Gen Chem Unit 4: Chemical Compounds Name: _____________________________________ Per: _______________________ Unit 4 Homework and Lab Packet ! # $ ' $( (' $ " (' ()# ) ! * )& , + ( % & , * ( ( 0) . (0 )& ) ( + ( )& (0) + * ) ( ( ( ( (0) ' +& + + ( ) 1 2 & ,3 . ) / ,) 0) ' ) ( 4, ( ( 5) - 5 ( 6 & - ( ) + * ) 78888888888888888888888888888888 Updated November 2009 1 Gen Chem Unit 4: Chemical Compounds Overall Objective: to be able to understand how and why atoms bond together and to recognize ionic and covalent compounds. At the end of the unit, you should: 1. be able to determine the common charge of the ions of the elements in groups IA, IIA, IIIA, IVA, VA, VIA, VIIA, VIIIA. 2. be able to differentiate between molecular (covalent) and ionic compounds. 3. be able to differentiate between covalent and ionic bonds. 4. know what a polyatomic ion is and how it bonds with other ions. 5. define nomenclature. 6. recognize the difference between acids, covalent compounds, and ionic compounds by name and formula. 7. correctly name acids, covalent compounds, and ionic compounds given a formula. 8. Write and give the formula for acids, covalent compounds, and ionic compounds given a chemical name. 9. know the different types of particles (atoms, molecule). 10. Explain how the octet rule applies to atoms of metallic and nonmetallic elements 11. Distinguish between melting and boiling points of molecular and ionic compounds. 12. Describe three properties of ionic compounds 13. Explain the importance of alloys 2 Gen Chem Unit 4: Chemical Compounds Common Ion Charges Write in the Lewis Dot structures for the atoms in the THIRD PERIOD. Also, fill in the number of protons, total electron (e), and valence electrons (Ve) for each atom P= P= P= P= P= P= P= P= e= e= e= e= e= e= e= e= Ve= Ve= Ve= Ve= Ve= Ve= Ve= Ve= For the table below, write the Lewis Dot structure for the most stable ion for each of the symbols written above. Also fill in the number of protons, total electrons (e), and valence electrons (Ve) for each atom. P= P= P= P= P= P= P e= e= e= e= e= e= e= Ve= Ve= Ve= Ve= Ve= Ve= Ve= 1. Nonmetals tend to _____________________ electrons to form a ______________ charged ion. 2. Metals tend to ______________________ electrons to form a ________________ charged ion. 3. Look at the nonmetal ions. The electron configuration is the same as what family on the periodic table? _________________________________________ Why is this important to notice? ___________________________________ 4. Complete the box for Neon. How do the positive ions compare to neon? P= e= Ve= Revised Fall 2005 3 Gen Chem Unit 4: Chemical Compounds Name: _________________ Counting Atoms makes me hungry! When atoms bond to form molecules, we use subscripts to tell how many atoms of each element are in the compound. We also use coefficients to tell how many molecules there are. For example, a sandwich has 2 slices of bread and one slice of meat. Using proper chemistry notation, we would write this as: Bread2Meat This tells me that I have two breads, and only 1 meat. If I had three slices of meat, how would I write that? __________________ I can also use coefficients to tell me that I have more than one molecule. If I had two Big Macs, we would write this as: 2Bread3Meat2 How many total breads do I have?__________________ How many total meats do I have? __________________ Finally, parenthesis set things aside, just like in math. For example, I have a salad that has 2 cucumbers for every one piece of tomato. There are two sets of tomatoes and cucumbers for every 15 pieces of lettuce. We would write this as: Lettuce15(Cucumber2Tomato)2 How many total lettuces do I have? __________________ How many total cucumbers do I have? _________________ How many total tomatoes do I have? _____________________ 4 Gen Chem Unit 4: Chemical Compounds Now you get to practice these with real compounds! Fe(OH)3 3 Fe(OH)3 2 Fe(NO3)3 H2CO3 4 Fe(HCO3)3 2 Fe(NO3)3 3 FeCO3 CO2 2 CO2 NaHCO3 4 NaOH NH4NO3 13 NH4NO3 SO2 A12(SO4)3 A12O3 2 NH4NO3 4 NH4NO2 Fe O H N C Na O H N C S O Al N H 5 Gen Chem Unit 4: Chemical Compounds Ionic and Metallic Bonding Reading Guide (Chapter 7; p.186-203) Directions: Use your textbook to complete the following notes. As you read the section and find the quote, explain the quote in your own words. Then, give an example of each quote from the reading. Summarize in your own words: “Valence electrons are the electrons in the highest occupied energy level of an element’s atoms. The number of valence electrons largely determines the chemical properties of an element.” Example from the Textbook: Summarize in your own words: “…the octet rule: in forming compounds, atoms tend to achieve the electron configuration of a noble gas. An octet is a set of eight. Example from the Textbook: 6 Gen Chem Unit 4: Chemical Compounds Summarize in your own words: “An atom’s loss of valence electrons produces a cation, or a positively charges ion. Example from the Textbook: Summarize in your own words: “The gain of negatively charged electrons by a neutral atom produces an anion. The name of the anion typically ends in –ide.” Example from the Textbook: 7 Gen Chem Unit 4: Chemical Compounds Chapter and Pages: 7.2 and 7.3; p.194-203 Topic: Ionic Bonds, Compounds, and Bonding in Metals Directions: Read the pages in the textbook. Fill in the graphic organizer with the information that will best answer the heading in each box. Describe an ionic bond What is a chemical formula vs. a formula unit? State and describe one property of ionic compounds State and describe a second property of ionic compounds State and describe a third property of ionic compounds What is an alloy? Why are they important? Give two examples. 