Unit 2 Matter Chem 1.

Unit 2 Matter Chem 1

Be Seated

CHEMISTRY

Agenda 10/4 Panther Drill 4 Notes (Properties and States of Matter)
PD Redux, If I knew then what I know now WS Sci Notebook Sec 3.1 Close/Exit Ticket

Panther Drill 4 Identify the state of matter of the following: (IE is it Liquid ect) O2 Water Ice Water Vapor Inside Florescent Lights Blood Jell-O The Sun Gas Liquid Solid Gas Plasma Liquid Solid Mostly Plasma, Some Gas

Substances A substance is matter that has definite composition and properties. i.e. Table salt (NaCl) always has the same make-up and properties no matter if you put it on your popcorn in Lake City, Murrells Inlet, or Lake City Colorado. Whereas salt water found in the pacific ocean is different than salt water found in the arctic ocean.

COMPOSITION OF MATTER What is MATTER? Anything that Takes up Space and Has Mass. What are the States of Matter? Solid, Liquid, Gas, Plasma 1) Solid: Definite volume and definite shape (Glass) 2) Liquid: Definite volume indefinite shape (Water)

Solids and Liquid In a solid. all molecules vibrate and forces of attraction hold them in place. In a liquid the molecules have partially overcome the forces of attraction and still partially in contact

COMPOSITION OF MATTER Gas: Indefinite volume, indefinite shape.
IE Car Exhaust Plasma: High temperature physical state, made up of free electrons and ions of the element IE Florescent Lights, Mushroom Cloud, the northern lights, and Plasma TVs.

Gas and Plasma Molecules have completely over come attractive forces, any contact is random. Movement is extremely fast and electrons are striped away from the molecules.

Characteristics of States of Matter

Properties Extensive properties: properties that depend on how much of matter is present. i.e. Volume and Mass Intensive properties: does not depend on how much matter is present i.e.: density and boiling point

Physical Properties Physical Properties: something that can be changed in a substance w/o changing its identity. i.e.: Melting Ice Cutting a 2x4 in half Boiling

Chemical Properties Matter
Chemical Properties: changes that result in a substance being changed into new substances. i.e.: Burning charcoal = carbon ash and O2 & CO2 Iron Rusting ** A physical or chemical change requires energy to be added to what ever is changing (aka the system) Energy can be heat or light other forms

Shoulder Partners Answer and check ea. other answers
Mushroom Cloud S,L,G,P Shampoo S,L,G,P Jell-o S,L,G,P Burning Gas Physical or Chemical Baking Cookies Physical or Chemical Maxing Salt water Physical or Chemical Odor Extensive or Intensive Weight Extensive or Intensive Color Extensive or Intensive

Compare and Contrast Extensive and Intensive properties
Before you pack up Compare and Contrast Extensive and Intensive properties Show it to me before you leave

10/5 PD 5 Notes Example Conservation of Mass
Do practice problems w/ partners Exit Problem

New Seats 1st Pd Abria Sam Jessica Howard Trevon Mary Brenton Qual
Raven Brad Drequan Latonya Cassidy Ware Cody Hank Quaneshia

Modified Seats 3rd Period
Go to your seats and Panther Drill will start at bell Justice Porchea Spud Yessie Galloway Gaskins Pace Stukes Ashley Belinda Amber Cordrick Wade Josh Kyianna Terrance Breanna

New Seats 5th Brianna Whitley Doward Ashley Charles Hunter Nigel Raven
Dela Jaleel Nessie Trevin Jamond Wu Tang Amanda Faith Aminia Will C. Tommy Chris Austin Eddy

Modified Seating 6th Period
Sade’ Jasmine Kayla Nasia Jaron Justin Demond Whitney Tykosha Terica Shekia Willie Quay Keshon Reggie Steve Tyiesha Rayneesha Jamika Diamond Dominque

Panther Drill #5 Think about what you know about nature, tell me about how the physical phase change of water, effects the natural world.

Kinds Physical Changes
Freezing is the change of state from a liquid to a solid. Melting is the change of state from a solid to a liquid. Vaporization is the change of state from a liquid to a gas. Condensation is the change of state from a gas to a liquid. Sublimation is the change of state from a solid directly into a gas. Deposition is the change of state from a gas directly into a solid.

