Today’s Schedule Agenda: 1.Obj 3 and 5 Station Recap 2.Whiteboard Review 3.TAKS Review Booklet Essential Questions What do I need to know for the TAKS test? Homework: Complete TAKS booklet April 24, 2011 Announcement: TAKS test is Thursday! Come to tutoring for help finishing TAKS booklet.

Elements, Compounds, and Chemical Equations Counting Atoms and Balancing Equations

1.Counting Subatomic Particles: Use the periodic table The atomic number is the same as the number of protons. The number of protons is the same as the number of electrons. The mass number is the protons added to the neutrons. Atomic Number = Protons = Electrons (APE) Mass Number = Protons + Neutrons Neutrons = Mass Number - Protons

1.Counting Subatomic Particles: Find the number of protons, neutrons, and electrons in: Lithium Atomic Number = Protons = Electrons (APE) Mass Number = Protons + Neutrons Neutrons = Mass Number - Protons

1.Counting Subatomic Particles: Find the number of protons, neutrons, and electrons in: Lithium Atomic Number = 3Mass Number = 7 Protons = 3 Neutrons = 4 Electrons = 3

1.Counting Subatomic Particles: Find the number of protons, neutrons, and electrons in: Gold Atomic Number = Protons = Electrons (APE) Mass Number = Protons + Neutrons Neutrons = Mass Number - Protons

1.Counting Subatomic Particles: Find the number of protons, neutrons, and electrons in: Argon

1.Counting Subatomic Particles: Find the number of protons, neutrons, and electrons in: Lead

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients Subscripts describe the number of that type of atom. They appear after the element symbol, are small, and written hanging below the symbol. Coefficients describe the number of molecules present. Coefficients apply to all elements in the molecule. They are written before the formula for the molecule and are large.

4H 2 O Coefficient: There are 4 molecules of water. Subscript: There are 2 atoms of Hydrogen in each water molecule.

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients Subscripts describe the number of that type of atom. They appear after the element symbol, are small, and written hanging below the symbol. Coefficients describe the number of molecules present. Coefficients apply to all elements in the molecule. They are written before the formula for the molecule and are large. H 2 O = 2 hydrogen and 1 Oxygen

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients Subscripts describe the number of that type of atom. They appear after the element symbol, are small, and written hanging below the symbol. Coefficients describe the number of molecules present. Coefficients apply to all elements in the molecule. They are written before the formula for the molecule and are large. 3H 2 O = 6 Hydrogen and 3 Oxygen

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients Count and Draw the atoms in the molecule. NH 4

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients Count and Draw the atoms in the molecule. NH 4 N = Nitrogen = 1 H = Hydrogen = 4

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients Count and Draw the atoms in the molecule. 2NH 4

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients Count and Draw the atoms in the molecule. NH 4

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients Count the atoms present: C 6 H 12 O 6

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients C 6 H 12 O 6 Carbon – C – 6 Hydrogen – H – 12 Oxygen – O – 6

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients 3C 6 H 12 O 6

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients 3C 6 H 12 O 6 Carbon – C – 6 x 3 = 18 Hydrogen – H – 12 x 3 = 36 Oxygen – O – 6 x 3 = 18

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients 2NaC 2 H 3 O 2

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients 2NaC 2 H 3 O 2 Sodium - Na – 1 x 2 = 2 Carbon – C – 2 x 2 = 4 Hydrogen – H – 3 x 2 = 6 Oxygen – O – 2 x 2 = 4

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients KNO 3

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients 4KNO 3

3. Balancing Equations: Count the atoms in the reactants and the products. Count the total number of each type of atom on the reactant (ingredient) side. Count the total number of each type of atom in the product (what you make) side If the number of each type of atom matches, the equation is balanced. If the numbers do not match the equation is not balanced. Equations must be balanced to show that the same atoms that go into a reaction are the atoms that come out, THEY ARE JUST REARRANGED to make new substances.

3. Balancing Equations: Count the atoms in the reactants and the products. 2Cu + O 2  2CuO ReactantsElementProducts Copper Oxygen

3. Balancing Equations: Count the atoms in the reactants and the products. 2Cu + O 2  2CuO The Equation is Balanced!!! ReactantsElementProducts 2Copper2 2Oxygen2

3. Balancing Equations: Count the atoms in the reactants and the products. 2H 2 O  3H 2 + O 2 ReactantsElementProducts Hydrogen Oxygen

3. Balancing Equations: Count the atoms in the reactants and the products. 2H 2 O  3H 2 + O 2 ReactantsElementProducts 4Hydrogen6 2Oxygen2

3. Balancing Equations: Count the atoms in the reactants and the products. 3Fe + 4H 2 O  4H 2 + Fe 3 O 4 ReactantsElementProducts Iron Hydrogen Oxygen

3. Balancing Equations: Count the atoms in the reactants and the products. 3Fe + 4H 2 O  4H 2 + Fe 3 O 4 ReactantsElementProducts 3Iron3 8Hydrogen8 4Oxygen4

3. Balancing Equations: Count the atoms in the reactants and the products. 2Fe 2 O 3 + 3H 2  2Fe + 3H 2 O ReactantsElementProducts Iron Oxygen Hydrogen

3. Balancing Equations: Count the atoms in the reactants and the products. CaCO 3  CaO + CO 2 ReactantsElementProducts Calcium Carbon Oxygen

3. Balancing Equations: Count the atoms in the reactants and the products. CaCO 3  CaO + CO 2 ReactantsElementProducts 1Calcium1 1Carbon1 3Oxygen3

3. Balancing Equations: Count the atoms in the reactants and the products. 2NaCl  2Na + Cl 2 ReactantsElementProducts

3. Balancing Equations: Count the atoms in the reactants and the products. 2NaCl  2Na + Cl 2 ReactantsElementProducts 2Na2 2Cl2

3. Balancing Equations: Count the atoms in the reactants and the products. CH 4 + 2O 2  CO 2 + 2H 2 O

3. Balancing Equations: Count the atoms in the reactants and the products. CH 4 + 2O 2  CO 2 + 2H 2 O ReactantsElementProducts 1 C 1 4H 4 4O4

3. Balancing Equations: Count the atoms in the reactants and the products. C 5 H O 2  5CO 2 + 6H 2 O

3. Balancing Equations: Count the atoms in the reactants and the products. C 5 H O 2  5CO 2 + 6H 2 O ReactantsElementProducts 5C 5 12H 17 12O16

2. Counting Atoms in Chemical Formulas: Examine the subscripts and coefficients C 6 H 12 O 6