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Entry Task- Block #1 Nov. 6 th -7 th

Entry Task- Block #1 Nov. 6 th -7 th. QUESTION: What holds atoms together AND what subatomic particle is involved? You have 5 minutes!. Agenda: . Ionic vs. Covalent Substance Demo Go over Ch. 8 section 1-2 notes HW: Ch. 8 sec 1-2 ws. Ionic and Covalent Substances- Demo.

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Entry Task- Block #1 Nov. 6 th -7 th

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  1. Entry Task- Block #1 Nov. 6th-7th QUESTION: What holds atoms together AND what subatomic particle is involved? You have 5 minutes!

  2. Agenda: • Ionic vs. Covalent Substance Demo • Go over Ch. 8 section 1-2 notes • HW: Ch. 8 sec 1-2 ws

  3. Ionic and Covalent Substances- Demo

  4. Sodium chloride 800°C HIGH NaCl SOLID YES YES Copper II sulfate 600°C HIGH CuSO4 SOLID YES YES Isopropyl alcohol -88.0°C LOW (CH3)2COH Liquid YES NO 177 °C LOW Camphor C10H16O SOLID NO NO Potassium nitrate 306°C HIGH KNO3 SOLID YES YES 80.5 °C LOW Naphthalene C10H8 SOLID NO NO 113-114 °C LOW Iodine I2 SOLID NO NO Potassium Iodide 681°C HIGH SOLID YES YES KI

  5. THINK- to yourself • Write your answer on the answer sheet- • QUESTION #1 • What is the correlation- connection- between conduction and melting point? Sort the chemicals to make it easier.

  6. PAIR- WITH ELBOW PARTNER • QUESTION #1 • What is the correlation- connection- between conduction and melting point? • Tweak or add to your answer- discuss the best answer.

  7. THINK- to yourself • Write your answer on answer sheet • QUESTION #2 • What is the correlation between dissolving in water and conduction? Sort the chemicals to make it easier

  8. PAIR- WITH ELBOW PARTNER • QUESTION #2 • What is the correlation between dissolving in water and conduction? Sort the chemicals to make it easier • Tweak or add to your answer- discuss the best answer.

  9. THINK- to yourself • Write your answer on answer sheet • QUESTION #3 • Look at the formulas- look up (on periodic table) what kind of elements (metal/metalloid/nonmetal) makes up the substance. What is the correlation between substances with metal elements and melting point of the substance? Sort the chemicals to make it easier.

  10. PAIR- WITH ELBOW PARTNER • QUESTION #3 • Look at the formulas- look up (on periodic table) what kind of elements (metal/metalloid/nonmetal) makes up the substance. What is the correlation between substances with metal elements and melting point of the substance? Sort the chemicals to make it easier. • Tweak or add to your answer- discuss the best answer.

  11. THINK- to yourself • Write your answer on answer sheet • QUESTION #4 • Pulling it ALL together. What did you discover? What are the relationships that connect?

  12. PAIR- WITH ELBOW PARTNER • QUESTION #4 • Pulling it ALL together. What did you discover? What are the relationships that connect? • Tweak or add to your answer- discuss the best answer.

  13. Flip Papers over

  14. IONIC and COVALENT Substances Substances • Made of elements • Metals/metalloids/nonmetal • Chemically bonded • Ionic versus covalent Affect the substances properties

  15. If the Substance IONIC Substances Contain Metals!!! Ionic Bonds (Tight bonds)

  16. IONIC Substances Properties • Solids at room temperature • Hard and brittle • Dissolves in water • High melting points • Conductive after dissolving in water

  17. If the Substance COVALENT Substances Contain Nonmetals only!!! Covalent Bonds (Lose bonds)

  18. COVALENT SUBSTANCES Properties • Liquid/gas at room temperature • Does not dissolve in water • Low melting points • Not conductive

  19. Flip Papers over to the front

  20. Sodium chloride 800°C HIGH NaCl Ionic SOLID YES YES Copper II sulfate Ionic 600°C HIGH CuSO4 SOLID YES YES Isopropyl alcohol -88.0°C LOW Covalent (CH3)2COH Liquid YES NO Covalent 177 °C LOW Camphor C10H16O SOLID NO NO Potassium nitrate Ionic 306°C HIGH KNO3 SOLID YES YES Covalent 80.5 °C LOW Naphthalene C10H8 SOLID NO NO 113-114 °C LOW Iodine Covalent I2 SOLID NO NO Potassium Iodide 681°C HIGH SOLID YES YES Ionic KI

  21. I can…. • Define a chemical bond. • Describe the formation of positive and negative ions • Create and name binary ionic compounds.

  22. 8.1 Forming Chemical Bonds • DESCRIBE a chemical bond. The force that holds two atoms together. Chemical bonds may form by the attraction between the positive nucleus and negative electrons or the attraction between a positive ion and negative ion.

  23. 8.1 Forming Chemical Bonds • Provide the electron dot structures for groups 1A-8A.

