Advertisements
Advertisements
Question
Use the periodic table to answer the following question.
Identify an element with five electrons in the outer subshell.
Solution
The electronic configuration of an element having 5 electrons in its outermost subshell should be ns2np3. This is the electronic configuration of the halogen group. Thus, elements in this group include nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi).
APPEARS IN
RELATED QUESTIONS
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 that would tend to lose two electrons.
Use the periodic table to answer the following question.
Identify an element that would tend to gain two electrons.
Assign the position of the element having an outer electronic configuration in the periodic table.
ns2 np4 for n = 3
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)
Write the outer electronic configuration of the following using the orbital notation method. Justify.
Po (belongs to period 6 and group 16)
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?
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?
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) \[\ce{Ti^{4+}, Ar, Cr^{3+}, V^{5+}}\]
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”.
Write down the outermost electronic configuration of alkali metals. How will you justify their placement in group 1 of the periodic table?
