Honors Chemistry
Name: ______________________________________ Date: ________________ Mods: ____________
Honors Chemistry Midterm: Review Packet
1. Write in the number of significant figures for each of the following measurements:
____
3.00 mL
___
0.00290 g
___
50.00 m
___
0.070 kg
___
400 L
2. Using the following masses: 0.0562 kg, 124.213 g and 1635 mg.
The answer should be reported as: ______________ g
3. a) A 5.75 mL sample of mercury has a measured mass of 77.05 g. The density is ___________.
b) Mercury’s accepted density is 13.53 g/mL. The % error in your measurement is: __________.
4. In the diagram below:
Is this person accurate? ___________
Is this person precise? ___________
5. Identify the following as a chemical change (CC), physical change (PC), chemical property (CP),
or physical property (PP):
a) burning wood __________
b) mass of wood _________
c) flammability of wood _________
d) chopping up wood __________
6. A calculator displays the answer to a problem as 53.09010
Report this answer to:
_______________________ 5 significant figures
_______________________ 3 significant figures
_______________________ 1 significant figure
7. a) What is an isotope?
b) Calculate the average atomic mass of silicon. The three silicon isotopes have atomic masses
and relative abundances of 27.9769 amu (92.2297%), 28.9765 amu (4.6832%) and 29.9738
amu (3.0872%).
8. a) Who is the scientist responsible for the discovery of the electron?
b) What was the experiment that led to this discovery?
9. Write the formulas for the following ionic and molecular compounds:
Name
tin (IV) chloride
Tetracarbon diphosphide
aluminum hydroxide
ammonium sulfate
nitrogen tribromide
calcium phosphate
Formula
10. Write the names of the following ionic and molecular compounds
Name
Formula
Pb3(PO4)2
KMnO4
O2F5
ZnSO4
MgO
PSe2
11. a) The molar mass of Ba(NO3)2 is ________________________________.
b) Calculate the percent composition of each element in Ba(NO3)2
Ba = ____________%
N = ___________%
O = ___________ %
12. How many particles of CO2 (MM = 44.0 g/mol) are in 17.75 grams of CO2?
13. List the seven diatomic molecules. (The ones that always come in pairs)
14. Balance the following chemical equations and classify their type (single replacement, double
replacement, etc.)
a) _____C5H12 + _____O2  _____CO2 + _____H2O
Classify this reaction: ______________________________________________________
b) _____H2O2  _____H2O + ______O2
Classify this reaction: ______________________________________________________
c) _____AgNO3 + _____K2CO3  _____Ag2CO3 + _____KNO3
Classify this reaction: ______________________________________________________
15. Consider the balanced equation: N2(g) + 3 H2(g)  2 NH3(g)
molar masses (g/mol):
(28.0)
(2.0)
(17.0)
a) What is the greatest mass of ammonia, NH3 (g), that will be formed when 12.80 grams of
H2(g) reacts with 55.25 grams of N2(g)? (Hint: this is a limiting reactant problem)
b) If this reaction was completed in the lab and it was determined that the quantity of ammonia
gas produced was 63.4 grams, what is the % yield of the ammonia?
16. A substance is 33.33% carbon, 7.47% hydrogen, and 59.20% oxygen.
a) What is its empirical formula?
b) If the molar mass of the compound is 216 g/mol, what is its molecular formula?
17. In the following, circle the precipitates:
PbI2
Ba(OH)2
Ag2CO3
CaF2
K2SO3
(NH4)2S
18. Write the balanced molecular, complete ionic, and net ionic equation for the following:
a)
Solutions of magnesium chloride and lead (II) acetate are mixed.
b)
Solutions of silver nitrate and sodium carbonate are mixed.
19. Write the balanced molecular equations.
a) ______Co(C2H3O2)2 (aq) + ______Ag (s) _______________________________________
b) ______Na (s) + ______AlCl3(aq) ______________________________________________
c) ______H2SO4(aq) + ______Ca (s) _____________________________________________
d) ______Br2(s) + ______CuI2(aq) ______________________________________________
20. Fill in the blanks:
a. The symbol for wavelength is ________ and it is measured in ________ or ________.
b. The symbol for frequency is ________ and it is measured in ________ = ________.
c. The speed of light, c, is a constant value of __________________________________.
d. Planck’s constant, h, is a constant value of __________________________________.
e. The equation relating wavelength and frequency is: ___________________________.
f.
