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Chemistry Grade 11 Unit 1: ATOMIC STRUCTURE AND PERIODIC PROPERTIES OF THE ELEMENTS

national exam questions have come from this unit. It runs 64 pages; one careful study pass takes about 6.5 hours, and its difficulty is harder among Chemistry units. Each section below lists the questions set from it, with the year, and opens the page that teaches it.

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1.1 Introduction · read p. 2
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1.2 Dalton’s Atomic Theory and the Modern Atomic Theory · read p. 3
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1.2.1 Postulates of Dalton’s Atomic Theory · read p. 3
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1.2.2 Postulates of Modern Atomic Theory · read p. 5
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1.3 Early Experiments to Characterize the Atom · read p. 7
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1.3.1 The Discovery of the Electron · read p. 7
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1.3.2 Radioactivity and the Discovery of the Nucleus · read p. 9
  • 2018 E.C., Q12 – On the gold foil experiment, most alpha particles passed straight through the foil while a few were strongly deflected. What conclusion can be drawn from this observation?
  • 2008 E.C., Q29 – Which of the following types of rays combine to form atoms of Helium?
  • 2007 E.C., Q6 – Of the three types of radioactivity characterized by Rutherford, which of the following are particles?
1.3.3 Discovery of the Neutron · read p. 11
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1.4 Make-up of the Nucleus · read p. 12
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1.4.1 Subatomic Particles · read p. 12
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1.4.2 Atomic Mass and Isotopes · read p. 13
  • 2013 E.C., Q66 – Silver (Z=47) has several known isotopes, but two occur naturally, 107 Ag and 109 Ag.Given the following mass spectrometric data, calculate the atomic mass of Ag
1.5 Electromagnetic Radiation and Atomic Spectra · read p. 15
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1.5.1 Electromagnetic Radiation · read p. 15
  • 2018 E.C., Q13 – Which of the following statements correctly relates wavelength, frequency, and speed of EMR in vacuum?
  • 2017 E.C., Q41 – Which of the following statements CORRECTLY describes the relationship among wavelength, frequency and speed in electromagnetic radiation?
  • 2017 E.C., Q8 – A mineral absorbs purple light of frequency $7.11\times10^{14}\,\text{Hz}$. What is the wavelength (in nm) of the absorbed light? ($c=3.00\times10^8\,\text{m/s}$)
  • 2016 E.C., Q47 – Which of the following characteristics of an electromagnetic radiation is CORRECT?
  • 2015 E.C., Q44 – Which one of the following explains that light has BOTH wave and particle nature?
  • 2014 E.C., Q33 – Which of the following explains the emission spectra of atoms consisting of a series of fine lines?
  • 2012 E.C., Q74 – Which one of the following electromagnetic radiations has the highest energy?
  • 2010 E.C., Q50 – Which of the following correctly lists electromagnetic waves in order from shortest to longest wavelength?
  • 2010 E.C., Q23 – Which of the following is fundamentally different from the others?
  • 2009 E.C., Q7 – The normal human eye responds to visible light of wavelength ranging from about 390nm to 710nm. What is the frequency range of the human eye? 7.7 × 10 s 14 −1 4.2 × 10 s 14 −1 4.2 × 10 s 14 −1 7.7 × 10 s 14 −1
  • 2008 E.C., Q30 – What is the relationship between frequency (V), wavelength ( ) and the speed of light (c)? λ
  • 2007 E.C., Q24 – The wave number of an electromagnetic radiation is $1\times10^5\,\text{cm}^{-1}$. The frequency of the radiation would be
  • 2007 E.C., Q60 – Which of the following statements is true?
  • 2007 E.C., Q22 – No axes, units or values are marked.]
  • 2005 E.C., Q2 – Which of the following statements is TRUE?
1.5.2 The Quantum Theory and Photon · read p. 18
  • 2014 E.C., Q32 – Which of the following statements is correct about the energy of a photon?
  • 2010 E.C., Q19 – The maximum kinetic energy of a photoelectron emitted from a metal is $1.03\times10^{-19}\,\text{J}$ when light that has a $656\,\text{nm}$ wavelength shines on the surface. What is the threshold frequency for this metal
  • 2010 E.C., Q52 – What would be the wavelength of a radio wave having a frequency of 3 MHz?
