HYDROGEN EMISSION SPECTRUM

Slides:

Advertisements

Similar presentations

Chemistry Daily 10’s Week 5.

Advertisements

LINKING THE ATOM TO THE ELECTROMAGNETIC SPECTRUM Electrons in the Atom 1 Chapter 4 - Section 1.

What do you see? Old woman? Or young girl?  Is turning a light on and off a chemical or physical change? ◦ Physical change  What creates light?

Anyone who is not shocked by quantum mechanics has not understood it. —Neils Bohr (1885–1962)

When current is passed through a gas at low pressure, the potential energy of some of the gas increases. The ground state of an atom is the lowest possible.

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

Emission and Absorption of Electromagnetic Energy

Electrons And Light. Electromagnetic Radiation Energy that travels as a wave through space Wavelength –λ – distance between corresponding points on adjacent.

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

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

Particle Nature of Light

Emission Spectra Bohr Model of the Atom.

Introduction to Excited Elements Lab

 The Bohr model was proposed:  1913  by Neils Bohr  After observing the H line emission spectrum.

Development of Modern Atomic theory. Modern Model of Atom When energy is added to an atom : Low NRG State (ground state)  High energy state (excited.

Niels Bohr (1913) Bright-Line Spectrum Energy Levels Planetary Model

Aim: How to distinguish electrons in the excited state

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

Student will learn: Relationship between light & electrons What produces color Electromagnetic Spectrum Readings Neils Bohr Model of Hydrogen Readings.

Warm-Up Lithium has an atomic weight of g/mol. When g of lithium is heated, it emits an energy measured at 262,500 joules. What is the energy.

Neils Bohr What keeps the negative electrons from falling toward the positive nucleus?

Section 4-1 Continued.  Ground State – the lowest energy state of an atom  Excited State – a state in which an atom has a higher energy than in its.

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.

The Bohr Model: Atoms with Orbits pg LO: I can explain what line spectra represent.

UNIT 3 ELECTRON CONFIGURATION AND MODERN ATOMIC THEORY.

Quantum Theory and the Atom In the early 1900s, scientists observed certain elements emitted visible light when heated in a flame. Analysis of the emitted.

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

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.

Wave-Particle Duality JJ Thomson won the Nobel prize for describing the electron as a particle. His son, George Thomson won the Nobel prize for describing.

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.

Electrons And Light. Electromagnetic Radiation Energy that travels as a wave through space Wavelength –λ – distance between corresponding points on adjacent.

Light and Electrons. Draw an atom of Lithium. Did you draw this? What exactly are the electrons rings around the nucleus?

Aim: How to distinguish electrons in the excited state

The Bohr Model of the Atom

Bohr Model Of Atom.

Bohr Model Of Atom.

Aim: How Do We Describe an Atoms Energy Levels?

BOHR’S ATOM AND ATOMIC SPECTRA

Atomic Emission Spectra

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

Bohr & Schrödinger.

Flame Test Lab.

Physics and the Quantum Mechanical Model

II. Bohr Model of the Atom (p )

Bohr and Introduction To Electron Structure Part I.

5.1 Light & Energy F. Electrons & Light

Electrons orbit the nucleus only within allowed energy levels.

Wave-Particle Duality

The Bohr Model (1913) revolve sun energy

Nature of light and atomic spectrum

Take out your Homework on Electron Configuration and Orbital Diagrams

Atomic Emission Spectrum

Energy and Electrons energy

The Bohr Model of the Hydrogen Atom

“Spanish Steps”, Francesco de Sanctis, 1726, Rome, Italy

Atomic Emission Spectra

II. Bohr Model of the Atom (p )

Light, Photon Energies, and Atomic Spectra

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

M. Billings North Surry High School

Neils Bohr Tried to use the emission spectrum of hydrogen to further explain the atom Proposed that electrons orbit the nucleus in circular paths of fixed.

Light and electrons.

The fingerprints of elements

The Atom Lesson 3 : The Bohr Model.

Atomic Spectra and Flame Test

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.

The Nature of Electrons

Presentation transcript:

HYDROGEN EMISSION SPECTRUM UNIT 1 NOTES

Which scientist was famous for the hydrogen emission spectrum experiment? What did he discover?

Hydrogen emission spectrum Neils Bohr noticed that atoms will emit a specific color of light when energy is added to the atom, like in a flame.

Visible light (sunlight) is dispersed (sorted) through the prism to produce a visible light spectrum (rainbow).

Have you ever played with a glass prism? What happens when light is shined on it?

Bohr used a hydrogen lamp that only emitted light from hydrogen gas and found a strange result— only some colors appeared in the spectrum.

Bohr concluded that the electron must be transitioning to different levels in the atom each with its own specific amount of energy.

The electron absorbs energy to move from its ground state (low level) to an excited state (high level). When the electron returns to the ground state a photon (particle of light) is emitted (released/given off).

The electron absorbs energy to move from its ground state (low level) to an excited state (high level). When the electron returns to the ground state a photon (particle of light) is emitted (released/given off).

When an electron transitions from an excited state back to a ground state a specific energy of light (color) is emitted.

FLame test lab They will not stay excited for long and when the electron drops down to the original ground state orbit the energy will be released in the form of light Energy is absorbed from the flame and electrons get excited. When the electrons get excited they transition or jump up orbits to a higher energy level.