Date: October 31, 2016 Objective: Name binary ionic compounds. Add ionic charges to your Periodic Table:
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1 Do Now Date: October 31, 2016 Objective: Name binary ionic compounds. Add ionic charges to your Periodic Table:
2 Quick practice Classify as ionic or covalent: CaCl 2 H 2 O KI NaCl Ca 2+ Ionic compounds = Metal and a NonMetal Covalent compounds = NonMetal and a NonMetal
3 October 31, 2016 Today: Intro to Naming and Practice Binary Ionic Compounds HW: Naming Worksheet: Set A B Quiz tomorrow (short)
4 Metal, Metalloid, or Non-Metal? H Ca Si Al B Cu
5 All about ions. When an atom loses or gains electrons, ions are formed. Na Na + + e - Cl + e - Cl -
6 Na Na + Ion Formation Cl Cl -
7 Cations Cations have a positive charge. Their name does not change. Ca 2+ Li 1+ Al 3+ calcium ion lithium ion aluminum ion Think ca+ion
8 Anions Anions have a negative charge. Their name ends in ide. S 2- F 1- P 3- O 2- sulfide ion fluoride ion phosphide ion oxide ion Think a-n-ion a negative ion
9 Practice What will the charge (or oxidation number) be for the ions of: Ca S Ne Se Ba O +2-2 Zero or No Charge
10 Ionic Compounds Metal + Nonmetal Key concept: - charge must balance (net charge = 0)
11
12 Naming Binary Ionic Compounds 1. Is it ionic or molecular (covalent)? CaCl 2 Ionic (metal + nonmetal)
13 Naming Binary Ionic Compounds 2. Is the metal a transition metal? CaCl 2
14 Naming Binary Ionic Compounds 3. Write the cation name calcium CaCl 2
15 Naming Binary Ionic Compounds 4. followed by the anion. The anion should have the ide ending. CaCl 2 calcium chloride
16 Naming Binary Ionic Compounds Try this one. LiBr lithium bromide
17 Naming Binary Ionic Compounds Another. MgF 2 magnesium fluoride
18 Naming Binary Ionic Compounds Practice BaS Na S 2 KCl AlF 3 barium sulfide sodium sulfide potassium chloride aluminum fluoride
19 Practice Practice Set A and B on worksheet.
20 Practice with Ions What will the charge (or oxidation number) be for the ions of: Na K He Al Mg O Zero or No Charge
21 Don t be like this cat
22
23 Do Now Date: November 1, 2016 Objective: Name binary ionic compounds containing transition metals. Name or write chemical formula: CaCl 2 KI magnesium sulfide Na 2 O calcium bromide sodium sulfide
24 Tuesday, November 1, 2016 Today: Naming and Practice Binary Ionic Compounds HW: Naming Worksheet: Set C - D
25 Do Now
26 Na Na + Ion Formation Cl Cl -
27 Cations Cations have a positive charge. Their name does not change. Ca 2+ Li 1+ Al 3+ calcium ion lithium ion aluminum ion Think ca+ion
28 Anions Anions have a negative charge. Their name ends in ide. S 2- F 1- P 3- O 2- sulfide ion fluoride ion phosphide ion oxide ion Think a-n-ion a negative ion
29 Practice with Ions What will the charge (or oxidation number) be for the ions of: Na K He Al Mg O Zero or No Charge
30 Homework Key: Set A Key: Binary Ionic 1) magnesium sulfide 2) potassium bromide 3) barium nitride 4) aluminum oxide 5) sodium iodide 6) strontium fluoride 7) lithium sulfide 8) radium chloride 9) calcium oxide 10) aluminum phosphide 11) potassium sulfide 12) lithium bromide 13) strontium phosphide 14) barium chloride 15) sodium bromide 16) magnesium fluoride 17) sodium oxide 18) strontium sulfide 19) boron nitride 20) aluminum nitride
31 Homework Key: Set B Key: Binary Ionic 1) MgO 2) LiBr 3) Ca 3 N 2 4) Al 2 S 3 5) KI 6) SrCl 2 7) Na 2 S 8) RaBr 2 9) MgS 10) AlN
32 If there s a transition metal FeCl 3 Transition metals can have more than one charge. For example, the Fe ion can be either Fe 2+ or Fe 3+
33 If there s a transition metal FeCl 3 Find the charge on Cl. The Fe must be able to balance this charge. iron (III) chloride
