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Ionic and Molecular Compounds

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This guide introduces ionic and molecular compounds, essential concepts in chemistry. A compound is defined as a pure substance formed from the combination of elements, represented by a chemical formula. Ionic compounds consist of a metal paired with a non-metal, where electrons are transferred, exemplified by NaCl. Conversely, molecular compounds are formed from non-metals, like H2O and CO2. This resource covers naming conventions for both types, including steps and examples for clarity. Perfect for students seeking to understand chemical bonding principles.

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Ionic and Molecular Compounds

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  1. Ionic and Molecular Compounds Science 9 – Matter and Chemical Change, Topic 6

  2. What is a compound? • A pure substance • A combination of elements • A chemical formula tells you the types and numbers of atoms present. • Example: H2O has two hydrogen (H) and one oxygen (O) • 2 types: • Ionic compounds • Molecular compounds

  3. Ionic Compounds • A metal paired with a non-metal • Ex: NaCl • Electrons are transferred from the metal to the non-metal. • Na  e-  Cl • ____________ becomes more positive and ____________ becomes more negative.

  4. Ionic Compounds • Metals: • Alkali metals like to transfer 1 electron • Alkaline earth metals like to transfer 2 electrons • Non-metals • Halogens like to receive 1 electron • OH likes to receive 1 electron • SO4 likes to receive 2 electrons • NO3 likes to receive 1 electron

  5. Ionic Compounds • Example: Copper likes to give away 2 electrons. How many chlorine atoms will be able to bond to copper? (remember, each chlorine atom receives 1 electron) • Answer: • 2 chlorine • CuCl2

  6. Ionic Compounds • Practice: • Li and F • Ca and Br • K and I • Ba and Cl • Cs and OH • Be and SO4 • Mg and OH

  7. Do Now! April 3, 2011 • Combine the following elements into the correct chemical formula: • Calcium fluoride • Na and OH • Al (3+) and Cl

  8. Molecular Compounds • A combination of non-metals • Ex: H2O, CO2, CCl4 • Some elements bind to themselves to form diatomic molecules • The diatomic molecules are: • H2, O2, N2

  9. Naming Ionic compoundsex: ZnF • Step 1 • Write down the names of both elements • zinc fluorine • Step 2 • Change the ending of the 2nd element to –ide. • zinc fluoride • Special rules • oxygen  oxide sulfur  sulfide • nitrogen  nitride carbon  carbide • boron  boride

  10. Naming Molecular compoundsCF4 • Follow the steps for naming ionic compounds • carbon fluoride • And then… • Step 3 • Add a prefix to elements to indicate their number • 1= mono* 2=di 3=tri 4=tetra • *mono is only used for the 2nd element • carbon tetrafuloride

  11. Naming Molecular Compounds • Practice • CO • CO2 • SiO2 • SO2 • BCl3

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