Student Workbook Physical Science Chemical Bonding- Chapter 20 Mr. Davis

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1 Broughton High School Name: Section 1 Chemical Bonding Chapter 20 Student Workbook Physical Science Chemical Bonding- Chapter 20 Mr. Davis

2 Broughton High School Chapter 20 Chemical Bonding Vocabulary Words Vocabulary Word Definition 2 1. Binary Compound 2. Chemical Bond 3. Chemical Formula 4. Covalent Bond 5. Hydrate 6. Ion 7. Ionic Bind 8. Molecule 9. Non Polar Molecule 10. Oxidation Number 11. Polar Molecule 12. Polyatomic Ion The Lewis Theory: Valence electrons, or the electrons in the outermost electron shell, have an essential role in chemical bonding. Ionic bonds are formed between atoms when electrons are transferred from one atom to another. Ionic bond is a bond between nonmetals and metals. Covalent bonds are formed between atoms when pairs of electrons are shared between atoms. A covalent bond is between two nonmetals. Electrons are transferred/shared so that each atom may reach a more stable electron configuration i.e. the noble gas configuration which contains 8 valence electrons. This is called octet rule. Student Workbook Physical Science Chemical Bonding- Chapter 20 Mr. Davis

3 Broughton High School 3 Metals & Non-Metals Metals Common characteristics: Metallic luster (shine) Generally solids at room temperature Malleable Ductile Conduct heat and electricity Exist as extended planes of atoms Combine with other metals to form alloys which have metallic characteristics Form positive ions, e.g. Na +, Mg 2+, and Al 3+ Nonmetals Common characteristics: Rarely have metallic luster (shine) Generally gases at room temperature Neither malleable nor ductile Poor conductors of heat and electricity Usually exist as molecules in their elemental form Combine with other nonmetals to form covalent Generally form negative ions, e.g. Cl -, SO 2-4, and N 3- The differences in the characteristics of metals and nonmetals can be explained by the following: 1. Metals have relatively few electrons in their valence shells. 2. Metals have lower ionization energies than nonmetals. 3. Metals have smaller electron affinities than nonmetals. 4. Metals have larger atoms than nonmetals. 1) As you move across a period, metallic character decreases and nonmetallic character increases. 2) As you move down a group, metallic character increases and nonmetallic character decreases. Semimetals (Metalloids) A class of 8 elements that have properties of both metals and nonmetals. B Si Ge As Sb Te Po At Common characteristics: Generally look metallic but are brittle (not malleable or ductile) Neither good conductors nor insulators; instead they are semiconductors. Student Workbook Physical Science Chemical Bonding- Chapter 20 Mr. Davis

4 Broughton High School Elements and their Symbols Directions: write the symbols for the following elements. 1. Oxygen 21. Xenon 2. Hydrogen 22. Arsenic 3. Chlorine 23. Gallium 4. Sodium 24. Chromium 5. Fluorine 25. Cobalt 6. Carbon 26. Krypton 7. Nitrogen 27. Vanadium 8. Helium 28. Aluminum 9. Copper 29. Mercury 10. Sulfur 30. Tin 11. Magnesium 31. Boron 12. Manganese 32. Nickel 13. Neon 33. Cadmium 14. Bromine 34. Beryllium 15. Silver 35. Polonium 16. Lead 36. Uranium 17. Iron 37. Cesium 18. Calcium 38. Strontium 19. Potassium 39. Palladium 20. Gold 40. Barium Directions: Write the name of the element that corresponds to each of the following symbols. 41. Cu 54. Sb 42. K 55. In 43. C 56. Ta 44. Au 57. Ce 45. Zn 58.Nb 46. Pb 59. I 47. At 60. In 48. Bi 49. W 50. Y 51. Mo 52. Rh 53. Zr 4 Student Workbook Physical Science Chemical Bonding- Chapter 20 Mr. Davis

