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Ionic Compounds

Ionic Compounds. Chapter 4.1 Binary/Simple Ionic Compounds: Pg. 139-146. Sodium Chloride. Chlorine. Sodium. 0. Compounds. Elements can combine to form compounds. Ionic Compounds. Ions are charged particles formed after the loss or gain of one or more electrons.

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Ionic Compounds

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  1. Ionic Compounds Chapter 4.1 Binary/Simple Ionic Compounds: Pg. 139-146

  2. Sodium Chloride Chlorine Sodium 0 Compounds • Elements can combine to form compounds

  3. Ionic Compounds Ions are charged particles formed after the loss or gain of one or more electrons. Click the “Start” button to review the formation of ions and ionic compounds.

  4. Ionic Compounds • are composed of oppositely charged ions. • are made of a metal and a non-metal

  5. Writing Formulas: Ionic Compounds • Is the compound ionic? If yes, • Write the symbols of the elements with the metal first, then the non-metal. • Write the ionic charge (valence) of each element, above and to the right, for each element. • Criss- cross the numbers down to become subscripts on the opposite element. • Cancel subscripts to the lowest ratio by dividing by the largest common factor.

  6. Step 4: AlCl 3 Writing Formulas: Ionic Compounds Example: Aluminum Chloride Step 1: Aluminum Chloride Is the compound ionic? If yes, 3+ Al Cl 1- Step 2: write symbols & charge of elements Al Cl Step 3: 1 3 criss-cross charges as subsrcipts Cancel to lowest ratio & combine as formula unit (“1” is never shown)

  7. AlO 3 Writing Formulas: Ionic Compounds Example: Aluminum Oxide Aluminum Oxide 3+ Al O 2- Al O 2 3 2

  8. Mg2O2 Writing Formulas: Ionic Compounds Example: Magnesium Oxide Magnesium Oxide 2+ Mg O 2- Mg O 2 2 MgO

  9. Formulas - Simple Ionic Compounds Formula Name lithium oxide • ________________ • ________________ sodium bromide • ________________ • ________________ • ________________ strontium fluoride • ________________ cesium fluoride magnesium hydride potassium chloride

  10. Naming Ionic Compounds • Is the compound ionic? If yes, • Write the symbol for the metal first, then the non-metal. • Name the metal (note: name of the metal does not change) • Name the non-metal. Change the ending to ide.

  11. Naming Ionic Compounds Step 1: NaCl Is the compound ionic?, If yes, Step 2: write symbols for the metal & then the non-metal Step 3: name the metal Step 4 sodium chloride name the non-metal change the ending to IDE

  12. Naming Ionic Compounds Examples: MgCl2 magnesium chloride (Mg2+ Cl1-) Al2S3 aluminum sulfide (Al3+ S2-) Li3N lithium nitride (Li1+ N3-)

  13. Naming Simple Ionic Compounds Formula Name barium oxide • BaO ____________________ • MgI2 ____________________ • KCl ____________________ • CaS ____________________ • GaBr3 ____________________ magnesium iodide potassium chloride calcium sulphide gallium bromide

  14. Look at the textbook • Pg. 146 # 5 – 8 • WS: Ionic Compounds (2 pages)

  15. Multivalent Ionic Compounds Chapter 4.1 Multivalent Ionic Compounds: Pg. 146-147 TEXTBOOK PAGE 146-147

  16. MULTIVALENT METALS Some metals can lose different number of electrons, having more than one possible ion charge or valence. These elements are known as multivalent metals. Examples of multivalent metals Copper (I) Oxide (contains Cu1+) Copper (II) Oxide (contains Cu2+)

  17. MULTIVALENT METALS The charge/valence of the metal is indicated in formula with ROMAN NUMERALS 1 6 2 7 3 8 4 9 5 10

  18. Naming Multivalent Metals • Is the compound ionic? If yes, •  Is the metal multivalent? If yes, •  Uncross the subscripts to determine the valence. •  Double check that the valence on the non-metal matches the value on the periodic table. • If non-metal does not have a correct charge, multiple all oxidation numbers by the charge of the non-metal. •  Write the name of the metal first, then •  Write the charge of the metal in Roman numerals in brackets (determined earlier by uncrossing). •  Name the non-metal. Change ending to ide. Video: http://www.youtube.com/watch?v=yuXNBWC4hTY

