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Questions and Answers
What is electronic configuration?
What is electronic configuration?
Electronic configuration is the arrangement of electrons in shells and subshells around the nucleus of an atom, ordered by increasing energy levels.
Which subshell is filled first in the electronic configuration?
Which subshell is filled first in the electronic configuration?
The s subshell is filled first.
What is the maximum number of electrons that the M shell can hold?
What is the maximum number of electrons that the M shell can hold?
The M shell can hold a maximum of 18 electrons.
How many electrons can a p subshell accommodate?
How many electrons can a p subshell accommodate?
What is the electronic configuration of a sodium ion (Na+)?
What is the electronic configuration of a sodium ion (Na+)?
Describe the electronic configuration for Mg2+.
Describe the electronic configuration for Mg2+.
By what process do electrons fill the subshells?
By what process do electrons fill the subshells?
What is the significance of the ground state configuration?
What is the significance of the ground state configuration?
What is the electronic configuration for Al3+?
What is the electronic configuration for Al3+?
Why do Na+, Mg2+, and Al3+ have the same electronic configuration?
Why do Na+, Mg2+, and Al3+ have the same electronic configuration?
Flashcards
Electronic Configuration
Electronic Configuration
Arrangement of electrons around an atom's nucleus.
K shell
K shell
Electron shell closest to the nucleus, holding a maximum of 2 electrons.
L shell
L shell
Electron shell, next to the nucleus, holding a maximum of 8 electrons.
s subshell
s subshell
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p subshell
p subshell
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Ground state electronic configuration
Ground state electronic configuration
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Ion electronic configuration
Ion electronic configuration
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Maximum electrons in shells (K, L)
Maximum electrons in shells (K, L)
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Ion Example: Na+
Ion Example: Na+
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Electron Filling Sequence
Electron Filling Sequence
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Study Notes
Electronic Configuration
- Electronic configuration describes the arrangement of electrons around an atom's nucleus in different energy levels (shells and subshells).
- Electrons fill shells and subshells in order of increasing energy.
- The lowest energy levels are filled first.
- Subshells within a shell have slightly differing energies. 's' subshells are filled first, then 'p', followed by 'd' and 'f'.
Maximum Capacity
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K shell accommodates 2 electrons.
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L shell accommodates 8 electrons.
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M shell accommodates 18 electrons.
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N shell accommodates 32 electrons.
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's' subshell holds 2 electrons.
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'p' subshell holds 6 electrons.
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'd' subshell holds 10 electrons.
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'f' subshell holds 14 electrons.
Basic Requirements
- Know the number of electrons in the atom.
- Understand the order of shells and subshells based on energy levels.
- Know the maximum number of electrons each shell and subshell can hold.
Examples (Na+, Mg2+, Al3+)
- Na+ has 10 electrons, with configuration: 2, 8 in shells (K, L). In terms of sub-shells: 1s2, 2s2, 2p6
- Mg2+ has 10 electrons, with configuration: 2, 8 in shells (K, L). In terms of sub-shells: 1s2, 2s2, 2p6
- Al3+ has 10 electrons, with configuration: 2, 8 in shells (K, L). In terms of sub-shells: 1s2, 2s2, 2p6
- All three ions have the same number of electrons in their outermost shell (8).
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