Topic 1 - Matter and Energy - Revsworld

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. Topic 4 – Chemical Bonding 10. Coordinate covalent bond: Definitions and examples Coordinate covalent bond is formed when both shared electrons are provided by ONLY one of the atoms. . This bond is formed when an H+ ( hydrogen ion), which does not have an electron, bonds with a molecule such as NH 3 (ammonia) or H 2 O (water). . NH 3 and H 2 O molecules have a lone pair (two unbonded) electrons that they can share with a H+ (hydrogen ion, proton) that doesn’t have any electron. Two (all you need to know) formulas containing a coordinate covalent bond NH 4 + (ammonium ion) forms from NH 3 (ammonia) and H + (hydrogen ion) H 3 O + (hydronium ion) forms from H 2 O (water) and H + (hydrogen ion) 11. Metallic bond: Definitions and facts Concept Facts: Study to remember these facts about metallic bonding. Metallic bonding is a force that holds metal atoms together in metallic substances. .Metallic bonding is described as positive ions “immersed in sea of mobile Valance electrons” . Mobile electrons allows for high electrical conductivity in metals Examples of formulas containing metallic bonds: Ca (calcium) Au (Gold) Fe (iron) (NOTE that substances containing metallic bonds are metallic elements) 12.Bond types: A summary table. Concept facts: Use this table for quick studying and comparisons Bond Type Metallic Type of elements involve in bonding metal atoms of the same element Bond description positive ions in sea of electrons Ionic metal - Nonmetal transfer of electrons Covalent nonmetals only sharing of electrons Polar covalent Nonpolar covalent Coordinate Covalent Network solid covalent Two different nonmetals same nonmetal (or nonmetal atoms with the same electronegativity) two different nonmetals nonmetals only unequal sharing equal sharing of electrons One atom provides both shared electrons No discrete particles Electronegativity difference -------------- Type of substances containing bond metallic substances 1.7 or greater ionic substances less than 1.7 greater than 0 but less than 1.7 zero ( 0 ) ------------------ ------------------- molecular substances polar and nonpolar substances diatomic nonpolar substances polyatomic ions network solids Example formula containing bond Copyright © 2011 E3 Scholastic Publishing. All Rights Reserved. 77 Ag K NaCl Li 2 O HCl H 2 O CH 4 H 2 O 2 NH 4 + H 3 O + C , SiC, SiO 2
Introduction Topic 4 – Chemical . Bonding Lesson 4 – Types of substances and their properties In the last lesson, you learned the different bond types found between atoms of different substances. For the most part, the bond name and the type of substances containing that bond are usually the same. For examples: 1. Ionic substances contain atoms held together by ionic bonds. 2. Metallic substances contain atoms held together by metallic bonds. 3. Network solid substances contain atoms held together by network solid bonds. 4. Molecular (Covalent) substances contain atoms held together by covalent bond 5. Polar molecular substances contain atoms held together by polar covalent bonds. 6. Nonpolar substances are the only substance which this is not always the case. A FEW nonpolar substances contain atoms held together by nonpolar bonds. BUT MOST nonpolar substances contain atoms held together by polar covalent bonds This exception will be explained later in this lesson. In this lesson, you will first learn of the four types of substances and their properties. Later, you will learn the relationship between bond polarity, molecular symmetry, molecular shape, and molecular polarity ( polar and nonpolar molecules). 14. Types of substance and their properties: Summary and facts: Concept facts Types of substance Phase at room Physical Properties (characteristics) temperature Melting point Conductivity Solubility (in water) Metallic Solid Very High Good (High) NO ( insoluble) (except Hg - liquid) (in Solid and Liquid phases) Ionic Solid only High Good (High) Yes (soluble) (in Liquid and Aqueous phases) Molecular solid, liquid, gas Low Poor (low) Yes (slightly soluble) (in all phases) Network solid Solid only Extremely high Very poor (in all phases) NO (Insoluble) More information about each type of substance are discussed in the next few page. 15.Example of the four types of substances and their melting points Below, solid forms of the four types of substances mentioned in the above table are given. NOTE the huge differences in temperatures at which each solid will melt at STP. Type of Molecular substance Ionic substance Metallic substance Network solid substance Example solid: Ice (H 2 O) Salt (NaCl) Gold (Au) Diamond ( C ) Melting point 0 o C 801 o C 1065 o C 3550 o C Copyright © 2011 E3 Scholastic Publishing. All Rights Reserved. 79
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Page 22 and 23: Introduction 4. The three types of
Page 24 and 25: . Topic 2 -The Periodic Table Atomi
Page 26 and 27: Topic 2 - The Periodic Table 18. Gr
Page 28 and 29: Concept Task: Be able to determine
Page 30 and 31: Topic 3 - The Atomic . structure To
Page 32 and 33: Topic 3 - The Atomic Structure . 10
Page 34 and 35: . Topic 3 - The Atomic Structure 17
Page 36 and 37: Lesson 3 - Electrons location and a
Page 38 and 39: 30. Spectral lines: Determining whi