Example More energy in the system Less energy in the system

State Changes and the Environment

Chemical Reactions In a chemical reaction there are the reactants and the products. Reactants: what you start with Products: what you end with 99.08g Fe g O2  155g Fe2O3(Rust) Reactants Products What is the mass of the Fe and the O? What is the mass of the Fe2O3? 99.08g g 155g

Law of Conservation of Mass
“Matter can’t be created or destroyed in a chemical reaction, it is conserved” That means the mass of the reactants = the mass of the products. Mass reactants = Mass products Get in your pairings and work on problems

Partners 1st Period Brad & LaTonya Mary & Qualisha Quanisha & Howard Hank & Brenton Jess & Abria Raven & Cody Sam and Devonte Cassidy and Devonta Trevon’ & Drequan

Partners 3rd Period Josh & Cordrick Kyiana & Belinda Breanna & Terrance Justice & Yessie Galloway & Cadejah Gaskins and Spud Brandon and Porschea Ashley, Amber, & Clarence

Partners 6th Period Jaron & Willie Steve & Diamond Jamika & Dominique Tiesha, Keshon &Shekia Reggie, & Kayla Nasia & Tykosha Justin & Quay Sade’ & Whitney Jasmine & Demond Rayneesha & Terica

Partner A show partner B how to do Problem #1 Then Reverse roles
When 245 grams of KClO3 are heated, the KClO3 breaks down into 78 grams of potassium, 71 grams of chlorine and some oxygen gas. What is the mass of oxygen gas formed? You have 729 g of NaOH (Sodium Hydroxide) is broken down into its parts. What resulted was 459 g of Na, 127 g of Oxygen, and how many grams of Hydrogen?

Do number 6,7&8 from pp 78 in your text by yourselves, and show it to me, before you pack-up

Agenda 10/6 PD #6 Notes/Discussion (Mixtures/Pure Substances/Separation) PD Redux Exit Assignment Lab Thurs. Reminder

Panther Drill #6 DRESS FOR LAB Tomorrow THURSDAY 10/7
Identify the following items (NOT as solid liquid or gas) but as mixtures or pure substances. Aluminum Table Salt Water Stainless Steel Kool Aid Carbon Pure Mixture Pure Mixture Mixture Pure DRESS FOR LAB Tomorrow THURSDAY 10/7

Classification of Matter
Matter is classified as either a MIXTURE or a PURE SUBSTANCE. 1) Pure Substances: is homogeneous and has a fixed composition. Every sample has the exact same properties IE all pure water boils at 100C and freezes at 0C Every sample has the exact same composition IE all pure water has 11.2% H and 88.8% O2

2 kinds of pure substances: Compounds and Elements Elements: a pure substances that can not be broken down into simpler parts IE Carbon Compound: a substance that can be broken in to simpler substances. IE WATER - H and O

2) Mixture: blend of 2 or more kinds of matter, where each different type of matter keeps its own identity or properties. Mixtures can be broken down into their original parts. 2 kinds of mixtures: Homogeneous: these have uniform composition always in a single phase, blended uniformly. Steel (a mix of carbon and iron) Milk Mayonnaise Solutions

Mixtures Cont. Heterogeneous: these are not uniform, their composition changes from sample to sample, they are not blended smoothly. Buttermilk Fresh squeezed orange juice Homemade mashed potatoes Pond water

Separating Mixtures Filtration: using a filter to separate the a heterogeneous mixture of solid and liquid Distillation: using different boiling points of substances in a homogeneous mixture to separate it

Separating Mixtures Crystallization: when pure solid forms from a liquid solution containing as much solid as can be held be the liquid (super saturated). Solid is then formed as the liquid evaporates (Think making rock candy.) Sublimation: separation of solids and gas w/o going through liquid state

Separating Mixtures Chromatography: separate the components of a mixture (liquid or gas) by allowing it to move across another material (i.e. paper). The components separate because the move across the paper at different rates.

If I only knew then what I know now…
Identify the following items as mixtures ore pure substances. Oxygen Sugar Gator Aid Pizza Water Pure Mixture Pure Mixture Mixture Pure

Text assignment pp 83 #16,18 Due before you leave

Get into you lab Groups Start Pre-Lab questions and assign jobs to members. Equipment Person Experimenter Recorder Leader/Clean up If 5 in group then divide leader and cleanup

Thursday 10/7 Agenda Panther Drill 7 Lab “” Closure

Panther Drill #7 Get into your lab groups and see who in your group is in violation of Lab Safety Rules.

Friday 10/8 Early Dismissal
Agenda Panther Drill 8 Turn in for quiz Finish Analysis and Conclusions for lab from 10/7

MONDAY Agenda 10/11 PD 8 quiz Notes/Discussion (Elements/Compounds/Periodic Table basics) (10 min) WS 3.4 (10 min) Trading Card Game Elements/Compounds (10 Min) Exit Ticket 5 min

Panther Drill #8 2 1 Can you explain in your own words….?
Write out 2 sample quiz questions based on last weeks material that start with: Write out 1 sample quiz questions based on last weeks material that start with: Can you explain in your own words….? How many...? Can you distinguish between ….? Can you name the...? Can you tell why...? Find the meaning of...? Can you design a ... to ...? Compare and contrast….? Explain the differences between…? Rank the following based on…..

