Chapter 5 Electrons in Atoms

Slides:



Advertisements
Similar presentations
Chapter Two …continued
Advertisements

Bohr model and electron configuration
Quantum Mechanical Model: Electron Configurations
Bohr’s Model of the Atom. Bohr’s Model  Why don’t the electrons fall into the nucleus?  e- move like planets around the sun.  They move in circular.
Day 1. Move like planets around the sun.  In specific circular paths, or orbits, at different levels.  An amount of fixed energy separates one level.
Chapter 13 Electrons in Atoms
1 Chapter 11 Electrons in Atoms Killarney School.
Chapter 10 Modern Atomic Theory. Greek Idea l Democritus and Leucippus l Matter is made up of indivisible particles l Dalton - one type of atom for each.
Chemistry Chapter 4 Arrangement of Electrons in Atoms
Chapter 13 Electrons in Atoms
The Quantum Mechanical Model
Chapter 4 Electron Configurations. Early thoughts Much understanding of electron behavior comes from studies of how light interacts with matter. Early.
Electronic Configurations of Atoms
1 Chemistry Chapter 11 Electron Configuration and the Periodic Table World of Chemistry Zumdahl Last revision Fall 2008.
The Modern Model of The Atom Chapter 4. Rutherford’s Model Discovered the nucleus Small dense and positive Electrons moved around in Electron cloud.
CHAPTER 5 ELECTRON CONFIGURATION. ANALOGY OF THE ATOM UNITED STATES  NEW JERSEY  MIDDLESEX COUNTY  EDISON Township  YOUR HOUSE  ATOM ENERGY LEVEL.
Chapter 5 “Electrons in Atoms” Chemistry. Ernest Rutherford’s Model Discovered dense positive piece at the center of the atom- “nucleus” Discovered dense.
Welcome to Chemistry! l Finish test (15 minutes) l Finish homework (if you finished test) l Notes on Orbital Notation and Electron Configuration l Practice.
Electron Configuration Notation (ECN). Bohr’s Model - electrons travel in definite orbits around the nucleus. Move like planets around the sun. Energy.
Chapter 13 Electrons in Atoms Walla Walla High School Mr. Carlsen.
Chapter 5 “Electrons in Atoms”
Chapter 12 Electrons in Atoms. Greek Idea lDlDemocritus and Leucippus l Matter is made up of indivisible particles lDlDalton - one type of atom for each.
CHAPTER 12 ELECTRONS IN ATOMS BRODERSEN HONORS CHEM 2013/14.
Ms. Cleary Chem 11. A model A representation or explanation of a reality that is so accurate and complete that it allows the model builder to predict.
$$$ Quiz $$$ Electrons. Who solved the photoelectric effect problem? Einstein.
Ernest Rutherford’s Model l Discovered dense positive piece at the center of the atom- “nucleus” l Electrons would surround and move around it, like planets.
Chapter 5 Electrons in Atoms The Bohr Model An electron is found only in specific circular paths, or orbits, around the nucleus. Each orbit has a fixed.
Electrons in Atoms Chapter 5. Chapter 5: Electrons in Atoms 5.1 Light and Quantized Energy Wave nature of light.
Electrons in Atoms Charles Page High School Dr. Stephen L. Cotton.
Bohr’s Model - electrons travel in definite orbits around the nucleus. Move like planets around the sun. Energy levels – the region around the nucleus.
Chapter 5 “Electrons in Atoms”
Electron Configurations. The way electrons are arranged in atoms.
Section 4-3 Electron Configurations. Quantum Mechanical Model Energy Levels have sublevels Each sublevel contains orbitals –Orbital – a 3-D region around.
Electron Configurations.  Energy level of an electron analogous to the rungs of a ladder  The electron cannot exist between energy levels, just like.
What are electron configurations? The way electrons are arranged in atoms. Used to indicate which orbitals (energy levels) are occupied by electrons for.
Bohr model and electron configuration. Bohr’s Model Why don’t the electrons fall into the nucleus? Move like planets around the sun. In circular orbits.
Unit 4 Energy and the Quantum Theory. I.Radiant Energy Light – electrons are understood by comparing to light 1. radiant energy 2. travels through space.
CHAPTER 5 “ELECTRONS IN ATOMS”. TERMS 1.Wavelength 2.Frequency 3.Amplitude 4.Electromagnetic spectrum 5.Atomic orbital 6.Excited state 7.Ground state.
Chapter 5 “Electrons in Atoms”. 1. Ernest Rutherford’s Model Discovered dense positive piece at the center of the atom- “nucleus” Electrons would surround.
“Electrons in Atoms” Original slides by Stephen L. Cotton and modified by Roth, Prasad and Coglon.
The QMM Model Mr. Zoitopoulos Legacy High School Chemistry.
Starter S-30 How many electrons are found in Carbon Nitrogen Argon
Bohr’s Model of the Atom
Arrangement of Electrons in Atoms
Bohr model and Quantum Numbers
Atomic Structure: The Quantum Mechanical Model
Quantum Numbers, Electron Configuration, and Orbital Diagrams
Electron Arrangement in an Atom
The whole range is called a continuous spectrum
Chapter 5 Electrons in Atoms.
Electron Configuration
Chapter 5 Notes Electrons.
Quantum Theory.
The QMM Model Mr. Matthew Totaro Legacy High School Honors Chemistry.
Chapter 5 Electrons in Atoms.
Chapter 5 “Electrons in Atoms”
Electrons in Atoms Chapter 5.
Electron Arrangement in Atoms
Chemistry Chapter 4 Notes
Electrons in Atoms Chapter 5.
Chapter 5 “Electrons in Atoms”
Chapter 5 Electrons In Atoms 5.2 Electron Arrangement in Atoms
Electrons in Atoms Bohr Model
Atomic Structure Orbital Diagrams.
Electron Configurations
Electron Configuration
How are electrons organized around a nucleus?
QMM Model Mr. Matthew Totaro Legacy High School Honors Chemistry.
Presentation transcript:

