Ch 12.1 What are compounds? Two or more elements chemically combined to form a new substance.

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1 Ch 12.1 What are compounds? Two or more elements chemically combined to form a new substance.

2 Structure of Compounds Network Structures = strong solids Molecules= weak solids, liquids, or gases

3 Bonding Chemical Bonds the attractive forces that hold different atoms or ions together -Bonds distinguish compounds from mixtures.

4 Why Bond? Valence electrons are the key important role Atoms bond to achieve a full outer energy level OCTET RULE: They want 8 VALENCE electrons.

5 I guess no everyone can hold 8 e-

6 Chemical Bonds: Types COVALENT METALIC IONIC ALL NONMETALS atoms METAL and NONMETAL ions Holding a compound Holding a compound ALL METALS together together holding an element together

7 Electronegativity Difference (ED) the difference in electronegativity between two or more elements in a compound. EX. NO N=3.07 O=3.50 [ ] = 0.43 Electronegativity difference of NO = 0.43 Tells us two things

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9 1. Bond Character (Type) If the compound has an ED of > 1.6, then the compound has more ionic properties. (network structure) If the compound has an ED of < 1.6, then the compound has more covalent properties. (molecule)

10 Ionic bond Properties Strong bonds (network structure) High melting points Good conductors of electricity when dissolved or melted (ions) solid phase (salts)

11 Covalent bond Properties Weak bonds (molecules) Low melting points Bad conductors of electricity (no ions) Weak solids, liquid or gas phase

12 2. Polarity (ch. 14.1) Property of a molecule caused by an unsymmetrical charge distribution Molecule with a positive and negative end. (polar) Polar molecules are unsymmetrical in shape Nonpolar molecules are symmetrical in shape

13 Unsymmetrical Shape Polar molecule

14 + Boron Trifluoride B + Same all around Symmetrical shape Nonpolar molecule +

15 2. Polarity If the compound has a ED of < 0.4, then the compound is nonpolar covalent. If the compound has a ED of < 1.6, (>0.4) then the compound is polar covalent.

16 Ch Metallic bond Formed by the attraction between positively charged metal ions and the sea of electrons around them. Held together by delocalized, free-flowing electrons along the bond

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18 Metallic bond Properties Strong Bonds High melting points Good conductors of electricity Metal elements and alloys

19 Ch7.1 LANGUAGE OF COMPOUNDS CHEMICAL SYMBOLS: ELEMENTS CHEMICAL FORMULA: COMPOUNDS SUBSCRIPT: NUMBER OF EACH ATOM BRACKETS: Mg 3 (PO 4 ) 2

20 Using Dot Diagrams Dot diagrams may be used to show how electrons are shared or how they will be transferred

21

22 1. Covalent Bonds A bond formed by the sharing of valence electrons (co VALENT) Also called molecules Formed between two or more nonmetal atoms

23 TYPES OF BONDS SINGLE BONDS DOUBLE BONDS TRIPLE BONDS

24

25 Ch. 7.2 Molecular Formula The actual formula of a covalent molecule.

26 Empirical Formula The simplest whole-number ratio a chemical formula can have. Different covalent compounds can have the same empirical formula

27 Organic Molecules

28 The other Organic molecules

29 Naming Covalent Compounds Prefixes for # of atoms Mono 1 Di - 2 Tri - 3 Tetra - 4 Penta - 5 Hexa 6 Hepta - 7 Octa - 8 Nona - 9 Deca - 10

30 Naming Covalent Compounds Step 1 Identify the number of atoms in the first element Ex. H O two H atoms 2

31 Naming Covalent Compounds Step 2 Identify the number of atoms in the 2 nd element. Ex. H 2 O one O atom

32 Naming Covalent Compounds Step 3 Name the compound with the appropriate prefixes. Ex. H O 2 dihydrogen monoxygen

33 Naming Covalent Compounds Step 4 add an -ide ending to the second element Ex. Dihydrogen monoxide

34 2. Ionic bond (ch. 7.1) A bond formed by the attraction between oppositely charge ions. The transferring of valence electrons Formed between metal ions and nonmetal ions Na + + Cl - NaCl

35

36

37 Oxidation # s/ion Charges Charge given to an ion to tell us how many electrons were lost or gained in order to become stable. Ionic compounds

38 Assigning Charges Group one have a 1 + ion charge Group two have a 2 + ion charge

39 Assigning Charges Group 17 have a 1 - ion charge O, S, and Se of group 16 have a 2 - ion charge

40 Assigning Charges N and P of group 15 have a 3 - ion charge Aluminum has a 3 + ion charge

41 Assigning Charges Group 3-12 have multiple charges depending on the nonmetal they are bonding. Same with metals in group 14. (Sn, Pb)

42 Writing Ionic Compounds Step 1 Calcium Fluoride Write both positive and negative ions (use ion table if you need it) Ca: = Ca 2+ :F: = F -1

43 Writing Ionic Compounds Step 2 Criss-cross charges down, making subscripts Ca 2+ F -1 Ca 1 F 2

44 Writing Ionic Compounds Step 3 Combine your new compound. Ca 1 F 2 Ca 1 F 2

45 Ionic bonds Ionic bonds may contain polyatomic ions in them. An ion made from two or more atoms covalently bonded together that act like a single ion. A molecule with a charge, example sulfate (SO 4 ) -2 EX Na +1 + (SO 4 ) -2 Na 2 (SO 4 ) Covalent Bond Ionic bond between 2 ions

46 Polyatomic ion Aluminum Carbonate Al +3 (CO 3 ) -2 Al 2 (CO 3 ) 3 Al 2 (CO 3 ) 3

47 Ch. 7.2 Naming Ionic Compounds Step one Name the first ion in the formula Ex. CaCl 2 calcium

48 Naming Ionic Compounds Step two Name the second ion Ex. CaCl 2 Calcium Chloride

49 PROBLEM Ex. Fe 2 O 3 and FeO are different compounds Fe 3+ O 2- = Fe 2 O 3 Fe 2+ O 2- = FeO

50 Solution-Roman Numerals Same naming scheme Add a Roman Numeral to identify the charge of the metal.

51 Solution-Roman Numerals Fe 3+ O 2- = Fe 2 O 3 Fe 2+ O 2- = FeO Fe 2 O 3 = iron(iii)oxide FeO = iron(ii)oxide

52 Naming Ionic Compounds Non binary Compounds (more than 2 elements) Step one Name the first ion in the formula Ex. Ca(CO 3 ) calcium Step two Name the second ion Ex. Ca(CO 3 ) Calcium Carbonate

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