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Review (Partner Talk)

Review (Partner Talk). Discuss the importance of sodium, calcium and potassium ions to your health. Differentiate between the following; a)atom vs. Ion b) cation vs. Anion 3) Draw the element with the following electron arrangement. 2:8:3

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Review (Partner Talk)

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  1. Review (Partner Talk) Discuss the importance of sodium, calcium and potassium ions to your health. Differentiate between the following; a)atom vs. Ion b) cation vs. Anion 3) Draw the element with the following electron arrangement. 2:8:3 4) Name the following ions. S2-, Na+, F-, Mg2+.

  2. Ionic Compounds • Look at the periodic table you filled in for the activity on page 191 and answer the following questions. • What would metal do to form cation? • Lose electrons. • What would non-metals do to form anions? • Gain electrons. • So metals have a weak hold on electrons and non-metals have a strong attraction for electrons.

  3. Formation of Ionic Compound The attraction holding the ions together is called an ionic bond Note: both ions have a stable outer shell as the nearest noble gas Chlorine takes electron to complete its shell Sodium loses its outmost electron to chlorine The opposite charges attract each other to form a compound.

  4. Formation of Ionic Compound • Develop the Bohr-Rutherford diagram for the formation of magnesium oxide (MgO).

  5. Ionic Crystal of Sodium Chloride • Alternating sodium and chloride ions come together in a 1:1 in a three dimensional structure to form an ionic crystal ‘NaCl’. The crystals appear as cubes Hence the ratio 1:1 and the formula for sodium chloride is NaCl But the no. Of sodium ions = no, of chloride ions. Each cube has billons of Na and Cl

  6. Properties of Ionic Compounds • 1) Are hard solid with high melting point (ionic bonds are strong) • 2) Brittle (slight shift in structure will lead to repulsion forces, because like charges would repel each other). • 3) Electrolytes – dissolves in water to produce a solution that conducts electricity.

  7. Properties of Ionic Compounds A solution can conduct electricity only if ions are free to move. In solution NaCl separates into ions.

  8. Summary • Metal and non-metals can form ionic compound. • The non-metal atoms pull electrons away from the metal. • Most ionic compounds have high melting points and are hard, brittle electrolytes • Most form three-dimensional crystals with many oppositely charged ions in a fixed ratio.

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