1. Midterm Review Topic 2 Formulas and Equations

2. Vocabulary Chemical Change Coefficient Decomposition Diatomic molecule Double replacement Empirical formula Endothermic Exothermic Formula Molecular formula Molecule Physical change Polyatomic ion Product Qualitative Quantitative Reactant Single replacement Subscript Symbol Synthesis

3. Chemical Symbols and Formulas Chemists have developed a universal language by which they can communicate chemical information and have the information understood by scientists around the world

4. Diatomic Molecule BrINClHOF

5. Chemical Formulas Compounds are composed of combinations of elements chemically combined in definite proportions – Formulas us chemical symbols and numbers to show both qualitative and quantitative information about a substance – The chemical formula CO tells the reader that the compound consists of Carbon and Oxygen. – The chemical formula CO 2 tell the reader that the compound consists of 1 carbon and 2 oxygen atoms

6. Types of Formulas Empirical Formula – Represents the simplest ratio in which atoms combine to form a compound Molecular Formula – Covalently bonded substances form discrete units called molecules. In some cases, such as H 2 O, the chemical formula is both empirical and molecular In other cases the molecular formula may be a multiple of the empirical formula, for example glucose, C 6 H 12 O 6

7. Atoms, Compounds, and Ions Ionic Charge – The charge of an ion is indicated by the superscript following the symbol of the ion. – Al +3 Polyatomic Ions – A polyatomic Ion is a group of atoms covalently bonded together, possessing a charge Reference table E

8. Atoms, Compounds, and Ions Forming a Compound – Compounds can be formed in several different ways One way is the attraction of oppositely charged ions Monatomic or polyatomic ions attract each other in a ration that produces a neutral compound

9. Atoms, Compounds, and Ions Coefficients – The coefficient tells how many units of the formula are present

10. Atoms, Compounds, and Ions Hydrates – When water from come ionic solution evaporates, the solute forms a crystal lattice that binds water with in the structure – CuSO 4 5H 2 O

11. Writing Formulas and Naming Compounds Equalizing charges – Compounds achieve neutrality by having an equal number of positive and negative charges. – When sodium ion (Na +1 ) and a chlorine ion (Cl -1 ) combine, they will do so in a 1:1 ratio – If you do not have a 1:1 ratio, they you must cross down the charges

12. Writing Formulas and Naming Compounds Naming Compounds – Compounds are named according to the types of elements that form them. Ionic compounds – Binary or polyatomic Covalent compounds – Binary or stock system

15. Chemical Reactions and Equations Physical Change – A change in state such as ice melting Chemical change – The substances produced are quite different form the starting material

16. Chemical Reactions and Equations Chemical Equations

17. Chemical Reactions and Equations Endothermic reaction Exothermic reaction

18. Chemical Reactions and Equations Balancing chemical equations – Law of Conservation of Mass

20. Types of Chemical Reactions Synthesis – A+B  AB

21. Types of Chemical Reactions Decomposition – AB  A + B

22. Types of Chemical Reactions Single Replacement – AB + C  AC + B

23. Types of Chemical Reactions Double Replacement – AB + CD  AD + CB