IPC Fall Semester Review
Name __________________________________ Period ___________ Teacher _______________
Sequence and define the common steps found in scientific methods in the correct order.
1. State the problem
2. Gather information
3. Form a hypothesis
4. Test the hypothesis
5. Analyze data
6. Draw a conclusion
Directions: Choose the term from the word list that best completes each statement. Write the term in the blank at the
left of each statement.
graph
y-axis
control
vertical
line
independent
1. A visual display of data or information is a _graph_____.
2. In a line graph, the __vertical____ axis is called the y-axis.
3. In a line graph, the dependent variable is plotted on the __y-axis____.
4. The type of graph that is useful for showing trends or continuous change is a __line____.
5. A variable that changes and affects the measure of another variable is called the __independent____ variable.
6. An experimental setup that does NOT contain the variable being tested is called the ___control__________.
Quantity Measured
Length
Mass
Time
Temperature
Unit
Meter
Kilogram
Second
Kelvin
Symbol
m
kg
s
K
Practice with these conversions:
3000 mg = 3 g
198 g = .198 kg
65 L= 65000 mL
8.3 cm = 83 mm
1. Long hair in the laboratory must be
A. cut short.
B. held away from the experiment with one hand.
C. always neatly groomed.
D. tied back or kept entirely out of the way with a hair band, hairpins, or other confining device.
2. If you wear contact lenses in the school laboratory,
A. take them out before starting the lab.
B. you do not have to wear protective goggles.
C. advise your science instructor that you wear contact lenses.
D. keep the information to yourself.
3. You are heating a substance in a test tube. Always point the open end of the tube
A. toward yourself.
B. toward your lab partner.
C. toward another classmate.
D. away from all people
E. none of the above
4. The attractive forces in a liquid are
a. strong enough to prevent the particles from changing positions.
b. too weak to hold the particles in fixed positions.
c. stronger than those in a solid and a gas.
d. strong enough to provide a definite shape and volume.
What is the 5. What is the physical change of a solid to a gas without production of liquid?
a. heat of fusion
c. sublimation
b. condensation
d. deposition
6. The energy required to completely change a solid to a liquid is
a. heat of fusion
b. boiling point
c. melting point
7. By which process do gases take the shape of their container?
a. evaporation
c. adhesion
b. expansion
d. diffusion
8. According to the kinetic-molecular theory, particles of matter
a. are in constant motion.
c. have different colors.
b. have different shapes.
d. are always fluid.
d. heat of vaporization
9. Particles within a liquid
a. do not move.
b. vibrate weakly about fixed positions.
c. Slide pass each other.
d. Rapidly collide with each other.
10.
___D___ good conductors of heat and electricity
___A___ break easy and have no magnetism
___B____ stable and nonreactive
___C___ considered semiconductors; solid at room temp but brittle
A. Non metals
B. Noble gases
C. Metalloids
D. Metals
11. A(n) _________ is a mixture that settles upon standing by which produces a sediment.
A. solution
B. colloid
C. suspension
D. element
12. A positive Tyndall Effect demonstrated by smoke and fog are examples of a _______________.
A. substance
B. solution
C. colloid
D. suspension
13. The law of conservation of mass states that mass cannot be __________________.
A. burned
B. changed in form
C. created or destroyed
D. heated or cooled
14. The resistance of a fluid is referred to as _____________.
A. pressure
B. energy
C. viscosity
D. buoyancy
15. Examine the figure to the right. Which of the following statements
explains why a steel ship will float on saltwater but a bar of steel will sink.
A. The density of the ship is greater than water.
B. The viscosity of saltwater is less than pure water.
C. The buoyancy force on the ship is greater than the weight of the ship.
D. The gravitational force is greater than the buoyany force.
16. What is the property of metals which allows them to be hammered into sheets?
A. luster
B. hardness
C. malleability
D. ductility
17. If a substance breaks easily, it is said to be ________________.
A. reactive
B. brittle
C. magnetic
D. ductile
18. One chemical property that can be measured in a substance is its reactivity with water. What is another chemical
property?
A. density
B. flammability
C. malleability
D. solubility
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19. A chemical change __________.
A. always can be reversed physically
B. results in a new substance
C. never will change state
D. requires an a acid in order to take place
20. Select from the scientist below to complete the statements:
Democritus
Bohr
Rutherford
Thomson
Dalton
___Bohr____________ determined that electrons orbit the nucleus like the planets around the sun
___Thomson______________ discovered electrons and developed the plum pudding model
____Rutherford___________ conducted the gold foil experiment and determined that atoms are mostly empty space
____Democritus____________ named the smallest indivisible particle Atomos
____Dalton___________ Stated 5 principles of atomic theory; one being that atoms of the same element have the
same properties
21. Complete the table below
Subatomic particle
Location
Charge
Relative Mass
Proton
Nucleus
Neutron
Nucleus
Electron
Cloud
+1
1
0
1
-1
0
22.
