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Unit 5: Bonding and Inorganic Nomenclature Chemistry NaClO 3 Fe(ClO 3 ) 2 lithium nitrate lithium nitride lithium nitrite lead (II) sulfide barium sulfide.

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Presentation on theme: "Unit 5: Bonding and Inorganic Nomenclature Chemistry NaClO 3 Fe(ClO 3 ) 2 lithium nitrate lithium nitride lithium nitrite lead (II) sulfide barium sulfide."— Presentation transcript:

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2 Unit 5: Bonding and Inorganic Nomenclature Chemistry NaClO 3 Fe(ClO 3 ) 2 lithium nitrate lithium nitride lithium nitrite lead (II) sulfide barium sulfide sulfur dioxide Fe(ClO 3 ) 3 NO 2 N 2 O 4 N 2 O 5

3 Bonding Types 1.Ionic Bonding with ions (+/- charges) atoms gaining/losing e- M + NM 2.Covalent Bonding atoms sharing e- NM + NM 3.Metallic Bonding metals share e- freely “sea of e-” good conductors

4 Chemical Bonding Ionic Bonds: atoms give up or gain e – and are attracted to each other by coulombic attraction Na Na + Cl Cl – loses e – gains e – Na + + Cl – NaCl K + + NO 3 – KNO 3 ionic compounds = salts where NO 3 – is a polyatomic ion: a charged group of atoms that stay together ionic bonds: M + NM cation + anion

5 Common Polyatomic Ions Names of Common Polyatomic Ions Ion Name Ion Name NH 4 + ammoniumCO 3 2- carbonate *NO 2 - *nitriteHCO 3 - bicarbonate NO 3 - nitrate*IO 3 - *iodate *SO 3 2- *sulfite*IO 4 - *periodate SO 4 2- sulfate *ClO - *hypochlorite HSO 4 - hydrogen sulfate*ClO 2 - *chlorite OH - hydroxide ClO 3 - chlorate CN - cyanide *ClO 4 - *perchlorate C 2 H 3 O 2 - acetate *BrO 3 - *bromate MnO 4 - permanganateC 2 O 4 2- oxalate PO 4 3- phosphateCr 2 O 7 2- dichromate *PO 3 3- *phosphiteCrO 4 2- chromate H 2 PO 4 - dihydrogen phosphateO 2 2- peroxide Zumdahl, Zumdahl, DeCoste, World of Chemistry  2002, page 100 Memorize the BOLD ions * = you will also be responsible for knowing these

6 Polyatomic Ion Trends *Charges NEVER change between different forms “Normal” “–ate” form BrO 3 - bromate ClO 3 - chlorate IO 3 - iodate NO 3 - nitrate CO 3 2- carbonate SO 4 2- sulfate PO 4 3- phosphate BrO 2 - ClO 2 - IO 2 - NO 2 - CO 2 2- SO 3 2- PO 3 3- BrO - ClO - IO - BrO 4 - ClO 4 - IO oxygen “-ite” form -2 oxygens “hypo___ite” +1 oxygen “Per____ate” bromite chlorite iodite nitrite sulfite phosphite hypobromite hypochlorite hypoiodite perbromate perchlorate periodate carbonite

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

8 Writing Formulas of Ionic Compounds chemical formula: To write an ionic compound’s formula, we need: 1. the two types of ions 2. the charge on each ion Na + and F – Ba 2+ and O 2– Na + and O 2– Ba 2+ and F – shows types of atoms and how many of each NaF BaO Na 2 O BaF 2 (i.e., cations and anions) has neutral charge;

9 O 2- K+K+ K+K+ Mg 2+ Br - K Br potassium atom bromine atom e-e- e-e- Br - K+K+ potassium ion bromide ion potassium bromide KBr MgBr 2 K2OK2O magnesium bromide potassium oxide Notice that the pink pieces are cations (metals) and the blue are anions (non-metals) 1 Mg 2+ 2 Br -

10 Chemical Bonding Activity Examples Na + Pb 4+ OH - Mg 2+ OH - N 3- Pb 4+ N 3- Pb 4+ N 3- Pb 4+ N 3- Pb 4+ N 3- Pb 3 N 4 1 Mg 2+ 2 OH - Mg OH 2 1 Na + 1 OH - NaOH

