Physical Science: Chemistry
Study Guide – Final Exam
Test consists of 68 multiple choice questions.
1. Understand the difference between CLAIM, EVIDENCE and REASONING and be able to identify them within
a scientific investigation.
2. Be able to read a short passage and identify the main idea and cite textual evidence.
Unit 1: States of Matter/Thermal Chemistry
Complete the following chart, listing the states of matter in order of least energy to most and stating
whether they have definite volume and/or a definite shape.
State of Matter
Volume
Shape
1.
What is the volume of the picture provided? _________
2.
What is the “meniscus” and where do you measure it from?
Below is a phase-change diagram of water.
1. Label the phase change diagram as the temperature is increasing and decreasing.
2. Explain what is happening during Leg B and Leg D.
3. Describe the intermolecular forces at Leg of the diagram.
4.Particles move as the states of matter change from low to high temperatures. Illustrate below the motion and spacing
of these particles in a melting ice cube. Describe the attractive forces between the particles in each state.
___________________
___________________
____________________
5.Heat (thermal energy) flows from objects/areas with a ____________________ temperature to objects/areas with a
______________________ temperature.
5. Give 3 examples of a good thermal conductor.
6. Give 3 examples of a good thermal insulator.
Unit 2: Atomic Theory/Periodic Table
7.
The building blocks of matter are________.
8.
What are the three subatomic particles, their charges and their locations in an atom?
9.
What are some uses for chlorine and fluorine?
10.
Define strong nuclear force.
11.
The atomic number of an element is the same as the ________. The number of neutrons + the number of
protons tells us the ________.
12.
Draw an example of a periodic table tile. Be sure to label the element name, chemical symbol, atomic
mass, mass number, and atomic number. Next, draw one to represent Fluorine.
13.
Define isotope and identify how many protons, neutrons, and electrons are in a Hydrogen-3
(Tritium) isotope?
14.
What are valence electrons? How can you figure out how many valence electrons an element has? Name
the diagram used to show the valence electrons of an element.
15.
Where are the number of each atom shown on chemical formulas?
16.
What is an oxidation number?
17.
What is the octet rule?
18.
Calcium has an atomic number of 20. How many filled energy levels does it have? How many electrons
are left over?
19.
Why are Noble Gases considered non-reactive?
20.
What do scientists call the place where electrons are found? ___________________________
21.
What state of matter are most metals at room temperature? ______________________________
22.
Identify where on the periodic table these families are found, their valence electrons and their oxidation
numbers:
Halogens: ______________________________________________________________________________
__________________________________________________________________________________ _____
Alkali metals: ___________________________________________________________________________
_______________________________________________________________________________________
Alkaline Earth Metals: ____________________________________________________________________
_______________________________________________________________________________________
Noble Gases: ________________________________________________________________________
__________________________________________________________________________________________
23.
As you move from left to right across the periodic table, what happens to the mass and size of the
elements?
24.
The ________ ________ of an element is the total number of protons and neutrons in the nucleus.
25.
Fill in the following chart.
Atomic Number
Protons
Neutrons
Mass
Electrons
Na
Cl-1
Li+1
26.
Elements with similar properties are listed in a single column on the periodic table called
______________.
27.
What are some characteristics of alkali metals? alkaline earth metals?
28.
Be able explain Ernest Rutherford's experiment and the discoveries from it.
29.
Where are nonmetals located on the periodic table? ___________________ Metals?
___________________
30.
Ionic bonds form between __________________________________
31.
Covalent bonds form between ________________________________
32.
In the formation of an ionic bond, the metal ________________ electrons and the nonmetal
____________ electrons.
33.
How do you figure out how many valence electrons an atom will have by looking at the periodic table?
34.
How many valence electrons does an atom need to be considered stable? _____
35.
What are the only 2 elements that don’t follow this rule? _____________. How many valence electrons
do they need? ____
36.
Using the Lewis Dot Diagram, draw the ionic bond between Potassium and Sulfur.
37.
How many atoms of each element are in 4H2O. Put a box around the coefficient and circle the subscript.
H= __________________________ O=_____________________________
Unit 3: Nomenclature,Formula Stoichiometry & Bonding
38. Complete the following table by writing the chemical formula of the compound formed by the two ions.
Br-
O2-
Ni3+
Ba+
Al3+
39. Complete the following table by writing the chemical formula and naming the compound formed.
Chlorine
Magnesium
Lithium
Nitrogen
Sulfur
Unit 4: Equations and Organic Chemistry
Oxygen
Balance the following equations:
42. __Ag2S ---> __Ag + __ S8
43. __KBr + __Fe(OH)3 ---> __KOH + __FeBr 3
44. __Pb(OH)4 + __Cu2O ---> __PbO2 + __Cu(OH)
45. __KOH + __ Co3(PO4)2 ---> __K3PO4 + __Co(OH)2
46. __KNO3 ---> __KNO2 + __O2
47. __BaF2 + __K3PO4 ---> __Ba3(PO4)2 + __KF
48. What is meant by “Atoms are conserved in chemical reactions” (Law of Conservation of Mass)?
49. Predict the products of the following reactions and identify what type of reaction it is. Circle the reactants in each
equation, highlight the products.
AgNO3 + Cu
2H2O
_______________ Type of reaction:
_______________ + ______________ Type of reaction:
50. Define physical property: _______________________________________________________________________
51. Define chemical property:
_______________________________________________________________________
Classify each of the following as being a physical (P) or chemical (C) property.
52. Blue color ____5
3. Density ____5
4. Flammability ____5 5. Melting point ____
56. Hardness ____5
7. Odor ____
8. Sour taste ____5
5
9. Reacts with acid to form H2 ____
60. Define physical change and give examples.
__________________________________________________________________________________________
61. Define chemical change and give examples.
__________________________________________________________________________________________
62. What is the result of a chemical change?
63. Compare/contrast endothermic and exothermic reactions in regards to heat energy.
64. Identify the following examples below as “endothermic” or “exothermic”.
_____________________ Instant cold pack
______________________ Meal, Ready to Eat (MRE)
Unit 5: Acids & Bases
65. Predict the product(s) of the following acid-base neutralization reaction.
HCl + NaOH ---> _______________ + _______________
66. What two products are formed from an acid/base reaction?
67. What is the pH scale and what does it measure?
68. List common tests used to indicate acids and bases.
69. List the formula and name for common acids and bases.
Chapter 22-Nuclear Reactions
70. Compare/contrast fission and fusion. (Include what happens inside the sun.)
71. Why does nuclear decay occur?
72. What is Carbon-14 used for?
73. Long term exposure to radiation is known to cause _______________.