Which of the following is an important feature of the Bohr model of the atom? A. Electrons exist anywhere around the nucleus. B. The energy of the light.

Slides:

Advertisements

Similar presentations

Light Unit David B. Brown 6C.

Advertisements

RADIO WAVES, MICROWAVES, INFRARED, VISIBLE, ULTRAVIOLET, X-RAYS, GAMMA RAYS HIGH< wavelength LOW.

Electromagnetic Waves

Chemistry Daily 10’s Week 5.

How do you excite an electron?

The Electromagnetic Spectrum. The name given to a group of energy waves that are mostly invisible and can travel through empty space Shorter waves have.

Unlocking Light The key to understanding the Cosmos.

Life always offers you a second chance. It’s called tomorrow.

The Electromagnetic Spectrum Rainbows plus a whole lot more.

Poster Project Waves.

Light and Electronic Transitions. The Big Questions What is light? How is light emitted? What do electrons have to do with light? What are emission spectra?

Flame Test and the EMS. Absorption and Emission of Light in a Flame When a substance is heated in a flame, the substances electrons absorb energy from.

Rutherford’s model -Shows where protons & neutrons are -Not good at showing the location of electrons.

Properties of Light Is Light a Wave or a Particle?

The Light Fantastic! Astronomy relies on messages from all kinds of light.

Waves….. What is a Wave? A Wave is a disturbance that carries energy through a medium or empty space. A Medium is a substance such as a solid, liquid,

Electromagnetic Waves. Electromagnetic wave is a wave that can travel through empty space or through matter and is produced by charged particles that.

Chapter SevenPrentice-Hall ©2002Slide 1 of 52 In chapter 6 we saw the energy can be transferred as heat. In this chapter, we shall see that energy can.

Quantum Mechanics.  Write what’s in white on the back of the Week 10 Concept Review  Then, answer the questions on the front Your Job.

Light. Light Terminology Which is not a measure we use to identify a type of light? A. Wavelength B. Speed C. Frequency D. Energy.

Energy Unit Learning Goal #1: Evaluate the quantum energy changes in the atom in terms of the energy contained in light emissions.

Warm Up Draw the Bohr Model for Aluminum and Neon.

Electron Energy Levels Not all electrons in an atom have the same energy They exist in discreet energy levels These levels are arranged in shells (n =

The Electromagnetic Spectrum Oooh…aaah. What is it? A spectrum is a RANGE of things The Electromagnetic Spectrum (EM Spectrum) is a RANGE of electromagnetic.

Electromagnetic Spectra Review Game. When do electrons emit light? Moving from higher to lower energy levels.

Many scientists found Rutherford’s Model to be incomplete  He did not explain how the electrons are arranged  He did not explain how the electrons were.

Aim: How are an atom’s electrons configured? Electromagnetic SpectrumElectromagnetic Spectrum -the total range of light including gamma rays, x-rays, ultraviolet,

Guiding Questions 1. How fast does light travel? How can this speed be measured? 2. Why do we think light is a wave? What kind of wave is it? 3. How is.

Chapter 10: Modern atomic theory Chemistry 1020: Interpretive chemistry Andy Aspaas, Instructor.

Energy Levels & Photons Atomic & Nuclear Lesson 2.

Atomic Emission Spectra

Electrons and the Electromagnetic Spectrum Table Team Review — DEFINE in your own words ‘Electromagnetic radiation’. LIST three examples.

Warm Up What is the wavelength defined as?

Electromagnetic Radiation & Light. 2 What are the atom models we know of? 2.

Bellwork What is the majority of the volume of an atom?

Section 5.3.  Neon advertising signs are formed from glass tubes bent in various shapes. An electric current passing through the gas in each glass tube.

1 CHAPTER 13: Electrons in the Atom. 2 Quantum Mechanical Model of the Atom and Ernest Schrodinger The model of the atom was developed based on the study.

“Physics and the Quantum Mechanical Model” Read pg. 138 p. 1

Slide 1 of 38 chemistry. Slide 2 of 38 © Copyright Pearson Prentice Hall Physics and the Quantum Mechanical Model > Light The amplitude of a wave is the.

Section 1 chapter 4. Electromagnetic Radiation (EMR) - a form of energy that travels in waves which includes radio waves, T.V. waves, microwaves, visible.

Unit 9: Atomic Theory and Periodicity Section 1: Structure of the Atom.

Energy Kinetic Energy Potential Energy.

Electrons Negative charge e- Located in the electron cloud far from the nucleus Have mass, but it is negligible Also have wave-like properties.

Light and Electrons! Ch 11. Light & Atomic Spectra A Brief Bit of History (development of the quantum mechanical model of the atom) Grew out of the study.

Chapter 5 Electronic Structure. Light Through a Prism W White light (sunlight) is a blend of all colors (ROY G BIV) combined together. T The wavelength.

