Download CHEMISTRY MIDTERM REVIEW

Name____________________________________________ Date________________ Hour______
Chemistry Semester 1 Review
Unit 1: Introduction and Review
1. What is the proper procedure if you get a chemical in your eye?
2. Draw a picture of and describe how to use the following pieces of laboratory equipment:
a. Beaker
d. crucible tongs
b. Graduated cylinder
e. beaker tongs
c. Evaporating dish
f. test tube holders
3. Convert the following units:
10.64 mL
__________L
3200 m
__________mm
14.32 L
__________kL
418 µg
__________g
0.000435 km
__________mm
13.2 kg
0.543 mm
53 mL
0.312 cg
10.555 L
__________g
__________km
__________cL
__________kg
__________µL
4. How many significant figures are in each of the following measurements?
a. 4.09 cm____
b. 10.450 L____
c. 0.00028 g____
d. 10 m____
5. What are the SI units for the following: time, temperature, length, volume, mass?
6. Define precision and accuracy.
7. Which measurement is most precise? Why? 12.3 g or 12.336 g
8. In a lab a student finds the density of copper to be 9.32g/cm3. If the actual density of copper is
8.96 g/cm3, what is the percent error?
9. Differentiate between physical and chemical properties.
10. List five physical properties of water.
11. List two chemical properties of gasoline.
12. Differentiate between physical and chemical changes.
13. List five ways you could physically change a piece of paper.
14. What are the five indicators of chemical change?
15. List three indicators of chemical changes when a steak is cooking.
16. State the Law Conservation of Mass (Matter).
Unit 2: Periodic Table, Atomic Structure, and Nuclear Chemistry
17. Label this blank periodic table using the terms underneath it.
group and family numbers
period numbers
representative elements
transition elements
inner transition elements
metals
nonmetals
s-block
d-block
18. Define the following terms:
atomic number
mass number
isotope
ion
metalloids
alkali metals
alkaline earth metals
halogens
noble gases
lanthanide series
actinide series
p-block
f-block
19. Complete the following table:
Shorthand
Atom/Ion
Notation
Name
Atomic
#
Mass #
# p+
# no
# e-
8
8
82
10
56
2H
Carbon
Calcium ion
Sulfide
20
32
20. Silver has two isotopes: Ag-107 and Ag-108. Looking at the atomic mass of silver, which
isotope is more abundant? How do you know this?
21. Lead has four isoptopes. The percent abundances of the isotopes are: 1.37% 204Pb, 26.26%
206Pb, 20.82% 207Pb, and 51.55% 208Pb. What is the average atomic mass of lead?
22. Nitrogen-13 emits beta radiation and decays to Carbon-13 with a half-life of 10 min. Assuming
a starting mass of 2.00 grams of Nitrogen-13, how many grams will be present at the end of
three half-lives?
23. Write an equation for the alpha decay of Pa-231.
24. Write an equation for the beta decay of H-3.
25. Write an equation for the beta capture of Hf-180.
26. Why is mass not conserved in a nuclear reaction, yet it is in a chemical reaction?
Unit 3 – Electronic Structure and Periodicity
27. Define the following:
atomic orbital
energy level
sublevel
quantum
ionization energy
atomic radius
electronegativity
28. List all the types of electromagnetic radiation in increasing WAVELENGTH.
29. List the colors of visible light in decreasing ENERGY.
30. Draw the 1s, 2s, 2p, 3s, and 3p orbitals on the same set of axes.
31. What is the maximum number of electrons allowed in each orbital type (s, p, d, f)?
32. What is the maximum number of electrons allowed in each energy level (1-4)?
33. Describe all of the things that happens to an electron in a copper atom when it absorbs a
quantum of energy.
34. Write electron configurations (no noble gas configurations) for the following:
a. Au
b. Ca2+
35. Write noble gas configurations for the following:
a. W
b. Te236. What types of elements often have exceptional (i.e. they do not follow the rules for filling
atomic orbitals) configurations?
37. Ca2+ has the same electron configuration of which noble gas?
38. Place the elements P, Sc, Cl, Sr, Ba, and F in order of:
a. Increasing size
b. Increasing ionization energy
c. Decreasing electronegativity
39. Ca2+ has the same electron configuration as which noble gas?
Unit 4 - Bonding
40. What are valence electrons?
41. How many valence electrons for S? For Ca? For S2-? For Ca2+?
42. How many electrons does nitrogen gain in order to achieve a noble gas electron configuration?
43. How do you know how many valence electrons are in any representative element?
44. Show the ionic bonding between calcium and iodine.
45. How many total electrons are transferred from calcium to iodine when forming the compound
above?
46. Which of the following pairs of elements is most likely to form an ionic compound? a)
magnesium and fluorine, b) sodium and aluminum, c) bromine and nitrogen, and d) chlorine
and lithium
47. What is the octet rule?
48. Draw the Lewis dot structures for the following: CH4, PF3, C2H2, O3, I3-,NO349. Write the shape of each molecule in the previous question next to its Lewis dot structure.
50. Why do atoms share electrons in covalent bonds?
51. How many lone pairs of electrons are there in the NH3 molecule?
Unit 5: Chemical Names and Formulas (Nomenclature)
52. List five properties of ionic compounds.
53. What are the chemical characteristics of covalent compounds?
54. Fill in the following table.
Ionic, Molecular,
Acid, or Base?
Name
Formula
dinitrogen hexabromide
ammonium carbonate
potassium phosphide
mercury (II) acetate
sulfuric acid
copper (II) sulfate
iron (III) dichromate
calcium hydroxide
carbon tetrachloride
aluminum sulfide
SrO
Cl2O
AgC2H3O2
NiF2
H2CO3
Ba3(PO4)2
As2S5
Mg(OH)2
HNO3
Dimensional Analysis
55. The tires on a car are to be inflated to a pressure of 2251 g/cm2. Convert this to lbs/in2
(1kg=2.2lbs) (1in=2.54cm).
56. It took 32,409 kilograms of steel to make the Mackinac Bridge. If the price of steel today is
$2.17 per pound, how much would it cost to purchase the steel in today’s market? (1kg=2.2lbs)