The equation relating energy and frequency is: _______________________________.
g. 1 nm = __________________________ m
21. Rank the following in order from lowest (1) to highest (7)energy:
gamma rays, visible light, microwaves, ultraviolet radiation, x-rays, radio waves, infrared radiation
1) ___________________________________ 2) _____________________________________
3) ___________________________________ 4) _____________________________________
5) ___________________________________ 6) _____________________________________
7) ___________________________________
22. A certain photon of light has a frequency of 4.59 x 1014 Hz. Calculate the wavelength, in
nanometers, of the light.
23. A wave of blue light has a wavelength of 422 nm. What is the energy, in J, of that wave?
24. Scientists and Energy:
Matching – match the letter of the scientist to the work that he contributed to the world
a) Heisenberg
b) Louis de Broglie
c) Niels Bohr
d) Rydberg
_________ responsible for the uncertainty principle which states that it is impossible to know
(with any great degree of certainty) both the location and velocity of an electron)
_________ responsible for the planetary model of the atom, where electrons traveled in
distinct paths around the nucleus
_________ responsible for the equation which determines the exact amount of energy
needed for electron promotion or demotion between energy levels
_________ responsible for the idea that if light can behave as particles of matter, matter
should also be able to exhibit wave properties.
25. Identify the elements with the following electron configurations:
a. ___________________________ 1s22s22p63s23p64s23d104p6
b. ___________________________ [Ar] 4s23d10
c. ___________________________ [Ne] 3s2 3p4
d. ___________________________ 1s22s22p63s23p64s23d104p65s24d2
26. Which six elements are exceptions because they have unusual/irregular electron configurations?
27. Write the condensed (noble gas) electron configuration for the following elements:
a. Tin
_________________________________________________________
b. Osmium
_________________________________________________________
c. Chromium
_________________________________________________________
28. Periodic Trends:
Matching – match the letter of the trend that is best described by the statements below
a) atomic radius
b) ionization energy
c) electronegativity
d) electron affinity
_________ the energy required to remove an electron from an atom or ion
_________ the energy change associated with an atom or ion gaining and electron
_________ the relative size of an atom
_________ the ability of an atom to attract electrons to itself
29. Complete the diagram to the
right by writing increase or
decrease along the period and
group arrows for each of the
periodic trend.(AR = atomic
radius, EN = electronegativity,
IE = ionization energy)
30. Use the following elements to
answer the questions below
(Note: an element can be used more than once):
Tellurium, Chlorine, Selenium
a.
b.
c.
d.
____________________________ has the lowest 1st ionization energy
____________________________ has the highest 1st ionization energy
____________________________ is the largest atom
____________________________ has the highest electronegativity
31. Use the following elements to answer the questions below (Note: an element can be used more
than once):
Aluminum, Beryllium, Nitrogen
a.
b.
c.
d.
____________________________ has the lowest 1st ionization energy
____________________________ is the smallest atom
____________________________ has the highest electronegativity
____________________________ has the lowest electronegativity
32. Circle the answer which makes the statements below true:
a. The strength of a covalent bond (increases/decreases) with increasing bond order. Therefore
(single/double/triple) bonds are the strongest.
b. The length of a covalent bond (increases/decreases) with increasing bond order. Therefore
(single/double/triple) bonds are the longest and (single/double/triple) bonds are the shortest.
33. Determine the number of valence electrons (VE) available and draw Lewis structures for the
following molecules:
a. SO3
VE = ____________
b. ClO3–
VE = ____________
c. CH2O
VE = ____________
d. BrF3
VE = ____________
34. For each of the following molecules below, give the (1) the molecular geometry geometry/shape
(2) state if it is a polar or nonpolar molecule
Questions #1 – 3
Molecule
a.
1)
2)
b.
1)
2)
c.
1)
2)