1 / 24

Naming and Writing Formulas

Naming and Writing Formulas. Types of Compounds. There are two types of compounds. Ionic: contain either… a metal (or metalloid to the left of the line) and an nonmetal (or metalloid to the right of the line) a polyatomic ion Covalent: Contain two nonmetals. Ionic Compounds.

hal
Download Presentation

Naming and Writing Formulas

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Naming and Writing Formulas

  2. Types of Compounds • There are two types of compounds. • Ionic: contain either… • a metal (or metalloid to the left of the line) and an nonmetal (or metalloid to the right of the line) • a polyatomic ion • Covalent: Contain two nonmetals

  3. Ionic Compounds • Must contain a positive ion (cation) and negative ion (anion). • The + is written first, the – is written second. • The total charge on the compound must equal 0.

  4. #1 – Name the metal #2 – Name the nonmetal, changing the ending to –ide. Examples: MgO CaCl2 NaBr Sr3P2 magnesium oxide calcium chloride sodium bromide strontium phosphide Naming Binary Ionic Compounds

  5. Writing Formulas • The subscripts tell how many of each atom you have. (The overall charge must equal zero!!) • EXAMPLE: Write the chemical formula for the compound containing Al and Br. • #1 – determine the charges Al+3 Br-1

  6. #2 – cross the charges. Al+3 Br-1 • #3 – Write the formula, simplify if needed AlBr3 1 3

  7. Try this one… • Write the chemical formula for the compound containing Mg and S • #1 – determine the charges Mg+2 S-2

  8. #2 – cross the charges. Mg+2 S-2 • #3 – Write the formula, simplify if needed Mg2S2 MgS 2 2

  9. #1 – name the 1st part of the compound #2 – name the 2nd part If it is a polyatomic ion, DO NOT change the ending If it is a nonmetal, change to –ide. Examples: CaCO3 Na3SO4 (NH4)2S Calcium carbonate Sodium sulfate Ammonium sulfide Ionic Compounds with Polyatomic Ions

  10. Writing Formulas: • Same rules apply, except if the polyatomic ion gets a subscript you MUST use parentheses around it. • Example: • Write the formula for sodium hydroxide. Na+1 OH-1 NaOH 1 1

  11. Calcium phosphate Ca+2 PO4-3 Ca3(PO4)2 3 2

  12. Aluminum nitrite Al+3 NO2-1 Al(NO2)3 1 3

  13. Compounds containing Metals with Variable Charges(The Stock System)

  14. Variable Charges • Metals in Group 1, Group 2, Zinc (+2), Silver (+1) and Aluminum only have one charge. • The rest have variable charges so we have to tell what charge the ion has in our compound when we name it.

  15. Naming • #1 – Name the metal. • #2 – Add a roman numeral telling the charge on the metal in parentheses. • I-1 II-2 III-3 IV-4 V-5 VI-6 VII-7 • #3 – Name the negative ion as before.

  16. Example • CrO • O is a -2 charge • To make a neutral compound, Cr must be a +2. • Chromium (II) oxide

  17. FeCl3 • Cl is a -1 charge • There are 3 chlorine ions  -3 • The ONE Fe must be a +3 • Iron (III) chloride

  18. CoCO3 • Carbonate is a -2 • Co is a +2 • Cobalt (II) carbonate

  19. Ni3(PO4)2 • Phosphate = -3 x 2 = -6 • There are 3 nickel atoms so each one = +2 to equal +6 • Nickel (II) phosphate

  20. Mn(SO4)2 • Sulfate is -2, there are two  -4 • so the ONE Manganese = +4 • Manganese (IV) sulfate

  21. Writing formulas: • Rules are the same as before.

  22. copper (III) oxide Cu+3 O-2 Cu2O3 2 3

  23. Manganese (IV) sulfide Mn+4 S-2 Mn2S4 MnS2 4 2

  24. Iron (II) nitrate Fe+2 NO3-1 Fe(NO3)2 1 2

More Related