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Chemistry
Huffman
Name:
Date:
Final Exam Review
Directions: Answer the following questions below. Show all work for full credit, label all units, put all calculation
answers in correct scientific notation (when needed) and significant figures and BOX all answers.
1.
What is the chemical symbol for: a. Gold ___ b. Tin____ c. Potassium ____ d. Radon ____
2.
What is the difference between atomic mass, mass number and atomic number.
3. For the elements whose outermost electron configurations are given below, tell the period and group
to which each belongs:
Symbol Name
Period
Group
a. 6s1
b. 5s25p4
c. 3s23p2
4. Write the electron configurations for the outermost energy level for each of the following:
a. Ar ____________
b. Ca ____________
c. Cl ____________
5. Arrange the following elements in order of decreasing ionization energy (highest  lowest).
a. Ca, Ba, Be, Sr ___________________________
b. Cl, Si, P, Ar ___________________________
c. Cs, Li, K ___________________________
6. Tell whether each of the following elements is an inner transition metal, noble gas, alkali metal,
alkaline earth metal, halogen, or transition metal.
a. K ___________________________
b. Cl ___________________________
c. Gd ___________________________
d. Co ___________________________
e. Mg ___________________________
f. Ar ___________________________
7. Circle the element of the following pairs that has the higher electronegativity:
a. Na, Mg
b. Rb, I
c. Cl, Br
8. Which of the following has the larger atomic radius?
a. Cl, Clb. Mg, Mg2+
Chapter 4:
1. Describe everything you know about the structure of an atom. (Draw Lithium here as an example:)
2.
What overall charge does the nucleus of the atom have? Why?
3.
What is the relative mass in grams for: a. electron__________
neutron__________
4.
An atom is identified as Uranium-235.
a. What does the number 235 tell you about uranium? _______________________________
b. Write the symbol for this atom using subscripts to show the mass number and atomic number.
____________
5.
Complete the following table:
Element
Atomic
Number
Element
Atomic Mass
Mass Number
48
b. proton__________
Number of
Protons
c.
Number of
Neutrons
Number of
Electrons
66
198
Tin
80
72
6.
Name an isotope of carbon-12: ____________________. Then draw a Double Bubble Map comparing the
similarities and differences between the two isotopes.
7.
What is the difference between mass number and atomic mass?
8.
How do atomic masses vary throughout the periodic table?
9. What force holds the atom together (ie. what force causes electrons to be attracted to the nucleus?
Chapter 5: Electrons in Atoms
1. Write the complete electron configuration for the following elements: (Follow the
orbital filling order!)
a. Ca
__________________________________________________________
b. Ni
__________________________________________________________
c. Rb
__________________________________________________________
d. Ag
__________________________________________________________
e. P
__________________________________________________________
Chapter 6: Periodic Trends
Do you remember how the periodic table is arranged?
 (Example: Noble gases – Elements with the outermost s and P sublevels are filled.)
 Transition metals –
 Inner transition metals –
 Representative elements –
 Alkali metals
 Alkaline earth metals
 Halogens
 Groups
 Periods
Can you define the following trends . . .do you know the trends in the periodic table. . . and can
you explain why these trends occur?? (Use arrows and color code these!)






Atomic Size
Ionization Energy
Ionic Size
Electronegativity
Shielding
Nuclear Charge
Chapter 7:
Element
Group #
# of Valence Electrons
Lewis Electron Dot Structure
1. Mg
Element
Number of electrons
gained or lost to fulfill
octet rule
Gained
2. Br
Resembles
which noble
gas?
Lost
Diagram of electron dot structure before
and after ionization.
(Include charge after ionization)
Before
After
(circle one)
# _______
Show the formation of the following compound:
* Draw the electron dot structure for each atom.
* Draw arrows showing the transfer of electrons.
* Write the charges on all ion products.
* Write the formula and name for the new compound formed.
Diagram
3. Magnesium and Fluorine
Formula:
Chapter 8:
Molecule
1.
Name:
# of Valence
Electrons?
Molecular Structure (w Eneg Numbers
from chart on page 177 and arrows.)
Polar or Nonpolar?
O2
Shape?
Molecule
# of Valence
Electrons
Molecular Structure (w Eneg Numbers
from chart on page 177 and arrows.)
2. NH3
Molecule
3.
Shape?
# of Valence
Electrons
Molecular Structure (w Eneg Numbers
from chart on page 177 and arrows.)
HCN
Chapter 9:
1.
Polar or Nonpolar?
Polar or Nonpolar?
Shape?
Polyatomic ions, Polyatomic ions, Polyatomic ions !!!!
What is difference between a cation and an anion.
How is each formed?
2.
Which groups of elements on the periodic table are cations and which group of elements are anions? Note the charges of
each group on the chart below. Draw in the line separating the metals from the nonmetals.