34 If there s a transition metal FeBr 2 iron (II) bromide
35 If there s a transition metal FeO iron (II) oxide
36 If there s a transition metal Fe 2 O 3 iron (III) oxide
37 Remember The net charge for a neutral compound must be zero.
38 I know, it s hard work
39 Practice CuCl 2 BaF 2 BeS AlBr 3 MnO copper (II) chloride barium fluoride beryllium sulfide aluminum bromide manganese (II) oxide
40 HW - Set C Key Set C Key: Formula to Name (Transition Metals) 1) copper (II) sulfide 2) lead (IV) bromide 3) lead (II) nitride 4) iron (III) oxide 5) iron (II) iodide 6) tin (IV) phosphide
41 HW - Set D Key Set D Key: Formula to Name (Transition Metals) 1) FeCl 2 2) Cu 2 S 3) PbI 4 4) SnF 2 5) Hg 2 Br 2 6) SnO
42
43 Do Now Date: November 2, 2016 Objective: Name molecular compounds. Name or write chemical formula: FeCl 2 FeCl 3 lead (II) sulfide iron (II) bromide copper (II) oxide
44 Wednesday- November 2, 2016 Today: W-Up, Computer Lab, Activity: Naming Ternary Compounds HW: Complete WS: Set E F
45 Ionic or Molecular? NH 3 H 2 O MgCl 2 Na 2 SO 4 KI C 6 H 11 O 12 C 2 H 6 N 2
46 Molecular Compounds nonmetal bonded to nonmetal CO 2 H 2 O N 2 O 5
47 Molecular Compounds Use prefixes to show number of atoms of each element. CO 2 H 2 O carbon dioxide dihydrogen monoxide N 2 O 5 dinitrogen pentoxide
48 Prefixes mono = 1 di = 2 tri = 3 Note: CO is carbon monoxide, not monocarbon monooxide
49 Prefixes Practice SF 6 - sulfur hexafluoride boron trifluoride - BF 3 dinitrogen tetraoxide - silicon dioxide - SiO 2 N 2 O 4 Cl 2 O 7 - dichlorine heptaoxide SiS 2 - K 3 N - silicon disulfide potassium nitride
50 ---
51 Yesterday Learned to name binary ionic compounds when given the chemical formula or name.
52 Remember The charges on the ions are the key.
53 Net Charge In neutral compounds the net charge is zero. The charges on the individual atoms will add up to zero.
54 So calcium fluoride Charge on a calcium ion is +2 Charge on a fluorine ion is -1 So the formula is CaF 2.
55 And Iron (II) iodide Charge on a iron (II) ion is +2 Charge on a iodine ion is -1 So the formula is FeI 2.
56 Try these barium sulfide cesium fluoride calcium oxide copper (I) oxide iron (III) oxide BaS CsF CaO Cu 2 O Fe 2 O 3
57 Name the following compounds 1. copper (II) sulfate CuSO 4 2. CaBr 2 3. FeCl 2 4. BF 3 calcium bromide iron (II) chloride boron trifloride we ll learn more next week 5. barium nitride Ba 3 N 2 6. chloride ion Cl - 7. Na + sodium ion
58
59 Do Now Date: November 3, 2016 Objective: Name ternary compounds.
60 Thursday, November 2, 2016 Today: Computer Lab: Naming Practice, Notes & Practice
61 Date: November 3, 2016 Objective: Name chemical compounds. Copy and name: CuCl 2 BaF 2 BeS AlBr 3 MnO copper (II) chloride barium fluoride beryllium sulfide aluminum bromide manganese (II) oxide
62 Ternary Ionic Compounds Ternary ionic compounds have three or more different elements. Usually made up of a metal attached to a polyatomic ion.
63 Ternary Ionic Compounds You will be given a list of polyatomic ions to use in class and on tests.
64 Polyatomic Ions Cyanide ion: CN - Nitrate ion: NO 3 -
65 A few more polyatomic ions Sulfate ion: SO 4 2- Phosphate ion: PO 4 3-
66 -ate vs. -ite Nitrate Ion Nitrite Ion Sulfate Ion Sulfite Ion
67 Remember: -ate vs. -ite -ate is greater: SO 4 2- is sulfate -ite is just a bite. SO 3 2- is sulfite -ate has one more O than -ite
68 Naming Ternary Compounds magnesium sulfate magnesium has a +2 charge the sulfate ion (SO 4 2- ) has a -2 charge MgSO 4
69 Naming Ternary Compounds copper (II) nitrate copper (II) has a 2+ charge the nitrate ion (NO 3- ) has a 1- charge Cu(NO 3 ) 2
70 A word about parentheses Cu(NO 3 ) 2 Number Cu atoms: Number N atoms: Number O atoms: 1 2 6
71 A word about parentheses Zn(OH) 2 Number Zn atoms: Number O atoms: Number H atoms: 1 2 2
72 Ammonium Ion NH 4 +1 is the only positive ion we will use in the class. For example: NH 4 NO 3 = ammonium nitrate NH 4 Cl = ammonium chloride
