Warm-up (Sept 28) Homework out, please!

Slides:



Advertisements
Similar presentations
Wed, Sept 23, 2009 Learning Goal – to understand Review for atomic quiz Atomic Quiz Discuss 13.3 Homework.
Advertisements

Chemistry Daily 10’s Week 5.
1 Electrons in Atoms Chapter Particle Nature of Light Max Planck ( ) 1900 German physicist Studied light emitted from objects Found matter.
Wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.
Wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.
[ ]
Copyright © Houghton Mifflin Company. All Rights Reserved.1 Chemistry 6/e Steven S. Zumdahl and Susan A. Zumdahl Chapter 7: ATOMIC STRUCTURE & PERIODICITY.
wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.
Dr. Jie ZouPHY Chapter 42 Atomic Physics (cont.)
EXAM #2 RESULTS THIS WEEK’S SCHEDULE LECTURE- LAB- Announcements.
Quantum Mechanical Model
14 November 2011  Objective: You will be able to:  describe evidence for the current theory of the electronic structure of atoms.  Homework: p. 312.
Chapter 10: Modern atomic theory Chemistry 1020: Interpretive chemistry Andy Aspaas, Instructor.
The Rutherford’s model of the atom did not explain how an atom can emit light or the chemical properties of an atom. Plum Pudding Model Rutherford’s Model.
Wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.
 Bohr model was 1 dimensional  Scientist started thinking about electrons in the forms of waves and particles  DeBrogile Equation  Schroedinger Equation.
Quantum Chemistry Chapter 6. Copyright © Houghton Mifflin Company. All rights reserved.6 | 2 Electromagnetic Radiation.
The Bohr Model. Do Now (3/24/14) (5 Minutes)  If you haven’t already Pass in Last week’s Do Now  What are some scientific examples of concepts humanity.
Electromagnetic Spectrum Atomic Emission Spectrum.
Arrangement of Electrons in Atoms Chapter 4. Properties of Light Electromagnetic Radiation- which is a form of energy that exhibits wavelength behavior.
1 Chemistry 111 Sections 10.1 – 10.4 Chemistry 111.
Modern Atomic Theory Chapter 4 Section 3.
Variation in Atomic Structure: Isotopes and Ions Monday November 14 th and Tuesday November 15 th.
Chapter 7 Atomic Structure & Periodicity. Electromagnetic Radiation O Waves (wavelength, frequency & speed) O  c (page 342: #39) O Hertz O Max Planck.
Electronic Behavior of Atoms. LO Describe how light is created. Explain how wavelengths of light relate to energy levels in the atom. SC View the spectrum.
X = c E  h (What atoms have to do with it) Chapter 4 H Chem The Atom…cont’d Bohr Model (Proven by looking at Bright-Line Spectra) Therefore These are.
Section 3: Modern Atomic Theory
Quantum Mechanical Model Or…”Electron Cloud Model” Electrons move freely within “clouds” (called orbitals) not just restricted to orbits. [
1. The first Bohr’s radius (for electron in hydrogen atom in the ground state): 2. The ground energy level in hydrogen atom:
Chemistry Jeopardy Chemistry Jeopardy Chapter 4 Catch the Wave Step into the Light Orbit an Orbital Electron Fun Figure or Configure Me Bohr Me Famous.
Section 11.2 The Hydrogen Atom 1.To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy 2.To learn about Bohr’s.
Warm Up Electrons are responsible for the atomic _____ (mass or volume) 2. List the number of protons, electrons and neutrons for the following.
Line Spectra When the particles in the solid, liquid, or gas accelerate, they will produce EM waves. Electron orbit to orbit transitions in atoms (gasses)
Chemistry Jeopardy Chemistry Jeopardy Chapter 4 Catch the Wave Step into the Light Orbit an Orbital Electron Fun Figure or Configure Me Bohr Me Famous.
Aim: How do chemists represent an atom’s “electron configuration”? Vocabulary: Electron configuration- probable location of electron; the electron’s “address.”
Characteristics of atoms. Key features of atoms All atoms are electrically neutral All atoms of the same element contain the same number of protons and.
Warm-Up What is the difference between the Bohr’s Model of the Atom and the Quantum Model of the atom. What wavelength is associated with an electron.
Warm up (Sept 27) Lab 3 on desk all done, please!
Arrangement of Electrons in Atoms
Bohr Model Of Atom.
After this class, I should be able to: - Write longhand and shorthand electron configurations - Apply Aufbau Principle, Pauli Exclusion Principle and Hund’s.
Quantum Theory and The Atom
Topic 2 Atomic Structure
3.2 Bohr’s model of the Atom
Electron Configuration HW #1 out, please
Welcome! (October 12) Presentations ready and sent to me?
Chapter 6: Electromagnetic Radiation
The whole range is called a continuous spectrum
Quantum Theory & Periodicity
TOPIC 2 ATOMIC STRUCTURE
Niels Bohr and the quantum atom
Bohr Model l , n l x n Light hn Matter
Announcements Lon-capa HW 6 – Type 1 due Monday (11/18) and Type 2 due Wednesday (11/20) by 7pm “Lab 5: Modern Atomic Theory” write-up due tomorrow in.
Spectra and Energy Levels in Atoms
Warm-up 11/6/15 Turn in Chapter 3 Warm-ups.
Hydrogen Atom Emission Spectrum
Topic 2/12 Overview 2.2: Electron configuration 2.1: The Nuclear Atom
Niels Bohr and the quantum atom
M. Billings North Surry High School
Section 3: Modern Atomic Theory
Electromagnetic Spectrum Atomic Emission Spectrum.
Image Bank Chapter 4 Preview Electromagnetic Spectrum
Bohr, Emissions, and Spectra
Quantum Theory.
Bohr Model of Hydrogen Visible Spectrum Full Spectrum.
Section 3: Modern Atomic Theory
Development of Quantum Mechanics Bohr’s Contribution
Development of a New Atomic Model
Chapter 6: Electromagnetic Radiation
The Bohr’s Hydrogen Atom
Presentation transcript:

