Advertisements
Advertisements
प्रश्न
Assign the position of the element having an outer electronic configuration in the periodic table.
ns2 np4 for n = 3
Advertisements
उत्तर १
Since n = 3, the element belongs to the 3rd period. It is a p - block element since the last electron occupies the p - orbital.
There are four electrons in the p - orbital. Thus, the corresponding group of the element
= Number of s - block groups + number of d - block groups + number of p - electrons
= 2 + 10 + 4
= 16
Therefore, the element belongs to the 3rd period and 16th group of the periodic table. Hence, the element is Sulphur.
उत्तर २
n = 3
Thus element belongs to 3rd period, p-block element.
Since the valence shell contains = 6 electrons, group No = 10 + 6 = 16 configuration
=1s2 2s2 2p6 3s23p4 element name is sulphur.
APPEARS IN
संबंधित प्रश्न
Write the atomic number of the element present in the third period and a seventeenth group of the periodic table.
Use the periodic table to answer the following question.
Identify an element with five electrons in the outer subshell.
Use the periodic table to answer the following question.
Identify an element that would tend to gain two electrons.
Use the periodic table to answer the following question.
Identify the group having metal, non-metal, liquid as well as gas at room temperature.
Assign the position of the element having an outer electronic configuration in the periodic table.
(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.
Cu (belongs to period 4 and group 11)
Answer the following.
La belongs to group 3 while Hg belongs to group 12 and both belong to period 6 of the periodic table. Write down the general outer electronic configuration of the ten elements from La to Hg together using the orbital notation method.
Answer the following question.
The electronic configuration of some element is given below:
1s2
In which group and period of the periodic table the element is placed?
Consider the oxides Li2O, CO2, B2O3.
Which oxide would be the most acidic?
The first ionisation enthalpies of \[\ce{Na, Mg, Al}\] and \[\ce{Si}\] are in the order:
Which of the following sets contain only isoelectronic ions?
(i) \[\ce{Zn^{2+}, Ca^{2+}, Ga^{3+}, Al^{3+}}\]
(ii) \[\ce{K+ , Ca^{2+}, Sc^{3+}, Cl-}\]
(iii) \[\ce{P^{3-}, S^{2-}, Cl- , K+}\]
(iv) \[\ce{Ti^{4+}, Ar, Cr^{3+}, V^{5+}}\]
Identify the group and valency of the element having atomic number 119. Also predict the outermost electronic configuration and write the general formula of its oxide.
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?
How does the metallic and non-metallic character vary on moving from left to right in a period?
Justify the given statement with suitable examples— “the Properties of the elements are a periodic function of their atomic numbers”.
The electronic configuration of Pt (atomic number 78) is ______.
The IUPAC nomenclature of an element with electronic configuration [Rn] 5f146d17s2 is ______.
