Multiple Choice QuestionsIdentify the correct statement.
Lead forms compounds in +2 oxidation state due to inert pair effect.
All halogens show only negative oxidation state.
Catenation property increases from boron to oxygen.
Oxadation state of oxygen is - 1 in ozonides.
An element has [Ar] 3d1 configuration in its +2 oxidation state. Its position in the periodic table is
period - 3, group - 3
penod - 3, group - 7
period - 4, group - 3
period - 3, group - 9
C.
period - 4, group - 3
Electronic configuration of the element in +2 oxidation state is [Ar] 3d1. This electronic configuration is obtained after losing 2 electrons.
Atomic number of the element
= Atomic number of Ar + 1 + 2
= 18 + 1 + 2
= 21
Thus, element is Scandium. It is a d-block element. The electronic configuration of Sc = [Ar] 3d1 4s2.
Here, n = 4; therefore, it belongs to 4th period.
Group = Total number of valence shell electrons = 3
So, the element belongs to period - 4 and group - 3.
Out of the following electronic configurations the one of a transition element, is
1s2, 2s2 2p6, 3s2 3p6 3d10, 4s2 4p6
1s2, 2s2 2p6, 3s2 3p6 3d3, 4s2
1s2, 2s2 2p6, 3s2 3p6, 4s2
1s2, 2s2 2p6, 3s2 3p6 3d10, 4s2 4p1
The element with atomic number 55 belongs to which block of the periodic table?
s-block
p-block
d-block
f-block
To which block is related an element having electronic configuration 1s2, 2s2 2p6, 3s2 3p6 3d10, 4s1 in the periodic table?
s-block
p-block
d-block
f-block
The electronic configuration of an element is 1s2, 2s2, 2p6, 3s2 3p6, 3d10, 4s2 4p3. Its properties would be similar to which of the following elements?
Boron
Oxygen
Nitrogen
Chlorine
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