YEAR 11 CHEMISTRY: ATOMIC THEORY TEST
NAME:
SECTION A: MULTIPLE CHOICE (16 marks). Total for test = 43 marks
1. An atom becomes a POSITIVE ion when it:
a) atomic number changes
b) mass number changes
c) gains protons
d) loses electrons
2. The electron subshell configuration of a carbon atom is:
a) 1s2 2s2 2p6
b) 1s2 2s2 2p6 3s1
c) 1s2 2s2 2p2
d) 1s2 2s2 2p4
3. The electron subshell configuration of a phosphorus atom is:
a) 1s2 2s2 2p3
b) 1s2 2s2 2p6 3s2 3p3
c) 1s2 2s2 2p6 3s2 3p6 3d3
d) 1s2 2s2 2p6 3s2 3p1
e) 1s2 2s2 2p1
4. The electronic structure 1s2 2s2 2p6 3s2 3p6 corresponds to the species:
a) O2b) S2c) Al3+
d) Na+
e) S
5. Fluorine, chlorine, bromine and iodine show many similarities in their chemical
behaviour. The most fundamental reason for this fact is that:
a) they all form hydrides of the general formula HX
b) they are all coloured, nonmetallic elements with steadily increasing melting
temperatures
d) all of their outer shell electrons in their ground states are in the same shell
e) they all have the same outer shell electron configuration
6. The largest number of electrons that can occupy a ‘p’ subshell is:
a) 2
b) 4
c) 6
d) 8
e) 10
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ITEMS 7, 8, 9 AND 10 REFER TO THE FOLLOWING INFORMATION
Species
Atomic number
Mass number
1
2
3
4
5
6
2
10
17
20
20
26
4
20
37
40
44
56
Electron configuration
1s2
1s2 2s2 2p6
1s2 2s2 2p6 3s2 3p6
1s2 2s2 2p6 3s2 3p6
1s2 2s2 2p6 3s2 3p6 3d1 4s1
1s2 2s2 2p6 3s2 3p6 3d6 4s2
7. The two species that would occupy the same position on the Periodic Table would
be:
a) 2 and 3
b) 2 and 4
c) 4 and 5
d) 1 and 6
8. The two species that represent different elements with similar chemical properties
are:
a) 1 and 2
b) 3 and 4
c) 4 and 5
d) 5 and 6
9. The two species that represent different elements in the same period of the Periodic
Table are:
a) 1 and 3
b) 2 and 4
c) 4 and 5
d) 5 and 6
10. Which of the following electron configurations represents an element in the
excited state?
a) 3
b) 4
c) 5
d) 6
Q11. A certain neutral atom has the electron configuration 1s2 2s2 2p6 3s2. The
electron configuration of the next atom in the group in the Periodic Table would be:
a) 1s2 2s2 2p6 3s2 3p1
b) 1s2 2s2 2p6 3s2 3p2
c) 1s2 2s2 2p6 3s2 3p6 4s2
d) 1s2 2s2 2p6 3s2 3p6 3d2 4s2
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12. One of the most harmful species from the fallout of an atomic bomb is a
radioactive isotope of the species 90Sr38. The number of neutrons in the nucleus of one
atom of this isotope is:
a) 38
b) 52
c) 90
d) 128
13. The elements in Group IV of the Periodic Table have atoms with:
a) identical chemical properties
b) identical physical properties
c) the same electron configuration
d) 2 electrons in a p subshell
14. Of the elements whose atomic numbers are given below, which one has quite
different physical and chemical properties from the others?
a) 12
b) 16
c) 20
d) 38
15. Elements in different groups in the Periodic Table (eg. sodium and chlorine)
generally have different chemical properties because they have:
a) different numbers of outer shell electrons
b) different shells as their outer shell
c) atoms that are different in size
d) different mass numbers
16. An element is a substance that consists of:
a) atoms of identical mass
b) atoms which have the same number of protons
c) atoms all of which are exactly the same
d) aggregates of single atoms, not molecules
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SECTION B: EXTENDED ANSWER QUESTIONS
(27 marks)
1. Define the following terms and give one example of each:
a) element
b) isotope
c) period
d) group
e) ion
(7.5 marks)
Q2.
For each of the following materials, link each with a property that it possesses.
You may only link each material with one property.
soft and flexible
diamond
brittle but heat resistant
ceramic
excellent conductor
polyester
extremely hard and wear resistant
polyurethane rubber
clothing fibre
copper
(2.5 marks)
Q3. What are the Group and Period numbers of the elements with atomic numbers of
a) 7
b) 16
(2 marks)
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Q4. Write out the electron configuration of the elements in:
a) Period 2, second element along in the p block
b) Period 4, first element along in the s block
c) Period 4, second element along in the d block
(3 marks)
Q5.
Complete the Table below:
Name
Symbol
Atomic number
No. of neutrons No. of electrons
6
Neon
19
35
17
8
6
12
10
20
18
Cl 
(10 x 0.5 = 5 marks)
Q6. Determine the names or formulae (as appropriate) of the following compounds:
a)
b)
c)
d)
e)
f)
g)
CaCO3 =
Mg(OH)2 =
Fe2O3 =
Zn(NO3)2=
Copper(II) iodide
Barium sulfate =
Aluminium nitrate =
(7 marks)
END OF TEST
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