{"id":8723,"date":"2019-11-26T17:28:19","date_gmt":"2019-11-26T11:58:19","guid":{"rendered":"https:\/\/kseebsolutions.guru\/?p=8723"},"modified":"2021-07-02T15:44:55","modified_gmt":"2021-07-02T10:14:55","slug":"1st-puc-chemistry-question-bank-chapter-2","status":"publish","type":"post","link":"https:\/\/kseebsolutions.guru\/1st-puc-chemistry-question-bank-chapter-2\/","title":{"rendered":"1st PUC Chemistry Question Bank Chapter 2 Structure of Atom"},"content":{"rendered":"

You can Download Chapter 2 Structure of Atom Questions and Answers, Notes, 1st PUC Chemistry Question Bank with Answers<\/a> Karnataka State Board Solutions help you to revise complete Syllabus and score more marks in your examinations.<\/p>\n

Karnataka 1st PUC Chemistry Question Bank Chapter 2 Structure of Atom<\/h2>\n

1st PUC Chemistry Structure of Atom One Mark Questions and Answers<\/h3>\n

Question 1.
\nMention the constituents of atom.
\nAnswer:
\nElectron, Proton & Neutron.<\/p>\n

Question 2.
\nWho discovered electron.
\nAnswer:
\nJ.J. Thomson<\/p>\n

Question 3.
\nWhat is the mass of electron?
\nAnswer:
\n9.108 \u00d7 1031 <\/sup>kg (0.0005487amu).<\/p>\n

Question 4.
\nMention the charge of electron in colomb.
\nAnswer:
\n1.61.6*1019<\/sup>C.<\/p>\n

Question 5.
\nWhat is the charge of proton ?
\nAnswer:
\nPositive charge.<\/p>\n

\"KSEEB<\/p>\n

Question 6.
\nWhat is the mass of proton ?
\nAnswer:
\n1.672 x 1027 <\/sup>kg(1.00728amu)<\/p>\n

Question 7.
\nWho discovered proton ?
\nAnswer:
\nE. Goldstein.<\/p>\n

Question 8.
\nWho invented charge on electron ?
\nAnswer:
\nRobert Millikan.<\/p>\n

Question 9.
\nName the experiment by which charge on electron determined.
\nAnswer:
\nRobert Millikan oil drop experiment.<\/p>\n

\"KSEEB<\/p>\n

Question 10.
\nWho discovered neutron ?
\nAnswer:
\nJames Chadwick.<\/p>\n

Question 11.
\nWhat is atomic number ?
\nAnswer:
\nAtomic number *Z’ is the number of protons present in the nucleus of an atom of an element or the number of electrons present in an atom of an element.<\/p>\n

Question 12.
\nWhat is mass number ?
\nAnswer:
\nAtomic mass ‘A’. The total number of protons and neutrons present in the nucleus of an atom of an element.<\/p>\n

Question 13.
\nWrite the relationship between mass number and atomic number.
\nAnswer:
\nNumber of neutrons = Mass number (A) – Atomic number (Z) = A – Z<\/p>\n

Question 14.
\nHow do you represent an atom symbolically with atomic number and mass number?
\nAnswer:
\nZ<\/sub>XA<\/sup> where A = Mass Number, X = atom, Z = Atomic number.<\/p>\n

Question 15.
\nWhat is the number of proton and neutron in 92<\/sub>X235<\/sup> ?
\nAnswer:
\n\"1st<\/p>\n

Question 16.
\nGive the number of Protons, Electrons and Neutrons present in the atom – having atomic number 27 and mass number 56.
\nAnswer:
\nNumber of Protons 27, Number of Electrons 27, Number of Neturons 29.<\/p>\n

Question 17.
\nMention the proton, neutron and electons 17<\/sub>C35<\/sup>.
\nAnswer:
\nNeutron = 35 – 17 = 18, Electron = Proton = 17 .<\/p>\n

Question 18.
\nName the species which has no electron.
\nAnswer:
\nProton<\/p>\n

\"KSEEB<\/p>\n

Question 19.
\nName the atom which has no neutron.
\nAnswer:
\nHydrogen<\/p>\n

Question 20.
\nWhat is the ratio between mass of proton and electron ?
\nAnswer:
\nMass of proton is 1837 times the mass of electron.<\/p>\n