11 charge on cation / anion “becomes” subscript of anion / cation ** Warning: Al 3+ and O 2– Ba 2+ and S 2– In 3+ and Br 1– Reduce to lowest terms Al O Ba S In Br Al 2 O 3 BaS InBr 3 criss-cross rule:

12 Writing Formulas w/Polyatomic Ions Parentheses are required only when you need more than one “bunch” of a particular polyatomic ion Ba 2+ and SO 4 2– Mg 2+ and NO 2 – NH 4 + and ClO 3 – Sn 4+ and SO 4 2– Fe 3+ and Cr 2 O 7 2– NH 4 + and N 3– BaSO 4 Mg(NO 2 ) 2 NH 4 ClO 3 Sn(SO 4 ) 2 Fe 2 (Cr 2 O 7 ) 3 (NH 4 ) 3 N

13 ide Calcium hydrox ide Ca 2+ OH - CaOH 2 Ca(OH) 2 Ca - O H H HO - Ca - OH vs. The Importance of Parentheses The formulas imply two totally different compounds!

14 1+ Charges Reminder! Group 1: Group 2: Group 3: Group 5: Group 6: Group 7: Group 8: – 2– 1– – 2– 1– 0

15 Inorganic Nomenclature potassium nitrate KNO 3 sodium hydroxide NaOH dinitrogen monoxide N2ON2O copper (II) sulfate CuSO 4

16 Nomenclature - Humor “Ferrous Wheel” Fe = iron (Latin = ferrum) Fe 2+ = lower oxidation state = ferrous Fe 3+ = higher oxidation state = ferric BaNa 2 “BaNaNa” Fe 2+ What weapon can you make from the elements nickel, potassium and iron? A KNiFe

17 Teacher: What is the formula for water? Student: H, I, J, K, L, M, N, O Teacher: That’s not what I taught you. Student: But you said the formula for water was…H to O. mis “Little Johnny took a drink, Now he shall drink no more. For what he thought was H 2 O, Was H 2 SO 4.” Under aged Pb walks into a bar and the bartender turns to the gold Bouncer and says, “Au, get the lead out!” "H-O-H"?! WHAT'S THAT SPELL?! WATER?

18 “Perhaps one of you gentlemen would mind telling me just what is outside the window that you find so attractive..?” Image courtesy NearingZero.net

19 Ionic Compounds (cation/anion combos) Fixed-Charge Cations with Elemental Anions The fixed-charge cations are: groups 1, 2, 13, Ag + and Zn 2+ i.e., “pulled off the Table” anions – 2– 1–

20 Fixed-Charge Exceptions Start with Al Go backwards down the stairs Decrease the charge after each stair Al 13 Zn 30 Ag

21 Li 3 H1H1 He 2 C6C6 N7N7 O8O8 F9F9 Ne 10 Na 11 B5B5 Be 4 H1H1 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 Cs 55 Ba 56 Hf 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 Mg 12 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm 100 Md 101 No 102 Lr 103 La 57 Ac   Fixed-charge cations Variable-charge cations Elemental anions

22 A. To name, given the formula: 2. Use name of anion (it has the ending “ide”) 1. Use name of cation NaF BaO Na 2 O BaF 2 sodium fluoride barium oxide sodium oxide barium fluoride Na Ba – 2– 1– 3+

23 1. Write symbols for the two types of ions 2. Balance charges to write formula silver sulfide zinc phosphide calcium iodide B. To write formula, given the name: Ag + S 2– Ag 2 S Zn 2+ P 3– Zn 3 P 2 I – Ca 2+ CaI 2 Ca Ag Zn – 2– 1– 3+

24 Variable-Charge Cations with Elemental Anions The variable-charge cations are: i.e., “pulled off the Table” anions Pb, Sn, and the transition metals (but – of course! – not Ag or Zn)

25 iron oxide A. To name, given the formula: 1.Figure out charge on cation. 2. Write name of cation. 3. Write Roman numerals in ( ) to show cation’s charge. 4. Write name of anion. FeO Fe 2 O 3 CuBr CuBr 2 iron oxide Cu Fe Stock System of nomenclature Fe ? O 2– iron (II) oxide Fe ? O 2– iron (III) oxide copper bromide copper bromide Cu ? Br – copper (I) bromide Cu 2+ Br – copper (II) bromide Fe ? Br – O 2– O 2– Fe 2+ Fe 3+ Cu + Cu ? - 6

