Name ________________KEY_______________________________
Block ___________
Chemistry Unit Review
Study all vocabulary terms used this quarter: atom, element, compound, proton, neutron, electron,
atomic mass, atomic number, valence electrons, molecules, mixture, homogeneous mixture, heterogeneous
mixture, pure substance, solution, period, group, reactivity, metals, nonmetals, metalloids, ductile,
malleable, luster, brittle, radioactive, synthetic, physical change, chemical change, chemical reaction,
precipitate, catalyst, corrosion, oxidation, subscript, coefficient, reactant, product, law of conservation
of mass.
Unit One: Matter
Element = A substance that cannot be broken down into a simpler substance. Made up of only
one type of atom.
Compound = A pure substance that is created by 2 or more elements chemically reacting and
joining together.
1. Circle all the elements and underline the compounds below. 2. On the line provided, record
the number of different symbols within the species.
CO __2_
(Mg) _1__
(Co) _1__
C2H5OH _4__
Al(CN)3 _3__
(Cl2)_1__
H2SO4 _3__
(He) _1__
NI3 _2__
(O2)_1__
H2O __2_
NaCl _2__
(C)_1__
(Cu) _1__
(I) _1__
Questions:
1) Does each compound have the same number of symbols? _______No__________
2) For each ELEMENT above, how many total symbols are listed? _______8____________
3) What is the minimum number of symbols that must be present in order for a species to be
considered a compound? ___2_____________________________________________
Classification of Matter: WORD BANK: Chemical changes, chemical property, compound, element,
heterogeneous matter, homogeneous matter, matter, mixture, physical changes,
physical property, property, substance
_____Matte___ is anything that has mass and volume. Matter that has uniform
characteristics throughout is called ___Homogenous Matter_______. Matter that has parts
with different characteristics is called ____Heterogenous Matter___________
_____. A characteristic by which a variety of matter is recognized is called a(n)
____Property_______. A characteristic that can be observed without producing new kinds of
matter is called a(n) _____Physical Property________. A characteristic that depends on how
a kind of matter changes its composition (or fails to change its composition) during interactions
with other kinds of matter is called a(n) __chemical property____. ____Chemical
Changes_____alter the identity of a substance, whereas ______physical changes_____ do not.
A simple substance that can not be broken down into other substances by chemical means is a(n)
_____element____. A chemical combination of simple substance is a __compound ___.
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Classify the following as an element (E), compound (C) or a mixture (M). If a mixture,
determine if it is a heterogeneous mixture or a homogeneous mixture.
Water is a compound.
Compound or heterogenous mixture
Air is a homogenous mxture.
Mercury is an element.
Carbon dioxide is a compound
Kool-aide is a homogenous mixture.
Copper is an element.
Concrete is a homogenous mixture.
Iron is an element.
Chicken noodle soup is a heterogenous mixture.
Salt water is a homogenous mixture.
Milk is a homogenous mixture.
Heterogenous Mixtures
Element
Homogenous Mixture
Compound
Homogenous Mixture
Heterogenous Mixture
Element
Heterogenous Mixture
Elements
Compounds
Mixtures
Mixtures
Compounds
Electrons and compounds
Compounds
Electrons
Mixtures
Mixtures
Elements
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B
C
D
A
B
A
E
A
E
B
D
D
D
D
3
E
Separating Mixtures:
1. Describe the separation technique you could use to separate a solid and a liquid.
Filtration and/or evaporation
2. Describe the separation technique that could be used to separate salt water.
Evaporation
3. Describe how you could separate a mixture of salt, water and sand.
Evaporation then magnetism.
Unit Two: Periodic Table and Properties of Matter
Atomic Structure:
**Nucleons = PROTONS and NEUTRONS; any subatomic particles found w/in the nucleus
Subatomic Particle
Charge
Location
Symbol
How to Calculate
Proton
Positive
Nucleus
+
= to atomic #
Neutron
Neutral
Nucleus
O
Atomic mass – atomic
#
Electron
Negative
Oribital/shell/Energy
Level
-
= to atomic #
What is the name of the element that has:
1. 5 protons? _Boron (B)________________
2. 16 electrons? __Sulfur (S)____________
3. 6 neutrons? __Carbon (C)_____________
4. 17 protons? __Chlorine (Cl)____________
5. 32 electrons? _Germanium (Ge)________
6. 25 protons? __Manganese (Mn)_________
7. 16 neutrons? __Phosphorus (P)_________
8. 1 electron? _Hydrogen (H)_____________
9. 82 protons? __Lead (Pb)______________
10. 8 electrons? __Oxygen (O)_____________
11. 92 protons? __Uranium (U)_____________
12. 2 electrons? __Helium (He)____________
13. 35 neutrons? __Zinc (Zn)_____________
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1. Draw the correct Bohr model for an atom
of oxygen.
