Worksheet 1: Atomic structure. Worksheet 2: Rules for electronic configurations.
Worksheet 3: Electronic configurations. Worksheet 4: More electronic ...
Chapter 1 Atomic structure Worksheet 1: Atomic structure Worksheet 2: Rules for electronic configurations Worksheet 3: Electronic configurations Worksheet 4: More electronic configurations End-of-chapter test Marking scheme: Worksheet 1 Marking scheme: Worksheet 2 Marking scheme: Worksheet 3 Marking scheme: Worksheet 4 Marking scheme: End-of-chapter test
Worksheet 1 Atomic structure [5.1.2.d] 1
Copy and complete the following table.
Element
Symbol
Atomic number
Mass number
Protons
Neutrons
Electrons
Electron config.
Common ion formed
Electrons gained or lost?
Oxygen
O
8
16
8
8
8
2,6
2–
2 gained
Sodium Fluorine Lithium Calcium Sulphur Chlorine [9]
2
3
4
Use information from your table from Question 1 to explain: a
Why lithium and sodium are both in Group I of the Periodic Table.
[1]
b
Why sulphur and sodium are both in Period 3 of the Periodic Table.
[1]
c
Why sulphur and oxygen are both in Group VI of the Periodic Table.
[1]
d
Why lithium and oxygen are both in Period 2 of the Periodic Table.
[1]
e
Why lithium and sodium both form a simple ion of the same charge.
[1]
f
Why fluorine and chlorine both form a simple ion of the same charge.
[1]
Write down the formulae of the following compounds and use your Periodic Table to calculate the relative molecular mass of each compound. a
Sulphuric(VI) acid
b
Nitric acid
c
Hydrochloric acid
d
Sodium hydroxide
e
Ammonia
f
Sodium chloride
g
Calcium oxide
h
Sodium oxide
i
Calcium fluoride
j
Lithium sulphide
[20]
Define a atomic number and b mass number.
[2] Total:
2
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1 Atomic structure
Worksheet 2 Rules for electronic configurations [5.1.2k] 1 2 3 4 5 6 7
Every electron in an atom or ion must be in an orbital. Each orbital can accommodate two electrons. For the elements H to Kr there are three types of orbital – s, p and d. The first energy level has one s orbital only – the 1s. The second energy level has one s orbital – the 2s – and three p orbitals – the 2p. We say the second energy level has a 2s subshell and a 2p subshell. The third energy level has one s orbital – the 3s – three p orbitals – the 3p – and five d orbitals – the 3d.
8 We say the third energy level has a 3s subshell, a 3p subshell and a 3d subshell. 9 The only orbitals in the fourth energy level that concern us are the 4s orbital and the three 4p orbitals.
10 In the third shell the 3s has the lowest energy, and the 3d has the highest energy. 11 Electrons fill lower energy orbitals first, but remember that the 4s fills before the 3d, except for Cr and Cu, both of which have only one electron in the 4s.
12 So the order of filling is 1s → 2s → 2p → 3s → 3p → 4s → 3d → 4p, but remember Cr and Cu.
13 If two electrons are in the same orbital they must spin-pair. Electrons don’t spinpair if they don’t have to.
14 When atoms form positive ions they lose the electrons in the outermost orbitals. 1
Fill in the boxes to show the electronic configurations of the following atoms and ions.
1s
2s
2p
2p
2p
3s
3p
3p
3p
4s
Na Na+ Ca Ca2+ Al Al3+ O O2– Cl Cl– P P3– [12] Total: 1 Atomic structure
/ 12 Score:
%
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3
4
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1 Atomic structure
Electronic configurations [5.1.2k]
Kr
Ge
Zn
Cu
Ni
Cr
V
Ti
Sc
Ar
Cl
Al
Na
Ne
O
N
Be
He
H
1s
2s
2p
2p
2p
3s
3p
3p
3p
Fill in the boxes to show the electronic configurations of the following atoms.
Worksheet 3: 4s
3d
3d
3d
3d
3d
Total:
4p
4p
/ 19 Score:
4p
%
1 Atomic structure
© Cambridge University Press 2005
5
Cr
Ca
As
Fe
Mn
Cu
Ga
K
Si
S
C
B
Li
Mg
Co
Br
F
P
Se
1s
2s
2p
2p
2p
3s
3p
3p
3p
4s
More electronic configurations [5.1.2k]
Fill in the boxes to show the electronic configurations of the following atoms.
Worksheet 4: 3d
3d
3d
3d
3d
Total:
4p
4p
/ 19 Score:
4p
%
End-of-chapter test 1
If a proton has a relative mass of 1 unit and a relative charge of +1 unit, what is the relative mass and charge of a
a neutron
[2]
b
an electron?
