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Molecules and Compounds
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Compound
• Formed from 2 or more elements in a specific proportion
• When combined, new properties are created
• They contain 2 or more different elements
• Examples: H20, NaCl, CO2
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Molecule
• A molecule is the smallest unit of a compound
• They are made up of 1 or more elements
• The elements can either be the same or different
• Examples: O2, O3, H2O, CO2
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So…
• All compounds are molecules, BUT not all molecules are compounds.
• Why?
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Chemical Formulas
• Scientists use chemical formulas to write the name of compounds
• It is a combination of numbers ( subscripts and coefficients) and symbols
• The subscript (small number) indicate how many of each atom are present
• The coefficient (larger number) indicate how many of each molecule is present
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Example
• C3H8O is the chemical formula for rubbing alcohol.
• There are ___carbon, ___ hydrogen, and 1 oxygen atom that make up one molecule of alcohol.
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Example
• NaCl is the chemical formula for salt
• There is ____ Na atom and ____ Cl atom
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Example
• NH3 is the chemical formula for ammonia
• There is ____ N atom and _____ H atoms
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Example
• 4CO2
• How many C and how many O?
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Example Cont.
• Think about it like a math problem- 4 X (CO2)
• So there are ____ C atoms and ____ O atoms
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Example
• 6H2O
• There are ___ H atoms and ____ O atoms
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Example
• 3C6H12O6
• There are ____ C atoms, ____ H atoms, and ____ O atoms
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Chemical Equations
• Chemists way of showing a chemical reaction with elements
• Reactant yields the product
• The arrow means “yields”
• Must be balanced (must have the same number of elements on both sides)
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Chemical Equations
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Chemical Equations
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Chemical Equations
• Important thing to remember is the law of conservation of matter
• If there are 4 carbons on one side, there must be 4 on the other side because matter can not be created or destroyed