2. Ions and Charges AA B CBC Valence Structure AA B CBC Formulas A BA B CC Ionization Energy ABC Molecular Shapes AA B CBC Polar/ Nonpolar AA B CBC Ionic Bonds AA B CBC Covalent Bonds AA B CBC Stoichiometry AA B CBC Balancing Equations AA B CBC Electronegativity AA B CBC Formulas with Polyatomic Ions AA B CBC

3. All elements are trying to achieve what electron configuration? A noble gas configuration

4. The element Sodium is likely to form an ion of what charge and why? +1 because it will give away it’s 1 valence electron to achieve a structure like Ne.

5. What charge will the element O be likely to form and why? -2 because it will want to take 2 electrons to form a full outside shell like the element Ne.

6. Given the electron configuration 1s 2 2s 2 2p 3 ; what element is this and what ion charge will it likely have? Element Nitrogen, -3 charge on the ion

7. An element has an electron configuration of 1s 2 2s 2 2p 5, what electron configuration will it try to form and why? 1s 2 2s 2 2p 6 ; in order that it have a full outside electron shell like a noble gas.

8. How many valence electrons does the following element have? 1s 2 2s 2 2p 6 3s 2 3p 2 4

9. What would be the formula for Calcium bonding with Iodine? CaI 2

10. What would be the formula for Cesium bonding with Phosphorus? Cs 3 P

11. What would be the formula for Carbon bonding with Hydrogen? CH 4

12. What does ionization energy tell us? What is an example of an element with low Ionization energy? Ionization energy tells us how easily and element will give away a valence electron. Any group 1 or 2 element has low ionization energy.

13. Which elements have very high ionization energies? Group 6A (16) and Group 7A (17) elements.

14. What is the relationship between ionization energy and electronegativity? They act like opposites, an element with low ionization energy will have high electronegativity and vice versa.

15. What shape will a molecule of NH 3 form? pyramidal

16. What molecular shape will the molecule AlF 3 form? Trigonal planer

17. What shape will water form and why? Bent, because there are two sets of lone pairs that push the bonds down closer together.

18. Is water a polar or non polar molecule and why? It is polar because the oxygen has a slightly negative charge and the hydrogen a slightly positive due to electronegativities and it’s shape.

19. Is CH 4 polar or non polar and why? Nonpolar, because with it’s tetrahedral shape the slightly positive H surround the C and there is no negative and positive end.

20. Is the molecule NH 3 polar or nonpolar and what is the difference between it and AlF 3 ? Ammonia is polar and is different from AlF 3 because AlF 3 is trigonal planer and the slightly negative charges surround the positive and so there is no + or – end.

21. How is an ionic bond formed? An atom forfeits it’s electrons due to low electronegativity to an atom that has high electronegativity and since the two ions have opposite charges they are drawn together to neutralize the charge.

22. If there is an ion with a charge of -2; name two ways that it’s charge could be neutralized in a bond. It could bond with an ion with a +2 charge or 2 ions with a +1 charge.

23. What do we call a negative ion? A positive ion? Anion; cation

24. How is a covalent bond different from an ionic? An ionic bond consists of exchange of electrons forming ions, in a covalent bond the electrons are shared between the atom’s electron shells.

25. What types of elements make up a covalent bond? 2 non metals joined together or in other words elements from groups 4A,5A and 6A.

26. Which is stronger an ionic bond or a covalent bond? Ionic bond because of the electromagnetic force holding the atoms tightly.

27. If you are given 17 grams of C how many grams of water would you need to react with that? C + H 2 O → CO + H 2 25.5 g of water

28. If you had 8 L of H 2, how many L of O 2 would you need to react? 2H 2 + O 2 → 2H 2 O 4L of O 2

29. If you have 12.04 x 10 23 molecules of H 2 O you have how many grams is that? 32 grams water

30. Balance the equation below: C 3 H 8 + O 2 → CO 2 + H 2 O 1:5:3:4

31. Why do we balance equations? So that the law of conservation of mass is satisfied and we can obtain the molar ratio of reactants and products.

32. Balance the equation below: HCl + Mg(NO 3 ) 2 → HNO 3 + MgCl 2 2:1:2:1

33. What is electronegativity and what causes it to increase or decrease? The ability of an atom to pull electrons from another atom and add them to its outside shell. The size of the atom affects it as well as the number of valence electrons. The smaller the atom the higher the electronegativity and the more valence the higher it is.

34. On the metals side of the Periodic Table what happens to the electronegativity values as you go down a group? They decrease

35. What is the most electronegative element on the Periodic Table? Fluorine F

36. What is the formula for Cu which has a +1 charge with nitrate? CuNO 3

37. What is the formula for Magnesium acetate? Mg(C 2 H 3 O 2 ) 2

38. What is the formula for calcium combing with a sulfate ion? CaSO 4