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formula unit

Covalent Bonding: Learning to Cooperate. formula unit. describe a covalent bond state the differences covalent and ionic bonds explain the term molecule describe a diatomic molecule. Key Words. covalent compound covalent bond diatomic molecule . Covalent Compound:

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formula unit

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  1. Covalent Bonding: Learning to Cooperate formula unit

  2. describe a covalent bond • state the differences covalent and ionic bonds • explain the term molecule • describe a diatomic molecule Key Words covalent compound covalent bond diatomic molecule

  3. Covalent Compound: Contains two or more NON-METAL atoms. Formed by SHARING valence electrons to fill outer shell – octet rule. • A molecule is the smallest unit of a covalent compound. Non-metal + Non-metal = covalent bonding

  4. Fluorine atom: 9 p+ 9 e- F Fluorine atom: 9 p+ 9 e- F F2 covalent compound

  5. Water H2O 8p 1p H O H 1p A molecule has different properties than the atoms from which it is formed

  6. Methane CH4 H H C H H

  7. Ammonia NH3 H H N H

  8. Atoms can share one pair of electrons, or two or three pairs. S O In the end – electrons must be arranged so that each atom has 8 electrons around it.

  9. Diatomic Elements Forming a Covalent Bond with Yourself

  10. Diatomic elements are unstableas single atoms. They form covalent bonds with a same atom to make a stable molecule. H H2 molecule H No new substance is formed - the covalent bond forms a molecule of only one type of atom.

  11. Diatomic Elements: ave o ight r ever riends I H N Br O Cl F 2 2 2 2 2 2 2

  12. F2 molecule (single bond) F F O O O2 molecule (double bond)

  13. Covalent Bonding: Naming and Writing

  14. Same – covalent compounds are also named using the “ide” ending for last non-metal. Different – covalent naming uses prefixes before the name of each element. Prefixes show the number of atoms of that element in the formula for the molecule. Diatomic Elements 2

  15. Step 1: firstnon-metal is named with a prefix to show the number of atoms. We do not use “mono” for the first non-metal. Step 2: secondnon-metal is named with a prefix AND with the “ide” ending. N O 2 4 nitrogen oxide di tetra dinitrogen tetroxide

  16. SO 3 mono sulfur oxide tri sulfur trioxide C Br 3 6 carbon bromide tri hexa tricarbon hexabromide

  17. Writing formulas Step 1: Write the symbol of each element. Step 2: Use a subscriptto show the number of each type of atom given by the prefix. Do not reduce covalent formulas. di phosphorus oxide penta PO 2 5

  18. nitrogen iodide tri NI 3 carbon oxide di CO 2 di silicon sulfide tetra SiS 2 4

  19. IMPORTANT POINTS: **Always identify a compound as ionic (m + nm) or covalent (nm + nm) before doing anything. Prefixes are used in naming covalent compounds ONLY. Criss-crossingis only used in ionic compounds. DO NOT reduce covalent compounds.

  20. metal non-metal non-metal non-metal BeCl SCl 2 2 ionic covalent - +2 Be S Cl Cl - Cl Cl beryllium chloride mono sulfur chloride di

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