QUIZ CHOOSE 4 TO ANSWER Compare and contrast a physical and chemical change. Explain the best way to separate the pulp from fresh squeezed OJ, and the best way to separate salt water into its components. Explain the law of conservation of mass. Compare the molecule structure of the all 4 states of matter. List and explain 5 of the 6 physical changes of matter.

Elements Elements are pure substances that can not be broken down into simpler substances by physical or chemical means. Oxygen, Carbon, Boron ect. Abbreviated by 1,2,or 3 letter abbreviation 1st letter always capitalized. O, Al, Zn, Uus (Ununseptium) 91 NATURALLY occurring elements on the earth.

List some compounds that you encounter every day life:
Compounds are a combination of 2 or more different elements that have combined or bonded chemically. Most of the matter in the universe is compounds. There are approx 10 million known compounds with more discovered or created all the time. List some compounds that you encounter every day life:

Gasoline C8H18 Baking soda CHNa03 Milk of magnesium (Medicine) Mg(OH2) Cream of tartar (Used in cooking) KC4H5O6

Periodic Table The periodic table is table that organizes all known elements into horizontal rows and vertical columns based on their properties. The modern periodic table is based mainly on the work of Russian Scientist Dmitri Mendeleev. Mendeleev’s predictions of blank yet to be discovered elements and where they would fit in the table were pretty much right on. We will do much more work with the periodic table later in the semester.

Mendeleev’s Periodic Table

Modern Periodic Table

Tuesday Agenda PD 8 How do compounds made of the same elements differ, and what does that mean to their properties. (5min) WS 3.4 (Notebook) 10 (min) Notes/Discussion Law of Definite proportions (10 min) Modeling Example Law of Definite proportion problems (10 min) Independent practice problems (20 Min) pp78 #s 20-23 Exit ticket (5 min)

New Seats 5th Brianna Whitley Doward Ashley Charles Hunter Nigel Raven
Dela Jaleel Nessie Trevin Jamond Wu Tang Amanda Faith Aminia Will C. Tommy Chris Austin Eddy

Answer the following question:
Panther Drill 9 Answer the following question: How do compounds, made of the same elements differ, and what does that mean to their properties? IE H2O and H2O2

WS 3.4 Take the first min to start WS # 3.4, us section 3.4 in the Chem Text to complete it and then put it in the Classwork Section of your notebook.

Law of Definite Proportion
Individual Compounds are named and defined by the number and ratio of the elements they are made of. WHAT IS A RATIO? Relationship between two of the same kind of numbers. The relationships in this case of the subscripts or small #s below each elements, which is the # of atoms of that element in the compound.

Law of Definite Proportion 2
This is so important that it is stated in a law of moderns Chemistry, The Law of Definite Proportion. This law says that in a compound the elements are always present in the same proportion. IE: H20 There are always 2 Hs for every 1 O in water.

Formula you need to know how to use
Percent mass or mass percent = Mass of the element x100 Mass of the compound …

Mass Percent A 25 gram sample of water contains 2.80 grams of hydrogen. What is the mass % of hydrogen? 2.80g/25g X 100 = 11.2%

Panther Drill 9 A Think about the law of conservation of matter. If a 13 gram sample of element X combines with a 34.7 gram sample of element Y, to form compound XY, what will the mass of compound XY be? A 25.3 sample of an unknown compound contains .0.8 grams of oxygen. What is the mass percent of the oxygen in the unknown compound? When mercury oxide is heated it breaks down into its components of mercury and oxygen grams completely breaks down it yields 2.0 grams of oxygen. What is the mass percent of mercury in mercury oxide? `

Law of Multiple Proportion
States: when different compounds are formed by the combination of the elements X and Y, then the ratios between elements change, one element is usually consistent in its subscript while the other usually changes. ie. H2O and H202 The H stays consistent and the Oxygen subscript changes

EXAMPLE Lets compare 2 different compounds a containing copper and chlorine. Compound 1 contains 64.2% copper and 35.8 % Chlorine. Compound 2 contains % Copper and % Chlorine.

Now we have to determine the RATIO of copper to Chlorine in each Compound. To do that we divide the Mass % of the copper by the mass % of the chlorine in each compound Formula: Mass % element 1 Mass % Element 2 = Ratio of g Element 1 per g Element 2

Compound 1: 64.2 % Cu = g Cu : 1 g Cl 35.8 % Cl

Compound 2: 47.27% Cu = g Cu : 1 g Cl % Cl

Now we find the ratio of copper between compound 1 and compound g Cu/1 g Cl = g Cu /1 g Cl SO The ratio is 2: 1 Compound 1 : Compound 2

This is important because there are only about 116 elements n the world and multiple proportion allows for exponentially more compounds