8 Gen Chem Unit 4: Chemical Compounds Chapter + Pages: 8.1 and 8.2; p.212-222 Topic: Covalent Bonding Read the pages in the textbook. Fill in the graphic organizer with the information that will best answer the heading in each column. Describe a covalent bond. What is the similarity/difference Describe the properties of molecular between a molecule, diatomic compounds molecule, and molecular compound? What is a molecular formula and what does it show? List 4 examples. What do electrons do in covalent bonds to achieve an octet? Compare and contrast, single, double, and triple bonds. 9 Gen Chem Unit 4: Chemical Compounds Type of Compounds Jigsaw Group 1 Your group’s very important job is the following: 1) Look at the following examples of ionic compounds 2) Figure out what is the same about all of the ionic compounds 3) Come up with rules for identifying ionic compounds from either the chemical symbols or the names 4) Prepare to teach the class your rules (you can use overhead transparencies, butcher paper, the chalk board, or anything else that you find useful) Ionic Compound Examples KF Li2O CaBr2 Ba3N2 FeS AlI3 Pt2Se FrF Copper(I) iodide Magnesium chloride Cesium chloride Manganese(III) telluride Lithium carbide Gold(I) astatide Rubidium sulfide Strontium bromide For comparison, these are NOT ionic compounds: CCl4 Silicon Dioxide PI3 Carbon Dioxide O2 Antimony tribromide 10 Gen Chem Unit 4: Chemical Compounds Group 2 Your group’s very important job is the following: 1) Look at the following examples of ionic compounds’ formulas and names 2) Figure out the process to go from the formula to the name and vice versa 3) Come up with rules for writing formulas for ionic compounds from their names and vice versa 4) Prepare to teach the class your rules (you can use overhead transparencies, butcher paper, the chalk board, or anything else that you find useful) Ionic Compound Examples KF Potassium flouride Li2O Lithium oxide CaBr2 Calcium bromide Ba3N2 Barium nitride FeS Iron(II) sulfide AlI3 Aluminum iodide Pt2Se Platinum(I) selenide FrF Francium flouride Copper(I) iodide CuI2 Magnesium chloride MgCl2 Cesium chloride CsCl Manganese(III) telluride Mn2Te3 Lithium carbide Li4C Gold(I) astatide AuAt Rubidium sulfide Rb2S Strontium bromide SrBr2 11 Gen Chem Unit 4: Chemical Compounds Group 3 Your group’s very important job is the following: 1) Look at the following examples of covalent compounds 2) Figure out what is the same about all of the covalent compounds 3) Come up with rules for identifying covalent compounds from either the chemical symbols or the names 4) Prepare to teach the class your rules (you can use overhead transparencies, butcher paper, the chalk board, or anything else that you find useful) Covalent Compound Examples CCl4 PI3 O2 NF3 Cl2 Silicon dioxide Carbon dioxide Antimony tribromide Carbon monoxide Selenium dioxide Nitrogen trioxide Silicon tetrabromide Sulfur dioxide For comparison, these are NOT covalent compounds: KF Copper (I) iodide Li2O Magnesium chloride CaBr2 Cesium chloride 12 Gen Chem Unit 4: Chemical Compounds Group 4 Your group’s very important job is the following: 5) Look at the following examples of covalent compounds 6) Figure out the process to go from the formula to the name and vie versa. 7) Come up with rules for writing formulas for covalent compounds from their names and vice versa. 8) Prepare to teach the class your rules (you can use overhead transparencies, butcher paper, the chalk board, or anything else that you find useful) Covalent Compound Examples CCl4 Carbon tetrachloride PI3 Phosphorous triiodide O2 Oxygen NF3 Nitrogen triflouride Cl2 Chlorine Silicon dioxide SiO2 Carbon dioxide CO2 Antimony tribromide SbBr3 Carbon monoxide CO Selenium dioxide SeO2 Nitrogen trioxide NO3 Silicon tetrabromide SiBr4 Sulfur dioxide SO2 13 Gen Chem Unit 4: Chemical Compounds Group 5 Your group’s very important job is the following: 1) Look at the following examples of acids’ formulas and names 2) Figure out the process to go from the formula to the name and vice versa 3) Come up with rules for writing formulas for acids from their names and vice versa 4) Prepare to teach the class your rules (you can use overhead transparencies, butcher paper, the chalk board, or anything else that you find useful) Acid Examples HF hydrofluoric acid HCl hydrochloric acid HBr hydrobromic acid HI hydroiodic acid H2SO4 sulfuric acid HNO3 nitric acid HClO3 chloric acid HC2H3O2 acetic acid HNO2 nitrous acid HClO3 chlorous acid 14 Gen Chem Unit 4: Chemical Compounds Bond Identification 1. When atoms share electrons to fill their outermost energy levels, they form ________________________ bonds. 