Please refer to Chapter 2 Structure of Atom MCQ Class 11 Chemistry with answers below. These multiple-choice questions have been prepared based on the latest NCERT book for Class 11 Chemistry. Students should refer to MCQ Questions for Class 11 Chemistry with Answers to score more marks in Grade 11 Chemistry exams. Students should read the chapter Structure of Atom and then attempt the following objective questions.

MCQ Questions Class 11 Chemistry Chapter 2 Structure of Atom

The Structure of Atom MCQ Class 11 Chemistry provided below covers all important topics given in this chapter. These MCQs will help you to properly prepare for exams.

Question. Which one of the following sets of ions represents a collection of isoelectronic species ? 
(a) K⁺, Cl^– , Ca²⁺, Sc³⁺
(b) Ba²⁺, Sr²⁺, K⁺,S^2-
(c) N^3-, O^2- , F^– , S^2-
(d) Li⁺, Na⁺,Mg²⁺,Ca²⁺   

Question. Ca²⁺ is isoelectronic with
(a) Na⁺ 
(d) Kr
(c) Mg²⁺
(b) Ar     

Question. Nuclear theory of the atom was put forward by [AMU]
(a) Rutherford
(b) Aston
(c) Neils Bohr
(d) J J Thomson       

Question. Which particle contains 2 neutrons and l proton ?
(a) ₁H²
(b) ₂He⁴
(C) ₁T³
(d) ₁D²         

Question. Number of neutron in C12 is
(a) 6
(b) 7
(c) 8
(d) 9               

Question. The Balmer series in atomic hydrogen is observed in the following spectral region 
(a) infrared
(b) ultraviolet
(c) visible
(d) far IR         

Question. The transition of electron in H atom that will emit maximum energy is
(a) n₃ → n₂
(b) n₄ → n₃
(c) n₅ → n₄
(d) n₄ → n₅     

Question. Which of the following is not true in Rutherford’s nuclear model of atom 
(a) Protons and neutrons are present inside the nucleus
(b) Volume of nucleus is very small as compared to the volume of an atom
(c) The number of protons and neutrons are always equal
(d) The number of electrons and protons are always equal       

Question. When the electrons ofhydrogen atom return toLshell from shells of higher energy, we get a series of lines in the spectrum. This series is called 
(a) Balmer series
(b) Lyman series
(c) Brackett series
(d) Paschen series       

Question. The kinetic energy of an electron in the second Bohr orbit of a hydrogen atom is 
(a) h²/4π²ma₀²
(b) h²/16π²ma₀²
(c) h²/32π²ma₀²
(d) h²/64π²ma₀²     

Question. Which transition in the hydrogen atomic spectrum will have the same wavelength as the transition, n = 4 to n = 2 of He+ spectrum?
(a) n = 4 to n = 3
(b) n = 3 to n = 2
(c) n = 4 to n = 2
(d) n = 2 to n = l     

     

Question. The energy of an electron in first Bohr orbit of H-atom is – 13. 6 e V. The possible energy value of electron in the excited state of Li²⁺ is 
(a) -122.4 eV
(c) -30.6eV
(b) 30. 6 eV
(d) 13 .6 eV   

Question. The electronic transitions from n = 2 to n = 1 will produce shortest wavelength in (where, n = principal quantum state)
(a) Li.²⁺
(b) He⁺
(c) H
(d) H⁺     

Question. The energy required to break one mole of Cl-Cl bonds in Cl₂ is 242 kJ mol^-1 • The longest wavelength of light capable of breaking a single Cl-Cl bond is
(a) 594 nm
(b) 640 nm
(c) 700 nm
(d) 494 nm           

Question. The number of photons emitted per second by a 60 W source of monochromatic light of wavelength 663 nm is (h = 6. 63 X 10^-34 Js)
(a) 4 x 10^-20
(b) 1.54 x 10^-20
(c) 3 x 10^-20
(d) 1 X 10^-20   

Question. Bohr’s radius of 2nd orbit of Be 3+ is equal to that of 
(a) 4^th orbit of hydrogen
(b) 2^nd orbit of He⁺
(c) 3^rd orbitof Li²⁺
(d) 1^st orbit ofhydrogen     