26 Roman Numeral Review Greek Number Roman Numeral 1I 2II 3III 4IV 5V 6VI 7VII 8VIII 9IX 10X NumberRoman Numeral 50L 100C 500D 1000M

27 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 tin (IV) oxide tin (II) oxide Co Sn Co 3+ Cl – CoCl 3 Sn 4+ O 2– O 2– Sn 2+ SnO 2 SnO

28 Ionic Nomenclature Practice 1.sodium hydroxide 2.HgSO 4 3. lead (II) phosphate 4. (NH 4 ) 2 S 5. aluminum chlorate 6. Cu 2 CO 3 7.manganese (IV) oxide 8.MnSO 4 9. iron (III) oxide 10. Mg(NO 3 ) calcium sulfide 12. K 2 O 13. magnesium chloride 14. Cr 2 O gold (III) bromide 16. Zn(NO 2 ) 2 NaOH mercury (II) sulfate Pb 3 (PO 4 ) 2 ammonium sulfide Al(ClO 3 ) 3 copper (I) carbonate MnO 2 manganese (II) sulfate Fe 2 O 3 magnesium nitrate CaS potassium oxide MgCl 2 chromium (III) oxide AuBr 3 zinc nitrite

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

30 ElementLatin root-ic-ous gold, Auaur-Au 3+ Au + lead, Pbplumb-Pb 4+ Pb 2+ tin, Snstann-Sn 4+ Sn 2+ copper, Cucupr-Cu 2+ Cu + iron, Feferr-Fe 3+ Fe 2+ Write formulas: cuprous sulfide auric nitride ferrous fluoride Write names: Pb 3 P 4 Pb 3 P 2 SnCl 4 Cu + S 2– Cu 2 S Au 3+ N 3- AuN Fe 2+ F–F– FeF 2 cuprous sulfide auric ferrous fluoride Pb 3 P 4 Pb 3 P 2 Sn P 3– Pb ? Pb ? P 3– Pb 4+ plumbic phosphide Pb 2+ plumbous phosphide Cl – Sn 4+ Sn ? stannic chloride

31 Compounds Containing Polyatomic Ions Insert name of ion where it should go in the compound’s name. Write formulas: iron (III) nitrite ammonium phosphide ammonium chlorate zinc phosphate lead (II) permanganate iron (III) nitrite ammonium phosphide ammonium chlorate zinc phosphate lead (II) permanganate Fe 3+ NO 2 – Fe(NO 2 ) 3 NH 4 + NH 4 + P 3– (NH 4 ) 3 P ClO 3 – NH 4 ClO 3 Zn 2+ PO 4 3– Zn 3 (PO 4 ) 2 Pb 2+ MnO 4 – Pb(MnO 4 ) 2

32 Write names: (NH 4 ) 2 S 2 O 3 AgBrO 3 (NH 4 ) 3 N U(CrO 4 ) 3 Cr 2 (SO 3 ) 3 (NH 4 ) 2 S 2 O 3 AgBrO 3 (NH 4 ) 3 N U(CrO 4 ) 3 Cr 2 (SO 3 ) 3 ammonium thiosulfate silver bromate ammonium nitride U ? CrO 4 2– CrO 4 2– CrO 4 2– uranium (VI) chromate Cr ? Cr ? Cr 3+ SO 3 2– SO 3 2– SO 3 2– chromium (III) sulfite U 6+

33 4. NaClO 3 5. Fe(ClO 3 ) 2 1. lithium nitrate 2. lithium nitride 3. lithium nitrite 7. lead(II) sulfide 8. barium sulfide 6. Fe(ClO 3 ) 3 9. Never show charges in a compound’s formula. (T/F) 10. When writing names with Group 9 cations, you need to use Roman numerals. (T/F) 11. When using an anion off the polyatomic ion sheet, change name’s ending to “-ide.” (T/F) 12. A Roman numeral indicates the charge on the anion. (T/F) Self-Test Quiz

34 4. NaClO 3 5. Fe(ClO 3 ) 2 1. lithium nitrate 2. lithium nitride 3. lithium nitrite 7. lead(II) sulfide 8. barium sulfide 6. Fe(ClO 3 ) 3 Self-Test Quiz Answers sodium chlorate iron(II) chlorate LiNO 3 Li 3 N LiNO 2 PbS BaS iron(III) chlorate

