2: Bonds, James Bonds Name: Unit 2 Reteach Packet Class: Date:

Transcription

1 2: Bonds, James Bonds Name: Unit 2 Reteach Packet Class: Date: Page 1 of 8 Use your table of elements to answer the following: 1. Explain how the staircase can be used to identify the metals, nonmetals, and metalloids. 2. Consider the electron configuration for the noble gases below. What do they all have in common? a. Ne: 1s 2 2s 2 2p 6 b. Ar: 1s 2 2s 2 2p 6 3s 2 3p 6 c. Kr: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 3. Provide an example for each of the following. Element Element A metal A transition metal A nonmetal A halogen A noble gas A diatomic gas An alkali metal A nonmetal liquid Which of the following would have the most similar properties? Why? a. Na and K b. Na and Mg c. Na and Ca d. Na and Al 5. Why is the radius of a chlorine atom smaller than the radius of a chloride ion (Cl -1 )?

2 6. Complete each of the following: Textbook Definition from Notes: Word: Atomic Radius Reminder Word: Use the Word and Reminder Word in a Sentence: Page 2 of 8 Draw a Picture of the Word: Word: Ionization Energy Reminder Word: Textbook Definition from Notes: Use the Word and Reminder Word in a Sentence: Draw a Picture of the Word: Word: Electronegativity Reminder Word: Textbook Definition from Notes: Use the Word and Reminder Word in a Sentence: Draw a Picture of the Word:

3 Page 3 of 8 7. Complete the table below by circling the element that best illustrates the given periodic trend; then explain your choice. Element (circle Trend Explain one) Smallest atomic radius Al, B, Ga Largest atomic radius Highest metallic character Highest first ionization energy Lowest first ionization energy Highest electronegativity Lowest electronegativity Most shielding F, Cl, Br As, Se, Br Oxygen, Sulfur, Selenium Gallium, Germanium, Arsenic N, O, F Boron, Carbon, Nitrogen Na, K, Rb Least positive nuclear charge Sn, Sb, Te 8. Explain the relationship between atomic radius and ionization energy.

4 9. Play one game of periodic trend war. Page 4 of 8 Directions: Each person gets one set of cards. There should be a total of seven cards per hand. The oldest person in the group rolls the dice twice to determine the periodic trend. o First roll: Even number (2,4,6): Highest Odd number (1, 3,5): Lowest o Second roll: 1: atomic radius 2: metallic character 3: ionization energy 4: electronegativity 5: shielding effect 6: wild, roller s choice Example: roll one: odd, lowest roll two: 2 metallic character cards chosen by players: F, C, Ca, Na winner: F Each player selects the card with the element on it that best represents that trend. The best card wins. Used cards go into a pile in the middle. All players write down the trend, cards drawn, and winner for the round. Next oldest person rolls the dice to begin the next round. Play until there are no more cards in your hand. Round 1 Highest or Lowest? Trend Elements Drawn Winning Element Winning Person

5 10. What kinds of elements are involved in each of the following? a. Ionic Page 5 of 8 b. Covalent c. Metallic d. Acid 11. What are the seven diatomic molecules? 12. Create flash cards to memorize the polyatomic ions (Quiz on 12/3): C2H3O2 acetate NO2 nitrite HCO3 hydrogen (bi)carbonate NO3 nitrate CO3 2 carbonate OH hydroxide ClO hypochlorite CN cyanide ClO2 chlorite PO4 3 phosphate ClO3 chlorate SO3 2 Sulfite ClO4 perchlorate SO4 2 sulfate

6 13. For each of the following compounds: a. Determine if ionic, molecular, or acid. b. Highlight polyatomic ions green. c. Circle cations that can have more than one charge. d. Highlight acidic hydrogens pink. e. Write the name or the formula. Page 6 of 8 Ionic, Molecular, or Acid? Name Formula Br2 sulfur trioxide (NH4)2SO4 tin(ii) sulfide HNO2 magnesium acetate Pb(CO3)2 hydrophosphoric acid N2O vanadium(v) hydrogen carbonate ZnF2 iron(iii) phosphate CCl4 dinitrogen trioxide H2SO4 fluorine Al(OH)3

7 2: Bonds, James Bonds Name: Optional Reteach Date: Class: The following items are not collected but are useful to help you prepare for the redo. Page 7 of 8 Atomic Trends (Questions 3, 4, 5, 7, 8) 1. Define electronegativity, ionization energy, and atomic radius. 2. Use shielding to explain each trend as you move down a column/ family/ group. a. Electronegativity b. Ionization Energy c. Atomic Radius 3. Use nuclear charge to explain each trend as you move across a period/ series/ row. a. Electronegativity b. Ionization Energy c. Atomic Radius 4. Explain what happens to the atomic radius when a cation forms. Explain what happens to the atomic radius when an anion forms. Periodic Table (Questions 1, 2, 6) 5. Color code on the table of elements on the back: metals, nonmetals, metalloids. Label the following: alkali metals, alkaline earth metals, halogens, noble gases. 6. Compare the properties of metals, nonmetals, and metalloids. VSEPR (Questions 16, 17) 7. Draw the Lewis structure of NH3. 8. Determine the VSEPR shape of NH3. Intermolecular Forces (Questions 18, 19, 21, 22, 23) 9. What are the three intermolecular forces and how do you know if a molecule has each one? 10. Explain how intermolecular forces can impact physical properties, such as boiling point? Bonding (Questions 12, 13, 15, 20) 11. Compare ionic and covalent bonds. Include how electrons behave and types of elements involved. 12. How many electrons are shared in single, double, and triple bonds? 13. Why do metals typically form cations when they form ionic bonds? Why do nonmetals typically form anions when they form ionic bonds? Formula Writing/ Naming (Questions 9, 10, 11, 14, 24, 25) 14. How do you know when an ionic formula is correct? 15. Explain how to name the following compounds: AlCl3, FeBr2, CO2, H3PO4 16. Explain how to write the following formulas: calcium chloride, iron(iii) oxide, sulfuric acid, carbon tetrafluoride

8 Page 8 of 8 On the central atom # of Bonded Atoms # of Lone Electron Pairs Molecular Shape 2 0 Linear 3 0 Trigonal planar 2 1 Bent 4 0 Tetrahedral 3 1 Trigonal pyramidal 2 2 Bent 5 0 Trigonal bipyramidal 4 1 Seesaw 3 2 T-shape 2 3 Linear 6 0 Octahedral 5 1 Square pyramidal 4 2 Square planar