[2]
2
Sketch an atom of deuterium, the isotope of hydrogen with mass number 2. Label your sketch. Include the labels ‘positive charge here’ and ‘negative charge here’. [3]
3
An atom has 40 protons and 50 neutrons in its nucleus. Another atom has 40 protons and 54 neutrons in its nucleus.
4
a
What is the atomic number and mass number of each atom?
[2]
b
Explain the meaning of the term ‘isotopes’ using these atoms as examples.
[2]
How many protons, neutrons and electrons are there in each of the following? (Use the Periodic Table to find atomic numbers.) a
5
An atom of zinc, mass number 64.
b
A Zn ion, mass number 66.
[2]
c
An N3– ion, mass number 14.
[2]
–
d
An H ion, mass number 1.
[2]
a
Sketch the shape of the 2s orbital and of one of the 2p orbitals.
[2]
b
How many orbitals are there:
c d
i
in the 3s subshell?
[1]
ii
in the 3p subshell?
[1]
iii in the 3d subshell?
[1]
Arrange the following four subshells in order of increasing energy (lowest energy first): 3d, 4s, 3s, 3p.
[3]
Use subshell notation (e.g. 1s2, etc.) to give the electronic configurations of the following atoms and ions: i
K
[1]
iv
Na+
[1]
ii
Cr
[2]
v
Cu2+
[1]
vi
–
[1]
iii Se
6
[2]
2+
a
[1]
F
Explain the meaning of the term ‘first ionisation energy’, including an equation in your answer.
[3]
Explain the meaning of the term ‘third ionisation energy’, including an equation in your answer.
[2]
Sketch a graph of the successive ionisation energies of element 12, magnesium.
[3]
d
Explain why the graph in part c has this shape.
[3]
e
Explain why:
b c
i
Na has a lower first ionisation energy than Li
[1]
ii
F has a lower first ionisation energy than Ne
[1]
iii Na has a lower first ionisation energy than Mg
[1]
iv Na has a lower first ionisation energy than Ne
[1]
v
[1]
Al has a lower first ionisation energy than Mg Total:
6
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%
1 Atomic structure
Marking scheme Worksheet 1: Atomic structure 1 Element
Symbol
Atomic number
Mass number
Protons
Neutrons
Electrons
Electron config.
Common ion formed
Electrons gained or lost?
Oxygen
O
8
16
8
8
8
2,6
2–
2 gained
Sodium
Na
11
23
11
12
11
2,8,1
1+
1 lost
Fluorine
F
9
19
9
10
9
2,7
1–
1 gained
Lithium
Li
3
7
3
4
3
2,1
1+
1 lost
Calcium
Ca
20
40
20
20
20
2,8,8,2
2+
2 lost
Sulphur
S
16
32
16
16
16
2,8,6
2–
2 gained
Chlorine
Cl
17
35 or 37
17
18 or 20
17
2,8,7
1–
1 gained
[1] for each correct column [9]
2
3
4
a
both have one electron in the outer shell [1];
b
both have their outer electron(s) in the third shell [1];
c
both have six electrons in the outer shell [1];
d
both have their outer electron(s) in the second shell [1];
e
both have one electron in the outer shell and lose it when they ionise [1];
f
both have one gap in the outer shell and fill it by gaining one electron when they ionise [1]
a
H2SO4 [1], 98.1 [1];
b
HNO3 [1], 63.0 [1];
c
HCl [1], 36.5 [1];
d
NaOH [1], 40.0 [1];
e
NH3 [1], 17.0 [1];
f
NaCl [1], 58.5 [1];
g
CaO [1], 56.1 [1];
h
Na2O [1], 62.0 [1];
i
CaF2 [1], 78.1 [1];
j
Li2S [1], 45.9 [1]
a
the number of protons in the nucleus of the atom [1];
b
the total number of protons and neutrons in the nucleus of the atom [1]
1 Atomic structure
© Cambridge University Press 2005
7
Marking scheme Worksheet 2: Rules for electronic configurations 1s
2s
2p
2p
2p
3s
3p
3p
3p
4s
Na
↑↓
↑↓
↑↓
↑↓
↑↓
↑
Na+
↑↓
↑↓
↑↓
↑↓
↑↓
Ca
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
Ca2+
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
Al
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑
Al3+
↑↓
↑↓
↑↓
↑↓
↑↓
O
↑↓
↑↓
↑↓
↑
↑
O2–
↑↓
↑↓
↑↓
↑↓
↑↓
Cl
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑
Cl–
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
P
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑
↑
↑
P3–
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
[1] for each correct row [12]
8
© Cambridge University Press 2005
1 Atomic structure
1 Atomic structure
© Cambridge University Press 2005
9
↑↓
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↑↓
↑↓
He
Be
N
O
Ne
Na
Al
Cl
Ar
Sc
Ti
V
Cr
Ni
Cu
Zn
Ge
Kr
2s
H
1s
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑
2p
Marking scheme:
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
