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Ionic compounds form by adding or removing electrons from one atom to the other.

Comparing covalent and ionic compounds . Ionic compounds form by adding or removing electrons from one atom to the other. Covalent compound form by sharing electrons between the two atoms. Ionic compound form between metals and non-metals. Covalent compound form between two non-metals.

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Ionic compounds form by adding or removing electrons from one atom to the other.

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  1. Comparing covalent and ionic compounds • Ionic compounds form by adding or removing electrons from one atom to the other. • Covalent compound form by sharing electrons between the two atoms. • Ionic compound form between metals and non-metals. • Covalent compound form between two non-metals.

  2. Ionic compound Covalent compound

  3. Naming ionic compound • Cations are named first, and anions are named last. • Cations names the element. • When an element forms two or more ions you include roman numerals to indicate the charge. • The anions always end in –ide.

  4. Naming Covalent Compounds • Unlike the names for ionic compounds, the names for covalent compounds must often distinguish between two different molecules made of the same elements. • These two compounds are given different names based on the number of each type of atom in the compound. • The first element named is usually the first one written in the formula. • The second element named has the ending –ide.

  5. Covalent Compounds

  6. Sulfur Trioxide • SO3 • Lewis Structure • (Trigonal Planar)

  7. Sulfur has 6 valence electrons • Oxygen has 6 valence electrons also. • Oxygen in this case is “trioxide” so oxygen is then used three times. • Each oxygen shares a double bond with sulfur. And each oxygen also has four unshared electrons. • Sulfur trioxide is generally a colorless liquid. It can also exist as ice or fiber-like crystals or a gas. When exposed to air, it rapidly takes up water and gives off white fumes. • Its also used to make explosives!!!

  8. Silicon Dioxide • SiO2

  9. Silicon has 6 valence electrons. • Oxygen has 6 valence electrons also. • Oxygen in this case is “dioxide” so oxygen is used two times. • Silicon dioxide has no set Lewis Structure • Also known as silica, quartz, and sand.

  10. Ionic Compounds

  11. Strontium Chloride SrCl2

  12. Charges and how it forms • Strontium becomes a cation by Losing 2 electrons. • And there are two chloride atoms That become anions by gaining 1 Electron.

  13. Fun facts • Strontium chloride is often used as a red colouring agent in pyrotechnics. • It is employed in small quantities in glass-making and metallurgy. • SrCl2 is useful in reducing tooth sensitivity by forming a barrier over microscopic tubules in the dentin containing nerve endings that have become exposed by gum recession.

  14. Sodium Oxide • Na2O

  15. Sodium has 1 valence electron. • Oxygen has 6 valence electrons. • Oxygen has to gain 2 valence electrons from two sodium atoms to become stable. • Also used to make Soda Glass Bottles!

  16. Work Sited • http://en.wikipedia.org/wiki/Silica • http://en.wikipedia.org/wiki/Sulfur_trioxide

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