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प्रश्न
Use the periodic table to answer the following question.
Identify an element that would tend to lose two electrons.
उत्तर १
An element having two valence electrons will lose two electrons easily to attain the stable noble gas configuration. The general electronic configuration of such an element will be ns2. This is the electronic configuration of group 2 elements. The elements present in group 2 are Be, Mg, Ca, Sr, Ba.
उत्तर २
Element belonging to alkaline earth family (group 2) e.g., magnesium
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संबंधित प्रश्न
Write the atomic number of the element present in the third period and a seventeenth group of the periodic table.
Assign the position of the element having an outer electronic configuration in the periodic table.
ns2 np4 for n = 3
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(n - 1)d2 ns2 for n = 4
Assign the position of the element having an outer electronic configuration in the periodic table.
(n - 2) f7 (n - 1)d1 ns2 for n = 6
Write the outer electronic configuration of the following using the orbital notation method. Justify.
Ge (belongs to period 4 and group 14)
Answer the following.
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Answer the following question.
The electronic configuration of some element is given below:
1s2 2s2 2p6
In which group and period of the periodic table the element is placed?
Answer the following question.
For s-block and p-block elements show that the number of valence electrons is equal to its group number.
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The period number in the long form of the periodic table is equal to ______.
How would you explain the fact that first ionisation enthalpy of sodium is lower than that of magnesium but its second ionisation enthalpy is higher than that of magnesium?
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\[\ce{_92U^235}\] is a member of VI B group. The new element formed by the emission of α-particle will be a member of ______ group.
The IUPAC nomenclature of an element with electronic configuration [Rn] 5f146d17s2 is ______.
