The fingerprints of elements

Slides:

Advertisements

Similar presentations

Atomic Emission Spectra. The Electromagnetic Spectrum High frequency Short wavelength High energy lower frequency longer wavelength lower energy.

Advertisements

Electron Configuration and Energy Levels: Ground state: All the electrons in an atom have the lowest possible energies Most stable electron configuration.

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?

Emission Spectra and Flame Tests. The Big Questions What is light? How is light emitted? What do electrons have to do with light? What are emission spectra?

Emission and Absorption of Electromagnetic Energy

Electrons and Light How does the arrangement of electrons in the atom determine the color of light that it emits?

Physics and the Quantum Model

Electrons Arrangement in the Atom Key words: Energy, wavelength, frequency, photon Use these terms in a sentence (s) which makes sense.

Aim: How to distinguish electrons in the excited state DO NOW: PREPARE FOR QUIZ. 10 MIN.

Ground State vs. Excited State Ground State – all electrons are in the lowest possible energy levels (normal) ex. 2 – 8 – 18 – 32 Excited State – if given.

Emission Spectra Bohr Model of the Atom.

Spectral Emission.

Introduction to Excited Elements Lab

Quantization of Energy. When the atom gets excited… To help visualize the atom think of it like a ladder. The bottom of the ladder is called GROUND STATE.

TOIPC: EMISSION SPECTRUM. Flame Test DEMO When Matter is heated it gives off light –Example: fire work, pyrotechnics, flame test –The heat energy absorbed.

Electron Energy and Radiation Quantum Mechanics and Electron Movement.

Light and Energy How the structure of electrons relates to the function of emitting energy as light.

Aim: How to distinguish electrons in the excited state

Evidence of Energy Levels. e-e- e-e- Ground state Excited state Electrons can only be at specific energy levels, NOT between levels.

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

 Fusion – process of 2 nuclei that combine to make one (a new element ) and emitting large amounts of energy.  The sun is a giant ball of hydrogen.

Topic: Electrons in Atoms Ground/Excited States Do Now: List the charge, number of protons, and number of electrons for: 1.Ca +2 2.Fe +3 3.F -1 4.P -3.

1.6.  A spectroscope separates light into its component wavelengths, revealing a line spectrum that is unique to each element.

Electrons “in Orbit” Topic 2.1. Emission line spectrum – energy is applied to a specific element this “excites” the element and the light is viewed.

THE ORIGIN OF LIGHT. The example on this slide looks at a Hydrogen atom that begins in the energy state of n=3 (Don't worry, it is just a system used.

Light and Electronic Transitions

Early models to Quantum Model

Aim: How to distinguish electrons in the excited state

The Bohr Model & Bright-Line Spectra

Bellwork 1) Get out electron configuration worksheet, atomic spectra worksheet (half paper), and stamp sheet. 2) Get out planner and write down homework.

Rutherford Model Know where the protons and neutrons are, but where are the electrons? If opposite charges attract, why do the electrons not fall into.

3.2 Bohr’s Model of the Atom

Ground State vs. Excited State Electrons

II. Bohr Model of the Atom (p )

Bohr Model of the Atom (p ) Read the text

BOHR’S ATOM AND ATOMIC SPECTRA

Understanding Flame Tests and Emission Spectra

YOYO: What element is this? How do you know?

Models of the Atom SCH4C September 2017.

II. Bohr Model of the Atom (p )

Atomic Emission Spectra

5.1 Light & Energy F. Electrons & Light

0:56 0:55 0:54 0:53 0:57 0:58 1:02 1:01 1:00 0:59 0:52 0:51 0:44 0:43 0:42 0:41 0:45 0:46 0:50 0:49 0:48 0:47 1:03 1:04 1:19 1:18 1:17 1:16 1:20 1:21 1:25.

Electrons orbit the nucleus only within allowed energy levels.

Chapter 5 Electrons in Atoms.

Light and Electronic Transitions

HYDROGEN EMISSION SPECTRUM

Atomic Emission Spectra

EXCITING OF ELECTRONS.

Energy and Electrons energy

WHAT THE HECK DO I NEED TO BE ABLE TO DO?

Light, Photon Energies, and Atomic Spectra

II. Bohr Model of the Atom (p )

Light and Quantized Energy

Light, Photon Energies, and Atomic Spectra

Notes #3: History of the Atom (Part 3)

M. Billings North Surry High School

Electromagnetic Spectrum

Atomic emission spectrum

Light and electrons.

Electromagnetic Radiation

3.5 Energy levels and spectra

Electrons and Light!.

Atomic Spectra and Flame Test

Electrons and Electron Arrangement.

Electron Configurations

4.6 NOTES Atomic Emission Spectra

Aim: How to identify elements based on their atomic spectra

Atomic Spectra As atoms gain energy their electrons can be excited and absorb energy in discrete amounts called quanta and produce absorption spectrums.

Presentation transcript:

The fingerprints of elements Emission Spectra The fingerprints of elements

What is emission spectra? When an electron is “excited” to a higher energy level, it wants to return to its original energy level. When it does this, it releases a photon of light which we see as different colors! Hydrogen’s emission spectrum

How can we use this? Each element has a unique number of electrons, so they have their own unique emission spectrum. This is why we call them the “fingerprints” of the element.

On to the demo!