wednesday , November 16 th

1. Quick Write! Quiz! wednesday, November 16th • SWBAT: • describe the following and provide examples: • Chemical formula • Chemical equation • describe the parts of an atom and draw an image • label the subatomic particles • compare and contrast between compounds and elements • Homework: • read workbook pgs 15-23 • complete all pages due • Friday! • find 10 chemical elements • that can be found in your house • by Friday • Test Tuesday 11/22

2. An atom • Basic unit of matter, “unable to be cut” An Element • Pure substance entirely of one atom

3. What are the Subatomic Particles? • Proton • Neutron • Electron

4. Cloud of negative charge (2 electrons) Electrons Nucleus (a) (b) The Atom

5. Who is Neils Bohr? He proposed a theory: • an atom is composed of a dense nucleus with electrons in its surrounding orbit • electrons must have a certain amount of energy to orbit the nucleus. • Electrons have a more fixed manner around the nucleus.

6. Modern Atom Model • Electron cloud model • Protons • Have a positive charge • have a mass of 1.67 x 10-24 g • Atomic number: • number of protons • Electrons: • Have a negative charge • If the atom has no charge there are the same number of electrons to protons • Mass number: • sum of the protons and neutrons together

7. Quick Write! Take out your sheet from yesterday. THursday, November 17th • SWBAT: • describe the following and provide examples: • Chemical formula • Chemical equation • describe the parts of an atom and draw an image • label the subatomic particles • compare and contrast between compounds and elements • Calculate the number of neutrons, protons and electrons • Homework: • read textbook pgs. 99 -104 • see website for details • read workbook pgs 15-23 • complete all pages due • Friday! • find 10 chemical elements • that can be found in your house • by Friday • Test Tuesday 11/22

8. Quick Write! Take out your sheet from yesterday. Answer the Quick Write Questions Friday, November 18th • SWBAT: • describe the following and provide examples: • Chemical formula • Chemical equation • describe the parts of an atom and draw an image • label the subatomic particles • compare and contrast between compounds and molecules • Calculate the number of atoms found in each chemical formula • Homework: • Test Tuesday 11/22 • Read pgs. 120- 126 practice note taking as you did last night

9. 1. List the subatomic particles. Proton Neutron Electron 2. Where are each of the particles found and what is their charge? Proton : + charge , found in nucleus Neutron: no charge, found in nucleus Electron: - charge, found outside of the nucleus Quick Write

10. 3. Identify one difference between a molecule and a compound. • Molecules are made of atoms, and compounds are made up of molecules, Label the molecule and the compound: ______________C2H4O2 ______________H2O

11. 4. What does a chemical formula tell you? A chemical formula tells you the elements and number of atoms that are needed to make the molecule or compound. 5. What does a chemical equation tell you? A chemical equation tells you the types of molecules and or compounds that are needed to complete a chemical reaction to form products.

12. 6. What is a subscript? They are found to the lower right of each element’s symbol. Provides you the number of atoms of the element in the compound or molecule. 7. What does the coefficient tell you? Tells you the number of molecules and atoms found in each chemical equation

13. Now let’s have some practice!

14. Quick Write! Place your homework on your desk. Complete last week’s worksheet Monday, November 21st • SWBAT: • identify the Atomic Mass and Atomic Number. • compare a solution to a compound. • compare a heterogeneous mixture to a homogeneous mixture. • Homework: • Study for Test see website for details.

15. Atomic Structure15 7N Mass Number = protons + neutrons • How can you identify it? It is the larger number. • It is the mass of the nucleus. • Why? Because it contains the protons + neutrons. Atomic number = number of protons • Smaller number • When an atom has no charge, the protons and electronsare equal in number! • Used to identify the element

16. protons electrons protons neutrons The Atom Atomic Number Symbol Name Mass Number Atomic number equals the number of ____________ or ________________. Mass Number equals the number of ______________ + _______________.

