Station 1 - The Periodic Table, Molecules and Molecular Compounds, and Ions and
Ionic Compounds
1. For each of the following elements, write its chemical symbol, locate it in the
periodic table, give its atomic number, and indicate whether it is a metal, metalloid,
or nonmetal:
(a) chromium
(b) helium
(c) phosphorus
(d) zinc
(e) magnesium
(f) bromine
(g) arsenic
2. For each of the following elements, write its name, locate it in the periodic table,
give its atomic number, and indicate whether it is a metal, metalloid, or nonmetal:
(h) Li
(i) Sc
(j) Ge
(k) Yb
(l) Mn
(m) Sb
(n) Xe
3. Does the following drawing represent a neutral atom or a ion? Write its complete
chemical symbol including mass number, atomic number, and net charge.
Fill in the tables below with the missing information
59Co3+
Symbol
Protons
34
76
Neutrons
46
116
Electrons
36
Net Charge
2+
Symbol
Protons
Neutrons
Electrons
Net Charge
80
120
78
31P3-
34
45
2-
50
69
46
118
76
3+
4. What is the mass in amu of a carbon-12 atom? Why is the atomic weight of carbon
reported as 12.011 on the periodic table?
5. Only two isotopes of copper occur naturally, 63Cu (atomic mass = 62.9296 amu;
abundance 69.17%) and 65Cu (atomic mass = 64.9278 amu; abundance 30.83%).
Calculate the atomic weight (average atomic mass) of copper.
6. Only two isotopes of Rubidium occur naturally, rubidium-85 (atomic mass =
84.9118 amu; abundance 72.15%) and rubidium-87 (atomic mass = 86.9092 amu;
abundance 27.85%). Calculate the atomic weight (average atomic mass) of
rubidium.
Station 2 – The Periodic Table and Naming
1. What is the distinction between atomic number and mass number? Between mass
number and atomic mass?
2. Distinguish between the terms family and period in connection with the periodic
table. For which of these is the term group also used.
3. When metals react with nonmetals, an ionic compound generally results. What is
the predicted general formula for the compound formed between an alkali metal
and sulfur? Between an alkaline earth metal and nitrogen? Between aluminum and a
halogen?
4. The compounds AlCl3, CrCl3, and ICI3 have similar formulas, yet each follows a
different set of rules to name it. Name these and then compare and contrast the
nomenclature rules.
5. How would you name HBrO4, KIO3, NaBrO2, and HIO?
6. Four of the boxes in the following periodic table are colored. Which of these are
metals and which are nonmetals? Which one is an alkaline earth metal? Which one
is a noble gas?
Station 3 – Isotopes and Atomic Structure
1. Answer the following questions:
a. What are the main subatomic particles that make up the atom?
b. What is the relative charge (in multiples of the electronic charge) of each of the
particles
c. Which of the particles is the most massive
d. Which is the least massive
2. Which of the statements is (are) true? For the False statements, correct them!
(T/F)
a. All particles in the nucleus of an atom are charged
b. The atom is best described as a uniform sphere of matter in which electrons are
embedded.
c. The mass of the nucleus is only a very small fraction of the mass of the entire atom
d. The volume of the nucleus is only a very small fraction of the total volume of the
atom
e. The number of neutrons in a neutral atom must equal the number of electrons
3. The isotope of an unknown element, X, has a mass number of 79. The most stable ion of the
isotope has 36 electrons and forms a binary compound with sodium having a formula of
Na2X. What might element X be?
4. Complete the table by placing symbols, formulas, and names in the blanks.
Cation
Anion
Name
Ammonium
Bromide
Ba2+
BaS
Cl-
Al3+
Formula
Iron (II) chloride
F(CO3)2-
PbF2
Iron (III) oxide
5. The average atomic mass of a chlorine atom is 35.45 amu. Chlorine consists of two
isotopes, 35Cl and 37Cl. Which of the following most closely approximates the relative
abundance of these isotopes?
a. 25% 35Cl and 75% 37Cl
b. 50% 35Cl and 50% 37Cl
c. 75% 35Cl and 25% 37Cl
d. 90% 35Cl and 10% 37Cl
6. A charged particle is caused to move between two
electrically plates, as shown here:
(a) Why does the path of the charged particle bend?
(b) What is the sign of the electrical charge on the particle?
(c) As the charge on the plates is increased, would you expect the bending to increase,
decrease, or stay the same?
(d) As the mass of the particle is increased while the speed of the particles remains the same,
would you expect the bending to increase, decrease or stay the same?