unit 2 chapter 4 day 1 objective : explain how the study of atoms has changed in the last century...
TRANSCRIPT
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Unit 2 Chapter 4 Day 1 OBJECTIVE:
Explain how the Study of Atoms has changed in the last century and identify subatomic particles
• Do Now:• The Elements in the Body – a graph• TURN IN: Current Events
Today: • Chapter 4 Notes – Part 1
• Atoms and Atomic Structure• Thomson’s and Rutherford’s experiments
• P-N-E worksheets• Homework:
• Read Chapter 4.1 & complete 4.1 GRWS
New Chapter New Notebook
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Unit 2 Chapter 4 Day 2 OBJECTIVE:
Explain how the Study of Atoms has changed in the last century and identify subatomic particles
• Do Now:• The Atom – Graphic Organizer
• Today: • Homework check and review 4.1 GRWS
• More P-N-E practice• What is Matter?
• Video: Bill Nye-Atoms & Molecules• Chapter 4 Notes – Part 2
• Ions, Isotopes and Excited Electrons• Homework:
• Chapter 4.2 GRWS
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Unit 2 Chapter 4 Day 3 OBJECTIVE:
Discuss variations of atoms and Investigate the structural differences of hydrogen isotopes
• Do Now:• Atoms and Parts crossword puzzle
• Today: • Homework check and review 4.2 GRWS• Finish Chapter 4 Notes – Part 2
• Ions, Isotopes and Excited Electrons• LAB: Modeling Isotopes of Hydrogen• R & R Structure of the Atom
• Homework:• Finish R & R
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Unit 2 Chapter 4 Day 4OBJECTIVE:
Construct and interpret Bohr’s models and Lewis dot diagrams for multiple elements
• Do Now:• What happens to Carbon if…• TURN IN HOMEWORK
• Today: • Return Unit 1 Test – Corrections Due TOMORROW• Intro - Chemistry Unit Project - Due Date = 4/1/15• Bohr and Lewis - Electron Models of the Atom
• “Bohr”ing practice and Making Lewis Dot Diagrams
• Homework:• Advertise-the-Elements project – Select your Elements!• Read Chapter 4.3 & complete GRWS• Progress Reports signed
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Unit 2 Chapter 4 Day 5 OBJECTIVE:
Construct and interpret Bohr’s models and Lewis dot diagrams for multiple elements.
• Do Now:• Word Wise Chapter 4
• What are YOUR Elements?• Today:
• Homework check and Review 4.3 GRWS• Element Practice
• What Atom am I? Review Bohr’s /Lewis Models• LAB: Modeling the Location of an Electron in a Cloud
• Homework:• Textbook Chapter 4 Assessment pg 121+
#1 – 32 Complete sentences
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PARCC BREAK
5 days of PARCC testing – no instructional classes!
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Unit 2 Chapter 4 Day 6 OBJECTIVE:
Demonstrate understanding of atomic structure basics.
• Do Now:• Chapter Assessment Homework Check and Review
• Today: • Atomic Basics – Chapter 4 Quiz
• Homework:• Everyday Elements!• Advertise-the-Elements project Due 4/1/15
POP
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Chapter 4
ATOMS and
AtomicStructure
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Matter•The term matter describes all of the physical substances around us: your table, your body, a pencil, water, and so forth•Anything that has mass and takes up space (has volume)•Made up of different kinds of atoms•Includes all things that can be seen, tasted, smelled, or touched
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Matter is made of atoms
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Models
Models are often used for things that are too small or too
large to be observed or that are too difficult to be understood easily
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Early Models of the Atom Democritus
Universe was made of empty space and tiny bits of stuff
Called these tiny bits of stuff atomos
Atoms could not be divided
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Early Models of the Atom Dalton
All elements are composed of indivisible particles. Atoms of the same element are the sameAtoms of different elements are different. Compounds consisted of atoms of different elements combined together
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Early Models of the AtomThomson
Plum pudding model
Atom made of a positively charged material with the negatively charged electrons scattered through it.
He discovered the ELECTRON!
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Early Models of the Atom Rutherford
Mostly empty space
Small, positive nucleus
Contained protons
Negative electrons scattered around the outside
He discovered the PROTON!
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Early Models of the Atom Bohr
Atom as a planetary arrangement
Electrons move in definite orbits around the nucleus
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Modern Model of the AtomThe Electron Cloud
Sometimes called the wave modelSpherical cloud of varying density Shows where an electron is more or less likely to be (quantum mechanics)
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Atomic Structure
Nucleus –Protons–Neutrons
Electrons
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Electrons Tiny, very light particles
Have a negative electrical charge (-)
Move around the outside of the nucleus
Always moving – can move in any direction within their shell
Is equal to the number of protons
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Protons Much larger and heavier than electrons
Protons have a positive charge (+)
Located in the nucleus of the atom
Identifies the Atomic Number
Made up of smaller particles called quarks
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NeutronsLarge and heavy like protons– 1840 times the mass of an electron
Neutrons have no electrical charge
Located in the nucleus of the atom
Made up of smaller particles called quarks
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Describing Atoms
Atomic Number = number of protons
Mass Number = number of protons plus neutrons.
