Chem 161 Exam 3 Review

Which element has a larger atomic radius?

What phenomenon causes cations to be smaller than their parent atoms?

Which ion is larger than its neutral atom?

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?

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?

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?

Which rule describes how electrons are distributed between degenerate orbitals?

Which of the following configurations corresponds to a stable state?

What do valence electrons determine about an element's chemical properties?

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, m_l)
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, m_l, m_s). 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

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.