Chemical Names, Formulas and Bonding

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Chemical Names, Formulas and Bonding General Chem Re: 10/11 JG

Nonmetal-nonmetal Share electrons No ions- nothing to balance Name must tell elements and amounts Covalent Naming Rules: Divide formula in half Name first element Name second element change the ending to -IDE Use Greek prefixes to identify subscripts (Mono is optional for first element, required with second element) Common Prefixes Common -Ide Names 1-mono 6-hexa bromide iodide selenide 2-di 7-hepta hydride carbide 3-tri 8-octa nitride oxide 4-tetra 9-nona fluoride phosphide 5-penta 10-deca sulfide chloride Sample: CO (mono)carbon monoxide Name: 1. P 4 O 10 tetraphosphorus decaoxide 5. SO 3 2. N 2 H 4 dinitrogen tetrahydride 6. N 2 O 6 3. SF 6 7. NO 4. C 3 H 8 8. SO 2 Write formulas for the following: 9. chlorine dioxide ClO 2 10. dichlorine monoxide Cl 2 O 11. iodine tribromide 12. nitrogen trioxide 13. diphosphorus tetraoxide 14. carbon tetrafluoride

Covalent Formula Writing and Naming Write the correct name or formula for each of the following: 1. dinitrogen trioxide 21. P 2 O 5 2. sulfur trioxide 22. N 2 S 3 3. carbon dioxide 23. CCl 4 4. tetraphosphorus decasulfide 24. CO 3 5. sulfur hexafluoride 25. PBr 3 6. oxygen difluoride 26. CO 7. dinitrogen tetraoxide 27. SCl 2 8. sulfur dioxide 28. S 2 Cl 2 9. diarsenic trioxide 29. N 2 O 4 10. disulfur dichloride 30. ClF 3 11. dinitrogen pentoxide 31. SiCl 4 12. sulfur diiodide 32. SO 4 13. nitrogen dioxide 33. N 2 O 5 14. iodine monochloride 34. Cl 2 O 15. silicon tetrabromide 35. NO 16. selenium difluoride 36. NO 2 17. carbon disulfide 37. ClO 6 18. dinitrogen trisulfide 38. N 2 Cl 4 19. silicon disulfide 39. N 2 O 20. diarsenic trisulfide 40. PCl 5

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NOTES:

ELECTRON DOT FORMULA WORKSHEET Background: Covalent bonding is formed between nonmetals and nonmetals. A covalent bond is a shared pair of electrons. Atoms share electrons to obtain an electron configuration of a noble gas, this allows the atoms to become more stable. Molecules can be represented by means of diagrams in which VALENCE electrons are shown as dots around the chemical symbols of the atoms and bonds are represented as lines. (This is especially useful when diagramming covalent bonds.) Historical Note: The dot formulas are sometimes referred to as Lewis Dot Structures after the chemist who first introduced them in 1916---G.N. Lewis. Rules: 1. Determine the total number of valence electrons. 2. Draw a skeleton structure: Aim for symmetry. Be sure to include all elements in the formula!! Do not string out oxygens. Do not make boxes. 3. Each bond - represents 2 electrons 4. Place electrons as dots around atoms to achieve stable octets (8) and stable duets (2) for hydrogen. Exceptions: 4 for Be and 6 for B 6. Be sure the total number of electrons in the diagram equals the original number of total valence electrons. Examples: 1. Nitrogen = N = group 5 (periodic table) = 5 valence electrons Electron Dot Formula 2. Cl 2 = group 7(periodic table) 2 atoms Cl x 7 valence electrons = 14 total valence electrons Electron Dot Formula 3. H 2 O H = group 1 = 1 valence electron O= group 6 = 6 valence electrons H = 2 atoms H X 1 valence electron = 2 valence electrons O = 1 atom O X 6 valence electron = + 6 valence electrons 8 total valence electrons Electron Dot Formula

1. Draw the electron dot structures for the following atoms. a) F b) Cl c) P d) O e) C f) N g) H h) Br 2. 1. Name the compound 2.draw the electron dot structures 3.state the geometric shape for the following molecules. a) Br 2 name & shape b) HCl name & shape c)ch 4 name & shape d) NH 3 name & shape e) H 2 S name & shape f) SiF 4 name & shape g) PF 3 name & shape h)c 2 H 6 name & shape i)c 2 Cl 2 H 4 j) N 2 H 4 name k) C 5 H 12 name l) Cl 2 O name & shape

The Saga Continues Single Bonds: one pair of electrons shared between bonding atoms Cl 2 14 total valence electrons Double Bonds: two pairs of electrons shared between bonding atoms O 2 12 total valence electrons Triple Bonds: Three pairs of electrons shared between bonding atoms N 2 10 total valence electrons All atoms still need to achieve a stable octet (or duet for H). Follow all bonding rules.

