CP1 CHEMISTRY CONNECTIONS
MID-YEAR EXAM STUDY GUIDE
The format of the mid-year exam is as follows:
30 Multiple Choice Questions (1 pt each)
10 Fill-in-the-Blank Questions (1 pt each)
2 Essay Questions (10 pts each)
For the essay section, you will be given three choices. It will be your choice for which two out of
the three you answer. You are not allowed to bring in a prepared essay or outline, but you can
look ahead at the questions:
Essay Choice #1: Explain how the photoelectric effect allows the automatic doors at the
supermarket to work. Your explanation must include the definition of the photoelectric effect.
Essay Choice #2: Carl Sagan, a famous astronomer, once said “we are all made of star stuff.”
Explain what this quote means by describing how elements are made in the stars. Your
explanation must include the definition of nuclear fusion and use specific elements when talking
about the process.
Essay Choice #3: Explain the difference between a hypothesis, a theory, and a law using any
scientific example.
The following guides provide you with the objectives from each unit and practice questions for
the multiple choice and fill-in sections of the test. Vocabulary is underlined within the objectives,
and a master word bank is given at the end.
TOPIC 1: EINSTEIN’S MIRACULOUS YEAR
Objectives:
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List the three particles that make up an atom. (MA 2.2)
Match each particle type with its charge, size, and location. (MA 2.2)
Label the crest, trough, and wavelength of a wave.
Define frequency and amplitude for a wave.
List the seven types of light that make up the electromagnetic spectrum.
List one use of each type of light in the electromagnetic spectrum.
Define photoelectric effect.
List three uses of the photoelectric effect.
Describe how intensity and frequency affect the photoelectric effect.
Define Brownian motion.
Practice Questions:
1) How many particles make up an atom?
a. One
b. Two
c. Three
d. Four
2) What is the distance between two waves?
a. Amplitude
b. Frequency
c. Wavelength
d. Trough
e. Crest
3) If a type of light has lots of waves, it has…
a. A high frequency
b. A low frequency
c. A high wavelength
d. A low wavelength
4) What particle is given off when light hits a
metal?
a. Proton
b. Electron
c. Neutron
5) What type of light would be able to cook your
popcorn?
a. Radio waves
b. Gamma rays
c. Visible light
d. Microwaves
6) True or False – The intensity of the light causes
the photoelectric effect.
a. True
b. False
7) True or False – Every metal has its own
threshold frequency.
a. True
b. False
8) To explain the photoelectric effect, Einstein said
it’s best to think of light as…
a. A wave
b. A particle
9) When does the photoelectric effect work?
a. When the incoming photon has more energy than the threshold frequency of the metal
b. When the incoming photon has less energy than the threshold frequency of the metal
10) What causes Brownian motion?
a. Pollen in water
b. Shaking a water sample
c. Collisions between particles
11) What did Brownian motion prove the existence of?
a. Atoms
b. Protons
c. Electrons
d. Neutrons
TOPIC 2: THE NEW ALCHEMY
Objectives:
 Define transuranium elements and locate them on a blank periodic table.
 Write the symbol for an alpha particle, beta particle, and positron.
 Identify the type of radioactive decay (alpha, beta, or positron) when given a nuclear equation
(MA 2.5)
 Fill in one missing particle for a nuclear equation and identify its type. (MA 2.5)
 Fill in two missing particles for a nuclear equation when given its type. (MA 2.5)
 Compare and contrast nuclear fission and nuclear fusion. (MA 2.7)
 Describe how stars create elements up to iron through fusion (hydrogen becomes helium, and
helium makes everything else).
Practice Questions:
1) An alpha particle is the same as what?
a. An electron
b. An electron with a positive charge
c. A helium nucleus
2) A beta particle is the same as what?
a. An electron
b. An electron with a positive charge
c. A helium nucleus
3) A positron is the same as what?
a. An electron
b. An electron with a positive charge
c. A helium nucleus
4) What must be equal about all nuclear
equations?
a. Mass numbers on both sides
b. Atomic numbers on both sides
c. Mass numbers & atomic numbers
on both sides
d. The atomic numbers on one side
and the mass numbers on the other
5) These are atoms that have the same atomic
number but different mass numbers.
a. Isotopes
b. Nuclei
c. Nucleons
d. Nuclides
6) Which of the following is an isotope of
tellurium?
a. 53Te
b.
53Te
c.
53Te
d.
52Te
7) Write balanced nuclear equations for the following, and name the type of radioactive decay (emission) for
the equation.
a. 24Cr + -1e  ________
type: ______________________________________
b.
88Ra
 _______ + 2He
type: ______________________________________
c.
