Electrical Engineering & Electronics /Electron Configuration Flashcards
Electron Configuration Flashcards
This deck covers key concepts related to electron configurations, including principles, rules, and exceptions in atomic structure.
What does electron configuration show
Shows the arrangement of electrons in the atom of an element
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Key Terms
Term
Definition
What does electron configuration show
Shows the arrangement of electrons in the atom of an element
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List the energy levels
4f
4d
4p
3d
4s
3p
3s
2p
2s
1s
How many electrons can the S orbital hold
2
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How many electrons can the P orbital hold
6
How many electrons can the d orbital hold
10
What is the Aufbau principle
When building up the electrons configuration of an atom in its ground state, electrons occupy the lowest available energy level where possible
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| Term | Definition |
|---|---|
What does electron configuration show | Shows the arrangement of electrons in the atom of an element |
List the energy levels | 4f
4d
4p
3d
4s
3p
3s
2p
2s
1s |
How many electrons can the S orbital hold | 2 |
How many electrons can the P orbital hold | 6 |
How many electrons can the d orbital hold | 10 |
What is the Aufbau principle | When building up the electrons configuration of an atom in its ground state, electrons occupy the lowest available energy level where possible |
What is the Hunds rule of multiplicity | States that when two or more orbitals of equal energy are available, the electrons occupy them singly before filling them in pairs |
What is the Pauli exclusion principle | States that no more than two electrons can occupy an orbital and they must have opposite signs |
Why do electrons fill the 4s sublevel before the 3d sublevel | The 4s sublevel is lower in energy than the 3d sublevel.
electrons fill the lowest available sub-levels first. |
Why are Cu and Cr different | They both have only one electron in the S orbital because the d block is more stable when half or completely filled |
Periodic table divided into what four blocks | S block, P block, D block, F block |
What determines a elements place in a block | All the elements in the s block have their outer electrons in a s sub level, all those in the P block have their outer elements in a P orbital |
What is the outer shell called | Valence shell |
Why does the electrons of Cr and Cu start filling up the 3d orbital before the 4s orbital is full? | This is because if an orbital is exactly half filled or completely filled then it gives the atom extra stability |
What is a ion | A charged atom |
What elements are an expectation to the Albafu principle | Cr and Cu |
What is an atomic orbit | Bohr believed that electrons moved around the nucleus in fixed paths called orbits |
What is atomic orbital | The region of space where there is a high possibility of finding an electron |
How is a transition element identified from its s.p configuration? | Transition elements form at least one ion that has an incomplete 3d sublevel |