2. Draw the correct Bohr model for an atom
of potassium.
3. How many valence electrons are there in an atom of fluorine? ___7_____
4. How many valence electrons are there in an atom of beryllium atom? ____2_____
5. How many energy levels are there in a phosphorus atom? ___3_____
6. How many valence electrons are there in a phosphorus atom? ___1_____
7. How many energy levels are there in a bromine atom? ___4_____
8. What is the one thing that can always be used to identify an element because it also never
changes? ___number of protons_________________________________________
9. The total number of electrons in a neutral atom is the same as which number? Atomic #
10. Which of the subatomic particles are located in the nucleus? _protons and neutrons____
11. Which of the subatomic particles are located outside the nucleus? ___electrons__
12. Which of the subatomic particles have charge (+ or -)? __protons (+) and electrons (-)____
13. Which of the subatomic particles have mass? __protons and neutrons____________
14. If you have the nuclear charge or the number of protons in a neutral atom, what other
number(s) or information do you also know? _the # of electrons and atomic #____________
15. What is the advantage to using the Bohr model as opposed to the Lewis model?
(a.) The Bohr model provides more information than the Lewis model.
b. The Bohr model is less bulky than the Lewis model.
c. The Bohr model shows the valence electrons.
d. The Bohr model shows how many bonds atoms of an element can form.
16. What is the advantage to using the Lewis model as opposed to the Bohr model?
a. The Lewis model provides more information than the Bohr model.
b. The Lewis model is less bulky than the Bohr model.
(c.) The Lewis model shows the valence electrons.
d. The Lewis model shows how many bonds atoms of an element can form.
17. What is the maximum number of electrons an atom or an ion can have in its valence shell?
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a. 2
b. 4
c. 6
(d.) 8
18. The number of bonds an atom of an element can form is the same as the number of
a. electrons in its valence shell.
b. paired electrons in its valence shell.
(c.) unpaired electrons in its valence shell.
19. An atom of which of the following elements can form the most bonds? (Hint: Look at your
Lewis diagrams)
a. Phosphorus
b. Oxygen
(c.) Sodium
d. Carbon
Element Practice:
__Rubidium (Rb)_________ 1. a alkali metal in the fifth period.
__Krypton (Kr)__________ 2. an element that completes the 4th period
__Astatine (Ar)_________ 3. the most reactive non metal
__Iodine (I)____________ 4. a solid halogen
__Mercury (Hg)_________ 5. a liquid element in transition metals
__Oxygen (O)__________ 6. a gas in the 16th group
__Calcium (Ca)__________ 7. a alkaline earth metal necessary for bones
__Hydrogen (H)_________ 8. an element that is in a family all by itself
__Carbon (C)___________ 9. a gas needed to support all living things
__Hydrogen (H)_________ 10. a flammable gas in the first period
__Iodine (I)____________ 11. a solid halogen used as an antiseptic medication
__Selenium (Se)_________ 12. a solid non metal in the 4th period
__Carbon (C)___________ 13. a black non metal used to make diamond, graphite, and charcoal
__Aluminum (Al)_________ 14. a period three element with 3 valence electrons
__Sodium (Na)_________ 15. potassium shares more properties with calcium or sodium?
Explain. Sodium and potassium are in the same group; therefore, the share similar properties.
