1. 6.1 Ionic Bonding   HES Chemistry Unit: Ions and Ionic Bonds

2. 6.1 Ionic Bonding Learning Targets Describe the role of valence electrons in the formation of chemical bonds. (Chapter 14, Section 1) Use the valence number of an atom to predict how likely it is to form a positive or negative ion. Show how two ions form an ionic bond due to their opposite charge Compare and contrast ionic and covalent bonds (coming soon) Key terms in this ppt - ions, compound, chemical bond

3. 6.1 Ionic Bonding Essential Questions 1. How do ions form? 2. How can I predict what an element will react with and if it will react? 3. What holds ions together in ionic bonds?

4. 6.1 Ionic Bonding Lewis Dot Structures show outer shell electrons Which elements shown are NOT likely to react?

5. 6.1 Ionic Bonding The answer Noble gases (group 8) are the most stable elements. All have full outer shells

6. 6.1 Ionic Bonding Why do elements react? Elements tend to react to achieve full outer shells like the noble gases

7. 6.1 Ionic Bonding Stable 8 Rule Atoms will share, gain or lose electrons to have 8 electrons in their outermost shell Stable 8 EXCEPTIONS –Unless really small like Hydrogen, Lithium or Helium, –These atoms are stable with a full 1st shell containing 2 electrons

8. 6.1 Ionic Bonding Elements that gain or lose electrons are no longer neutral atoms because the number of protons and electrons are not the same They are now called ions and have either a positive or negative charge –Atoms that gain electrons take on extra negative charges so they become negative ions (proton number cannot change) –Atoms that lose electrons become positive ions Ions are charged atoms

9. 6.1 Ionic Bonding Which groups would form positive ions? negative ions? HINT: What is the easiest way to get to stable 8?

10. 6.1 Ionic Bonding Answer Groups 1, 2, and 3 lose electrons and become positive ions

11. 6.1 Ionic Bonding Metal Groups 1, 2 and 3 Group 1 loses 1 electron so charge = ____ +1 Group 2 loses 2 electrons so charge = ___ +2 Group 3 loses 3 electrons so charge =___ +3

12. 6.1 Ionic Bonding Groups 6, and 7 gain electrons and become negative ions

13. 6.1 Ionic Bonding Nonmetal groups 6, 7 Group 6 gains 2 electrons so = __?____ -2 ion Group 7 gains 1 electron so = __?_____ -1 ion

14. 6.1 Ionic Bonding Practice If lithium loses one electron what is it’s net charge? The atom has 1 lost one negative particle so net charge is +1 Li +1 If oxygen gains two electrons what is it’s net charge? You have 2 extra negative particles so net charge is -2 O -2 Remember that the number of protons does not change

15. 6.1 Ionic Bonding Part 2: Making Ionic Bond

16. 6.1 Ionic Bonding Formation of Ionic Bonds A particle with a negative charge will attract a particle with a positive charge. A chemical bond is the force that holds atoms or ions together as a unit. An ionic bond is the force that holds positive and negative ions together. An ionic bond forms when electrons are transferred from one atom to another. Ionic Bonds

17. 6.1 Ionic Bonding How would sodium and chlorine react? What group is sodium in and how many outer shell electrons does it have? Group 1 with 1 electron What group is Chorine in and how many outer shell electrons does it have? Group 7 with 7 electrons

18. 6.1 Ionic Bonding Draw it/solve it 1.Draw the Lewis dot structure for sodium next to the Lewis dot for chlorine. 2.Add arrows to show the transfer of electrons 3.Show the ions formed with their charges 4.Write the formula for the new compound formed.

19. 6.1 Ionic Bonding NaCl forms or sodium chloride, commonly called table salt Ionic Bonds

20. 6.1 Ionic Bonding How do sodium and fluorine react? 1.Draw the Lewis dot structure for sodium next to the Lewis dot for fluorine. 2.Add arrows to show the transfer of electrons 3.Show the ions formed with their charges 4.Write the formula for the new compound formed.

21. 6.1 Ionic Bonding Are all compounds formed in a 1 to 1 ratio? Predict what will happen if Magnesium reacts with chlorine. How many electrons does magnesium need to donate? How many does chlorine need? How can magnesium solve this problem? Draw it/solve it

22. 6.1 Ionic Bonding Did you get it? Ionic Compounds

23. 6.1 Ionic Bonding What is the chemical formula for magnesium chloride? The Chemical formula is MgCl 2 Ionic Compounds

24. 6.1 Ionic Bonding Properties of Ionic Compounds 1.Form between metals and nonmetals 2.Are generally solids at room temperatures with specific crystal shapes 3.Many soluble in water but not in alcohol. 4.Conduct electricity when melted. Ionic Compounds http://tpt.pbslearningmedia.org/resource /lsps07.sci.phys.matter.ionicbonding/ioni c-bonding/

25. 6.1 Ionic Bonding Predict: How do you think the elements in group 4 and 5 react? Answer the essential questions and do the practice problems