Try This 1 Draw table and fill in the information
Compound Total Mass Compound Mass Iron Mass Oxygen Mass % Iron Mass % Oxygen A 75.00 g 52.46 g 22.54 g B 56.00 g 43.53 g 12.47 g Mass % = Mass Element x 100 Mass Compound

Mass % Compound A= Fe: 52.46/75.00 x 100 = about 70 %
Total Mass Compound Mass Iron Mass Oxygen Mass % Iron Mass % Oxygen A 75.00 g 52.46 g 22.54 g 70 % 30 % B 56.00 g 43.53 g 12.47 g 77.7 % 22.3 % Mass % Compound A= Fe: /75.00 x 100 = about 70 % O: 100 % - 70% = 30 % Mass % Compound B= Fe: /56 x 100 = about % O: 100 % - 76% = %

Use the Law of Multiple proportion to find the ratio between Compound A and Compound B from the table. Mass Ratio Formula For a Compound: Mass of Element 1 (Fe) Mass Element 2 (O) g Fe g O Compound A Ratio= 2.33 g Fe/ 1 g O

Now compare compound A to Compound B
You Do Compound B 43.53 g Fe g O = 3.5 g Fe/g O in Compound B Now compare compound A to Compound B 3.49 g Fe Comp B/ 2.33 g Fe Comp A = 3.5 g Fe Comp B: 2.33 g Fe Comp. A

Chapter 4 Friday: 4.1 TSWBAT: Define and atom Create a time line citing the key milestones leading to the modern atomic theory.

Panther Drill # 11 Brainstorm Quick Write: Just “stream of consciousness” write and put down as many facts that you can think of about the atom!!!

Early Theories of matter and atoms
Greek Philosopher Democritus about 400 BC 1st to suggest atoms 1st to suggest matter is empty space that atoms move through Atoms were solid and could not be divided into any thing smaller. Atoms were of different sizes and shapes Properties depended on shape, size and movement of atoms

Early Theories of matter
Greek Philosopher Aristotle about 350 BC He was the “Rock Star” of his time He rejected Democritus’s Ideas because the were opposite of his.

Not much new progress made for about 2100 years or so

John Dalton All elements are made up of atoms. It is impossible to divide or destroy an atom. All atoms of the same elements are alike. Atoms of different elements are different. Atoms of different elements combine to form a compound.

Thompson’s Plum Pudding Model J.J. Thompson Late 1800’s English scientist. He discovered the electron when he was experimenting with gas discharge tubes. He saw that they moved to the positive end of the gas tube and figured out that they had a – charge.

Lord Ernest Rutherford Famous for gold foil experiment that showed that some + charged particles could pass through a thin layer of gold foil and some bounced back proving that matter contained empty space and atoms had a + charged nucleus that made some particles “bounce back”.

Niels Bohr Early 1900’s He proposed a model of the atom that is similar to the model of the solar system. There are different energy levels or electron orbits around the nucleus, like the different planets orbit the sun at different distances. Bohr Model Nitrogen

Your Assignment: Use the notes you have plus the book if you have it to create a time line the tells the story of the development of the atomic theory. Use color and try to make it as neat as you can the best will be put up on the wall of fame. The Assignment is due Monday 10/18 and is worth 15 points it will be graded as follows: 6-7 Entries 12 points 5 entries 11 points 2-4 entries 8 points 1 entry 5 points Neatness, and Creativity can get you up to 3 points

Example of a time Line

Monday 10-18 PD 12 Demo Rutherford experiment Work on project

Panther Drill 12 In your opinion who do you think is the most important person in the development of the modern atomic theory. Use your notes and your own research to decide.

New Seats 1st Pd Abria Sam Jessica Howard Trevon Mary Brenton Qual
Raven Brad Drequan Latonya Cassidy Ware Cody Hank Quaneshia

Panther Drill #13 Period 1 Write down 2 possible test questions about atomic theory, on the paper on your desk. One can be a basic question, one needs to be a harder extended response type question using question stems for analyzing and applying for the second question. PLEASE WRITE IN THE ½ SHEETS YOU HAVE AND NOT THE FULL SHEETS.

Panther Drill #13 Particle Location Charge Size Electron Proton
Proton Neutron Create and fill in the blanks in the table, for size rank the particles 1 2 or 3 for size

Atoms The Atom: Smallest particle of matter that will retain its properties. Size: A single copper atom is or 1.28 x meters in diameter. The only way it is possible to see an atom is to use a scanning tunneling microscope STM, a very fine sharp point is moved over a sample and it interacts w/ the superficial or surface atoms and this interaction is recorded by a computer.

STM images Silicon Nickel

STMs Informational Only STMs are allowing science to start to develop “nanotechnology” meaning they are able to build machines the size of a molecule, 1 atom at a time. Here is an example of a scientist w/ too much time on their hands!!!!!!

