Unit 6 Practice Packet: Bonding PDF

PRACTICE PACKET UNIT 6: BONDING Regents Chemistry: Mr. Palermo Practice Packet Unit 6: Bonding Vocabulary: _______________ Lesson 1: __________________...

PRACTICE PACKET UNIT 6: BONDING Regents Chemistry: Mr. Palermo Practice Packet Unit 6: Bonding Vocabulary: _______________ Lesson 1: __________________ Lesson 2: __________________ Review: __________________ Lesson 3: __________________ Lesson 4: __________________ Lesson 5: __________________ Lesson 6: ___________________ 1 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING Vocabulary For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something to help you remember the word. Explain the word as if you were explaining it to an elementary school student. Give an example if you can. Don’t use the words given in your definition! Ionic Bond: ___________________________________________________________________________________________________________ Covalent Bond: _______________________________________________________________________________________________________ Metallic Bond: ________________________________________________________________________________________________________ Molecular: ____________________________________________________________________________________________________________ Sea of mobile electrons: _____________________________________________________________________________________________ Electronegativity: ____________________________________________________________________________________________________ Polar Bond: ___________________________________________________________________________________________________________ Nonpolar Bond: ______________________________________________________________________________________________________ Polar Molecule: ______________________________________________________________________________________________________ Nonpolar Molecule: __________________________________________________________________________________________________ Linear Molecule: _____________________________________________________________________________________________________ Bent Molecule: _______________________________________________________________________________________________________ Pyramidal Molecule: _________________________________________________________________________________________________ Tetrahedral Molecule: _______________________________________________________________________________________________ Shared pairs: ________________________________________________________________________________________________________ Unshared pairs: ______________________________________________________________________________________________________ Symmetrical: _________________________________________________________________________________________________________ Intermolecular Forces: ______________________________________________________________________________________________ Hydrogen Bonding: __________________________________________________________________________________________________ 2 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING INQUIRY LESSON1: SUBSTANCE MODEL #1: For each of the following substances, place the symbol of the first element in its spot on the periodic table using pen. Then, place the symbol of the second element in the substance in its spot on the periodic table using pencil. NaCl LiBr KF ZnCl2 Fe2O3 CuI2 Al2S3 QUESTIONS FOR SUBSTANCE MODEL #1: 1. Where are all the first elements located on the periodic table (symbols in pen)? 2. Based on your knowledge about the periodic table, what “classification” would you give these elements? Metal or Non-Metal? 3. Where are all the second elements located on the periodic table (symbols in pencil)? 4. Based on your knowledge about the periodic table, what “classification” would you give these elements? Metal or Non-Metal? 3 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING SUBSTANCE MODEL #2 For each of the following substances, place the symbol of the first element in its spot on the periodic table. Then, place the symbol of the second element in the substance in its spot on the periodic table. CCl4 P2O5 N2O4 NI3 PBr3 F2Se QUESTIONS FOR SUBSTANCE MODEL #2: 1. Where are all the first elements located on the periodic table? 2. Based on your knowledge about the periodic table, what “classification” would you give these elements? Metal or Non-Metal? 3. Where are all the second elements located on the periodic table? 4. Based on your knowledge about the periodic table, what “classification” would you give these elements? Metal or Non-Metal? 4 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING TYING IT TOGETHER: 1. MODEL 1 substances are called ionic compounds and MODEL 2 substances are called covalent molecules. Write a simple rule that will allow you to classify compounds as ionic or covalent on the basis of what you have learned from the model. 2. Did the subscripts (the little numbers shown in the compound formulas) provide any insight into determining whether a substance is ionic or covalent? Why or why not? ELEMENT EVALUATION: Fill in the following tables identifying the type of element present in the substance. Use “M” for metal, and “NM” for non-metal. 