1.18-1.24 IGCSE Chemistry 2018

1 Principles of chemistry 

2 Inorganic chemistry 

3 Physical chemistry 

4 Organic chemistry 

1 Principles of chemistry  

(d) The Periodic Table 

Students should:

 1.18 understand how elements are arranged in the Periodic Table: • in order of atomic number • in groups and periods. 1.19 understand how to deduce the electronic configurations of the first 20 elements from their positions in the Periodic Table 1.20 understand how to use electrical conductivity and the acid-base character of oxides to classify elements as metals or non-metals 1.21 identify an element as a metal or a non-metal according to its position in the Periodic Table 1.22 understand how the electronic configuration of a main group element is related to its position in the Periodic Table Pearson Edexcel International GCSE in Chemistry – Specification – Issue 2 – April 2018 © Pearson Education Limited 2018 13 Students should: 1.23 understand why elements in the same group of the Periodic Table have similar chemical properties 1.24 understand why the noble gases (Group 0) do not readily react

Notes:

The Periodic Table

• The Periodic Table MS
• The Periodic Table QP

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• The Periodic Table MS
• The Periodic Table QP

1.18: Understand How Elements are Arranged in the Periodic Table: In Order of Atomic Number, In Groups and Periods

PERIOD: Horizontal Rows that Show the Number of Shells of Electrons an Atom Has

GROUP: Vertical Columns that Show How Many Outer Electrons an Atom Has

THE PERIODIC TABLE:

All Elements are Arranged in the Order of Increasing Atomic Number from Left to Right

1.19: Understand How to Deduce the Electronic Configuration of the First 20 Elements from their Positions in the Periodic Table

ELECTRONIC CONFIGURATION: The Arrangement of Electrons into Shells for an Atom

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• Electrons Always Occupy Shells that are Closest to the Nucleus First
• When a Shell Becomes Full, Electrons will Fill the Next Shell

ELECTRONIC CONFIGURATION OF FIRST 20 ELEMENTS:

ELEMENT	NUMBER OF ELECTRONS	ELECTRONIC CONFIGURATION
HYDROGEN	1	1
HELIUM	2	2
LITHIUM	3	2 . 1
BERYLLIUM	4	2 . 2
BORON	5	2 . 3
CARBON	6	2 . 4
NITROGEN	7	2 . 5
OXYGEN	8	2 . 6
FLUORINE	9	2 . 7
NEON	10	2 . 8
SODIUM	11	2 . 8 . 1
MAGNESIUM	12	2 . 8 . 2
ALUMINIUM	13	2 . 8 . 3
SILICON	14	2 . 8 . 4
PHOSPHORUS	15	2 . 8 . 5
SULFUR	16	2 . 8 . 6
CHLORINE	17	2 . 8, . 7
ARGON	18	2 . 8 . 8
POTASSIUM	19	2 . 8 . 8 . 1
CALCIUM	20	2 . 8 . 8 . 2

1.20: Understand How to Use Electrical Conductivity and the Acid-Base Character of Oxides to Classify Elements as Metals or Non-Metals

METALS	NON - METALS
Basic Oxides (Alkaline)	Acidic Oxides (Acidic)
Good Conductors of Electricity	Poor Conductors of Electricity
High Melting and Boiling Point	Low Melting and Boiling Point
Malleable	Flaky

1.21: Identify an Element as a Metal or a Non-Metal According to its Position in the Periodic Table

THE PERIODIC TABLE:

A Zig - Zag Line in this Diagram Separates the Metals on the Left, from the Non - Metals on the Right

1.22: Understand How the Electronic Configuration of a Main Group Element is Related to its Position in the Periodic Table

ELECTRONIC CONFIGURATION: The Arrangement of Electrons into Shells for an Atom (E.g Electronic Configuration of Carbon is  2 . 4 )

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ELECTRONIC CONFIGURATION AND POSITION IN PERIODIC TABLE

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• The Number of Notations in the Electronic Configuration will show the Number of Shells of Electrons the Atom has, Showing the Period
• The Last Notation Shows the Number of Outer Electrons the Atom has, Showing the Group

EXAMPLE:  Electronic Configuration of Chlorine:

PERIOD: The Red Numbers at the Bottom Show the Number of Notations which is 3, Showing that a Chlorine Atom has 3 Shells of Electrons

GROUP: The Green Box Highlights the Last Notation which is 7, Showing that a Chlorine Atom has 7 Outer Electrons

ON THE PERIODIC TABLE:

Diagram Showing the Position of Chlorine on the Periodic Table

1.23: Understand Why Elements in the Same Group of the Periodic Table have Similar Chemical Properties

GROUP: Vertical Columns that Show How Many Outer Electrons an Atom Has

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CHEMICAL PROPERTIES OF ELEMENTS IN THE SAME GROUP:

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• Elements in the Same Group in the Periodic Table will have Similar Chemical Properties
• This is because they have the Same Number of Outer Electrons so will React and Bond Similarly
• For Example, Both Lithium and Sodium are in Group 1 and can React with Elements in Group 7 to Form an Ionic Compound (Charges of Group 1 Elements are +1, Charges of Group 7 Elements are -1)

1.24: Understand Why the Noble Gases (Group 0) Do Not Readily React

NOBLE GASES: Group 0 Elements that are Unreactive

Noble Gases are Inert (Unreactive) as they Have a Full Outer Shell of Electrons so Do Not Easily Lose or Gain Electrons