Question 21.
\nName the particles which constitute cathode rays.
\nAnswer:
\nElectrons<\/p>\n

Question 22.
\nWho demonstrated the particle property of an electron ?
\nAnswer:
\nJ. J. Thomson<\/p>\n

\"KSEEB<\/p>\n

Question 23.
\nWho showed the wave property of electrons ?
\nAnswer:
\nG.P. Thomson<\/p>\n

Question 24.
\nWhat is the charge on neutrons ?
\nAnswer:
\nNil \/ Zero<\/p>\n

Question 25.
\nMention the mass of neutron.
\nAnswer:
\n1.675 \u00d7 1027 <\/sup>kg(1.00866 amu)<\/p>\n

Question 26.
\nName the scientist who proposed the nuclear theory (Solar model of atom) theory and discovered the existence of nucleus of an atom ?
\nAnswer:
\nErnest Rutherford.<\/p>\n

Question 27.
\nWhat is photon ?
\nAnswer:
\nElectromagnetic radiations are emitted or absorbed or propagated in the form of small pockets of energy called photon.<\/p>\n

Question 28.
\nWhat is Isotopes ?
\nAnswer:
\nAtoms of the same element having the same atomic number but different mass numbers are called isotopes.<\/p>\n

Question 29.
\nWhat is Isobars ?
\nAnswer:
\nAtoms of different elements having the same mass number but different atomic numbers are called isobars.<\/p>\n

Question 30.
\nWhat is Isotones ?
\nAnswer:
\nAtoms of different elements which contain the same number of neutrons, but different mass numbers are known as isotones.<\/p>\n

Question 31.
\nDefine the term ‘radiation’
\nAnswer:
\nRadiation is the emission and transmission of energy through space in the form of waves.<\/p>\n

\"KSEEB<\/p>\n

Question 32.
\nHow are velocity, frequency and wavelength of light radiation related ?
\nAnswer:
\n\"1st<\/p>\n

Question 33.
\nState Pauli’s exclusion principles.
\nAnswer:
\nNo two electrons in an atom can have the same set of four quantum numbers.<\/p>\n

Question 34.
\nAn atom having mass number 40 has 20 neutrons in its nucleus. What is the atomic number of the element ?
\nAnswer:
\nMass Number = Number of protons + Number of neutrons
\n40 = Number of protons + 20
\n\u2234Atomic number = Number of protons = 20.<\/p>\n

Question 35.
\nWhat is aufbau principle ?
\nAnswer:
\nAufbau principle is also known as the building up principle. According to this principle, electrons should eneter the subshells in the order of increasing energies.<\/p>\n

Question 36.
\nWhat is emission spectrum ?
\nAnswer:
\nThe spectrum of radiation emitted by a substance that has absorbed energy is called in emission spectrum.<\/p>\n

Question 37.
\nHow is the magnetic moment of paramagnetic species is related to the number of unpaired electrons present in it ?
\nAnswer:
\nMagnetic moment \\(\\mu=\\sqrt{n(n+2) B M}\\) where n is the number of unpaired electrons.<\/p>\n

Question 38.
\nDifferentiate between the terms ‘ground state’ and ‘excited state’.
\nAnswer:
\nGround state means the least energy state or the most stable state. Excited state means the higher energy state, in which the electrons are in the higher energy level (unstable state).<\/p>\n

\"KSEEB<\/p>\n

Question 39.
\nWhat is the expression for the energy of a photon ?
\nAnswer:
\nE = hu where, h = planks constant = 6.626 \u00d7 10-34<\/sup> Js , \u03b3 = frequency or radiation.<\/p>\n

Question 40.
\nWrite the unit for frequency of radiation.
\nAnswer:
\nCycles per sec (sec-1<\/sup>) or Hertz (Hz)<\/p>\n

Question 41.
\nName the experiment which shows that light has particle property.
\nAnswer:
\nPhotoelectric effect.<\/p>\n

