Unit 3 – Electron Configurations Part B: Bohr’s Model of Hydrogen "Every word I utter is to be understood not as an affirmation but as a question."

Slides:

Advertisements

Similar presentations

Chemistry Daily 10’s Week 5.

Advertisements

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.

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.

ELECTROMAGNETIC RADIATION AND THE NEW ATOMIC MODEL.

What can happen when an atom absorbs energy?

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

NCCS & Properties of Light The Wave Description of Light Electromagnetic radiation is a form of energy that exhibits wavelike behavior.

Chapter 2: The Atom Atom: The smallest unit of an element that retains the chemical properties of the element.

Atomic Spectra. Much of what we know about atomic structure comes from analysis of light either being emitted or absorbed by substances. Elements can.

Particle Nature of Light

Electrons in Atoms. Bohr’s Model  Electrons move like planets around the sun.  In circular orbits at different levels.  Amounts of energy separate.

Honors Chemistry Chapter 5 Electrons “The more success the quantum theory has, the sillier it looks.” ~Albert Einstein, Nobel Prize in Physics, 1921.

Chapter 5 Section 5.1 Electromagnetic Radiation

Modern Chemistry Chapter 4 Arrangement of Electrons in Atoms

Chapter 4 Electrons. ELECTRON BEHAVIOR Who made this model of the atom?

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

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

The wave theory of light was unable to explain something known as the “photoelectric effect”

Electrons in Atoms The Development of a New Atomic Model.

Section 4.3 Modern Atomic Theory

Chapter 7. Electromagnetic Radiation  aka. Radiant energy or light  A form of energy having both wave and particle characteristics  Moves through a.

Electronic Structure of Atoms Chapter 4 Electronic Structure of Atoms.

Mullis Chemistry Holt Ch.41 Arrangement of Electrons in Atoms Principles of electromagnetic radiation led to Bohr’s model of the atom. Electron location.

Electromagnetic radiation – transmission of energy through space in the form of oscillating waves wavelength, – distance between identical points on successive.

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

Bohr Diagrams Electron Energy States. Bohr Model Bohr - electrons in an atom can have only specific amounts of energy NEW idea! quantum number (n) assigned.

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.

UNIT 3 ELECTRON CONFIGURATIONS Part B Bohr’s Model of Hydrogen.

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.

Electron Arrangement Review Unit 3. NC Essential Standards Chm Analyze diagrams related to the Bohr model of the hydrogen atom in terms of allowed,

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.

Atomic Spectra and Electron Orbitals. The Classical Atom Electrons orbited the nucleus. Electrons orbited the nucleus. Problem!! Problem!! Accelerating.

Properties of Light The Wave Description of Light

Electron Structure. Bohr Model Used to explain the structure of the Hydrogen Atom –Hydrogen has only one electron This electron can only circle the nucleus.

Each energy level is like a step on a stair. Electrons move up or down energy levels like going up or down stairs.

Models of the Atom Chapter 4 Chm and

Section 1 The Development of a New Atomic Model Objectives Explain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic.

Chemistry Notes: Electromagnetic Radiation. Electromagnetic Radiation: is a form of energy that exhibits wavelike behavior as it travels through space.

Electrons in Atoms The Development of a New Atomic Model.

Preview Objectives Properties of Light Wavelength and Frequency The Photoelectric Effect The Hydrogen-Atom Line-Emission Spectrum Bohr Model of the Hydrogen.

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

Planetary Model At first, Bohr thought the atom was much like the sun (nucleus) with the planets (e-) orbiting around it.

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.

Early models to Quantum Model

3.2 Bohr’s Model of the Atom

Valence Electrons, Bohr Diagrams, & Light

Bohr Model of the Atom & Light

Ch. 4-1 Models of the Atom Atomic Structure.

The Nuclear Atomic Model

Arrangement of Electrons in Atoms

II. Bohr Model of the Atom (p )

Chapter 4 The Wave Description of Light

Electrons orbit the nucleus only within allowed energy levels.

The Bohr Model (1913) revolve sun energy

Bohr’s Model Why don’t the electrons fall into the nucleus?

Unit 3 – Electron Configurations Part B: Bohr’s Model of Hydrogen

Energy and Electrons energy

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

The Bohr Model of the Hydrogen Atom

II. Bohr Model of the Atom (p )

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.

M. Billings North Surry High School

Chemistry “Electrons in Atoms”

The Nuclear Atomic Model

Arrangement of Electrons

Aim: How are an atom’s electrons configured?

Presentation transcript:

Unit 3 – Electron Configurations Part B: Bohr’s Model of Hydrogen "Every word I utter is to be understood not as an affirmation but as a question."

What have we learned so far? Discharging Tubes The Flame Test The light coming out of the excited atomic entities is very specific to particular element! Results are quite reproducible.

Conclusions: Electromagnetic radiations (lights) coming out or being absorbed by atoms indicate that there are very specific energy changes within the atomic entities (atoms and ions). No nuclear changes have ever been observed indicate that the energy changes have to come from electrons surrounding the nucleus.

How come? Classic Model: Problems with the classic model:

Niels Bohr (1885 – 1962)

Bohr’s Model of Hydrogen Atom Increasing energy Nucleus First Second Third Fourth Fifth } Further away from the nucleus means more energy. There is no “in between” energy Energy Levels

Bohr’s Model of Hydrogen Atom quantum – quantity of energy gained or lost by an atom when electrons are excited photon – a quantum of light ground state – lowest energy level of an atom excited state – a heightened state of energy in an atom Electrons of hydrogen circle the nucleus in orbits 1. orbits have a fixed amount of energy in the ground state. 2. orbits are a fixed distance from the nucleus. 3. orbits furthest from the nucleus have the greatest energy.

Bohr’s Model of Hydrogen Atom

SUPPLIMENTARY WEBSITES: /Bohratom2.html n5bohrmodel.html /Bohratom2.html n5bohrmodel.html

Bohr’s Model of Hydrogen Atom