Chemistry Day 32. Monday, November 26 th Tuesday, November 27 th, 2018
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1 Chemistry Day 32 Monday, November 26 th Tuesday, November 27 th, 2018
2 Do-Now: Unit Exam Day Do-Now 1. Write down today s FLT 2. The element in group 7A & period 4 is. 3. The are in group 2A and have valence electrons. 4. The formula for calcium chloride is and it has a(n) bond. 5. If you are drawing a Lewis structure, when do you form double or triple bonds? 6. Which elements are naturally found as diatomic molecules? 7. Take 5 minutes to review for your unit test. Take out your planner and ToC
3 FLT I will be able to demonstrate my understanding of atoms and bonding by completing Unit 2 Exam Standard HS-PS1-1: Use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms.
4 Chemistry Day 33 Wednesday, November 28 th Thursday, November 29 th, 2018
5 Do-Now: Nomenclature Notes Complete on the back of the notes packet 1. Write down today s FLT 2. On a scale of 1-5, 5 being best, how do you think you did on the test? 3. Identify three things you could do to effectively prepare for the next test. 4. What is the name of: a. CaCl 2 b. H 2 O 5. Why do you think it s important for scientists to have a system for naming molecules and compounds? Take out your planner and ToC
6 FLT I will be able to write the names and formulas of molecules and compounds by completing Nomenclature Notes Standard HS-PS1-1: Use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms.
7 Nomenclature
8 Recall
9 Recall Ionic Bond = electrostatic attraction due to the transfer of vse - s between a metal and nonmetal Covalent Bond = sharing of valence electrons between nonmetals
10 Naming Rule #1 Identify if it is: 1. Ionic (NaCl) 2. Covalent (CO 2 ) 3. Acidic (HCl)
11 Naming Ionic Compounds (Salts)
12 Examples of Salts NaCl KBr CaF 2 NaNO 3 Al 2 (CO 3 ) 3
13 Formulas Atoms gain or lose electrons to form ions Metals lose e - s to form cations Cations have the same name as their metal Ex/ Ca 2+ = Calcium
14 Formulas Atoms gain or lose electrons to form ions Nonmetals gain e - s to form anions Anions end in -ide Ex/ F - = Fluoride
15 Name the following: 1. Na + 2. Br - 3. Be Al S 2-6. O 2-
16 Naming Ionic Compounds are usually named as metal + nonmetal -ide Ex/CaCl 2 = calcium chloride
17 What would you name these? 1. NaF 2. KI 3. Rb 2 S 4. MgO 5. Al 2 O 3
18 Metals with Multiple Charges
19 Naming Some metals (esp. transition metals) have multiple possible charges. If metals have multiple possible charges, use roman numerals to indicate charge of cation Ex/ Fe 2+ is Iron (II) and Fe 3+ is Iron (III)
20 Predicting Ionic Charges Group B elements: Many transition elements have more than one possible oxidation state. Note the use of Roman Iron (II) = Fe 2+ numerals to show charges Iron (III) = Fe 3+
21 Predicting Ionic Charges Some of the post-transition elements also have more than one possible oxidation state. Tin (II) = Sn 2+ Lead (II) = Pb 2+ Tin (IV) = Sn 4+ Lead (IV) = Pb 4+
22 Predicting Ionic Charges Group B elements: Some transition elements have only one possible oxidation state, such as these three: Silver = Ag 1+ Zinc = Zn 2+ Cadmium = Cd 2+
23
24 Exceptions: Some of the transition metals have only one ionic charge, and do not need roman numerals: Silver is always Ag 1+ Cadmium is always Cd 2+ Zinc is always Zn 2+
25 Example What is the name of HgO?
26 Transition Metals If you have a transition metal other than Ag, Cd, or Zn USE ROMAN NUMERALS Include metals such as Sn and Pb in this category since they have multiple possible charges
27 What would the names be? 1. KCl 2. MgS 3. CuS 4. SnCl 2 5. FeF 3
28 Polyatomic Ions
29 Polyatomic Ions Polyatomic Ions = a charged group of atoms that stay together Usually end in ate or ite Acetate: C 2 H 3 O 2 1- Nitrate: NO 3 1- Nitrite: NO 2 1- Permanganate: MnO 4 1- Hydroxide: OH 1- Cyanide: CN 1-
30
31 Naming Use the table for naming Ex/ NaNO 3 = sodium nitrate
32 What would the names be? 1. KOH 2. CaCO 3 3. MgSO 4
33 Note: When writing formulas, you must balance the charge of the polyatomic ion as a whole Use parentheses
34 Note: When writing formulas, you must balance the charge of the polyatomic ion as a whole Ex/ calcium nitrate
35 Try One: What would the formula be for sodium sulfate? What about calcium hydroxide?
36 Covalent Bonding
37 Covalent Bonding Use prefixes to indicate the number of each atom
38 Prefixes To write the name: prefix + 1 st element + prefix + 2 nd element ide Note: do not use the prefix mono for the first element Ex/ N 2 O = dinitrogen monoxide NO 2 = nitrogen dioxide
39 Practice by naming these: 1. Cl 2 O 3 2. CBr 4 3. CO 2 4. BaCl 2
40 Write formulas for these: 1. diphosphorus pentoxide 2. tetraiodine monoxide 3. sulfur hexafluoride 4. nitrogen trioxide 5. phosphorus trifluoride 6. aluminum chloride
41 Naming
42 Naming
43 Naming
44 Naming
45 Acids For now, understand that acids usually begin with H 1. Binary acids are named: Hydro- -ic acid 2. Oxyacids (polyatomic ions) are named: ic acid (-ate polyatomic ions) ous acid (-ite polyatomic ions)
46 Acids Binary acids are named: Hydro- -ic acid ü Ex/ HBr = hydrobromic acid ü HCl? ü H 2 S?
47 Acids Oxyacids (polyatomic ions) are named: ic acid (-ate polyatomic ions) ous acid (-ite polyatomic ions) ü Ex/ HNO 3 = nitric acid ü Ex/ HNO 2 = nitrous acid ü H 2 SO 4?
48 CW 1. Naming WS Periodate is IO - 4 Bromite is BrO - 2 We will take a KAHOOT to practice shortly 2. Finished? Work on ToC or study quietly
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