Question 42.
\nName the experiment which shows that light has wave property.
\nAnswer:
\nRefraction.<\/p>\n

Question 43.
\nHow is wave number and wavelength of a wave related?
\nAnswer:
\n\"1st<\/p>\n

Question 44.
\nWhat is the velocity of light?
\nAnswer:
\n3 \u00d7 108<\/sup> m\/sec<\/p>\n

\"KSEEB<\/p>\n

Question 45.
\nDefine wavelength.
\nAnswer:
\nIt is the distance between two successive crests (peaks) or trough in a wave.<\/p>\n

Question 46.
\nDefine Wave number.
\nAnswer:
\nIt is the number of waves present per meter and is equal to the reciprocal of wavelength. \\(\\left(\\frac{1}{\\lambda}\\right)=\\bar{v}\\)<\/p>\n

Question 47.
\nDefine frequency of light.
\nAnswer:
\nThe number of waves which pass through a given point in one second is called frequency of light.<\/p>\n

Question 48.
\nWhat type of waves does light constitute?
\nAnswer:
\nElectromagnetic waves.<\/p>\n

Question 49.
\nWhat is orbital (atom orbital) ?
\nAnswer:
\nOrbital is a three dimensional region in space around the nucleus in which the probability of finding an electron is maximum.<\/p>\n

Question 50.
\nHow many electrons can be accommodated in an orbital?
\nAnswer:
\nTwo electrons.<\/p>\n

\"KSEEB<\/p>\n

Question 51.
\nWrite the de Broglie’s equation.
\nAnswer:
\n\\(\\lambda=\\frac{\\mathbf{h}}{\\mathbf{m} \\mathbf{V}}\\) where \u03bb – wavelength of wave, h = Plank’s constant, m = mass of the electron, V – velocity of the electron.<\/p>\n

Question 52.
\nWrite Rydberg’s formula.
\nAnswer:
\n\"1st<\/p>\n

Question 53.
\nWrite the Balmer equation.
\nAnswer:
\n\"1st<\/p>\n

Question 54.
\nWhat are the four prominent lines in Balmer series of hydrogen spectrum ?
\nAnswer:
\nH\u03b1<\/sub>, H\u03b2<\/sub>, H\u03b3<\/sub> and H????<\/sub><\/p>\n

Question 55.
\nWhat is the value of Rydberg’s constant?
\nAnswer:
\n10.97 \u00d7 106 <\/sup>m-1<\/sup><\/p>\n

Question 56.
\nGive the range of wavelengths of visible light.
\nAnswer:
\n400 nm to 750 nm.<\/p>\n

\"KSEEB<\/p>\n

Question 57.
\nGive the Rydberg equation where R is Rydberg constant?
\nAnswer:
\n\"1st<\/p>\n

Question 58.
\nName the element whose atom contain six protons in the nucleus.
\nAnswer:
\nCarbon<\/p>\n

Question 59.
\nName the different series of hydrogen spectrum.
\nAnswer:
\n(i) Lyman
\n(ii) Balmer
\n(iii) Pachen
\n(iv) Bracket
\n(v) Pfund<\/p>\n

Question 60.
\nName two series of hydrogen spectra which fall in the infra – red region.
\nAnswer:
\nBrackett series and P-fund series.<\/p>\n

Question 61.
\nMatch the following:
\n\"1st
\nAnswer:
\na-iii, b-iv, c-ii, d-i<\/p>\n

1st PUC Chemistry Structure of Atom Two Marks Questions and Answers<\/h3>\n

Question 1.
\nWrite the difference between isotope & isobars.
\nAnswer:
\n\"1st<\/p>\n

Question 2
\nExplain Planks quantum theory.
\nAnswer:
\nElectromagnetic radiations are emitted, absorbed and propagated discontinuously in the form of small packet of energy called photon. A body emits (absorbs) radiations in the integral multiples of \u2018photon\u2019.
\nEnergy associated with each photon is E = hv, h = 6.626 \u00d7 10 -34<\/sup> Js<\/p>\n

