Introduction to Atomic Theory Today is November 6th Introduction to Atomic Theory OBJ 1: Compare the different models of an atom. OBJ 2: Explain how atomic theory has changed as scientists have discovered new information about the atom. Homework: Read pages 87-93. Purpose for reading: Take notes on “terms to learn.” Science in the News #9 due 11/6 and #10 due 11/13. *TURN in Periodic table activity! *ALL SF Experiments are to be done by 11/26 Warm-up: Why is it important to repeat an experiment? Day 1

To do: Complete page 83 Section Review Sugar Cube Lab

Introduction to Atomic Theory Today is November 10th Introduction to Atomic Theory OBJ 1: Compare the different models of an atom. OBJ 2: Explain how atomic theory has changed as scientists have discovered new information about the atom. Homework: Review pages 87-93.” Science in the News #10 due 11/13. *ALL SF Experiments are to be done by 11/26 Warm-up: none Day 2

To do: Sugar Cube Lab: 1.) Review procedures– Be sure you aren’t missing any info 2.) Begin lab 3.) Go on to day 3

Introduction to Atomic Theory Today is November 11th Introduction to Atomic Theory OBJ: Same. Warm-up: none. To do: See above slides Homework: Science in the News #10 due 11/13. Study terms. *ALL SF Experiments are to be done by 11/26. Day 3

Introduction to Atomic Theory Today is November 12th Introduction to Atomic Theory OBJ 1: Compare the different models of an atom. OBJ 2: Explain how atomic theory has changed as scientists have discovered new information about the atom. Homework: Science in the News# 10 due 11/13. Study terms. *ALL SF Experiments are to be done by 11/26. To do: See next slide Day 4

To do: 1.) 10 minutes to finish Sugar Cube Lab 2.) Jigsaw

Word or phrase Tool Atom Model Activities Today: “A timeline of the Atom” You will be put into groups. I will assign you a person to research in the book Research that person. Write a word, phrase or sentence that the person would likely say about the atom. Describe the tools that person used to make his discovery. Make an atom model that the person proposed. We will come back together to make a timeline & present. To-Do List: Word or phrase Tool Atom Model

Groups/ Assignment Group 1: Dalton Group#2: Rutherford Group# 3: Thomson Group# 4: Bohr Group# 5: Democritus

Conclusion How does mixing or stirring, heating and crushing a solute affect how quickly solids dissolve in liquids?

Introduction to Atomic Theory Today is November 13th Introduction to Atomic Theory OBJ 1: Compare the different models of an atom. OBJ 2: Explain how atomic theory has changed as scientists have discovered new information about the atom. Homework: Review all notes. * TURN in Science in the News #10 * ALL SF Experiments are to be done by 11/26. To do: See next slides Day 5

To do: 1.) Jigsaw 2.) Notes

Democritus: *“uncuttable” particle = atom (“indivisible”) Atoms: *Small *Hard *Made of single material in differ shapes/ sizes *Always moving *Form different materials by joining together

1.) All substances: made of atoms Dalton: Atomic Theory 1.) All substances: made of atoms “atoms cannot be created or destroyed” 2.) Atoms of the SAME element are exactly alike 3.) Atoms join with other atoms to form NEW substances Hmm…

J.J. Thomson: *Small particles ARE inside atom *Atom CAN be divided Negative Corpuscles = electrons *Atoms have no overall charge, thus positive charge MUST be present *Plum-pudding model

http://www.chem.uiuc.edu/clcwebsite/cathode.html#

Ernest Rutherford: Atoms were NOT soft “blobs” *Particles deflected- bounced in various directions THUS: *Center of atoms = positive charge (nucleus) *particles that headed toward nucleus were pushed in the opposite direction *New model

Niels Bohr: *Electrons travel around nucleus in definite paths *Paths are at certain distances from nucleus *Electrons jump

Modern Quantum Theory Atomic orbitals are the basic building blocks of the atomic orbital model (alternatively known as the electron cloud or wave mechanics model),

Modern Quantum Theory: Max Planck Louis de Broglie Erwin Schrodinger Wolfgang Pauli Max Born &Werner Heisenberg James Chadwick Murray Gell-Mann George Zweig Albert Einstein Marie Curie Lise Meitner Enrico Fermi And …. http://particleadventure.org/index.html http://atomictimeline.net/index.php

Ruđer Josip Bošković

Conclusion Take a QUIZ: http://www.neok12.com/quiz/ATOM0005 Who do you think had the biggest impact on today’s present-day atomic theory?

