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Periodic Properties of Elements Test - 6

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Periodic Properties of Elements Test - 6
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  • Question 1
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    The element having least difference in the values of first and second ionization potential is
    Solution
    Magnesium attains stable noble gas configuration after the loss of two electrons. So it has least difference in the values of first and second ionization potential.
  • Question 2
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    The Modern Periodic Law was given by
    Solution
    The Modern Periodic Law was given by Mosley
  • Question 3
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    Directions: The following question has four choices, out of which ONLY ONE is correct.

    The first four ionisation energy values of an element are 191, 578, 872 and 5962 kcal. The number of valence electrons in the element is
    Solution
    Since the value of fourth ionisation energy is very high, there are three valence electrons in the element.
  • Question 4
    1 / -0
    The electronegativity of Be is the same as
    Solution
    The electronegativity of elements increases on moving left to right in a period and decreases down the group.
    The electronegativity of Be (period II, group 2) is the same as Al (period III, group 13) and they exhibit similarity in some of the properties, which is referred to as diagonal relationship.
  • Question 5
    1 / -0
    Atomic number of next inert gas, if discovered, will be
    Solution
    Since difference in atomic numbers between the elements of period 6 and period 7 is 32, hence the atomic number of next inert gas, if discovered, will be 118.
  • Question 6
    1 / -0
    The ionization potential of Na would be numerically the same as the

    Solution
    The ionization potential of Na would be numerically the same as the electron affinity of Na+
  • Question 7
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    With the increase of atomic number across a period, there is
    Solution
    With increase in the atomic number across a period, there is increase in the nuclear charge and hence, decrease in electropositive character.
  • Question 8
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    Which of the following configurations is associated with the biggest jump between 2nd and 3rd I.E.?
    Solution
    The element with the electronic configuration 1s2 2s2 2p6 3s2 is Magnesium (Mg).
    After losing two electrons, it acquires the stable octet configuration of Neon and there will be a quantum jump between the values of second and third ionization energies.
    Hence, option (3) is correct.


  • Question 9
    1 / -0
    Which element has the maximum electron affinity?
    Solution
    Electron affinity increases as we move from felt to right along the period in a periodic table.
  • Question 10
    1 / -0
    The ion which has the maximum value of hydration energy is
    Solution
    Hydration enthalpy decreases down the group because the size of the atom increases due to addition of a shell.
    The Lithium ion, being smaller in size, has a higher charge density and hence, a higher hydration enthalpy.
  • Question 11
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    Which element has the highest 1st ionisation energy?
    Solution
    Nitrogen atom has stable electronic configuration due to half filled p subshell. So it will have very high value of the first electronic configuration.
  • Question 12
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    The process requiring absorption of energy is
    Solution
    Energy is required to release an electron from an atom. So F F+ will require the absorption of energy.
  • Question 13
    1 / -0
    Which of the following elements has the greatest tendency to lose electrons?
    Solution
    The tendency to lose electrons increases as we go down a group because the atomic radius increases and the ionisation energy decreases. So, in the case of alkali metals, Fr has the highest tendency to lose electrons.
  • Question 14
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    To which group of the periodic table does the element with electronic configuration 1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s2, 4p6, 4d10, 5s2, 5p3 belong?
    Solution
    Since each atom of this element contains five valence electrons, it belongs to group 15 of the periodic table.
    Also, it has five shells occupied with electrons, hence it is an element of period V.
  • Question 15
    1 / -0
    Modern periodic table is based on the atomic numbers of elements. Which of the following experiments proved the significance of the atomic number?
    Solution
    Moseley was able to show that the frequencies of certain characteristic X-rays emitted from chemical elements are proportional to the square of a number which is close to the element\'s atomic number; a finding which supported van den Broek and Bohr\'s model of the atom in which the atomic number is the same as the number of positive charges in the nucleus of the atom.
  • Question 16
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    Choose the correct increasing order of electronegativities of the corresponding elements.
    Solution
    Electronegativity increases on moving from left to right across a period and decreases on moving from top to bottom in a group in the periodic table. Hence, the correct order is Si < P < C < N.
  • Question 17
    1 / -0
    Diagonal relationship in the periodic table is shown by the elements of
    Solution
    On moving diagonally across the periodic table, the elements particularly those of the second and third periods show certain similarities. This is referred to as the diagonal relationship.
    This is because the diagonally opposite neighbours have the same charge density and hence the same polarising power.

  • Question 18
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    Which of the following pairs contains an example of metalloid elements in the periodic table?
    Solution
    Boron and silicon are metalloid elements in the periodic table.
  • Question 19
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    Iron triad of elements also contains
    Solution
    Iron, nickel and cobalt make up the iron triad. They are called so because all the three have similar properties, even though they are distinct elements.
  • Question 20
    1 / -0
    Which of the following statements is correct?
    Solution
    The ionic radius of a metal is less than its atomic radius because metal forms positive ions due to low ionisation energy. Since positive ions are formed by loss of electrons from valence shells, but nuclear charge remains same, thus, the ionic radius of metal is smaller in size as compared to their source atom.
  • Question 21
    1 / -0
    The decreasing order of the first ionisation energies of the following elements is
    Solution
    First ionisation energy decreases as the stability of the configuration after the loss of first electron increases. So, the correct decreasing order of first ionisation energies is C > Be > B > Li.
  • Question 22
    1 / -0
    Directions: The following question has four choices out of which ONLY ONE is correct.

    Which of the following orders of elements is correct in terms of decreasing ionisation enthalpies?
    Solution
    Ionisation energy decreases on moving down a group in the periodic table. This is due to increase in the size of the atoms on moving down the group.
  • Question 23
    1 / -0
    Consider the iso-electronic series: K+, S2-, Cl- and Ca2+. There are four alternatives indicating the decreasing order of the radii of the ions. Choose the correct one.
    Solution
    For iso-electronic species, the ionic radii decreases as the nuclear charge increases.
    It increases with the increase in anionic charge and decreases with increase in the cationic charge.
    Hence, the series in the decreasing order of ionic radii are:
    S2- > Cl- > K+ > Ca2+
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