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: 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: 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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• Number of notations in electronic configuration will show the number of shells of Electrons the Atom has, showing the Period
• Last Notation shows the number ofouter Electrons the Atom has, showing the Group

EXAMPLE:  Electronic Configuration of Chlorine:

PERIOD: Red numbers at the Bottom Show the number of notations which is 3, indicating that Chlorine atom has 3 shells of Electrons

GROUP: Green box highlights the last notation which is 7, indicating that 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 as 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