Warm Up….complete on the top third of page 7 in your notebook Where is the mass in an atom? What is the overall charge of the nucleus of an atom? How do you know? 3. Sesame street: For the 4 vocab terms listed, Which three go together? WHY? Which does not belong? WHY? Proton Nucleus Electron Neutron Homework: Study for Quiz States of matter Atomic structure Periodic table cells M&M’s or skittles Date Session # Activity Page 9/7-8 3 Subatomic Particle Calculations 7 Subatomic Information on the Periodic Table -Notes 8 Bohr Model & Lewis Dot Practice 9 Bohr Model & Lewis Dot Diagram Rules 10

8.P.1 Understand the properties of matter and changes that occur when matter interacts in an open and closed container. 8.P.1.1 Classify matter as elements, compounds, or mixtures based on how the atoms are packed together in arrangements.

TLW calculate atomic structure by taking notes, summarizing demonstrations and completing atom family periodic table cells.

Bringing it all together… For example, OXYGEN is an element on the periodic table. It is made of only one type of atom Actual Oxygen Atom Oxygen on the Periodic Table

In the middle section of p. 3… Compare and contrast protons, neutrons and electrons. Protons Neutrons electrons

Bottom Third of page 3 Explain the following cartoon. Your answer should be in complete sentences and use correct vocabulary. Vocabulary today: Matter States of Matter Solid Liquid Gas Atom Element Proton Neutron Electron Volume Mass

Atomic Number = number of protons PERIODIC TABLE CELLS Atomic Number = number of protons atomic ID # In a neutral atom, the number of protons is equal to the number of electrons What other numbers in your life act as an identification number?

CO ≠ Co SYMBOL RULES: ELEMENTS START WITH A CAPITAL LETTER Any other letters in the symbol are lower case…Just like when you write your name Co ≠ CO !! CO ≠ Co

Comparing protons, neutrons & electrons P 7 middle section Comparing protons, neutrons & electrons Mass demonstration (this is text!!) The mass of an atom is…. Based on the demonstration, what can you conclude about the relationship between an atom’s mass and its subatomic particles? EVIDENCE I saw, I noticed…. INTERPRETATION I wondered, connected, inferred, concluded…

Atomic Mass = The number of protons + number of neutrons inside the nucleus

Are Units Important? So what units should we use when describing the mass of an proton, or neutron or electron?

How far is it from Charlotte to San Diego?

How far is it from Charlotte to San Diego? 3,835,000,000 mm OR 150,990,000 inches 2,385.3 miles

So what units should we use when describing the mass of an proton, or neutron or electron?

1 proton = 3.687502724 x 10-27 lb =.000000000000000000000000003687502724 lb 1 electron = 2.006647510 × 10−30 lb .000000000000000000000000000002006647510 lb

Atomic Mass Units…just for atoms! Protons = 1 amu Neutrons = 1 amu Electron mass insignificant …0. (their charge and configuration are VERY IMPORTANT, not their mass)

How can you use the information in the cells of the periodic table to find the number of neutrons in an atom? (hint: you can’t have part of a neutron)

In your notebook, on the paper under the note sheet on page 8 To find the number of neutrons: Round the Atomic Mass to a whole number Atomic Mass – Atomic Number=NEUTRONS P + N -- P = N Nucleus -- protons = neutrons

The periodic table has ALL the answers Atomic Number = Protons = Electrons Mass - Neutrons The periodic table has ALL the answers KING KONG CHEMISTRY Guided Practice: have the students use the EOG copy of the periodic table to find: an element given its atomic number, the number of protons in a specific element, the number of electrons in an element/atomic number, an element with X neutrons. Candy rewards??? Quick Quiz!!!

P 7 Using your notes and the periodic table at your seat, complete the following worksheet

P 7

What if the model doesn’t look like you expect

What if the model doesn’t look like you expect?

What if the model doesn’t look like you expect?

How are subatomic particles arranged? Bohr Model of the atom: All of the protons and the neutrons The 3rd ring can hold up to 8 e- 10P 11N The 1st ring can hold up to 2 e- The 2nd ring can hold up to 8 e- ***once a ring is full, it will not give up any electrons in the full ring

Valence electrons determine: how an atom bonds with other atoms (or if it will bond at all). atom’s reactivity (how easily it bonds with other elements.) Atoms with a complete set of valence electrons are stable. They don’t bond with other atoms: don’t gain/lose electrons, don’t share electrons. Word origin/stem late Middle English: from late Latin valentia ‘power, competence,’ from valere ‘be well or strong.’ P 10

(because the others are in full rings and aren’t going anywhere) Lewis Dot Structures The behavior of an atom is determined by the VALENCE ELECTRONS…so wouldn’t it be easier to just draw those?? (because the others are in full rings and aren’t going anywhere)   Write the symbol for the element Calculate the number of valence electrons (Use dots to represent the electrons.) Place electron “dots” around the symbol, starting on the left and moving clockwise. Begin by placing only one electron dot per side of the element symbol. More than 4 valence electrons? Add the second dot to each side (clockwise) Max of two electron dots per side

Hydrogen   Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminum Silicon Phosphorus Sulfur Chlorine Argon

Draw Bohr models (atomic models) for P 9 As a class: B (Boron, element 5) Na (Sodium, element 1) On your own: O (Oxygen, element 8) Li (Lithium, element 3)

Matter MATTER IS NEUTRAL AS LONG AS AN ATOM HAS THE SAME NUMBER OF PROTONS (+) AND ELECTRONS (-) SO THE ATOM HAS A BALANCED CHARGE!

An atom can become stable by changing the # of Electrons = Ions Ions are atoms that have a charge Ions form when an atom: Gain an electron = negative charge (#p < #e), (+<-) Lose an electron = positive charge (#p > #e), (+>-)

Changing the # of Neutrons = Isotopes Isotopes are atoms of the same element that have a different number of neutrons. Adding or losing a neutron is like gaining or losing weight…same element, different mass!

Changing the # of Protons = Different Element Changing the number of protons results in a different element. The number of protons determines what element it is! (ID number!) Atoms that change proton number are radioactive