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7 Broughton High School Number of Atoms in a Formula Directions: Determine the number of atoms in the following chemical formulas. 1. NaCl 2. H 2 SO 4 3. KNO 3 4. CaCl 2 5. C 2 H 6 6. Ba(OH) 2 7. NH 4 Br 8. Ca 3 (PO 4 ) 2 9. Al 2 (SO 4 ) Mg(NO 3 ) Cu(NO 3 ) KMnO H 2 O H 3 PO (NH 4 ) 3 PO Fe 2 O NaC 2 H 3 O Mg(C 2 H 3 O 2 ) Hg 2 Cl K 2 SO 3 7 Hint: Coefficients: Coefficients apply to the entire compound. You multiply the coefficients and the subscripts. Example: 2 H 2 S Atoms of Hydrogen = (2 X 2) = 4 Atoms of Sulfur = (2 X 1) = 2 Total Atoms equals = 6 atoms If there isn t a subscript behind an element, there is only one atom of that element. Student Workbook Physical Science Chemical Bonding- Chapter 20 Mr. Davis

8 Directions for each problem Broughton High School Practice Counting Atoms Worksheet 1. Write down the different elements in each compound. 2. Write down how many of that particular atom there are 3. How many atoms are there total in the compound. 8 Examples: A) MgCl 2 Mg 1 B) 5 ZnSO4 Zn 5 Cl 2 S 5 3 total O total 1) NaOH 2) 4 HNO 3 3) MgCl 2 4) 4 Li 2 O 5) 2 NaOH 6) Li 2 SO 4 7) 3 H 2 O 8) NaC 2 H 3 O 2 9) 3 Al 2 O 3 10) NH 4 Cl 11) 5 ZnSO 4 12) 7 C 2 S 2 SUPER STAR CHALLENGE! 13) 2 Sr 3 (PO 4 ) 2 14) 4 Al(OH) 3 15) Ca (C 2 H 3 O 2 ) 2 16) 4 Al 2 (SO 3 ) 3 17) 2 (NH 4 ) 3 PO 4 18) 4 Mg(OH) 2 Student Workbook Physical Science Chemical Bonding- Chapter 20 Mr. Davis

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10 Types of Chemical Bonds Ionic Bonds Broughton High School The ionic bond is formed by the attraction between oppositely charged ions. Ionic bonds are formed between metals and nonmetals. Remember that metal atoms lose one or more valence electrons in order to achieve a stable electron arrangement. When a metal atom loses electrons it forms a positive ion or cation. When nonmetals react they gain one or more electrons to reach a stable electron arrangement. When a nonmetal atom gains one or more electrons it forms a negative ion or anion. The metal cations donate electrons to the nonmetal anions so they stick together in an ionic compound. This means that ionic bonds are formed by the complete transfer of one or more electrons. Covalent Bond A covalent bond is formed between nonmetal atoms. The nonmetals are connected by a shared pair of valence electrons. Remember, nonmetals want to gain valence electrons to reach a stable arrangement. If there are no metal atoms around to give them electrons, nonmetal atoms share their valence electrons with other nonmetal atoms. Since the two atoms are using the same electrons they are stuck to each other in a neutral particle called a molecule. A molecule is a neutral particle of two or more atoms bonded to each other. Molecules may contain atoms of the same element such as N 2, O 2, and Cl 2 or they may contain atoms of different elements like H 2 O, NH 3, or C 6 H 12 O 6. Therefore, covalent bonding is found in nonmetallic elements and in nonmetallic compounds. Covalent bonds are intramolecular forces; that is, they are inside the molecule and hold the atoms together to make the molecule. Covalent bonds are strong bonds and it is difficult and requires a lot of energy to break a molecule apart into its atoms. However, since molecules are neutral one molecule does not have a strong electrical attraction for another molecule. The attractions between molecules are called intermolecular forces and these are weak forces. Covalent substances have low melting points and boiling points compared to ionic compounds or metals. At room temperature, covalent substances are gases, liquids or low melting point solids. They do not conduct electricity as solids or when molten and usually do not conduct when dissolved in water. 10 Student Workbook Physical Science Chemical Bonding- Chapter 20 Mr. Davis

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15 15 Chemical Bonding Worksheet Ionic Bond between a Metal and Non-Metal (M + NM) Covalent Bond between a Non-Metal and Non-Metal (NM + NM) Metallic Bond between a Metal and Metal (M+ M) Directions: 1. Determine if the elements in the following compounds are metals or non-metals 2. Describe the type of bonding that occurs in the compound. Compound Element 1 Element 2 Bond Type (Metal or non-metal?) (Metal or non-metal?) NO 2 N = non-metal O = non-metal covalent NaCl SO 2 PO 4 3- MgBr 2 CaO H 2 O K 2 O Cu-Zn alloy O 2 CuCl 2 NO 2 - TiO 2 HF Rb 2 S Au-Ag mixture Fe 2 O 3 C 6 H 12 O 22

