PreAP Final Exam review
Chapters/ Topics for Day 2 Final
Electron configuration
Periodic table trends
Moles
EM spectrum
Bonding
Nomenclature
1. How many electrons occupy the following energy levels:
a. n=1
b. n=2
c. n=3
d. n=4
2. Electrons are located in __________________ surrounding the nucleus.
3. Write the Electron Configuration, Noble Gas Notation, and Orbital
Notation for:
a. Mg
b. Br
c. Ni
4. Define/understand: Pauli’s Exclusion principle, Hund’s Rule, and the
Aufbau principle
5. What is the relationship between wavelength/frequency/energy?
Which ones are directly related, which ones are indirectly related?
6. Which types of waves & colors of the visible light spectrum have the
highest & lowest: energy, frequency, wavelength
7. What are the units for energy, frequency, and wavelength?
8. Calculate the following:
a. If you have a frequency of 3.55 x 1017 Hz determine the energy.
b. If you have a wavelength of 5.0 x 10-7 m, what is the frequency?
9. Define and identify the Periodic Trends: Ionization Energy,
Electronegativity, Ionic Radius, Atomic Radius
10. Which element has the highest Electronegativity?
11. Which element has the biggest Atomic Radius?
12. Define: ionic bond, covalent bond (molecular compound), and
metallic bond.
12. Fill out the table:
Symbol/Formula compound/
Element
Ionic,
covalent,
or metallic
transfer of esharing of esea of e-
Cu
H2O
NaCl
MgSO4
C6H12O6
13. Define Lewis structure. What is used to draw them.
14. Draw a Lewis structure showing the bonds for: HBr, CCl4, H2O
15. Show how the following ions combine. Show the transfer of
electrons along with the appropriate charges. Draw the final formula.
a. Mg and Cl
b. K and N
c. Al and O
16. When drawing Lewis structures (dot diagrams) how many does
every element need? What is the exception and how many does is
need?
17. How many valence electrons do groups number 1,2, 13, 14, 15, 16,
17, 18 have? What is group 18 called and why are they special?
18. What is the oxidation numbers (charges for each of the above
groups in #17?
19. Name the following compounds:
a. CuCl2
b. NaCl
c. FeBr3
d. H2O
e. (NH4)2CO3
f. N2Cl
g. Fe(OH)2
h. CCl4
i. Ca(C2H3O2)2
j. Na2SO4
20. Write the formulas for the following:
a. iron (II) nitrate
b. aluminum oxide
c. potassium iodide
d. sodium nitrate
e. copper (I) nitrate
f. iron (III) oxide
g. iron (III) hydroxide
h. carbon monoxide
i. zinc nitrate
j. dihydrogen pentasulfide
k. lead (II) sulfate
l. potassium chromate
21. Find the molar masses of the following:
a.
b.
c.
Ca(OH)2
Na3PO4
(NH4)2CO3
22. Calculate the following:
a. How many moles are in 25.0 grams of water, H2O?
b. How many grams are in 4.50 moles of Lithium Oxide, Li2O?
c. How many molecules are in 23.0 moles of oxygen, O2?
d. How many molecules are in 25.0 grams of ammonia, NH3?
e. How many atoms of Oxygen are in 60 g of baking soda (NaHCO3)?
Remember baking soda is a formula unit!!! This is a three step problem!