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Ionic Bonding and IMF

Ionic Bonding and IMF. Unit 3. 12.1 Types of Chemical Bonds. What is a bond and what holds it together? What are the two types of bonds?. 12.2 Electronegativity. How does electronegativity affect the bond type?. 12.2 Electronegativity. Which elements will form each type of bond?.

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Ionic Bonding and IMF

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  1. Ionic Bonding and IMF Unit 3

  2. 12.1 Types of Chemical Bonds • What is a bond and what holds it together? • What are the two types of bonds?

  3. 12.2 Electronegativity • How does electronegativity affect the bond type?

  4. 12.2 Electronegativity • Which elements will form each type of bond?

  5. 12.3 Bond Polarity and Dipole Moments • When will a dipole moment occur within a compound?

  6. 12.4 Stable Electron Configurations and Charges on Ions • Look at the electron configuration of sodium: • Look at the electron configuration of the sodium ion: • Look at the electron configuration of neon: • Notice anything? • In almost all stable chemical compounds of the representative elements, all of the atoms have achieved a noble gas electron configuration

  7. 12.5 Ionic Bonding and Structures of Ionic Compounds • Formed between two oppositely charged ions. • We write the formulas for these compounds, but they are empirical formulas. • Ionic compounds can be formed with monatomic ions as well as polyatomic ions.

  8. 5.2 Naming Binary Compounds that Contain a Metal and a Nonmetal • Metals with FIXED Charges: • Ag+ • Zn2+ • Cd2+ • Al3+ • All alkali and alkaline earth metals • Metals w/o a Fixed Charge

  9. FIXED CHARGED METALS • Cation(metal) is named first • Anion (non-metal) is named second • The name of the anion takes the root name of the element with an “ide” ending. • Examples: • NaCl is sodium chloride. • CaCl2 is calcium chloride.

  10. Practice • AlCl3 • CaO • Li3N • MgI2 • Ag2S

  11. VARIABLY CHARGED METALS • Cation (metal) is named first • Denote the charge on the metal using Roman Numerals (I, II, III, IV, V, VI, VII, VIII, IX, X) • Must be determined by using the known charge of the non-metal • Anion (non-metal) is named second • The name of the anion takes the root name of the element with an “ide” ending. • Examples: • CuCl is copper (I) chloride. • CuCl2 is copper (II) chloride.

  12. Practice • FeCl3 • CrO • Mn2O7 • CrN • Mn2S

  13. 5.4 Naming Binary Compounds: A Review

  14. 5.5 Naming Compounds that Contain Polyatomic Ions • Not a binary compound; therefore, it contains a polyatomic ion • Polyatomic ions are groups of elements covalently bound that have a charge. • A list of polyatomic ions are found on the back of your periodic table. • Example: • NH4+ is an ammonium ion • SO32- is a sulfite ion • SO42- is a sulfate ion • PO43- is a phosphate ion

  15. 5.5 Naming Compounds that Contain Polyatomic Ions • Cationcomes first, anion second • Polyatomic ion names are NOT altered with “ide” endings or prefixes • All other rules for ionic compounds apply. • Examples: • NH4Cl is ammonium chloride. • Na3PO4 is sodium phosphate. • CuSO4 is copper (II) sulfate.

  16. Practice • NaNO3 • CaSO3 • (NH4)2O • Mn3(PO4)7 • NH4NO3

  17. 5.7 Writing Formulas from Names • Write each ion. • Determine how many you need of each to form a neutral compound and put this number as a subscript. • Keep polyatomic ions in parentheses if you have more than one.

  18. Practice • Magnesium fluoride • Iron (I) nitride • Potassium phosphate • Copper (II) nitrate • Manganese (VII) oxide • Aluminum oxide

  19. 14.3 Intermolecular Forces • INTRAmolecular vs. INTERmolecular Forces: • Intermolecular forces in ionic compounds is the result of an electrostatic attraction between oppositely charged ions. • The strongest of all intermolecular forces. • Most ionic compounds are found in the solid form.

  20. 14.5 The Solid State: Types of Solids • Crystalline solids: regular arrangement of components • Ionic solids are comprised of oppositely charges ions. • The ions are in a closely packed arrangement called a lattice.

  21. 14.6 Bonding in Solids • Ionic Solids • Extremely stable with high melting points • If dissolved in water, the solid dissociates and can conduct electricity.

  22. Summary • Covalent Compounds • NO metals • Share Electrons • Lewis Structures • Names Use Prefixes • IMF: • H bond>Dipole>LD • Lower melting points and boiling points • Strength increases with more electrons • Form Organic Compounds • Ionic Compounds • Metal with Nonmetal • Transfers Electrons • Opposite Ions Attract • Nomenclature Determined by the Metal or Polyatomic Ion • IMF: • Electrostatic attractions • Strongest • High melting points and boiling points • Usually found as solids

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