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Chemistry · Textbook solutions

Structure of Atom

Every solved example, exercise, and miscellaneous question — in the order the textbook teaches them. · 84 questions

Worked Examples

18 q

Solved Examples

Worked · 18
  1. Eg 2.1
    Calculate the number of protons, neutrons and electrons in 3580Br^{80}_{35}\text{Br}.
  2. Eg 2.2
    The number of electrons, protons and neutrons in a species are equal to 18, 16 and 16 respectively. Assign the proper symbol to the species.
  3. Eg 2.3
    The Vividh Bharati station of All India Radio, Delhi, broadcasts on a frequency of 1,368 kHz (kilo hertz). Calculate the wavelength of the electromagnetic radiation emitted by transmitter. Which part of the electromagnetic spectrum does it belong to?
  4. Eg 2.4
    The wavelength range of the visible spectrum extends from violet (400 nm) to red (750 nm). Express these wavelengths in frequencies (Hz). (1 nm=10−9 m1\,\text{nm} = 10^{-9}\,\text{m})
  5. Eg 2.5
    Calculate (a) wavenumber and (b) frequency of yellow radiation having wavelength 5800 A˚5800\,\text{Å}.
  6. Eg 2.6
    Calculate energy of one mole of photons of radiation whose frequency is 5×1014 Hz5 \times 10^{14}\,\text{Hz}.
  7. Eg 2.7
    A 100 watt bulb emits monochromatic light of wavelength 400 nm. Calculate the number of photons emitted per second by the bulb.
  8. Eg 2.8
    When electromagnetic radiation of wavelength 300 nm falls on the surface of sodium, electrons are emitted with a kinetic energy of 1.68×105 J mol−11.68 \times 10^{5}\,\text{J mol}^{-1}. What is the minimum energy needed to remove an electron from sodium? What is the maximum wavelength that will cause a photoelectron to be emitted?
  9. Eg 2.9
    The threshold frequency ν0\nu_0 for a metal is 7.0×1014 s−17.0 \times 10^{14}\,\text{s}^{-1}. Calculate the kinetic energy of an electron emitted when radiation of frequency ν=1.0×1015 s−1\nu = 1.0 \times 10^{15}\,\text{s}^{-1} hits the metal.
  10. Eg 2.10
    What are the frequency and wavelength of a photon emitted during a transition from n=5n = 5 state to the n=2n = 2 state in the hydrogen atom?
  11. Eg 2.11
    Calculate the energy associated with the first orbit of He+\text{He}^{+}. What is the radius of this orbit?
  12. Eg 2.12
    What will be the wavelength of a ball of mass 0.1 kg moving with a velocity of 10 m s−110\,\text{m s}^{-1}?
  13. Eg 2.13
    The mass of an electron is 9.1×10−31 kg9.1 \times 10^{-31}\,\text{kg}. If its K.E. is 3.0×10−25 J3.0 \times 10^{-25}\,\text{J}, calculate its wavelength.
  14. Eg 2.14
    Calculate the mass of a photon with wavelength 3.6 A˚3.6\,\text{Å}.
  15. Eg 2.15
    A microscope using suitable photons is employed to locate an electron in an atom within a distance of 0.1 A˚0.1\,\text{Å}. What is the uncertainty involved in the measurement of its velocity?
  16. Eg 2.16
    A golf ball has a mass of 40 g, and a speed of 45 m/s45\,\text{m/s}. If the speed can be measured within accuracy of 2%, calculate the uncertainty in the position.
  17. Eg 2.17
    What is the total number of orbitals associated with the principal quantum number n=3n = 3?
  18. Eg 2.18
    Using s,p,d,fs, p, d, f notations, describe the orbital with the following quantum numbers (a) n=2n = 2, l=1l = 1, (b) n=4n = 4, l=0l = 0, (c) n=5n = 5, l=3l = 3, (d) n=3n = 3, l=2l = 2

Exercises

66 q
  1. Ex 2.1
    (i) Calculate the number of electrons which will together weigh one gram. (ii) Calculate the mass and charge of one mole of electrons.