73 Confusing?
74 Try these aluminum nitrate Al(NO 3 ) 3 sodium sulfate Na 2 SO 4 manganese (II) hydroxide Mn(OH) 2 ammonium bromide NH 4 Br
75 Molecular Compounds nonmetal bonded to nonmetal CO 2 H 2 O N 2 O 5
76 Molecular Compounds Use prefixes to show number of atoms of each element. CO 2 H 2 O carbon dioxide dihydrogen monoxide N 2 O 5 dinitrogen pentoxide
77 Prefixes mono = 1 di = 2 tri = 3 Note: CO is carbon monoxide, not monocarbon monooxide
78 Prefixes Practice SF 6 - sulfur hexafluoride boron trifluoride - BF 3 dinitrogen tetraoxide - silicon dioxide - SiO 2 N 2 O 4 Cl 2 O 7 - dichlorine heptaoxide SiS 2 - K 3 N - silicon disulfide potassium nitride
79
80 Do Now Date: November 4, 2016 Objective: Name ionic and molecular compounds. Write the name or chemical formula: BaCl 2 Fe 2 O 3 CaSO 4 PCl 3 Calcium fluoride iron(ii) chloride dihydrgon monoxide
81 Friday, November 4, 2016 Today: W-Up, Lab: Ionic and Molecular Compounds HW:
82 Name the following compounds Sodium Nitride Na 3 N Potassium Bromide Iron (III) Chloride KBr FeCl 3 Phosphorous trichloride PCl 3
83 Lab: Properties of Ionic and Molecular Bonds Task: Using your notes and chemistry book design a procedure to determine whether a compound has ionic bonds or covalent (also called molecular) bonds. Purpose: Safety: Procedure: Observations: Data Table (observations): Conclusion: Be sure to include the letter of your unknown substances (A, B, C, ), important observations, problems you needed to overcome, any changes you made to your procedure, and a statement about the nature of you unknown samples supported by evidence from your observations and data.
84 HW Set E Key: Formula to Name 1) aluminum phosphate 2) potassium nitrite 3) sodium hydrogen carbonate 4) calcium carbonate 5) magnesium hydroxide 6) sodium chromate
85 HW Set F Key: Formula to Name 1) Ag 2 CO 3 2) K 2 HPO 4 3) Al(OH) 3 4) NaHCO 3 5) Ca(CH 3 COO) 2 6) KMnO 4
86 Name the following compounds SnS PbS 2 tin (II) sulfide lead (IV) sulfide calcium chloride CaCl 2 NaI ZnF 2 sodium iodide zinc fluoride lithium oxide Li 2 O BeO beryllium oxide
87
88 Name the following compounds 1. magnesium sulfide 2. aluminum oxide MgS Al 2 O 3 3. FeCl 3 4. MgF 2 iron (III) chloride magnesium fluoride 5. sodium oxide 6. fluoride ion Na 2 O F -
89
90 Diatomic Elements H 2 N 2 O 2 In chemical equations, the compound has the same name as the element. Cl 2 Br 2 I 2 F 2 hydrogen + oxygen water is H 2 + O 2 H 2 O
91 So for H, N, O, F, Cl, I, Br You could also say dihyrogen, dioxygen, dinitrogen,
92 Molecular Compounds nonmetal bonded to nonmetal CO 2 H 2 O N 2 O 5
93 Molecular Compounds Use prefixes to show number of atoms of each element. CO 2 H 2 O carbon dioxide dihydrogen monoxide N 2 O 5 dinitrogen pentoxide
94 Prefixes mono = 1 di = 2 tri = 3 Note: CO is carbon monoxide, not monocarbon monooxide
95 Prefixes Practice SF 6 - sulfur hexafluoride boron trifluoride - BF 3 dinitrogen tetraoxide - silicon dioxide - SiO 2 N 2 O 4 Cl 2 O 7 - dichlorine heptaoxide SiS 2 - K 3 N - silicon disulfide potassium nitride
96
97 Common Acids HCl hydrochloric acid H 2 SO 4 H 3 PO 4 H 2 CO 3 HC 2 H 3 O 2 sulfuric acid phosphoric acid carbonic acid acetic acid
98 Common Bases NaOH KOH NH 3 sodium hydroxide potassium hydroxide ammonia
99
100
101
102 Old Notes and Practice
103 Types of Compounds: Ionic
104 Ionic Compounds: Formula Unit Smallest representative unit of an ionic compound.
105 Formula Unit of NaCl Image from media_portfolio/text_images/fg03_03.jpg
106 H Hydrogen Ion Charge +1
107 He Helium No Charge.
108 Li Lithium Charge +1
109 Be Beryllium Charge +2
110 B Boron Charge +3
111 C Carbon Charge +4 or -4
112 N Nitrogen Charge -3
113 O Oxygen Charge -2
114 F Fluorine Charge -1
115 Ne Neon No Charge.
116 ---
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