Page 40 and 41: . Topic 3 - The Atomic Structure 36
Page 42 and 43: Topic 4 - Chemical . Bonding Topic
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Page 48 and 49: Topic 4 .- Chemical Bonding 25. Deg
Page 50 and 51: . Topic 4 - Chemical bonding 32. Le
Page 52 and 53: Topic 4 - Chemical . Bonding 38. Si
Page 54 and 55: . Topic 5 - Chemical formulas and e
Page 56 and 57: Lesson 3 - Writing and naming chemi
Page 58 and 59: Topic 5 - Chemical . formulas and e
Page 60 and 61: 18. cont. Topic 5 - Chemical . form
Page 66 and 67: . Topic 6 - Mole interpretation : M
Page 68 and 69: 6. Mass - mole relationship: Unders
Page 70 and 71: 12. . Percent composition of hydrat
Page 72 and 73: 16. Mole - mole problems: Calculati
Page 74 and 75: Topic 6 - Mole interpretation: Math
Page 76 and 77: 4. Properties of solution: Facts To
Page 78 and 79: Topic 7 - Solutions . 10. Soluble a
Page 80 and 81: Topic 7 - Solutions . 15. Saturated
Page 82 and 83: Topic 7 - Solutions . 21. The solub
Page 84 and 85: Topic 7 - Solutions . Lesson 5 : Bo
Page 86 and 87: Topic 7 - Solutions . 32. Effect of
Page 88 and 89: Topic 8 - Acids, . Bases and Salt T
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Topic 8 - Acids, . Bases and Salt 2
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Topic 8 - Acids, Bases . and Salt I
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Topic 8 - Acids, . Bases and Salt 3
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Topic 9 - Kinetics and . equilibriu
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Topic 9 - Kinetics . and equilibriu
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Concept Terms . Topic 9 - Kinetics
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Topic 10 - Organic . Chemistry 3. B
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Topic 10 - Organic . Chemistry 9. A
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Topic 10 - Organic . Chemistry 17.
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25. Ketones: Definitions, facts, an
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Topic 10 - Organic . Chemistry Less
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Topic 10 -. Organic Chemistry 39. c
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Topic 10 .- Organic Chemistry 42. A
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Topic 11 - Redox . and Electrochemi
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Topic 11 - Redox and Electrochemist
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14. Redox equations Topic 11 - Redo
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Topic 11 - Redox and . Electrochemi
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Topic 11 - Redox . and Electrochemi
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33. Electrolytic cells: Diagram and
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37. Electroplating: How does it wor
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Concept Terms Topic 11 - Redox . an
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Topic 12: Nuclear Chemistry . 4. Nu
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Topic 12: Nuclear . Chemistry 11. B
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Topic 12: Nuclear . Chemistry 17. F
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Topic 12: Nuclear . Chemistry 22. N
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Topic 12: Nuclear . Chemistry 26. R
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Topic 12: Nuclear . Chemistry 30. H
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. Topics Review Questions 317
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Constructive Response Questions Top
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Constructed Response Questions Topi
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. Topic 3 - The Atomic Structure Co
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Topic 4 - Chemical Bonding Construc
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. Topic 6 - Mole interpretation: Ma
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. Topic 7 - Solutions 23. According
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. Topic 8 - Acids, Bases, and Salts
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. 20. A potential energy diagram fo
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. 28. Given the reaction below: C 4
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Topic 11 - Redox and Electrochemist
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Topic 12: Nuclear . Chemistry Const
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Table G: Solubility Curves . Refere
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Table P: Organic Prefixes . Referen
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. Reference Tables 373
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C Glossary Calorimeter a device use
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Glossary . H cont. Half-reaction a
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P Glossary . Parts per million conc
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Index . Absolute zero 10 Accelerato
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Index . Law of conservation 113 - 1
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