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Periodic Properties of Elements Test - 5

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Periodic Properties of Elements Test - 5
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Weekly Quiz Competition
  • Question 1
    1 / -0
    What is the collective name given to the elements of group 1, 2, 13, 14, 15, 16 , 17 and 18?
    Solution
    These elements of s and p blocks are collectively called representative elements.
  • Question 2
    1 / -0
    Which of the following elements do not belong to the same group, but show chemical similarities?
    Solution
    Be belongs to group 2 and Al belongs to group 13, but they have chemical similarity due to diagonal relationship.
  • Question 3
    1 / -0
    Which of the following elements is not correctly matched with its family?
    Solution
    Zinc is a transition metal and belongs to d- block of periodic table
  • Question 4
    1 / -0
    Which of the following isoelectronic ions has the lowest ionisation energy?
    Solution
    It has higher negative charge, so will have lower ionisation energy.
  • Question 5
    1 / -0
    Which of the following processes requires the highest energy?
    Solution
    Ionisation energy increases with increase in the effective nuclear charge.
    IE1 < IE2 < IE3
    Hence, option (2) is correct.
  • Question 6
    1 / -0
    Which of the following will have the highest second ionisation energy from the ground state of electronic configuration of various electrons?
    Solution
    1s2, 2s2, 2p6, 3s1 represents the configuration of sodium. After losing one electron, it acquires the stable electronic configuration of neon. Hence, the second ionisation energy will be exceptionally high.
  • Question 7
    1 / -0
    The ionisation energy of the element is the measure of
    Solution
    Higher IE means the electrons are more attracted towards the nucleus of the atom.
  • Question 8
    1 / -0
    Which of the following processes refers to IE2?
    Solution
    It refers to the conversion of unipositive ion to a dipositive ion in the gaseous state.
  • Question 9
    1 / -0
    On moving down the group, the ionisation energy decreases because of
    Solution
    Both these factors decrease the attractive pull of nucleus on outer most electrons and facilitate their removal.
  • Question 10
    1 / -0
    Which of the following configurations indicates fourth transition metal?
    Solution
    This correctly represents the fourth element with singly filled orbitals.
  • Question 11
    1 / -0
    Which of the following has the highest ionisation energy?
    Solution
    It has completely filled s orbital,so removal of electron from it is harder.
  • Question 12
    1 / -0
    In which of the following pairs is the ionisation energy of first species less than that of second?
    Solution
    P has higher IE due to stable half - filled configuration.
  • Question 13
    1 / -0
    Arrange S, P and As in order of increasing ionisation energy.
    Solution
    P and As belong to the same group, i.e. 15, whereas S belongs to group 16. Also, S and P belong to the same period. As P has exactly half filled orbitals. Therefore, As < S < P.
  • Question 14
    1 / -0
    What is the correct order of the size of the given species?
    Solution
    Atomic or ionic radius depends on the effective nuclear charge. Loss of an electron increases the effective nuclear charge and decreases the radius. Gain of an electron expands the radius due to electronic repulsions. Thus, the size of anion is larger and that of a cation is smaller than the neutral atom.
    Hence, the correct decreasing order of radii is:
    Cl- > Cl > Cl+
  • Question 15
    1 / -0
    Which of the following is the correct order of increasing ionic radii?
    Solution
    This is the correct order. Be2+ is from period 2, so its size is smaller. Also, Na+ is from group 1, so it is larger in size.
  • Question 16
    1 / -0
    The electronic configuration of elements of group 18 is represented by :
    Solution
    Completely filled s and p orbitals is the representation of group 18 , noble gases.
  • Question 17
    1 / -0
    General configuration of elements of transition metals belonging to d block is
    Solution
    D block Elements have a general electronic configuration of (n-1)d 1-10ns 1-2. These elements can find stability in half-filled orbitals and completely filled d orbitals.
  • Question 18
    1 / -0
    In transition elements, the incoming electron occupies (1-n)d subshell in preference to
    Solution
    The filling of the orbitals is in the order: ns, (n-1)d, np, so (n-1)d orbitals are filled before np orbital in transition elements.
  • Question 19
    1 / -0
    Which of the following configurations represents the most electropositive element?
    Solution
    Single electron of s orbital is easily removed, also it has 6 shells, so there is sheilding effect due to which the electron is easily removed.
  • Question 20
    1 / -0
    What information about the chemical nature of the element is given by the configuration 1s2 2s2 2p6 3s2?
    Solution
    It is an alkaline earth metal belonging to group 2 and period 3.
  • Question 21
    1 / -0
    Which of the following ions does not have the configuration of argon?
    Solution
    After addition of an electron, the configuration of iodine becomes equal to that of xenon.
  • Question 22
    1 / -0
    The general electronic configuration of transition elements is
    Solution
    The outer electrons in transition elements (d-block elements) may occupy the d subshell of the penultimate shell or the s subshell of the ultimate shell.
    The general valence shell electronic configuration of d-block elements is: (n-1)d 1-10 ns1-2

  • Question 23
    1 / -0
    The anion O2- is isoelectronic with
    Solution
    F- ion is isoelectronic with O2- ion.
    Both the ions have 10 electrons and the stable octet configuration of Neon: 2,8.
  • Question 24
    1 / -0
    Among the following which one is not isoelectric with the other species?
    Solution
    Isoelectric species have equal number of electrons. Out of the given species NO- has (7+ 8+1) = 16 electrons while rest have 14 electrons. Therefore, it is not isoelectric with other species.
  • Question 25
    1 / -0
    In which of the following binary compounds the ration r cation / r anion is the least?
    Solution
    The cation is very small and anion is large, so the ratio is the least.
  • Question 26
    1 / -0
    While moving from F to I, which of the following trends is observed?
    Solution
    The shells keep on adding with every period, so the size of atom increases from F to I.
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