17. II. Periodic Table

19. Answer the following: 1. What is the difference between a heterogeneous and homogeneous mixture? • The heterogeneous mixture will separate upon standing, you can still see the individual particles and it is not uniform throughout. • A homogeneous mixture is uniform throughout, will not separate upon standing and you cannot see individual particles. 2. What is the difference between a compound and a solution? • A compound must be separated by chemical means and a solution can be separated by physical means. closure

20. Number of neutrons = mass # - atomic # Question: If the mass number is 15, there is no charge on the atom and the atomic number is 7. How many electrons and neutrons do you have? Solving for the number of neutrons

21. Assignment: Finish the rest of the worksheet and turn it in to your teacher.

22. Name__________________________ Date ______________ Atom Activity

23. Describe the subparts of the atom: Draw and label an atom What is an atom?

24. Compare and Contrast between a compound and molecule

25. Chemical formulas Chemical equations Explain and provide 3 examples for each

27. Each electron in an atom has its own distinct amount of energy. When electrons are in their lowest energy state, it is called the ground state The ground state for Na is 2-8-1

28. elements: Periodic Table are arranged in increasing atomic number. • Placement or location of elements on the Periodic Table indicates the physical and chemical properties of that element. • Number of protons in an atom (atomic number) identifies the element • Atomic mass: found on the Periodic Table of the Elements

29. Classifying Elements • Metals • Nonmetals • metalloids or semimetals (B, Si, Ge, As, Sb, Te), • noble gases Nonmetals on the right Metals on the left Metalloids semimetals

30. Group numbers and family names • Group 1 Alkali Metals • Very reactive metals, always found as compounds in nature • 1 valence electron - lose 1 electron to form +1 ions • Group 2 Alkaline Earth Metals • Reactive metals, always found as compounds in nature • 2 valence electrons - lose 2 electron to form +2 ions • Group 17 Halogens • Reactive nonmetals • 7 valence electrons - gain 1 electron to form –1 ions • Groups 18 Noble Gases • Not reactive – do not form ions • Filled, stable valence shell (8 electrons except He which has 2)

31. Classification of the Elements • Groups 3 - 11 Transition elements: an element in a transition, hard solids with high melting point, half filled orbitals, far less reactive than Group 1 & 2 • Metalloids/Semimetals: on the zigzag separates metals from nonmetals B, Si, Ge, As, Sb, Te, At • Nonmetals: gases, liquids or crystalline solids C, N, O, F, P, Br, gain electrons to become – ion, poor conductors of heat and electricity • Other metals: metals good conductors of heat and electricity, luster and shine, malleable (can change shape) Zn, Hg, Sn, Bi, Po

32. Silvery gray color except copper and gold Solid at room temperature except mercury Good conductors of heat and electricity Malleable – can be hammered into shapes (thin sheets) Ductile – can be pulled into wires Many different colors Sulfur – yellow Chlorine – green Bromine – orange Iodine - purple Many different states (phases) H, N, O – gas Br – liquid S, C, I – solid Poor conductors of heat and electricity (except carbon) Brittle – breaks when hit Comparing the physical properties of metals and nonmetals Metals Nonmetals

33. Find the name of each symbol • Group 1 Alkali metals: Li, Na, K, Rb, Cs, Fr • Group 2 Alkaline earth metals: Be, Mg, Ca, Sr, Ba, Ra • Transition elements: groups 3 - 11 • Other metals: Zn, Hg, Sn, Bi, Po • Semimetals: B, Si, Ge, As, Sb, Te, At • Nonmetals: C, N, O, F, P, Br • Group 18 Noble gases: He, Ne, Ar, Kr, Xe, Rn

34. Liquids Mercury (Hg) - the only liquid metal at room temperature Bromine (Br) - the only liquid nonmetal at room temperature Gases Hydrogen (H) Oxygen (O) Nitrogen (N) Fluorine (F) Chlorine (Cl) All of group 18 (noble gases) Helium (He), Neon (Ne) Argon (Ar), Krypton (Kr), Xenon (Xe), Radon (Rn) All elements are solid at room temperature except for the following: