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Unit 2 Properties of Matter

Unit 2 Properties of Matter. 2.1 Distinguish between physical and chemical properties and changes. Put a P next to Physical Changes Put a C next to Chemical Changes 1. A piece of wood burns to form ash. _________ 2. Water evaporates into steam. _________

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Unit 2 Properties of Matter

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  1. Unit 2 Properties of Matter

  2. 2.1 Distinguish between physical and chemical properties and changes. Put a P next to Physical Changes Put a C next to Chemical Changes 1. A piece of wood burns to form ash. _________ 2. Water evaporates into steam. _________ 3. A piece of cork is cut in half. _________ 4. A bicycle chain rusts. _________ 5. Food is digested in the stomach. _________ 6. Water is absorbed by a paper towel. _________ 7. Hydrochloric Acid reacts with zinc. _________

  3. 8. A piece of an apple rots on the ground. _________ 9. A tire is inflated with air. _________ 10. A plant turns sunlight, CO2, and water into sugar and oxygen. _________ 11. Sugar dissolves in water. _________ 12. Eggs turn into an omelette. _________ 13. Milk sours. _________ 14. A popsicle melts. _________ 15. Turning brownie mix into brownies. ________

  4. 2.2 Understand the difference between elements, compounds, and mixtures.

  5. Use the periodic table to identify each element in the following compounds and tell how atoms of each element are present in the compound. H2O ___ CO2 ___ NaHCO3 ___ Fe203 ___ KAl3Si3O10 ___ CaCO3 ___

  6. 2.3 Distinguish between protons, neutrons, and electrons and be able to describe the composition of an atom of any particular element in terms of these subatomic particles. Zumdahl page 71: 44, 46

  7. 2.4 Know the difference between an atom, an ion, and a molecule. Zumdahl page 71: 48, 50

  8. 2.5 Have a basic knowledge of the periodic table, which includes being able to predict whether an element is a metal or a nonmetal, and what will be the probable charge of its ion. • As you go from left to right across the periodic table, the elements go from (metals / nonmetals) to (metals / nonmetals). • Where are the most active metals located? • Where are the most active nonmetals located?

  9. Elements of Group 1 are called _______ • Elements of Group 2 are called _______ • Elements of Group 3-12 are called _______

  10. Group 17 elements are called _______ • The most active element in Group 17 is _____ • Group 18 elements are called _______

  11. The majority of elements in the periodic table are (metals / nonmetals). • Elements in the periodic table are arranged according to their _______ • An element with both metallic and nonmetallic properties is called a _______

  12. 2.6 Be able to write the correct name of an inorganic compound from its formula and vice versa. Type I: Binary Ionic Writing Names from Formulas 1. Identifying the cation as a Group I metal , Group II metal, Aluminum, Zinc, or Silver 2. Identify the anion as a nonmetal 3. Name the cation (the metal) with its full name 4. Name the anion (the nonmetal) by changing the ending to -ide Example: NaCl cation: sodium & anion: chlorine Name: sodium chloride

  13. NaClBeO AlCl3 KBr CaF2 Zn2O MgI2 Cs2S Ag3P

  14. Writing Formulas from Names 1. Identify charge of cation (1+, 2+, 3+) 2. Identify charge of anion (1-, 2-, 3-) 3. Balance the charges 4. The charge of the cation becomes the subscript of the anion 5. The charge of the anion becomes the subscript of the cation 6. Reduce subscripts if necessary

  15. Aluminum Sulfide Potassium Oxide Sodium Nitride Barium Carbide Zinc Chloride Potassium Iodide Lithium Sulfide Silver Fluoride

  16. Type I: Polyatomic Writing Names from Formulas 1. Identifying the cation as a Group I metal , Group II metal, Aluminum, Zinc, or Silver 2. Identify the anion as a polyatomic ion 3. Name the cation (the metal) with its full name 4. Name the anion (the polyatomic) with its full name Example: KOH cation: potassium & anion: hydroxide Name: potassium hydroxide

  17. KCN LiSO3 FrClO2 NaOH CsPO4 MgSiO3 CaCO3 NH4Cl BaC2O4

  18. Writing Formulas from Names (polyatomics) silver nitrate strontium chlorate aluminum dichromate magnesium sulfate barium cyanide ammonium sulfate calcium hydroxide zinc silicate

  19. Type II: Transition Metals Writing Names from Formulas 1. Identify the cation as a transition metal 2. Identify the anion 3. Identify the charge of the cation 4. Name the cation (the transition metal) with its full name and the charge of the ion in roman numerals 5a. Name the anion (the nonmetal) by changing the ending to –ide 5b. Name the anion (the polyatomic) with its full name Example: CoBr2 Cation: cobat 2+ & anion: 2 bromine Name: cobalt (II) bromide

  20. CuI Co2(CO3)3 HgBr2CuI2 SnO Hg2Br2 CoCO3 SnO2 SnS

  21. Writing Formulas from Names (transitional metals) iron(II) oxide chromium(III) phosphate iron(III) hydroxide iron(III) oxide manganese (II) fluoride lead(IV) sulfite chromium(II) phosphate manganese (III) fluoride mercury(I) sulfide

  22. Naming Molecular Compounds Writing Names from Formulas 1. Both cation and anion are nonmetals 2. Use prefixes to indicate how many atoms are present 3. Name the first element: prefix with its full name 4. Name the second element: prefix element name and change the ending to -ide 5. Do not use “mono” when naming the first element Example: CS2 Elements: carbon & 2 sulfur Name: carbon disulfide

  23. Prefixes: 1: ______ 2: ______ 3: ______ 4: ______ 5: ______ 6: ______ 7: ______ 8: ______ 9: ______ 10: ______ CO PCl3 N2O CO2 SO3 P2O5 NO2 SF6 NF3

  24. Writing Formulas from Names 1. Identify the elements 2. Identify prefixes for each element 3. Charges do not matter for molecular formulas!! diphosphorousmonosulfidecarbonmonoxide diphosphoroustrioxidesulfur tetrafluoride nitrogen triiodide carbon tetrabromide nitrogen monoxide phosphorous hexabromide dichlorineheptoxide

  25. Naming Acids Binary Acids Binary acids contain only two different elements. One of them is H+ and the other is an anion. To name them take the anion root word, put hydro in front of it and change the ending from ide to ic acid. Examples: HCl – hydrochloric acid HI – hydroiodic acid

  26. OxyacidsOxyacids are acids whose anions are polyatomic anions that contain oxygen. H+ is still the cation. These acids are named based on the nature of the anion as shown in the table below. Examples: HClO4 – perchloric acid HClO3 – chloric acid HClO2 – chlorous acid HClO – hypochlorous acid

  27. HF H3PO4 HNO3 HI HC2H3O2 H2SO3 HBr H2CO3 HCN

  28. Writing Formulas from Names 1. Identify elements 2. Identify type of anion 3a. Hydro : there is no oxygen in the formula 3b. –ic acid : look for the polyatomic with –ate ending 3c. –ous acid: look for polyatomic with –ite ending

  29. hydrobromic acid hydrocyanic acid nitrous acid hydrofluoric acid carbonic acid nitric acid

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