Chapter 5 Electrons in Atoms Chemistry Adapted from Stephen L. Cotton 1

The Basics Energy level of an electron analogous to the rungs of a ladder The electron cannot exist between energy levels, just like you can’t stand between rungs on a ladder. A quantum of energy is the amount of energy required to move an electron from one energy level to another. 2

Atomic Orbitals Principal Quantum Number (n) = the energy level of the electron: 1, 2, 3, etc. These are called orbitals-regions where there is a high probability of finding an electron. Sublevels- arranged in sections by letters s, p, d, and f. 3

Principal Quantum Number Generally symbolized by “n”, it denotes the shell (energy level) in which the electron is located. 4

Energy Levels Maximum number of electrons in each energy level: 1st Level 2 electrons 2nd Level 8 electrons 3rd Level 18 electrons 4th Level 32 electrons 5

Filling by Energy Level First Energy Level Has only an s orbital only 2 electrons 1s2 2 total electrons Second Energy Level Has s and p orbitals 2 in s, 6 in p 2s22p6 8 total electrons 6

Third energy level Fourth energy level Has s, p, and d orbitals 2 in s, 6 in p, and 10 in d 3s23p63d10 18 total electrons Fourth energy level Has s, p, d, and f orbitals 2 in s, 6 in p, 10 in d, and 14 in f 4s24p64d104f14 32 total electrons Any more than the fourth and not all the orbitals will fill up. You simply run out of electrons. 7

Electron Configuration Rules …are the way electrons are arranged in various orbitals around the nuclei of atoms. Three rules tell us how to arrange them: Aufbau principle- electrons enter the lowest energy first. This causes difficulties because of the overlap of orbitals of different energies – follow the Aufbau diagram! 8

Increasing energy 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p 3s 2p

2) Pauli Exclusion Principle- at most, 2 electrons per orbital - but have different spins. 3) Hund’s Rule- When electrons occupy orbitals of equal energy, they don’t pair up until they have to.

-We need to account for all 15 electrons in phosphorus. Let’s diagram the electron configuration for Phosphorus using all three rules. -We need to account for all 15 electrons in phosphorus. 11

Increasing energy 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p The first two electrons go into the 1s orbital Notice the opposite direction of the spins only 13 more to go... 12

Increasing energy 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p 3s The next electrons go into the 2s orbital only 11 more... 13

Increasing energy The next electrons go into the 2p orbital 3d 4d 5d 7p 6d 4f 5f The next electrons go into the 2p orbital only 5 more... 14

Increasing energy The next electrons go into the 3s orbital 2p 3p 4p 5p 6p 3d 4d 5d 7p 6d 4f 5f The next electrons go into the 3s orbital only 3 more... 15

Increasing energy 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p 3s 2p The last three electrons go into the 3p orbitals- 3 unpaired electrons The electron configuration for Phosophorus is 1s22s22p63s23p3 16

Increasing energy 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p 3s 2p Now lets try Potassium-It’s atomic number 19.

Light The study of light led to the development of the quantum mechanical model. Light is a kind of electromagnetic radiation. Electromagnetic radiation includes many types: gamma rays, x-rays, radio waves. 18

- Page 139 “R O Y G B I V” Frequency Increases Wavelength Longer 19

Parts of a wave Crest Wavelength Amplitude Origin Trough 20

Wavelength and Frequency Are inversely related…As one goes up the other goes down. Energy follows frequency. Different frequencies of light are different colors of light. There is a wide variety of frequencies. The whole range is called a spectrum. 21

Atomic Spectrum Each element gives off its own characteristic colors. Can be used to identify the atom. This is how we know what stars are made of. 22

These are called the atomic emission spectrum Unique to each element, like fingerprints! Very useful for identifying elements 23

Light Production Let’s look at a hydrogen atom with only one electron in the first energy level. 24

Heat, electricity, or light can move the electron up to different energy levels. The electron is now said to be excited. 25

As the electron falls back to the ground state, it gives the energy back as light. 26