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WHY DO ATOMS BOND ?

WHY DO ATOMS BOND ?. GROUPS. The Periodic Table. 1. 8. H. He. 2. 3. 4. 5. 6. 7. Li. Be. B. C. N. O. F. Ne. Na. Mg. Al. Si. P. S. Cl. Ar. K. Ca. Learning Objective To understand covalent bonding. Electron arrangement in outer shells. 1. 8. H. He. 2. 3. 4.

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WHY DO ATOMS BOND ?

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  1. WHY DO ATOMS BOND?

  2. GROUPS The Periodic Table 1 8 H He 2 3 4 5 6 7 Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca

  3. Learning ObjectiveTo understand covalent bonding Electron arrangement in outer shells 1 8 H He 2 3 4 5 6 7 Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca

  4. Why do atoms form bonds? Octet Rule Atoms need to be stable Stable = full outer energy level Full = 8 electrons (except level 1) Ex. Neon

  5. BONDING = STABILITY 8 IS GREAT!

  6. A covalent bond exists when two electrons are shared by two non-metallic atoms.*

  7. Ionic Bonding • Is when atoms gainor loseup to 3 electrons to get a full valence • shell • When they do this they become ions • An ion is an electrically charged atom i.e. there are more or less • electrons than protonse.g. Metals in Group 1, 2 and 3 lose • electrons and become positively charged: Mg2+ Na+ Al3+ • Non-metals in Group 5, 6 and 7 gain electrons to become negatively • charged: F- P3- S2- • Ions in a compound are held together by the attraction of (+) and (–) • charges • The compound has no overall charge because there is the same • amount of (+) and (–) charges

  8. ION (charged particle) Na

  9. 11 ION (charged particle) Na Na+ 23

  10. Ion Atom that has lost or gained electrons Atom with a charge Ca+ion positive ion metals ex. Ca+2 *superscript shows charge Anion negative ion nonmetal ex. Cl-1

  11. You must follow the rules! Naming Ions Anions take element name and change the ending to –ide ex. Fluorine  fluoride Bromine  bromide Cations use the element name ex. Calcium  calcium

  12. Monoatomic Mono = one Ion Single atom with + or – charge ex. Ca+2 Polyatomic ion ion made of 2 or more types of atoms that act as a single ion ex. Nitrate (NO3)-1

  13. CROSSOVER RULE TO FIND FORMULAE • Write the name and symbol of the ions • Write the valencies • Crossover the valencies • Write the formula

  14. Potassium and sulfur

  15. PART C. Research on the 5 new compounds by finding its: • description • use/importance • Work in pairs/groups of 3. • Use the given “ion” pieces to find the corresponding “ion partners to form an ionic compound. ACTIVITY: IONIC BONDING PART A. Form the different ionic compounds listed in the handout. PART B. Make a new ionic compound using the “ion pieces”. Form at least 5 new compounds, and write the chemical name and formula for each compound. QUESTION: What are the properties of ionic compounds?

  16. ACTIVITY: IONIC BONDING PART A. Form the different ionic compounds listed above. PART B. Make a new ionic compound using the “ion pieces”. Form at least 5 new compounds, and write the chemical name and formula for each compound. PART C.Research on the 5 new compounds by finding its: description and use/importance

  17. Use the model pieces to construct compounds out of the elements listed below. Write the name and formula of the element in your note book. • magnesium & bromine • lead & nitrate • lithium & sulfate • copper & hydroxide • potassium & oxygen • ammonium & sulfate • sodium & phosphate • silver & chlorine • iron (III) & oxygen • zinc & carbonate 11. lead and iodine 12. aluminum & hydroxide 13. calcium & phosphate 14. sodium & hydrogen carbonate 15. iron (II) & sulfate 16. potassium & sulfur 17. lithium & bromine 18. silver & nitrate 19. copper & carbonate 20. ammonium & chloride

  18. IONIC COMPOUNDS

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