Electrons Formally discovered to have a negative charge and a definitive mass, by JJ Thompson in 1897, use a cathode ray tube. The strength of the – charge was determined by Millikan and the oil drop experiment. The electron was found to have a mass of 1/1840 of 1 Hydrogen atom or 9.1 x grams.

Electron Cloud Electrons are not really in defined orbitals, but are found in a cloud. The cloud shows where the electrons are likely to be at any given time.

Heisenberg uncertainty principle
A math equation that states position and momentum, cannot be simultaneously known to high precision. Means that we can either know what way an electron is moving or where it is but not both at the same time.

Schrödinger's cat Schrödinger's cat is a thought experiment, often described as a paradox, devised by Austrian physicist Erwin Schrödinger in It illustrates what he saw as the problem of the Copenhagen interpretation of quantum mechanics applied to everyday objects. The thought experiment presents a cat that might be alive or dead, depending on an earlier random event. In the course of developing this experiment, he coined the term quantum entanglement.

Quarks There are six quarks, these are the particles that make up protons and neutrons for our purposes we will deal with up and down quarks. Up quarks have a + 2/3 charge Down quarks have a -1/3 charge

Protons, Neutron and the Nucleus
Protons: Found by Rutherford Charge of +1 Mass x

Protons, Neutron and the Nucleus
Neutron: Confirmed by James Chadwick in 1932 Charge : Neutral or 0 Mass x

To Sum it Up a.m.u. = atomic mass unit, about 1 proton or neutron of a Hydrogen atom.

Panther Drill # 14 Sketch an atom.
How many Protons, Neutrons and Electrons are in the following element.

Different Elements We know protons and neutrons are in the nucleus and electrons are outside but how do atoms for different elements vary? I mean how is Hydrogen different from Helium? See the atomic # on the periodic table H=1 and He = 2 ect This means that H has 1 proton and 1 electron And Helium has 2 protons and 2 electrons ***REMEMBER # OF ELECTRONS = # PROTONS IN A NORMAL ATOM***

Reading the Periodic Table
Atomic Number Elements Symbol Chemical Name Average Atomic Mass

Reading the Periodic Table No need to write this
Remember not all periodic tables are as detailed as others some have more information than the basics like this one.

Neutrons Lets look at Hydrogen and Helium on the periodic table

We see the atomic #, but what is the number underneath the symbol?
THAT IS THE ATOMIC MASS To find the # of Neutrons all we do is round the atomic mass to the nearest whole number. This is called the mass number Try it w/ H and He H= 1 He = 4 Then we subtract the # of protons from the Mass Number Neutrons = Mass Number - #protons H: 1-1 =0 (no neutrons in Hydrogen) He 4 – 2 = 2 (2 neutrons in Helium)

Lets Try Some Get w/ a Partner
How Many protons neutrons and electrons in Lithium? In Carbon? In Zinc (Zn)? Mass Number = = 7 Atomic # = 3 Protons = atomic # = 3 Electrons = protons = 3 Neutrons = Mass Number - # protons = Neutrons Mass Number = = 12 Atomic # = 6 Protons = atomic # = 6 Electrons = protons = 6 Neutrons = Mass Number - # protons = Neutrons Mass Number = = 65 Atomic # = 30 Protons = atomic # = Electrons = protons = 30 Neutrons = Mass Number - # protons = Neutrons

Run it back What element has 5 neutrons and 4 protons. Atomic # = # Protons = 4 = Beryllium What is the name of the element with 31 neutrons and 28 electrons? What is the element? # of electrons = # protons = atomic # = 28 = Nickel = (atm mass)

Try Some on Your Element Sheet

Panther Drill 15 How many protons, neutrons and electron does Gold have? What is a isotope? How do you explain hydrogen with 2 protons?

Isotopes LCHS Laptop Isotopes Flash Drive
Isotope Video Clip Isotopes LCHS Laptop Isotopes Flash Drive

Isotopes Atoms that have the same number of protons but different numbers of neutrons. Most atoms have isotopes. Hydrogen has 3 different isotopes.

Remember SO # Neutrons = Mass # - Atomic #
Isotopes Remember # Neutrons = Mass # - Atomic # SO Mass # = atomic # (aka # protons) + # neutrons.