1ST ELEMENT 2nd ELEMENT CLASSIFICATION FORMULA (Metal Or Non Metal) (Metal Or Non Metal) (Ionic or Covalent?) NaBr SF6 CoBr2 BaS NO2 C6H6 CrCl3 Determine the Properties of Ionic and Covalent Substances (At your lab station, observe the properties of both ionic and covalent substances and write them in the table below. Ionic Properties Covalent Properties 5 www.mrpalermo.com  PRACTICE PACKET UNIT 6: BONDING LESSON 1: INTRO TO BONDING & TYPES OF BONDS Objective:  Identify whether a bond is being broken or formed based upon energy being absorbed or released  Distinguish between the three types of bonds and Decide which type of bond is present based upon the atoms involved  Classify a substance as Ionic, Covalent or Metallic based upon its properties 1. For each phrase, check either “bond breaking” or “bond forming” Bond Bond Breaking Forming a. Stability of the chemical system increases b. Energy is released c. Cl + Cl  Cl2 d. exothermic e. endothermic f. N2  N + N g. Energy is absorbed h. Stability of the chemical system decreases Complete the Venn diagram below with properties of ionic and Covalent Bonds: Ionic Bonds Covalent Bonds Bonds formed between two nonmetals are _______________ and involve the ____________ of electrons. Bonds formed between two atoms of the same metal involve a sea of _______________________ electrons. Bonds formed between metals and nonmetals are ____________ and involve the ___________ of electrons. 6 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING Describe the following as ionic, metallic, or covalent (molecular): NaCl _____ Al _____ Lithium _____ CO2 _____ C6H12O6 _____ Strontium bromide _____ Au _____ Ti _____ Tin (II) chloride _____ MgBr2 _____ K2O _____ Nitrogen (IV) oxide _____ Fe _____ CH4 _____ Hydrogen selenide _____ H2O _____ H2S _____ Copper (II) phosphate _____ Ca3(PO4)2 _____ PI3 _____ Lead (IV) nitrate _____ REGENTS PRACTICE ASSESS YOURSELF ON THIS LESSON: If you missed any regents practice questions you should see me for extra help and/or re-watch the lesson video assignment 7 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING LESSON 2: Bond Polarity Objective:  Assess compounds and identify the presence polyatomic ions  Describe the type of bonds present in a polyatomic ion 1. Electronegativity values generally _______________ down a group and ____________ across a period. 2. Metals tend to have ____________ electronegativity values and nonmetals are _____________ values. Fill in the table below determining if the substance is ionic or covalent. If it is covalent then determine the electronegativity difference to identify if the covalent bond is polar or nonpolar. Covalent Substance Ionic Electronegativity Polar Non Polar Difference 1. I2 2. PCl3 3. SiO2 4. Br2 5. CO2 6. NaCl 7. CH4 8. N2O5 9. NH3 10. KCl 11. Indicate which atom will have the positive charge and which will have the negative charge in the following polar bonds: H-Cl H-F S-F N-O 8 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING 12. Organize the following in order from least to most polar bonds: HCl, HF, H2O, NH3, HI 13. Identify and explain each bond drawn below: Type of Bond Explanation For each statement check if it describes ionic, polar covalent, nonpolar covalent, or metallic bonds: Ionic Polar Nonpolar Metallic Covalent Covalent 15. A transfer of electrons between two atoms 16. Positive nuclei dispersed in a sea of mobile electrons 17. Metals and nonmetals bonding 18. One atom loses, and another atom gains electrons 19. Two atoms share electrons equally 20. Metals bonding only 21. Electronegativity differences under 0.4 22. A bond resulting from electrostatic charges between opposite charged particles 23. Two atoms share electrons unequally 24. Nonmetals bonding only 25. Electronegativity differences over 0.4 and between 2 Non metals 9 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING REGENTS PRACTICE ASSESS YOURSELF ON THIS LESSON: If you missed any regents practice questions you should see me for extra help and/or re-watch the lesson video assignment 10 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING PROPERTIES OF BONDS REVIEW: 1. Imagine you shrunk yourself down to the size of a molecule and were placed inside a beaker of water. Draw what you would see after you dissolved NaCl in the water. 2. Why does NaCl(aq) conduct electricity but NaCl(s) does not? 3. Imagine you shrunk yourself down to the size of a molecule and were placed inside a beaker of water. Draw what you would see after you dissolved C6H12O6 in the water. 4. Why doesn’t C6H12O6 (aq) conduct electricity? 