Bonding and Inorganic Nomenclature

1. lithium nitrate lead (II) sulfide barium sulfide lithium nitride Chemistry sulfur dioxide lithium nitrite Bonding and Inorganic Nomenclature NO2 NaClO3 N2O4 Fe(ClO3)2 N2O5 Fe(ClO3)3

2. potassium nitrate copper (II) sulfate sodium hydroxide KNO3 NaOH Cu2SO4 dinitrogen monoxide N2O Inorganic Nomenclature

3. Vocabulary Chemical Bond attractive force between atoms or ions that binds them together as a unit bonds form in order to… decrease potential energy (PE) increase stability Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

4. Types of Bonds Covalent Bonding - True Molecules Nitrogen Water Ammonia Diatomic Molecule

5. Metallic Bonds In metals, valence shells of atoms overlap, so v.e– are free to travel between atoms through material. Not so in metals. In insulators (like wood), the v.e– are attached to particular atoms.

6. ductile conduct heat and electricity malleable Properties of Metals All due to free-moving v.e–.

7. Types of Bonds Table salt Ionic Bonding - Crystal Lattice

8. calcite Properties of Salts 1. very hard – each ion is bonded to several oppositely -charged ions 2. high melting points – many bonds must be broken with sufficient force, like atoms are brought next to each other and repel 3. brittle –

9. loses e– gains e– Na1+ + Cl1– K1+ + NO31– Chemical Bonding Ionic Bonds: atoms give up or gain e– and are attracted to each other by coulombic (electrical) attraction Na1+ Cl Cl1– Na NaCl ionic compounds = salts KNO3 where NO31– is a polyatomic ion: a charged group of atoms that stay together

10. has neutral charge; Writing Formulas of Ionic Compounds chemical formula: shows types of atoms and how many of each To write an ionic compound’s formula, we need: 1. the two types of ions (i.e., “pink” and “blue”) 2. the charge on each ion NaF Na1+andF1– BaO Ba2+andO2– Na2O Na1+andO2– BaF2 Ba2+andF1–

11. 2 2 2 1 3 3 charge on cation / anion “becomes” subscript of anion / cation criss-cross rule: ** Warning: Reduce to lowest terms. Al3+andO2– Ba2+andS2– In3+andBr1– AlO InBr BaS InBr3 Al2O3 BaS

12. Writing Formulas w/Polyatomic Ions Parentheses are required only when you need more than one “bunch” of a particular polyatomic ion. Ba2+andSO42– BaSO4 Mg2+andNO21– Mg(NO2)2 NH41+andClO31– NH4ClO3 Sn4+andSO42– Sn(SO4)2 Fe3+andCr2O72– Fe2(Cr2O7)3 NH41+andN3– (NH4)3N

13. Na Ba A. To name, given the formula: 1. Use name of cation. 2. Use name of anion (it has the ending “ide”). sodium fluoride NaF barium oxide BaO sodium oxide Na2O barium fluoride BaF2

14. Zn Ca B. To write formula, Ag given the name: 1. Write symbols for the two types of ions. 2. Balance charges to write formula. Ag1+ Ag2S S2– silversulfide Zn2+ P3– Zn3P2 zincphosphide Ca2+ I1– CaI2 calciumiodide

15. Ionic Compounds (cation/anion combos) The Unique-Charge Cations (Always have the same charge when ionized) The unique-charge cations are: groups 1, 2, 13, and Ag1+, Cd2+, and Zn2+ 1 2 13

16. Zn Cd Ag Variable-Charge CationswithElemental Anions The Variable (multiple)-charge cations are: Pb, Sn, and the transition elements (but – not Ag+1, Cd+2, or Zn+2)

17. Cu Fe A. To name variable charge elements, given the formula: • Figure out charge on • cation. 2. Write name of cation. 3. Write Roman numerals in ( ) to show cation’s charge. Stock System of nomenclature 4. Write name of anion. iron oxide Fe2+ Fe? iron (II)oxide FeO O2– iron oxide Fe? O2– Fe2O3 Fe? Fe3+ O2– O2– Fe3+ iron (III)oxide CuBr copper bromide Cu? Br1– copper (I)bromide Cu1+ CuBr2 copper bromide Br1– copper (II)bromide Cu2+ Cu? Br1–

18. Co Sn B. To find the formula, given the name: 1. Write symbols for the two types of ions. 2. Balance charges to write formula. cobalt (III) chloride Co3+ Cl1– CoCl3 Sn4+ O2– SnO2 tin (IV) oxide Sn2+ tin (II) oxide O2– SnO

