Advertisements
Advertisements
Question
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) \[\ce{Ti^{4+}, Ar, Cr^{3+}, V^{5+}}\]
Solution
(ii) \[\ce{K+ , Ca^{2+}, Sc^{3+}, Cl-}\]
(iii) \[\ce{P^{3-}, S^{2-}, Cl- , K+}\]
Explanation:
(a) \[\ce{Zn^{2+}}\] (30 – 2 = 28), \[\ce{Ca^{2+}}\] (20 – 2 = 18), \[\ce{Ga^{3+}}\] (31 – 3 = 28), \[\ce{Al^{3+}}\] (13 – 3 = 10) are not isoelectronic.
(b) \[\ce{K+}\] (19 – 1 = 18), \[\ce{Ca^{2+}}\] (20 – 2 = 18), \[\ce{Sc^{3+}}\] (21 – 3 = 18), \[\ce{Cl-}\] (17 + 1 = 18) are isoelectronic.
(c) \[\ce{P^{3-}}\] (15 + 3 = 18), \[\ce{S^{2-}}\] (16 + 2 = 18), \[\ce{Cl-}\] (17 + 1 = 18), K+ (19 – 1 = 18) are isoelectronic.
(d) \[\ce{Ti^{4+}}\] (22 – 4 = 18), \[\ce{Ar}\] (18), \[\ce{Cr^{3+}}\] (24 – 3 = 21), \[\ce{V^{5+}}\] (23 – 5 = 18) are not isoelectronic.
APPEARS IN
RELATED QUESTIONS
Use the periodic table to answer the following question.
Identify an element that would tend to lose two electrons.
Assign the position of the element having an outer electronic configuration in the periodic table.
(n - 1)d2 ns2 for n = 4
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?
The first ionisation enthalpies of \[\ce{Na, Mg, Al}\] and \[\ce{Si}\] are in the order:
The period number in the long form of the periodic table is equal to ______.
In the modern periodic table, elements are arranged in order of increasing atomic numbers which is related to the electronic configuration. Depending upon the type of orbitals receiving the last electron, the elements in the periodic table have been divided into four blocks, viz, s, p, d and f. The modern periodic table consists of 7 periods and 18 groups. Each period begins with the filling of a new energy shell. In accordance with the Arfbau principle, the seven periods have 2, 8, 8, 18, 18, 32 and 32 elements respectively. The seventh period is still incomplete. To avoid the periodic table being too long, the two series of f-block elements, called lanthanoids and actinoids are placed at the bottom of the main body of the periodic table.
The electronic configuration of the element which is just above the element with atomic number 43 in the same group is ______.
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?
E.N. of Si is ______. (Covalent radius of Si = 1.175 Å)
\[\ce{_92U^235}\] is a member of VI B group. The new element formed by the emission of α-particle will be a member of ______ group.