35 9. Never show charges in a compound’s formula. 10. When writing names with Group 9 cations, you need to use Roman numerals. 11. When using an anion off the polyatomic ion sheet, change the name’s ending to “-ide.” 12. A Roman numeral indicates the charge on the anion. Self-Test Quiz Answers T T F F

36 Covalent Bonds (2 nonmetals) …atoms share e– to get a full valence shell C1s 2 2s 2 2p 2 F1s 2 2s 2 2p 5 Both need 8 valence e - for a full outer shell… otherwise known as the octet rule o 4 valence e- 7 valence e- o x o o C x x x x x x F

37 Draw the Lewis dot structure for the following elements: Si O P B Ar Br 1s 2 2s 2 2p 6 3s 2 3p 3 1s 2 2s 2 2p 4 1s 2 2s 2 2p 1 1s 2 2s 2 2p 6 3s 2 3p 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 1s 2 2s 2 2p 6 3s 2 3p 2 4 valence e- 6 valence e- 5 valence e- 3 valence e- 8 valence e- 7 valence e-

38 Notice any trends…?

39 Drawing Lewis Structures Lewis structure: 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 – a model of a covalent molecule that shows all of the valence e –

40 C F F F F Let’s bond two F atoms together… Each F has 7 v.e. and each needs 1 more e- F F F F Now let’s bond C and F atoms together… C F F F F carbon tetrafluoride (CF 4 ) F2F2

41 And now, a video break…

42 oo o o N o nitrogen triiodide (NI 3 ) carbon dioxide (CO 2 ) x x x x xx I x x xx x xx I x x xx x xx I x x xx xx I x x x xx x xx I x x xx x xx I x oo o o N oN o o C o o ox xx x x O x x xx x x O x x xx x x O x o C o o o O = C = O x x x xx x x O x

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

44 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

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

46 EXAMPLES: carbon dioxide CO dinitrogen trioxide N2O5N2O5 carbon tetrachloride NI 3 CO 2 carbon monoxide N 2 O 3 dinitrogen pentoxide CCl 4 nitrogen triiodide

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

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

49 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). Other Types of Forces/Attractions dipole-dipole forces hydrogen bonds London dispersion forces ion-dipole forces DNA boiling H 2 O

50 Empirical Formula and Molecular Formula Compound Molecular Formula Empirical Formula glucoseC 6 H 12 O 6 propaneC3H8C3H8 butaneC 4 H 10 naphthaleneC 10 H 8 sucroseC 12 H 22 O 11 octaneC 8 H 18 lowest-terms formula shows the true number and type of atoms in a m’cule CH 2 O C3H8C3H8 C2H5C2H5 C5H4C5H4 C 12 H 22 O 11 C4H9C4H9

51 Nomenclature Review Flow Chart

52 Metal + Nonmetal? Formula  Name? Ionic Covalent Two Nonmetals? Variable Fixed Use Prefixes! *Mono* Hexa Di Hepta Tri Octa Tetra Nona Penta Deca 1.Write name of cation (metal) 2.Determine the charge on the metal by balancing the (-) charge from the anion 3.Write the charge of the metal in Roman Numerals and put in parentheses 4.Write name of anion (Individual anions need –ide ending!) Steps 1 & 4 ONLY d,f-block Pb,Sn Columns 1, 2, 13 Ag +, Zn 2+ (Including NH 4 + ) Metal Type? Add –ide to 2 nd element

53 Name  Formula? No Prefixes? Prefixes? 1.Determine the ions present and the charge on each (Roman Numeral = cation charge, otherwise use PT) 2.Balance formula (criss-cross) 3.Reduce subscripts (if needed) 1.FORGET CHARGES!!! 2.Use prefixes to determine subscripts 3.Do NOT reduce subscripts! Ionic Covalent

