Questions and Answers
What are orbitals?
A region or volume where the electron is most likely to be found.
How many electrons can each orbital hold?
2
What is a wave function?
What is the maximum number of electrons in the 1st energy level?
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What is the structure of the 2nd energy level?
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What does the 3rd energy level consist of?
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How many orbitals are in sublevel S?
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How many orbitals are in sublevel P?
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How many orbitals are in sublevel D?
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How many orbitals are in sublevel F?
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Describe the shape of an S sublevel.
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Describe the shape of a P sublevel.
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Describe the shape of a D sublevel.
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Give the electronic configuration of lithium.
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Electronic configuration of Boron?
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Electronic configuration of Scandium?
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Electronic configuration of Gallium?
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What does a box or line represent?
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What do the arrows represent?
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Orbital diagram for helium?
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Orbital diagram for lithium?
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What does the Pauli exclusion principle state?
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What does the Aufbau principle state?
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How do you use the noble gas configuration?
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Noble gas configuration of Boron?
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Noble gas configuration of Iron?
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What is the ground state configuration?
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What are cations?
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What are anions?
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Where can you only lose valence electrons?
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Give the configuration of the anion Se²⁻.
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Give the configuration of the cation Ca²⁺.
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What does isoelectric mean?
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Give an example of two isoelectric elements.
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Study Notes
Orbitals and Electrons
- Orbitals indicate regions in space where electrons are likely to be found.
- Each orbital can hold a maximum of 2 electrons, categorized into types: s, p, d, and f.
- The 1st energy level contains one 1s orbital capable of holding 2 electrons, with no other orbital types available.
- The 2nd energy level has one 2s and three 2p orbitals (2s, 2px, 2py, 2pz), accommodating up to 8 electrons total.
- The 3rd energy level consists of one 3s, three 3p, and five 3d orbitals, allowing up to 18 electrons.
Sublevels and Shapes
- Sublevel s contains 1 orbital, with a spherical shape.
- Sublevel p has 3 orbitals, shaped like dumbbells.
- Sublevel d consists of 5 unique orbitals, while sublevel f contains 7 orbitals.
Electronic Configurations
- Lithium has the configuration 1s²2s¹.
- Boron is represented as 1s²2s²2p¹.
- Scandium's configuration is 1s²2s²2p⁶3s²3p⁶4s²3d¹.
- Gallium's configuration is 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p¹.
- The configuration for the anion Se²⁻ is 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶.
Orbital Diagrams
- A box or line represents an orbital in diagrams.
- Arrows illustrate electron spins: ↑ for one spin direction and ↓ for the opposite direction.
- Helium's orbital diagram shows two electrons with opposite spins (↑↓), while lithium's shows one paired and one unpaired (↑↓ ↑).
Principles and Exclusions
- The Pauli Exclusion Principle states that an orbital can hold 2 electrons with opposite spins.
- The Aufbau Principle dictates that electrons fill from the lowest to highest energy levels.
- Noble gas configuration starts with a noble gas symbol in brackets, continuing from there for electron configuration.
Ions and Charges
- Cations (positively charged) result from the loss of electrons, while anions (negatively charged) are formed by the gain of electrons.
- The ground state configuration indicates the lowest energy arrangement of electrons.
- Isoelectronic species possess the same number of electrons and thus identical electronic configurations; for example, Ca²⁺ and Argon both share the configuration 1s²2s²2p⁶3s²3p⁶.
Valence Electrons
- Valence electrons can only be lost from the outermost energy levels during ion formation.
- For cation Ca²⁺, the configuration changes after losing 2 electrons, while the anion Se²⁻ gains electrons to fill its outer shell.
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Test your knowledge of atomic structure with these flashcards! This quiz covers key concepts such as orbitals, their capacity, and wave functions, providing a solid foundation in atomic theory. Perfect for students preparing for chemistry exams!