19. Compounds Containing Polyatomic Ions Insert name of ion where it should go in the compound’s name. Write formulas: iron (III) nitrite Fe3+ NO31– Fe(NO3)3 iron (III)nitrite ammonium phosphide (NH4)3P ammoniumphosphide NH41+ P3– ammonium chlorate NH4ClO3 ClO31– NH41+ ammonium chlorate zinc phosphate Zn3(PO4)2 PO43– Zn2+ zincphosphate lead (II)permanganate lead (II) permanganate MnO41– Pb2+ Pb(MnO4)2

20. Write names: (NH4)2S2O3 (NH4)2S2O3 ammonium thiosulfate AgBrO3 silverbromate AgBrO3 (NH4)3N (NH4)3N ammoniumnitride CrO42– uranium (VI)chromate U6+ U? U(CrO4)3 CrO42– U(CrO4)3 CrO42– Cr2(SO3)3 Cr2(SO3)3 Cr? chromium (III)sulfite Cr3+ SO32– Cr3+ Cr? SO32– SO32–

21. Binary Molecular Compounds(Covalent Compounds) Nonmetal + Nonmetal

22. Covalent Bonds …atoms share e– to get a full valence shell C Group 14 (4 v.e–) Group 17 (7 v.e–) F both need 8 v.e– for a full outer shell (octet rule) Lewis structure: a model of a covalent molecule that shows all of the valence e– 1. Two shared e– make a single covalent bond, four make a double bond, etc. 2. unshared pairs: pairs of unbonded valence e– 3. Each atom needs a full outer shell, i.e., 8 e–. Exception: H needs 2 e–

23. x x x x o o x x F H x x x x x x x x x o o x F H o o C C x x x x F F H F H H H F x x x x x x x x x o o C C x x x o o x x x x x x o o x x o o x x x x x x x x o o x x x H F x x x x x x x H F x x x x x x x carbon tetrafluoride (CF4) methane (CH4)

24. x x x x x x x x O x x x O x O = C = O x x x x x x x x x x x x x x O O x x x x x x x x x x x I x x x o o x o x o x x o o x I x o x x o No I I I No x x x x o o C C x x x x x x x o o x x o x o x x x x x o o x x I x x x x x nitrogen triiodide (NI3) carbon dioxide (CO2)

25. covalent compounds = molecular compounds -- have lower melting points than do ionic compounds (consist of two nonmetal elements) butter

26. What to do: 1 – 6 – 2 – 7 – 3 – 8 – 4 – 9 – 5 – 10 – Covalent Compounds -- contain two types of nonmetals nonmetals ** Key: FORGET CHARGES! Use Greek prefixes to indicate how many atoms of each element, but don’t use “mono” on first element. hexa mono di hepta tri octa tetra nona penta dec

27. EXAMPLES: CO2 carbon dioxide carbon monoxide CO N2O3 dinitrogen trioxide dinitrogen pentoxide N2O5 CCl4 carbon tetrachloride nitrogen triiodide NI3

28. Binary Compounds Containing Two Nonmetals To name these compounds, give the name of the less electronegative element first with the Greek prefix indicating the number of atoms of that element present, followed by the name of the more electronegative non- metal with the Greek prefix indicating the number of atoms of that element present and with its ending replaced by the suffix –ide. Prefixes you should know: Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca 1 2 3 4 5 6 7 8 9 10

29. Dihydrogen Monoxide: A Tale of Danger and Irresponsibility -- major component of acid rain -- found in all cancer cells -- inhalation can be deadly -- excessive ingestion results in acute physical symptoms: e.g., frequent urination, bloated sensation, profuse sweating -- often an industrial byproduct of chemical reactions; dumped wholesale into rivers and lakes

30. Binary CompoundsContaining Two Nonmetals (Type III Compounds) As2S3 • ________________ diarsenic trisulfide • ________________ sulfur dioxide • P2O5 ____________________ • ________________ carbon dioxide • N2O5 ____________________ • H2O ____________________ SO2 diphosphorus pentoxide CO2 dinitrogen pentoxide dihydrogen monoxide

31. Binary Molecular Compounds N2O dinitrogen monoxide N2O3dinitrogen trioxide N2O5dinitrogen pentoxide ICl iodine monochloride ICl3 iodine trichloride SO2 sulfur dioxide SO3 sulfur trioxide

32. Naming Binary Compounds Binary Compound? Yes Metal Present? No Yes Type III Use Greek Prefixes Does the metal form more than one cation? No Yes Type II Determine the charge of the cation; use a Roman numeral after the cation name. Type I Use the element name for the cation. Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 98