  2. Ex 2.2
    (i) Calculate the total number of electrons present in one mole of methane. (ii) Find (a) the total number and (b) the total mass of neutrons in 7 mg of 14C^{14}\text{C}. (Assume that mass of a neutron =1.675×10−27 kg= 1.675 \times 10^{-27}\,\text{kg}). (iii) Find (a) the total number and (b) the total mass of protons in 34 mg of NH3\text{NH}_3 at STP. Will the answer change if the temperature and pressure are changed?
  3. Ex 2.3
    How many neutrons and protons are there in the following nuclei? 613C^{13}_{6}\text{C}, 816O^{16}_{8}\text{O}, 1224Mg^{24}_{12}\text{Mg}, 2656Fe^{56}_{26}\text{Fe}, 3888Sr^{88}_{38}\text{Sr}
  4. Ex 2.4
    Write the complete symbol for the atom with the given atomic number (Z) and atomic mass (A) (i) Z=17Z = 17, A=35A = 35. (ii) Z=92Z = 92, A=233A = 233. (iii) Z=4Z = 4, A=9A = 9.
  5. Ex 2.5
    Yellow light emitted from a sodium lamp has a wavelength (λ)(\lambda) of 580 nm. Calculate the frequency (ν)(\nu) and wavenumber (νˉ)(\bar{\nu}) of the yellow light.
  6. Ex 2.6
    Find energy of each of the photons which (i) correspond to light of frequency 3×1015 Hz3 \times 10^{15}\,\text{Hz}. (ii) have wavelength of 0.50 A˚0.50\,\text{Å}.
  7. Ex 2.7
    Calculate the wavelength, frequency and wavenumber of a light wave whose period is 2.0×10−10 s2.0 \times 10^{-10}\,\text{s}.
  8. Ex 2.8
    What is the number of photons of light with a wavelength of 4000 pm that provide 1 J of energy?
  9. Ex 2.9
    A photon of wavelength 4×10−7 m4 \times 10^{-7}\,\text{m} strikes on metal surface, the work function of the metal being 2.13 eV. Calculate (i) the energy of the photon (eV), (ii) the kinetic energy of the emission, and (iii) the velocity of the photoelectron (1 eV=1.6020×10−19 J)(1\,\text{eV} = 1.6020 \times 10^{-19}\,\text{J}).
  10. Ex 2.10
    Electromagnetic radiation of wavelength 242 nm is just sufficient to ionise the sodium atom. Calculate the ionisation energy of sodium in kJ mol−1\text{kJ mol}^{-1}.
  11. Ex 2.11
    A 25 watt bulb emits monochromatic yellow light of wavelength of 0.57 μm0.57\,\mu\text{m}. Calculate the rate of emission of quanta per second.
  12. Ex 2.12
    Electrons are emitted with zero velocity from a metal surface when it is exposed to radiation of wavelength 6800 A˚6800\,\text{Å}. Calculate threshold frequency (ν0)(\nu_0) and work function (W0)(W_0) of the metal.
  13. Ex 2.13
    What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n=4n = 4 to an energy level with n=2n = 2?
  14. Ex 2.14
    How much energy is required to ionise a H atom if the electron occupies n=5n = 5 orbit? Compare your answer with the ionization enthalpy of H atom (energy required to remove the electron from n=1n = 1 orbit).
  15. Ex 2.15
    What is the maximum number of emission lines when the excited electron of a H atom in n=6n = 6 drops to the ground state?
  16. Ex 2.16
    (i) The energy associated with the first orbit in the hydrogen atom is −2.18×10−18 J atom−1-2.18 \times 10^{-18}\,\text{J atom}^{-1}. What is the energy associated with the fifth orbit? (ii) Calculate the radius of Bohr's fifth orbit for hydrogen atom.
  17. Ex 2.17
    Calculate the wavenumber for the longest wavelength transition in the Balmer series of atomic hydrogen.
  18. Ex 2.18
    What is the energy in joules, required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of the light emitted when the electron returns to the ground state? The ground state electron energy is −2.18×10−11 ergs-2.18 \times 10^{-11}\,\text{ergs}.
