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Entry task: Nov. 1 st Friday

Entry task: Nov. 1 st Friday. *Sign up for a turning point clicker. Agenda:. Discuss Ch. 8 Review sheet Clicker Ch. 8 review HW: Ch. 3-8 review ws. I Can… Describe the formation of positive and negative ions. Define a chemical bond. Describe the properties of ionic substances

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Entry task: Nov. 1 st Friday

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  1. Entry task: Nov. 1st Friday *Sign up for a turning point clicker

  2. Agenda: • Discuss Ch. 8 Review sheet • Clicker Ch. 8 review • HW: Ch. 3-8 review ws

  3. I Can… • Describe the formation of positive and negative ions. • Define a chemical bond. • Describe the properties of ionic substances • Create and name binary ionic compounds and provide the mass of its formula. • Create polyatomic compounds formulas • Count the # of elements in a compound. • Check my formula with the given formula mass

  4. Clear off your deskHave out:ClickerCalculatorPeriodic tableCh. 8 review wswriting utensil

  5. What is a chemical bond? • A force that holds2 or more atoms together.

  6. Why do ions form? • They lose or gain electrons to have a stable electron arrangement.

  7. What family of elements is relatively unreactive and why? • Noble Gases are unreactive because they have a filled valence orbit.

  8. Describe the formation of cation and how does this relate to ionization energy? • Atoms lose their valence electrons becoming a positive chargebecause metals (cations) have low ionization energy.

  9. Describe the formation of anion and how does this relate to electronegativity? • Atoms gain electrons becoming a negative charge because they have high electronegativity “wanting” electrons.

  10. Explain the formation of the ionic compound composed of lithium and oxygen. • Oxygen gains both of those electrons becoming a -2 charge. • 2 Lithium atoms loses their valence electron becoming +1 charge. • They fill create a stable orbital arrangement • Cancel each other charges out.

  11. Provide the 5 properties of an Ionic substance. • High melting point • Dissolves in water • Conductive (after being dissolved in H2O) • Solids at room temperature • Brittle (not malleable)

  12. What is the difference between a formula unit, and crystal lattice? • Formula Unit is the simplest form of an ionic compound- NaCl. • Crystal Lattice is the repeating formula unit forming a lattice. NaClNaClNaClNaCl NaClNaClNaCl NaClNaClNaClNaCl NaClNaClNaCl

  13. What is the difference between a monatomic ion and a polyatomic ion? • Monatomic ion is a one atom ion. • Polyatomic ion is a 2 or more atoms that are covalently bonded that carry a charge.

  14. For the following, provide the correct names Fe2(SO3)3________________(H3O)3BO3________________Hg3(PO4)2________________Cu2CO3________________Al(NO3)3________________ Iron III sulfite Hydronium borate Mercury II phosphate Copper I carbonate Aluminum nitrate

  15. For the following, provide the formula & masses- SHOW YOUR WORK!!!Gallium cyanide- 121.76 g Ga+3 Ga is 69.723 g (1) = 69.723 g CN-1 C is 12.011 g (2) = 24.02 g Ga(CN)3 N is 14.007 g (2) = 28.01 g Formula masses = 121.76 g

  16. For the following, provide the formula & masses- SHOW YOUR WORK!!!Bismuth III chromate – 765.94 g Bi+3 Bi is 208.98 g (2) = 417.96 g CrO4-2 Cr is 51.996 g (3) = 155.988 g Bi2(CrO4)3 O is 15.999 g (12) = 191.988 g Formula masses = 765.94 g

  17. For the following, provide the formula & masses- SHOW YOUR WORK!!!Iron III hydroxide – 106.87 g Fe+3 Fe is 55.845 g (1) = 55.845 g OH-1 H is 1.0079 g (3) = 3.023 g Fe(OH)3 O is 15.999 g (3) = 47.997 g Formula masses = 106.87 g

  18. For the following, provide the formula & masses- SHOW YOUR WORK!!!Hydronium phosphide– 88.04 g H3O+1 P is 30.974 g (1) = 30.974 g P-3 H is 1.0079 g (9) = 9.071 g (H3O)3P O is 15.999 g (3) = 47.997 g Formula masses = 88.04 g