Isotope Carbon has 2 isotopes Carbon-12 & Carbon-14

Isotopes Find out the number of neutrons in an isotope the same way as in a normal element. Neutrons = Mass Number - Atomic # or protons

Isotope Notation How do I write and isotope? Sym
Mass # ATM # How would you write the isotopes of copper: 1 w/ a mass number of 63 1 w/ a mass # of 65

63 Mass # 29 # protons 65 Mass # 29 # protons
How would you write the isotopes of copper: 1 w/ a mass number of 63 1 w/ a mass # of 65 a) Cu b) Cu 63 Mass # 29 # protons 65 Mass # 29 # protons

Why not whole # atomic mass
Elements have isotopes so we don’t whole # atomic masses. Atomic mass = Atomic # Elements and their isotopes occur in different natural abundances To find the atomic mass we use a weighted average

Weighted Average If a 75% of the apples in a box have a mass of 149 grams and 25 % of the apples a mass of 153 grams. What is the average mass of an apple in the box? Formula: [mass (item1) + (% item1 x .01)] X [mass (item2)x (% item2 x .01)]

Weighted Average Item 1 = Apple 1 = mass 149g and 75% abundance
[mass (item1)x (% item1 x .01)] + [mass (item2)x (% item2 x .01)] Item 1 = Apple 1 = mass 149g and 75% abundance Item 2 = Apple 2 = mass 153g and 25% abundance Avg. mass of apple = [149 g x (75% x .01)] + [ 153 g x (25% x .01) 111.75g g = 150 g The average apple has a mass of 150 grams

Do Problems 18 and 24 on page 121 in your book
Class Work Do Problems 18 and 24 on page 121 in your book on handout Let me see at least 18 before you leave!!!

Panther Drill 16 Silver has 2 isotopes 107 & 109 Ag Ag
Ag Ag Based on Silvers atomic mass from the periodic table, which isotope is more abundant??

Agenda 10/25 Panther Drill 17 (3 Q’s 1 review from last week and 2 to assess pre-knowledge of today’s topic) Notes and Discussion (Teacher will explain Nuclear rxns, Radioactive decay (Unstable Nuclei), alpha, beta, and gamma radiation). WS 4.4 From Text. Thumbs up or Down Review.

Panther Drill 17 Why do elements have on the periodic table have decimals in their atomic masses instead of whole numbers. What is radiation? What is a nuclear reaction?

Radioactivity Discovered in 1890s when scientists noticed energy constantly being emitted they called this radioactivity. This energy was called radiation. Atoms that emit radiation are called radioactive atoms. The energy emitted was in the form of particles and rays of energy.

Nuclear reactions It was found the radioactive atoms were not undergoing a chemical reaction but what is called a nuclear reaction. Nuclear reactions are changes in the nucleus of an atom where energy is released. Atomic nuclei that emit energy through nuclear reactions are called unstable. After the unstable nuclei release energy and become stable, they become new isotopes or even other elements. This is called radioactive decay.

Radioactive decay

Positive charged plate Negative charged plate
In an experiment shows the 3 types of radiation

Alpha Radiation Alpha particles are the form of radiation that is drawn to the neagative charged plate in the experiment. An alpha particle contains 2 protons and 2 neutrons so it is the same as a helium atom. Alpha particle is shown as 4HE or a 2

Beta Radiation Beta particles were drawn to the + charged plat in the experiment. A beta particle is really and – charged electron and is shown as an electron or b particle This release allows the neutron to change to proton b

Gamma Radiation Gamma radiation or g is the only of the 3 types to be an energy ray instead of a particle It is not influenced by the + or – charged plate. It has no mass whereas the other 2 do.

Agenda 10/27 PD # 18 (3 Q’s, 1 review and 2 to assess prior knowledge.) (7 min) Notes/Discussion (Students will be re-introduced to electron configuration models, Including Bohr Models) (15 min) Guided Practice (Instructor will model for students creating Bohr models) (5-10 min) Students will illustrate electron configurations using Bohr models, of simple atoms in pairs. Instructor will observe and assist struggling students. (15 min) Some groups will show their models on the Prom Board.

Panther Drill 18 What are the differnece between alpha and beta radiation. How many electrons are in a Carbon atom? How do you show them in a Bohr Model?

Electron distribution
We will talk a lot more about electrons in a month or so but lets look at how to create models of the atoms showing electrons, protons, and neutrons. Now in reality we know that the electrons exist in electron clouds around the nucleus, but we will use MODELS that show them in orbitals like the a solar system. These are called BOHR MODELS.

Electron Cloud vs Bohr Model
CHLORINE Electron Cloud Bohr Model

Electron Orbitals n=5 n=4 Orbitals are abbreviated as n. There are more than can be as many as 7 orbitals or energy levels. n=3 n=2 n=1 Nucleus

Electron Orbitals Max Electrons for each n level. Level1 2 e- Level2: 8e- Level3 18e- Level 4 32e- Level 5 50e- N=5 N=4 N=3 N=2 N=1 8 e- 32 e- Nucleus 2 e- 50 e- 18 e-

Atom with 7 protons and 6 neutrons. Atom with 3 protons and 3 neutrons
Lets try some Atom with 7 protons and 6 neutrons. Atom with 3 protons and 3 neutrons