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↑↓
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↑
↑
2p
↑↓
↑↓
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↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
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↑↓
↑
↑
2p
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑
3s
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑
3p
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
3p
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑
3p
↑↓
↑↓
↑↓
↑
↑↓
↑
↑↓
↑↓
↑↓
4s
↑↓
↑↓
↑↓
↑↓
↑↓
↑
↑
↑
↑
3d
Worksheet 3: Electronic configurations
↑↓
↑↓
↑↓
↑↓
↑↓
↑
↑
↑
3d
↑↓
↑↓
↑↓
↑↓
↑↓
↑
↑
3d
↑↓
↑↓
↑↓
↑↓
↑
↑
3d
↑↓
↑
4p
↑↓
↑
4p
↑↓
4p
[19], [1] for each correct row
↑↓
↑↓
↑↓
↑↓
↑
↑
3d
10
© Cambridge University Press 2005
1 Atomic structure
2s
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑
↑↓
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↑↓
1s
↑↓
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↑↓
↑↓
↑↓
↑↓
Se
P
F
Br
Co
Mg
Li
B
C
S
Si
K
Ga
Cu
Mn
Fe
As
Ca
Cr
↑↓
↑↓
↑↓
↑↓
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↑↓
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↑
↑
↑↓
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2p
↑↓
↑↓
↑↓
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↑↓
↑↓
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↑
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↑↓
2p
↑↓
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↑
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2p
↑↓
↑↓
↑↓
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3s
↑↓
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↑↓
↑↓
↑↓
↑↓
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↑
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↑
↑↓
3p
↑↓
↑↓
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↑↓
↑↓
↑↓
↑↓
↑↓
↑
↑
↑↓
↑↓
↑
↑↓
3p
Worksheet 4: More electronic configurations
Marking scheme
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑↓
↑
↑↓
↑↓
↑
↑↓
3p
↑
↑↓
↑↓
↑↓
↑↓
↑
↑↓
↑
↑↓
↑↓
↑↓
4s
↑
↑↓
↑↓
↑
↑↓
↑↓
↑↓
↑↓
↑↓
3d
↑
↑↓
↑
↑
↑↓
↑↓
↑↓
↑↓
↑↓
3d
↑
↑↓
↑
↑
↑↓
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↑
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↑↓
3d
↑
↑↓
↑
↑
↑↓
↑↓
↑
↑↓
↑↓
3d
↑
↑
↑↓
↑↓
4p
↑
↑↓
↑
4p
↑
↑
↑
4p
[19], [1] for each correct row
↑
↑↓
↑
↑
↑↓
↑↓
↑
↑↓
↑↓
3d
Marking scheme End-of-chapter test 1
a b
2
Sketch shows one electron in shell and one proton and one neutron in nucleus [1], shell area labelled ‘negative charge here’ [1], nucleus labelled ‘positive charge here’ [1]
3
a b
40 and 90 [1], 40 and 94 [1]; atoms that have the same atomic number, 40 in this case [1], but different mass numbers, 90 and 94 in this case [1]
4
a
30, 34, 30 [2];
b
30, 36, 28 [2];
c
7, 7, 10 [2];
d
1, 0, 2 [2]
a
s is spherical [1], p is hour-glass/dumbbell shaped [1];
b
i
1 [1];
ii
3 [1];
5
1 [1], 0 [1]; 0 (or negligible) [1], –1 [1]
iii 5 [1]; c
3s before 3p [1], 3p before 4s [1], 4s before 3d [1];
d
i
1s2 2s2 2p6 3s2 3p6 4s1 [1];
ii
1s2 2s2 2p6 3s2 3p6 4s1 3d5 [2];
iii 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4 [1]; iv 1s2 2s2 2p6 [1]; v
1s2 2s2 2p6 3s2 3p6 4s0 3d9 [1];
vi 1s2 2s2 2p6 [1]
6
a
the energy required to remove 1 mole of electrons [1], from 1 mole of gaseous atoms [1], X(g) → X+(g) + e– [1];
b
the energy required to remove 1 mole of electrons from 1 mole of gaseous 2+ ions [1], X2+(g) → X3+(g) + e– [1];
c
first 2 low [1], next 8 middle [1], last 2 high [1];
d
2 outer electrons are easy to remove [1], 8 electrons in 2nd shell are not so easy to remove [1], final 2 electrons in 1st shell are very hard to remove [1];
e
i
in Na, the outer electron is further from the nucleus/more shielded [1];
ii
Ne has one more proton in nucleus than F, so electron attracted more in Ne [1];
iii Mg has one more proton in nucleus than Na [1]; iv in Na, the outer electron is further from the nucleus/more shielded/the Na atom has a smaller effective nuclear charge [1]; v
the outer electron in Al is further from the nucleus than the outer electron in Mg (different subshells) [1]
1 Atomic structure
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