\"KSEEB<\/p>\n

Question 3.
\nDistinguish between emission spectra & atomic spectra.
\nAnswer:
\nEmission spectra : When an object is strongly heated, it starts to emit light. When the emitted light is subjected to depression, emission spectrum is obtained)
\nAtomic spectra : When an atom of an element is strongly heated, it starts emitting light energy in different region. This emitted light when dispersed, a large number of closely spaced lines where formed they are called atomic spectra.<\/p>\n

Question 4.
\nWhat do you mean by electromagnetic spectra ?
\nAnswer:
\nThe complete range of electromagnetic waves in the increasing order of wavelength (decreasing order of frequency) is known as electromagnetic spectra.<\/p>\n

Question 5.
\nWrite the electromagnetic spectra in the increasing order of wave length. (Decreasing order of frequency)
\nAnswer:
\nIncreasing order of wave length > Cosmic rays > Gamma rays < X-rays < U.V. rays < Visible rays < IR rays < Microwave rays < Radio waves (i.e, decreasing order of frequency).<\/p>\n

Question 6.
\nDeduce the de-Broglies matter wave equation.
\nAnswer:
\nDual nature of electron – de-Broglie\u2019s matter wave equation
\nAccording to Einstein\u2019s mass – energy relation, E = mc2<\/sup> … (1)
\nWhere m and c are the mass and velocity of an electron respectively.
\nAccording to quantum theory, Energy E = hv = (he) \/ \u03bb … (2)
\nWhere h is Plank\u2019s constant = 6.626 \u00d7 10-34<\/sup> Js, u is the frequency of moving electron.
\nComparing(1)and(2)me2 = (hc)\/\u03bb >me = h\/\u03bb > = \u03bb = h \/me … (3)
\nEquation (3) is called de-Broglie\u2019s equation.
\nFor an electron its velocity is given as V, So the de-Broglie\u2019s equation for an electron is given by,
\n\u03bb = h \/ mv (mv = p = momentum of electron)
\n\u03bb = h \/ p is called de-Broglie\u2019s matter – wave equation<\/p>\n

\"KSEEB<\/p>\n

Question 7.
\nExplain the wave nature of light.
\nAnswer:
\nWave nature of light: According to Newton, light is a stream of particles which are also known as corpuscles of light. This could not account for the phenomena of interference and deflection (as Rutherford\u2019s model) but justified reflection and refraction.<\/p>\n

Hygen suggested in his wave theory that the fight travels in the form of waves, later James Maxwell proposed that fight and other radiations are transmitted, these waves are associated with oscillating electric and magnetic field.<\/p>\n

Question 8.
\nDistinguish between particle and wave.
\nAnswer:
\n\"1st<\/p>\n

Question 9.
\nExplain Werner Heisenberg\u2019s uncertainty principle (qualitative)
\nAnswer:
\nIt is impossible to determine both the momentum (particle nature) and position (wave nature) of a moving sub atomic particle simultaneously with absolute accuracy.
\nMathematically \u2206x \u00d7 Ap = h \/ 4\u03c0 where \u2206x = uncertainty in position :
\n\u2206p = uncertainty in momentum ; h = Plank’s constant = 6.626 \u00d7 10-34<\/sup> Js.<\/p>\n

Question 10.
\nMention the Merits of Bohr\u2019s theory.
\nAnswer:<\/p>\n

    \n
  1. Explains the formation of hydrogen spectrums<\/li>\n
  2. It explains the stability of atom<\/li>\n
  3. Ryd berg constant is calculated by it.<\/li>\n<\/ol>\n

    \"KSEEB<\/p>\n

    Question 11.
    \nWrite any two limitations of Bohr’s theorem.
    \nAnswer:<\/p>\n

      \n
    1. Not explained spectra of atoms containing more than one electrons.<\/li>\n
    2. Not explained fine spectra (when spectroscope of high resolving power is used, it is found that each line in the ordinary specrum spilts into number of components differing in frequency).<\/li>\n
    3. Not given explanation regarding Stark effect (spiltting of spectral line in electric field) and Zeeman Effect (splitting of spectral fine in magnetic field).<\/li>\n<\/ol>\n