  19. Ex 2.19
    The electron energy in hydrogen atom is given by En=(−2.18×10−18)/n2 JE_n = (-2.18 \times 10^{-18})/n^2\,\text{J}. Calculate the energy required to remove an electron completely from the n=2n = 2 orbit. What is the longest wavelength of light in cm that can be used to cause this transition?
  20. Ex 2.20
    Calculate the wavelength of an electron moving with a velocity of 2.05×107 m s−12.05 \times 10^{7}\,\text{m s}^{-1}.
  21. Ex 2.22
    Which of the following are isoelectronic species i.e., those having the same number of electrons? Na+\text{Na}^{+}, K+\text{K}^{+}, Mg2+\text{Mg}^{2+}, Ca2+\text{Ca}^{2+}, S2−\text{S}^{2-}, Ar\text{Ar}.
  22. Ex 2.23
    (i) Write the electronic configurations of the following ions: (a) H−\text{H}^{-} (b) Na+\text{Na}^{+} (c) O2−\text{O}^{2-} (d) F−\text{F}^{-} (ii) What are the atomic numbers of elements whose outermost electrons are represented by (a) 3s13s^1 (b) 2p32p^3 and (c) 3p53p^5? (iii) Which atoms are indicated by the following configurations? (a) [He] 2s1[\text{He}]\,2s^1 (b) [Ne] 3s2 3p3[\text{Ne}]\,3s^2\,3p^3 (c) [Ar] 4s2 3d1[\text{Ar}]\,4s^2\,3d^1.
  23. Ex 2.24
    What is the lowest value of nn that allows gg orbitals to exist?
  24. Ex 2.25
    An electron is in one of the 3d3d orbitals. Give the possible values of nn, ll and mlm_l for this electron.
  25. Ex 2.26
    An atom of an element contains 29 electrons and 35 neutrons. Deduce (i) the number of protons and (ii) the electronic configuration of the element.
  26. Ex 2.27
    Give the number of electrons in the species H2+\text{H}_2^{+}, H2\text{H}_2 and O2+\text{O}_2^{+}.
  27. Ex 2.28
    (i) An atomic orbital has n=3n = 3. What are the possible values of ll and mlm_l? (ii) List the quantum numbers (mlm_l and ll) of electrons for 3d3d orbital. (iii) Which of the following orbitals are possible? 1p1p, 2s2s, 2p2p and 3f3f
  28. Ex 2.29
    Using s,p,ds, p, d notations, describe the orbital with the following quantum numbers. (a) n=1n = 1, l=0l = 0; (b) n=3n = 3; l=1l = 1 (c) n=4n = 4; l=2l = 2; (d) n=4n = 4; l=3l = 3.
  29. Ex 2.30
    Explain, giving reasons, which of the following sets of quantum numbers are not possible.
    nnllmlm_lmsm_s
    (a)000+12+\tfrac{1}{2}
    (b)100−12-\tfrac{1}{2}
    (c)110+12+\tfrac{1}{2}
    (d)210−12-\tfrac{1}{2}
    (e)33−3-3+12+\tfrac{1}{2}
    (f)310+12+\tfrac{1}{2}
  30. Ex 2.31
    How many electrons in an atom may have the following quantum numbers? (a) n=4n = 4, ms=−12m_s = -\tfrac{1}{2} (b) n=3n = 3, l=0l = 0
  31. Ex 2.32
    Show that the circumference of the Bohr orbit for the hydrogen atom is an integral multiple of the de Broglie wavelength associated with the electron revolving around the orbit.
  32. Ex 2.33
    What transition in the hydrogen spectrum would have the same wavelength as the Balmer transition n=4n = 4 to n=2n = 2 of He+\text{He}^{+} spectrum?
  33. Ex 2.34
    Calculate the energy required for the process He+(g)→He2+(g)+e−\text{He}^{+}(g) \rightarrow \text{He}^{2+}(g) + e^{-} The ionization energy for the H atom in the ground state is 2.18×10−18 J atom−12.18 \times 10^{-18}\,\text{J atom}^{-1}.
  34. Ex 2.35
    If the diameter of a carbon atom is 0.15 nm, calculate the number of carbon atoms which can be placed side by side in a straight line across length of scale of length 20 cm long.