Panther Drill # 19 What is the difference between the Bohr model and the “more realistic” electron cloud model? What are valance electrons? Is this Bohr model correct, if not why? e- 5P 4N e- e- e- e- e-

Valence Electrons The electrons in the outermost shell are the valence electrons The valance electrons are the electrons on an atom that can be gained or lost in a chemical reaction. What element is this? How do you know? Where are the valence electrons? e- e- e- e- e- e-

Circle the valence electrons
Volunteer or Victim Circle the valence electrons e- e- e- e- e- e- e- 13 P 14N e- e- e- e- e- e- e- e-

Review of Bohr Max Electrons for each n level. Level1 2 e- Level2: 8e- Level3 18e- Level 4 32e- Level 5 50e- n=5 n=4 n=3 n=2 n=1 8 e- 32 e- Nucleus 2 e- 50 e- 18 e-

Project You will be assigned your choice of a poster project of an atom or creating a 3-D Bohr model of an atom. It is your choice the assignments can be seen in full on the assignment sheet handout. When you have decided then get a full handout that includes the rubric, real quick let’s look at some examples of real creative 3-D models from other students. 3D EXAMPLES The basics of the projects can also be seen on the front bulletin board if you can need them.

3-D Model Due Friday 11/5 Your 3‐D model of your atom is DUE ON Friday 11/5. In addition to your 3-D model, you should include a short write up that includes al of the following list: Element Name Atomic number Chemical symbol Metal/non‐metal/metalloid? State or phase at room temp. Uses Any interesting facts Characteristics or properties Number of electrons, neutrons, and protons The elements you have to choose from for the 3-D model are Hydrogen through Argon on the periodic table. If you need to see examples again go to website (Power Point Note section) and look at the 3-D model Power Point.

Poster Due Wednesday 11/3 Along with a Bohr model drawing of your atom your poster must display the following information on the front so it can be seen: Element Name Atomic number Chemical symbol Metal/non‐metal/metalloid? State or phase at room temp. Uses Any interesting facts Characteristics or properties Number of electrons, neutrons, and protons Your choices for your Bohr Model atom posters are any atom from sodium and higher in atomic number on the periodic table.

Exit Ticket Name________________________________
Circle the valence electrons. What is their function. On the back sketch and label a Bohr model of Silicon or Magnesium Drop in basket before you leave. HAVE A GREAT DAY!! e- e- e- e- e- e- 13 P 14N e- e- e- e- e- e-

Panther Drill 20 Define valence electrons and state their main job in the atom.

Heisenberg Uncertainty Principle (review)
The Heisenberg Uncertainty Principle says - loosely - that you can't know with certainty both where an electron is and where it's going next. What it actually says is that it is impossible to define with absolute precision, at the same time, both the position and the momentum of an electron.

Purpose Electron configuration notation is a written and visual and written method of noting every thing we can about 1 given electron in an atom’s ground state. Ground state: the atom’s lowest most stable energy state or condition. This the condition represented on the periodic table.

Orbitals and principal quantum numbers
As we learned with Bohr models, n = the electron energy levels or orbitals. n is also referred to as the principal quantum level. Trends As n increases, the orbital becomes larger and the electron becomes farther from the nucleus. As n increases the amount of energy of the electrons increase. ADD THIS: The higher the quantum levels are less stable than the lower levels.

In the Bohr Model Nucleus Principal Quantum Level 1

Sublevels Principal energy levels contain energy sublevels or orbitals. (n=1) Principal energy level 1 contains 1 sublevel (n=2) Principal energy level 2 contains 2 sublevels (n=3) Principal energy level 3 contains 3 sublevels

Sublevels are labeled s, p, d, or f depending on their shape

S orbitals s orbitals are spherically and symmetric around the nucleus

P orbitals A p orbital is rather like 2 identical balloons tied together at the nucleus.

P orbitals At any energy level (or n level) it is possible to have 3 p orbitals or sub-levels at right angles to each other P sub shell can have a total of 6 e- (2 in each orbital)

D sub level “d” sub level has 5 orbital and can hold 10 electrons. “d” does not start to get filled untill after 4s is filled.

F sub level “f” orbital has 7 orbitals, and the first ‘”f” orbital is seen in the 4th energy level. 4f does not begin to fill until after level 6s is full.

Aufbau Principle The Aufbau principle states that each electron occupies the lowest energy level available.

This is the order they fill up in. Just follow the arrow.
Start here and follow the arrow This is the order they fill up in. Just follow the arrow.

Would you want to share a room with someone if you didn’t have to?
Hund's Rule Within a subshell, the electrons will occupy the orbitals by themselves first, and will only pair up when there are no longer any empty orbitals available in that subshell. Would you want to share a room with someone if you didn’t have to?