      Question 12.
      \nWrite the difference between orbit & orbital.
      \nAnswer:
      \n\"1st<\/p>\n

      Question 13.
      \nDraw the structure of p-orbitals. (Draw the shape of orbital whose Azimuthal quantum no is 1).
      \nAnswer:
      \np orbital has 3 orientations px<\/sub>,py<\/sub> &pz<\/sub>
      \n\"1st<\/p>\n

      Question 14.
      \nDraw the structure of d-orbital (Orbital whose Azimuthal quantum no = 2).
      \nAnswer:
      \nd- orbital has 5 orientations.
      \n\"1st<\/p>\n

      \"KSEEB<\/p>\n

      Question 15.
      \nWhat do you mean by electronic configuration ? With the sequence.
      \nAnswer:
      \nElectronic Configuration is the distribution of electrons in the various available orbitals of an atom of an element.
      \nThe sequenced in which the electron occupy the various oribitals is as follows.
      \nIs, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p….<\/p>\n

      Question 16.
      \nExplain the electronic Configuration of cation Fe+.
      \nAnswer:
      \nExample for electronic configuration of cation.
      \n\"1st<\/p>\n

      Question 17.
      \nExplain electronic configuration of anion using N.
      \nAnswer:
      \nExample for electronic configuration of anion.
      \n\"1st<\/p>\n

      Question 18.
      \nState & Explain Paul’s Exclusion Principle.
      \nAnswer:
      \nPaul’s Exculsion principle : No two electrons in the same atom can have all the four quantum numbers same.
      \nIllustration : In Is orbital there are two electrons, the set of quantum number of one electron differ with another in spin quantum number.
      \n\"1st<\/p>\n

      Question 19.
      \nState and explain Hunds Rule of maximum multiplicity.
      \nAnswer:
      \nHund’s rule or maximum multiplicity : Electron pairing does not take place until orbitals of same energy are singly occupied.<\/p>\n

      Question 20.
      \nWhat are quantum number and Name them ?
      \nAnswer:
      \nIn order to define state energy and location of electron a set of four numbers are used.
      \nThese numbers are called quantum numbers.<\/p>\n

        \n
      • Principal quantum number (n)<\/li>\n
      • Azimuthal quantum number (1)<\/li>\n
      • Magnetic quantum number (m)<\/li>\n
      • Spin quantum number (s).<\/li>\n<\/ul>\n

        Question 21.
        \nWrite all quantum number values for 3s orbital electrons.
        \nAnswer:
        \nS – orbital has two electrons.
        \n3s; n = 3; 1 = 0; m = 0; s = + 1\/2 for first electron,
        \nn = 3; 1 = 0; m = 0; s = -1\/2 for second electron.<\/p>\n

        \"KSEEB<\/p>\n

        Question 22.
        \nAn orbital can contain only two electrons. Why ?
        \nAnswer:
        \nAn orbital can have only two electrons, provided these two electrons have anti parallel spins. This arrangement is represented, as \u2193\u2191<\/p>\n

        Question 23.
        \nWrite the atomic number at an element with outer configuration,
        \ni) 4s1, ii) 3d3 .
        \nAnswer:
        \n(i) Electronic configuration for outer configuration 4s1<\/sup> = 1s2<\/sup>. 2s2<\/sup>,2p6<\/sup>, 3s2<\/sup>, 3p6<\/sup>, 4s1<\/sup>.
        \nAtomic number =19
        \n(ii) Exact configuration for outer configuration 3d3.
        \n1s2<\/sup>, 2s2<\/sup>, 2p6<\/sup>, 3s2<\/sup>,3p6<\/sup>, 4s2<\/sup>, 3d3<\/sup> = 23 Atomic number = 23<\/p>\n

        Question 24.
        \nWrite the electronic configuration of
        \n1. Cl–<\/sup> 2. Na+<\/sup> ion
        \nAnswer:
        \nElectronic configuration
        \n1) Cl–<\/sup> = 1s2<\/sup>, 2s2<\/sup>, 2p6<\/sup>, 3s2<\/sup>, 3p6<\/sup>
        \n2) Na+ = 1s2<\/sup>, 2s2<\/sup>, 2p6<\/sup><\/p>\n