  19. Example: CuCl2 Step 1: 1- 2+ Cu Cl2 Ionic ? multivalent ? un-criss cross” the charges Step 2: verify that metal is multivalent; verify charge of non-metal Step 3: copper write the name of the metal Step 4: copper(II) Use the Roman numeralsinbracketsto indicate the chargeof the metal ion copper(II) chloride Step 5: Write name of non-metal; change suffix to ide

  20. Example: FeCl2 Step 1: 1- 2+ Fe Cl2 Ionic ? multivalent ? un-criss cross” the charges Step 2: verify that metal is multivalent; verify charge of non-metal Step 3: Iron write the name of the metal Step 4: Iron (II) Use the Roman numeralsinbracketsto indicate the chargeof the metal ion Iron (II) chloride Step 5: Write name of non-metal; change suffix to ide

  21. Example: FeCl3 Step 1: 1- 3+ Fe Cl3 Ionic ? multivalent ? un-criss cross” the charges Step 2: verify that metal is multivalent; verify charge of non-metal Step 3: Iron write the name of the metal Step 4: Iron (III) Use the Roman numeralsinbracketsto indicate the chargeof the metal ion Iron (III) chloride Step 5: Write name of non-metal; change suffix to ide

  22. Example: SnO Step 1: 1- 1+ Sn O Ionic ? multivalent ? un-criss cross” the charges Step 2: * Charge of non-metal does not match; multiple all charges with charge of non-metal verify charge of non-metal 2(1-) Sn O 2(1+) Step 3: 2+ write the name of the metal 2- Sn O Step 4: Tin (II) Use the Roman numeralsinbracketsto indicate the chargeof the metal ion Tin (II) oxide Step 5: Write name of non-metal; change suffix to ide

  23. Example: SnO2 Step 1: 1- 2+ Sn O2 Ionic ? multivalent ? un-criss cross” the charges Step 2: * Charge of non-metal does not match; multiple all charges with charge of non-metal verify charge of non-metal 2(1-) Sn O 2(2+) Step 3: 4+ write the name of the metal Sn O 2- Step 4: Tin (IV) Use the Roman numeralsin bracketsto indicate the chargeof the metal ion Tin (IV) oxide Step 5: Write name of non-metal; change suffix to ide

  24. Naming Multivalent Ionic Compounds Formula Name tin (IV) fluoride • SnF4 ____________________ • HgO ____________________ • ____________________ • ____________________ • Cr2O3 ____________________ • _____________________ mercury (II) oxide CuF2 copper (II) flouride Cu2S copper (I) sulphide chromium (III) oxide PbO2 lead (IV) oxide

  25. Writing Formulas for Multivalent Metals • Write the symbols for both metal and non-metal. • Write the charges above the symbol (for the metal, use the charge provided in brackets!!!). • Criss-cross charges. • Cancel subscripts to the lowest ratio by dividing by the largest common factor.

  26. Example: Iron (III) bromide Step 3: FeBr 3 Step 1: 3+ 1- Fe Br write charges above symbols of elements (for the multivalent metal, use the charge in the brackets) Fe Br 1 3 Step 2: criss-cross charges as subscripts 1 combine as formula unit FeBr Step 4: 3 simplify if possible

  27. Formulas – Multivalent Ionic Compounds Formula Name nickel (II) oxide • ________________ • ________________ iron (III) phosphide • ________________ • ________________ • ________________ titanium (III) flouride • ________________ titanium (IV) flouride tin (II) sulphide Vandium (V) oxide

  28. Try This • Page 150 question 9 (a-e) • 9a Ni2O3 • 9b CuI2 • 9c Sn3N4 • 9d CrBr2 • 9e FeP • Okay lets have a quiz on this 

  29. Homework • WS: Multivalent Ionic Compound Grid • WS: Binary & Multivalent Ionic Compounds

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