Electronic Configuration
Chemistry ⇒ Atomic Structure and the Periodic Table
Electronic Configuration starts at 8 and continues till grade 12.
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See sample questions for grade 10
Describe Hund's Rule of Maximum Multiplicity.
Explain why copper (Cu, atomic number 29) has an electronic configuration of [Ar] 4s1 3d10 instead of [Ar] 4s2 3d9.
Explain why the 4s orbital is filled before the 3d orbital.
How many electrons are present in the 2p subshell of a nitrogen atom (atomic number 7)?
How many electrons are present in the 3p subshell of phosphorus (atomic number 15)?
How many electrons are present in the valence shell of magnesium (Mg, atomic number 12)?
How many unpaired electrons are present in the ground state of nitrogen (atomic number 7)?
State the electronic configuration of a chloride ion (Cl-, atomic number 17).
State the electronic configuration of a sulfur atom (atomic number 16).
State the maximum number of electrons that can be accommodated in a d-subshell.
State the Pauli Exclusion Principle.
What is the electronic configuration of potassium (K, atomic number 19)?
What is the electronic configuration of sodium (Na, atomic number 11)?
What is the general electronic configuration of halogens?
What is the general electronic configuration of noble gases?
What is the valence shell electronic configuration of an alkali metal?