        1st PUC Chemistry Structure of Atom Three \/ Four Marks Questions and Answers<\/h3>\n

        Question 1.
        \nSummarize the Bohr’s Model of an atom,
        \nAnswer:
        \nBohr’s Model of an atom, the postulates are<\/p>\n

          \n
        1. Electrons revolve around the nucleus of an atom in a certain definite path called Orbit or stationary state of shell.<\/li>\n
        2. The shells are having different energy levels denoted as K, L, M, N<\/li>\n
        3. As long as the electron remains in an orbit, they neither absorb nor emit energy.<\/li>\n
        4. The electron can move only in that orbit in which angular momentum is quantized, i.e., the angular momentum of the electron is an integral multiple of \\(\\frac{\\mathrm{h}}{2 \\pi}\\)<\/li>\n<\/ol>\n

          \"KSEEB<\/p>\n

          Question 2.
          \nExplain the experimental set up and different series of emission spectrum of hydrogen.
          \nAnswer:
          \nHydrogen Spectrum : Hydrogen spectrum is obtained by exciting electrons present in hydrogen gas using a discharge tube under low pressure and high voltage of current. The electrons present in various atoms of Hydrogen absorb energy and jumps to higher energy levels. Later they return back to the lower energy levels by emitting excess of energy in the form of photons. When these electrons are coming to the lower energy state a series of lines were formed called Hydrogen spectrum. Denoted as H\u03b1<\/sub>,H\u03b2<\/sub>,H\u03b3<\/sub> and H????<\/sub>H\u03b5<\/sub><\/p>\n

            \n
          • Lyman Series : This series is formed when the electron jumps from 2nd, 3rd, 4th, …. Higher energy level to first (K shell) level by emitting excess of energy in UV region.<\/li>\n
          • Baimer Series ; This series is formed when the electron jumps from 3rd, 4th, 5th,… higher energy level to 2nd (L shell) level by emitting excess of energy in visible region.<\/li>\n
          • Paschen Series : This series is formed when the electron jumps from 4th, 5th, 6th higher energy level to 3rd (M Shell) level by emitting excess of energy in Infra Red (IR Region).<\/li>\n
          • Brackett Series : This series is formed when the electron jumps from 5th, 6 th…. higher energy level to 4th (N shell) level by emitting excess of energy in Infra Red (IR) region.<\/li>\n
          • Pfund Series : This series is formed when the electron jumps from 6th, 7th …. higher energy level to 5th (0 shell) level by emitting excess of energy in Infra Red (IR) region.<\/li>\n<\/ul>\n

            Question 3.
            \nWhat is Wave number, Frequency and Amplitude ? Give its SI Units.
            \nAnswer:
            \nWave Number ( \\(\\overrightarrow{\\mathrm{v}}\\) ) : Number of waves per unit length. Units : m-1<\/sup>
            \nFrequency (v) ; Number of wave peaks that pass a given point in time unit.
            \nUnits: Hz
            \nAmplitude (A): Height of the wave above the central line.<\/p>\n

            1st PUC Chemistry Structure of Atom Four \/ Five Marks Questions and Answers<\/h3>\n

            Question 1.
            \nCalculate the wave number, wavelength and frequency first line of hydrogen spectrum Or Calculate the maximum wave length of a line in the Lyman series.
            \nAnswer:
            \nFirst line is Lyman Series, where n1<\/sub> = 1, n2<\/sub> = 2. Maximum wave length corresponds to minimum frequency i.e., n1<\/sub> = 1, n2<\/sub> = 2.
            \n\"1st
            \nR = Rydberg constant = 1.097 \u00d7 10+7<\/sup> m. n1<\/sub> = 1 n2<\/sub> = 2
            \n\"1st
            \nWave length \u03bb = 0.8227 \u00d7 107 = 8.227 \u00d7 106<\/sup> m-1<\/sup>
            \n\"1st<\/p>\n