16. all alkali metals are highly reactive. What causes this similarity among the family? _______
_______They all have 1 valence electron._________________________________
17. number of valence electrons in the halogen family. ____7____________
18. this family has two valence electrons _____Alkaline Earth Metal___________________
Choose the best element from the following choices: Si, Fr, Hg, and Ne
1. one valence electron ___Fr_______
2. the shiny, brittle element that conducts electricity and does not react with acid __Si_____
3. the least reactive element ___Ne_______
Choose the best element from the following choices: N, P, O, and S
4. the element in the third period ___P________
5. a gas with 5 valence electrons ___N__________
6.a yellow solid with six valence electrons ____S__________
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Choose from the following elements:
Cs, Na, Si, P, Cl, and Ar
7. the least reactive element _______Ar________________
8. the most reactive metal ____Cs___________________
9. a metalloid ______Si______________________
10. a solid brittle, dull element that does not conduct electricity ____P_________________
11. an element with 5 valence electrons ________P________________
12. Which of the following in each pair of elements is more reactive? Circle answer.
a. (Cs), Ba
b.( Cl), Ar
c. Na, (Rb)
d. F, (Br)
e. (O), F
f. N, (C)
The Periodic Table:
Use your notes or your textbook, the blank periodic table worksheet, and crayons or colored
pencils to identify and indicate the different parts of the periodic table as instructed below:
1. Color the alkali metals green.
2. Color the alkaline earth metals blue.
3. Color the transition metals yellow.
4. Color the noble gases orange.
5. Color the halogens pink
6. Color the lanthanides purple.
7. Color the actinides red.
8. Highlight the line that separates the metals from the nonmetals with black.
9. Put a black dot in the metalloid element boxes.
10. Outline the boxes of the elements that are gases at room temperature with red.
11. Outline the boxes of the elements that are liquids at room temperature with blue.
12. Include a key in a blank area of the periodic table worksheet to indicate each of the above
parts of the table.
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Properties: Identify the following as being a physical or chemical property.
_____P_______ 1. The mass of copper wire is 255 g.
_____P_______ 2. The boiling point of ethyl alcohol is 77°C.
_____C_______ 3. Baking soda reacts with vinegar to make carbon dioxide gas.
_____P_______ 4. The density of mercury is 13.6g/mL.
_____P_______ 5. The solubility of sodium chloride in water is 40g/100mL of water.
Unit Three: Changes & Law of Conservation of Matter
Identify the following changes as either physical (P) or chemical (C):
1. __P____ Water boiling
2. ___C___ iron rusting
3. __P____ butter melting
4. ___P___ rubbing alcohol evaporating
5. __C____ wood rotting
6. ___P___ leaves changing color
7. __P____ glass breaking
8. ___P___ mowing the lawn
9. __P____ magnetizing a nail
10. ___C___ baking a cake
11. __C____ a piece of wood burns to form ash 12. ___P___ water turns into steam
13. __P____ a piece of cork is cut in half
14. ___C___ a bicycle chain rusts
15. __C____ food is digested in the stomach
16. ___P__ water is absorbed by a paper towel
17. __C___ Hydrochloric acid reacts with zinc 18. ___C__ a piece of apple rots on the ground
19. __P____ a tire is inflated with air
20. ___C___ a plant makes its own food
21. __P____ sugar dissolved in water
22. ___C___ eggs turn into an omlet
23. __C____ milk sours
24. ___P___ a popsicle melts
25. __C____ turning brownie mix into brownies
LAW of CONSERVATION of ENERGY/MASS/MATTER = during a chemical reaction, energy,
mass, and atoms can __not____ be created or destroyed.
Consider the following balanced equation for the reaction between iron metal and water:
3Fe + 4H2O → Fe3O4 + 4H2
1. Is the 3 in 3Fe a subscript or a coefficient? ____coefficient_____________________
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2. What is the subscript in the water molecule? ______2_________________
3. How can you tell that a chemical equation is balanced? __The number of atoms must be the
same for each element on both sides of the chemical equation. _______________
4. Water vapor and nitrogen dioxide gas (NO2) are combined to manufacture ammonia (NH3). A
byproduct of this reaction is oxygen gas. Write the balanced chemical equation for this
reaction. __3H2O + 2NO2 - 2NH3 + 7O_____________________________
5. Iron can be obtained by reacting the naturally occurring ore hematite (Fe2O3) with carbon.
The carbon is converted to CO2. Write the balanced chemical equation for this reaction.
__2Fe2O3 + 3C  3CO2 + 4Fe_______________________________________
6. Granules of zinc oxide (ZnO) will react with hydrochloric acid (HCl) to form zinc chloride
(ZnCl2) and water. Write the balanced chemical equation for this reaction.
___ZnO + 2HCl  ZnCl2 + H2O_________________________________________
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