Unit 1 Quiz 2 Review
Name: ___________________________________________ Date: ________________ P: ______
Information
1 m = 1.094 yd
1 kg = 2.205 lb
16 ounces = 1 lb
2000 lbs = 1 ton
12 in = 1 ft
1 pint = 473 mL
3 feet = 1 yard
1 mile = 5280 ft
1 mL = 1 cm3
454 g = 1 lb
F = 9/5C + 32
C = 5/9(F-32)
0.61 miles = 1 kilometer
1 gal = 4.546 L
2.54 cm = 1 in
Conversions
1) How many milligrams are in 17.6 kilograms?
2) How many centiliters are in 0.46 cubic centimeters?
3) How many inches are in 42 kilometers?
4) Convert 1800 kilometers per hour into miles per millisecond.
5) How many cubic yards are in 1.00 cubic meter?
6) Room temperature is 21 degrees C, what is it in Farenheit?
7) A lot with dimensions of 120 ft by 75 ft is to be sold for $6500. What is the price per acre.
Use the following 1 acre = 160 rod2 and 1 rod = 5.5 yards.
8) The density of pure silver is 10.5 g/cm3 at 20ºC. If 5.25 g of pure silver pellets is added to a graduated
cylinder containing 11.2 mL of water, to what volume level will the water in the cylinder rise?
Types of Matter
1) The boiling of water is a (choose one):
a. physical change because the water disappears
b. physical change because the gaseous water is chemically the same as the liquid
c. chemical change because heat is needed for the process
d. chemical change because hydrogen and oxygen gases are formed
e. chemical and physical change
2) Identify whether the following statements about phosphorus describes a chemical or physical property (take a look
your page 58-59 on properties).
a. Phosphorous is never found free in nature. For example, phosphorous catches fire spontaneously in
air.
b. The common form of phosphorus is white.
c. Phosphorus melts at 44.1ºC.
d. Phosphorus can be stored under water.
e. Phosphorus combines easily with halogens.
3) Classify each of the following as an element, compound, heterogeneous or homogenous mixture.
a. aluminum foil
b. blueberry muffins
c. hot tea without any tea leaves in it
d. salt
e. carbon dioxide
f. water
g. spaghetti with meatballs
h. blood
Atomic Structure
1)
Between two isotopes of the same element, circle the following that would be the same!
Atomic Number,
Number of Protons,
Number of Neutrons, Number of Electrons,
Isotope Symbol – it’s like the box on the periodic table flipped.
2)
How many protons, neutrons and electrons does the following nuclear symbol
have?
P = ______
N = ______
E = ______
Element Symbol
*Mass # = P + N  the mass number may be different than the periodic table – why? The number on the periodic table
(atomic mass) is the weighted averages that exist for all the different isotopes for that element
Use the atomic mass from the periodic table only when you can’t add up the P + N to get the mass #, round that
number, example Boron’s atomic mass is 10.81, mass number is 11 (we don’t want decimal protons and neutrons).
Atomic Mass = Straight from periodic table; Mass # = Mass of the actual atom
(Hyphen Notation: Element Name – Mass # For Example: Carbon-12 or Hydrogen-1)
3)
Complete the following table:
Element
# of
Protons
Strontium
# of
Neutrons
# of
Electrons
50
36
Atomic
#
Mass
Number
Atomic
Mass
26.98
80
47
80
Nuclear
Symbol
27
13Al
200
108
10847Ag+1