1. Show the Arrangement of Particles in Solid, Liquid and Gaseous Water

2. Density of Water / Ice
Why does ice float on water? Relate your answer to the kinetic molecular theory of matter.

3. Observe Isopropyl Alcohol Oil Water
Add an ice cube with red food coloring to each container.
Explain your observations in terms of relative densities, solubilities, and the kinetic molecular theory of matter.

4. Chapter 1 Terms
Sort the terms provided into categories and name each category.
Construct a sentence for each category showing the interrelationships between the terms in the category.
Revise your categories for homework as you read chapter 1.

5. Making Peanut Brittle - Demonstration
Place ½ c corn syrup, 1 c sugar, and 1 c peanuts in a large measuring cup
Microwave for 4 minutes. Stir.
Heat for another 4 minutes.
Stir in 1T butter, 1 t vanilla, and 1 t baking soda
Quickly spread on greased aluminum foil
Explain your observations using at least 10 terms presented in chapters 1.
4/16/2017

6. Electric Current & Tin (II) Chloride
Working with your lab partner, dissolve 1 plastic spoonful of SnCl2 in 50 mL of water.
Place the solution in a petri dish.
Connect alligator clips to one post of a battery and to a wire attached to the side of the petri dish. Connect another set of clips to the other post of the battery and to a second wire in the petri dish.
Record your observations. Explain the chemistry involved.
Petri dish with SnCl2
battery
4/16/2017

7. Decomposition of Tin Chloride
Electrolysis –
Signs of chemical change –
Physical properties –
Atoms, Compounds and Ions –

8. Determining the Area of an Irregularly Shaped Piece of Cardboard
Using graphical analysis (with your graphing calculator), find the area of the irregularly shaped piece of cardboard. What is another variable that is directly proportional to area?

9. Percent Composition of Margarine
Spend five minutes with your partner developing a procedure and discussing the data and calculations

10. Ion Naming
Monoatomic Ions (periodic table)
Transition Metals

11. Polyatomic Ions Naming Ions when number of oxygen atoms changes:
Perchlorate
Chlorate
Chlorite
Hypochlorite

12. Naming Ions When Number of Hydrogen Atoms Changes
Phosphate
Hydrogen phosphate
Dihydrogen phosphate
Carbonate
Bicarbonate
Sulfate
Bisulfate

13. Use your knowledge of the metric system and the use of conversion factors to prove Peter’s math correct or incorrect.

14. 0.5t(5mL/1t)(1 cc/1 mL) = 2.5 cc
Volume – 2 x 3.5 x = in3
Density - 1 lb / in3 = lb / in3
lb / in3 (453.6g / 1 lb) (1 in3 / cm3) =
g / cm3
2.5 cc (1.0906g / cc) = g
While the math is correct, the sig figs ARE NOT!!

15. TEST TUBE WITH NAIL -
OBSERVATIONS:
EXPLANATIONS?????

16. CuSO4 and NaCl combine:

17. Activity Series: Fe, Cu

18. Iron ions react with oxygen and water:

19. New Concepts:
Complex ion ~
Redox Reactions ~
Base Anhydride ~

20. Ion Quiz Write formulas for: 1. sodium acetate 6. ammonium carbonate
2. cupric chloride hydrogen cyanide
3. aluminum chlorate potassium dichromate
4. calcium bisulfate magnesium bicarbonate
5. cuprous oxide lithium chromate

21. Isotopes
Antimony has two stable isotopes, Sb-121 and Sb-123 with masses of and amu respectively. Calculate the percent abundance of each.

22. Calculation of Weighted Average Atomic Mass Using Percent Abundance of Isotopes of the Element
Silver has an atomic mass of amu. If 51.84% of Ag exists as Ag-107 ( amu), what is the identity and atomic mass of the other isotope?
.5184( ) x = x= or 109.0

23. Molecules Diatomic – H2, O2, N2, Cl2, Br2, I2, F2
Polyatomic molecules – S8, P4, O3

24. Allotropes
O, P, S, C exist in different forms
Carbon:

25. O O2 and O3 (Electricity converts O2 to O3
O O2 and O3 (Electricity converts O2 to O3. Ozone is a blue colored gas with a pungent odor. Its name comes from ozein which means “to smell”) S

26. What is the average mass of one atom of titanium in grams?

28. What is the mass percent
of C in chloroform
(CHCl3)?

29. Calculating Empirical Formulas
In a chemical reaction, g of sulfur combines with g of copper to give a pure compound. What is the empirical formula of this compound?

30. Calculating Molecular Formulas
A compound was analyzed and found to contain 53.50% carbon, 11.19% hydrogen, and 35.51% oxygen by mass. If the molar mass of this compound is g/mol, what is the molecular formula of the compound?

31. Review: Isotopes
Uranium has an atomic mass of It consists of two isotopes: uranium-235 with a mass of amu and uranium-238 with a mass of amu. Calculate the % abundance of the U-235 isotope.

32. Mass Percent
Calculate the mass percent of sulfur is barium sulfate

33. Mass / Moles / Particles
Calculate the number of atoms in 12 grams of iron.

34. Formulas
Determine empirical and molecular formulas for a compound that is 71.65% Cl, 24.27% C, and 4.07% H. The molar mass of the compound is g/ mol

35. Coulomb's Law
The force of attraction between ions in an ionic compounds is due to:
The magnitude of charge on the ions
The distance between the ions
Smaller ions and ions with greater charge have greater forces of attraction

36. Naming Hydrocarbons: Alkanes: 1 carbon: CH4 – 2 carbons: C2H6 –

37. Naming Hydrocarbons
Alkanes, continued:
6 carbons: C6H14 –
7 carbons: C7H16 –
8 carbons: C8H18 –
9 carbons: C9H20 –
10 carbons: C10H22 –
Alkenes –
Alkynes –

38. Substituted Hydrocarbons
Halocarbon – chloroform
Carboxylic acid – acetic acid
Ester – methyl acetate
Aldehyde – formaldehyde
Ketones – acetone
Alcohols – ethyl alcohol
propyl alcohol
isopropyl alcohol
Amines - methyl amine

39. Naming Molecules CO
CO2
N2O
N2O5
N2O3

42. Radioactivity
Alpha particles:
Beta Particles:
Gamma Rays:

43. U-235 loses 1 alpha particle. What element is formed
U-235 loses 1 alpha particle. What element is formed? What is its atomic mass and number?
Co-60 loses 1 beta particle. What element is formed? What is its atomic mass and number?

44. Radioactive Decay Series
U-238 undergoes a series of 14 reactions to form lead The first four reactions are alpha, beta, beta, and alpha decay, in that order. Write the equations for these first four steps.

46. Stability of Atomic Nuclei
Only 2 stable isotopes (H, He) have more p than n
Up to Ca, stable isotopes may have equal numbers of p and n or one or two more n than p
Beyond Ca, stable isotopes must have a ratio of n:p that is greater than one
Beyond Bi, (83p, 126n) there are no stable isotopes, heavier nuclei cannot be held together
Elements with even atomic numbers have more stable isotopes than those with odd atomic numbers

47. What Holds a Nucleus Together?
The mass of 1 p = amu and the mass of 1 n = amu. Therefore an alpha particle (2p, 2n) has an expected mass of amu.
The actual mass of an alpha particle = amu. The difference, amu, is called nuclear mass defect.
Mass defect can be converted into energy units using E=mc2
This amount of energy is released when the nucleus is formed and is called nuclear binding energy.

49. Peanut Brittle and Chapter 1:
Physical Properties:
State Changes:
Heat Energy:
Chemical Changes:
Mixture Types: