Chemistry Honors Fall Final Exam Study Guide for Multiple Choice Portion
1. You need to be able to read articles and answer questions about the information in the
article
A. What is a byproduct we produce by using nuclear materials? Nuclear waste
B. How long does it take the most dangerous byproduct to decay to half of its potency?
25,000 years
C. List 5 dangers associated with plutonium waste?
1) Cancer
2) Genetic damage
3) death
5) can be used to create nuclear weapons
4) radiation sickness
D. Describe how the military is contributing to the problem of nuclear waste.
Arms reduction by the military is creating waste
E. How is waste stored from power plants?
Water filled basins and dry casks
F.
How is military nuclear waste currently stored and what is the danger this poses?
Dry casks – plutonium
dust
2. a. Would you expect the density of air at a temperature of 450 oF to be 0.0440, 0.200, 0.0432,
or 0.0150? 0.0440
b. In general, what is the trend for the density of air as temperature increases?
The density decrease as the temperature increases
c. Which is the independent variable and which is the dependent variable?
Independent: temperature (the variable that you would change in an experiment)
Dependent: air density (changes as a result of you chaning the independent var.)
d. In general are the two variable directly related or indirectly related? Explain.
Indirectly related because as one variable increases the other decreases.
3. Place the contributors to atomic theory in chronological order and explain what contributions
they made (Aristotle, Democrites, etc.)
a. Aristotle/Copernicus: believed in 4 elements (fire, water, wind, earth) & not
atoms
b. Democritus: proposed that matter is made up of atoms
c. Dalton: Atomic theory
d. Thomson: discovered the electron
e. Rutherford: discovered the proton and that they are in a nucleus
4. Which one of these guys came up with the plum pudding model? Thomson
5. Which one of these guys used the Cathode Ray tube as an experiment? Thomson
6. Which one of these guys used the gold foil experiment? Rutherford
7. Differentiate between the properties of solids, liquids, and
gases and draw a simple particle diagram for each.
Gases – no definite volume or shape
Liquids – no definite shape but definite volume
Solids – definite shape and volume
8. Define the following:
a. atom smallest particle of an element that keeps its properties
b. ion atom of bonded group of atoms that has a charge
c. isotope atoms of the same element with a different number of neutrons
9. What is the group and period that [Ar] 4s23d104p2 is found in? Group: IVA Period: 4
10. How many valence electrons are in number 9? 4
11. Is number 9 a metal, non metal, or metalloid? metalloid
12. What is the abbreviated configuration for Scandium? [Ar] 4s2 3d1
13. What is a valence electron? The electrons in an atom’s outer most orbitals and it
determines the chemical property of the element.
14. Write out the electron configuration for Zr. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d2
15.
Element
# of Valence e-
Label as either:
- reactive
- unreactive
Oxidation State
Alkali metals
reactive
+1
Any group 1A
1
Alkaline earth
metals
Halogens
reactive
+2
Any group 2A
2
reactive
-1
Any group 7A
7
Noble gases
unreactive
0
Any group 8A
8
Give an example of
an element found
here
16. What block contains the most reactive elements: s
p
d
f
17. Write the formulas for the following:
a. beryllium chloride BeCl2
c. carbon trisulfide CS3
b. copper(II) phosphate Cu3(PO4)2
d. trinitrongen tetraoxide N3O4
18. If you had a mixture of sugar, water, and sand, how would you separate the materials from
each other? Describe the equipment you would need.
I would filter out the sand with a sieve and then evaporate the water to leave the
sugar
19. Determine the subatomic particles for the following atoms, ions, and isotopes:
Element
Protons
Neutrons
Electrons
12
12
12
Mg
2+
38
50
36
Sr
30 −3
15
15
18
𝑃
15
20. List the valence electrons that each of the following has
Transition metals 2
Group 3A 3
Group 4A 4
Type of particle
Atom
Ion
Ion
Group 5A 5
21. What form of energy is light? electromagnetic
22. During a fireworks explosion, light is released. Is the light released when the electrons are
going from ground state to the excited state or from excited state to the ground state?
