Questions and Answers
What is the electron configuration for an atom?
1s2, 2s2, 2p6...etc
How many electrons can the S, P, D, and F subshells hold?
What is the formula for the number of orbitals in each shell?
n^2
What is the formula to calculate the maximum number of electrons in every shell?
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How does the periodic table organize elements based on orbitals?
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What are the examples of electron configurations for standard and noble gas configurations?
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Which elements are exceptions in electron configuration due to their stability?
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What is the electron configuration for Sulfur (S)?
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What defines anions and cations?
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What is the difference between the ground state and excited state of an electron configuration?
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What distinguishes paramagnetic from diamagnetic substances?
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What are core electrons and valence electrons?
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Study Notes
Electron Configuration
- Electron configuration follows the sequence 1s², 2s², 2p⁶, etc., demonstrating the arrangement of electrons in orbitals.
Orbital Structure
- S orbitals: 1 orbital, can hold 2 electrons
- P orbitals: 3 orbitals, can hold 6 electrons
- D orbitals: 5 orbitals, can hold 10 electrons
- F orbitals: 7 orbitals, can hold 14 electrons
- Each shell can accommodate increasing types and numbers of orbitals as shell numbers increase.
Orbitals and Electrons
- Formula for orbital count per shell: n² (n is the shell number).
- Maximum electrons per shell formula: 2(n²), reflecting the total possible occupants across all subshells.
Periodic Table and Orbitals
- Periodic Table elements increase in atomic number, with each added proton also adding an electron in neutral atoms.
- Helium is placed next to hydrogen but behaves like a noble gas, influencing its orbital configuration.
Standard and Noble Gas Configurations
- Example for Bromine (Br):
- Standard: 1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁵
- Noble gas: [Ar] 4s², 3d¹⁰, 4p⁵
- Alkali metals end with s¹, alkaline earth with s², halogens with p⁵, and noble gases with p⁶.
Electron Configuration Exceptions
- Elements like Cu, Ag, Au, Cr, and Mo deviate from predicted configurations for energetic stability.
- Copper's configuration: [Ar] 4s¹, 3d¹⁰ instead of 4s², 3d⁹, stabilizing subshells.
Ions and Electron Configuration
- Sulfur's configuration: [Ne] 3s², 3p⁴ becomes [Ne] 3s², 3p⁶ for sulfide ion (S²⁻).
- Potassium ion (K⁺) loses an electron from the 4s orbital, resulting in [Ar].
- Zinc ion (Zn²⁺) removes its 4s electrons, leading to [Ar] 3d¹⁰.
Anions and Cations
- Anions are negatively charged ions formed by gaining electrons.
- Cations are positively charged ions formed by losing electrons.
Electron Configuration in Excited State
- Excited zinc configuration: Zn: [Ar] 4s¹, 3d¹⁰, 6p¹ after absorbing energy to promote electrons.
Ground State vs. Excited State
- Ground state represents an atom's lowest energy configuration.
- Excited state indicates an atom has absorbed energy, resulting in higher energy levels.
Magnetic Properties
- Paramagnetic materials have unpaired electrons and are attracted to magnetic fields.
- Diamagnetic materials have all paired electrons, showing slight deflection away from magnetic fields.
Core vs. Valence Electrons
- Core electrons are lower energy and not involved in bonding, while valence electrons are involved in chemical reactions.
- Valence electron examples: Sulfur has 6, potassium has 1, chromium has 6, bromine has 7, zinc has 2, and copper has around 1.
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Description
Test your knowledge on electron configurations and the distribution of electrons in various orbitals. This quiz covers essential concepts such as subshells and the number of electrons and orbitals for each shell. Perfect for students studying Chemistry.
