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Representing Chemical Compounds

Representing Chemical Compounds. Naming Compounds and Writing Chemical Formulas. Chemical Formula. Shows the kinds and numbers of atoms in the smallest representative unit of the substance.

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Representing Chemical Compounds

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  1. Representing Chemical Compounds Naming Compounds and Writing Chemical Formulas

  2. Chemical Formula • Shows the kinds and numbers of atoms in the smallest representative unit of the substance. • If only one atom of the element in a compound, you only write the element’s symbol. (Ex: Lithium fluoride  LiF) • If the molecules of the element each have more than one atom, a number is used as a subscript. (Ex: Lithium oxide  Li2O).

  3. Molecular Formulas • Chemical formula for a molecular compound is called a molecular formula. • Shows the kinds and numbers of atoms present in a molecule of a compound. • Examples: CO, CO2 • Tells nothing about the structure of the molecule --- doesn’t show arrangement of the various atoms.

  4. Molecular Formulas (continued) • Refer to page 129, Figures 6.6 – 6.8. • Use models and/or diagrams to show the arrangements of molecules in a molecular compound. • IMPORTANT NOTE: Be familiar with the various types of representations of molecular compounds: Molecular formula, Space-filling molecular model, Perspective Drawing, Ball-and-Stick Molecular Model.

  5. Formula Units • Chemical formulas represent ionic compounds. • Formula units – lowest whole-number ration of ions in the compound.

  6. Laws of Definite and Multiple Proportions • Law of Definite Proportions: in samples of any chemical compound, the masses of the elements are always in the same proportions. • Law of Multiple Proportions: whenever two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers. • Refer to page 142, Practice Problems.

  7. Ionic Charges • For most of the Group A elements, the Periodic Table can tell what kind of ion they will form from their location. • Elements in the same group have similar properties. • Including the charge when they are ions.

  8. +1 +2 +3 -3 -2 -1

  9. Naming ions • We will use the systematic way. • Cation- if the charge is always the same (Group A) just write the name of the metal. • Transition metals can have more than one type of charge. • Indicate the charge with roman numerals in parenthesis.

  10. Name These • Na+1 • Ca+1 • Al+3 • Fe+3 • Fe+2 • Pb+3 • Li+1

  11. Write Formulas for these • Potassium ion • Magnesium ion • Copper (II) ion • Chromium (VI) ion • Barium ion • Mercury (II) ion

  12. Naming Anions • Anions are always the same. • Change the element ending to – ide. • F-1 Fluorine • F-1 Fluoride

  13. Name These • N-3 • Br-1 • O-2 • Ga+3

  14. Write These • Sulfide ion • iodide ion • phosphide ion • Strontium ion

  15. Polyatomic Ions • Groups of atoms that stay together and have a charge.

  16. Ions in Ionic Compounds

  17. Naming Binary Ionic Compounds • Binary Compounds - 2 elements. • Ionic - a cation and an anion. • To write the names just name the two ions. • Easy with Representative elements. • Group A • NaCl = Na+ Cl- = sodium chloride • MgBr2 = Mg+2 Br- = magnesium bromide

  18. Naming Binary Ionic Compounds • The problem comes with the transition metals. • Need to figure out their charges. • The compound must be neutral. • same number of + and – charges. • Use the anion to determine the charge on the positive ion.

  19. Naming Binary Ionic Compounds • Write the name of CuO • Need the charge of Cu • O is -2 • copper must be +2 • Copper (II) chloride • Name CoCl3 • Cl is -1 and there are three of them = -3 • Co must be +3 Cobalt (III) chloride

  20. Naming Binary Ionic Compounds • Write the name of Cu2S. • Since S is -2, the Cu2 must be +2, so each one is +1. • copper (I) sulfide • Fe2O3 • Each O is -2 3 x -2 = -6 • 3 Fe must = +6, so each is +2. • iron (III) oxide

