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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?
Today is November 6th
To do:
Complete page 83 Section ReviewSugar Cube Lab
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
Today is November 10th
To do:Sugar Cube Lab:
1.) Review procedures– Be sure you aren’t missing any info2.) Begin lab 3.) Go on to day 3
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.
Today is November 11th
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
Today is November 12th
To do:
1.) 10 minutes to finish Sugar Cube Lab2.) Jigsaw
Activities Today: “A timeline of the Atom”
1.You will be put into groups.2.I will assign you a person to research in the book3.Research that person.4.Write a word, phrase or sentence that the person would likely say about the atom. 5.Describe the tools that person used to make his discovery.6.Make an atom model that the person proposed. 7.We will come back together to make a timeline & present.
To-Do List:
Word or phraseToolAtom Model
Group 1: DaltonGroup#2: RutherfordGroup# 3: Thomson
Group# 4: BohrGroup# 5: Democritus
Groups/ Assignment
Conclusion
How does mixing or stirring, heating and crushing a solute affect how quickly solids dissolve in liquids?
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
Today is November 13th
To do:
1.) Jigsaw2.) Notes
Atoms:*Small*Hard*Made of single material in differ shapes/ sizes*Always moving*Form different materials by joining together
Democritus:
*“uncuttable” particle = atom (“indivisible”)
Dalton: Atomic Theory
1.) All substances: made of atoms“atoms cannot be created or destroyed”2.) Atoms of the SAME element are exactly alike3.) Atoms join with other atoms to form NEW substances
Hmm…
J.J. Thomson:
*Small particles ARE inside atom*Atom CAN be dividedNegative 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 directionsTHUS:*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
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
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 FermiAnd ….
http://atomictimeline.net/index.php
Ruđer Josip Bošković
Who do you think had the biggest impact on today’s present-day atomic theory?
ConclusionTake a QUIZ: http://www.neok12.com/quiz/ATOM0005
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
To do: See next slides
Today is November 14th
* ALL SF Experiments are to be done by 11/26.
An An IntroductiIntroducti
on to on to Atomic Atomic ModelsModels
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.
MatterSince the atom is Since the atom is too small to be too small to be seen even with seen even with
the most the most powerful powerful
microscopes, microscopes, scientists rely scientists rely
upon models to upon models to help us to help us to
understand the understand the atom.atom.
Believe it or not this is a Believe it or not this is a microscope. Even with the microscope. Even with the worldworld’’s best microscopes s best microscopes
we cannot see the we cannot see the structure or behavior of the structure or behavior of the
atom.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 This is a model of one very complex molecule made of complex molecule made of
many different kinds of many different kinds of atoms. Each colored ball atoms. Each colored ball represents an atom of a represents an atom of a
different element.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 This is a painting of a young
woman by Pablo Picasso. Does woman by Pablo Picasso. Does it actually look like a young it actually look like a young
woman?woman?
Is this really an Atom?
The model above represents the most
modern version of the atom, but it’s still a model
(Artist drawing)
Many of the models that you Many of the models that you have seen may look like the one have seen may look like the one
below. It shows the parts and below. It shows the parts and structure of the atom. Even structure of the atom. Even
though we do not know what an though we do not know what an atom looks like, scientific atom looks like, scientific models must be based on models must be based on
evidence. evidence.
Indirect EvidenceIndirect 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 HistoryThe 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 Niels Bohr is one of many scientists that many scientists that
have given us a have given us a better understanding better understanding
of Atoms.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
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
Today is November 17th
* 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 . . .
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
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 MassWhat 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. 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?!
Today is November 18th
* ALL SF Experiments are to be done by 11/26.
Concept Map
Higgs Boson Explained video: http://player.vimeo.com/video/
41038445?portrait=0&
Example
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
To Do: Questions about SF Check last night’s HWNotes from yesterday
Today is November 19th
* ALL SF Experiments are to be done by 11/26.
“Made to Order” No new objectives. Homework: TEST on 11/21.
To Do: QuestionsLesson Wrap-up: Chapter Review
Today is November 20th
* 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
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?
For today and tomorrow we will…
• 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 substances6. Temperature affects the speed of the particles. The
higher the temperature, the faster the speed of the particles.
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