Download MYP 10 PeriodicityWS

MYP 10 Chemistry 2013-14
Periodicity Worksheet
Name: _________________________________ ( )
Class: _________ Date: _____________
_________________________________________________________________________________
3.1 The Periodic Table
3.1.1 Describe the arrangement of elements in the periodic table in order of increasing atomic number.
3.1.2 Distinguish between the terms group and period.
3.1.3 Apply the relationship between the electron arrangement of elements and their position in the periodic table up to Z = 20.
3.1.4 Apply the relationship between the number of electrons in the highest occupied energy level for an element and its position
in the periodic table.
3.2 Physical properties
3.2.1 Define the terms first ionization energy and electronegativity.
3.2.2 Describe and explain the trends in atomic radii, ionic radii, first ionization energies, electronegativities and melting points
for the alkali metals (Li  Cs) and the halogens (FI).
3.2.3. Describe and explain the trends in atomic radii, ionic radii, first ionization energies and electronegativities for elements
across period 3.
3.3 Chemical properties
3.3.1 Discuss the similarities and differences in the chemical properties of elements in the same group.
3.3.2 Discuss the changes in nature from ionic to covalent and from basic to acidic, of the oxides across the period 3.
1. Explain what is meant by the term electronegativity and explain why the electronegativity of
fluorine is greater than that of chlorine.
2. What are isoelectronic species? Explain with an illustration of at least 2 species.
3. The following table shows values that appear in the Data Booklet.
Table 1 Covalent (atomic) radii / 10–12 m
Na
186
Mg
160
Al
143
Si
117
N
70
P
110
0
66
S
104
F
58
Cl
99
N3–
171
P3–
O2–
146
S2–
F–
133
Cl–
212
190
181
Table 2 Ionic radii/10–12 m
Na+
98
Mg2+
65
Al3+
45
Si4+
42
Explain why
(i) the magnesium ion is much smaller than the magnesium atom.
(ii) there is a large increase in ionic radius from silicon to phosphorus.
(iii) the ionic radius of Na+ is less than that of F–.
1
4(a) The diagram below shows the melting points of some of the elements in Period 3.
2000
1600
Melting
point/K
1200
800
400
0
Na Mg
Al
Si
P
S
Cl
Ar
(i)
On the diagram, use crosses to mark the approximate positions of the melting points for
the elements silicon, chlorine and argon. Complete the diagram by joining the crosses.
(ii)
By referring to its structure and bonding, explain your choice of position for the melting
point of silicon.
(iii) Explain why the melting point of sulphur, S8, is higher than that of phosphorus, P4
(b)
State and explain the trend in melting point of the Group II elements Ca–Ba and Group VII
elements F – At.
5(a) Draw a diagram to show the structure of sodium chloride. Explain, in terms of bonding, why
sodium chloride has a high melting point.
(b) Lithium reacts with water. Write an equation for the reaction and state two observations that could be
made during the reaction.
[SL paper 2, Nov 05]
6 (a) For each of the following reactions in aqueous solution, state one observation that would be made,
and deduce the equation.
(i) The reaction between chlorine and potassium iodide.
(ii) The reaction between silver ions and bromide ions.
7(a) The acid-base properties of the oxides are closely linked to their bonding.
Metallic elements, which form ________ oxides are basic ; non-metal oxides, which are
____________, are acidic.
Complete the table below:
Formula of
oxide
Acid-base
character
Na2O
MgO
Al2O3
SiO2
SO3(l) /
SO2(g)
(b) Explain the acid-base character of Al2O3 or SiO2 with illustrations of relevant reactions.
2
Cl2O7(l) /
Cl2O(g)