1 / 37

Writing and Naming Compounds

Writing and Naming Compounds. You will be writing the black words on your foldable, and the white words in your notes. Metal + Nonmetal Polyatomic Ions Nonmetal + Nonmetal Funny Metals Binary Acid Ternary Acid. It should open like a book. On the front Flaps.

solada
Télécharger la présentation

Writing and Naming 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. Writing and Naming Compounds You will be writing the black words on your foldable, and the white words in your notes.

  2. Metal + Nonmetal Polyatomic Ions Nonmetal + Nonmetal Funny Metals Binary Acid Ternary Acid It should open like a book On the front Flaps

  3. Inside flaps will have 3 examples for each rule Back of book will have the RULE INSIDE THE FOLDABLE

  4. Metal + Nonmetal

  5. Binary Ionic Compound • 1. Write the cation (metal) first • 2. Write the anion (nonmetal) second with –IDE ending • Binary means there are only two types of atoms in the compound • Remember, the total charge on an ionic compound is ZERO.

  6. Examples: • NaCl – Sodium Chloride • MgBr2 – Magnesium Bromide • CaO – Calcium Oxide

  7. Examples for you to try… • LiF • Lithium Fluoride • KCl • Potassium Chloride • BaS • Barium Sulfide • CaF2 • Calcium Fluoride

  8. Writing a formula from the name… • Looking at the name of a compound and using regular ionic charges, you can work backwards and find the formula of a compound • EX: Calcium Chloride • Regular charges: Ca2+ Cl1- • Balance out charges… Ca2+ x 1 Cl1- x 2 • Write out equation… CaCl2

  9. Examples for you to try… • Calcium Bromide • CaBr2 • Sodium Oxide • Na2O • Magnesium Chloride • MgCl2

  10. Polyatomic Ion

  11. You can write all of your polyatomic ions on the back of your foldable to reference

  12. Ternary Ionic Compounds • Ternary means you have 3 or more types of atoms, so you must have a Polyatomic Ion involved • Remember, a Polyatomic Ion is a group of atoms that have a charge when they are together • Most Poly Ions are negative, with the exception of ammonium (NH41+)

  13. Ternary Ionic Compounds • 1. Write your cation first • 2. Write your anion second (if Poly Ion, keep ending; if nonmetal, gets –ide ending)

  14. Examples: • KCN – Potassium Cyanide • Ca(OH)2 – Calcium Hydroxide • NH4F – Ammonium Fluoride

  15. Examples for you to try… • KOH • Potassium Hydroxide • CaSO4 • Calcium Sulfate • BaCO3 • Barium Carbonate

  16. Writing a formula from the name… • Writing a formula from the name of a Polyatomic Ion compound works the same way at Ionic Compounds • Look at the charges and balance them out!

  17. Examples for you to try… • Sodium Carbonate • Na2CO3 • Magnesium Nitrate • Mg(NO3)2 • Ammonium Sulfide • (NH4)2S

  18. Nonmetal + Nonmetal

  19. Covalent Compound • Covalent compounds involve 2 non-metals WITHOUT CHARGES • No balancing of charges are necessary • You look at the number of elements present to determine the name

  20. Covalent Compound • 1. prefixes and –IDE ending • 1 – mono 5 - penta 9 - nona • 2 - di 6 - hexa 10 - deca • 3 - tri 7 - hepta • 4 – tetra 8 – octa

  21. Examples… • CO2 – Carbon Dioxide • (mono NOT used on first word!) • P2O5 – Diphosphorous Pentoxide • Cl9F8 – Nonachlorine Octafluoride

  22. Examples for you to try… • N2Br4 • Dinitrogen Tetrabromide • SO3 • Sulfur Trioxide • Cl2F6 • Dichlorine Hexafluoride

  23. Writing a formula from the name… • By looking at the prefix, you may figure out how many of that nonmetal is used in your formula • Example: Tricarbon Hexaoxide • Tri = 3 carbons, Hexa = 6 oxygens • C3O6

  24. Examples for you to try… • Carbon Heptabromide • CBr7 • Pentanitrogen Octaflouride • N5F8 • Tetraphosphorous Decachloride • P4Cl10

  25. Funny Metals Transition Metals

  26. Transition Metals • Our transitions metals do not follow common ionic charge rules • Some even have more than one possible charge associated with them, meaning there are two possibilities for naming

  27. Transition Metal Compounds • 1. If two charges possible on metal… • Look at anion to determine charge on metal • Write metal with charge in roman numerals after • Write nonmetal with –IDE ending

  28. +2 or +3 Cu, Fe +2 or +4 Sn, Pb

  29. Examples… • FeCl2 • iron(II) chloride • FeCl3 • iron(III) chloride • Sn(NO3)4 • tin(IV) nitrate

  30. Writing a formula from the name… • When working backwards, first look at the roman numeral to determine the charge • Balance out the nonmetal charge • Ex: Lead (IV) Oxide • Charge on lead is 4+ • Charge on oxygen is 2- • To balance out, need two oxygens for every lead • PbO2

  31. Acids • All formulas begin with H (for now) • All names end with “acid” • Acids are covalent compounds that ionize in water

  32. Binary Acids

  33. Binary Acids (H and element) • If the anion ends in –IDE, the acid name is hydro-”stem”-ic acid.

  34. Examples • HCl – Hydrochloric Acid • HS – Hydrosulfuric Acid • HF – Hydrofluoric acid

  35. Ternary Acid

  36. If the anion ends in –ITE, the acid name is “stem”-ous acid.If the anion ends in –ATE, the acid name is “stem”-ic acid. Ternary Acid (H and polyatomic ion)

  37. Examples for you to try… • H2SO3 • sulfurous acid • H3PO4 • phosphoric acid • HNO2 • Nitrous Acid

More Related