2. When atoms transfer electrons to fill their outermost energy levels, they form ________________________ bonds. 3. Indicate whether the atoms listed below will share electrons or transfer electrons (HINT: when electrons are transferred, both atoms will have complete outermost energy levels. Otherwise, atoms share electrons.) a. O -- O a. ____________________________ b. K -- Cl b. ____________________________ c. C -- O c. ____________________________ d. H -- F d. ____________________________ e. I -- I e. ____________________________ f. S -- O -- O f. ____________________________ g. Na -- Na -- S g. ____________________________ h. Li -- Cl h. ____________________________ i. Ca -- Br -- Br i. ____________________________ j. N -- N j. ____________________________ 4. Write IONIC or COVALENT under each substance below to identify the type of bond. a. Calcium chloride b. Sulfur trioxide c. Phosphorus pentaflouride d. Sodium iodide e. Carbon monoxide e. Cesium fluoride 15 Gen Chem Unit 4: Chemical Compounds Ionic Bonding and Chemical Formulas When a chemical formula for a compound is written correctly, it shows the number of each type of atom in the compound. These numbers, called subscripts, are determined by the bonding between the atoms. The table shows two columns of elements. The elements in the first column usually give up electrons when they form compounds. The elements in the second column usually gain electrons when they form compounds. The column next to the elements gives the number of electrons found in the outer level of each element. Using this information, determine the charge on the ion after the exchange of electrons. Remember, atoms that give up electrons become positive ions, while atoms that gain electrons become negative ions. Now, show how the positive ion would combine with the negative ion to make a neutral compound. For example, sodium (Na) has one electron in its outer level. It gives up this electron and becomes a 1+ ion. Sulfur (S) having six electrons in its outer level gains two electrons to fill this outer level with eight electrons. Sulfur becomes 2- ion. These two ions then combine to form Na2S. This formula is correct because it takes two sodium ions to match the 2- charge on one sulfur ion. Element Sodium Electrons in the outer level 1 Charge on the ion +1 Element Sulfur Magnesium Bromine Sodium Oxygen Lithium Oxygen Calcium Phosphorus Barium Chlorine Beryllium Sulfur Strontium Fluorine Sodium Astatine Aluminum Oxygen Electrons in the outer level 6 Charge on the ion 2- Formula Na2S 16 Gen Chem Unit 4: Chemical Compounds Name: ____________________________ Date: _______________ Hour: _____ Information: Naming Ions To write an ion, you write the symbol of the atom and put the charge in the upper right corner. Consider the following examples: Al3+, O2-, Mg2+. You should verify that each of the charges is correct. Positive and negative ions are named differently. Positive ions retain the same name as the parent atom. For example, Al3+ is called the “aluminum ion” and Mg2+ is called the “magnesium ion.” Negative ions are named a little differently. For negative ions, you change the ending of the name to “-ide”. Therefore, O2- is named oxide and P3- is named phosphide. Critical Thinking Questions 1. Write the symbol (including the charge) and name for each of the ions for each of the following: a) Ca b) Cl c) N d) K e) S f) B g) P Information: Ionic Bonding and Formulas There are two ways in which atoms can “bond” to each other and form a compound. The means of bonding that we will consider now is called ionic bonding, which occurs between a metal and a nonmetal. As you know, opposite charges attract. Ionic bonding is when two ions of opposite charge attract and bond to each other forming an ionic compound. Consider the following examples of formulas for ionic compounds: • • • • One Na+ (sodium ion) and one Cl- (chloride ion) bond to make NaCl, “sodium chloride.” One Mg2+ (magnesium ion) and two F- (fluoride ion) bond to make MgF2, “magnesium fluoride.” Three Ca2+ (calcium ion) and two N3- (nitride ion) bond to make Ca3N2, “calcium nitride.” One Al3+ (aluminum ion) and one N3- (nitride ion) bond to make AlN, “aluminum nitride.” The small numbers at the bottom right of each symbol in a formula are called “subscripts”. Subscripts tell us how many of each type of atom are present. For example in the formula Mg3N2 there are three magnesium ions and two nitride ions. 17 Gen Chem Unit 4: Chemical Compounds Critical Thinking Questions 2. Consider the formula NaCl in the above example. It tells us that one Na+ ion is bonded to one Cl- ion. What is the overall charge for NaCl? Is it positive, negative, or neutral? 