1 / 11

Naming Binary Compounds

Naming Binary Compounds. **** CRISS-CROSS METHOD!!!!! *** Take the oxidation state of each element and/or polyatomic ion and criss-cross them to get your formula!! (Do not include charge in formula) Always reduce ionic compounds so that atoms are in their smallest whole # ratio!

jlenoir
Download Presentation

Naming Binary Compounds

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 Binary Compounds ****CRISS-CROSS METHOD!!!!!*** Take theoxidation state of each element and/or polyatomic ion and criss-cross them to get your formula!! (Do not include charge in formula) Always reduce ionic compounds so that atoms are in their smallest whole # ratio! Mg+2 and Cl-1 MgCl2 (magnesium chloride)

  2. Table E—Selected Polyatomic Ions

  3. Variations for Type 1 Compounds Metal & Non-metal (NaF= sodium fluoride) Metal & - polyatomic ion (NaOH = sodium hydroxide) +Polyatomic ion & Non-metal (NH4F = ammonium fluoride) 2 polyatomic ions (NH4OH = ammonium hydroxide)

  4. If metal has more than one + oxidation number use roman numerals to show which one FeCl3 = Iron (III) chloride FeCl2 = Iron (II) chloride

  5. Naming Binary Compounds Type 3 Rules for Naming Binary Covalent/Molecular Compounds (non-metal & non-metal) The first element in the formula is named first, using the full element name. Drop the ending of the 2nd element in the compound and add the ending –ide. Prefixes(shown below) denote the # of atoms present Also consider that: The prefix mono is never used with the first element, only from -di on. The second non-metal always gets a prefix

  6. Names and Formulas of Ionic Compounds (Type 1 & 2) Putting It All Together: PRACTICE!! Name the following compounds given the formula: 1) Na2SO4 9) Al(NO3)3 10) Cu(ClO4)2 3) Fe(NO3)3 11) NH4Br 4) Mn(OH)2 12) Cr2O3 5) Na2SO3 13) Co(NO3)2 6) Na2CO3 14) K2SO4 7) CaCl2 15) Ba(OH)2 8) FeCl3

  7. Names and Formulas of Ionic Compounds Putting It All Together: PRACTICE!! Write the formula for each compound, given the name: Sodium hydrogen carbonate 7) Nickel (II) perchlorate Cesium perchlorate 8) Iron (II) phosphate Sodium hypochlorite 9) Titanium (IV) oxide Sodium selenate 10) Magnesium sulfate Potassium bromate 11) Silver sulfide Potassium sulfide 12) Lead (II) nitrate

  8. Names and Formulas of Binary Covalent/Molecular Compounds Name the following compounds: Cl2O 5) SO2 N2O4 6) PCl5 NF3 7) N2O3 P4S10

  9. Classifying Chemical Reactions • Synthesis: H2O + CO2 H2CO3 • Decomposition:NaCl Na + Cl • Single Replacement: Fe + CuSO4 FeSO4 + Cu • Double Replacement: NaCl + AgNO3 NaNO3 + AgCl

  10. Balancing Chemical Reactions LAW OF CONSERVATION OF MASS, ENERGY, & CHARGE: In all chemical reactions there is conservation of mass, energy and charge. The amount of matter stays the same (one side equals the other). The total amount of energy stays the same (one side equals the other). The number of positive (or negative) charges stays the same (one side equals the other). In a chemical reaction, all of the elements or compounds found to the left of the equation are known as the reactant(s), and resulting elements or compounds are known as the product(s). 2H2 + O22H2O (reactants) (product)

  11. IUPAC International Union of Pure and Applied Chemistry When a question states “Write the IUPAC name” they are talking about the organization above. All chemical and “common” names must be approved by them. Basically it means “JUST NAME IT!!” 

More Related