Name: ______________________________________________________________________ Date: _________________ Period: ____________
1.
2.
3.
4.
5.
6.
What branch of chemistry is concerned with the theories and experiments that describe chemical behavior?
________________________________________
What branch of chemistry studies all substances that contain carbon? _____________________
What branch of chemistry studies processes that take place within living organisms? ____________________________
What branch of chemistry studies the composition of substances? ________________________
What branch of chemistry studies substances that do not contain carbon? ________________
Complete the table:
Compound
Organic or Inorganic?
KI
NaOH
C6H12O6
7.
Compare and contrast elements and compounds. What is the smallest particle of each. Give an example of each.
8.
9.
10.
11.
12.
13.
14.
The state of matter in which all particles are packed closely together while vibrating in place: ____________________
The state of matter that has a definite shape and a definite volume: ______________
The state of matter in which the particles are spread out and move rapidly: _____________
The state of matter in which the particles slide past another: ____________
The state of matter that is characterized by a definite volume and indefinite shape is: _____________________
The state of matter that is characterized by an indefinite shape and an indefinite volume is: ____________________
Compare and contrast chemical and physical changes.
15. What the 4 signs of a chemical change?
16. Circle the physical changes below
Leaves change color in the fall
Water evaporates
Glass breaks
17. Read the ruler to the nearest centimeter:
Milk spoils
Ring turns your finger green
Zinc bubbles when it is added to HCl
18. Read the graduated cylinder to the nearest milliliter:
19. Read the triple beam balance to the nearest gram:
20. How many significant figures?
a.
5001
b. 0.0009
c.
900000
21. Report to the correct number of significant figures:
a.
9.01 – 2.1 =
b. 5.56 + 12 =
c.
7.00 x 0.045 =
d. 9.80 ÷ 0.7 =
d.
e.
f.
90000.
0.000080
8.01 x 107
e.
f.
g.
1.278 x 103 ÷ 1.4267 x 102 =
55.46 - 28.9 =
2.01 + 35.2 + 6 =
22. What is the base unit for mass? Length? Volume? Time?
23. Convert 73 km to meters.
25. Convert 76 inches to meters (Given: 2.54 cm = 1 inch)
24. Convert 8.900 moles/L of barium iodide to grams/mL.
26. Convert 100 yards to cm2. (Given: 1 yard = 0.9144
meters)
27. Eggs are shipped from a poultry farm in trucks. Each carton of eggs holds 12 eggs. The cartons of eggs are then placed in a crate that
holds 20 cartons. The cartons are packed in trucks that carry 3125 crates of eggs. How many truckloads will it take to carry 3.75 x
106 eggs?
28. Determine the density of 101.9 grams of acetic acid whose volume is 27.3 mL.
29. Determine the mass of a sample of zinc whose density is 7.113 g/cm3 and whose volume is 45.3 L. (Given: 1 mL = 1 cm3)
30.
31.
32.
33.
34.
35.
36.
37.
_______________ and __________________ are located in the nucleus; _________________ surround the nucleus.
_______________ discovered the electron in the cathode ray experiment.
Rutherford discovered the ___________________ in the gold-foil experiment.
Rutherford concluded that the _______________ makes up most of the mass of the atom.
______________ proposed the idea that everything is made up of small particles and coined the term “the atom.
Thompson’s model of the atom is called ___________________________________ model.
Bohr stated that electrons move in ____________________________________.
Complete the table below:
Particle
Charge
Protons
Electrons
Neutrons
38. Complete the table below:
Element
Atomic Number
Atomic Mass
Number of protons
Number of
electrons
Number of
neutrons
74
Fe
O211
Al3+
39. ___________________ are atoms of the same element with the same atomic number but have a different number of neutrons.
Therefore, the atomic mass of these atoms varies.
40. What is average atomic mass of Lithium if 7.42% exists as 6Li (6.015 amu) and 92.58% exists as 7Li (7.016 amu)?
41. Magnesium has three naturally occurring isotopes. 78.70% of Magnesium atoms exist as Magnesium-24 (23.9850 amu). Magnesium25 has a mass of 24.9858 amu and Magnesium-26 has a mass of 25.9826 amu. What is the percent abundance of the other two
isotopes?
42. How many ions of Na+ are present in 10.0 grams of sodium nitrate. Report your answer to the correct number of significant figures.
43.
44.
45.
46.
47.
Group 1 elements belong to the _____________________ group.
Group 3-12 elements are _______________metals.
Group 17 elements are ______________________.
Group 18 elements are ______________________.
Where are the metals located on the periodic table? Where are the nonmetals located on the periodic table?
48. What is the difference between ionic and covalent compounds?
49. What is the difference between acids and bases?
50. What is the difference between ionic compounds and hydrates?
51. Write the formula for the following compounds
A. Magnesium oxide
B. Titanium (III) sulfide
C. Sulfuric acid
D. Hydrosulfuric Acid
E. Copper (II) hydroxide
F.
Manganese (IV) hypochlorite
G.
H.
I.
J.
K.
Ammonium Chloride
Dinitrogen tetrafluoride
Acetic Acid
Titanium (IV) hydroxide
Cobalt (III) chloride tetrahydride