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4.1 Representing Ionic Compounds Part III

4.1. 4.1 Representing Ionic Compounds Part III. Pop Quiz. Name K 3 P What is the chemical formula for beryllium nitride? Draw a Lewis dot diagram for calcium chloride. Bonus Name CuO . 4.1. Multivalent Metals.

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4.1 Representing Ionic Compounds Part III

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  1. 4.1 4.1 Representing Ionic Compounds Part III

  2. Pop Quiz • Name K3P • What is the chemical formula for beryllium nitride? • Draw a Lewis dot diagram for calcium chloride. Bonus • Name CuO.

  3. 4.1 Multivalent Metals • Some metals have more than one ion charge in the periodic table…..which ones?? • These metals are known as multivalent metals and can form different ions depending on the chemical reactions they are involved in • Example: Copper can form ions with +1 or +2 charge Copper II oxide Copper I oxide

  4. 4.1 Multivalent Metals • To distinguish between the different ions, roman numerals are written after the name of the metal • Cu+ is written as copper (I) and Cu2+ is written as copper (II) • On the periodic table, the most common ion is listed at the top of the element’s box

  5. 4.1 Naming Ionic Compounds with Multivalent Metals • When naming a compound with a multivalent ion, you must include a roman numeral to show the charge the ion has • To determine this charge, you need to work back from the charge of the anion…..

  6. 4.1 Naming Ionic Compounds with Multivalent Metals

  7. 4.1 Naming Ionic Compounds with Multivalent Metals • You can also use the reverse cross-over method: • Example: FeO • Add the charge signs for each ion • For FeO, the oxide ion is O2- so the charge on the iron must be 2- • The name of the compound must be iron (II) oxide Fe O Fe+O- Fe?O2-

  8. Multivalent Metals Naming Multivalent Ions • Use Roman numeral to indicate the charge number (e.g.) iron (II) chloride or iron (III) chloride Sample Problem Write the name of CuBr2. • Step 1: Cu can be either Cu+ or Cu2+. We need the total charge to be equal to zero. CuBr2 x+ 2(-1) = 0 x = +2 • Step 2: Write the name of the compound; remember to include a Roman numeral to indicate the charge on copper • the name of CuBr2 is copper (II) bromide

  9. 4.1 Ionic Compounds with Polyatomic Ions • Polyatomic Ion: An ion composed of more than one atom that behaves as a single particle • Example: Carbonate ion (CO32-) • Calcium Carbonate CaCO3 is a ternary compound (not a binary compound!) since it contains more than two elements (Ca, C and O) • Ternary compounds are named the same way as binary compounds: by writing the name of the cation (Calcium, Ca2+) followed by the anion (Carbonate, CO32-)

  10. 4.1 Ionic Compounds with Polyatomic Ions • A few common Polyatomic ions:

  11. 4.1 Ionic Compounds with Polyatomic Ions • A sentence to remember the most common polyatomic ions: • “Nick the Camel ate Clams for Supper in Phoenix” • First letters represent names of polyatomic ions and the number of vowels in each word represents the charge • There is no need to memorize the polyatomic ions, you will always have access to references….

  12. 4.1 Naming compounds that contain polyatomic ions • Calcium hydroxide Ca(OH)2 consists of 1 calcium (Ca)2+ ion and two hydroxide ions (OH)- • Brackets must be used to write polyatomic ions and would be wrong if left out CaOH2 ….why is this the case?

  13. 4.1 Steps for naming compounds that contain polyatomic ions

  14. 4.1 Naming compounds that contain polyatomic ions • The prefixes and suffixes “Ate, Per-Ate, Iteand Hypo-ite” signify the number of oxygens present in the polyatomic ion

  15. Polyatomic Ions Polyatomic ion: an ion made up of more than one atom that acts as a single particle • Name the ionic compound in the same way, with the cation first and the anion second • (e.g.) Na2CO3 sodium carbonate • (e.g.) Ca(OH)2 calcium hydroxide

  16. 4.1 Naming Acids • There are two different types of acids: Binary acids and Oxoacids • When naming acids, there are specific steps that must be taken • Binary Acids are acids composed of two elements – hydrogen and a non-metal Steps to naming Binary acids: Write the root of the non-metal name Add the prefix hydro- to the root name Add the ending –ic to the root name

  17. 4.1 Common Binary Acids

  18. 4.1 Naming Oxoacids • Oxoacidsare composed of hydrogen, oxygen and another element • An acid can be formed with hydrogen and a polyatomic ion that contains oxygen Steps to naming Oxoacids: Write the name of the anion (without –ate or –ite) If the anion ended with –ate, replace it with –icat the end of the name If the anion name ended in –ite, replace it with –ousat the end of the name Add the word acid

  19. 4.1 Common Oxoacids

  20. 4.1 Naming Oxoacids • Notice that for acids names composed of sulfur, the name sulfur- is used and not just sulf- • Notice that for acids names composed of phosphorus, the name phosphor- is used and not just phosph-

  21. 4.1 Writing the Chemical formulas of Acids • To write the chemical formula of an acid, first determine the anion to use in the formula • For Binary acids, use the periodic table to determine the symbol and charge of the anion • For oxoacids, use your table of polyatomic compounds to determine the formula and charge

  22. 4.1 Writing the Chemical formulas of Acids • Example: What is the chemical formula for Carbonic acid? Solution: Step 1: Is it a binary acid, or an oxoacid with a polyatmic ion? The name ends in “-ic” so it must be an oxoacid that contains a polyatomic ion ending with “-ate” Step 2: Use your table of polyatomic ions to find the formula for carbonate CO3-2

  23. 4.1 Writing the Chemical formulas of Acids Step 3: Determine how many H+ ions are needed to have a net charge of 0…..each H+ ion is +1, so I must need 2 H+ ions to neutralize the carbonate ion CO32- Step 4: Write the chemical formula for the acid: Carbonic acid must be H2CO3 Do practice problems #1-2 on page 224

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