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

Slides:

Advertisements

Similar presentations

Chemistry Daily 10’s Week 5.

Advertisements

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.

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 can happen when an atom absorbs energy?

Introduction to Excited Elements Lab

Chapter 5 Section 5.1 Electromagnetic Radiation

Arrangement of Electrons in Atoms The Development of a New Atomic Model.

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.

Electrons in Atoms The Development of a New Atomic Model.

Electronic Structure of Atoms Chapter 4 Electronic Structure of Atoms.

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

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.

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.

Dr. Chin Chu River Dell Regional High School Unit 3 – Electron Configurations Part E: Electron Configurations.

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.

CHAPTER 2 ATOMIC STRUCTURE 2.1 Bohr's atomic model 2.2 Electronic configuration.

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.

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.

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.

Electrons in Atoms Chapter 4.

Models of the Atom.

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

Chapter 5 Review Electrons in Atoms.

II. Bohr Model of the Atom (p )

Chapter 4 The Wave Description of 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.

Summary of Flame Testing and Bohr’s Quantum Model of the Atom

Models of the Atom.

Electromagnetic spectrum

The Bohr Model (1913) revolve sun energy

Matter is a Wave Does not apply to large objects

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

Electromagnetic Spectrum and the Atom

Unit 3 – Electron Configurations Part C: Quantum Mechanical Model

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.

Light and Quantized Energy

M. Billings North Surry High School

Section 3: Modern Atomic Theory

Electromagnetic spectrum

Bohr, Emissions, and Spectra

The Bohr Model.

Quantum Theory.

A New Atomic Model Section 4.1.

Chemistry “Electrons in Atoms”

The Nuclear Atomic Model

Section 3: Modern Atomic Theory

Modern Atomic Theory Chapter 4 Section 3.

Quantum Mechanical Model

Arrangement of Electrons

Excited State vs. Ground State

Aim: How are an atom’s electrons configured?

Presentation transcript:

Unit 3 – Electron Configurations Part B: Bohr’s Model of Hydrogen Dr. Chin Chu River Dell Regional High School

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 } Fifth Further away from the nucleus means more energy. There is no “in between” energy Energy Levels Fourth Third Increasing energy Second First Nucleus

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

Bohr’s Model of Hydrogen Atom

Bohr’s Model of Hydrogen Atom

Bohr’s Model of Hydrogen Atom

Bohr’s Model of Hydrogen Atom