Unit 2 Atomic Structure and Periodic Trends Review
The review contains previous Cambridge practice test questions similar to what is on the test. The
questions represent the objectives but may not be the actual content of the test. Make sure that you
also study notes, worksheets and labs.
Objective 3.1 Atomic Structure and Periodic Table
1. Complete the following table which gives the number of protons, electrons and neutrons in each
of the five particles.
2. The electronic structures of five atoms of different elements A, B, C, D, and E, are shown below.
Answer the following questions about these structures. Each structure may be used once, more
than once or not at all. [6]
Which structure
a. Is in Period 4 of the periodic table
b. Is a noble gas
c. Is in group II on the periodic table
d. Has five electrons in its outer shell
e. Has a proton (atomic) number of 7
f.
Represent a fluorine atom
3. Iron has several isotopes.
a. What do you understand by the term isotopes? [2]
b. The table shows the number of subatomic particles in an atom of iron. Complete the
table to show the relative charge on each particle. [3]
c. State the mass number in this isotope of iron. [1]
d. Write the formula for this isotope of iron. [1]
Objective 9.1 Periodic Table and 9.2 Periodic Trends
1. Part of the Periodic Table of elements is shown below. Answer the following questions using
only the elements shown in the table above.
Write the symbol for an element which
a. Is used to fill light bulbs. [1]
b. Is in Group VI and Period 3 of the Periodic Table. [1]
c. Is a black solid [1]
d. Forms about 79% of the air [1]
e. Consists of single atoms with a full outer shell of electrons [1]
2. Dmitri Mendeleev published his first periodic table in 1869.Part of this table is shown below.
a. What differences are there between Mendeleev’s table and the Periodic Table we use
today? [4]
b. State the names of any two elements in the table above which exist as diatomic
molecules. [1]
Objective 9.3 Group Properties
3. Some properties of the Group I metals are shown in the table
metal
melting point oC
hardness
lithium
fairly hard
sodium
98
fairly soft
potassium
63
soft
rubidium
39
very soft
cesium
29
extremely soft
density g per cm3
0.53
1.53
1.88
i.
Estimate the melting point of lithium. [1]
ii.
How does hardness of these metals change down the group? [1]
iii.
Estimate the density of potassium [1]
4. The table shows some physical properties of the Group VII elements.
a. Use the information to explain why
i. Chlorine is a gas at room temperature. [1]
ii. Bromine is a liquid at room temperature. [1]
b. Describe the trend in atomic radius going down the group from chlorine to iodine. [1]
c. Suggest a value for the atomic radius of fluorine. [1]
d. Describe the color of chlorine. [1]
e. A chlorine atom has 17 electrons. Complete the following structure to show how the
electrons are arranged.
Objective 9.4 Transition Elements
5. Iron is a typical metal.
a. Give three characteristics of a typical metal. [3]
b. Iron is a transition metal. Give three physical characteristics of transition metals. [3]
c. Give a chemical characteristic of transition metals.
Objective 9.5 Noble Gases
6. Group 0 contain the noble gases.
a. Why are noble gases unreactive?
b. Give a use of noble gases.