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Naming Ionic Compounds

Naming Ionic Compounds. “Perhaps one of you gentlemen would mind telling me just what is outside the window that you find so attractive..?”. Ionic Bonding. Atoms lose or gain electrons to form ions Cations are positive ions metals generally form cations Anions are negative ions

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Naming Ionic Compounds

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  1. Naming Ionic Compounds

  2. “Perhaps one of you gentlemen would mind telling me just what is outside the window that you find so attractive..?”

  3. Ionic Bonding • Atoms lose or gain electrons to form ions • Cations are positive ions • metals generally form cations • Anions are negative ions • non-metals generally form anions • Ionic compounds are held together by electrostatics- the positive charge of the cation attracting the negative charge of the anion.

  4. Oxidation Numbers • The number of electrons an atom gains or loses to have a full outer energy level. • The charge an atom acquires when it becomes an ion. • Includes a + or – sign following by a number.

  5. Ionic Compound • METAL + NONMETAL • Important metal ions • group 1 - lose 1 electron (+1 oxidation #) • group 2 - lose 2 electrons (+2 oxidation #) • group 13 - lose 3 electrons (+3 oxidation #) • Transition metals also form ionic compound • Their behavior is less predictable – multiple oxidation states • Ionic Charge shown as Roman Numerals in compound name • Iron forms Fe+2 or Fe+3 Fe (II) or Fe (III) • Copper forms Cu+ or Cu+2 Cu (I) or Cu (II)

  6. Important Nonmetal Ions • Group 17 gain 1 electron (-1 oxidation #) • Group 16 gain 2 electrons (-2 oxidation #) • Group 15 gain 3 electrons (-3 oxidation #) Main group elements gain or lose electrons so that they have 8 valence electrons. (Octet Rule).

  7. Polyatomic Ions • Compounds which carry a charge. (Usually negative) • Never change a polyatomic ions’ subscripts! • Polyatomic ions are listed on your periodic table. • Examples: • NO3- Nitrate • OH- Hydroxide • SO42- Sulfate

  8. Naming Ionic Compounds • Positive (Cation) ion always written first and left unchanged. • The charge of an element with multiple oxidation states is identified by Roman Numerals in parenthesis after its name. • Negative (Anion) ion’s ending is changed to – ide if its an element. • Polyatomic ions always are written with name unchanged.

  9. Name These Ionic Compounds • NaCl • MgBr2 • CaO • FeO (if Fe has a +2 charge) • Fe2O3 (if Fe has a +3 charge) • NaOH • BaSO4

  10. Criss Cross Methodof Writing Chemical Formulas • Write the symbol for the cation first, then the anion. (Make sure to put parentheses around any polyatomic ions.) • Write the charges after each ion as superscripts • If the charges are equal and opposite, write the formula without any subscripts. • If the charges are not equal an opposite, Criss Cross the numbers only, not the + and – signs. • Simplify all subscripts to the least common multiples.

  11. Criss Cross Method Example Write the chemical formula for an ionic compound made of magnesium and nitrogen. Mg+ N- Mg N 2 3

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