11 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING At each lab station is a substance to be tested. Using the conductivity tester, determine if the substance conducts in the solid phase and record in the table below. Now using the tester, determine if the substance conducts in solution (aq). Wipe of the end of the tester with a paper towel and move on to the next station. Use information in the table below to identify each compound as Ionic or Covalent Compounds. Substance Phase at Conductivity as Conductivity as a Melting Point Ionic or Room a pure solid liquid Covalent Temperature (aq or molten) A solid 1049oC B solid 223oC C liquid 20oC D solid 378oC E liquid -94oC F solid 650oC List the properties of Ionic compounds: _________________________________________________________ List the properties of Covalent compounds: ______________________________________________________ 5. For each example, check if it describes breaking or forming bonds: Breaking bonds Forming bonds The stability of the system increases N2  N + N Endothermic I + I  I2 The stability of the system decreases Exothermic 6. For each example provide the molecule, bond and determine when and if it conducts electricity: Type of Bond Type of Molecule Conducts electricity? (Metallic, ionic, covalent, (metallic, ionic, molecular) (check all that apply) both ionic and covalent) No (s) (l) (aq) a. Li2O b. AlCl3 c. F2 d. CH4 e. HI f. Fe g. Na3PO4 h. CaO 12 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING 7. Indicate which type of substance is described by each statement. Type of substance a.Can conduct electricity in the solid and liquid phases A soft substance whose atoms are held together by b. covalent bonds c. Low melting point and poor electrical conductor d. Can conduct electricity when aqueous or molten (liquid) e. Can be polar or nonpolar f. Can dissolve in water to produce mobile ions 8. Explain the following in terms of charged particles: a. liquid mercury is a good electrical conductor b. molten NaCl conducts electricity while solid NaCl does not c. an aqueous solution of KBr conducts electricity while solid KBr does not d. CH4 is a poor electrical conductor How do you rate your understanding so far? 4 I “get” it. 3 I am almost there 2 I need help 1 I need lots of help 13 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING INQUIRY ACTIVITY LESSON 3 Lewis Dot Lewis Dot Structure Becomes Metal or Gain or lose How Element Structure of Stable ION like which Nonmetal electrons? many e- as an ATOM noble gas? Lithium Aluminum Radium Fluorine Sulfur Phosphorous Recall that all compounds are neutral so the total charge must equal zero. Using your chart, draw Lewis structures for the following compounds: Lithium Fluoride Lithium Sulfide Lithium Phosphide Aluminum Fluoride Aluminum Sulfide Aluminum Phosphide Radium Fluoride Radium Sulfide Radium Phosphide 1. Why do the metals bond with nonmetals? 2. What determines how many atoms of the metal and nonmetal will combine to form the compound? 14 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING LESSON 3: LEWIS (ELECTRON) DOT DIAGRAMS FOR IONIC COMPOUNDS Objective:  Construct Lewis diagrams for ionic compounds 1. Complete the table below (electron dot diagrams for ions) Electron- Electron Electron- Electron Ion dot Configuration Ion dot Configuration Diagram structure sodium oxide a. c. Na+ O2 aluminum bromide b. d. Al3+ Br 2. How many valence electrons do cations show in the Lewis dot diagrams? ____ anions? ____ 3. Draw the following LEWIS DOT DIAGRAMS for ionic compounds and give their formula and/or name: Lewis Diagram Formula Lewis Diagram Name Sodium fluoride CsCl Potassium oxide MgO Rubidium nitride SrI2 Calcium bromide BaS 15 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING Lewis Diagram Formula Lewis Diagram Name Strontium sulfide Fe2O3 Aluminum iodide CuO Copper (I) sulfide NiCl3 REGENTS PRACTICE ASSESS YOURSELF ON THIS LESSON: If you missed any regents practice questions you should see me for extra help and/or re-watch the lesson video assignment 16 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING LESSON 4: LEWIS (ELECTRON) DOT DIAGRAMS FOR COVALENT SUBSTANCES Objective:  Construct lewis dot diagrams for covalent compounds Complete the chart. Compound Total valence Lewis Diagram Shared pairs of Unshared pairs of electrons electrons electrons H2 2 H:H 1 0 F2 O2 H2O Cl2 NH3 CO2 CH4 17 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING Compound Total valence Lewis Diagram Shared pairs of Unshared pairs of electrons electrons electrons CCl4 N2 HF H2S REGENTS PRACTICE ASSESS YOURSELF ON THIS LESSON: If you missed any regents practice questions you should see me for extra help and/or re-watch the lesson video assignment 18 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING LESSON 5: MOLECULAR POLARITY Objective:  Determine the polarity of a molecule  Determine the shape of a molecule 1. Fill in the chart below. 2. In terms of lone pair electrons, how can you determine if a molecule is polar? 3. What molecular shapes are always polar? 4. What molecular shapes are always nonpolar? 5. How can a molecule be nonpolar if it contains polar bonds? 19 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING 6. Fill in the chart below Molecule Dot Diagram Distribution of Charge Molecular Polarity Molecular Shape (symmetrical or (polar or nonpolar (linear, pyramidal, asymmetrical) molecule) tetrahedral or bent) CO2 CH4 NH3 H2O REGENTS PRACTICE ASSESS YOURSELF ON THIS LESSON: If you missed any regents practice questions you should see me for extra help and/or re-watch the lesson video assignment 20 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING LESSON 6: INTERMOLECULAR FORCES (IMF’S) Objective:  Determine the type of intermolecular force that exists between covalent compounds 1. Fill in the table below: London Dipole-Dipole Hydrogen Bonds Dispersion Forces Forces **only force tested on Regents Type of molecule Strength Example In terms of Intermolecular Forces, to explain the following phenomenon: 2. Why does gasoline (C8H18) remain in the liquid phase but our Bunsen burner gas made out of the same elements (CH4) remain in the gas phase? 