Electron As a Particle and Wave Electrons get excited when energy is absorbed by using heat or electrical energy Electrons get excited when energy is absorbed.

KWL CHART--ELECTRONS WHAT DO I ALREADY KNOW ABOUT ELECTRONS? WHAT DO I WANT TO KNOW CONCERNING ELECTRONS? WHAT HAVE I LEARNED TODAY ABOUT ELECTRONS?

P HYSICAL S CIENCE The Electromagnetic Spectrum. O BJECTIVES Explain the properties of the electromagnetic spectrum Differentiate between the different.

Physics and the Quantum Mechanical Model.  Light consists of waves  A wave cycle begins at zero, increases to its highest value (crest), returns to.

Do Now: 1.If you could solve one problem using science, what would it be? 2.What branch of science do you think you would need to use to solve the problem?

Models of the Atom Chapter 4 Chm and

Sound waves transfer energy through vibrations. Sound Produced by vibrations Mechanical waves Vibrate particles Medium affects sound waves. (p. 42) Temperature.

Models, Waves, and Light Models of the Atom Many different models: – Dalton-billiard ball model (1803) – Thompson – plum-pudding model (1897) – Rutherford.

Life always offers you a second chance. It’s called tomorrow.

Electrons in Atoms Chapter 4. RUTHERFORD MODEL A NEW ATOMIC MODEL The ____________ model of the atom was a great improvement, but it was incomplete.

Light 1)Electrons (charged –1 each, with a mass of 1/1836 amu each) surround the nucleus of the atom in distinct energy levels. Electrons occupy the.

Electromagnetic Waves. Electromagnetic Spectrum.

Physics and the Quantum Mechanical Model

Light, Electromagnetic Spectrum, & Atomic Spectra

Light Ken Rogers Miami Killian.

Electromagnetic Spectrum Project

Physics and the Quantum Mechanical Model

Have you ever wondered how you get different colored fireworks?

Electromagnetic Radiation

Quantum Theory.

Electromagnetic Waves

Warm-up Example 3 from Practice Atomic Mass notes on pg 31!

Aim: How are an atom’s electrons configured?

2 Light & Electromagnetic Spectrum

Presentation transcript:

Which of the following is an important feature of the Bohr model of the atom? A. Electrons exist anywhere around the nucleus. B. The energy of the light is directly proportional to its wavelength. C. Atoms emit energy when jumping from a lower to a higher energy level. D. Atoms emit energy when jumping from a higher to a lower energy level.

A continuous visible spectrum is A. the distance between two equivalent points on a wave. B. a rainbow. C. light with shorter wavelengths than visible. D. light with longer wavelengths than visible. E. when an electron occupies an energy level higher than the lowest available energy available.

An excited electron state is A. the distance between two equivalent points on a wave. B. a rainbow. C. light with shorter wavelengths than visible. D. light with longer wavelengths than visible. E. when an electron occupies an energy level higher than the lowest available energy available.

A wavelength is A. the distance between two equivalent points on a wave. B. a rainbow. C. light with shorter wavelengths than visible. D. light with longer wavelengths than visible. E. when an electron occupies an energy level higher than the lowest available energy available.

Ultraviolet light is A. the distance between two equivalent points on a wave. B. a rainbow. C. light with shorter wavelengths than visible. D. light with longer wavelengths than visible. E. when an electron occupies an energy level higher than the lowest available energy available.

This picture is an example of: A. an emission spectrum. B. an absorption spectrum. C. a continuous spectrum. D. an excitation spectrum.

This picture is an example of: A. an emission spectrum. B. an absorption spectrum. C. a continuous spectrum. D. an excitation spectrum.

This picture is an example of: A. an emission spectrum. B. an absorption spectrum. C. a continuous spectrum. D. an excitation spectrum.

A unit that could be used to describe wavelength is A. hertz B. joules C. meters D. electron volts

A unit that could be used to describe frequency is A. hertz B. joules C. meters D. electron volts

In order to take a picture of bones inside your body you would need to be exposed to A. visible light waves. B. gamma rays C. X-rays. D. radio waves. E. infrared waves. F. ultraviolet waves. G. microwaves.

If you got a sunburn, that means you were exposed to A. visible light waves. B. gamma rays C. X-rays. D. radio waves. E. infrared waves. F. ultraviolet waves. G. microwaves.

Your cell phone emits A. visible light waves. B. gamma rays C. X-rays. D. radio waves. E. infrared waves. F. ultraviolet waves. G. microwaves

A photon is A. a nuclear particle with a positive charge. B. a nuclear particle with no charge. C. a particle of light or energy without mass. D. a very small particle with a negative charge that occupies distinct orbits around the nucleus.

A chemical reaction or process that uses heat or energy is called A. ectomorphic. B. endothermic. C. eukaryotic. D. exothermic.

A chemical reaction that produces heat or energy is called A. ectomorphic. B. endothermic. C. eukaryotic. D. exothermic.