Electronic Configuration
Chemistry ⇒ Atomic Structure and the Periodic Table
Electronic Configuration starts at 8 and continues till grade 12.
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Describe the difference between the electronic configuration of a neutral atom and its cation.
Describe the difference between the terms 'shell', 'subshell', and 'orbital' in the context of electronic configuration.
Explain why copper has an anomalous electronic configuration.
Explain why noble gases are chemically inert based on their electronic configuration.
Explain why the 4s electrons are removed before 3d electrons when transition metals form cations.
How many electrons are present in the 3rd shell (n=3) of a phosphorus atom?
How many electrons are present in the 4d subshell of a cadmium atom (atomic number 48)?
How many electrons are present in the 4f subshell of a gadolinium atom (atomic number 64)?
How many electrons are present in the valence shell of phosphorus (atomic number 15)?
How many electrons can be accommodated in all the orbitals having n = 3?
How many unpaired electrons are present in the ground state of an oxygen atom?
State Pauli’s exclusion principle.
State the Aufbau principle in your own words.
State the electronic configuration of the Al3+ ion.
State the electronic configuration of the S2- ion.
The electronic configuration 1s2 2s2 2p6 3s2 3p6 4s1 corresponds to which element?
The electronic configuration of an element is [Kr] 5s2 4d10 5p2. Identify the element.
What is the electronic configuration of a neutral sodium atom (atomic number 11)?
What is the total number of electrons in the p orbitals of a neon atom?
Which element has the electronic configuration [He] 2s2 2p2?