            \"KSEEB<\/p>\n

            Question 2.
            \nCalculate the limiting frequency of Balmer series.
            \nAnswer:
            \nLimiting frequency for Balmer series possible when n1<\/sub> = 2 and n2<\/sub> = \u221e.
            \n\"1st
            \n\"1st<\/p>\n

            Question 3.
            \nCalculate the wavelength and wave numbers of the first and second lines in the Balmer series of hydrogen spectrum. Given R = 1.096 \u00d7 107<\/sup>m-1<\/sup>
            \nAnswer:
            \nFor Balmer series n1<\/sub> = 2 , for third line n2<\/sub> = 3, for fourth line n2<\/sub> = 4
            \ni. Wave number \\(\\overrightarrow{\\mathbf{V}}\\) of the third line is given by
            \n\"1st<\/p>\n

            Question 4.
            \nCalculate the wavelength and wave number of H\u03b3<\/sub> and H????<\/sub> line (R = 10.97 \u00d7 106 m-1<\/sup>)
            \nAnswer:
            \nFor Balmer series n1<\/sub> = 2 , for third line n2<\/sub> = 5, for fourth line n2<\/sub> = 6
            \ni. Wave number \\(\\overrightarrow{\\mathbf{V}}\\) of the third line is given by
            \n\"1st
            \n= 364 \u00d7 10-9<\/sup>m = 364.9nm
            \nWavelength of H line = 364.9nm<\/p>\n

            \"KSEEB<\/p>\n

            Question 5.
            \nCalculate the wave number and wavelength of the first spectral line of Lyman series of hydrogen spectrum.
            \nRydberg constant R = 10.97 \u00d7 106 m-1<\/sup>
            \nAnswer:
            \n\"1st<\/p>\n

            Question 6.
            \nCalculate the wave number of the spectral line when electron jumps from the seond Bohr orbit to the ground state. R = 1.097 \u00d7 107<\/sup> m-1<\/sup>.
            \nAnswer:
            \n\"1st
            \nWavelength of the spectral line = 8.2258 \u00d7 106<\/sup>m-1<\/sup><\/p>\n

            Question 7.
            \nIn a hydrogen atom, an electron jumps from third orbit to the first orbit. Find out the frequency and wavelength of the spectral line. Given R = 1.097 \u00d7 107<\/sup>m-1<\/sup>
            \n\"1st
            \nWavelength of the spectral line = 1025.4 A0<\/sup>
            \nFrequency of the spectral line = 2.9257 \u00d7 1015<\/sup> s-1<\/sup><\/p>\n

            Question 8.
            \nCalculate the wavelength of 2nd<\/sup> line and limiting line of Balmer series. If wave length of first line of Balmer series is 656 nm.
            \nAnswer:
            \n\"1st
            \nFor first line m = 2, m = 3 & \u03bb = 656 nm
            \n\"1st
            \nFor secong line n1 = 2,n2 = 4
            \n\"1st
            \n\u2234 Wavelength of the limiting line n1<\/sub> = 2, n2<\/sub>\u00a0= \u221e
            \n\"1st<\/p>\n

            \"KSEEB<\/p>\n

            Question 9.
            \nCalculate the wavelength of a wave of frequency 1012 Hz, travelling with the speed of light 3 x 108 <\/sup>ms-1<\/sup>
            \nAnswer:
            \n\"1st<\/p>\n

            Question 10.
            \nCalculate the frequency of electromagnetic radiation having the wavelength 3 \u03bc. Calculate the wave number corresponding to it. (1\u03bc = 10-6<\/sup> m)
            \nAnswer:
            \n\"1st<\/p>\n

            Question 11.
            \nCalculate the frequency and energy per quantum of a radiation with a wavelength of 200 nm. (c = 3 \u00d7 108<\/sup> ms-1<\/sup> and h = 6.625 \u00d7 10-34<\/sup> Js)
            \nAnswer:
            \n\"1st
            \n= 1.5 \u00d7 1015 <\/sup>Hz = 1.55 \u00d7 10 15<\/sup>Hz.
            \nE = hv = 6.625 \u00d7 10 -34<\/sup> x 1.5 \u00d7 1015<\/sup>= 9.9375 \u00d7 10-19<\/sup> J<\/p>\n

