Chemical Names and Formulas Chapter 6 Assignment & Problem Set Name_______________________ Warm-Ups (Show your work for credit) Date______________ Answer: 1. Date______________ Answer: 2. Date______________ Answer: 3. Date______________ Answer: 4. Date______________ Answer: 5. Date______________ Answer: 6. Date______________ Answer: 7. Date______________ Answer: 8. Chemical Names and Formulas Chapter 6 Assignment & Problem Set 2 Study Guide: Things You Must Know Vocabulary (know the definition and what it means): atom ion cation anion chemical formula compound molecular compound ionic compound molecular formula formula unit binary compound monatomic ion Stock system Classical system polyatomic ion criss-cross method molecular attraction acid Learning Objectives: why systematic names are given to chemical compounds the difference between an atom and an ion only electrons are lost when a cation is formed from an atom and only electrons are gained when an anion is formed from an atom how to recognized the difference between a molecular compound and an ionic compound how to name molecular compounds using the prefix system how to determine the charge and name of a monatomic cations and anions using the Periodic Table how to use the Stock system for naming cations with more than one charge how to determine the formula and charge of a polyatomic ion using Table E how to write formulas for ionic compounds by balancing charges (criss-cross method) general properties of molecular and ionic compounds how to recognize the formula of an acid how to name the three types of acids based on anion name Key Reference Tables Table E: Selected Polyatomic Ions Table K: Common Acids Periodic Table Chemical Names and Formulas Chapter 6 Assignment & Problem Set 3 •Read Chapter 6 (Chemical Names and Formulas) •Regents students can earn 10 extra credit points by doing problems 24 & 25. •There is no lab. •Regents Tables Table E: Selected Polyatomic Ions Table K: Common Acids Table L: Common Bases Periodic Table of the Elements •Warm-ups and problems will be collected before you take the test. Answer all problems in the space provided. For problems involving an equation, carry out the following steps: 1. Write the equation. 2. Substitute numbers and units. 3. Show the final answer with units. There is no credit without showing work. Molecular and Ionic Compounds 1. What are the only elements that exist in nature as isolated atoms? 2. Differentiate between molecular formula and formula unit. 3. Would you expect the following pairs of atoms to form an ionic (I) or a molecular (M) compound? a. Li and S c. Al and O e. I and K b. O and S d. F and Cl Molecular Compounds 4. Name these binary molecular compounds. a. OF2 b. Cl2O8 5. Write the formula or name for these compounds. a. CS2 c. carbon tetrabromide b. Cl2O7 d. diphosphorus trioxide Ions and Ionic Compounds 6. Write the symbol and name for the cation formed when a. a potassium atom loses one electron b. a zinc atom loses two electrons 7. Write the symbol and name for the anion formed when a. a fluorine atom gains one electron b. a sulfur atom gains two electrons f. H and N c. SO3 Chemical Names and Formulas Chapter 6 Assignment & Problem Set 4 8. Using only the periodic table, name and write the formula for the typical ion of each representative element. a. potassium c. argon e. beryllium b. sulfur 9. Write the formula for each ion. a. ammonium ion b. tin(II) ion d. bromine f. sodium c. nitrate ion e. permanganate ion d. cyanide ion f. manganese(II) ion 10. State the number of electrons either lost or gained in forming each ion. a. Brc. As-3 e. Cu+ b. Na+ d. Ca+2 11. Write names for these binary ionic compounds. a. CaO b. Cu2Se f. H- c. FeS d. AlF3 12. Write formulas for compounds formed from these pairs of ions. a. NH4+, SO3-2 b. calcium ion, phosphate ion c. Al+3, NO3- d. potassium ion, chromate ion Chemical Names and Formulas Chapter 6 Assignment & Problem Set 5 13. State whether the following compounds are molecular (M) or ionic (I), then give the name or formula. a Potassium iodide b Magnesium nitride c SnO2 d N2O e Lithium sulfide f Zinc hydrogen sulfate g Ammonium iodide h Cu2S i Barium sulfate j Aluminum hydrogen carbonate k Sodium hypochlorite l Pb(CrO4) 2 m LiCN n Fe(ClO3)3 o Carbon tetrachloride p Mg3(PO4)2 q CBr4 r N2O5 s AlCl3 t Diphosphorous trioxide Chemical Names and Formulas Chapter 6 Assignment & Problem Set 6 14. Complete the table by writing correct formulas for the compounds formed by combining positive and negative ions. Then name each compound. NO3- CO32- PO43- NH4+ Sn+4 Fe+3 Mg+2 15. List two characteristics that distinguish ionic compounds from molecular compounds. 16. The melting point of a compound is 1240oC. Is this compound an ionic or a molecular compound? Explain. Naming Acids 17. Give the name or the formula for these acids. a. HCl c. HNO3 b. H2SO4 d. H2CO3 e. sulfuric acid g. acetic acid f. nitric acid h. phosphoric acid c. strontium ion d. sulfide ion Review 18. Make the following conversions. a. 775ml to microliters(L) b. -65oC to K c. 8.32 mg Ag to centigrams of silver 19. How many protons and electrons are in each ion? a. magnesium ion b. bromide ion 20. A student finds that 6.62g of a substance occupies a volume of 12.3cm3. What is the density of the substance? Chemical Names and Formulas Chapter 6 Assignment & Problem Set 7 21. (Honors; Regents can do for 1 point extra credit) The Handbook of Chemistry and Physics is a reference work that contains a wealth of information about elements and compounds. Use the sections in this book, “Description of the Elements” and "Physical Constants of Inorganic Compounds" to complete the table. Name Ammonium Chloride Barium Barium Sulfate Bromine Calcium Carbonate Chlorine Copper(II) sulfate Pentahydrate Iodine Iron(II) sulfate pentahydrate Mercury Potassium Carbonate Sulfur Formula Color Density (g/mL) Melting Pt. (oC) Boiling Pt. (oC) Solubility (g per 100 g cold H2O) Chemical Names and Formulas Chapter 6 Assignment & Problem Set 8 22. (Honors; Regents can do for 1 point extra credit) Use the table you prepared in question 21 to answer the following questions. a. You have two unlabeled bottles, each containing a white powder. One of the substances is calcium carbonate, and the other is potassium carbonate. Describe a simple physical test you could carry out to distinguish between these two compounds. b. How would you distinguish between samples of copper(II) sulfate pentahydrate and iron(II) sulfate pentahydrate? c. A bottle contains a mixture of ammonium chloride and barium sulfate. What method could you use to separate these two compounds? d. List the elements in the table in order of increasing density. e. Calculate the mass of 47.0 cm3 of mercury. f. Calculate the volume of 16.6g sulfur. g. How would you distinguish among the Group 7A elements (halogens) listed on the table?
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