1. Bonding Review!

2. What are Valence electrons?

3. Valence Electrons Valence electrons are the electrons in the outermost s- and p-orbitals that can be involved in chemical reactions. 1s orbital is not involved

4. Valence Electrons Valence electrons are the electrons in the outermost s and p-orbitals that can be involved in chemical reactions. 1s orbital is not involved Outer octet of 2s and 2p orbitals are involved

5. How many valence electrons do these elements have? Calcium Two Iodine Seven

6. What is an ion? Positively or negatively charged atom

7. What are the charges of the following ions? Strontium Sr 2+ Bromine Br 1-

8. Ions Cation Positively Charged Atom (loses electrons) K +1 Pronounced CAT-ion

9. Ions Cation Positively Charged Atom (loses electrons) K +1 Anion Negatively Charged Atom (gains electrons) Cl -1 Pronounced AN-ion

10. Ions Cation Positively Charged Atom (loses electrons) K +1 Anion Negatively Charged Atom (gains electrons) Cl -1 Ionic Bonding occurs when a cation gives electrons to an anion and the atoms become attracted to each other due to the opposite charges.

11. What is an ionic bond? A transfer of electrons between a metal and a non-metal

12. Ionic Bonds Sodium has one valence electron it wants to lose Chlorine has 7 valence electrons, so it wants to gain one more to make it to eight. · Na Cl : : · :

13. Ionic Bonds The Sodium atom donates its one valence electron to Chlorine. · Na Cl : : · : +-

14. Ionic Bonds This means Na +1 has the electron configuration of the noble gas before it, which is Neon Sodium’s electron configuration is now written as [Ne] + · Na +1 Cl -1 : : · :

15. Ionic Bonds Chlorine now has the electron configuration of the noble gas after it, which is Argon. Chlorine’s electron configuration is now written as [Ar] - · Na +1 Cl -1 : : · :

16. Ionic Bonds The positively charged ion then moves toward the negative ion through electrostatic attraction. Sodium and Chloride are now ionically bonded to form a new compound known as sodium chloride (NaCl). Na + Cl - : : : :

17. Ionic Bonds Now each sodium is positively charged and each chlorine is negatively charged. They are attached because opposite charges attract electrostatically. However, together they balance each other out. Na +1 Cl : : : :

18. Ionic Bonds But, the positive charge, does attract other negatively charged molecules, such as other chlorine ions The same holds true for negatively charged chlorine ions attracting other positive ones Na +1 Cl : : : : Cl : : : : Na +1

19. Ionic Bonds Soon, they all begin to line up In fact, they will also line up 3-Dimensionally Na +1 Cl : : : : Cl : : : : Na +1 Na +1 Cl : : : :

20. Ionic Bonds This then forms crystals of salt Na +1 Cl : : : : Cl : : : : Na +1 Na +1 Cl : : : : Cl : : : : Na +1

21. Ionic Bonds This then forms crystals of salt Na +1 Cl : : : : Cl : : : : Na +1 Na +1 Cl : : : : Cl : : : : Na +1

22. Ionic Bonds Bonding that involves a transfer of electrons. Positively and negatively charged atoms (ions) result from this transfer The resulting positive and negative charged atoms are “attracted” to each because of their opposite charges. Na + Cl -

23. Solvents and Solutions Because ionic molecules have positive and negative atoms, they can be pulled apart by other substance with positive and negative charges.

24. Solvents and Solutions One example is dissolving salt into water Water molecules have positive ends near the hydrogens and negative ends near the oxygen.

25. Solutions Since all of the ions are evenly dispersed and dissolved in the water, it makes a solution of salt water. This solution is transparent.

26. Reforming Crystals When the water evaporates, the positive sodium ions and the negative chlorine ions come back together again!

27. Polyatomic Ion Polyatomic ions are ions that have multiple atoms attached to each other, but as a unit have a net charge. Sulfate (SO 4 -2 ) is an example.

28. Polyatomic Ions Anions AcetateCH 3 COO − Bicarbonate (hydrogen carbonate)HCO 3 - CarbonateCO 3 -2 CyanideCN − HydroxideOH − NitrateNO 3 - PhosphatePO 4 -3 SulfateSO 4 -2 SulfiteSO 3 -2 Cations AmmoniumNH 4 + HydroniumH3O+H3O+ Mercury(I)Hg 2 +2 State−1+1+3+5+7 Anion namechloridehypochloritechloritechlorateperchlorate FormulaCl − ClO − ClO 2 − ClO 3 − ClO 4 − Structure Polyatomic Cations are more rare

30. So, Who Makes Ions Anyways? It all depends on how many valence electrons they have and what they need to get to noble gas configuration. Question #1: How many valence electrons does Aluminum have?

31. So, Who Makes Ions Anyways? It all depends on how many valence electrons they have and what they need to get to noble gas configuration. Question #1: How many valence electrons does Aluminum have? Answer: 3 Question #2: What ionic charge will it have to become noble gas configuration?

32. So, Who Makes Ions Anyways? It all depends on how many valence electrons they have and what they need to get to noble gas configuration. Question #1: How many valence electrons does Aluminum have? Answer: 3 Question #2: What ionic charge will it have to become noble gas configuration? Answer: Al +3

33. Alkali Metals Charge: +1

34. Alkaline Earth Metals Charge: +2

35. Boron Family Charge: +3

36. Carbon Family Do not usually make ions, but could be +4 or -4

37. Nitrogen Family Charge: -3

38. Oxygen Family Charge: -2

39. Halogens Charge: -1

40. Noble Gas Family Do not make ions, because they already have full orbitals

41. Transition Metals A variety of positive ions from +1 to +7 We’ll discuss these in more detail later

42. Acetic Acid Dissolving in Water + Acetic AcidWaterAcetate ionHydronium ion

43. Content Objectives SWBAT describe the process of ionic bonding due to some atoms removing electrons from other atoms to reach the Octet Rule and then attracting to each other due to electrostatic charger.