Question. Splitting of spectrum lines in magnetic field is 
(a) Stark effect
(b) Raman effect
(c) Zeeman effect
(d) Rutherford effect     

Question. The scientist who proposed the atomic model based on the quantisation of energy for the first time is 
(a) Max Planck
(b) Niels Bohr
(c) de-Broglie
(d) Heisenberg       

Question. What is the lowest energy of the spectral line emitted by the hydrogen atom in the Lyman se1ies ?
(h = Planck’s constant, c = velocity oflight,R = Rydberg’s constant). 
(a) 5hcR/36
(b) 4hcR/3
(c) 3hcR/4
(d) 7hcR/144       

Question. The energy of second Bohr orbit of the hydrogen atom is – 328 kJ mol- 1 ; hence the energy of fourth Bohr orbit would be 
(a) – 4l kJ mol^-1
(b) – 1312kJ mol^-1
(c) – 164 kJ mol^-1
(d) – 82 kJ mol^-1     

Question. The wavelength of a spectral line emitted by hydrogen atom in the Lyman series is 16/15R cm What is the value of n₂? (R = Rydberg constant)
(a) 2
(b) 3
(c) 4
(d) 1      

Question. The value of Rydberg constant is 
(a) 109678cm^-1
(b) 109876cm^-1
(c) 108769cm^-1
(d) 108976cm^-1         

Question. The wavelength of a spectral line in Lyman series, when electron jumps back from 2nd orbit, is 
(a) 1162 Å
(b) 1216 Å
(c) 1362 Å
(d) 1176 Å       

Question. Bohr model can explain 
(a) the solar spectrum
(b) the spectrum of hydrogen molecule
(c) spectrum of any atom or ion containing one electron only
(d) the spectrum of hydrogen atom only     

Question. The energy of a photon is 3 x 10^-12 ergs. What is its wavelength in nm ?
(h = 6. 62 x 10^-27 ergs, c = 3 x 10¹⁰ emfs)
(a) 662
(b) 1324
(c) 66.2
(d) 6.62         

Question. What is the energy (in eV) required to excite the electron from n = l ton = 2 state in hydrogen atom ?
(n = principal quantum number)
(a) 13.6
(b) 3.4
(c) 17.0
(d) 10.2         

Question. Energy of photon of visible light is 
(a) l eV
(b) l MeV
(c) l eV
(d) l keV           

Question. The relationship between the energy E₁ of the radiation with a wavelength 8000 Å and the energy E₂ of the radiation with a wavelength 16000 Å is 
(a) E₁ = 6E₂
(b) E₁ = 2E₂
(c) E₁ = 4E₂
(d) E₁ = 1/2E₂
(e) E₁ = E₂     

Question. Angular momentum of an electron hydrogen atom is given by
(a) nh/2π
(b) nh
(c) 2π/nh
(d) π/2nh         

Question. Magnitude of kinetic energy in an orbit is equal to
(a) halfofthe potential energy 
(b) twice of the potential energy
(c) one fowth of the potential energy
(d) None of the above         

Question. As per de-Broglie’s formula a macroscopic particle of mass 100 g and moving a velocity of 100 cm s^-1 will have a wavelength of 
(a) 6.6 x 10^-29 cm
(b) 6.6 x 10^-3o cm
(c) 6.6 x 10^-31 cm
(d) 6.6 x 10^-32 cm       

Question. The energy rejuired to remove an electron from metal X is E = 3.31 x 10^-20 J. Calculate the maximum wavelength of light that can photo eject an electron from metal X
(a) 6.01 x 10^-6 m
(b) 3.01 x 10^-3 m
(c) 5.01 x l0^-6 m
(d)  Noneofthese     

Question. If helium atom and hydrogen molecule are moving with the same velocity, their wavelength ratio will be
(a) 4 : 1
(b) 1: 2 
(c) 2 : 1
(d) 1 : 4     

