Name: _________________________________________ Date: ________________ Period: ___________
CP Chemistry Semester 1 Final Test Review
CHAPTERS 1 & 2: Scientific Method, Density, Metric Conversions, Accuracy/Precision, Significant Figures
1. Know the steps in the scientific method.
A. Define each of the steps.
B. What is the difference between a theory and a scientific law?
C. What is the difference between a hypothesis and a theory?
2. Know the symbol and the power of 10 for the following metric prefixes:
A. Mega
D. deka (or deca)
G. centi
B. kilo
E. base units (m, s, L, g)
H. milli
C. hecto
F. deci
I. micro
3. Metric Conversions: Give the value of the following in the units indicated.
a. 6.92 cm = ____________ m
e.
934 µm = ___________ mm
b. 8 Mg = ______________ kg
f.
550 mL = ____________ L
c. 35 km = _____________ cm
g.
6,450,000 mg = _______kg
d. 520 ml = _____________ L
h.
0.075 g = ____________ mg
Density Problems: Calculate the following using correct units and significant digits.
4. A metal has a volume of 8.4 mL and a mass of 32.0 g. What is its density?
5. A solid object has a density of 7.00 g/mL and a volume of 12.0 mL. What is its mass?
6. An object has a density of 9.0 g/mL and a mass of 41.2 g. What is its volume?
7. Be able to read and interpret data off a line graph.
a. If the mass is 30 grams,
what is the volume?
b. What is the mass if you
have 10 mL of substance X?
30
c. Calculate the approximate
slope of the line.
20
d. Calculate the approximate
density of the substance X.
10
Mass in grams
40
50
MASS v. VOLUME FOR SAMPLES OF
SUBSTANCE X
5
10
15
20
25
30
35
Volume in mL
8. Know the correct number of significant figures to report in calculations.
Report these answers to the correct number of significant figures.
A. 3.461 + 14.9 + 5.26331
B.
4605.32 ÷ 6.5
9. Know the difference between Precision and Accuracy.
Identify each of the targets to the right as
ACCURATE and/or PRECISE.
CHAPTER 3: Matter: Physical and Chemical Changes
10. Explain the difference between a homogeneous mixture (solution) and a heterogeneous mixture. Give an
example of each.
Heterogeneous Mixture :
Homogeneous Mixture:
11. Explain the difference between a physical change and a chemical change. Give an example of each.
Physical Change :
Chemical Change:
12. Conservation of mass problems (mass of reactants = mass of products):
a.
Water is decomposed into hydrogen and oxygen. If 10.0 grams of hydrogen and 79.5 grams of
oxygen are collected, how much water did you start with?
b.
If 25 grams of sodium reacts with chlorine to form 99 grams of salt (NaCl). How many grams of
chlorine reacted?
CHAPTERS 4 & 25: The Atom and Nuclear Chemistry
13.
Which part of the atom has most of the mass but very little volume?
14.
What are the charges and masses of protons, electrons, and neutrons?
symbol
mass (amu)
charge
proton
neutron
electron
15.
What are the differences in the atomic number, atomic mass and mass number?
Definition
Atomic
number
Mass
number
Atomic
mass
How to calculate
16.
What is the definition of an isotope?
17.
Why do isotopes of the same element (ex. carbon-12, carbon-13, carbon-14) have different mass
numbers?
Which isotope is the standard for the atomic mass unit (amu)?
18.
19.
Calculate the number of protons, neutrons and electrons in an isotope when given its mass number
and atomic number.
Element
atomic
number
mass
number
protons
64
29
Copper (Cu)
Neon (Ne)
neutrons
10
electrons
Isotope name
(using name)
Isotope name
(using
symbol)
11
Magnesium-26
20.
In a chemical reaction, what changes in the atom and what is formed?
21.
In a nuclear reaction, what changes in the atom and what is formed?
22.
Use the following data table on the isotopes of element “X” to answer Questions A&B listed below:
Percent
Isotope
Mass in amu
Abundance %
X-20
19.992
90.48
X-21
20.994
0.2700
X-22
21.991
9.250
A. What is the weighted average atomic mass of element “X”?
B. Using the periodic table what is the identity and atomic number of element “X”?
23.
24.
Assume the following three isotopes of element Z exist: Z-248, Z-252, and Z-259. If the atomic
mass of Z is 258.63 amu, which of these isotopes is most abundant?