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28 Nomenclature - (Naming Compounds) 28 Section A: Binary Compounds Metals and Non-Metals Name the 1 st Element Change the root of the 2 nd element with ide ending Name the Following Binary Compounds: Write Formulas for the following 1. NaF 14. Aluminum chloride 2. K 2 O 15. Lithium sulfide 3. LiBr 16. Calcium phosphide 4. CaCl Barium fluoride 5. BaS 18. Potassium oxide 6. BaF Sodium bromide 7. Na 2 S 20. Barium nitride 8. MgI Lithium oxide 9. K 3 N 22. Aluminum oxide 10. BeSe 23. Rubidium iodide 11. CO 24. Carbon dioxide 12. SO Nitrogen dioxide 13. N 2 O 26. Sulfur trioxide

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31 Section B: Transition Compounds Transition Metals and Non-Metals Broughton High School of Wake County Name the Transition Metal with a Roman Numeral 2- Change the root of the 2 nd Non-Metal with ide ending Name the Following Binary Compounds: Write Formulas for the following 1. CuCl 11. Mercury (II) sulfide 2. CuCl Copper (I) nitride 3. FeO 13. Iron (III) bromide 4. MnS 14. Mercury (I) oxide 5. Cr 2 O Silver fluoride 6. NiF Copper (II) oxide 7. SnCl Chromium (III) iodide 8. Ag 3 P 18. Nickel (II) bromide 9. ZnS 19. Tin (IV) sulfide 10. Hg 2 Cl Zinc oxide

32 Section C: Non-Metal & Non-Metal Compounds Broughton High School of Wake County 1. Non-Metals and Non-Metals 2. Name the 1 st element (with prefix if more than one atom) 3. Change the root of the 2 nd Non-Metal with ide ending 32 Name the Following Binary Compounds: Write Formulas for the following 1- SO Sulfur dioxide 2- AsCl Phosphorus trichloride 3- N 2 O Nitrogen monoxide 4- P 2 O Carbon tertafluoride 5- GeCl Dinitorgen pentoxide 6- XeF Sulfur trioxide 7- SF Carbon monoxide 8- NO Phosphorus pentachloride 9- SiO2 19. Arsenic tribromide 10- CO 20. Nirtogen triiodide Section D: Compounds with Polyatomic Ions Non-Metals and Non-Metals Name the 2 parts (ion names) Prefixes 1. (Mono) 2. (Di) 3. (Tri) 4. (Terta) Name the Following Binary Compounds: Write Formulas for the following 1- BaSO4 31. Aluminum sulfate 2- (NH 4 ) 2 CO Zinc nitrite 3- Li 2 SO Magnesium chlorate 4- CrPO Sodium bicarbonate 5- NaC 2 H 3 O Calcium hydroxide 6- BaOH 36. Copper (II) carbonate 7- Fe(NO 3 ) Ammonium sulfide 8- KCN 38. Iron (III) acetate 9- SrCrO Lithium bisulfate 10- CaCrO Strontium phosphate 11- Al(OH) Ammonium nitrate 12- BaCO Iron (II) chlorate 13- K 2 SO Sodium carbonate 14- ZNF Copper (II) chloride 15- Ca 3 (PO 4 ) Silver phosphate 16- Ag 2 S 46. Barium acetate 17- Na 3 N 47. Lithium hydroxide 18- ZNBr Zinc hydroxide 19- Fe(NO 3 ) Iron (II) iodide 20- H 2 SO Potassium carbonate 21- Cu 2 S 51. Silver nitrate 22- KBr 52. Copper( II) oxide 23- Fe 2 O Aluminum hydroxide 24- Cu(OH) Calcium sulfide 25- NiBr Ammonium carbonate 26- MgSO Sodium acetate 27- NH 4 Cl 57. Silver hydroxide 28- FeO 58. Iron(III) bromide 29- FeI Copper (I) nitrate 30- Ba(ClO 3 ) Lithium Fluoride

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35 Color the elements on the Periodic Table Broughton High School of Wake County 35

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