Podcast
Questions and Answers
Which element has a larger atomic radius?
Which element has a larger atomic radius?
- F
- Rb (correct)
- Na
- Cl
What phenomenon causes cations to be smaller than their parent atoms?
What phenomenon causes cations to be smaller than their parent atoms?
- Loss of electrons leading to less electron-electron repulsion (correct)
- Increased electron repulsion
- Decreased nuclear charge
- Additional energy levels being added
Which ion is larger than its neutral atom?
Which ion is larger than its neutral atom?
- Cl-
- O2- (correct)
- Mg2+
- K+
Which of the following trends describes the atomic radius as you move down a group in the periodic table?
Which of the following trends describes the atomic radius as you move down a group in the periodic table?
Why does the electronegativity generally decrease as you move down a group in the periodic table?
Why does the electronegativity generally decrease as you move down a group in the periodic table?
What is the maximum number of electrons that can occupy a single orbital?
What is the maximum number of electrons that can occupy a single orbital?
Which principle states that electrons fill lower energy levels before higher ones?
Which principle states that electrons fill lower energy levels before higher ones?
What distinguishes paramagnetic substances from diamagnetic substances?
What distinguishes paramagnetic substances from diamagnetic substances?
What is the term for the state where an electron configuration deviates from the ground state by having higher energy levels filled?
What is the term for the state where an electron configuration deviates from the ground state by having higher energy levels filled?
Which rule describes how electrons are distributed between degenerate orbitals?
Which rule describes how electrons are distributed between degenerate orbitals?
Which of the following configurations corresponds to a stable state?
Which of the following configurations corresponds to a stable state?
What do valence electrons determine about an element's chemical properties?
What do valence electrons determine about an element's chemical properties?
Flashcards
Atomic Radius
Atomic Radius
A measure of the size of an atom, representing how close electrons are to the nucleus.
Cation vs Atom Size
Cation vs Atom Size
Cations are smaller than their corresponding neutral atoms because losing electrons reduces electron-electron repulsion, pulling the remaining electrons closer to the nucleus.
Anion vs Atom Size
Anion vs Atom Size
Anions are larger than their corresponding neutral atoms due to the addition of electrons, increasing electron-electron repulsion and pushing the electron cloud further out.
Zeff
Zeff
Signup and view all the flashcards
Electron Energy Levels
Electron Energy Levels
Signup and view all the flashcards
Quantum Numbers
Quantum Numbers
Signup and view all the flashcards
Aufbau Principle
Aufbau Principle
Signup and view all the flashcards
Hund's Rule
Hund's Rule
Signup and view all the flashcards
Pauli Exclusion Principle
Pauli Exclusion Principle
Signup and view all the flashcards
Ground State
Ground State
Signup and view all the flashcards
Excited State
Excited State
Signup and view all the flashcards
Valence Electrons
Valence Electrons
Signup and view all the flashcards
Paramagnetic
Paramagnetic
Signup and view all the flashcards
Study Notes
Chem 161 Exam 3
- Exam 3 is on Thursday, November 21st
- Focus on chapters 7, 8, and 9
- A quarter of the exam will include review questions from previous material
- No assignments due on Saturday
Exam 3 Details
- Bring a pencil, photo ID, and calculator
- A photo ID is required to submit the exam
- Room assignments are based on last name
- Students with last names A-L go to SPAL 155
- Students with last names M-Z go to BIL 152
Guest Speaker Information
- Billy Pieper, Director of Strategic Partnerships and Mortgage at ASB
- Senior Vice President and Director of Strategic Partnerships for American Savings Bank
- Played college football and baseball at UCLA
- Professional baseball with the Kansas City Royals
- Master of Business Administration degree from the University of Hawaii at Mānoa
- Shares financial knowledge with University of Hawaii students at Ma'noa's Shidler College of Business
- Hui Kapili - Building a better Hawai`i together
Schrödinger Equation
- Input: Quantum numbers (n, l, m, ml)
- Output: Probability map showing where an electron can exist in an atom (orbital)
- The Schrödinger equation describes how electrons exist in atoms
Periodic Table
- Periodic table used to determine electron orbital patterns
- s, p, d, f blocks
- Full, empty, or half-filled electron shells tend to be more stable
- Example: Ca: [Ar]4s2 Cr: [Ar]4s13d5
- valence electrons primarily determine element properties
- Electron configuration defines how electrons fill atomic orbitals
Rules for Electron Orbital Filling
- Pauli Exclusion Principle: No two electrons can have the same four quantum numbers (n, l, ml, ms). Maximum of 2 electrons per orbital.
- Aufbau Principle: Electrons fill lower energy levels first (ground state).
- Hund's Rule: When filling degenerate orbitals (same energy), electrons fill each orbital individually before pairing up.
Ground State vs. Excited State Configurations
- Configurations following all rules are ground state
- Configurations that violate the rules are excited state
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Related Documents
Description
Prepare for your upcoming Chem 161 Exam 3 by focusing on chapters 7, 8, and 9. This exam will also include review questions from previous material, so be sure to review past content. Remember to bring the necessary materials and check your room assignments based on your last name.