Draw electron dot structures for the following compounds. 1. CO 2 name 2. SiS 2 name 3. C 2 H 4 name 4. H 2 CO 5. H 2 C 2 O 2 6. NH 4 +1 shape 7. N 2 O 2 name 8. HCN name 9. C 2 H 2 name 10. C 2 H 5 OH 11. C 2 H 3 OH 12. C 2 N 2 name 13. OH -1 14. CN -1

More Dot Structures 1. CF 4 shape, name 2. CH 2 Cl 2 shape 3. PF 3 shape, name 4. H 2 S shape, name 5. F 2 shape, name 6. N 2 H 4 name 7. CH 3 COOH 8. CH 3 NH 2

9. C 3 H 4 name 10. CCl 2 O 11. CH 3 CN 12. P 2 H 2 name 13. CS 2 name 14. N 2 O 2 name 15. C 2 H 3 O 16. SI 2 name, shape

Ionic Compounds There are four places to find the charge of an ion: 1. The main block elements 2. The Roman numerals 3. The polyatomic ion sheet 4. Determine the charge from the other ions in the compound. All compounds have a net charge of zero. How to Write Ionic Formulas Ex: Determine the chemical formula for magnesium oxide. 1. Always write the cation first then the anion. To find the ionic charge look at your main block elements, the Roman numerals, and/or your polyatomic ion sheet. Mg +2 O -2 2.Write the compound using subscripts so that the net charge is equal to ZERO MgO Ex : Determine the chemical formula for ammonium carbonate 1. Always write the cation first then the anion. To find the ionic charge look at your mainblock elements, the Roman numerals, and/or your polyatomic ion sheet. (NH 4 ) +1 (CO 3 ) -2 2.NEVER CHANGE THE POLYATOMIC ION.For multiple polyatomic ions use ( ). The net charge of the compound must equal zero. (NH 4 ) 2 CO 3

How to Name Ionic Compounds. Ex: Write the chemical name for CaCl 2 1. Write the cation first calcium 2. If the cation is a transition metal, tin(sn), lead(pb), animony(sb), or bismuth(bi). Write the charge as a Roman numeral. does not apply 3. Write the anion. If the ion is a nonmetal element change the ending to -ide. calcium chloride Ex: Write the chemical name for PbO 1. Write the cation first lead 2.If the cation is a transition metal, tin(sn), lead(pb), animony(sb), or bismuth(bi). Write the charge as a Roman numeral. lead(ii) 3. Write the anion. If the ion is a nonmetal element change the ending to -ide. lead(ii) oxide Ex: Write the chemical name for (NH 4 ) 2 SO 4 1. Write the cation first(taken form the polyatomic ion sheet) ammonium 2. If the cation is a transition metal, tin(sn), or lead(pb) Write the charge as a Roman numeral. does not apply 3. Write the anion. If the ion is a nonmetal element change the ending to -ide. ammonium sulfate ex: MgO magnesium oxide Fe 2 (CO 3 ) 3 iron(iii) carbonate AuN gold(iii)nitride AgC 2 H 3 O 2 silver acetate

NOTES:

NOTES:

Ionic Formula Writing 1. Al +3 Br -1 21. lead(ii) chloride 2. Al +3 (C 2 H 3 O 2 ) -1 22. silver nitrate 3. Ba +2 S -2 23. mercury(ii) iodide 4. (NH 4 ) +1 (NO 3 ) -1 24. strontium nitrite 5. Ca +2 I -1 25. barium sulfate 6. Cr +3 F -1 26. tin(iv) sulfide 7. (NH 4 ) +1 (OH) -1 27. copper(ii) chlorate 8. Cu +1 Cl -1 28. iron(ii) oxide 9. H +1 S -2 29. lead(ii) bromide 10. K +1 (OH) -1 30. iron(iii) phosphate 11. H +1 (CO 3 ) -2 31. lead(ii) chromate 12. Hg +1 (C 2 H 3 O 2 ) -1 32. magnesium fluoride 13. Cu +1 S -2 33. hydrogen bromide 14. Al +3 O -2 34. magnesium sulfide 15. Sn +2 O -2 35. lithium iodide 16. Ag +1 Cl -1 36. silver carbonate 17. Ca +2 (PO 4 ) -3 37. zinc sulfite 18. Ba +2 (Cr 2 O 7 ) -2 38. iron(ii) chlorate 19. Bi +3 (AsO 4 ) -3 39. barium oxide 20. Na +1 (ClO) -1 40. ammonium phospate

