Test: Periodic Trends - JEE MCQ
20 Questions MCQ Test - Test: Periodic Trends
The first ionisation energies of magnesium and aluminium are respectively given by
of 
of 
has stable configuration (fulfilled) than 
so removal of an electron is difficult hence, required more energy i.e. more ionisation energy.| 1 Crore+ students have signed up on EduRev. Have you? Download the App |
Electron gain enthalpy values of noble gases are positive because:
The formation of the oxide ion 
, from oxygen atom requires first an exothermic and then an endothermic step as shown below:
Thus process of formation of 
in gas phase is unfavourable even though 
is isoelectronic with neon. It is due to the fact that
shell, also negative charge on oxygen 
is another factor due to which incoming electron feel repulsion. Hence electron repulsion outweigh the stability gained by achieving noble gas configuration.(i) Atomic radii decreases across a row of the periodic table when we move from left to right.
(ii) Atomic radii increases down the column as we move from top to bottom.
(iii) Although the order of elements is based on atomic numbers, vertical families share similar chemical properties.
Which of the statement(s) given above is/are correct?
Consider the following changes
and 
The energy required to pull out the two electrons are 
and 
respectively. The correct relationship between two energies would be
is always less than 
.Ionization energies of atoms A and B are 400 and 
cal 
respectively. The electron affinities of these atoms are 
and 
cal 
respectively. Then which is the correct statement regarding electronegativity 
.
as the electronic configuration. Which one of the following statements regarding this element is not correct?
Which of the following series correctly represents relations between the elements from 
to 
Elements X, Y and Z have atomic numbers 19,37 and 55 respectively. Which of the following statements is true about them ?
and As is
'-orbitals due to which it has higher electron affinity than nitrogen. As also has vacant 
-orbitals but its atomic size is very big thus its electron affinity will be lesser than 
.Identify the element which has highest second ionisation enthalpy.
increases and so do the ionisation energy and moving down a group, effective nuclear charge 
decreases and so do the ionisation energy. So, phosphorus belonging to 3 rd period will have less ionisation energy than 2nd period elements.
is greater than 
as 
has half-filled stable electronic configuration, but after the removal of 1 electron, oxygen acquires a half-filled stable electronic configuration, the second ionisation potential of oxygen becomes more than of 
and 
.Which property decreases from left to right across the periodic table and increases from top to bottom?
(i) Atomic radius
(ii) Electronegativity
(iii) Ionisation energy
(iv) Metallic character
N0/4 atoms of X(g) are converted into X+(g) by energy E1. N0 /4 atoms of X(g) are converted into X–(g) by energy E2. Hence, ionisation potential and electron affinity of X(g) are :
TThe formation of the oxide ion O2−(g) requires first an exothermic and then an endothermic step as shown below. 
This is because
The electronic configuration of elements A,B and C are [He]2s1, [Ne]3s1 and [Ar] 4s1 respectively, which one of the following order is correct for the first ionization potentials (in kJmol−1) of A,B and C ?
and 
elements decreases with the ease of removal of electron from 
to 
. Atomic size increase from 
to 
, hence ionisation potential decrease in the same order.
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