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Classification of Elements and Periodicity in Properties
Which one of the element with the following outer orbital configuration may exhibit the largest number of oxidation states?
3d5,4s2
3d5,4s1
3d5,4s2
3d2,4s2
C.
3d5,4s2
A number of oxidation states exhibited by d-block elements is the sum of the number of electrons (unpaired) in d-orbitals and number of electrons in s - orbital.
a) 3d3, 4s2 ⇒ Oxidation state = 3+2 = 5
b) 3d5, 4s1 ⇒ Oxidation state = 5+1 = 6
c) 3d5, 4s2 ⇒ Oxidation state = 5+2 = 7
d) 3d4, 4s2 ⇒ Oxidation state = 2+ 2 = 4
Hence, an element with 3d5, 4s2 configuration exhibits the largest number of oxidation states.
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How many elements are present in:
(i) second period
(ii) fourth period
(iii) sixth period?
What is the name given to the s-block elements?
To which block the element with outer electronic configuration 4s23d10 belongs?
Why are there 10 elements in each series of d-block?
In terms of electronic configuration,
what is common in a given period and group?
Give the general electronic configuration of
(i) Transition elements (ii) Inner transition elements.
Name the group and period to which an element with Z = 15 belongs ?
What are the advantages of periodic classification of elements?
In the modern periodic table, the period indicates the value of:
(a) atomic number
(b) atomic mass
(c) principal quantum number
(d) azimuthal quantum number.
Which of the following statements related to the modern periodic table is incorrect?
(a) The p-block has 6 columns, because a maximum of 6 electrons can occupy all the orbitals in a p-shell.
(b) The d-block has 8 columns, because a maximum of 8 electrons can occupy all the orbitals in a d-subshell.
(c) Each block contains a number of columns equal to the number of electrons that can occupy that subshell.
(d) The block indicates value of azimuthal quantum number (l) for the last subshell that received electrons in building up the electronic configuration.
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