  35. Ex 2.36
    2×1082 \times 10^{8} atoms of carbon are arranged side by side. Calculate the radius of carbon atom if the length of this arrangement is 2.4 cm.
  36. Ex 2.37
    The diameter of zinc atom is 2.6 A˚2.6\,\text{Å}. Calculate (a) radius of zinc atom in pm and (b) number of atoms present in a length of 1.6 cm if the zinc atoms are arranged side by side lengthwise.
  37. Ex 2.38
    A certain particle carries 2.5×10−16 C2.5 \times 10^{-16}\,\text{C} of static electric charge. Calculate the number of electrons present in it.
  38. Ex 2.39
    In Milikan's experiment, static electric charge on the oil drops has been obtained by shining X-rays. If the static electric charge on the oil drop is −1.282×10−18 C-1.282 \times 10^{-18}\,\text{C}, calculate the number of electrons present on it.
  39. Ex 2.40
    In Rutherford's experiment, generally the thin foil of heavy atoms, like gold, platinum etc. have been used to be bombarded by the α\alpha-particles. If the thin foil of light atoms like aluminium etc. is used, what difference would be observed from the above results?
  40. Ex 2.41
    Symbols 3579Br^{79}_{35}\text{Br} and 79Br^{79}\text{Br} can be written, whereas symbols 7935Br^{35}_{79}\text{Br} and 35Br^{35}\text{Br} are not acceptable. Answer briefly.
  41. Ex 2.42
    An element with mass number 81 contains 31.7% more neutrons as compared to protons. Assign the atomic symbol.
  42. Ex 2.43
    An ion with mass number 37 possesses one unit of negative charge. If the ion conatins 11.1% more neutrons than the electrons, find the symbol of the ion.
  43. Ex 2.44
    An ion with mass number 56 contains 3 units of positive charge and 30.4% more neutrons than electrons. Assign the symbol to this ion.
  44. Ex 2.45
    Arrange the following type of radiations in increasing order of frequency: (a) radiation from microwave oven (b) amber light from traffic signal (c) radiation from FM radio (d) cosmic rays from outer space and (e) X-rays.
  45. Ex 2.46
    Nitrogen laser produces a radiation at a wavelength of 337.1 nm. If the number of photons emitted is 5.6×10245.6 \times 10^{24}, calculate the power of this laser.
  46. Ex 2.47
    Neon gas is generally used in the sign boards. If it emits strongly at 616 nm, calculate (a) the frequency of emission, (b) distance traveled by this radiation in 30 s, (c) energy of quantum and (d) number of quanta present if it produces 2 J of energy.
  47. Ex 2.48
    In astronomical observations, signals observed from the distant stars are generally weak. If the photon detector receives a total of 3.15×10−18 J3.15 \times 10^{-18}\,\text{J} from the radiations of 600 nm, calculate the number of photons received by the detector.
  48. Ex 2.49
    Lifetimes of the molecules in the excited states are often measured by using pulsed radiation source of duration nearly in the nano second range. If the radiation source has the duration of 2 ns and the number of photons emitted during the pulse source is 2.5×10152.5 \times 10^{15}, calculate the energy of the source.
  49. Ex 2.50
    The longest wavelength doublet absorption transition is observed at 589 and 589.6 nm. Calcualte the frequency of each transition and energy difference between two excited states.
  50. Ex 2.51
    The work function for caesium atom is 1.9 eV. Calculate (a) the threshold wavelength and (b) the threshold frequency of the radiation. If the caesium element is irradiated with a wavelength 500 nm, calculate the kinetic energy and the velocity of the ejected photoelectron.
  51. Ex 2.52
    Following results are observed when sodium metal is irradiated with different wavelengths. Calculate (a) threshold wavelength and, (b) Planck's constant.
    λ\lambda (nm)500450400
    v×10−5v \times 10^{-5} (cm s−1\text{cm s}^{-1})2.554.355.35
  52. Ex 2.53
    The ejection of the photoelectron from the silver metal in the photoelectric effect experiment can be stopped by applying the voltage of 0.35 V when the radiation 256.7 nm is used. Calculate the work function for silver metal.