3. Consider MgF2. This formula tells us that one Mg2+ ion bonds with two F- ions. What is the overall charge on MgF2? 4. What is the overall charge on any ionic compound? 5. Why is calcium nitride written like Ca3N2 and not something like CaN2 or Ca2N3? In other words why do exactly three calcium ions bond with exactly two nitride ions? 6. The formula Ca3N2 can never be written as N2Ca3. To find out why, take note of each of the four example formulas given above. a) In terms of charge, what do the first ions named all have in common? b) In terms of charge, what do the second ions named all have in common? c) Now, why can’t Ca3N2 ever be written like N2Ca3? 7. There are two rules to follow when writing formulas for ionic compounds. One has to do with charges (see questions 4 and 5) and the other has to do with which atom to write first and which one to write second (see question 6). What are these two rules? 8. What is wrong with the following formulas? a) Al2S b) PNa3 c) Mg2S2 18 Gen Chem Unit 4: Chemical Compounds 9. Write the formula and name for the compound that forms when the following atoms form ionic compounds. The first is done for you. a) nitrogen and sodium b) barium and sulfur c) magnesium and iodine Na3N sodium nitride d) oxygen and aluminum e) calcium and phosphorus f) sodium and sulfur 10. Given the following compounds, determine the charge on the unknown ion “X”. a) X2S b) MgX c) X3P2 19 Gen Chem Unit 4: Chemical Compounds Formula Writing for Binary Ionic Compounds Write the formula for the following binary compounds. 1. sodium bromide ________________________________________________ 2. manganese (IV) oxide ________________________________________________ 3. iron (II) sulfide ________________________________________________ 4. barium nitride ________________________________________________ 5. silver chloride ________________________________________________ 6. copper (II) oxide ________________________________________________ 7. nickel (II) bromide ________________________________________________ 8. magnesium phosphide ________________________________________________ 9. aluminum iodide ________________________________________________ 10. calcium oxide ________________________________________________ 11. strontium arsenide ________________________________________________ 12. lead (IV) chloride ________________________________________________ 13. silver selenide ________________________________________________ 14. copper (I) phosphide ________________________________________________ 15. magnesium chloride ________________________________________________ 16. thallium (VI) oxide ________________________________________________ 17. barium iodide ________________________________________________ 18. iron (I) bromide ________________________________________________ 19. Lithium bromide ________________________________________________ 20. palladium (III) sulfide ________________________________________________ WHAT RULES DO I NEED TO REMEMBER TO ANSWER THESE QUESTIONS? 20 Gen Chem Unit 4: Chemical Compounds Nomenclature Writing for Binary Ionic Compounds Write the name for the following binary ionic compounds. 1. CaBr2 ________________________________________________ 2. AlCl3 ________________________________________________ 3. Zn3N2 ________________________________________________ 4. KCl ________________________________________________ 5. Na2S ________________________________________________ 6. AlN ________________________________________________ 7. CsI ________________________________________________ 8. Ca3P2 ________________________________________________ 9. BaO ________________________________________________ 10. BeF2 ________________________________________________ 11. FeCl2 ________________________________________________ 12. FeCl3 ________________________________________________ 13. Ag2O ________________________________________________ 14. CuS ________________________________________________ 15. CoP ________________________________________________ 16. MnBr3 ________________________________________________ 17. NiN ________________________________________________ 18. ZnF2 ________________________________________________ 19. VO2 ________________________________________________ WHAT RULES DO I NEED TO REMEMBER TO ANSWER THESE QUESTIONS? 21 Gen Chem Unit 4: Chemical Compounds Formula Writing for Polyatomic Ionic Compounds Write the formulas for the following polyatomic ionic compounds. 