lithium nitrate lead II sulfide lithium nitride barium

lithium nitrate lead (II) sulfide lithium nitride barium sulfide lithium nitrite Outline Chemistry sulfur dioxide Unit 5: Bonding and Inorganic Nomenclature Na. Cl. O 3 NO 2 Fe(Cl. O 3)2 N 2 O 4 Fe(Cl. O 3)3 N 2 O 5 Power. Point Presentation by Mr. John Bergmann

Chemical Bonding Ionic Bonds: atoms give up or gain e– and are attracted to each other by coulombic attraction Na loses e– Na 1+ + Cl 1– Cl gains e– Na. Cl ionic compounds = salts K 1+ + NO 31– KNO 3 where NO 31– is a polyatomic ion: a charged group of atoms that stay together Cl 1–

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

Covalent Bonds …atoms share e– to get a full valence shell C (4 v. e–) 1 s 2 2 p 2 1 s 2 2 p 5 (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–

carbon tetrafluoride (CF 4) o x x o o C o x x x x F x x x x o o o C o H H x o x H x o H H C x o Hx x x F x o x x x x Co F x x o x x methane (CH 4) x x x F

nitrogen triiodide (NI 3) o x x o o No o x x o o I N o x x x x x o x x I x x x Ix x x x x Ix xx carbon dioxide (CO 2) o o x x o C o x x Ox x x Ox x o o o C o x xx Ox x x xx xx O =C=O xx xx

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

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

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

Other Types of Bonds dipole-dipole forces hydrogen bonds London dispersion forces ion-dipole forces boiling H 2 O DNA 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).

Writing Formulas of Ionic Compounds chemical formula: has neutral charge; 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 Na 1+ and F 1– Na. F Ba 2+ and O 2– Ba. O Na 1+ and O 2– Na 2 O Ba 2+ and F 1– Ba. F 2

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

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 42– Ba. SO 4 Mg 2+ and NO 21– Mg(NO 2)2 NH 41+ and Cl. O 31– NH 4 Cl. O 3 Sn 4+ and SO 42– Sn(SO 4)2 Fe 3+ and Cr 2 O 72– Fe 2(Cr 2 O 7)3 N 3– (NH 4)3 N NH 41+ and

Inorganic Nomenclature potassium nitrate KNO 3 copper (II) sulfate Cu 2 SO 4 dinitrogen monoxide N 2 O sodium hydroxide Na. OH

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

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

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

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

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. Fe Cu Stock System of nomenclature Fe. O 2+oxide ? iron Fe O 2– Fe 2 O 3 ? 3+oxide iron Fe Fe? 3+ O 2– iron (III) oxide Cu. Br ? Brbromide 1– copper Cu 1+ copper (I) bromide Cu. Br 2 1– Br 1– copper Cu? 2+ Brbromide copper (II) bromide iron (II) oxide

B. To find the formula, given the name: 1. Write symbols for the two types of ions. 2. Balance charges to write formula. Co Sn cobalt (III) chloride Co 3+ Cl 1– Co. Cl 3 tin (IV) oxide Sn 4+ O 2– Sn. O 2 tin (II) oxide Sn 2+ O 2– Sn. O

Compounds Containing Polyatomic Ions Insert name of ion where it should go in the compound’s name. Write formulas: iron (III) nitrite Fe 3+ NO 31– Fe(NO 3)3 ammonium phosphide NH 41+ P 3– (NH 4)3 P ammonium chlorate NH 41+ Cl. O 31– NH 4 Cl. O 3 zinc phosphate Zn 2+ PO 43– Zn 3(PO 4)2 lead (II) permanganate Pb 2+ Mn. O 41– Pb(Mn. O 4)2

Write names: (NH 4)2 S 2 O 3 ammonium thiosulfate Ag. Br. O 3 silver bromate (NH 4)3 N ammonium nitride Cr. O 42– ? Cr. O 2– uranium (VI) chromate U(Cr. O 4)3 U 6+ 4 Cr. O 42– ? SO 2– Cr 2(SO 3)3 Cr 3+ chromium (III) sulfite 3 Cr? 3+SO 32–

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

EXAMPLES: carbon dioxide CO 2 CO carbon monoxide dinitrogen trioxide N 2 O 3 N 2 O 5 dinitrogen pentoxide carbon tetrachloride CCl 4 NI 3 nitrogen triiodide

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

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

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

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 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.

Element gold, Au lead, Pb tin, Sn copper, Cu iron, Fe Latin root aurplumbstanncuprferr- Write formulas: cuprous sulfide Cu 1+ S 2– Cu 2 S auric nitrite Au 3+ NO 21– Au(NO 2)3 ferrous fluoride Fe. F 2 Fe 2+ F 1– -ic Au 3+ Pb 4+ Sn 4+ Cu 2+ Fe 3+ -ous Au 1+ Pb 2+ Sn 2+ Cu 1+ Fe 2+ Write names: 3– P 4+ ? ? 4+ Pb 3 P 4 Pb Pb Pb P 3– plumbic phosphide ? Pb 2+ ? P 3– Pb 3 P 2 Pb? 2+ Pb 2+ plumbous 1– OH phosphide Sn(OH) Sn? 4+ OH 1– 1– 4 OH stannic hydroxide

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

Writing Chemical Names Use poly. Formula RN/GP/neither ion sheet? Name 7. S O 3 8. Sn Br 4 GP neither no no sulfur trioxide tin (IV) bromide 9. K 3 PO 4 neither yes potassium phosphate 10. NH 4 OH neither yes ammonium hydroxide 11. C S 2 12. Cu F GP RN no no carbon disulfide copper (I) fluoride

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.

Element gold, Au lead, Pb tin, Sn copper, Cu iron, Fe Latin root aurplumbstanncuprferr- Write formulas: cuprous sulfide Cu 1+ S 2– Cu 2 S auric nitrite Au 3+ NO 21– Au(NO 2)3 ferrous fluoride Fe. F 2 Fe 2+ F 1– -ic Au 3+ Pb 4+ Sn 4+ Cu 2+ Fe 3+ -ous Au 1+ Pb 2+ Sn 2+ Cu 1+ Fe 2+ Write names: 3– P 4+ ? ? 4+ Pb 3 P 4 Pb Pb Pb P 3– plumbic phosphide ? Pb 2+ ? P 3– Pb 3 P 2 Pb? 2+ Pb 2+ plumbous phosphide 1– OH Sn(OH)4 Sn? 4+ OH 1–OH 1– stannic hydroxide

Empirical Formula and Molecular Formula shows the true number and type of atoms in a m’cule lowest-terms formula Compound Molecular Formula Empirical Formula glucose C 6 H 12 O 6 CH 2 O propane C 3 H 8 butane C 4 H 10 C 2 H 5 naphthalene C 10 H 8 C 5 H 4 sucrose C 12 H 22 O 11 octane C 8 H 18 C 4 H 9

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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 - traditional system of nomenclature Worksheet - covalent binary cmpds: non-metal - non-metal Worksheet - empirical and molecular Worksheet - vocab (bonding) Worksheet - ionic cmpds: polyatomic ions Worksheet - ionic binary cmpds: multiple charge cation Worksheet - errors in chemical formulas and nomenclature Worksheet - oxidation numbers and ionic cmpds Activity - bonding pieces Activity - molecular models Activity - mole pattern Textbook - questions Worksheet - names and formulas of cmpds Outline (general)