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Ch 8.2 Ionic Bond Properties

Ch 8.2 Ionic Bond Properties. Ionic Bonds. Ions – Atom or group of atoms that has become electrically charged Negative ion (-) – gains extra electron Positive ion (+) – loses an electron Forming IONs depends upon Valence Electrons

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Ch 8.2 Ionic Bond Properties

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  1. Ch 8.2 Ionic Bond Properties

  2. Ionic Bonds • Ions – Atom or group of atoms that has become electrically charged • Negative ion (-) – gains extra electron • Positive ion (+) – loses an electron • Forming IONs depends upon Valence Electrons • Sodium has ONE Valence Electron (wants to give one away to have full electron shell) • Chlorine has SEVEN Valence Electrons (wants to TAKE one electron to have full electron shell)

  3. Ionic Bonds • IONIC Bond is formed by the ATTRACTION between 2 oppositely charged ions • IONIC Bonds are caused by DONATING Electrons • Ions are electrically charged • Ionic compounds are electrically neutral

  4. IONIC Bonds

  5. Ionic Bonds • The number of electrons lost by the Cation MUST EQUAL the number of electrons gained by the Anion. • Calcium makes a 2+ cation • Fluorine makes a 1- anion • Therefore it takes 2 fluorine atoms to combine with one calcium atom to create calcium fluoride • Chemical formula is CaF2

  6. IONIC Bonds • Polyatomic Ions – an ion made of more than one atom • CO3 (Carbonate) • SO4 (Sulfate) • Naming Ionic Compounds • Name of positive ion comes first • Name of negative ion comes second, plus –ide • Example: NaCl = sodium chloride, • Example: KI = potassium iodide

  7. Properties of Ionic Compounds • Crystal shape • Alternate positive and negative ions in patterns • Crystals are all the same shape for each compound • High melting points • Table Salt Melting point is 801oC • Conduct electricity • Dissolve in water • Ions become more loosely associated • Pass electrical charges along

  8. 2.3 Review Questions • How does an Ion form from an atom? • The atom gains or loses an electron • What properties may be used to identify an ionic compound? • Crystal shape, high melting point, conducts electricity • Why are ions in an ionic compound attracted to each other? • They are oppositely charged

  9. 2.3 Review Questions • Name these compounds: NaF, BeI2, K2SO4, CaO, H2S, MgCO3 • Sodium fluoride • Berylium Iodide • Potassium Sulfate • Calcium Oxide • Hydrogen Sulfide • Magnesium Carbonate

  10. 2.3 Review Questions • Solid Salt does not conduct electricity. How then does dissolving salt in water allow electricity to flow? • Water breaks the ions apart, allowing the ions to move freely. • The metal Scandium has 3 valence electrons. What is the formula for the ionic compound formed from Scandium and Iodine? • ScI3 • Scandium has 3 valence electrons to donate, but each Iodine can only take one. Therefore, it takes 3 iodines to bond with one Scandium.

  11. Ionic Compounds Lab #1 Substances Tested: • benzoic acid, (C6H5COOH) • magnesium chloride, (MgCl2) • petrolatum (vaseline) • potassium iodide (KI) replaced with potassium BROMIDE (KBr) • sodium sulfate (Na2SO4) • sucrose (C12H22O11) • sodium bicarbonate (NaHCO3) • Unknown #1 • Unknown #2 What do you observe about the unknown? • Is it ionic or not? • What do you think it might be good for? • What do you think it is? • How could you test it further to find out?

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