AS Chemistry Unit 1 Module 3 –The Periodic Table Periodicity

Objectives for Module 3 part 1 (a) describe the Periodic Table in terms of the arrangement of elements: (i) by increasing atomic (proton) number, (ii) in periods showing repeating trends in physical and chemical properties, (iii) in groups having similar physical and chemical properties; (b) describe periodicity in terms of a repeating pattern across different periods; (c) explain that atoms of elements in a group have similar outer shell electron configurations, resulting in similar properties; (d) describe and explain the variation of the first ionisation energies of elements shown by: (i) a general increase across a period, in terms of increasing nuclear charge, (ii) a decrease down a group in terms of increasing atomic radius and increasing electron shielding outweighing increasing nuclear charge; (e) for the elements of Periods 2 and 3: (i) describe the variation in electron configurations, atomic radii, melting points and boiling points, (ii) explain variations in melting and boiling points in terms of structure and bonding; (f) interpret data on electron configurations, atomic radii, first ionisation energies, melting points and boiling points to demonstrate periodicity.

Specification link (a) describe the Periodic Table in terms of the arrangement of elements: (i) by increasing atomic (proton) number, (ii) in periods showing repeating trends in physical and chemical properties, (iii) in groups having similar physical and chemical properties; (b) describe periodicity in terms of a repeating pattern across different periods; (c) explain that atoms of elements in a group have similar outer shell electron configurations, resulting in similar properties; (d) describe and explain the variation of the first ionisation energies of elements shown by: (i) a general increase across a period, in terms of increasing nuclear charge, (ii) a decrease down a group in terms of increasing atomic radius and increasing electron shielding outweighing increasing nuclear charge; (e) for the elements of Periods 2 and 3: (i) describe the variation in electron configurations, atomic radii, melting points and boiling points, (ii) explain variations in melting and boiling points in terms of structure and bonding; (f) interpret data on electron configurations, atomic radii, first ionisation energies, melting points and boiling points to demonstrate periodicity.

Periodicity Definition: Periodicity is a regular periodic variation of properties of elements with atomic number and position in the Periodic Table.

Order of the Periodic Table The first attempts to arrange the periodic table arranged the elements in order of atomic mass. The modern periodic table organises them in a closely related way –by atomic number the number of protons. Identify the elements where these two orders are different.

The Periodic Table Groups (columns) Metals, left of red line Non metals, right of red line 1 2 3 4 5 6 7 0 1 2 3 4 5 6 7 1 2 3 4 5 6 7 Transition metals Periods (rows) Elements are arranged in order of their atomic number. The elements in each group have similar properties. Elements show changing trends across a period.

Periodicity Across a period elements change from metallic to non-metallic. What do you notice as you descend the table? The dividing line moves to the right.

Your task..... Look at the information you have been given Describe all the trends you can see for each one and explain them First look at 1 – 4 first

What do you notice about this group? 1 Group 4: What do you notice about this group?

Periodic table and electron structure In terms of electron structure: What do elements of a group have in common? Same number of electrons in outer shell Same type of orbitals Hence similar chemical behaviours

First ionisation energies of the first 20 elements Describe all the trends you can see in the graph. Can you explain this trend in terms of the atomic structure? © Pearson Education Ltd 2008 This document may have been altered from the original

Ionisation Energy The nuclear attraction is affected by three things: Atomic radius Greater radius = less attraction. Nuclear charge Larger charge = larger attraction. Electron shielding Inner shells repeal electrons outside them, this is called shielding or screening. More inner shells = lower attraction

Across a Period There is a general increase across the period The number of protons increases, so there is more attraction acting on the electrons Electrons are added to the same shell, so the outer shell is drawn inwards slightly. Same no. of shells = same level of shielding, but more nuclear charge.

Across a Period There is a sharp decrease in 1st IE between the end of one period and the start of the next. This reflects the addition of a new shell. Increased distance from the outer shell to the nucleus Increased electron shielding of the outer electrons by the inner shells.

Trend in first ionisation energy and atomic radius across a period 3 Describe all the trends you can see in the diagram Can you explain these in terms of atomic structure? Atomic radius gets smaller Across the period electrons are being added to the same principal energy level. The nuclear charge increases. The degree of shielding is the same for each successive element. As a result, the electrons are pulled nearer the nucleus, reducing the atomic radius. © Pearson Education Ltd 2008 This document may have been altered from the original

Trend in first ionisation energy and atomic radius down a group 4 Trend in first ionisation energy and atomic radius down a group 1st IE’s decrease The number of shells increases, so the distance between the nucleus and the outer electrons – weaker attractive force. More inner shells, so the shielding increases – less attraction. Describe all the trends you can see in the diagram Can you explain these in terms of atomic structure? © Pearson Education Ltd 2008 This document may have been altered from the original

Trend in first ionisation energy and atomic radius down a group 4 Trend in first ionisation energy and atomic radius down a group Ionic radius increases More shells of electrons Increased electron shielding Also less attraction means electrons are pulled in less by the nucleus Describe all the trends you can see in the diagram Can you explain these in terms of atomic structure? © Pearson Education Ltd 2008 This document may have been altered from the original

Now look at numbers 5 – 6 Describe all the trends that you can see Explain them

Boiling points of Period 2 and Period 3 elements 5 Boiling points of Period 2 and Period 3 elements Describe all the trends you can see in the graph. Can you explain this trend in terms of the bonding and structure of the elements? Look at the elements. What happens to the elements as you move across a period?

Trends in Boiling Points Look at the table on page 87. Boiling points are based on the type of bonding present. And there are trends within each type of bonding….

Boiling Points Trend in BP across each period: Group 1 – 4 Group 4 – 5 Group 5 – 0 Li  C C  N N  Ne Na  Si Si  P P  Ar General increase in Boiling point Sharp decrease in boiling point Comparatively low boiling points Distinct change between group 4 and 5 in structure and forces From giant structures to simple molecular From strong to weak forces. Trend in melting point is similar – sharp decrease between group 4 and 5 marking the change from giant to simple molecular.

Increase in boiling point from Na to Al 6 Increase in boiling point from Na to Al Describe all the trends you can see in the diagram Can you explain these in terms of atomic structure? The ions are drawn to reflect their relative size. From sodium to aluminium: The positive charge increases and the atomic radii decreases The number of delocalised electrons per atom increases. This results in a higher charge density This increases the strength of the metallic bond which in turn increases the melting and boiling points.

Complete the worksheets. (pages 3 and 4 starter for 10 printed)

Atomic Radius Across Period 3 State and explain the general trend in atomic radius across Period 3 (excluding Argon). (4 marks) 2. Atomic radius is a general term. Measurements are taken of metallic radii for metals and covalent radii for molecules. Draw a diagram to show how you could calculate the atomic radius of 2 covalently bonded atoms. (3 marks) 3. Why does Argon not follow the trend? (2 marks) 4. State the effect of atomic radius on the first ionisation energy of an element. (1 mark)

Atomic Radius Across Period 3 State and explain the general trend in atomic radius across Period 3 (excluding Argon). (4 marks)

Atomic Radius Across Period 3 2. Atomic radius is a general term. Measurements are taken of metallic radii for metals and covalent radii for molecules. Draw a diagram to show how you could calculate the atomic radius of 2 covalently bonded atoms. (3 marks)

Atomic Radius Across Period 3 3. Why does Argon not follow the trend? (2 marks) 4. State the effect of atomic radius on the first ionisation energy of an element. (1 mark)

Exam Questions June 2012 Q2 6 marks June 2012 Q2