1. Most Missed Questions You need to know this stuff…

2. Atomic Theory Nuclear charge = # of protons or Atomic # # neutrons = mass# - Atomic #(# of protons) ex: Ca-37 37-20= 17 neutrons What is the total number of neutrons in an atom of O-18? 10 What is the net charge of an ion that has 8 protons, 9 neutrons, and 10 electrons? negative 2 Electrons farther away from nucleus have more energy

3. Atomic Mass Calculate atomic mass from the masses of the NATURALLY occurring isotopes and the relative abundance(%) MAD

4. Nuclear Matter is converted into energy Fusion: joining hydrogen to make helium Fission: splitting uranium with neutrons Natural Transmutation one isotope on reactant side: Complete the nuclear equation for the beta decay of the Co-60 by writing an isotopic notation for the missing product.

5. Half lives: use table What is the total number of years that must pass before only 25.00 grams of an original 100.0-gram sample of C-14 remains unchanged? ¼ left, 2 half lives, 11, 430 yrs. # half live TIME Fraction remaining MASS 01 11/2 21/4 31/8 41/16

6. More Nuclear

8. Fission Mass is converted to energy Nuclear Fusion

9. Periodic TABLE Non-metals gain electrons, become negative ions and the radius of the ion is bigger than the radius of the atom Elements get more metallic going down ANY group on table Radius decreases going to the right in a period because of increasing nuclear charge. Put in order of increasing radius… Cl Cl - Li Li + Determine the Group # of X: X2O3X2O3 XO X2OX2O XCl 2

10. Bonding Add energy to break a bond Making bonds releases energy Bond Type: subtract electronegativity (END) Non Polar bond, same nonmetal bonded, END= 0 Polar Molecules have uneven distribution of charge Molecular= covalent= all nonmetals=sharing of electrons Different structure=different properties ee: graphite and diamong,O 2 vsO 3, isomers

11. More Bonding Polyatomics are generally covalently bonded Identify both types of bonds in the NH 4 NO 3(s) Ionic and covalent Which pair represents two forms of an element in the same phase at STP but with different structures and different properties? (1) I 2 (s) and I 2 (g) (3) H 2 (g) and Hg(g) (2) O 2 (g) and O 3 (g) (4) H 2 O(s) and H 2 O(ℓ) Answer 2

13. Answers Symmetrical Polar molecule stronger IMF’s KCl ionic transfer of electrons A,B, C all covalent sharing electrons

14. Formula Writing Stock system or IUPAC The Roman # is the POSITIVE CHARGE of the 1 st element In an experiment, 2.54 grams of copper completely reacts with sulfur, producing 3.18 grams of copper(I) sulfide. Determine the total mass of sulfur consumed. 3.18- 2.54=.64g Write the chemical formula of the compound produced. Cu 2 S What is the IUPAC name for the compound ZnO? Zinc oxide no roman # only one possible oxidation state

16. Kinetics  H= Heat of Reaction = PE product-PE reactant Find if a reaction is Endo or Exothermic using TABLE I

17. Matter and Energy Define Solution in 2 words: Homogenous mixture What symbol will be with a solution’s formula? (aq)

18. Gas Laws Ideal gas: no IMF’s, No volume per molecule, elastic collisions Increase temp and decrease pressure to make real like ideal Which statement describes the particles of an ideal gas according to the kinetic molecular theory? (1) The gas particles are arranged in a regular geometric pattern. (2) The gas particles are in random, constant, straight-line motion. (3) The gas particles are separated by very small distances, relative to their sizes. (4) The gas particles are strongly attracted to each other

19. Most missed last year 76 Describe a procedure to physically remove the water from mixture 1.

21. Q= Q= mc  T when temp changes Q= mH f freezing/ melting Q= mH v Boiling/ l to g /g to l The temperature of a sample of water changes from 10°C to 20°C when the sample absorbs 418 joules of heat. What is the mass of the sample?

22. Shift Happens Given the equation representing a reaction at equilibrium: N 2 (g) + 3H 2 (g)  2NH 3 (g) What will cause a shift left? What will cause a shift right?

23. REDOX & Electrochemistry Voltaic cell: chemical energy converted to electrical Voltaic Cell: + cathode Electrolysis: hook cathode to NEGATIVE(--) Which ionic equation is balanced? (1) Fe 3+ + Al → Fe 2+ + Al 3+ (2) Fe 3+ + 3Al → Fe 2+ + 3Al 3+ (3) 3Fe 3+ + Al → 3Fe 2+ + Al 3+ (4) 3Fe 3+ + Al → Fe 2+ + 3Al 3+

24. Practice REDOX ?

25. Types of Reactions (2) 2Mg + O2 → 2MgO (1) Mg + 2AgNO3 → Mg(NO3)2 + 2Ag (3) MgCO3 → MgO + CO2 (4) MgCl2 + 2AgNO3 → 2AgCl + Mg(NO3)2 Synthesis Single replacement Decomposition(need a compound to start0 Double replacement ALL but (4) are REDOX!!!

26. ACID BASE Hydronium (H 3 O+) is an acid ion = hydrogen ion (H+) Hydroxide (OH-) is a base ion………….. both are on table E and T If pH goes up by 1 Hydronium ion concentration decreases by a factor of 10 If pH goes up by 2 Hydronium ion concentration decreases by a factor of 100 If pH goes down by 1 Hydronium ion concentration increases by a factor of 10 A student, wearing chemical safety goggles and a lab apron, is to perform a laboratory test to determine the pH value of two different solutions. The student is given one bottle containing a solution with a pH of 2.0 and another bottle containing a solution with a pH of 5.0. The student is also given six dropping bottles, each containing a different indicator listed in Reference Table M. Compare the hydronium ion concentration of the solution having a pH of 2.0 to the hydronium ion concentration of the other solution given to the student. Use M A V A when you see…

27. Questions that look hard to me…

28. Organic Esterification: alcohol + organic acid  ester + H 2 O What are the functional groups in each? Name a homologous series. Ester name: 1st prefix-alcohol, 2 nd add -anoate to acid name Draw the condensed structural formula for: propyl heptanoate CH 3 CH 2 CH 2 OOCCH 2 CH 2 CH 2 CH 2 CH 2 CH 3

29. Organic