1. sodium hydroxide ________________________________________________ 2. iron (III) sulfate ________________________________________________ 3. potassium permanganate ________________________________________________ 4. copper (II) hydroxide ________________________________________________ 5. ammonium sulfide ________________________________________________ 6. ammonium sulfate ________________________________________________ 7. mercury (I) sulfite ________________________________________________ 8. magnesium phosphate ________________________________________________ 9. cobalt (IV) bicarbonate ________________________________________________ 10. zinc bicarbonate ________________________________________________ 11. aluminum phosphate ________________________________________________ 12. lithium carbonate ________________________________________________ 13. strontium acetate ________________________________________________ 14. copper (II) nitrate ________________________________________________ 15. sodium phosphite ________________________________________________ 16. rubidium carbonate ________________________________________________ 17. tin (II) thiocyanate ________________________________________________ 18. ammonium arsenate ________________________________________________ 19. iron (II) hydroxide ________________________________________________ 20. manganese (VI) carbonate ______________________________________________ WHAT RULES DO I NEED TO REMEMBER TO ANSWER THESE QUESTIONS? 22 Gen Chem Unit 4: Chemical Compounds Nomenclature Writing for Polyatomic Ionic Compounds Write the names for the following polyatomic ionic compounds. 1. Cs2(Cr2O7) ________________________________________________ 2. K2(SO4) ________________________________________________ 3. (NH4)2SO4 ________________________________________________ 4. Co(ClO3)3 ________________________________________________ 5. NiPO4 ________________________________________________ 6. Fe(NO3)3 ________________________________________________ 7. MgCrO4 ________________________________________________ 8. CaCO3 ________________________________________________ 9. KMnO4 ________________________________________________ 10. NaC2H3O2 ________________________________________________ 11. PbCrO4 ________________________________________________ 12. CoPO4 ________________________________________________ 13. NiCr2O7 ________________________________________________ 14. (NH4)2SO3 ________________________________________________ 15. KClO3 ________________________________________________ 16. Os3(PO3)2 ________________________________________________ 17. ZrHCO3 ________________________________________________ WHAT RULES DO I NEED TO REMEMBER TO ANSWER THESE QUESTIONS? 23 Gen Chem Unit 4: Chemical Compounds Chemical Formulas Pairs Check Directions: Write the chemical formula for each word formula listed. Check your partner as they are completing their formula. Praise or coach each other until both partners understand all sixteen formulas. 1. Sodium Chloride 2. Magnesium Oxide ______________________________ _______________________________ 3. Aluminum Sulfide 4. Potassium Oxide ______________________________ _______________________________ 5. Calcium Chloride 6. Lithium Nitride ______________________________ _______________________________ 7. Lead (II) Oxide 8. Iron (III) Flouride ______________________________ _______________________________ 9. Copper (I) Flouride 10. Zinc Oxide ______________________________ _______________________________ 11. Rubidium Bromide 12. Potassium Chloride ______________________________ _______________________________ 13. Titanium (III) Sulfide 14. Calcium Iodide ______________________________ _______________________________ 15. Lithium Phosphide 16. Silver Oxide ______________________________ _______________________________ 24 Gen Chem Unit 4: Chemical Compounds Bond with a Classmate When you find another ion with which you can bond, write in each symbol and charge. Then write the new compound formed by combining the two. Give the compound’s name. Remember-positive ions can only bond with negative ions and vice versa!!! Cation Mg2+ Cl- Anion Compound MgCl2 Name Magnesium Chloride 25 Gen Chem Unit 4: Chemical Compounds Supplemental Problems Section 7.1 (p.193) 3) How can you determine the # of valence e- in an atom of a representative element? 4) Atoms of which elements tend to gain e-? Atoms of which elements tend to lose e-? 5) How do cations form? 6) How to anions forms? 7) How many valence e- are in each atom? a. potassium b. carbon c. magnesium d. oxygen 9) How many e- will each element gain or lose in forming an ion? a. calcium (Ca) b. fluorine (F) c. aluminum (Al) d. oxygen (O) Section 7.2 14) How can you describe the electrical charge of an ionic compound? 15) What properties characterize compounds? 16) Define an ionic bond. 20) What pairs of elements are likely to form ionic compounds? Explain your answers. a. Cl, Br b. Li, Cl c. K, He d. I, Na 26 Gen Chem Unit 4: Chemical Compounds Section 7.3 (p.203) 26) Describe what is meant by ductile and malleable. 27) Why is it possible to bend metals but not ionic crystals? Standardized Test Prep (p.211) 1. Which of these is not an ionic compound? Circle your answer. A. KF b. Na2SO4 c. SiO2 d. Na2O 3. How many valence electrons does arsenic have? a. 5 b. 4 c. 3 d. 2 4. For which compound name is the incorrect formula given? a. magnesium iodide, MgI2 b. potassium selenide, K2Se c. calcium oxide, Ca2O2 d. aluminum sulfide, Al2S3 6. When a bromine atom gains an electron a. a bromide ion is formed. b. the ion formed has a 1- charge. c. the ion formed is an anion. d. all the above are correct. 