            Question 12.
            \nCalculate the number of photon of light with a wavelength of 6000A that provide I joule of energy.
            \nAnswer:
            \n\"1st
            \n= 0.00331 \u00d7 10-16<\/sup>J = 3.31 \u00d7 10-19<\/sup> J
            \nNumber of photons 3.31 \u00d7 10-19<\/sup> J make 1 photon
            \n1J = \\(\\frac{1}{3.31 \\times 10^{-19}}\\) = 3.021 \u00d7 1020 <\/sup>photons<\/p>\n

            Question 13.
            \nA major line in an atomic emission spectrum occurs at 450 nm. Find the energy decrease, as this photon is emitted.
            \nAnswer:
            \n\"1st<\/p>\n

            \"KSEEB<\/p>\n

            Question 14.
            \nCalculate the wave number, wavelength and frequency of the first line in the Baimer series.
            \nAnswer:
            \n\"1st
            \nFor Balmer Series
            \nn1<\/sub> = 2 and n2<\/sub> = 3 for the first time
            \n\"1st<\/p>\n

            Question 15.
            \nThe red light of neon signs has a wavelength of 693 nm. Find the energy difference (per mole of atoms) between the two energy levels involved.
            \nAnswer:
            \n\"1st
            \n= 2.8684 \u00d7 1015 <\/sup>J
            \nEnergy difference per mole of atoms = 2.8684 \u00d7 1015<\/sup> \u00d7 6.022 \u00d7 1023<\/sup><\/p>\n

            Question 16.
            \nCalculate the wavelength of an electron moving with a velocity of 2.5 \u00d7 10-7<\/sup> ms-1<\/sup> h = 6.626 \u00d7 10-34<\/sup> Js ; mass of an electron = 9.11 \u00d7 10-31<\/sup> kg.
            \nAnswer:
            \n\"1st<\/p>\n

            Question 17.
            \nFind the mass of an electrically charged particle moving with a velocity of 3 \u00d7 106 ms-1<\/sup> and having a de Broglie wavelength of 2\u00c5.
            \nAnswer:
            \n\"1st<\/p>\n

            \"KSEEB<\/p>\n

            Question 18.
            \nCalculate the energy of a photon whose wavelength is 3.864 \u00d7 10-7<\/sup>m.
            \nAnswer:
            \n\\(\\mathrm{E}=\\mathrm{h} \\vartheta=\\frac{\\mathrm{h} \\mathrm{c}}{\\lambda}\\)
            \nh = 6.626 \u00d7 10-34<\/sup>
            \nc = 3.0 \u00d7 108 <\/sup>ms-1<\/sup>
            \n\"1st
            \n\u03bb = 3.864 \u00d7 10-7<\/sup><\/p>\n

            Question 19.
            \nCalculate the de Broglie wavelength of (a) an electron of mass 9.11 \u00d7 10-31<\/sup> kg and moving with a velocity of 1.0 \u00d7 106 ms-1<\/sup> (b) a bullet of mass 25g moving with a velocity of 100ms-1<\/sup>
            \nAnswer:
            \n\"1st<\/p>\n","protected":false},"excerpt":{"rendered":"

            You can Download Chapter 2 Structure of Atom Questions and Answers, Notes, 1st PUC Chemistry Question Bank with Answers Karnataka State Board Solutions help you to revise complete Syllabus and score more marks in your examinations. Karnataka 1st PUC Chemistry Question Bank Chapter 2 Structure of Atom 1st PUC Chemistry Structure of Atom One Mark …<\/p>\n","protected":false},"author":5,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[81],"tags":[],"jetpack_sharing_enabled":true,"jetpack_featured_media_url":"","_links":{"self":[{"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/posts\/8723"}],"collection":[{"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/users\/5"}],"replies":[{"embeddable":true,"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/comments?post=8723"}],"version-history":[{"count":0,"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/posts\/8723\/revisions"}],"wp:attachment":[{"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/media?parent=8723"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/categories?post=8723"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/kseebsolutions.guru\/wp-json\/wp\/v2\/tags?post=8723"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}