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Classification of Elements and Periodicity in Properties Test - 30

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Classification of Elements and Periodicity in Properties Test - 30
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  • Question 1
    1 / -0
    In FF and ClCl  which one has higher electron affinity :
    Solution
    ClCl has higher affinity thanF F because it can accommodate the incoming electron more easily thanF.F F. F has small size and there will be repulsions for incoming electrons.
  • Question 2
    1 / -0
    State the electronic configuration for Helium [p=2, n=2p=2,\ n=2].
  • Question 3
    1 / -0
    Refer to changes in properties of elements  on moving left to right across a period of the periodic table.For each property , choose the letter corresponding to the correct answer from A,B,C and D.

    The electron affinity of the elements in groups 1 to 7 :
    Solution
    As we move from left to right, tendency of elements to accept electron and completes theri octet increases so electron affinity increases.

  • Question 4
    1 / -0

    Identify the elements in the Periodic Table:

    A: Which shows diagonal relationship to BeBe

    B: Which shows diagonal relationship to LiLi

    Solution
    In addition to horizontal and vertical trends, there is a diagonal relationship between elements such as LiLi and MgMg, BeBe and Al,BAl, B and SiSi, that have an adjacent upper left/lower right relative location in the periodic table. 
    These pairs of elements have similar size and electronegativity, resulting in similar properties.
  • Question 5
    1 / -0
    An element in period 3 whose electron affinity is zero is:
    Solution
    Electron affinity is defined as the change in energy (in kJ/mole) of a neutral atom (in the gaseous phase) when an electron is added to the atom to form a negative ion.In other words, the neutral atom's likelihood of gaining an electron.
    Argon has ns2p6ns^2p^6 configuration, an octet is complete so it does not have any tendency to gain an electron and they have zero electron affinity.

  • Question 6
    1 / -0
    Atomic number of an element XX is 1616 its group number will be :
    Solution
    Element X has configuration of 2,8,6 so it has 6 electron in outmost shell and it belongs to group 16.
  • Question 7
    1 / -0
    'Electronic configuration' represents :
    Solution
    The electronic configuration of an atom shows the number of electrons in each sublevel in each energy level of the ground-state atom. To determine the electronic configuration of a particular atom, start at the nucleus and add electrons one by one until the number of electrons equals the number of protons in the nucleus.

  • Question 8
    1 / -0
    Match the statements in List I with the correct answers in list II
    List IList II
    1. The basic unit of matterA: Proton
    2. The sub-atomic particle with a positive chargeB: Neon
    3. An atom having stable electronic configurationC: Oxygen
    4. A molecule formed by sharing of electron [covalency]D: Sodium
    5. A metallic atom having unstable electronic configurationE: Atom
    Solution
    Atoms are the basic building blocks of matter that make up everyday objects.
    Proton has a positive charge of +1.
    An atom having stable electronic configuration is neon as its octet is complete.
    A molecule formed by sharing of electron is oxygen as it is formed by sharing of two electrons by each oxygen atom.
    A metallic atom having unstable electronic configuration is sodium as its outer shell is incomplete 1s22s2p63s11s^2 2s^2p^6 3s^1
  • Question 9
    1 / -0
    Which element  is considered radioactive among the options given below?
    Solution
    an element subject to spontaneous degeneration of its nucleus accompanied by the emission of alpha particles, beta particles, or gamma rays. All elements with atomic numbers greater than 8383 are radioactive. Naturally occurring radioactive elements include radium, thorium, and uranium. Several radioactive elements not found in nature have been produced by the bombardment of stable elements with subatomic particles in a cyclotron.
  • Question 10
    1 / -0
    Electron affinity on moving down the group in the periodic table:
    Solution
     Electron affinity reflects the ability of an atom to accept an electron. It is the energy change that occurs when an electron is added to a gaseous atom. Atoms with stronger effective nuclear charge have greater electron affinity. Electron affinity decreases moving down a group.
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