23. Draw a Lewis dot structure for the following elements:
Ca
Calcium
N
Nitrogen
O-2
O
24. What is the definition for temperature? A measure of the average kinetic energy of the
particles of a substance
25. What general form of energy is this: Kinetic
or
Potential
26. Define the Law of conservation of matter.
Matter is neither created or destroyed, it is just transferred
27. How is a balanced equation a verification of the law of conservation of matter?
It shows that there are equal number of atoms of all elements on the reactant & product
side of the chemical reaction
28. Balance and classify equations as either synthesis, decomposition, single replacement,
double replacement, combustion, or acid-base.
Cl2 2NaCl
a.
2Na +
b.
H2SO4 +
c.
3Sr +
d.
Ca3(PO4)2 + 6LiCl
e.
CH4 +
2NaOH
2Cu(NO3)3 
2O2 -> CO2 +
synthesis
Na2SO4 +
2Cu +
2H2O
3Sr(NO3)2
acid/base
single replacement
 2Li3PO4 + 3CaCl2 double replacement
2H2O
combustion
29. Predict the products formed in each of the following
a. 2Li + Mg(NO2)2 2LiNO2 + Mg
b. 3HCl + Al(OH)3 3H20 + AlCl3
c. Strontium + chlorine gas SrCl2
d. Copper (I) sulfide + calcium chlorate  2CuClO3 + CaS
30. Define the following:
a. Atomic Size distance from the center of the nucleus to the outermost electron
b. Ionic Size distance from the center of the nucleus to the outermost electron
c. Ionization Energy energy needed to remove the outermost electron
d. Electronegativity ability of a nucleus to attract and electron
e. Electron Affinity energy change that occurs when an atom gains an electron
31. Place the following in smallest to largest radius: Ca2+, S2-, Ar, S1Ca2+, Ar, S-1, S-2
32. Place the following in lowest to highest ionization energy: Na, S, Cl
Na, S, Cl (lowest to highest IE would be the largest atom to the smallest atom
because ionization energy increases with decreased size due to the nucleus having a
better attraction for the valence electrons).
33. Based on your answer to #32, which of the elements has the greatest tendency to lose
electrons in bonding? Is this element a metal or nonmetal?
Na (lowest ionization energy) and it is a metal
Ionization
Energies of
metals vs
nonmetals
Electronegativities of
metals vs
nonmetals
Electron
Affinities of
metals vs
nonmetals
Metals
High
High
High
Low
Low
Low
Nonmetals
34. Answer the following:
List physical properties
High
High
High
Low
Low
Low
Except Noble
Gases
35. The strongest forces of attraction occur between the atoms of which two elements: O-F, OBr, O-Cl, O-I? (Hint: Use the ideas of electronegativity to think about the answer to this
question).
Since F is the most electronegative element it has the strongest ability to attract
electrons to itself. Therefore it has the “strongest forces of attraction”. Answer: O-F
36. Based on your answer to #35, which has a higher boiling point? O-F
37. Consider the orbital diagram to the right. What atom is it
representing? Boron (since it has 5 electrons)
38. What is the density of an object (in g/L) that has a mass of 8.4 g and a volume of 34 cm 3?
𝒎
𝟖.𝟒𝒈
34 cm3 = 34 mL = 0.034 L
D = 𝑽 = 𝟎.𝟎𝟑𝟒𝑳 = 247 g = 250 g (with 2 sf)
39. Categorize the following elements from the periodic table: Na, Se, P, Cu, Fr, U, Be, O, Ar
Tend to gain electrons: Se, P, O, Ar (negative ions)
Tend to lose electrons: Na, Cu, Fr, U, Be (positive ions)
40. Refer to question #39, what do the elements that gain electrons have in common based off
where they are on the periodic table?
Nonmetals tend to gain electrons and metals tend to lose electrons.
41. When aluminum metal reacts with fluorine gas, give the formula for the resulting compound.
AlF3
42. Based on your answer to #41, what is the ratio of aluminum to fluorine?
1 Al : 3 F
43. Would this ratio work for all elements in group 3A and 7A? Yes / No
44. Identify the types of energy at each point in the following images:
a)
b)
chemical
chemical
thermal
thermal
electromagnetic
electromagnetic
45. Discuss the following scientists contributions to the Periodic Table development:
Mendeleev, Moseley, and Newlands
Newlands – arrange elements by increasing atomic mass, properties repeat ever 8 – law
of octaves
Mendeleev-arrange elements by inc. atomic mass, formed 1st periodic table
Moseley-discovered atomic number & arranged elements this way
Einstein-