7QuestionA particle having a mass of 1.0 mg has a velocity of 3600 km/h. Calculate the wavelength of the particle. (h = 6. 626 x 10^-27 erg-s) 
(a) 6.626x 10^-28 cm
(b) 6.626x 10^-29 cm
(c) 6.626x 10^-30 cm
(d) 6.626x 10^-31 cm           

Question. A particle moving with a velocity l 06 mis will have de-Broglie wavelength nearly,
(given, m = 6. 62 x 10^-27 kg, h = 6. 62 x 10^-34 J-s)
(a) 10-⁹ m
(b) 10^-13 m
(c) 10^-19 m
(d) 10^-18 m  

Question. A cricket ball of 0.5 kg is moving with a velocity of 100 mis. The wavelength associated with its motion is
(a) 0.01 cm
(b) 6.6 x 10^-34 m
(c) I. 32 x 10^-35 m
(d) 6.6 x 10^-28 m       

Question. The de-Broglie wavelength of a tennis ball of mass 60 g moving with a velocity of 10 m/s is approximately (Planck’s constant, h = 6. 63 x 10^-34 Js)
(a) 10^-33
(b) 10^-31
(c) 10^-16 m
(d) 10^-25 m         

Question. The total number of orbitals associated with the principal quantun1 nwnber n = 3 is
(a) 9
(b) 8
(c) 5
(d) 7   

Question. Impossible orbital among the following is
(a) 3f
(b) 2p
(c) 4d
(d) 2s     

Question. Which of the following orbitals bas zero probability of finding the electron in the xy-plane? 
(a) P_x
(b) p₂
(c) d_yz
(d) d_x2 __y2 

Question. The maximum number of electrons that can have principal quantum number, n = 3 and spin quantwn nwnber, 1 . m_s =- 1/2 . is
(a) 3
(b) 5
(c) 7
(d) 9       

Question. Which one of the following sets of quantum numbers represents the highest energy level in an atom? 
(a) n = 4, l = 0, m = 0, s = + II 2
(b) n = 3, l = 1, m = l, s = + 1/ 2
(c) n = 3, / = 2, m = -2, s = + II 2
(d) n = 3, l = 0, m = 0, s = + 112     

Question. When the azimuthal quantum number bas the value of 2, the number of orbitals possible are
(a) 7
(b) 5
(c) 3
(d) 0         

Question. The values of four quantum numbers of valence electron of an element are n = 4, I= 0, m = 0 and s = + 1/ 2 The element is 
(a) K
(b) Ti
(c) Na
(d) Sc     

Question. Which of the following sets of quantum represents numbers the highest energy of an atom ?
(a) n = 3, I = l, m = l, s = +1/2
(b) n = 3, l = 2, m = 1, s = + 1/2
(c) n = 4, I = 0, m = 0, s = + 1/2
(d) n = 3, l = 0, m = 0,s = + 1/2     

Question. The number of 2p-electrons having spin quantum number s = – 1/2 are
(a) 6
(b) 0
(c) 2
(d) 3       

Question. Which of the following is non-pemlissible ? 
(a) n = 4,l = 3,m= 0
(b) n = 4,l = 2,m=I
(c) n = 4,l = 4,m= l
(d) n = 4,l = 0,m = 0         

Question. How many electrons in ₁₉ K haven= 3; I= 0
(a) l
(b) 2 
(c) 4
(d) 3   

Question. The electrons identified by quantum numbers n and /
(1) n = 4, / = 1
(2) n = 4, / = 0
(3) n = 3, / = 3
(4) n = 3, / = 1      
can be placed in order of increasing energy as
(a) (3) < (4) < (2) < (1)
(b) (4) < (2) < (3) < (1)
(c) (2) < (4) < (1) < (3)
(d) (1) < (3) < (2) < (4)   

Question. The number of unpaired electrons in Fe³⁺ ion is
(a) 3
(b) 1 
(c) 5
(d) 2       

Question. What does the electronic configuration 1s², 2s², 2p⁵, 3s¹ indicate?
(a) Ground state of fluorine
(b) Excited state of fluorine
(c) Excited state of neon
(d) Excited state of the o; ion       

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