33. Naming Simple Chemical Compounds Ionic (metal and nonmetal) Covalent (2 nonmetals) Metal Nonmetal First nonmetal Second nonmetal Forms only one positive ion Forms more than one positive ion Single Negative Ion Polyatomic Ion Use the name of element Use element name followed by a Roman numeral to show the charge Use the name of the element, but end with ide Use the name of polyatomic ion (ate or Ite) Before element name use a prefix to match subscript Use a prefix before element name and end with ide

34. Prefixes – Binary Molecular Compounds Page 131 in text Greek Prefixes for Two Nonmetals Number Indicated Prefixes 1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca-

35. NH41+ …………… OH1- …………… CN1- ………….. ammonium hydroxide cyanide Polyatomic Ions - Memorize Eight “-ATE’s” PO43- …………… SO42- …………… CO32- ………….. ClO31- ………….. NO31- ………..…. phosphate sulfate carbonate chlorate nitrate phosphATE sulfATE carbonATE chlorATE nitrATE Exceptions:

36. Pattern to Memorizing Nomenclature XY “-ide” XYO4 XYO3 XYO2 XYO “per___-ate” “-ate” “-ite” “hypo___-ite” 1 more oxygen normal 1 less oxygen 2 less oxygen

37. Polyatomic Ion: a group of atoms that stay together and have a single, overall charge.

38. Common Polyatomic Ions(pg 123 in text) Names of Common Polyatomic Ions Ion Name Ion Name NH41+ ammonium CO3 2- carbonate NO21- nitrite HCO31- hydrogen carbonate NO31- nitrate (“bicarbonate” is a widely SO32- sulfite used common name) SO42- sulfate ClO 1- hypochlorite HSO41- hydrogen sulfate ClO21- chlorite (“bisulfate” is a widely ClO31- chlorate used common name) ClO41- perchlorate OH 1- hydroxide C2H3O22- acetate CN 1- cyanide MnO41- permanganate PO43- phosphate Cr2O72- dichromate HPO42- hydrogen phosphate CrO42- chromate H2PO41- dihydrogen phosphate O22- peroxide Print Version Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 100

39. Binary Hydrogen Compoundsof Nonmetals When Dissolved in Water (These compounds are commonly called acids.) The prefix hydro- is used to represent hydrogen, followed by the name of the nonmetal with its ending replaced by the suffix –ic and the word acid added. (See page 133 in text for common acids) Examples: *HCl HBr Hydrochloricacid Hydrobromicacid *The name of this compound would be hydrogen chloride if it was NOT dissolved in water.

40. Common Acids (pg 133 in text) • Hydrochloric HCL • Sulfuric H2SO4 • Nitric HNO3 • Acetic HC2H3O2 • Phosphoric H3PO4 • Carbonic H2CO3 • Hydrofluoric HF

41. shows the true number and type of atoms in a m’cule lowest-terms formula Empirical Formula and Molecular Formula CH2O C3H8 C2H5 C5H4 C12H22O11 C4H9

42. Traditional System of Nomenclature …used historically (and still some today) to name compounds w/multiple-charge cations 1. Use Latin root of cation. To use: 2. Use -ic ending for higher charge; -ous ending for lower charge. 3. Then say name of anion, as usual.

43. Element Latin root -ic -ous gold, Au aur- Au3+ Au1+ lead, Pb plumb- Pb4+ Pb2+ tin, Sn stann- Sn4+ Sn2+ copper, Cu cupr- Cu2+ Cu1+ iron, Fe ferr- Fe3+ Fe2+ Write formulas: Write names: P3– P3– Pb3P4 Pb3P4 cuproussulfide cuprous sulfide Pb4+ Pb? Pb? Pb4+ Pb4+ Pb? P3– P3– plumbicphosphide S2– Cu1+ Cu2S Pb3P2 Pb3P2 auricnitrite auric nitrite Pb? Pb2+ Pb? P3– Pb2+ Pb? P3– Pb2+ plumbousphosphide Au3+ NO21– Au(NO2)3 OH1– Sn(OH)4 Sn(OH)4 ferrousfluoride ferrous fluoride OH1– Sn? OH1– Sn4+ OH1– stannichydroxide F1– FeF2 Fe2+

44. Metallic Bonds In metals, valence shells of atoms overlap, so v.e– are free to travel between atoms through material. Not so in metals. In insulators (like wood), the v.e– are attached to particular atoms.

45. ductile conduct heat and electricity malleable Properties of Metals All due to free-moving v.e–.