The Pauli Exclusion Principle
This principle says that an orbital is filled when it contains 2 electrons. After that, you have to put the electrons in a different orbital. Each type of subshell (sublevel) contains a different number of orbitals. And, each orbital can hold ONLY 2 electrons.

The Pauli Exclusion Principle
Subshell Type # of Orbitals Maximum # of Electrons s 1 2 p 3 6 d 5 10 f 7 14

Write the notation this way
Carbon= 6 electrons It fills like this 2s 2 p The arrows point in opposite directions in each box because they spin in opposite directions because the – charges repel each other 3s 3 p 4s 3d

Write the notation this way
Why do the fill each box w/ one arrow 1st The arrows point in opposite directions in each box because they spin in opposite directions because the – charges repel each other 2s 2 p 3s 3 p 4s 3d

Lets try some

1s 2s 2 p 3s 3 p 4s 3d

Panther Drill 21 How many electrons can be in each ORBITAL ?
Complete the electron configuration for Fluorine. 1s 2s 2 p

Panther Drill #22 In what order do the following sublevels fill up with electrons? 4s 3s 2p 3d 2s 3p 1s How many valence electrons are in N and in Mg?

Principal energy levels contain energy sublevels or orbitals.
(n=1) PQL 1 contains 1 sublevel (s) (2 total e-) (n=2) PQL 2 contains 2 sublevels (s & p) (8 e- total) (n=3) PQL 3 contains 3 sublevels (s, p, & f) (18 e- total)

Written Electron Configuration
After the standard orbital notation (boxes and arrows), we need to know how use written electron notation. This is much simpler! All you do is look at the boxes and write out what is in them.

Written Electron Configuration
2 p 1s 2s Write this as follows: 1s22s22p3 2p3 n or quantum level Number of electrons in the sub level. Sub Level

Write the correct electron notation and identify the element.
1s2 2s2 2p6 3s2 3p4 1s 2s Atomic # 16 S Sulfur 2p 3s 3p 4s 3d 4p

Write the correct electron notation and identify the element.
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4 Write the correct electron notation and identify the element. 1s 2s Atomic # 34 Se Selenium 2p 3s 3p 4s 3d 4p

Panther Drill 23 In electron notation (not box and arrow diagrams), write the notation for the following elements: Oxygen Neon Argon 1s22s22p4 1s22s22p6 1s22s22p63s23p6 4s23d104p6

Still a lot of writing? We can use the Noble Gas Notation. Noble gases come from group 18 on the periodic table Put the noble gas symbol in brackets [Ne] to show that the all levels in it are full and stable. Then use notation to show the electrons in the outermost orbital. Try Magnesium in your notes Mg = [Ne] 3s2

In your notes Write the noble gas notation for: Nitrogen Calcium Copper

Noble Gas Electron Notation Potassium - Krypton Electron Configuration
Element Atomic Number Electron Configuration K 19 [Ar]4s1 Ca 20 [Ar]4s2 Sc 21 [Ar]4s23d1 Ti 22 [Ar]4s23d2 V 23 [Ar]4s23d3 Cr 24 [Ar]4s13d5 - note: 1/2 filled subshells Mn 25 [Ar]4s23d5 Fe 26 [Ar]4s23d6 Co 27 [Ar]4s23d7 Ni 28 [Ar]4s23d8 Cu 29 [Ar]4s13d10 - note: 1/2 filled s subshell Zn 30 [Ar]4s23d10 Ga 31 [Ar]4s23d104p1 Ge 32 [Ar]4s23d104p2 As 33 [Ar]4s23d104p3 Se 34 [Ar]4s23d104p4 Br 35 [Ar]4s23d104p5 Kr 36 [Ar]4s23d104p6 = [Kr]

Orbital Filling Periodic Table
1s 2s 2p 3s 3p 4s 4p 3d 5s 5p 4d 6s 6p 5d 7s 6d 7p when more discovered 4f 5f

Orbital Filling Periodic Table Fill-in

GO TO ACTIVE INSPIRE ELECTRON DOT DIAGRAM

Electron Dot Diagrams Because valence electrons are the ones that are involved in CHEMICAL BONDING, we often represent them in a visual short-hand called electron dot diagrams or Lewis diagrams. These are simple to do, they only show the valence electrons. So for the simplest atoms like we will look at

Lewis or electron Dot Diagrams
Here is an example: Phosphorus has how many valence electrons? 5

Fill in the Electrons in this order.
1st e- 3rd e- 7th 5th 2nd e- 6th

Panther Drill Take a few minutes to either study or add to your cheat sheets. If you can do this reasonably quietly, you can have up to 10 min. As soon as it becomes too loud, you will not have any more time and we will start the test. Notebooks for unit 2 will be checked after you turn your test in.

Unit 2 Matter Chem 1.

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Unit 2 Matter Chem 1.

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