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MOLECULAR COMPOUNDS

MOLECULAR COMPOUNDS. What are they and how to name them?. Molecular Compounds. Definition: A compound formed when atoms of two or more different elements share electrons Usually formed between 2 or more non-metals and are also called covalent compounds. Ionic vs. Molecular?.

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MOLECULAR COMPOUNDS

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  1. MOLECULAR COMPOUNDS What are they and how to name them?

  2. Molecular Compounds Definition: A compound formed when atoms of two or more different elements share electrons • Usually formed between 2 or more non-metals and are also called covalent compounds

  3. Ionic vs. Molecular? Ionic Compounds Molecular Compounds How atoms bond? Transfer of electron opposite charges attract Atoms share electrons to complete valence shells What bonds with what? Metal to non-metal Non-metal to non-metal What do they form? Lattice structure (solids) Smaller compounds with 2-3 atoms linked

  4. Ionic Covalent

  5. Naming Molecular Compounds Naming molecular compounds is different from ionic and polyatomic compounds. In molecular compounds the name uses a prefix to indicate the number of each atom present. Example: Carbon Dioxide tells us it is made of carbon and oxygen in a ratio of 1 carbon atoms to 2 oxygen atoms.

  6. Prefixes Prefix Number of atoms Example mono 1 (CO) carbon monoxide di 2 (CO2) carbon dioxide tri 3 (SO3) sulfur trioxide tetra 4 (CF4) carbon tetrafluoride penta 5 (PBr5) phosphorus pentabromide hexa 6 (SF6) sulfur hexafluoride hepta 7 octa 8 nona 9 deca 10 (P4O10) tetraphosphorous decaoxide

  7. Writing Names • Count the # of atoms of the first element. • Write the prefix for this number followed by the name of the first element. If there is only one of the first element we leave out the prefix. • Count the # of atoms of the second element. • Write the prefix for this number followed by the name of the element using the suffix –ide.

  8. Examples N2O4 Nitrogen atoms = 2  dinitrogen Oxygen atoms = 4  tetraoxide Full name = dinitrogen tetraoxide C2F6 Carbon atoms = 2  dicarbon Fluoride atoms = 6  hexafluoride Full name = dicarbon hexafluoride

  9. Writing Formulas • Write the symbol for the elements. • Write the subscript for the number of atoms represented by the prefix. • Notice—the ratio in the formula is not reduced to its simplest form like ionic compounds.

  10. Examples sulfur trioxide SO3 diphosphorus pentasulfide P2S5

  11. Diatomic Elements Some elements are diatomic. This means they exist naturally as two of the same element bonded together Examples: Hydrogen gas H2 Bromine liquid Br2 Oxygen gas O2 Iodine solid I2 Nitrogen gas N2Fluorine gas F2 Chlorine gas Cl2

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