93Np
 _______ + +1e
type: ______________________________________
d.
91Pa
 _______ + -1e
type: ______________________________________
TOPIC 3: SOLUTIONS & CLASSIFYING MATTER
Objectives:
 Explain the difference between pure substances (elements and compounds) and mixtures. (MA
1.2)
 Differentiate between heterogeneous and homogeneous mixtures. (MA 1.2)
 Define solution, solute, and solvent. (MA 7.1)
 Explain the process of solvation. (MA 7.1)
 Identify and explain four factors that affect how fast a solid solute can dissolve (temperature,
surface area [crushed vs. cube], mixing, and polarity [“like dissolves like”].) (MA 7.3)
 Name the three types of bonds (polar, nonpolar, ionic).
 Define saturated solution, unsaturated solution, and supersaturated solution.
 Explain how to test a solution to see if it is saturated, unsaturated, or supersaturated.
 Define crystal.
 Define electrolyte and nonelectrolyte and give an example of each.
Practice Questions:
1) Sand is an example of a(n)
a. Compound
b. Element
c. Heterogeneous mixture
d. Solution
2) Which of the following is a homogeneous
mixture?
a. iron filings (little pieces of iron you
can use to find a magnetic field)
b. sugar dissolved in water
c. sand in water
d. solid carbon dioxide (dry ice)
3) A substance made of only one kind of atom
is a(n)_____________
a. element
b. compound
c. solution
d. heterogeneous mixture
4) In a solution, the substance being dissolved
is the ________
a. solvent
b. solute
c. mole fraction
d. hydrate
5) The process by which solvent molecules
surround solute particles is…
a. efflorescence
b. solvation
c. displacement
d. deliquescence
6) A solution in which more solute can
dissolve is called a(n) __________
a. dilute solution
b. supersaturated solution
c. saturated solution
d. unsaturated solution
7) Two words that describe the pattern of the
arrangement of the atoms in a crystal are…
a. disorderly and repeating
b. orderly and repeating
c. disorderly and non-repeating
d. orderly and non-repeating
8) A crystal of copper (II) sulfate is added to a
copper (II) sulfate solution. After 15
minutes, the crystal is still there on the
bottom of the solution, unchanged. On the
basis of this observation, the solution is best
described as…
a. supersaturated
b. dilute
c. saturated
d. unsaturated
9) Which of the following explains the ability
of water (polar covalent) to dissolve ionic
substances?
a. like dissolves like
b. unlike dissolves like
c. unlike dissolves unlike
d. polar and ionic mean the same
thing
10) Gatorade will light up a light bulb because it contains
a. nonelectrolytes
b. sugar
c. electrolytes
d. water
TOPIC 4: WHY WE USE WHAT WE DO
Objectives:
 Distinguish between chemical and physical properties and between chemical and physical
changes. (MA 1.1)
 Classify specific examples as either chemical or physical properties and chemical or physical
changes. (MA 1.1)
 Classify specific elements as metals, nonmetals, or metalloids based on observations of chemical
and physical properties. (MA 3.2)
 Use the periodic table to locate periods and groups (families) of elements. (MA 3.1)
Practice Questions:
1) A chemical change must produce a…
a. Solution
b. Gas
c. New substance
d. Mixture
2) Which of the following is a chemical
property of magnesium?
a. Oxidizes to produce a white
powder
b. Has a density of 1.738 g/cm3
c. Is ductile
d. Melts at 650°C
3) Which of the following is an example of a
chemical change?
a. Wood burning
b. Snow melting
c. Cheese being shredded
d. An orange being squeezed
4) Which of the following is a physical
change?
a. Bread toasting
b. Butter melting
c. An egg frying
d. An apple being digested
5) In the periodic table, all of the elements in a
horizontal row are referred to as a…
a. Period
b. Group
c. Family
d. Triad
6) Groups 16, 17, and 18 of the periodic table
contain mostly
a. Alkaline earth metals
b. Transition metals
c. actinides
d. nonmetals
7) Which of the following describes the
locations of the halogens in the periodic
table?
a. Column 18
b. Columns 3-12
c. Column 16
d. Column 17
8) A substance that conducts heat well, is
shiny, and is malleable is best classified as
a…
a. Nonmetal
b. Metalloid
c. Metal
9) Which of the following is an example of a
metalloid?
a. I
b. B
c. Br
d. In
10) In the periodic table, Group 2 is known as
the …
a. Alkaline earth metal family
b. Noble gases
c. Chalcogen family
Topic 5: Earth’s Natural Resources
Objectives:
 Describe Earth’s atmosphere, hydrosphere, and lithosphere, including the distribution of
resources among them.
