a. Located in the. b. Charge is. c. Found on periodic table by looking at the of an element. d. Has a mass of

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1 Unit 4 Atomic Structure, Periodic Table, Matter, and Chemical Equations Name: Period: I. Atomic Structure: A. Atomic Theory. a. All matter is made of b. Atoms are and cannot be divided into c. Atoms of one element are, but they are from atoms of other B. Subatomic Particles: Actually means atom. 1. Electrons: This is what makes elements. a. Located. b. Charge is. c. Electrons so they can. d. Have no e. Exist at different. The number of can be found by looking at the element f. The only electrons that can bond with other atoms are the. Called. 2. Protons: Protons make elements because their positive charge controls the attractions of an atom, thus controlling it s Carbon a. Located in the. b. Charge is. c. Found on periodic table by looking at the of an element. d. Has a mass of Example: Potassium has how many protons? Potassium (K) has how many electrons? Potassium has how many energy levels? Diagram here: K has how many outer electrons for bonding?

2 3. Neutrons: This is what adds to the of an atom. a. Located in the b. Charge is d. Total mass of an atom from the and the 4. Isotopes: All atoms of an element have same number of. But, in nature, some atoms of the same element have different numbers of, they are called different. This causes their masses to be different. Diagram of Neon-20 and Neon 22 b. When reading the periodic table, round to the nearest number to find the most for that element. Q: How many protons, neutrons, electrons are in the most common isotope of potassium? How many protons, neutrons, electrons are in the most common isotope of aluminum? Obj. 1: Fill in the grid below for each subatomic particle. Protons Location in atom Symbol Charge Mass Neutrons Electrons

3 Obj. 2: Directions: Complete the table for the following isotopes of each element: Element Symbo l Number of Protons Number of Electrons Number of Neutrons Atomic Number Mass Number Sodium 13 Valence Electrons X 4 5 F 19 II. Obj. 3: Bohr Models: Uses to show the energy levels. The number of rings should match the of that element. This model is. 1. mass of all the isotopes found in nature =. 2. The protons in the nucleus are found by looking at the. 3. The neutrons plus the protons must add up to. 4. The electrons fill the shells from until they match the number of. They fill in the following order a. You can check you outer electrons to make sure they match the b. This model can only be used for the first 20 atoms. After that it i.e. Calcium 44 i.e. lithium 7 Obj. 3: Draw Bohr Models for the following Isotopes. Include # of Electrons in correct rings, # of Protons in nucleus # of Neutrons in nucleus Sulfur 34 Boron 10 Helium 3

4 Sulfur 32 Boron 14 Helium 4 III. Obj. 4: Classifying matter A. Matter: Anything that has and. B. Pure Substances: Matter that has fixed and definite. Cannot be broken down by means. a. Element: a substance that cannot be by chemical means. i.e. b. Compound: a substance made of that are chemically combined. 1. Every compound is from the that it contains. i.e. Water: H 2 O Physical Properties: Hydrogen: H 2 Physical Properties: Oxygen: O 2 Physical Properties: Chemical Properties: Chemical Properties: Chemical Properties: 2. Chemical formula: Shows the in a compound. It also shows are in the compound. try 4 Ca(ClO3)2 c. Mixtures: Matter that has compositions that are not or. Mixtures can be separated by into the that are mixed w/in them. 1. Homogeneous Mixture: (homo = )The composition is the throughout.

5 a. Homogeneous Mixture Examples. Something must be in order to be truly. b. If something is dissolved in water, we call it and label it.,, & are always aqueous. 1) Solid Solid: 2) Liquid Liquid: 3) Gas Gas: 4) Solid (dissolves) Liquid: 5) Gas (dissolves) Liquid: 2. Heterogeneous Mixture: (Hetero = ) The composition is. a. Anytime more than one exists in a mixture, it is considered heterogeneous b/c states of matter are of composition. Question: Which three types of matter will always look homogeneous? Why.

6 Practice Problems Hetero or Homo Mixture 1. Dish Soap: 2. A Rock: 3. Stainless Steel: 4. Saltwater: 5. Pen ink: 6. An Egg: 7. Dust Free Air: 8. Rusty Nail: Why? IV. Obj. 5: Reading trends in the Periodic Table (Ch 3.2) A. Go down, pass across. 1. Tall groups tell you the number of electrons in that group. 2. Some common names for special groups a. Group 1A: b. Goup 2A: c. Group 7A: d. Group 8A: 3. Size (pgs ): Atoms get as you go down a Group, but as you go to the right b/c more in outer energy level. 4. The identifies to the left, to the right, and touch the ladder a. Short groups are metals, charges may change (are in transition) b. To remember where metals and non-metals are, just. 5. The will tell you the number of.

7 V. Obj. 6: Properties and Changes in Matter A. Physical Change: Affects one or more properties of a substance w/o. Chemical properties are. i.e. 1. More on Dissolving. Two different substances visually become 2. Phase changes= B. Chemical Changes: Occur when one or more substances are changed into that have. i.e. Chemical or Physical Property? Chemical or Physical Change? 1. Tarnishes in Rain: 1. Lighting a firework: 2. Bends easily: 2. Boiling Pasta: 3. Decomposes: 3. Chewing gum: 4. Reusable/Recyclable: 4. Running your car: 5. Shiny 5. Rolling your bike: 6. Not Flammable: 6. Melting a crayon: 7. Perishable Food: 7. Rusting a nail: 8. Freezable Food: 8. Opening a can of pop: Chemical equation: Describes the original beginning substances (called ) using chemical formulas. Then an arrow points to the newly created substances (called ). (s) = (l) = (g) = (aq) = + = = = H 2 (subscripts) = 2 H 2 = (Coefficients) = Example: VI. Obj. 7: Balancing Equations: The law of conservation of mass states that matter cannot be or. So, the number of atoms reacting must equal the number of atoms produces. However, a chemical change rearranges these atoms into new.

8 To balance equations, follow these steps. 1. Count atoms on each side of. They should be. If not, you need to them. 2. Balance both sides by using. Remember, they multiply through everything inside of that compound. NEVER change. 3. Double check work. Try These KClO 3 KCl + O 2 AlBr 3 + K 2 SO 4 KBr + Al 2 (SO 4 ) 3 C 3 H 8 + O 2 CO 2 + H 2 O Examples from class demos and life examples. Balance as well