3.
Complete the following table. Write the chemical name and the chemical formula for the compounds formed.
Ca
Na
Mn3+
N
I
Se
Sn4+
Mg
Ga
PO33-
C2O42-
CN4.
5.
Complete this table:
Symbol of Element
Change in Electrons
S
Gain / lose _____ e-
Al
Gain / lose _____ e-
Formula of Ion
Identify the compound type: ionic (I), molecular (M), or acid (A). Then name the compound.
a.
CaCO3
______
______________________________________________
b.
PBr5
______
______________________________________________
c.
HNO2
______
______________________________________________
d.
Cl2
______
______________________________________________
e.
Fe2S3
______
______________________________________________
Name of Ion
6.
f.
HCN
______
______________________________________________
g.
C2F6
______
______________________________________________
Give the chemical formula for the following:
a.
Sulfuric acid
f.
Phosphorus heptachloride
b.
Dinitrogen tetroxide
g.
Hydrosulfuric acid
c.
Copper (II) nitride
h.
Calcium oxalate
d.
Boron trichloride
i.
Potassium oxide
e.
Hydrohydroxic acid
j.
Titanium (IV) sulfide
Chapter 11: Answer all questions in space provided.
1.
Predict the products and balance the following chemical reactions. Write the type of reaction and then give the chemical
name of the products.
a.
_____ Be(OH)2
+ _____ H3PO4  ______________________________________________
Type of reaction: __________________________
b.
_____ Li + _____ H2O  ________________________________________
Type of reaction: __________________________
c.
Hint: write water as HOH
A piece of aluminum foil is placed into a solution of copper chloride (Copper has a charge of +2).
___________________________________________________________________________
Type of reaction: __________________________
d.
_____ Zn + _____ AgNO3
 _____________________________________________________
Type of reaction: __________________________
e.
_____ Ca + ______ S  _____________________________________________________
Type of reaction: __________________________
f.
_____ Ag2SO4 + _____ AlCl3
 _______________________________________________
Type of reaction: __________________________
2.
Explain what determines if one single metal may or may not replace another metal from a compound in a single
replacement reaction.
3.
Define and explain the law of conservation of mass. Prove the law using this equation: N2 + 3 H2  2 NH3
4.
A student prepares hydrogen bromide by reacting sodium bromide with phosphoric acid.
a. Write a balanced chemical equation for this reaction.
b. What type of reaction is this? _________________________________
Chapter 12
1.
If you start with ten grams of lithium hydroxide, how many grams of lithium bromide will be produced?
LiOH + HBr  LiBr + H2O
2.
If you start with 45 grams of ethylene (C2H4), how many grams of carbon dioxide will be produced?
C2H4 + O2  CO2 + H2O
3.
If you start with 5.5 grams of sodium fluoride, how many grams of magnesium fluoride will be produced?
Mg + NaF  MgF2 + Na
4.
If you start with 20 grams of hydrochloric acid, how many grams of sulfuric acid will be produced?
HCl + Na2SO4  NaCl + H2SO4
Chapter 16
1.
How many moles of sodium hydroxide would be needed to make 1 liter of 2M solution?
2.
How many moles of sodium hydroxide would be needed to make 1.2 liters of 3M solution?
3.
How many grams of sodium hydroxide would be needed to make 1 liter of 2M soln?
4.
How many grams of sodium hydroxide would be needed to make 9.75 L of 4.5M solution?
5.
What would be the Molarity of a NaOH solution where 655.0 g NaOH are used to make a total of 4.7 L of solution?
6.
What would be the Molarity of a MgCl2 solution where 207 g MgCl2 are used to make a total of 950 mL of solution?
Chapter 17
Convert: Show work using DA!
1. 1.69 Joules = _____ cal
2. 68 cal = _____ kcal
3. 0.3587 J = _____ cal
Calculate the temperature change:
4. 20.0 g of water is heated from 16.8 °C to 39.2 °C.
5. 35.0 g of water is cooled from 56.5 °C to 5.9 °C.
6. If 400 cal raises 14.67 g of a substance from 20°C to 87°C, what is the specific heat
capacity of the substance?
7. When 435 J of heat energy is added to 3.4 g olive oil at 21oC, the temperature
increases to 85oC. What is the specific heat of the oil?
8. Al + O2
Al2O3
Hrxn = 400 kcal/mol
exothermic/endothermic
_______________________________________________________________________
9.
CH4 + O2
CO2 + H2O
Hrxn = -890 kJ/mol
exothermic/endothermic
_______________________________________________________________________
10. Find the heat required to change 14.2 g ice at -2.0oC to steam at 215.6OC. What segments on a phase
change graph (letters A, B, C, D, or E) are represented in this problem?