 Describe or recognize factors that determine the feasibility of mining an ore at a specific site.
 Use the activity series to explain why minerals of more active metals are more difficult to refine
and process than minerals of less active metals.
 Match chemical reactions with their type. (MA 5.2)
Practice Questions:
1) Which of the following is NOT a place
where we find Earth’s natural resources?
a.
lithosphere
b.
atmosphere
c.
blogosphere
d.
hydrosphere
2) Which of the following resources would
be found in the hydrosphere?
5) Which TWO the following are a qualities
of a “useful ore”?
a.
low percent of metal within the
ore
b.
high percent of metal within the
ore
c.
difficulty in processing the ore
d.
easy to process the ore
a.
nitrogen gas
b.
iron ore
a.
active metals
c.
water
b.
non-active metals
d.
silicates
c.
radioactive metals
3) Where do we get natural resources from in
the lithosphere?
6) Which metals are easier to process?
7) Are metals at the top of the activity series
active or non-active?
a.
inner core
a.
active
b.
crust
b.
non-active
c.
mantle
d.
outer core
4) List four factors that must be considered
when opening a new mine.
8) In the reaction A + BC  B + AC, A must
be __________ B on the activity series.
a.
higher than
b.
lower than
c.
equal to
9) A + BC  B + AC = what type of reaction?
a.
synthesis
b.
decomposition
c.
single replacement
d.
double replacement
10) AB  A + B = what type of reaction?
a.
Synthesis
b.
Decomposition
c.
Single replacement
Unit 6: Conserving Matter
Objectives:
 Define hypothesis, theory, and law.
 State the law of conservation of mass (matter).
 Count the number of atoms of each element within a compound.
 Balance chemical reactions. (MA 5.1)
Practice Questions:
1) Using the law of conservation of mass, explain why the following reaction is wrong: HCl + NaOH 
NaCl.
2) How can you tell when an equation is balanced?
3) Consider the following balanced equation for the reaction between iron metal and water:
3 Fe + 4 H2O  Fe3O4 + 4 H2
a.
Is the 3 in 3 Fe a subscript or a coefficient?
b.
What is the subscript in the water molecule?
c.
How does changing a coefficient different from changing a subscript?
d.
Why is Fe balanced as 3Fe instead of Fe3?
e.
What do the 4 and 2 mean in 4 H2? How many hydrogen atoms are there?
4) Balance the following reactions:
a.
___H2O + ___NO2  ___NH3 + ___O2
b.
___Fe2O3 + ___C  ___Fe + ___CO2
c.
___ZnO + ___HCl  ___ZnCl2 + ___H2O
d.
___Cu + ___HNO3  ___Cu(NO3)2 + ___NO + ___H2O
e.
___C2H6 + ___O2  ___CO2 + ___H2O
CHEMISTRY CONNECTIONS MID-YEAR WORD BANK
Actinides
Activity series
Alkali metals
Alkaline earth metals
Alpha particle
Amplitude
Aqueous solution
Atmosphere
Atomic number
Atom
Beta particle
Brownian motion
Chemical bond
Chemical change
Chemical equation
Chemical formula
Chemical property
Chemical reaction
Compound
Concentration
Core
Covalent bond
Crest
Crust
Crystalline solid (crystal)
Decomposition reaction
Density
Double replacement reaction
Ductile
Electrolyte
Electromagnetic spectrum
Electrons
Element
Excited state
Family
Fission
Frequency
Fusion
Gamma rays
Ground state
Group
Half-life
Halogens
Heterogeneous mixture
Homogeneous mixture
Hydrosphere
Hypothesis
Infrared light
Intensity
Intermolecular forces (IMFs)
Ion
Ionic bonds
Isotopes
Lanthanides
Law
Law of conservation of mass
(matter)
Lithosphere
Malleability
Malleable
Mantle
Mass number
Matter
Metal
Metalloid
Microwaves
Mineral
Molecule
Neutrons
Noble gases
Nonelectrolyte
Nonmetal
Nonpolar bond
Nucleus
Ore
Periodicity
Periodic table
Periods
Photoelectric effect
Photon
Physical change
Physical property
Polar bond
Positron
Products
Protons
Radioactive decay
Radio Waves
Rare earth metals
Reactant (reagent)
Saturated solution
Scientific method
Single replacement reaction
Soluble
Solute
Solution
Solvent
Supersaturated solution
Synthesis reaction
Theory
Transition metals
Transuranium elements
Trough
Ultraviolet light
Unsaturated solution
Valence electrons
Visible light
Wavelength
Wave-particle duality
X-rays