Introduction to Atomic Theory Today is November 14th Introduction to Atomic Theory OBJ 1- 2: See previous slides. OBJ 3: Compare the charge, location, and relative mass of protons, neutrons, and electrons. OBJ 4: Calculate the number of particles in an atom using the atomic number, mass number, and overall charge. Homework: {Review pages 84-93 (i.e. skim your notes)} Answer Section Review questions on pages 86, 89 and 93. *TEST on 11/21 Day 6 To do: See next slides * ALL SF Experiments are to be done by 11/26.

An Introduction to Atomic Models ATOMS An Introduction to Atomic Models

Please Take Notes in your Notebook as we proceed! Atomic Theory? In the following lectures, you will learn about the Atomic - Molecular Theory of Matter. You will also learn about scientists and how they have gathered evidence about atoms. Please Take Notes in your Notebook as we proceed!

Atomic - Molecular Theory of Matter The Atomic - Molecular Theory of Matter states that all matter is composed of small, fast moving particles called atoms. These atoms can join together to form molecules. This theory is really thousands of individual ideas and models that provide evidence for the whole theory.

Matter Since the atom is too small to be seen even with the most powerful microscopes, scientists rely upon models to help us to understand the atom. Believe it or not this is a microscope. Even with the world’s best microscopes we cannot see the structure or behavior of the atom.

Scientific Models Scientists create models to help them to visualize complex properties, structures or behaviors. Since the atom is so small, scientists must gather Indirect Evidence to develop their models. This is a model of one very complex molecule made of many different kinds of atoms. Each colored ball represents an atom of a different element.

What should a Model look like? Scientific models may not always look like the actual object. A model is an attempt to use familiar ideas to describe unfamiliar things in a visual way. This is a painting of a young woman by Pablo Picasso. Does it actually look like a young woman?

Is this really an Atom? Many of the models that you have seen may look like the one below. It shows the parts and structure of the atom. Even though we do not know what an atom looks like, scientific models must be based on evidence. The model above represents the most modern version of the atom, but it’s still a model (Artist drawing)

Indirect Evidence Indirect Evidence is evidence gathered without being able to directly observe the object. The Atomic - Molecular Theory of Matter is based upon a vast amount of indirect evidence gathered over a long period of time. Just like pieces being added to a puzzle, each new bit of information gives us a better understanding of atoms.

How can Indirect Evidence be Gathered? Pretty much everything we know about atoms is indirect evidence. One can't really see atoms. We do see enough of their effects that we can, with confidence, describe the nature of atoms. It's like putting together a puzzle that's missing some pieces. If you get enough pieces in the right place you can tell what the picture is even though it still has holes.

Can a Model be Changed? A model can be changed as new information is collected. From the early Greek concept to the modern atomic theory, scientists have built upon and modified existing models of the atom.

Where did it all begin? The word “atom” comes from the Greek word “atomos” which means indivisible. The idea that all matter is made up of atoms was first proposed by the Greek philosopher Democritus in the 5th century B.C.

More History The concept of atoms as proposed by Democritus remained relatively unchanged for over 2,000 years. Beginning in the late 18th century new discoveries were made that led to a better understanding of atoms and chemistry. Many scientists since that time have contributed new evidence for the “Atomic Theory” Niels Bohr is one of many scientists that have given us a better understanding of Atoms.

How small is an atom? Bryson? 3 hundred-millionths of a centimeter

“Weighing” an atom Since atoms are sooo small, scientists developed a new unit: Atomic mass unit (amu): 1 Proton = 1 amu 1 neutron = 1 amu 1 electron = almost 0 (we don’t consider the mass of an electron when finding the mass number). It takes more than 1800 electrons to equal 1 amu.

The Nucleus Small, positively charged center of the atom. Contains most of the atom’s mass

Inside the Nucleus Protons: positively charged particles Neutrons: particles in atom with no charge What is the charge of the nucleus?

Outside the nucleus Electrons: negatively charged particles in atoms. Likely to be found around the nucleus within electron clouds

What makes up P, N & E?

Take a QUIZ: http://www.neok12.com/quiz/ATOM0001 http://www.neok12.com/quiz/ATOM0002 http://www.neok12.com/quiz/ATOM0003 http://www.neok12.com/quiz/ATOM0008

The Atom Today is November 17th OBJ 1- 4: See previous slides. Take out: Section Review questions on pages 86, 89 and 93. Homework: *TEST on 11/21 To do: See next slides Day 7 * ALL SF Experiments are to be done by 11/26.

An Atom is neutral! Equal number of protons and electrons The charges of protons and electrons are opposite, but equal in size. What if they aren’t equal?

Ions A charged particle If # protons > # electrons . . .

