1. #9 Charge It Answers

2. 1) Why are Ne and Ar chemically stable? Because they have _____ valence electrons. 8 (full outer energy levels)

3. 2. Look at your Lewis Dot Structures for Group 1A elements. a. How many valence electrons do they have? ____ b. What does each atom want to do with its electrons? ____________ c. How many electrons do Group 1A atoms want to give away? ______ a. 1 b. Give it away c. 1 d. What is the charge for Group 1A ions? [hint – when they lose the 1 electron, they will have 1 more proton (+) than electrons (-)] _______ d. 1+

4. 3. Look at your Lewis Dot Structures for Group 2A elements. a. How many valence electrons do they have? ____ b. What does each atom want to do with its electrons? ____________ c. How many electrons do Group 2A atoms want to give away? ______ So these atoms will give away 2 electrons to become stable, which means they form ions. d. What is the charge for Group 2A ions? [hint – when they lose the 2 electrons, they will have 2 more protons (+) than electrons (-)] _______ a. 2 b. Give them away c. 2 d. 2+

5. 4. Look at your Lewis Dot Structures for Group 3A elements. a. How many valence electrons do they have? ____ b. What does each atom want to do with its electrons? ____________ c. How many electrons do Group 3A atoms want to give away? ______ So these atoms will give away 3 electrons to become stable, which means they form ions. D. What is the charge for Group 3A ions? [hint – when they lose the 3 electrons, they will have 3 more protons (+) than electrons (-)] _______ a. 3 b. Give them away c. 3 d. 3+

6. 5. Look at your Lewis Dot Structures for Group 4A elements. a. How many valence electrons do they have? ____ b. What does each atom want to do with its electrons?____________________ c. How many electrons do Group 4A atoms want to give away? ______ or how many will they steal? _______ So these atoms will give away or steal 4 electrons to become stable, which means they form ions. d. What is the charge for Group 4A ions? If they give away electrons? _______ If they steal electrons? _________ a. 4 b. Give them away/keep them/ share them c. 4 and 4 d. 4- or 4+

7. 6. Look at your Lewis Dot Structures for Group 5A elements. a. How many valence electrons do they have? ____ b. What does each atom want to do with its electrons?____________________ c. How many electrons do Group 5A atoms want to steal? _______ So these atoms will steal 3 electrons to become stable, which means they form ions. d. What is the charge for Group 5A ions? [hint – when they steal the 3 electrons, they will have 3 more e - s than p + s]_________ a. 5 b. Keep them c. 3 d. 3-

8. 7. Look at your Lewis Dot Structures for Group 6A elements. a. How many valence electrons do they have? ____ b. What does each atom want to do with its electrons?____________________ c. How many electrons do Group 6A atoms want to steal? _______ So these atoms will steal 2 electrons to become stable, which means they form ions. d. What is the charge for Group 6A ions? [hint – when they steal the 2 electrons, they will have 2 more e - s than p + s]_________ a. 6 b. Keep them c. 2 d. 2-

9. 8. Look at your Lewis Dot Structures for Group 7A elements. a. How many valence electrons do they have? ____ b. What does each atom want to do with its electrons?____________________ c. How many electrons do Group 7A atoms want to steal? _______ So these atoms will steal 1 electron to become stable, which means they form ions. d. What is the charge for Group 7A ions? [hint – when they steal the 1 electron, they will have 1 more e - s than p + s]_________ a. 7 b. Keep them c. 1 d. 1-

10. 9. Look at your Lewis Dot Structures for Group 8A elements. a. How many valence electrons do they have? ____ b. What does each atom want to do with its electrons?____________________ c. How many electrons do Group 8A atoms want to steal? _______ d. What is the charge for Group 8A ions?_________ a. 8 b. Keep them c. 0 d. 0

11. Questions Identify the oxidation numbers for each element and circle the CATIONS 1) 13 Al _____ 2) 35 Br _____ 3) 37 Rb _____ 4) 14 Si _______ 5) 1 H _____ 6) 8 O ______ 7) 4 Be ____ 8) List the metals from above - ______________________________ 9) Q -3 – explain how atom Q became ion Q with a -3 charge - 1- 3+ 1+ 4+-4+- 2- 2+ Al, Rb, Be (not Si it is a metalloid) It must lose 3 electrons