  19. For the following, provide the formula & masses- SHOW YOUR WORK!!!Copper I selenate – 270.40 g Cu+1 Cu is 63.723 g (2) = 127.446 g SeO4-2 Se is 78.96 g (9) = 78.96 g Cu2SeO4 O is 15.999 g (4) = 63.996 g Formula masses = 270.40 g

  20. Clicker ReviewIonic Bonding and Formulas

  21. In the periodic table, the elements are arranged in 
__________. 30 • alphabetical order • order of increasing atomic number • order of increasing metallic properties • order of increasing neutron content 23

  22. Elements __________ exhibit similar physical and chemical properties. 30 • in the same period of the periodic table • on opposite sides of the periodic table • in the same group of the periodic table • with similar atomic masses 21

  23. Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties? 30 • H, Li • C, O • Ga, Al • Cs, Ba 22

  24. Which one of the following is a nonmetal? 30 • W • Sr • Os • S 19

  25. Potassium is a __________ and chlorine 
is a __________. 30 • metal, nonmetal • metal, metal • metal, metalloid • metalloid, nonmetal 20

  26. How many valence electrons does 
Aluminum have? 30 • 5 • 3 • 7 • 13 23

  27. How many valence electrons does Barium have? 30 • 1 • 2 • 3 • 4 19

  28. Metals tend to __________ electrons and 
non metals tend to __________ electrons. 30 • gain, gain • lose, lose • gain, lose • lose, gain 22

  29. Anions tend to be __________ and cations 
tend to be __________. 30 • Metal, metal • nonmetals, nonmetals • metals, nonmetals • nonmetals, metals 20

  30. Nonmetals tend to be __________ and Metals
tend to be __________. 30 • Cations, anions • Anions, cations 22

  31. This is the ion formed from a calcium atom. 30 • Ca+ • Ca2+ • Ca- • Ca2- 19

  32. Barium forms an ion with a charge of __________. 30 • +1 • -2 • +3 • +2 17

  33. Aluminum forms an ion with a charge of 
__________. 30 • +1 • -2 • +3 • +2 24

  34. Of the following, __________ contains the 
greatest number of electrons. 30 • P+3 • P • P-2 • P-3 19

  35. Oxygen forms an ion with a charge of __________. 30 • -2 • +2 • -3 • +3 18

  36. Iodine forms an ion with a charge of __________. 30 • -7 • +1 • -1 • +3 17

  37. Which pair of atoms will form an ionic bond? 30 • Li & Ne • K & Br • K & Ca • S & Cl 23

  38. Which pair of atoms will form an ionic bond? 30 • Li & Be • Na & Mg • S & O • Rb & Cl 18

  39. Which of the following compounds would you 
expect to be ionic? 30 • S2 • SO2 • SrSO2 • SO2-2 15

  40. What is the correct formula for Aluminum sulfite? 30 • Al2(SO4)3 • Al3(SO3)2 • Al2(SO3)3 • Al(SO3)3 24

  41. What is the correct name for Pb(SeO4)2 30 • Lead selenate • Lead II selenate • Lead IV selenate • Lead II selenide 19

  42. What is the correct formula for Iron III chromate? 30 • Fe2(CrO4)3 • Fe3(CrO4)2 • Fe2CrO4 • Fe3CrO12 22

  43. What is the correct name for Mn(ClO3)2 30 • Manganese II chlorate • Magnesium IV chlorate • Manganese II chlorite • Manganese IV chlorate 18

  44. STUDY for P of UCh. 3-8For the LOVE OF PETEBring textbook to do HW

  45. Flip paper overTo Know ListSTUDY for P of UCh. 3-8

  46. To Know List- Ch. 8 Test • Concentration of MOSTLY Ch. 8 (75%) • Why bond? • Ionic substances- properties • Naming ionic substances • Providing the formula • Transitional metals- ROMAN NUMERALS • Binary compounds vs. polyatomic compounds

  47. To Know List- Ch. 8 Test • Concentration of MOSTLY Ch. 8 (75%) • Periodic trends- • Ionization energy • Electronegativity • Size of atoms verse ions • Energy levels-light, E-dot/valence-Ch. 5 • Particles- Protons, Electrons Neutrons-Ch. 4 • Physical chemical properties/changes-Ch. 3 25%

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