3. Why does dry ice (solid CO2) sublime (go from a solid directly to a gas) at room temperature but sugar and salt don’t even melt? 4. Which substance has the strongest intermolecular forces of attraction and which has the weakest? Molar mass Boiling Point (˚C) H2O 18.0 100 H2S 34.1 -62 H2Se 81.0 -42 H2Te 129.6 -2 21 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING 5. In terms of intermolecular forces, why does water have the highest boiling point in the table above? 6. Which substance has the strongest intermolecular forces of attraction and which has the weakest? Molar mass Boiling Point (˚C) HF 20.0 19 HCl 36.5 -84 HBr 80.9 -67 HI 12.9 -35 7. Why does HF have the highest boiling point in the table above? 8. Surface tension is a result of strong intermolecular forces. Which of the compounds in question 4 has the strongest surface tension? 9. Which of the following will have the higher boiling point? Explain your answer using intermolecular forces. NH3 or N2 22 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING REGENTS PRACTICE ASSESS YOURSELF ON THIS LESSON: If you missed any regents practice questions you should see me for extra help and/or re-watch the lesson video assignment 23 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING READING: NETWORK SOLIDS The best example of a network solid is a “diamond”. Look at the model of a diamond below. Note that the carbon atoms are bonded together with covalent bonds. The basic building unit is an atom of carbon. The structure has a very definite tetrahedral crystal shape, because these atoms are arranged and held rigidly in a fixed pattern. A diamond is very hard (a “10” on the Moh’s Scale of Hardness…the highest value possible). In order to scratch a diamond, you must break 1000’s of very strong covalent bonds! Similarly, to melt (or boil) a network solid, like a diamond, you must break 1000’s of these covalent bonds. This involves considerable energy and is the reason for their high melting points. It is because of these high temperatures and their hardness that network solids are frequently used in industry as “abrasives” (on sandpaper and on the tips of drills for cutting tools). You don’t have to worry about them melting if it gets too hot from friction or being scratched and dulled when contacting most other surfaces. Network solids have the type of properties you would expect from atoms being held together via strong covalent bonds, e.g. diamonds. They have very high melting points and are practically insoluble; are mostly nonconductors (no free electrons or ions); and they are very brittle (atoms must maintain a fixed crystal structure, if they are pushed too close together …. they repel). Graphite is also shown below. Note that it is also pure carbon, like a diamond. However, the covalent bonds only attach carbon atoms in 2 directions, not 3 like diamonds. The dashed lines between the layers of covalently bonded carbon atoms represent weak Van der Waal forces. Graphite is a 2 dimensional network solid. The strong covalent bonds only go in “plates”, in 2 directions. The “plates” are connected via weak VDW forces. Graphite STILL has a high melting point. – You must weaken/break all of its bonds (VDW and Covalent) to melt it. But since the weaker VDW forces are present and break easily, graphite is often used as a “dry lubricant”. If you squirt graphite dust into a lock, it will lodge between the lock’s moving metallic parts. When you put in a key and turn, the graphite structure will break apart between its “plates.” VDW’s break and make it turn more easily. Graphite also has free, “delocalized” electrons (it is a resonant structure… there really are no double bonds present, but free electrons) thus…graphite is a network solid that is capable of conducting electricity. This is not characteristic of most network solids. Of course, pencil lead is graphite. What bonds break when you write??? Silicon bonds like carbon to form a network structure. The computer industry depends on “silicon chips,” which are made conductive by placing impurities in their structure. These then provide for free electrons and allow the chip to do its job. But, pure silicon does not conduct. 24 www.mrpalermo.com PRACTICE PACKET UNIT 6: BONDING Many network solids are composed of various combinations of relatively few elements on the periodic table. The elements B, C, Al, Si are found in many network solids. They can be pure or combine with one another or combine with elements near them. For example, SiO2, quartz is an example of a network solid. Corundum, Al2O3, is a network and a common abrasive used on “sandpaper”. Many gemstones, like diamond, are network solids. Emerald is made of the mineral “beryl”. Its formula is Be3Al2 (Si6O18). Ruby is a form of corundum. 1. What is a Network solid? Give an example 2. What are some physical properties of Network solids? 25 www.mrpalermo.com