19,000+ solved questions for JEE Advanced, JEE Mains, NEET & IChO — with answers and expert explanations.
When a chlorine atom becomes chloride ion, its size
Which of the following order is correct for the size of Fe³⁺, Fe, and Fe²⁺?
The electronic configuration of the element which is just above the element with atomic number 43 in the same group is ............
The last element of the p-block in the 6th period is represented by the outermost electronic configuration.
The element with the lowest atomic number that has a ground state electronic configuration of (n-1) d6ns2 is located in the
The number of elements present in fifth period of Periodic Table is
The ions O₂–, F–, Na⁺, Mg2+and Al3+are isoelectronic. Their ionic radii show
Amongst the elements with the following electronic configurations which one of them may have the highest ionization energy?
The correct order of decreasing electronegativity values among the elements I-beryllium, II-oxygen, III-nitrogen and IV-magnesium, is (Kerala CEE 2011)
The transition elements have a characteristic electronic configuration which can be represented as
The elements with atomic numbers 9, 17, 35, 53, 85 are all
Molybdenum metal is related to which block?
Elements whose outer electronic configuration vary from ns2np1 to ns2np6 constitute
Which one of the following pair of elements has similar properties?
ns and ns outermost electronic configuration belongs to the
Which of the following is not a Dobereiner’s triad?
The correct order of decreasing first ionisation potential is (UP CPMT 2013)
The basis of modern periodic table is
The element with atomic number 57 belongs to
Which of the following ions has the smallest radius?
The element with lowest electron gain enthalpy is:
The most ionic compound will be formed between:
The element with highest I.E. is:
Assertion: Generally, ionization enthalpy increases from left to right in a period. Reason: When successive electrons are added to the orbitals in the same principal quantum level, the shielding effect of the inner co…
Assertion: Electron gain enthalpy becomes less negative as we go down a group. Reason: The size of the atom increases on going down the group and the added electron would be farther from the nucleus.