  53. Ex 2.54
    If the photon of the wavelength 150 pm strikes an atom and one of tis inner bound electrons is ejected out with a velocity of 1.5×107 m s−11.5 \times 10^{7}\,\text{m s}^{-1}, calculate the energy with which it is bound to the nucleus.
  54. Ex 2.55
    Emission transitions in the Paschen series end at orbit n=3n = 3 and start from orbit nn and can be represeted as ν=3.29×1015 (Hz) [1/32−1/n2]\nu = 3.29 \times 10^{15}\,(\text{Hz})\,[1/3^2 - 1/n^2] Calculate the value of nn if the transition is observed at 1285 nm. Find the region of the spectrum.
  55. Ex 2.56
    Calculate the wavelength for the emission transition if it starts from the orbit having radius 1.3225 nm and ends at 211.6 pm. Name the series to which this transition belongs and the region of the spectrum.
  56. Ex 2.57
    Dual behaviour of matter proposed by de Broglie led to the discovery of electron microscope often used for the highly magnified images of biological molecules and other type of material. If the velocity of the electron in this microscope is 1.6×106 ms−11.6 \times 10^{6}\,\text{ms}^{-1}, calculate de Broglie wavelength associated with this electron.
  57. Ex 2.58
    Similar to electron diffraction, neutron diffraction microscope is also used for the determination of the structure of molecules. If the wavelength used here is 800 pm, calculate the characteristic velocity associated with the neutron.
  58. Ex 2.59
    If the velocity of the electron in Bohr's first orbit is 2.19×106 ms−12.19 \times 10^{6}\,\text{ms}^{-1}, calculate the de Broglie wavelength associated with it.
  59. Ex 2.60
    The velocity associated with a proton moving in a potential difference of 1000 V is 4.37×105 ms−14.37 \times 10^{5}\,\text{ms}^{-1}. If the hockey ball of mass 0.1 kg is moving with this velocity, calcualte the wavelength associated with this velocity.
  60. Ex 2.61
    If the position of the electron is measured within an accuracy of ±0.002 nm\pm 0.002\,\text{nm}, calculate the uncertainty in the momentum of the electron. Suppose the momentum of the electron is h/4πm×0.05 nmh/4\pi_m \times 0.05\,\text{nm}, is there any problem in defining this value.
  61. Ex 2.62
    The quantum numbers of six electrons are given below. Arrange them in order of increasing energies. If any of these combination(s) has/have the same energy lists: 1. n=4n = 4, l=2l = 2, ml=−2m_l = -2, ms=−1/2m_s = -1/2 2. n=3n = 3, l=2l = 2, ml=1m_l = 1, ms=+1/2m_s = +1/2 3. n=4n = 4, l=1l = 1, ml=0m_l = 0, ms=+1/2m_s = +1/2 4. n=3n = 3, l=2l = 2, ml=−2m_l = -2, ms=−1/2m_s = -1/2 5. n=3n = 3, l=1l = 1, ml=−1m_l = -1, ms=+1/2m_s = +1/2 6. n=4n = 4, l=1l = 1, ml=0m_l = 0, ms=+1/2m_s = +1/2
  62. Ex 2.63
    The bromine atom possesses 35 electrons. It contains 6 electrons in 2p2p orbital, 6 electrons in 3p3p orbital and 5 electron in 4p4p orbital. Which of these electron experiences the lowest effective nuclear charge?
  63. Ex 2.64
    Among the following pairs of orbitals which orbital will experience the larger effective nuclear charge? (i) 2s2s and 3s3s, (ii) 4d4d and 4f4f, (iii) 3d3d and 3p3p.
  64. Ex 2.65
    The unpaired electrons in Al and Si are present in 3p3p orbital. Which electrons will experience more effective nuclear charge from the nucleus?
  65. Ex 2.66
    Indicate the number of unpaired electrons in : (a) P, (b) Si, (c) Cr, (d) Fe and (e) Kr.
  66. Ex 2.67
    (a) How many subshells are associated with n=4n = 4? (b) How many electrons will be present in the subshells having msm_s value of −1/2-1/2 for n=4n = 4?