Station 1. Ionic Charge Review Using your periodic table complete the questions below. Part 1: Determine the # of valence electrons for each element. Phosphorus Bromine Xenon Nitrogen Halogens Alkali metals Part 2: Determine the oxidation # for each element. Phosphorus Copper (II) Xenon Nitrogen Halogens Alkali metals Nickel (I) Sodium Why do metals tend to form cations? _ Why do nonmetals tend to form anions? _ Why do noble gases have a zero ionic charge? _ Part 3: Determine the energy level being filled for each element. Phosphorus Bromine Xenon Magnesium Part 4: Label each element as a metal (M), a nonmetal (NM).or a metalloid (MT). Chlorine Calcium Rubidium Boron Argon Lithium Silicon Oxygen Sodium Carbon Astatine Potassium Part 5: Draw the electron structure for the following: Beryllium Sulfur Oxygen Aluminum Draw the Lewis Dot for each of the following: Ca K C Ne Sb Rb Te Be Si Cl
Station 2. Identify the following as Ionic (I), Covalent (C), or Metallic (M). a. MgCl 2 f. carbon monoxide k. PCl 5 b. KCl g. dihydrogen triiodide l. alloys c. Zn-Zn h. calcium chloride m. FeCl 3 d. N 2O 5 i. copper (II) bromide n. brass e. CuS j. carbon tetraflouride o. CO 2 Part F: Use the information given to complete the following questions. 59 2+ 16 8 O 2-39 19K 1+ 80 35Br1-31 15P 3-27Co Atomic #: Metal Nonmetal Mass #: # protons: Mass #: Mass #: Ion type: # protons: Metal Nonmetal # neutrons: # electrons: # electrons: ion type: Family: # electrons: Family: Period #: # valence e : # electrons: Ion type: 27 3+ 121 50Sn2+ 2He 13Al 4 Se 79 2-12 34 6 C Atomic #: Metal Nonmetal Family: # protons: Mass #: Mass #: Ion type: # protons: Metal Nonmetal # neutrons: # electrons: # electrons: # electrons: # neutrons: # electrons: Group #: Mass #: # valence e : # electrons: # protons: Fill in the table below with information regarding the two elements that would be present in the following types of bonds. Ionic: Define Charges involved ( + or -) Ions involved Metal or nonmetal Covalent: Metallic:
Station 3. Given the chemical compound or molecule, count the number of atoms for EACH element. a. B(NO 3) 3 b. 2 NH 4NO 3 c. 3 Al 2(SO 4) 3 d. 4 Ba(OH) 2 Identify if the following equations obey or disobey the law of conservation of mass. Show your work by counting the atoms for each equation. In your own words explain the law of conservation of mass: (A) Obeys the Law (B) Disobeys the Law 1. C 6H 6 + 8 O 2 6 CO 2 + 3 H 2O 2. Cl 2 + 2 LiF 2 LiCl + F 2 3. 8 Al 2S 3 16 Al + 3 S 6 4. 2 KClO 3 + Ba(PO 4) 2 K 3PO 4 + Ba(ClO 3) 2 5. CaO + H 2O Ca(OH) 2 Use the following equation to explain the following terms. 2 KClO 3 + Ba(PO 4) 2 K 3PO 4 + Ba(ClO 3) 2 Reactants: Products: Subscript: Coefficient:
Station 3 - Level B Balancing Equations: Count the atoms for each element on the reactant side and on the product side to determine if the Law of Conservation of Mass is Obeyed or Disobeyed. Next balance the equation if needed. Lastly answer the questions to the right. 1. H 2O + SO 3 H 2SO 4 Is SO 3 a compound or molecule? How many ve' does sulfur have? 2. Mg + Fe 2O 3 Fe + MgO What family does Fe belong to? Oxidation # of Fe in underlined compound? 3. C 2H 4 + O 2 CO 2 + H 2O Is the underlined molecule ionic or covalent? What type of bond does CO 2 have? 4. PbSO 4 PbSO 3 + O 2 What is the ox # of oxygen? What period does sulfur belong to? 5. NH 3 + I 2 N 2I 6 + H 2 What type of molecule is I 2? What energy level are the ve for N in?
Station 4 Naming ionic compounds and covalent molecules. Before the # -label the problem as Ionic (I), Covalent (C) or Metallic (M). If it is metallic do not name it. Level C Level C and B Mixed 1. KBr 2. S2F6 3. N2O3 4. Ca3P2 5. SiO2 6. NaCl 7. CO 8. PCl5 9. BeS 10. H2O 11. CaBr2 12. BrO3 13. Mg3(PO4)2 14. Ca F2 15. FeBr3 16. KNO3 17. NaOH 18. CuI 19. Mn2O3 20. Mg(OH)2 21. Li2SO4 22. Fe2S2 23. N2O5 24. CCl4 B. Before the # - label the problem as Ionic (I), Covalent (C), Transition Metal (I-TM), Given the name, write the formula of the compound. 1. calcium fluoride 6. copper (II) iodide 2. sodium nitride 7. aluminum fluoride 3. silicon tetrafluoride 4. cobalt (II) fluoride 5. dinitrogen pentaoxide 8. sodium phosphide 9. magnesium sulfide 10. carbon monoxide When are Greek prefixes used in naming? When are Roman numerals used in naming?