Warm-up (Sept 28) Homework out, please! What is the wavelength (in nm) of an electronic transition in Neon with an energy of 3.45 x 10-19 J? About 576 nm

Multiple Choice! A) 3  2 B) 4  3 C) 3  ∞ D) 3  1 Which of the following transitions in the Hydrogen atom would give a wavelength in the IR (infrared) region of the spectrum? A) 3  2 B) 4  3 C) 3  ∞ D) 3  1 B

Summer Homework Back (keep it forever – we’ll reference it often) Let’s grade chapter 2 questions (we’ll save the others as we are reviewing chapters 1, 3, and 4) Numbers 2, 6, and 8

Waves – a recap c = νλ E = hν Why does this equation make sense? What else is it useful for?

Bond breaking energy The bond strength of Cl2 is 242 kJ/mol. Find the wavelength of energy needed to break one Cl-Cl bond. What do we need to do??? Many steps! 4.94 x 10 -5 m (or 0.0494 mm) http://www.chemhume.co.uk/ASCHEM/Unit%201/Ch3Chemstr/Images%203/covalent_bonding_cl2.jpg

Cool Article! https://www.sciencedaily.com/releases/2017 /03/170313135050.htm

NOW: Split! Andrea and Laura with me (front row) 12.1 Lab A – Analysis of the Lyman series The rest of you - in the back to work on: Lab 1 Report Due Tomorrow MAKE IT AWESOME! Use your time wisely Look over Homework Key for SL Homework – work through and see what questions you have Study for Quiz on Chapter 2 Monday in class! The whole key to every practice question is your SL Key for Homework – do any extras we didn’t do!

Look Over Homework Keys SL and HL different – find on Moodle and look through

12.1 – Supplementary info! What evidence does the Bohr model give us? What evidence do we have that Bohr’s model is incomplete? Energy levels and quantum jumps Did not work for anything else than H, (ionization energy and davisson-germer/debroglie test for waves helped debunk)

Aluminum – compare to your orbital diagram from last class!

Practice This is evidence that our orbital diagrams are accurate – sublevels, etc

Why non-linear? Evidence for singly filled (Pauli) orbitals, etc

Lab A (HL) – Finding Ionization Energy in Hydrogen using Lyman Series Take a look at pg 86-87

Homework Day 9 Lab 1 Formal Write-up due TOMORROW shared with me on Google Quiz Monday on chapter 2! HL – Lab A by Wednesday