  • 2009 E.C., Q11 – What is the energy associated with one photon of a microwave radiation having a frequency of $2.45\times10^9\,\text{s}^{-1}$?
  • 2009 E.C., Q12 – What is the frequency of a radiation (in Hz) from an atom if its wavelength is $1.0 \times 10^{-9}\,\text{nm}$?
  • 2008 E.C., Q31 – What is the magnitude of quantum energy and the frequency for an object whose wave length is $0.6 \times 10^{-6}\,\text{m}$?
  • 2006 E.C., Q53 – What is the ionization energy of an iron atom if it requires a radiation of $276\,\text{nm}$ to completely remove its outer most electron in the gaseous state? (Plank's constant, $h=6.626\times10^{-34}\,\text{Js}$, speed
1.5.3 Atomic Spectra · read p. 23
  • 2011 E.C., Q55 – Which of the following is NOT true about the photoelectric effect?
  • 2006 E.C., Q10 – What is the ratio of the energy of a photon of 300 nm wavelength radiation to that of 600 nm radiation?
1.5.4 The Bohr Model of the Hydrogen Atom · read p. 25
  • 2017 E.C., Q9 – Why do atoms absorb energy when their electrons undergo transitions from a lower energy to a higher energy level? This is because
  • 2016 E.C., Q42 – "The hydrogen atom moves in a fixed circular orbit associated with allowable energy states" This is called ____.
  • 2011 E.C., Q45 – The energy of an electron in the first Bohr orbit of hydrogen atom is -13.6 eV. The possible value of the excited state for electron in Bohr orbits of hydrogen is_______.
  • 2011 E.C., Q19 – In the electromagnetic spectrum with wavelengths shown (in micrometers, m), which bracketed section of the μ spectrum represents visible light? μm [Figure: A horizontal axis labeled 'wavelength ( )' with tick marks at 0.
  • 2007 E.C., Q35 – Which of the following transitions will emit maximum energy in the hydrogen atom?
1.5.5 Limitations of the Bohr Model · read p. 32
  • 2012 E.C., Q75 – When electrons fall down from the higher energy level to the first excited state, the spectral lines correspond to:
  • 2011 E.C., Q32 – Consider the following two possibilities for electron transfer in a hydrogen atom, given below: First: The electron drops from the Bohr orbit n = 3 to the orbit n = 2, followed by the transition from n = 2 to n = 1 Secon
  • 2011 E.C., Q64 – When an electron in a hydrogen atom makes the transition from the $n=4$ state to the $n=2$ state, blue light with a wavelength of 434 nm is emitted. Which of the following expressions gives the energy released by the tra
  • 2006 E.C., Q8 – Which electron transition in a hydrogen atom releases the largest energy?
1.5.6 The Wave-Particle Duality of Matter and Energy · read p. 33
  • 2010 E.C., Q21 – Which of the following questions expresses de Broglie's hypothesis?
  • 2005 E.C., Q56 – What is the wavelength associated with an electron of mass, $m = 9.11 \times 10^{-28}\,\text{g}$, travelling at 40% of the velocity of light?
1.6 The Quantum Mechanical Model of the Atom · read p. 35
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1.6.1 The Heisenberg’s Principle · read p. 35
  • 2013 E.C., Q67 – Which statement correctly describes Heisenberg's uncertainty principle?
  • 2009 E.C., Q9 – The Heisenberg uncertainty principle states that
1.6.2 Quantum Numbers · read p. 36
  • 2018 E.C., Q14 – Which combination represents all possible sets of quantum numbers for the 3d electrons?
  • 2015 E.C., Q42 – What are the four quantum numbers for an electron in a 2s orbital?
  • 2015 E.C., Q31 – Which one of the following describes the quantum mechanical model?
  • 2010 E.C., Q20 – What is the maximum number of electrons in an atom that can have the principal quantum number n = 4?
  • 2010 E.C., Q18 – Which quantum number is used to be determine sub shells?
  • 2009 E.C., Q8 – How many different types of orbitals are there in the third energy level?
  • 2008 E.C., Q33 – What values of l are permitted for an electron with n = 4?
  • 2007 E.C., Q16 – How many orbital are there in an atom with n = 4?
  • 2007 E.C., Q5 – Which one of the following represents an acceptable possible set of quantum numbers (in the order $n, l, m_l, m_s$) for an electron in an atom?
