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Representing Chemical Compounds Naming Compounds and Writing Chemical Formulas.

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Presentation on theme: "Representing Chemical Compounds Naming Compounds and Writing Chemical Formulas."— Presentation transcript:

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  Li 2 O).

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, CO 2 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.


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. l Change the element ending to – ide. l F-1 Fluorine l 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 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 Na 3 N CrN Sc 3 P 2 PbO PbO 2 Na 2 Se

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 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. –H–Have to figure out charges. –H–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 -ic acid HNO3 Hydrogen and nitrate ions Nitric acid change the suffix -ite to -ous acid HNO2 Hydrogen and nitrite ions Nitrous acid

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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