2. 200 400 600 800 1000 1200 Chemical RxStructure of the Atom Stoichiometry Ionic Bonding Nuclear Chemistry Electrons in Atoms Final

3. Ions that do not participate in a chemical Rx

4. Daily Double

5. This controls the extent of the reaction

6. The gain of electrons create this

7. The splitting of atomic nuclei

8. A wave’s height

9. This is used to determine if a specific Rx will proceed

10. This will tell you the difference between any type of atom

11. Relationship between any two substances in a balanced chemical R x

12. The formula of Perclorate ion

13. Half the original amount

14. This form of energy exhibits wavelike behavior as it travels through space

15. A solid produced during a chemical R x is a solution

16. The smallest particle of an element that retains the properties of the element

17. The most product that can be made from a given reaction

18. This type of ion is formed when valence electrons are removed to make it more stable

19. A particle with no mass, but a negative charge

20. Daily Double

21. When oxygen is added to this reaction, these products always form

22. This was used to discover the electron

23. Aluminum Nitrate + Sulfuric Acid  The mole ratio of Sulfuric acid to Nitric acid is

24. When atoms valence electrons can move “freely” between other atoms that are bonded

25. This type of particle makes up visible light

26. This rule states that single electrons w/ the same spin must occupy each equal energy orbital before pairing up

27. Double Replacement Reactions in Aqueous Solutions can produce these 3 products (Hint: Net ionic)

28. This man’s experiment proved the existence of the atomic nucleus

29. In the unbalanced reaction of P 4 + O 2  P 4 O 10, if 25.0 g of P 4 react w/ 50.0 g of O 2, what is the limiting Reagent

30. Elements in this group can have multiple charges

31. 210 84 Po  206 82 Pb + ? According to this reaction, the mass of this radioactive particle is lost

32. This principal states that a maximum of 2 electrons can occupy a single atomic orbital and cannot have the same 4 quantum numbers

33. The balanced products in net ionic when Aluminum Nitrate is mixed with Sulfuric Acid

34. The average of these determines the mass of any atom

35. In the unbalanced reaction of P 4 + O 2  P 4 O 10, if 25.0 g of P 4 react w/ 50.0 g of O 2, how much of the excess reagent (g) remains

36. The energy involved in forming an ionic compound (solid)

37. During Beta decay, the atomic number is altered by this

38. Knowing the position and velocity of an electron simultaneously is not possible b/c of this man’s theory

39. This mans’ theory says that matter is composed of extremely small particles called atoms, all atoms of the same element are identical, and atoms cannot be created, divided, or destroyed

40. Probability of finding an electron

41. Spectator Ions Dalton Limiting Reagent AnionFission Amplitude Activity Series Atomic # Molar Ratio Perchlorate Half-life Electromagnetic Radiation Precipitate Atom Theoretical Yield CationBeta Atomic Orbital CO 2 + H 2 O Cathode Ray tube 3:6 Sea of Electrons Photons Hund’s Rule S, L, G Rutherford’s Gold Foil P4P4 Transition 4 2 He Pauli Exclusion Nothing Isotopes 17.6 g O 2 Lattice E Increase by 1 Heisenberg

42. Stoichiometry

43. During the combustion of Acetone (C 3 H 6 O), 4.5 L of water is produced. How much Oxygen in ml is required to produce this much water Density of O = 1.308 g/L

44. Rx: C 3 H 6 O + 4O 2  3CO 2 + 3H 2 O 4.5 L x 1000 ml/L = 4500 ml 4500 ml x 1.0 g/ml = 4500 g H 2 O 4500 g H 2 O x 1 mol/18 g H 2 O = 250 mol H 2 O 250 mol H 2 O x 4 mol O 2 /3 mol H 2 O = 333.33 mol O 2 333.33 mol O 2 x 32 g/1 mol = 11,000 g O 2 11,000 g O 2 x 1/1.308 g/L x 1000ml/1L = 8.4E 6 ml O 2