1. Bond. Ionic Bond.

2. To get started… We should refresh our memories about the structure of atoms: _________ and _________ are found inside the nucleus, __________ are found in ______________ outside the nucleus. Protonsneutrons electrons energy levels The electrons in the energy level farthest from the nucleus are called ___________ electrons. valence

3. Valence matters Valence electrons are the only particles that are involved in _________________. chemical reactions Every atoms wants to have a ______ valence shell – it’s more ________ than an __________ one. full stable unfilled This gives them the same electron configuration as a ___________! noble gas

4. Octet Rule This filling of your valence shell is known as the _______ _____. Octet rule This means that atoms will _________ in such a way that they have ___ electrons in their valence shells – just like a _____________. combine 8 Noble gas

5. Win, Lose or Draw There are ___ options for filling your valence shell: 3 1. You can _______ electrons. lose 2. You can _______ electrons.gain 3. You can _______ electrons.share The option you choose all depends on how many __________ electrons you _______ with… valence start

6. Alkali Metals Consider ____ for a moment… Li 3 P 4 N Lithium has ___ valence electron. 1 But its valence shell can hold ___. 8 So Li has to ________ electrons to fill its valence shell…? gain 7

7. What if…? What if Li gave up its one valence electron? 3 P 4 N

8. What if…? What if Li gave up its one valence electron? 3 P 4 N

9. What if…? What if Li gave up its one valence electron? 3 P 4 N

10. What if…? What if Li gave up its one valence electron? 3 P 4 N We are left with _____ energy level, which now becomes the _________ shell! one valence (And would you look at that – it’s already _______!!!!) FULL

11. The Path of Least Resistance Atoms will take the _________ path to a full valence shell. shortest **Keep in mind that this may be __________!* backward

12. The Other Side What about elements on the other side of the table? Let’s look at ____… Cl 17 P 18 N Chlorine only needs ______ electron to complete its valence shell. one It’s easier for Cl to _______ one electron! gain

13. Which way? Here’s the general rule: If you have ______ than 4 valence electrons, you will tend to ______ them. less lose If you have ______ than 4 valence electrons, you will tend to _____ them. more gain Therefore, _________ tend to ______ electrons, and ___________ tend to _____ them! metalslose nonmetals gain

14. Charges, charges… Remember what you become when you lose or gain electrons? (An _____!) ion **An ion is a ________ particle – with an ________ number of _________ and __________. charged unequalprotons electrons And remember that electrons have a __________ charge, so if you _______ electrons, you become a __________ ion! negativelose positive

15. “When I see a cation, I see a positive ion; ion: anion: a (–) ion cation: a (+) ion -- a charged particle more e – than p + formed when atoms _____ e – -- more p + than e – formed when atoms _____ e – a n ions negativeions. are I think that that is, I… C ion.” A + gainlose

16. What now…? What you end up with is an atom that will _____ electrons and become a _________ ion… lose positive Right next to an atom that will ______ electrons and become a ________ ion… gain negative Hmmm… What do we know about opposites and attraction????

17. Opposites ________, so the _________ ion will be attracted to the ________ ion. attractpositive negative LiCl Li +1 Cl -1 LiCl lithium chloride + +

18. Match made in Heaven! This ________ of electrons is known as an _____________! transfer Ionic Bond Ionic bonds are always formed between a _______ and a _________! metalnonmetal The _________ of electrons creates ______, and the ___________ forces between the ions are what hold the ____________ together. transfer ionsattractive compound

19. Those ‘Dot’ things again?!? To show ionic bonds, we use the Electron Dot diagrams – and draw _________ to show the _________ of electrons between atoms. arrowstransfer Make sure you show the ____ that results from that transfer of electrons! ion

20. Na Examples: Let’s combine sodium and chlorine: + Cl Na +1 Cl -1 + The compound created: ___________ NaCl

21. Naming Ionic Compounds Ionic compounds are always formed between a _______ and a _________. metalnonmetal To name them: 1. ________ goes first.Metal 2. ____________ goes second – but you change the end of the nonmetal’s name to _______. Nonmetal “-ide” Example: NaCl = sodium chloride

22. More than one??? What happens if one atom needs to lose ___ electrons, but the other only gets __? 21 Mg Cl Now Cl’s valence shell is _________, but Mg still has one electron to unload! complete Each Cl atom can only ________ 1 electron – but who says there’s only one Cl hanging around? accept

23. More than one? To have a place for Mg’s other valence electron, we need ____________. another Cl Cl Mg Cl Mg +2 **We have 2 Cl’s – not just one! (Cl -1 ) 2 +

24. More than one? So our formula is really: Mg +2 +Cl -1 + -- OR -- MgCl 2 Name: __________________magnesium chloride

25. Things to remember… Ionic bonds are formed between a ________ and a __________. metalnonmetal Metals ______ electrons and become ___ ions; nonmetals ______ them and become ____ ions. lose gain Draw ________ to show the ________ of electrons, then draw the _______ with their _________. arrowstransfer ions charges When naming, it’s _______, then __________ -- ending in _______. metal nonmetal“-ide” + -