  21. Naming Binary Ionic Compounds • Write the names of the following • KCl • Na3N • CrN • Sc3P2 • PbO • PbO2 • Na2Se

  22. Ternary Ionic Compounds • Will have polyatomic ions • At least three elements • name the ions • NaNO3 • CaSO4 • CuSO3 • (NH4)2O

  23. Ternary Ionic Compounds • LiCN • Fe(OH)3 • (NH4)2CO3 • NiPO4

  24. Writing Formulas • The charges have to add up to zero. • Get charges on pieces. • Cations from name of table. • Anions from table or polyatomic. • Balance the charges by adding subscripts. • Put polyatomics in parenthesis.

  25. Writing Formulas • Write the formula for calcium chloride. • Calcium is Ca+2 • Chloride is Cl-1 • Ca+2 Cl-1 would have a +1 charge. • Need another Cl-1 • Ca+2 Cl 2-

  26. Write the formulas for these • Lithium sulfide • tin (II) oxide • tin (IV) oxide • Magnesium fluoride • Copper (II) sulfate • Iron (III) phosphide • gallium nitrate • Iron (III) sulfide

  27. Write the formulas for these • Ammonium chloride • ammonium sulfide • barium nitrate

  28. Things to look for • If cations have (), the number is their charge. • If anions end in -ide they are probably off the periodic table (Monoatomic) • If anion ends in -ate or -ite it is polyatomic

  29. Molecular Compounds Writing names and Formulas

  30. Molecular compounds • made of just nonmetals • smallest piece is a molecule • can’t be held together because of opposite charges. • can’t use charges to figure out how many of each atom

  31. Easier Ionic compounds use charges to determine how many of each. • Have to figure out charges. • Have to figure out numbers. • Molecular compounds name tells you the number of atoms. • Uses prefixes to tell you the number

  32. Prefixes • 1 mono- • 2 di- • 3 tri- • 4 tetra- • 5 penta- • 6 hexa- • 7 hepta- • 8 octa-

  33. Prefixes • 9 nona- • 10 deca- • To write the name write two words

  34. Prefixes • 9 nona- • 10 deca- • To write the name write two words • Prefix name Prefix name -ide

  35. Prefixes • 9 nona- • 10 deca- • To write the name write two words • One exception is we don’t write mono- if there is only one of the first element.

  36. Prefixes • 9 nona- • 10 deca- • To write the name write two words • One exception is we don’t write mono- if there is only one of the first element. • No double vowels when writing names (oa oo)

  37. Name These • N2O • NO2 • Cl2O7 • CBr4 • CO2 • BaCl2

  38. Write formulas for these • diphosphorus pentoxide • tetraiodide nonoxide • sulfur hexaflouride • nitrogen trioxide • Carbon tetrahydride • phosphorus trifluoride • aluminum chloride

  39. Acids Writing names and Formulas

  40. Acids • Compounds that give off hydrogen ions when dissolved in water. • Must have H in them. • will always be some H next to an anion. • The anion determines the name.

  41. Naming acids • If the anion attached to hydrogen is ends in -ide, put the prefix hydro- and change -ide to -ic acid • HCl - hydrogen ion and chloride ion • hydrochloric acid • H2S hydrogen ion and sulfide ion • hydrosulfuric acid

  42. Naming Acids • If the anion has oxygen in it • it ends in -ate of -ite • change the suffix -ate to -icacid • HNO3 Hydrogen and nitrate ions • Nitricacid • change the suffix -ite to -ous acid • HNO2 Hydrogen and nitrite ions • Nitrousacid

  43. Name these • HF • H3P • H2SO4 • H2SO3 • HCN • H2CrO4

  44. Writing Formulas • Hydrogen will always be first • name will tell you the anion • make the charges cancel out. • Starts with hydro- no oxygen, -ide • no hydro, -ate comes from -ic, -ite comes from -ous

  45. Write formulas for these • hydroiodic acid • acetic acid • carbonic acid • phosphorous acid • hydrobromic acid

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