53
The atomic number for this element is ___53____________
I
The atomic mass for this element is ___126______________
126
Number of protons____53_____; neutrons _____73_____; electrons _____53______
Group Number____17_________; Name of group_____Halogen_________________
Number of valence electrons ____7__________; draw Lewis dot structure
Which group of elements would have similar properties to I?
F Cl Br
sb Te Xe
I
C P Se
23. Which is an example of an ion? Isotope?
 An atom loses 2 electrons __ion______
Oxygen-16 and Oxygen-18 ___isotope__________
 Number of protons stays the same, but the mass changes _____isotope_________________
 An atom gains 1 electron ___ion_______
24. Select from the following:
Metal
Non-Metal
Metalloid
___Metalloid_________ Elements that lie along the stair-step line
____Non-Metal________ Poor conductors of electricity
__Metal__________ Malleable and ductile
____Non-Metal________ Gas at room temperature
____Metalloid________ Semiconductors
___Metal_________ Lustrous
___Non-Metal_________ Brittle
25. Select from the following
Alkali Metals
Alkaline Earth Metals
___Halogen___________________ Group 17
Transition Metals
Noble Gas
_____Alkali__________________ 1 valence electron
___Alkali_______________Highly reactive metal
___Transition___________________ Groups 3-12
26. Name the element
Halogens
_____Alkaline Earth__________________2 valence electrons
____Noble gas_____________ Complete valence shell
_______________ I’m in energy level 5 and have 6 valence electrons
_______________ I’m in Group 17 and have a mass greater than Cl
_______________I’m an alkaline earth metal with 56 neutrons
_______________ I’m the lightest noble gas
_______________ I have one valence electron but I’m a nonmetal
_______________ I’m the heaviest alkali metal
27. The forces that hold different atoms or ions together are __________
a. Electric currents
c. physical bonds
b. Chemical bonds
d. nuclear forces
28. Ionic bonds occur between _____________ and ________________
a. Metals, metals
c. metals, nonmetals
b. Nonmetals, nonmetals
d. ions
29. Covalent bonds occur between ____________ and _________________
a. Metals, metals
c. metals, nonmetals
b. Nonmetals, nonmetals
d. cations, anions
30. A charged atom is call a/an _________________
a. Ion
c. formula
b. Molecule
d. valence electron
31. Atoms joined by covalent bonds ________________ electrons
a. Gain
c. reject
Lose
d. share
32. According to the __________________, atoms will form bonds by gaining, losing or sharing valence electrons in
order to become more stable
a. Octet rule
c. Law of Conservation of Mass
b. Periodic Law
d. Chemistry Guidelines
33. The bonding characteristics of oxygen are most similar to the bonding characteristics of_
a. Hydrogen
b. Silicon
c. sulfur
d. helium
34. Which of these elements is most likely to donate one electron?
c. Be
d. Si
c. K
d. He
35. The elements of which of these groups on the periodic table are most resistant to forming compounds?
e. Group 1
f. Group 9
c. Group 14
d. Group 18
36. Elements in Group 16 of the periodic table usually
g. Form large molecules
c. gain electrons when bonding
h. Act like metals
d. solidify at room temperature
37. Which compound is formed from two oppositely charges ions?
i.
j.
Sugar, C12H22O11
Quartz, SiO2
c. carbon dioxide, CO2
d. salt, NaCl
38. According to the periodic table, which of these elements will form an ion with a -2 charge?
k. S
l. Mg
c. F
d. Rb
39. Matching
Match the molecule or compound with the type of bond: a) Covalent bond or b) Ionic bond
MgBr2 Ionic
O2
Covalent
NaF
Ionic
P205
Covalent
CO2
Covalent
40. Using subscripts in the chemical formula to make the charges of ions cancel out, which is the correct chemical
formula for Cs+1 , O-2?
a. CsO2
b. Cs2O
c. CsO
d. Cs3O
41. Using subscripts in the chemical formula to make the charges of ions cancel out, which is the correct chemical
formula for Al+3 , N-3?
c. Al3N3
d. AlN
c. AlN3
d. Al2N
42. Using subscripts in the chemical formula to make the charges of ions cancel out, which is the correct chemical
formula for Li_ , F_ (you must determine the superscripts/oxidation numbers)?
e. LiF
f. Li2F2
c. LiF3
d. Li2F
43. Using subscripts in the chemical formula to make the charges of ions cancel out, which is the correct chemical
formula for Al_ , Cl_ (you must determine the superscripts/oxidation numbers)?
g. AlCl
h. Al2Cl2
c. AlCl3
d. Al3Cl
44. Matching
Match the element with its oxidation number
C-D
a. +1
Na - A
b. -2
S-B
c. 0
He - C
d. +/- 4
45. A bond in which electrons are shared unequally resulting in a slightly positive and slightly negative end is called a
i.
j.
Nonpolar bond
Hydrate bond
c. Polar bond
d. Metallic bond
46. Metals typically lose electrons and become positively charged ions called
k. Anions
l. Cations
c. positrons
d. isotopes