Ionic Naming 1. CaCl 2 21. PbCl 2 2. Al 2 O 3 22.Sr(NO 3 ) 2 3. Na 2 S 23. AuI 3 4. FeS 24. CuO 5. NH 4 NO 2 25. HgBr 6. Ba 3 N 2 26. BeSO 4 7. AlF 3 27. Co 3 N 8. Ca 3 P 2 28. AuI 9. K 2 CO 3 29. W 2 O 3 10. KI 30. Co(OH) 2 11. Li 2 C 2 O 4 31. SnF 4 12. SrBr 2 32. AgCl 13. FeCl 3 33. CuO 14. AgNO 3 34.Al 2 (CO 3 ) 3 15. MgSO 3 35. Cu 2 O 16. CdI 2 36. AlN 17. BaSO 4 37. Pb(CO 3 ) 2 18. Fe 2 S 3 38. K 3 N 19. SnO 39. Au 3 PO 4 20. Be(C 2 H 3 O 2 ) 2 40. NaCl

Ionic Roman # & Polyatomics Write the following compounds: 1. beryllium nitrate 2. manganese (II)iodide 3. chromium (III) sulfide 4. lithium chromate 5. ammonium chloride 6. copper (I) phosphide 7. sodium phosphate 8. iron (III) hydroxide 9. zinc sulfite 10. gold (II) acetate Name the following compounds: 1. FeCl 2 2. CrO 3. Mg(OH) 2 4. Ca(NO 2 ) 2 5. NiBr 2 6. Cu 2 SO 4 7. HgCO 3 8. K 2 CO 3 9. (NH 4 ) 2 O 10. SnI 4

Ionic Naming Provide the formula for the following: 1. potassium phosphate 6. Ca 3 N 2 2. iron (III) chloride 7. Li 2 SO 4 3. mercury (I) oxide 8. Ni(CN) 2 4. aluminum carbonate 9. SnF 4 5. sodium chromate 10. Sr(NO 3 ) 2 Each of the following name-formula pairs is incorrect. Determine what is wrong with the pair, write a sentence explaining what is wrong, and then provide the correct name or formula as needed. 11. PbCl 2 lead chloride 12. CuO copper (I) oxide 13. Co 3 (PO 4 ) 2 carbonate phosphate 14. CdI 2 cadmium (II) iodide 15. NH 4 NO 2 nitrogen tetrahydride mono nitrogen dioxide 16. copper (II) chlorate Cu 2 ClO 3 17. lithium iodide LiIO 3 18. barium oxide BaO 2 19. lead (III) sulfide Pb 2 (SO 4 ) 2 20. hydrogen bromide H 2 Br

Mixed Practice Ionic vs. Covalent Compounds Is the compound ionic or covalent? Name the following compounds: 1. CO 2. BaI 2 3. CrF 3 4. CaCrO 4 5. Cu(OH) 2 6. N 2 O 3 7. SrO 8. NH 4 Br 9. PF 3 10. CoCl 3 11. Al 2 O 3 12. Mg(NO 3 ) 2 13. NaCl 14. K 2 SO 4 15. P 2 O 3

Is the compound covalent or ionic? Write the correct formula. 1. aluminum chloride 2. calcium oxide 3. lithium hydroxide 4. diphosphorous tetraoxide 5. cobalt (II) sulfate 6. ammonium iodide 7. sodium phosphate 8. iron (III) oxide 9. sulfur trioxide 10. nickel (II) acetate 11. carbon tetrachloride 12. potassium sulfide 13. dinitrogen pentoxide 14. magnesium nitride 15. barium phosphate

Mixed practice Mixed Practice Writing and Naming Name the following compounds: Write the following formulas: 1. C 2 H 6 21. copper (II) nitrate 2. CaBr 2 22. dinitrogen trioxide 3. LiMnO 4 23. lead (IV) chloride 4. H 2 O 24. aluminum hydroxide 5. HF 25. ammonium acetate 6. P 4 O 10 26. silicon disulfide 7. Al 2 O 3 27. sulfur dioxide 8. Na 2 SO 3 28. copper (I) oxide 9. BaO 29. diphosphorus pentasulfide 10. H 3 PO 4 30. carbon tetrafluoride 11. Na 2 O 31. zinc permanganate 12. Hg(OH) 2 32. tin (II) phosphate 13. SO 3 33. iron (III) carbonate 14. NI 3 34. silver phosphide 15. Cu 2 CO 3 35. silicon tetraiodide 16. NO 36. strontium fluoride 17. P 2 S 5 37. cadmium hydroxide 18. Co 3 PO 4 38. iron (III) chromate 19. CS 2 39. ammonium sulfide 20. SF 2 40. lithium oxide

Electronegativity Values

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