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Published byLilli Kohler Modified over 6 years ago
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Part B. Definitions Empirical Formula = a formula giving the ratios (proportions) of the elements present in a compound but not the actual numbers or arrangement of atoms… aka the reduced/simplest form Examples: CH2O --- this is the empirical form for glucose, C6H12O6 C3H4O --- the subscripts cannot be simplified so must be in their reduced form, making this empirical
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Part B. Definitions Molecular Formula = a formula giving the number of atoms of each of the elements present in one molecule of a specific compound (not necessarily the reduced form, but it could be) Examples: C6H12O6 (sugar) --- Dividing all subscripts by 6 would give the empirical form, CH2O N2O4 --- dividing all subscripts by 2 would give the empirical form NO2 H2O --- this is the molecular and empirical form because this is actually what the H2O molecule looks like
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Part B. Definitions Mole Ratio = ratio of atoms within a compound or the ratio of compounds in a reaction Examples: H2O has a 2:1 ratio of hydrogen to oxygen. C6H12O6 (sugar) has a 6:12:6 ratio of carbon to hydrogen to oxygen.
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PART C. Identify the following as empirical or molecular
1. Formaldehyde CH2O 2. dinitrogen tetroxide N2O4 3. carbon monoxide CO 4. acetic acid C2H4O2 5. Hydrogen peroxide H2O2
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PART C. Identify the following as empirical or molecular
6. Acetylene C2H2 7. Water H2O 8. Carbon dioxide CO2 9. Butene C4H8 10. glucose C6H12O6
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