27 Gen Chem Unit 4: Chemical Compounds ! " # ! ! & ' " " # $% $ ( ! ) $ $ * $ + , - . ( ! $0 " ( # / 1 2 $ $ $ $ $ 28 Gen Chem Unit 4: Chemical Compounds 3 4 ! ) "! 56 ! ! " #! ) ) "! 7 "$ # " " ! $ ) ! )8 .6 " # ! "9/ % ! ! ! ! : " $ " ! " $ 8 # $ 29 Gen Chem Unit 4: Chemical Compounds Formula Writing for Covalent Compounds Write the formulas for the following covalent compounds. 1. Carbon dioxide ________________________________________________ 2. Nitrogen dioxide ________________________________________________ 3. Dinitrogen monoxide ________________________________________________ 4. Sulfur trioxide ________________________________________________ 5. Tetraphosphorus decaoxide ______________________________________________ 6. Silicon tetraoxide ________________________________________________ 7. Boron trichloride ________________________________________________ 8. Phosphorus pentafluoride ________________________________________________ 9. Tellurium hexabromide ________________________________________________ 10. Diarsenic pentoxide ________________________________________________ 11. Diphosphorus pentasulfide ______________________________________________ 12. Xenon tetrafluoride ________________________________________________ 13. Selenium Diiodide ________________________________________________ Write the formulas for the following acids. 14. Hydrochloric Acid ________________________________________________ 15. Sulfuric Acid ________________________________________________ 16. Acetic Acid ________________________________________________ 17. Phosphoric Acid ________________________________________________ 18. Nitric Acid ________________________________________________ 19. Carbonic Acid ________________________________________________ 30 Gen Chem Unit 4: Chemical Compounds Name Writing for Covalent Bonds and Acids Write the name for the following covalent and acidic molecules. 1. H2CO3 ________________________________________________ 2. CCl4 ________________________________________________ 3. SF3 ________________________________________________ 4. HCl ________________________________________________ 5. N2O ________________________________________________ 6. NO2 ________________________________________________ 7. P4O10 ________________________________________________ 8. PO3 ________________________________________________ 9. H3PO4 ________________________________________________ 10. XeF4 ________________________________________________ 11. PF3 ________________________________________________ 12. ICl ________________________________________________ 13. KrCl2 ________________________________________________ 14. SiO2 ________________________________________________ 15. HC2H3O2 ________________________________________________ 16. Se2S4 ________________________________________________ 17. SO3 ________________________________________________ 18. H2SO4 ________________________________________________ 19. TeI2 ________________________________________________ 20. AsBr3 ________________________________________________ 31 Gen Chem Unit 4: Chemical Compounds 6 #" ! " " " ! "$ ' ) $ 96 ! ! " ) # " #" " # ( " ! $% " "; $6 $< ! # "# ! ! ! " ) $< ! "# ! " $% $% & $% ,$ % #$ 4 " ) ) ( " % ) "# " ) ) ) ) = ) ) " " ( # ) ) $ & 9 " " $0 ! " "; ) ) " ") " " "$ < ! #" ) ) ( ( 9 9 9 ' > ! 4 " ) + @@! ! ! $ 0 B( B( ( ? $ )@ ) ) @@! ! ! $ ( ! $ @ ! "! 4 " ) + @@! ! ! $ C C 4 +A ) ! ) " ) $ 4 " 4 " 4 " $ ) @ " " @ " 4 +A @ A$ ( $ @ "@ $ 32 Gen Chem Unit 4: Chemical Compounds 4 " ? ) + ( C @@( $ @ 4 +A - 4 " 4 ) + ( @@! ! ! $ ) 4 " ) 4 " ) @@! ! ! $ ( @F $ D > $ "4 @ ) " B ) ) ; E @ ! @) ( C ( $ $ 2 @ $ ( $G $% " ! ! " 6 " ( ) " " ( $ < 4 " 9 ) + ( " " " # " ! HC 3 C ! $+ " ! 9 # " ! )$ ' ( " # ! ) " $ > ! ) ) " ! ( * ' $ + ' ' , + ) , + ) , %!@ ! G G G %- ! !@ 33 Gen Chem Unit 4: Chemical Compounds 0 0 0 + ) , %!@ ! A 4 +A A I . A A , 8 0 0 , I ) Write opinion paper here: 34 Gen Chem Unit 4: Chemical Compounds Covalent & Ionic Bonding Lab Materials Distilled water Ethanol Salicylic acid Sodium carbonate Test tubes (8) Sodium chloride Sucrose 250 mL beakers (3) 400 mL beakers (2) Graduated cylinder Bunsen burner Conductivity tester Test tube holder Stoppers (4) Procedure Part 1: Melting Point Heat 0.5 g of each substance in a test tube, using a test tube holder, over a Bunsen burner for 30 seconds. Hold the test tube so that the bottom of the test tube is held above the inner blue cone of the flame. Observe and record whether any melting occurs. Do this for all four substances: salicylic acid, sodium carbonate, sodium chloride, sucrose. Part 2: Solubility in Water For this part it is important that all of the glassware is extremely clean! Place 0.25 g of the four substances, salicylic acid, sodium carbonate, sodium chloride, sucrose, in its own test tube. Add 5.0 mL of distilled water to each test tube, stopper, and shake. Observe and record whether or not the substances dissolve. Part 3: Conductivity For this part it is important that all of the glassware is extremely clean! For those substances that dissolved in water, pour the solutions into a 250 mL beaker, adding more distilled water if necessary to cover the bottom of the beaker. Use the conductivity tester to determine whether the solutions conduct electricity. Make sure that you clean off the conductivity tester leads between tests with distilled water. Part 4: Solubility in Ethanol Follow the same procedure as part 2, but use ethanol in place of water as the solvent. 