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Chemistry: Bonding and Nomenclature

This PowerPoint presentation by Mr. John Bergmann explains the concepts of bonding and inorganic nomenclature. It covers topics such as ionic bonds, covalent bonds, metallic bonds, and other types of bonds. The presentation also includes examples and guidelines for writing formulas of ionic compounds and compounds containing polyatomic ions.

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Chemistry: Bonding and Nomenclature

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  1. lithium nitrate lead (II) sulfide Outline barium sulfide lithium nitride Chemistry sulfur dioxide lithium nitrite Unit 5: Bonding and Inorganic Nomenclature NO2 NaClO3 N2O4 Fe(ClO3)2 N2O5 Fe(ClO3)3 PowerPoint Presentation by Mr. John Bergmann

  2. 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 attraction Na1+ Cl Cl1– Na NaCl ionic compounds = salts KNO3 where NO31– is a polyatomic ion: a charged group of atoms that stay together

  3. 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 –

  4. Covalent Bonds …atoms share e– to get a full valence shell C (4 v.e–) 1s2 2s2 2p2 1s2 2s2 2p5 (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–

  5. 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)

  6. 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)

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

  8. 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.

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

  10. boiling H2O DNA • Other Types of Bonds dipole-dipole forces hydrogen bonds London dispersion forces ion-dipole forces These are much weaker than ionic, covalent, or metallic bonds, but very important in determining states of matter, boiling and melting points, and molecular shape (among other things).

  11. 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–

  12. 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

  13. 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

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

  15. i.e., “pulled off the Table” anions • Ionic Compounds (cation/anion combos) Single-Charge CationswithElemental Anions The single-charge cations are: groups 1, 2, 13, and Ag1+, Cd2+, and Zn2+

  16. 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

  17. 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

  18. i.e., “pulled off the Table” anions Multiple-Charge CationswithElemental Anions The multiple-charge cations are: Pb, Sn, and the transition elements (but – of course! – not Ag, Cd, or Zn)

  19. Cu Fe A. To name, 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–

  20. 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

  21. 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

  22. 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–

  23. 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

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

  25. 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

  26. Writing Chemical Names Use poly. ion sheet? Formula RN/GP/neither Name 1. Ni2 S3 RN no nickel (III) sulfide 2. N F3 GP no nitrogen trifluoride 3. Na BrO3 neither yes sodium bromate 4. S F6 GP no sulfur hexafluoride 5. Fe (NO3)3 RN yes iron (III) nitrate 6. Sr SO4 neither yes strontium sulfate

  27. Writing Chemical Formulas Use poly. ion sheet? Name Charges matter? Formula 1. copper (II) phosphide yes no Cu3P2 2. lithium phosphate yes yes Li3PO4 3. phosphorus triiodide no no PI3 4. zinc arsenate yes yes Zn3(AsO4)2 5. silver nitride yes no Ag3N 6. sulfur dibromide no no SBr2 7. dinitrogen pentasulfide no no N2S5 8. tin (IV) nitride yes no Sn3N4 9. rubidium nitrite yes yes RbNO2 no OF2 10. oxygen difluoride no yes Fe2(SO3)3 11. iron (III) sulfite yes yes (NH4)2O 12. ammonium oxide yes

  28. Traditional System of Nomenclature (i.e., NOT the Stock System) …used historically (and still some today) to name compounds w/multiple-charge cations Fe Cu Sn Au Pb 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.

  29. 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+

  30. Writing Chemical Formulas Use poly. ion sheet? Name Charges matter? Formula 1. copper (II) phosphide yes no Cu3P2 2. lithium phosphate yes yes Li3PO4 3. phosphorus triiodide no no PI3 4. zinc arsenate yes yes Zn3(AsO4)2 5. silver nitride yes no Ag3N 6. sulfur dibromide no no SBr2 7. dinitrogen pentasulfide no no N2S5 8. tin (IV) nitride yes no Sn3N4 9. rubidium nitrite yes yes RbNO2 no OF2 10. oxygen difluoride no yes Fe2(SO3)3 11. iron (III) sulfite yes yes (NH4)2O 12. ammonium oxide yes

  31. Writing Chemical Names Use poly. ion sheet? Formula RN/GP/neither Name 7. S O3 GP no sulfur trioxide 8. Sn Br4 neither no tin (IV) bromide 9. K3 PO4 neither yes potassium phosphate yes ammonium hydroxide 10. NH4 OH neither no carbon disulfide 11. C S2 GP no copper (I) fluoride 12. Cu F RN

  32. 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.

  33. 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+

  34. 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

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  37. Resources - Nomenclature Objectives Worksheet - binary cmpds: single charge cation Worksheet - binary compounds Worksheet - ions in chemical formulas Worksheet - ions in chemical compounds Worksheet - ionic cmpds: polyatomic ions w multiple-charge cation Worksheet - ionic formulas (binary, polyatomic, transition) Worksheet - empirical and molecular Worksheet - traditional system of nomenclature Worksheet - vocab (bonding) Worksheet - covalent binary cmpds: non-metal - non-metal Worksheet - ionic cmpds: polyatomic ions Activity - bondingpieces Worksheet - ionic binary cmpds: multiple charge cation Activity - molecular models Worksheet - errors in chemical formulas and nomenclature Activity - mole pattern Worksheet - oxidation numbers and ionic cmpds Textbook - questions Worksheet - names and formulas of cmpds Outline(general)

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