2. Ions and Ionic Compounds Science 10 Spring 2003 Miss. Barteaux H Mg Continue

3. This presentation is a continuation of the periodic table activity we completed earlier. It can be used as a review of what the activity involved, as well as applying what was learned to new concepts. Continue Electron Configurations Periodic Table Activity Click below to view and save a copy of:

4. Back to Question

5. Patterns in the Periodic Table Looking at the completed periodic table on the last screen, what patterns exist among the groups and the periods? The number of electrons in the outermost shell increases as you move to your right to the next group, and the number of shells around each nucleus increases by one as you move from one element to the next down each periods. The number of electrons in the outermost shell decreases as you move to your left to the next group, and the number of shells around each nucleus increases by one as you move to the right to the next group. The number of electrons in the outermost shell decreases as you move to your right to the next group, and the number of shells around each nucleus increases by one as you move from one element to the next down each periods. Completed Table

6. Not quite, but good try !! Take another look and try again!! Take another look and try again!! Go back

7. Not quite, but good try !! Take another look and try again!! Take another look and try again!! Go back

8. You are correct!!! See explanation Go back

9. From viewing the last two slides, what would you say a cation is? How does a cation differ from a neutral atom? Cation Formation Go back to cation demonstration Continue

10. Anion Formation F Fluoride Atom- neutral Click the space bar to see the Fluoride atom gain an electron, and to find out what it becomes! 9 protons and 9 electrons = +9 + (-9) = 09 protons and 10 electrons = +9 + (-10) = -1 charge Fluoride Ion- Anion F Fluorine Atom- Neutral Compare the two fluorine atom models. What differences exist? What does this tell you about the fluoride ion formation? Continue Click the space bar to answer a question

11. Anion Formation S Sulfur Atom - Neutral 16 protons and 16 electrons = +16 + (-16) = 0 Sulfide Ion - Anion 16 protons and 18 electrons = +16 + (-18) = -2 charge Click the space bar to see the Sulfur atom gain electrons, and to find out what it becomes! Compare the two sulfur atom models. What does this tell you about sulfur ion formation? - 2 Sulfide Atom - Neutral S Continue Click the space bar to answer a question

12. From viewing the last two slides, what would you say an anion is? How does an anion differ from a neutral atom? Anion Formation Go back to cation demonstration Continue

13. Why does this happen???? Cation The metallic elements tend to form positive ions (cations) by losing one or more electrons. They do this because they want to have a full valence (outer) shell like the group 8 noble gases. Click here to an animation Click here to an animation Anion The non-metallic elements tend to form negative ions (anions) by gaining one or more electrons. They do this because they also want a full valence (outer) shell like the group 8 noble gases. Click here to an animation Continue

14. Neon Sodium – Pay attention to the structure at the start to be able to see the difference at the end. (Just click on the movie screen for the morph to begin. If you want to see it again, just click on the movie screen!) Cation Formation Go back

15. Anion Formation Argon Chlorine - Pay attention to the structure at the start to be able to see the difference at the end. (Just click on the movie screen for the morph to begin. If you want to see it again, just click on the movie screen!) Go back

16. S Mg When atoms collide, valence electrons on each atom interact. A chemical bond forms between atoms if their valence electrons make a new arrangement that has less energy than their previous arrangement. (click the space bar to see the electrons move) For many atoms, the lowest energy arrangement of valence electrons is the same as the arrangement for the noble gas to which they are closes in the periodic table. In this example, the ions have equal, but opposite charges so they form a bond called an ionic bond. +2 -2 Play again Continue

17. S Mg When atoms collide, valence electrons on each atom interact. A chemical bond forms between atoms if their valence electrons make a new arrangement that has less energy than their previous arrangement. (click the space bar to see the electrons move) For many atoms, the lowest energy arrangement of valence electrons is the same as the arrangement for the noble gas to which they are closes in the periodic table. In this example, the ions have equal, but opposite charges so they form a bond called an ionic bond. +2 -2 Continue

18. Mg +2 S -2 Electrostatic attraction between ions because of the opposite charges. MgS Therefore they form an ionic bond and the result is an ionic compound called Magnesium Sulfide. Continue

19. Mg +2 S -2 Electrostatic attraction between ions because of the opposite charges. MgS ( Magnesium Sulfide) What do you notice when you add the charges of the two ions? What do you notice about the name of the compound? Continue

20. F H +1 Play again Electrostatic attraction between ions because of the opposite charges. HF Therefore they form an ionic bond and the result is an ionic compound called Hydrogen Fluoride. Click to see electrons move Continue

21. F H +1 Electrostatic attraction between ions because of the opposite charges. HF Therefore they form an ionic bond and the result is an ionic compound called Hydrogen Fluoride. Click to see electrons move Continue

22. What do you notice when you add the charges of the two ions? What do you notice about the name of the compound? Continue F H +1 Electrostatic attraction between ions because of the opposite charges. HF (Hydrogen Fluoride)

23. FF Mg +2 Click the space bar to see what happens next Electrostatic Attraction These ions can now combine to form an ionic compound. What will the chemical formula be for this compound if the charges must add up to zero? How would you name this compound? Click the space bar to answer a question Click the space bar to see the animation Check your Answer

24. MgF 2 +2(-1) x 2 +2 + (-2) = 0 Continue Click space bar for explanation Magnesium Fluoride Go back

25. H S -2 +1 H Click the space bar to see the animation Click the space bar to see what happens next Electrostatic Attraction Click the space bar to answer a question These ions can now combine to form an ionic compound. What will the chemical formula be for this compound if the charges must add up to zero? How would you name this compound? Check your Answer

26. H2SH2S (+1) x 2(-2) +2 + (-2) = 0 Click space bar for explanation Continue Hydrogen Sulfide Go back

27. So what can we conclude?? What is an ionic bond? What elements are involved in ionic bonds? What kind of compound is formed by ionic bonds? Does this compound have a charge? Continue

28. Examining the reactivity of the elements MgCl 2 or HCl ??? Which cation would react more energetically with Cl? Mg or H 2 ? Continue

29. Reactivity of The Elements Watch a video on group 1 elements Watch a video on group 7 elements Continue

30. Reactivity of Group 1 Elements Click on the video screen to play the movie. Go back Li Na K

31. Reactivity of Group 7 Elements Click on the video screen to play the video. Go back Continue F Cl

32. So what can we conclude?? How does the reactivity of the elements differ within the groups? Give two examples and discuss how they would differ in reactivity and explain why! Continue Go back to reactivity page

33. The end!!!