Why does radioactivity occur?
25. Know that the forms of natural radioactivity are alpha, beta, and gamma.
symbol
Mass (amu)
charge
Damage caused
Alpha α
Beta β
Gamma γ
26. Which form of radiation has the lowest energy (ex. can be stopped by paper)?
Which form has the highest energy (ex. will pass through several feet of concrete)?
27. What particles would you use to balance the following nuclear reactions?
A.
(a)
(b)
(c)
B.
(a)
(b)
(c)
C.
(a)
(b)
(c)
28. What is the difference between nuclear fusion and nuclear fission?
29. Identify the following as fission or fusion reactions and fill in the blank:
A.
 _______ +
______________________

B.
______________________
30. What is half – life?
31. Know how to solve half-life problems: Na- 24 has a half-life of 15 hours. How long will it take for a
sample to decay to 12.5% of its original mass
32. Write and balance the following equations:
A.
Radon-222 undergoes alpha decay
B.
Uranium-238 undergoes beta decay
CHAPTER 5: Electrons in Atoms
33. Give the (1) electron configuration (2) noble gas shorthand and (3) orbital filling diagram for the
following elements.
a. Sulfur
b.
Copper
34. Give the Lewis electron dot diagrams for the following elements.
C. Ge
A. Mg
B.
K
D.
F
E.
O
F.
B
35. Know how to convert between wavelength and frequency (c = 3.00 x 108 m/s).
a. What is the wavelength of electromagnetic radiation having a frequency of 5.00×1012 Hz?
b. What is the frequency of electromagnetic radiation having a wavelength of 3.33×10-8 m?
CHAPTER 6 – The Periodic Table
36. Periodic Table Organization
A. The periodic table is arranged by increasing ________________.
B.
Rows on a periodic table are called _______________. Columns on a periodic table are called
_________________________.
C.
Properties of elements in the same (period or group) change as you move left to right or right
to left and repeat as you move from one to the next.
D.
Properties of elements in a (period or group) are similar.
E.
All atoms of the same element contain the same number of what particle?
____________________
F. Identify the location of these groups or families: Alkali Metals _______________ Alkaline
Earth Metals ______________ Halogens _____________ Noble Gases ____________________
G.
Given the electron configuration, identify the element, period and group on the periodic table:
[Ne]3s23p2
[Kr]5s2
[Ne]3s23p6
[Ar] 4s1
[Ne]3s23p5
Element
Period
Group
Metal/ nonmetal/
metalloid?
37. Periodic Table Trends
Know the definitions of each property and the general trends by group and period for:
Electronegativity:
Which element has the highest electronegativity?
Which group/family has ZERO electronegativity?
Ionization Energy:
Atomic Size (atomic radius):
Ionic size (ion radius):
A.
Identify which of the element in each pair has the LARGER atomic radius:
a.
B.
K and Sc
b. Cl and I
c. Ca or Ga
List the elements in order of INCREASING electronegativity:
a.
O, S, Se
b. Al, Cl, P
c. Ca, Mg, Sr
d. Se or O
CHAPTER 8 – Ionic Compounds
38. An ion is an atom that has gained or lost ___________ in order to become more stable; by achieving the
noble gas configuration.
39. Complete the table for the ATOMS and IONS of these elements:
Element
Element
Symbol
Atomic
Number
# Valence Electrons in
the Atom
Total Number of
Electrons in an Atom
Total Number of
Electrons in an Ion
Ion symbol
Mg2+
Magnesium
Oxygen
O
Phosphorus
P
13
Iodine
I
3
40. An ionic bond forms between what types of elements? ____________________________________
An ionic bond is the attraction between _________________________ and ____________________
In an ionic bond, electrons are __________________________.
What is the structure of a solid ionic compound?
What are properties of ionic compounds?
41. A chemical formula tells you _________________________________, as indicated by subscripts.
MgCl2 means ______ magnesium and _____ chlorine atoms in the compound.
42. Complete the tables below:
Compound Name
Chemical Formula
Iron (III) Sulfate
NiCl3
Aluminum Sulfide
BeF2
43. What is the charge of the manganese ion in each of the compounds listed below?
a. MnSO3
B. MnPO4
C. Mn3Al2
D. MnO2