Name:
Unit 3 Study Guide
PHYSICAL PROPERTIES
For the following vocabulary words you should know and understand the definition.
Kinetic Energy
Heat Energy
Law of conservation of energy
Melting point
Boiling Point
Freezing point
Condensation
Sublimation
Deposition
Liquid
Solid
Gas
Matter
Atom
Physical change
Physical properties
Intensive properties
Extensive properties
Hydrogen Bonds.
Intermolecular Forces
polarity
Be able to address the below assessment statements:
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Identify properties of matter as extensive or intensive
Define physical property and list several common physical properties of substances
Differentiate among three states of matter
Describe a physical change
Know how matter changes between phases (liquid, solid, gas)
Be able to look at a heat curve and label the following features:
a. Liquid
b. Solid
c. Gas
d. Melting point
e. Boiling point
Be able to look at the melting and boiling point of a substance and determine what state (liquid, solid,
gas) it is in at a given temperature.
Determine the relationship between intermolecular forces (i.e. hydrogen bonds) and boiling points
Draw and label a diagram showing the structure of water molecules to show their polarity and
hydrogen bond formation.
Be able to analyze a phase change diagram (the graph that shows how a substance changes phases (gas,
solid, liquid) because of pressure (atm) and temperature changes.
CHEMICAL PROPERTIES
Know the definitions to the following vocabulary words:
Chemical change
Protons
Chemical reaction
Atomic mass
Physical change
Mass number
Atom
Atomic number
Electrons
Oxidation number
Valence electrons
Octet rule
Electron/ energy
Ion
shells
Cation
Neutrons
Anion
Address the learning objectives below
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Element
Period
Groups/ families
Metals
Non-metals
Metalloids
alkali metals
alkaline earth
metals
transition metals
chalcogens
halogens
noble gases
isotope
Compare a physical change to a chemical change
Using you periodic table be able identify and calculate the number of protons, neutrons, electrons, atomic
number, and atomic mass of any element.
Explain what makes elements and isotopes different from each other
Calculate the number of neutrons in an atom
Calculate the atomic mass and the average atomic mass of an element
Using your periodic table be able to draw the electrons and electron shells of the first 18 elements on the
periodic table.
Using your periodic table be able to predict valence electrons and oxidation number of the group A
elements.
Using your periodic table be able to predict the number of electron shells/ energy levels of any element.
Know the basic characteristics of the following families/ groups of elements on the periodic table (alkali
metals, alkaline earth metal, chalcogens, halogens, noble gases, and transition metals.
Compare ionic, covalent bonding, metallic bonding.
Given a name of an ionic compound or a covalent molecule be able to write its chemical formula with correct
subscript
Given a chemical formula be able to write its proper chemical name.
Term 2: Summative Test 1 Review Packet
1. Unit 3: Use the graphic organizer below to compare Gas, Liquid, Solid
Gas
Liquid
Volume (Yes, no)
Density (High, Low)
Energy (High, Low)
Shape (Yes, no)
Compress ability (yes,
no)
Solid
2. Unit 3: Use the graphic organizer below to compare intensive and extensive properties.
Extensive
Intensive
Definition
Example
On Crosbia, bolonium (Bg) and manasium (Ma) react together to form the compound tastegudum. For each of the
questions on this worksheet, refer to the phase diagram for tastegudum.
1. Label the regions of the diagram that correspond to the solid, liquid, and vapor phases. (Write the names of these
phases in the appropriate regions directly on the diagram.)
2. What is the boiling point temperature for tastegudum when the external pressure is 60 atmospheres? Ans:
______________________
3. What is the freezing point temperature for tastegudum when the external pressure is 60 atmospheres? Ans:
______________________
4. A container of tastegudum is sitting at a pressure of 45 atmospheres and temperature of 100 °C. Describe what will
happen as the temperature is raised by 400 °C (identify the phase change)
5. A container of tastegudum is sitting at a temperature of 300 °C under 1 atmosphere of pressure. Describe what will
happen as the pressure is increased to 90 atmospheres (identify the phase change).
PART B – HEATING CURVES. Use the heating curve to the right to answer the following questions:
6. What is the melting point of the substance?
.
7. What is the boiling point of the substance?
.
8. Which letter represents heating of the solid?
.
9. Which letter represents heating of the vapor?
.
10. Which letter represents melting of the solid?
.
11. Which letter represents boiling of the liquid?
.
12. At points b and d why doesn’t the temperature
change even though heat energy is added?
.
13. Why is an atom electrically neutral?
14. What does the atomic number of each atom represent?
15. How many protons are in the nuclei of the following atoms?
a. phosphorus
.
b. molybdenum
.
c. aluminum
.
d. cadmium
.
e. chromium
.
f. lead
.
