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Classification of Elements and Periodicity in Properties Test - 38

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Classification of Elements and Periodicity in Properties Test - 38
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  • Question 1
    1 / -0
    A newly discovered element XX is placed in group IAIA of the periodic table since it forms :
    Solution

    The elements in group I of the periodic table are called the alkali metals. They form ionic compounds when they react with non-metals. Their ions have a single positive charge. For example, sodium forms sodium ions, Na+Na^+.

    The elements in Group 7 of the Periodic Table are called the halogens. They form ionic compounds when they react with metals. Their ions have a single negative charge. For example, chlorine forms chloride ions, ClCl^-.

    Group 1A1A elements form XClXCl type chloride.

  • Question 2
    1 / -0
    Element AA has electronic configuration 2,8,1 and BB has 2,8,7. Which one will have higher electron affinity?
    Solution
    B has 77 electrons in the outermost shell so it tends to accept one to complete the octet. Also, A has 11 electron in the outermost shell, so it tends to donate to complete octet. Thus B has a higher affinity towards electrons.
  • Question 3
    1 / -0
    Which of the following metal forms amphoteric oxide?
    Solution
    An amphoteric oxide is a substance that can chemically react as either acid or base. Aluminium oxide shows acid and basic properties of oxide so it is amphoteric. Thus, Al2O3Al_2O_3 entails the marking point at which a change over from a basic oxide to acidic oxide occurs.
  • Question 4
    1 / -0
    The element with highest electron affinity in the periodic table is:
    Solution
    As an exception to the rule, Cl has higher EA as compared to F. Fluorine has very small atomic size and this makes the fluoride anion unstable due to very high charge/mass ratio. F has no d orbitals so it has small atomic size. F has EA less than that of Cl.
  • Question 5
    1 / -0
    On the four halogens, the one which has the highest electrons affinity is_______.
    Solution
    Fluorine, though higher than chlorine in the periodic table, has a very small atomic size. This makes the fluoride anion so formed unstable (highly reactive) due to a very high charge/mass ratio. The electron being gained by fluorine would be taken in to a much smaller 2p orbital and requires more electron coupling energy than that of much larger 3p orbital of chlorine. Therefore, there are more repulsions in smaller 2p orbital and it has lower electron affinity than chlorine.
  • Question 6
    1 / -0
    Which of the following has the highest electron affinity?
    Solution
    Electron affinity is defined as the change in energy of a neutral atom when an electron is added to the atom to form a negative ion, i.e., an atom gains the electron. Electron affinity decreases down the group but ClCl has more affinity than FF because of the smaller size of fluorine.
  • Question 7
    1 / -0
    Which of the following burns to form an oxide, which is gaseous at room temperature?
    Solution
    H2+O2H2O(l)H_2+O_2 \rightarrow H_2O(l)
    P+O2P4O10(s)P+O_2 \rightarrow P_4O_{10}(s)
    Ca+O2CaO(s)Ca+O_2 \rightarrow CaO(s)
    S+O2SO2(g)S+O_2 \rightarrow SO_2(g)
  • Question 8
    1 / -0
    Which of the following property generally decrease along a period?
    Solution
    Metallic character decreases on moving across the periodic table from left to right. This occurs as atoms more readily accept electrons to fill a valence shell than lose them to remove the unfilled shell.
  • Question 9
    1 / -0
    Electron affinity depend on :
    Solution
    Electron affinity is the amount of energy released when an electron is added to a neutral atom to form a negative ion. EA decreases on moving down the group as the atomic size increases and net nuclear charge increase is offset by extra screening electrons as the additional electron enters an orbital away from the nucleus. So, it is less attracted to nucleus and would release less energy when added.
  • Question 10
    1 / -0
    The elements with atomic numbers 2,10,18,36,542, 10, 18, 36, 54 and 8686 are all______.
    Solution
    Noble gases have stable configuration in their outermost shell.
    2=2
    10=2,8
    18=2,8,8
    36=2,8,8,18
    54=2,8,8,18,18
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