35 Gen Chem Unit 4: Chemical Compounds Data Table: Salicylic acid Sodium chloride Sucrose Sodium carbonate Melting Solubility in Water Solubility in Ethanol Conductivity (dissolved in water) Questions 1) Using your textbook, identify properties of ionic and covalent compounds. 2) According to the data collected in the lab, which of the four compounds are ionic and which are covalent. Explain your reasoning. 3) A ceramic company wants to put a glaze on their product so that it gives it a nice shine. The four compounds in this lab are the choices they are considering. The glaze must be able to withstand high temperatures, is soluble in water, and must conduct electricity when dissolved. According to your data, which compound(s) would be appropriate for the company’s needs? Conclusion 1) Was the purpose achieved? Support your answer with your data. 2) Two examples of events the affected your data. Where they errors or mistakes? 3) What principle(s) of chemistry were present in this lab? 36 Gen Chem Unit 4: Chemical Compounds Compound Naming Race Be the first team in the room to correctly get all the formulas on this sheet right. When you have finished the first ten problems, bring them up to the teacher to be checked. Once these have been checked, move to the second ten. Once all forty problems have been solved, you’re the winner! 1) copper (II) acetate __________________ 2) sodium hydroxide __________________ 3) lithium oxide __________________ 4) cobalt (III) carbonate __________________ 5) aluminum sulfide __________________ 6) ammonium cyanide __________________ 7) iron (III) phosphide __________________ 8) vanadium (V) phosphate __________________ 9) sodium permanganate __________________ 10) manganese (III) fluoride __________________ 11) beryllium nitrate __________________ 12) nickel (III) sulfite __________________ 13) potassium oxide __________________ 14) silver bromide __________________ 15) zinc phosphate __________________ 16) copper (II) bicarbonate __________________ 17) nickel (II) selenide __________________ 18) manganese (IV) carbonate __________________ 19) lead (IV) nitride __________________ 20) tin (II) hydroxide __________________ 37 Gen Chem Unit 4: Chemical Compounds 21) lithium arsenide __________________ 22) chromium (VI) sulfate __________________ 23) calcium bromide __________________ 24) ammonium sulfate __________________ 25) copper (II) oxide __________________ 26) platinum (IV) phosphate __________________ 27) aluminum carbonate __________________ 28) silver nitrate __________________ 29) magnesium acetate __________________ 30) nickel (III) cyanide __________________ 31) vanadium (IV) phosphate __________________ 32) silver sulfate __________________ 33) cobalt (III) sulfide __________________ 34) iron (II) sulfite __________________ 35) copper (II) nitrite __________________ 36) nickel (II) hydroxide __________________ 37) zinc nitride __________________ 38) manganese (VII) nitrate __________________ 39) gallium sulfate __________________ 40) sodium nitrate __________________ 38 Gen Chem Unit 4: Chemical Compounds Ultimate Nomenclature Given the name, identify each of the following as Ionic (I), covalent (C), or acid (A). Then, write the formula. _____ 1. sulfuric acid __________________________________________ _____ 2. sodium hydroxide __________________________________________ _____ 3. sodium bromide __________________________________________ _____ 4. barium hydroxide __________________________________________ _____ 5. manganese (IV) oxide __________________________________________ _____ 6. sulfur dioxide __________________________________________ _____ 7. iron (II) sulfide __________________________________________ _____ 8. hydrochloric acid __________________________________________ _____ 9. potassium permanganate __________________________________________ _____ 10. sulfur trioxide __________________________________________ _____ 11. copper (II) hydroxide __________________________________________ _____ 12. ammonium sulfide __________________________________________ _____ 13. nickel (II) bromide __________________________________________ _____ 14. iron (II) oxide __________________________________________ _____ 15. acetic acid __________________________________________ _____ 16. ammonium chlorate __________________________________________ _____ 17. diarsenic pentoxide __________________________________________ _____ 18. iron (III) oxide __________________________________________ _____ 19. magnesium phosphate __________________________________________ _____ 20. nickel (III) bicarbonate __________________________________________ _____ 21. zinc carbonate __________________________________________ 39 Gen Chem Unit 4: Chemical Compounds _____ 22. diphosphorus pentoxide __________________________________________ _____ 23. aluminum phosphate __________________________________________ _____ 24. thallium (I) oxide __________________________________________ _____ 25. nitric acid __________________________________________ _____ 26. lithium sulfite __________________________________________ _____ 27. carbon monoxide __________________________________________ _____ 28. strontium acetate __________________________________________ _____ 29. copper (II) nitrate __________________________________________ _____ 30. phosphorus trichloride __________________________________________ _____ 31. nitrogen dioxide __________________________________________ _____ 32. sodium phosphate __________________________________________ _____ 33. phosphoric acid __________________________________________ _____ 34. lead (IV) chloride __________________________________________ _____ 35. tin (II) hydroxide __________________________________________ _____ 36. ammonium hydroxide __________________________________________ _____ 37. carbon dioxide __________________________________________ _____ 38. dinitrogen perntoxide __________________________________________ _____ 39. silver oxide __________________________________________ _____ 40. aluminum nitride __________________________________________ _____ 41. xenon tetrafluoride __________________________________________ _____ 42. zinc oxide __________________________________________ _____ 43. beryllium sulfide __________________________________________ _____ 44. silicon tetraoxide __________________________________________ 40 Gen Chem Unit 4: Chemical Compounds Given the formula, identify each of the following as Ionic (I), covalent (C), or acid (A). Then, write the name. _____ 1. CaCO3 ________________________________________________ _____ 2. FeO ________________________________________________ _____ 3. H2CO3 ________________________________________________ _____ 4. AgCl ________________________________________________ _____ 5. N2O ________________________________________________ _____ 6. Ba(OH)2 ________________________________________________ _____ 7. Na2S ________________________________________________ _____ 8. KrCl2 ________________________________________________ _____ 9. H3PO4 ________________________________________________ _____ 10. (NH4)2SO4 ________________________________________________ _____ 11. HC2H3O2 ________________________________________________ _____ 12. Zn(NO2)2 ________________________________________________ _____ 13. CuSO4 ________________________________________________ _____ 14. XeF4 ________________________________________________ _____ 15. NaOH ________________________________________________ _____ 16. PbCl2 ________________________________________________ _____ 17. SO3 ________________________________________________ _____ 18. NH4NO2 ________________________________________________ _____ 19. Ca(HCO3)2 ________________________________________________ _____ 20. Ba(ClO3)2 ________________________________________________ _____ 21. RhCN ________________________________________________ _____ 22. SF3 ________________________________________________ 41 Gen Chem Unit 4: Chemical Compounds _____ 23. K2SO3 ________________________________________________ _____ 24. Hg(OH)2 ________________________________________________ _____ 25. Cu2S ________________________________________________ _____ 26. KHCO3 ________________________________________________ _____ 27. AlBr3 ________________________________________________ _____ 28. CCl4 ________________________________________________ _____ 29. NaClO4 ________________________________________________ _____ 30. Be3N2 ________________________________________________ _____ 31. Cs2Cr2O7 ________________________________________________ _____ 32. Fe2(CrO4)3 ________________________________________________ _____ 33. AlCl3 ________________________________________________ _____ 34. HCl ________________________________________________ _____ 35. NO2 ________________________________________________ _____ 36. NO2 ________________________________________________ _____ 37. KNO3 ________________________________________________ _____ 38. Mg(CN)2 ________________________________________________ _____ 39. Ca3(PO4)2 ________________________________________________ _____ 40. PbO2 ________________________________________________ _____ 41. P4O10 ________________________________________________ _____ 42. PO3 ________________________________________________ _____ 43. KF ________________________________________________ _____ 44. FeCl2 ________________________________________________ _____ 45. ICl ________________________________________________ 42