16. What is the difference between the mass number and the atomic number of an atom?
17. What is the atomic mass of an element?
18. How many electrons are in the highest occupied energy level (valence Electrons) of these atoms?
a. Barium
.
b. sodium
.
c. aluminum
.
d. oxygen
.
19. Here are three isotopes of an element:
12C
13C
14C
a. The element is: __________________
b. The number 6 refers to the _________________________
c. The numbers 12, 13, and 14 refer to the ________________________
d. How many protons and neutrons are in the first isotope? _________________
e. How many protons and neutrons are in the second isotope? _________________
f.
How many protons and neutrons are in the third isotope? _________________
20. Complete the following chart:
Isotope name
atomic #
mass #
# of protons
# of neutrons
# of electrons
Potassium-37
Oxygen-17
uranium-235
uranium-238
boron-10
boron-11
DIRECTIONS: For the following problems, show your work! Be thorough.
21. Naturally occurring europium (Eu) consists of two isotopes was a mass of 151 and 153. Europium-151 has
an abundance of 48.03% and Europium-153 has an abundance of 51.97%. What is the atomic mass of
europium?
22. Strontium consists of four isotopes with masses of 84 (abundance 0.50%), 86 (abundance of 9.9%), 87
(abundance of 7.0%), and 88 (abundance of 82.6%). Calculate the atomic mass of strontium.
46
47
48
23. Titanium has five common isotopes: Ti (8.0%), Ti (7.8%), Ti (73.4%),
49Ti (5.5%), 50Ti (5.3%). What is the average atomic mass of titanium?
17. Draw the electrons and the energy levels of the following elements
a. magnesium
b. silicon
18. Write formulas for each of the following ionic compounds.
a. Potassium fluoride
b. Calcium nitride
c. Aluminum chloride
.
.
.
19. Write the names for each of the following containing polyatomic ions.
a. CaCO3
.
b. NaOH
.
c. Mg(NO3)2
.
d. Al2(C2O4)3
.
20. Write the formulas for each of the following containing polyatomic ions.
a. potassium sulfate
.
b. cesium sulfite
.
c. potassium chromate
d. calcium hydroxide
.
21. Draw lewis dot structures for the following atoms:
a. potassium
b. silcon
c. bromine
22. Name these covalent compounds:
a. CBr4
.
b. PCl5
.
c. C3N4
.
d. NO
.
e. CCl4
.
f.
.
N2O5
23. Write the formulas for these covalent compounds:
a. Dinitrogen monoxide:
b. Sulfur trioxide:
c. Triphosphorus octafluoride:
.
.
.
24. Whoa! Now there all mixed up. For each one state the type of compound (ionic, covalent) and
write the name
c. AlCl3
d. CO
e. NaCl
f. Ba(NO3)2
g. SO3
h. PCl5
.
25. Periodic Trends: Use your periodic table to answer the questions below
a.
The largest 5th period metal.
b.
The fourth period metalloid with the largest atomic mass.
c.
The smallest of the Alkaline Earth Metals.
d.
The halogen in the fourth period.
e.
A third period inert gas.
f.
Lightest atom of all the elements.
g.
An atom whose oxidation number is 0 and is the second largest in its group.
h.
An element with the largest atoms in the first period.
i.
A second period element with a 2- oxidation number.
j.
Noble gas element whose atoms are the heaviest.
k.
The heaviest metalloid
l.
An element with 73 protons
m.
The transition element with the smallest atomic mass.
n.
The largest 4th period metal
o.
The nonmetal with an oxidation number of (3-) that has the greatest atomic mass.
p.
The nonmetal with an oxidation number of (1-) that has the smallest atomic mass.
q.
The synthetic element with the smallest atomic number.
r.
The least reactive third period element.
26. For each of the following determine whether the statement applies to metals, salts, both or neither.
i. _________________ They have high melting & boiling points.
j. _________________ They are arranged into crystals.
k. _________________ They conduct electricity as solids.
l. _________________ They have free moving electrons.
m. _________________ They are malleable and ductile.
n. _________________ They conduct electricity only when they are molten or dissolved in water.
o. _________________ Their bonds are formed between a cation and an anion.
p. _________________ They are generally solid at room temperature.
27. Fill in the table below comparing ionic, covalent and metallic bonding
Ionic Bonding
Types of elements that
bond (metals, nonmetals)
State (liquid, Solid, Gas)
at room temperature
How does it achieve an
octet (full outer shell (
Transfer electrons, share
electrons, sea of
electrons)
Conduct electricity
Melting Point (high/ Low)
Physical property
28. Finish Filling in the table below.
Covalent Bonding
Metallic Bonding
29. Describe the differences between a physical and chemical change.
30. Give an example of a physical change
31. Give an Example of a chemical change