  24. 8.1 Forming Chemical Bonds • RECALL from Ch. 6, what is ionization energy? Ionization energy is how easily an atom loses electrons.

  25. 8.1 Forming Chemical Bonds • What is electron affinity? How much attraction an atom has for electrons

  26. 8.1 Forming Chemical Bonds • State the octet rule? When atoms have 8 electrons in its valence orbit it’s chemically stable- like the noble gases

  27. 8.1 Forming Chemical Bonds • How are positive ions formed? What are they called? When atoms loses electrons they form positive ions called cations. Metals are cations

  28. 8.1 Forming Chemical Bonds 1+ • What are the charges on group 1A?_______ • What are the charges on group 2A________ • What are the charges on group 3A?_______ 2+ 3+

  29. Predicting Ionic Charges Group 1: Lose 1 electron to form 1+ ions H+ Li+ Na+ K+

  30. Predicting Ionic Charges Loses 3 electrons to form 3+ ions Group 13: B3+ Al3+ Ga3+

  31. Predicting Ionic Charges Lose 4 electrons or gain 4 electrons? Group 14: Depends! If it’s a metal it will lose 4 electrons = +4

  32. 8.1 Forming Chemical Bonds • What are pseudo-noble gas configurations? YOU NEED TO READ!! When the inner groups 4-6 lose electrons to fill their s, p, d orbitals by “stealing” from the higher s group. This forms a “fake (pseudo) noble gas configuration.

  33. 8.1 Forming Chemical Bonds • How are negative ions formed? What are they called? When atoms gain electrons they form negative ions called anions. Nonmetals are anions

  34. 8.1 Forming Chemical Bonds 3- • What are the charges on group 5A?_______ • What are the charges on group 6A________ • What are the charges on group 7A?_______ 2- 1-

  35. Predicting Ionic Charges Group 17: Gains 1 electron to form 1- ions F1- Fluoride Cl1- Chloride Br1- Bromide I1- Iodide

  36. Predicting Ionic Charges Group 18: Stable Noble gases do not form ions!

  37. Predicting Ionic Charges Many transition elements have more than one possible oxidation state. Groups 3 - 12: Iron(II) = Fe2+ Iron(III) = Fe3+

  38. Predicting Ionic Charges Some transition elements have only one possible oxidation state. Groups 3 - 12: Zinc =Zn2+ Silver = Ag+

  39. 8.2 The Formation & Nature of Ionic Bonds • Formation of an Ionic Bond- READ THIS PART!! • DESCRIBE an ionic bond When atoms transfer electrons creating a positive-negative ion, the electrostatic forces that hold these opposing particles together is called ionic bonding Transfer electrons +/- Metal-nonmetal Compound

  40. 8.2 The Formation & Nature of Ionic Bonds • What are ionic compounds? Compounds that contain ionic bonds are called ionic compounds Transfer electrons +/- Metal-nonmetal Compound

  41. 8.2 The Formation & Nature of Ionic Bonds • What are binary ionic compounds? Compounds that contain 2 different elements EXAMPLES: NaCl MgF2 Al2O3

  42. 8.2 The Formation & Nature of Ionic Bonds • Properties of Ionic Compounds • What are ionic crystals? When ionic compounds are packed in a repeated pattern of +/- they create an ionic crystal

  43. 8.2 The Formation & Nature of Ionic Bonds • Properties of Ionic Compounds • What are crystal lattices? Crystal lattices are three-dimensional geometric arrangement of particles. Each positive ion is surround by a negative ion

  44. 8.2 The Formation & Nature of Ionic Bonds • What specific properties do ionic crystals have? They have high melting and boiling points. The color is related to their structure. Brittle solids Dissolves in water Conductive (when dissolved in water) Electrolytes

  45. 8.2 The Formation & Nature of Ionic Bonds • What causes these particular properties? The bonded atoms have a strong attraction to each other (+/-).

  46. 8.2 The Formation & Nature of Ionic Bonds • What creates an electrolyte? When ionic compounds dissolve in water the ions are free from each other and conduct a current.

  47. 8.2 The Formation & Nature of Ionic Bonds • Energy and the ionic bond • What is an endothermic reaction? Exothermic? When energy is absorbed during a chemical reaction, the reaction is endothermic. When energy is released during a chemical reaction, the reaction is exothermic.

  48. 8.2 The Formation & Nature of Ionic Bonds • Energy and the ionic bond • The creation of an ionic bond is which type of energy reaction? Exothermic.

  49. 8.2 The Formation & Nature of Ionic Bonds • Energy and the ionic bond • What is lattice energy? What is the strength determined by? Lattice energy is the energy required to separate ions from each other in an ionic compound. The strength is determined by hold of each ion has to each other. The MORE negative the lattice energy the stronger the attraction

  50. 8.2 The Formation & Nature of Ionic Bonds • Energy and the ionic bond • How does the size of the ions affect lattice energy? The smaller the ion the MORE negative value for lattice energy (stronger the attraction). This is because the valence electrons are closer to the nucleus.

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