  • 2006 E.C., Q23 – Which set of quantum numbers (n, l, , ) is not possible?
  • 2005 E.C., Q19 – Which of the following quantum number (s) is (are) related to the size and energy of an electron in a hydrogen atom?
  • 2005 E.C., Q20 – An electron has a spin quantum number, s = +1/2 and a magnetic quantum number, . In which of the following orbital will it NOT be present?
1.6.3 Shapes of Atomic Orbitals · read p. 39
  • 2011 E.C., Q20 – Which of the orbitals in the figure below has (have) an angular momentum quantum number of $\ell=2$? [Figure: Four electron density cross-section diagrams labeled I, II, III, and IV. I and III are spherically symmetric s
1.7 Electronic Configurations and Orbital Diagrams · read p. 41
  • 2009 E.C., Q6 – Which of the following is the correct order for electrons filling in orbitals?
  • 2006 E.C., Q20 – Which one of the following atoms in its ground state has the greatest number of unpaired electrons?
1.7.1 Ground State Electronic Configuration of the Elements · read p. 42
  • 2018 E.C., Q10 – Why does the electron configuration of chromium (Cr) deviate from the expected [Ar] 4s²3d⁴?
  • 2017 E.C., Q11 – Which of the following is CORRECT about the set of quantum numbers assigned to the two electrons of the helium atom?
  • 2016 E.C., Q43 – Which of the following is the core electron configuration of the metal ion in ferric sulfate, Fe 2 (SO 4 ) 3 ? (Atomic Number of Fe = 26)
  • 2013 E.C., Q45 – According to Hund's rule equal energy (degenerate) orbitals are filled with
  • 2012 E.C., Q77 – Which of the following electrons, identified only by their n and l quantum numbers, have the highest energy?
  • 2012 E.C., Q20 – What are the four quantum numbers of 4d^6 orbital? (Options in table)
  • 2008 E.C., Q26 – What is the maximum number of unpaired electron in a d subshell?
  • 2008 E.C., Q25 – Which of the following electrons, identified only by their n and l quantum numbers have the highest energy? n=3, l=0 n=4,l=1 n=3, l=2 n=4, l=2
  • 2008 E.C., Q27 – So the diagram shows a full 3s level below and three 3p levels above, of which only the first holds one electron.]
  • 2007 E.C., Q33 – The maximum number of electrons in P-orbital with n = 6, ml = 0 is
  • 2006 E.C., Q59 – How many 3d electrons are present in the ground state of chromium atom?
  • 2006 E.C., Q54 – Which of the electron configurations describes the ground state electron configuration of $\mathrm{Cl^-}$?
  • 2005 E.C., Q5 – Which of the following groups in the periodic table has paramagnetic atoms?
  • 2005 E.C., Q22 – Which of the following represents the general configuration of the transition elements?
  • 2005 E.C., Q57 – The quantum numbers listed below are meant for four different electrons in an atom: I. II. III. IV. = 1 0, m = s −1/2 When these sets of quantum numbers are arranged in order of increasing energy, one may get:
1.8 Electronic Configurations and the Periodic Table of the Elements · read p. 47
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1.8.1 The Modern Periodic Table · read p. 47
  • 2015 E.C., Q33 – An element is located in Group VIIA and 3 period of the modern periodic table. On the basis of this the element;
1.8.2 Classification of the Elements · read p. 48
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1.8.3 Periodic Properties · read p. 49
  • 2018 E.C., Q4 – The periodic table contains two separate rows of inner transition elements located below the main table. These rows contain 14 elements each and belong to the 6th and 7th periods. Based on their position and electron con
  • 2018 E.C., Q16 – Given elements: O, Be, N, B, F: which is the correct increasing order of first ionization energy?
  • 2017 E.C., Q45 – Scandium (Sc) has the electron configuration $[\mathrm{Ar}]\,4s^2 3d^1$. To which group of elements does it belong to?
  • 2016 E.C., Q32 – Consider the following chart of general periodic properties in the periodic table. From the given periodic properties, which one CORRECTLY agrees with the periodic trend in the chart?
  • 2011 E.C., Q33 – Which of the following elements has the highest fifth ionization energy (IE₅)?
1.8.4 Advantages of Periodic Classification of the Elements · read p. 58
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