Elements & Atoms Each element is made of a different amount of protons, neutrons, and electrons. For example: Hydrogen= 1 proton, 0 neutron, 1 electron Helium= 2 protons, 2 neutrons, 2 electrons Gold= 79 protons, 118 neutrons, 79 electrons

**THE NUMBER OF PROTONS DETERMINES THE ELEMENT** ATOMIC NUMBER: THE NUMBER OF PROTONS IN THE NUCLEUS OF THE ATOM ALL ATOMS OF THE SAME ELEMENT HAVE THE SAME AMOUNT OF PROTONS.

So…the amount of P doesn’t have to equal N. . . Isotopes: atoms that have the same number of protons, but a different number of neutrons. This means it has a different mass number. Mass number = Sum of protons + neutrons Boron= 5 Protons + 5 Neutrons = 10 amu Or 5 Protons + 6 Neutrons = 11 amu

Properties of Isotopes Each element has a limited number of isotopes (meaning, you can’t assign “random” numbers of neutrons) Can be unstable: meaning, the nucleus can change it’s composition. If it is unstable it’s RADIOACTIVE Will have the same physical & chemical properties of the stable isotope

To find the # of neutrons Simple subtraction Mass Number – Atomic number (# of p) Carbon -12 Mass number= 12 Atomic Number= 6 Neutrons= 6

Calculating the Mass of an Element Atomic Mass: weighted average of the masses of all naturally occurring isotopes of an element MathBREAK on page 92: To calculate the atomic mass of an element, multiply the mass number of each isotope by its percentage abundance in decimal form. Then add these amounts together to find the atomic mass.

Calculate the Atomic Mass What is the atomic mass of: Titanium-46 (8%) Titanium-47 (7.3%) Titanium-48 (73.8%) Titanium-49 (5.5%) Titanium-50 (5.4%)

“Made to Order” No new objectives. Today is November 18th “Made to Order” No new objectives. Homework: Test on 11/21. Handout and Lab (finish whatever you didn’t finish in class today!) Warm-up: Copper- 63 occurs in nature 69% of the time. Copper- 65 occurs in nature 31% of the time. Calculate the Atomic Mass. How do I calculate this?! Day 8 * ALL SF Experiments are to be done by 11/26.

Concept Map Higgs Boson Explained video: http://player.vimeo.com/video/41038445?portrait=0&amp

Example Chlorine-35 makes up 76% abundance in nature +_______ 35.5 amu

Calculate Boron Boron-10 occurs 20% Boron- 11 occurs 80%

Forces in an atom Gravity: (acts between all objects) It affects an atom, but very small affect. Electromagnetic Force: Same charges repel, opposite charges attract. This is what holds electrons around the nucleus. Strong Force: keeps the nucleus together because protons would repel each other. Stronger than E.M. Force. Weak Force: in radioactive atoms. . .a neutron can change into a proton.

Draw a concept map Proton Atomic mass unit Neutron Atomic number Isotopes Mass number Atomic mass

Atom Builder Activity http://www.nclark.net/Atom_Builder.pdf

“Made to Order” No new objectives. Homework: Study- Test on 11/21 Today is November 19th “Made to Order” No new objectives. Homework: Study- Test on 11/21 To Do: Questions about SF Check last night’s HW Notes from yesterday Day 9 * ALL SF Experiments are to be done by 11/26.

“Made to Order” No new objectives. Homework: TEST on 11/21. To Do: Today is November 20th “Made to Order” No new objectives. Homework: TEST on 11/21. To Do: Questions Lesson Wrap-up: Chapter Review Day 10 * ALL SF Experiments are to be done by 11/26.

TEST right NOW! Homework: Today is November 21st * ALL SF Experiments are to be done by 11/26.

REVIEW of SMALL PARTICLE THEORY For today and tomorrow we will… REVIEW of SMALL PARTICLE THEORY Homework: none- if you do your work! -BOTH labs are due by the end of class on 11/25! To do: What does the small particle theory say… again? Day 7 and 8 ALL SF Experiments are to be done by 11/26. FULL SF papers (DRAFT ONLY) are due 12/3

The Particle Theory of Matter: 1. Matter is made up of tiny particles (Atoms & Molecules) 2. Particles of Matter are in constant motion. 3. Particles of Matter are held together by very strong elastic forces 4. There are empty spaces between the particles of matter that are very large compared to the particles themselves. 5. Each substance has unique particles that are different from the particles of other substances 6. Temperature affects the speed of the particles.  The higher the temperature, the faster the speed of the particles.

Next up: LABS *Molecular Motion and Spacing The particle theory of matter explains the following scientific phenomena:  Pure substance are homogeneous (one phase - one unique kind of particle)  Physical Changes - Melting, Evaporation, Sublimation, Dissolving.....  Characteristic Physical Properties - Density, Viscosity, Electrical & Thermal Conductivity Next up: LABS *Molecular Motion and Spacing * Space between particles of liquid