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IONIC COMPOUNDS

Learn how sodium and fluorine atoms form stable compounds through electron rearrangement to create ionic bonds. Discover the concept of valence, valence electrons, and the formation of strong crystal lattices in ionic compounds.

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IONIC COMPOUNDS

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  1. IONIC COMPOUNDS Joining Atoms Together

  2. Questions • How can a soldium atom get rid of its “extra” electron to become chemically stable • Where can a fluorine atom get the extra electron it needs to make a stable octet? • What is a stable octet?

  3. Valence • The outer energy shell of an atom is called its VALENCE SHELL • The electrons in the valence shell are called the VALENCE ELECTRONS

  4. NaFl • With Na and Fl, the concept of electron rearrangement explains the formation of the compound sodium fluoride. • Both atoms lose their original properties. • Fluorine now has a slightly negative charge • Sodium now has slightly positive charge • Where do you think you might find NaFl

  5. What bonds with what? • Look at the table… knowing how ionic bonds form, how might the different groups bond with each other? • Ionic bonds form between metals and non-metals

  6. How many…? • Alkali metals + Halogens • Alkaline Earth Metals + Halogens • Alkali Metals + Oxygen group

  7. Ions • Atoms are neutral (charge) because they have the same number of electrons and protons. • When an atom gains or loses an electron it becomes an ion ( + or -) • Na becomes Na+ • Cl becomes Cl- • O becomes O2-

  8. sodium chloride • NaCl, Na completely transfers an electron to Clhas low electronegativity; Cl has high electronegativity. The Cl will completely remove from Na its only valence electron. • The result is that both atoms will have full octets. • The positive and negative ions that form attract one another to form the compound.

  9. What forms Ionic bonds • What elements can you predict will form ionic bonds? • Ionic bonds are formed between metals and non metals.

  10. Strong Compounds • Ions in an ionic compound form regluar, repeating patterns called a crystal lattice • The bond is very strong and the same in all directions • Solid ionic compounds are hard and don’t conduct electricity well. • In water the ions separate

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