54 Two nonmetalsVariable-charge cationFixed-charge Roman numeral Polyatomic ions OK Roman numeral for name only Polyatomic ions Greek prefixes Charge Criss- Cross Rule Roman numeral OK Where would you file this? VCrO 4 BaO CBr 4 Nb(ClO 4 ) 5 SCl 2 Rb 2 SO 4 dinitrogen pentoxide platinum (IV) iodate ammonium chlorate potassium iodide nitrogen trichloride manganese (V) sulfide vanadium (II) chromate VCrO 4 N2O5N2O5 dinitrogen pentoxide barium oxide BaO Pt(IO 3 ) 4 platinum (IV) iodate carbon tetrabromide CBr 4 NH 4 ClO 3 ammonium chlorate niobium (V) perchlorate Nb(ClO 4 ) 5 KI potassium iodide sulfur dichloride SCl 2 NCl 3 nitrogen trichloride rubidium sulfate Rb 2 SO 4 Mn 2 S 5 manganese (V) sulfide Covalent Ionic Compounds Don’t know the charge from PT Know the charge from PT

55 fluoride sulfide bromide diphosphide iodide tetrachloride oxide phosphide iridium (III) calcium titanium (IV) hydrochloric acid barium trinitrogen hydrofluoric acid zinc nitrogen gold (III) sodium Ir Ca Ti H Ba N 3 H Zn N Au Na F 3 S S 2 Cl(aq) Br 2 P 2 F(aq) I 2 Cl 4 2 O 3 3 P Ionic/variable Ionic/fixed Ionic/variable Acid Ionic/fixed Covalent Acid Ionic/fixed Covalent Ionic/variable Ionic/fixed Overall Nomenclature Practice

56 dichromate hydroxide acid acetate acid sulfate cyanide nitrite chlorate phosphate acid iridium (III) calcium nitric platinum (II) bromous strontium potassium zinc manganese (IV) gold (III) sulfurous (Cr 2 O 7 ) 3 (OH) 2 NO 3 (aq) (CH 3 COO) 2 BrO 2 (aq) SO 4 CN (NO 2 ) 2 (ClO 3 ) 4 PO 4 SO 3 (aq) Ir 2 Ca H Pt H Sr K Zn Mn Au H2H2 Ionic/variable Ionic/fixed Acid Ionic/variable Acid Ionic/fixed Ionic/variable Acid Ionic Nomenclature Practice

57 Write the total number of atoms that make up each compound. Write the compound formed by the following ions: 1) Al 3+ S 2- 2) Mg 2+ PO 4 3- When a formula is given…write the proper name. When a name is given…write the proper formula. 3) BaO 4) lithium bromide 5) Ni 2 S 3 6) triphosphorus heptoxide 7) N 2 O 5 8) molybdenum (VI) nitride 9) trinitrotoluene (TNT)… CH 3 C 6 H 2 (NO 2 ) 3 10) phosphoric acid H 3 PO 4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb 2+ or Pb 4+ )

58 Write the total number of atoms that make up each compound. Write the compound formed by the following ions: 1) Al 3+ S 2- 2) Mg 2+ PO 4 3- When a formula is given…write the proper name. When a name is given…write the proper formula. 3) BaO 4) lithium bromide 5) Ni 2 S 3 6) triphosphorus heptoxide 7) N 2 O 5 8) molybdenum (VI) nitride 9) trinitrotoluene (TNT)… CH 3 C 6 H 2 (NO 2 ) 3 10) phosphoric acid H 3 PO 4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb 2+ or Pb 4+ ) POP QUIZ

59 Write the total number of atoms that make up each compound. Write the compound formed by the following ions: 1) Al 3+ S 2- 2) Mg 2+ PO 4 3- When a formula is given…write the proper name. When a name is given…write the proper formula. 3) BaO 4) lithium bromide 5) Ni 2 S 3 6) triphosphorus heptoxide 7) N 2 O 5 8) molybdenum (VI) nitride 9) trinitrotoluene (TNT)… CH 3 C 6 H 2 (NO 2 ) 3 10) phosphoric acid H 3 PO 4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb 2+ or Pb 4+ ) Answer Key Al 2 S 3 Mg 3 (PO 4 ) 2 barium oxide nickel (III) sulfide LiBr dinitrogen pentoxide MoN PbI 4 P3O7P3O7

60 4. S F 6 5. Fe (NO 3 ) 3 1. Ni 2 S 3 2. N F 3 3. Na BrO 3 6. Sr SO 4 Writing Chemical Names FormulaRN/GP/neither Use poly. ion sheet? Name GP RN GP neither no yes no yes sulfur hexafluoride iron (III) nitrate nickel (III) sulfide nitrogen trifluoride sodium bromate strontium sulfate

