/strong><\/li>\n\n\n\n
                                            7. Relation of X with new atom<\/strong> The new atom will be an isotope of chlorine (same atomic number, different mass number).<\/li>\n<\/ol>\n\n\n\n
                                              \n\n\n\n

                                              Q.36: In an atom, there are 12 protons and 12 neutrons in the nucleus. Now, imagine that all the electrons are replaced with some hypothetical particles that have the same charge as electrons but are 500 times heavier. What effect will this replacement have on the atom\u2019s:<\/strong><\/p>\n\n\n\n

                                                \n
                                              1. Atomic number<\/li>\n\n\n\n
                                              2. Atomic mass<\/li>\n\n\n\n
                                              3. Mass number<\/li>\n\n\n\n
                                              4. Overall charge<\/li>\n<\/ol>\n\n\n\n

                                                Solution: Given:
                                                Protons {tex}=12{\/tex}
                                                Neutrons {tex}=12{\/tex}
                                                Electrons are replaced by heavier particles (same charge, {tex}500 \\times{\/tex} mass)<\/p>\n\n\n\n

                                                  \n
                                                1. Atomic number Atomic number depends only on number of protons.
                                                  So, atomic number = 12 (unchanged)<\/li>\n\n\n\n
                                                2. Atomic mass Atomic mass depends mainly on protons and neutrons.
                                                  Electrons contribute very little in normal case, but now they are heavy, so atomic mass will increase significantly.<\/li>\n\n\n\n
                                                3. Mass number Mass number = protons + neutrons
                                                  = 12 + 12 = 24 (unchanged)<\/li>\n\n\n\n
                                                4. Overall charge Charge depends on protons (+) and electrons (\u2212).
                                                  Since number of electrons is still equal to protons, even though heavier:
                                                  Overall charge = 0 (neutral atom)<\/strong><\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"

                                                  Journey Inside the Atom – NCERT Solutions Class 9 Science Exploration includes all the questions with solutions given in NCERT Class 9 Science Exploration textbook. NCERT Solutions Class 9 Journey Inside the Atom \u2013 NCERT Solutions Q.1: Are atoms the smallest indivisible particles? Solution: No, atoms are not the smallest indivisible particles. According to modern … Read more<\/a><\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[281,2071,2072],"tags":[216],"class_list":["post-31539","post","type-post","status-publish","format-standard","hentry","category-ncert-solutions","category-ncert-solutions-class-9","category-ncert-solutions-class-9-science-exploration","tag-ncert-solutions"],"yoast_head":"\nJourney Inside the Atom - NCERT Solutions Class 9 Science Exploration | myCBSEguide<\/title>\n<meta name=\"description\" content=\"Journey Inside the Atom - NCERT Solutions Class 9 Science Exploration includes all the questions with solutions given in NCERT Class 9\" \/>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/mycbseguide.com\/blog\/journey-inside-the-atom-ncert-solutions-class-9-science-exploration\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Journey Inside the Atom - 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