Name _______________________________ Date ______________ Period ______
Study Guide
12) Titanium has five common isotopes: 46Ti (8.0%), 47Ti (7.8%), 48Ti (73.4%), 49Ti (5.5%), 50Ti (5.3%). What
is the average atomic mass of titanium?
1)Determine the number of significant digits in
900 - _______
9004 - ________
0.005016 - ________
13) The half-life for Fm-255 is 20.1 hours. How long will it take for a 32.0g sample to decay until only
2.00g remains?
8.0400 - _______
2) Calculate the following measurements and round off using the correct number of significant digits.
3.4 cm x 10.9 cm x 0.92 cm = __________
(103.45 g – 99.7 g)  7.43 mL = ___________
3) Identify the following as an element, compound, hetero or homo mixture
a. Iron
b. steel
c. water
d. sugar
e. air
f. has atoms
g. has identifiable parts
h. contains molecules
i. kool-aid
j. must combine atoms chemically
4) Which boxes contain:
- one element
- a compound
5) Identify the following as chemical or physical changes.
a. melting ice
b. burning rubber
d. dissolving sugar
e. boiling salt water
14) Three grams of Bismuth-218 decay to 0.375 grams in one hour. What is the half-life of this isotope?
15) Actinium-226 has a half-life of 29 hours. If 100 mg of actinium-226 disintegrates over a period of 58
hours, how many mg of actinium-226 will remain?
16) Fill in the following nuclear decay equations:
59 Co 4 He + ___________
27
2
214 Pb 0  + ___________
82
-1
238 U 234 Th
92
90
234 Th234 Pa +
90
91
+ _____
______ + γ
- a mixture
c. exploding fireworks
6) Give an example of a chemical and physical change that can occur to the following:
Paper
Salt
Metal
7) Identify the four indicators of a chemical reaction.________________, ________________,
________________, ________________.
8) Which of the following statements are true about subatomic particles? Can be more than one!!
a) Protons and electrons can be found in the nucleus.
b) Electrons are found in orbitals around the nucleus
c) Neutrons are positively charged particles
d) Protons and electrons weigh the same
e) Isotopes of an element have different numbers of neutrons
f) Ions of an element have different numbers of protons
9) Determine the number of protons, neutrons and electrons in
A. Silicon – 29
p = ____ n = _____ e = ____
B. 24 Na p = ____ n = _____ e = ____
C. 35Cl
p = ____ n = _____ e = ____
D. 36 Cl-2 p = ____ n = _____ e = ____
10) Consider the following % Abundances for these isotopes of Oxygen. Then calculate the average
atomic mass for the sample:
Oxygen-15 (13.5%)
Oxygen-16 (83.9%)
Oxygen-18 (2.6%)
11) There are two isotopes of O: O-15 and O-16. Using Oxygen’s average atomic mass from the periodic
table, explain which isotope is the most abundant and how you know.
17) Which section of the EM spectrum has the:
Lowest energy?
Shortest Wavelength?
Smallest Frequency?
18) What wavelength of energy is released when an electron moves from:
a. 6 to 1
b. 5 to 3
c. 4 to 1
d. 4 to 2
19) What are the periodic table trends for:
Ionization Energy
Activity or Reactivity
Atomic Radius
Electronegativity
20) This picture could represent which of the following?
a. Iron
b. Potassium
c. Silver d. Carbon e. Argon
f. Barium
21) Write the orbital notation for
a. Li
b. Si
c. Na
22) Determine the element represented below
a. 1s22s22p63s23p64s23d6
b. 1s22s22p4
d. [Rn]7s2
e. [Xe] 6s24f145d7
d. F
c. [Kr]5s24d3
32) Write the formulas for the substances:
a. magnesium carbonate
b. iron (II) hydroxide
d. silver nitride
e. lean (III) chloride
c. silicon disulfide
f.heptanitrogen trichloride
33) Name the following substances
a. N2O
d. Mn(C2H3O2)2
c. K2SO4
f. FeO2
b. SiF4
e. C4F5
34) Determine the molar (formula) mass of
a.Al(C2H3O2)3
b. Cr(OH)3
c. MnF
35) Convert 915 g of SiBr4 to molecules.
36) How many moles in 8.2 x 10 21 atoms of Xe?
23) Draw the electron dot structures for the following elements:
a. Rb
b. Ba
c.Cl
d.As
e. B
f. Cr
37) How many grams are in 3.9 x 1025 atoms of Ba?
24) Which element is in Group 3& Period 6 of the periodic table?
38) Determine the number of moles in 250 g of CO2.
25) Which element in Group 16 has the least tendency to gain electrons?
39) Calculate the % composition of O in the following
a. P2O5
b. MgSO4
26) Within each of the following groups, state which has the largest ionization energy:
a. Mg and Be
b. As and Se
c. Fr and Ba
d.Cl and Ar
27) Within each of the following groups, state which has the greatest electronegativity:
a. Na and Mg
b. C and Si
c. Ge and P
d.Cl and Ar
28) Rank the following from least to most reactive:
a. Ba, Fe, Y
b. S, Se, I
c. F, Cl, Br
d. Na, K, Rb
29) For each of the following compounds, determine if it is ionic or covalent and draw the dot diagram.
If it is covalent, identify the shape, overall polarity, and intermolecular forces present:
a.
NH3
b.
PF3
c.
KF
d.
CH4
e.
HF
f.
Li2O
g.
H2O
h. CO2
30) Fill out the following table:
Type of bond
Metallic
Ionic
Polar Covalent
Non-Polar Covalent
Does it dissolve?
Does it conduct electricity?
c. Fe3(PO4)2
40) What is the empirical formula for a compound which contains 0.0134 g of iron, 0.00769 g ofsulfur
and 0.0115 g of oxygen?
41) What’s the empirical formula of a molecule containing 65.5% carbon, 5.5% hydrogen, and 29.0%
oxygen?
42) What is the molecular formula of a compound that is 0.606 g of N and 1.29 g of O if the mass is 92g?
43) What is the molecular formula if the empirical is CH2 and the molecular molar mass is 70g?
List properties of the following:
Metals –
Nonmetals –
Endothermic Reactions –
Exothermic Reactions –
Define the following:
Ionization Energy –
Electronegativity –
Ionic Bond –
Covalent Bond –
Metallic Bond –
Polar –
Nonpolar –
Lewis Structure –
Valence Electron –
Isotope –
Ion –