61 10. oxygen difluoride 4. zinc arsenate 5. silver nitride 1. copper (II) phosphide 2. lithium phosphate 3. phosphorus triiodide 7. dinitrogen pentasulfide 8. tin (IV) nitride 6. sulfur dibromide Writing Chemical Formulas 9. rubidium nitrite 11. iron (III) sulfite 12. ammonium oxide NameCharges matter? Use poly. ion sheet? Formula yes no yes no yes no yes no yes no yes no Zn 3 (AsO 4 ) 2 Ag 3 N Cu 3 P 2 Li 3 PO 4 PI 3 N2S5N2S5 Sn 3 N 4 SBr 2 RbNO 2 Fe 2 (SO 3 ) 3 (NH 4 ) 2 O OF 2

62 7. S O 3 8. Sn Br 4 Writing Chemical Names 9. K 3 PO C S Cu F 10. NH 4 OH FormulaRN/GP/neither Use poly. ion sheet? Name GP neither GP RN neither no yes no yes sulfur trioxide tin (IV) bromide potassium phosphate carbon disulfide copper (I) fluoride ammonium hydroxideyes

63 10. oxygen difluoride 4. zinc arsenate 5. silver nitride 1. copper (II) phosphide 2. lithium phosphate 3. phosphorus triiodide 7. dinitrogen pentasulfide 8. tin (IV) nitride 6. sulfur dibromide Writing Chemical Formulas 9. rubidium nitrite 11. iron (III) sulfite 12. ammonium oxide NameCharges matter? Use poly. ion sheet? Formula yes no yes no yes no yes no yes no yes no Zn 3 (AsO 4 ) 2 Ag 3 N Cu 3 P 2 Li 3 PO 4 PI 3 N2S5N2S5 Sn 3 N 4 SBr 2 RbNO 2 Fe 2 (SO 3 ) 3 (NH 4 ) 2 O OF 2

64 10. oxygen difluoride 4. zinc arsenate 5. silver nitride 1. copper (II) phosphide 2. lithium phosphate 3. phosphorus triiodide 7. dinitrogen pentasulfide 8. tin (IV) nitride 6. sulfur dibromide Writing Chemical Formulas 9. rubidium nitrite 11. iron (III) sulfite 12. ammonium oxide NameCharges matter? Use poly. ion sheet? Formula yes no yes no yes no yes no yes no yes no Zn 3 (AsO 4 ) 2 Ag 3 N Cu 3 P 2 Li 3 PO 4 PI 3 N2S5N2S5 Sn 3 N 4 SBr 2 RbNO 2 Fe 2 (SO 3 ) 3 (NH 4 ) 2 O OF 2

65 4. S F 6 5. Fe (NO 3 ) 3 1. Ni 2 S 3 2. N F 3 3. Na BrO 3 7. S O 3 8. Sn Br 4 6. Sr SO 4 Writing Chemical Names 9. K 3 PO C S Cu F 10. NH 4 OH FormulaRN/GP/neither Use poly. ion sheet? Name GP RN GP neither GP neither GP RN neither no yes no yes no yes no yes sulfur hexafluoride iron (III) nitrate nickel (III) sulfide nitrogen trifluoride sodium bromate sulfur trioxide tin (IV) bromide strontium sulfate potassium phosphate carbon disulfide copper (I) fluoride ammonium hydroxide

66 10. oxygen difluoride 4. zinc arsenate 5. silver nitride 1. copper (II) phosphide 2. lithium phosphate 3. phosphorus triiodide 7. dinitrogen pentasulfide 8. tin (IV) nitride 6. sulfur dibromide Writing Chemical Formulas 9. rubidium nitrite 11. iron (III) sulfite 12. ammonium oxide NameCharges matter? Use poly. ion sheet? Formula yes no yes no yes no yes no yes no yes no Zn 3 (AsO 4 ) 2 Ag 3 N Cu 3 P 2 Li 3 PO 4 PI 3 N2S5N2S5 Sn 3 N 4 SBr 2 RbNO 2 Fe 2 (SO 3 ) 3 (NH 4 ) 2 O OF 2


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