Atomic Mass (or Weight) = average mass of the naturally occurring isotopes of an element .
In a neutral atom, the # of protons = # of
electrons
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5 6 7 8
B C N O11 12 14 16
Boron Carbon Nitrogen Oxygen
13 14 15 16
Al Si P S27 28 31 32
Aluminum Silicon Phosphorus Sulfur
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Chapter 4
Atoms and Atomic Structure
Part 2
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IonsAn atom that carries an electrical charge is called an ion– The number of protons does not change
in an ion– The number of neutrons does not
change in an ion
SO…both the atomic number and the atomic mass remain the same
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IonsIf the atom loses electrons, the atom becomes positively charged (because the number of positively charged protons will be more the number of electrons)
If an atom gains electrons, the atom becomes negatively charged (more negative charges than positive charges)
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IonsThis atom has lost an electron. Now it has one more proton than electron.
One more proton means one more positive charge.
This makes the total charge of the atom POSITIVE.This atom has gained an electron. Now it has one less proton than electron.
One less proton means one less positive charge.
This makes the total charge of the atom NEGATIVE.
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IsotopesHave the same atomic number (number of protons) The number of protons for a given atom never changes.
The number of neutrons can change.
Two atoms with different numbers of neutrons are called isotopes
Have different atomic mass numbers (number of protons + neutrons)
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Three Isotopes of Hydrogen
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Write symbols for each of the three Isotopes of
Hydrogen?
H H H
Protium Deuterium Tritium
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Isotopes
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Add or Subtract a PROTON
• NEW ELEMENT
Add or Subtract a NEUTRON • ISOTOPE
Add or Subtract an ELECTRON • ION
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Atomic OrbitalsAn orbital is the region of space around the nucleus where an electron is likely to be found
The electron cloud model approximates how electrons behave in their orbitals.
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Electrons and Energy Levels
Each electron in an atom has a specific amount of energy
Possible energies that electrons can have in an atom are called energy levels
An electron can move from one energy level to another when the atom gains or loses energy
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Electron ConfigurationElectron configuration is the specific arrangement of electrons in orbitals.– Each energy level can only hold a specific
amount of electrons– Each energy level must be completely filled
before electrons fill the next level
The number of electrons in the outermost level are called valence electrons– These are the electrons used for bonding!
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Electron Diagrams
Bohr and Lewis
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Bohr’s Model of the Atom
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Rules for filling the model– Start at the lowest energy level
• 1st energy level = 2 electrons(electrons #1 and 2)Place them opposite each other
• 2nd energy level = 8 electrons(electrons #3 to 10)Place them opposite each other -and-Make pairs for easier counting
• 3rd energy level = 18 electrons(electrons #11 to 28)
Bohr’s Model of the Atom
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ELEMENT _____________
# Protons ________
# Neutrons ________
Bohr’s Model of the Atom
ELEMENT _____________
# Protons ________
# Neutrons ________
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Lewis Dot Structures
Lewis dot diagrams are a simple way to show how the electrons are arranged in their outer shell.
This is where chemical reactions take place and how elements bond together.
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Lewis Dot StructuresRules for filling the model:
ONLY VALENCE ELECTRONS
ARE USED
2
3 1
4
WHAT ARE
VALENCE ELECTRONS
?
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Lewis Dot Structures VALENCE ELECTRONS are the electrons found in the OUTERMOST shell of the Bohr’s model.
ELEMENT _____________
# electrons (total) _______
# Valence electrons _______
ELEMENT _____________
# electrons (total) _______
# Valence electrons _______
ELEMENT _____________
# electrons (total) _______
# Valence electrons _______
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Lewis Dot StructuresRules for filling the model:
ONLY VALENCE ELECTRONS
ARE USED
2
3 1
4
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Lewis Dot Structures
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Advertise-the-ElementsGeneral Information
Due date is Wed 4/1 at the beginning of class…Not after you finish gluing this on, or tying that together…Nor after you borrow my scissors and tape…NO…you must walk in here with it ready to turn in or it will be LATE! (Projects turned in after Spring Break cannot earn more than 50% credit MAX)
The Unit Project is worth as much as the Unit Test. Make that work for you.
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Internet SourcesWikipedia (or Wiki-anything) is NOT an acceptable scientific source for this project and cannot be used as a source.
Cost for elements can be found on various sites. Try:Periodic Table of Elements: Los Alamos National Laboratory at http://periodic.lanl.gov/
OR even places like…
http://www.elementsales.com/pl_element.htm
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Cool interactive periodic tables can be found at lots of sites…Try:
http://www.chemicalelements.com/ http://elements.wlonk.com/ElementUses.htm
http://education.jlab.org/itselemental/
Repeat…wiki-ANYTHING is not acceptable
• Try searching for your element in Science Journals. You could find innovative uses and new discoveries.