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Writing Ionic Formulas and Naming Ionic Compounds

Writing Ionic Formulas and Naming Ionic Compounds. Example. Writing Formulas. Hint: Switchy-Switchy. Steps 1. Write each element with its charge (Periodic Table Columns can help with this) 2. Switchy-Switchy. Example: Let’s make a compound using magnesium and chlorine. +2. -1. Mg.

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Writing Ionic Formulas and Naming Ionic Compounds

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  1. Writing Ionic Formulas and Naming Ionic Compounds

  2. Example Writing Formulas Hint: Switchy-Switchy • Steps • 1. Write each element with its charge (Periodic Table Columns can help with this) • 2. Switchy-Switchy Example: Let’s make a compound using magnesium and chlorine +2 -1 Mg Cl

  3. Writing Formulas Hint: Switchy-Switchy • Steps • 1. Write each element with its charge (Periodic Table Columns can help with this) • 2. Switchy-Switchy • 3. Reduce Example: Let’s make a compound using magnesium and chlorine Example Mg Cl 1 2

  4. Naming Ionic Compounds • Example: MgCl2 • Steps • 1. Name the metal (cation) • 2. If the metal is a transition element, you must add a Roman Numeral in ( ) for the charge number (oxidation number) • 3. Name the non-metal (anion) changing ending to –ide Magnesium Chloride

  5. Let’s look at TiO Titanium (II) Oxide Is titanium a transition element? Then we need a Roman Numeral But which one? We need to balance the charge The charge of O is _____, so we must be using a Ti with a charge of _____. -2 +2 Remember Switchy-Switchy then reduce

  6. Anion Endings • If you see a name that ends in –ide, you are dealing with an element, unless peroxide, hydroxide, or cyanide • If you see a name that ends in -ate or –ite, you are dealing with a polyatomic ion (Page 178 or back of periodic table)

  7. Polyatomic Hint • Nick the Camel ate Supper in Phoenix. • OHNicky! • In the first saying, the first letter gives element, number of consonants gives number of oxygens, and number of vowels give charge. • Second is for Hydroxide (OH-) and ammonia (NH4+)

  8. How to read/name Polyatomic Ions • The first “rule” looks at the number of oxygens in an ion • Think of the -ate ion as being the "base" name • The per- prefix adds an oxygen. • -ite will reduce the oxygens by one. • Adding hypo- to the –ite version will reduce the number of oxygens by another 1 • In all situations, the charge is NOT affected.

  9. For example, let’s look at the polyatomic ions that involve chlorine • Cl- • ClO- • ClO2- • ClO3- • ClO4- chloride hypochlorite chlorite chlorate perchlorate

  10. How to read/name Polyatomic Ions • “Rule 2”: when the prefix bi- is added to a name, a hydrogen is added to the ion's formula and its charge is increased by +1 • An Example: • Carbonate – CO32- • Bicarbonate – HCO3-

  11. How to work with polyatomic ions • Think of them as a single ion • All the atoms stay together and if you need more than one, you have to use parenthesis. • For example, Magnesium Hydroxide +2 -1 ( ) Mg OH 2

  12. Practice Li+ Br- LiBr Na+ O-2 Sodium oxide Pb+2 F- Lead (II) Fluoride Magnesium phosphate Mg3(PO4)2 Copper (I) Carbonate Cu+ CO3-2 (NH4)2SO4 NH4+ SO4-2

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