Electron Configuration and the Periodic Table

Holt: Modern Chemistry © 2009

Section 5:2 Electron Configuration and Periodic Properties

L. Blanchard Byrne

5-2020

Target 00-03: I can use the periodic table to predict qualities of elements.

Target 05-02: I can use periodic law to predict the properties of elements.

Target 05-03: I can use the periodic table to write the noble gas configuration for an element.

Noble Gas Configuration

Electrons and Families

Noble Gas Configuration

Electrons and Families

Noble Gas Configuration is a shortcut method of writing electron configurations that replaces some of the orbital notations with the noble gas located in the period above.

Chlorine [ Ne] 3s² 3p⁵

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Noble Gas Configuration

1) Find the element location on the table.

2) Locate the noble gas at the end of the period above the element.

3) Start with that element in brackets and then follow the Periodic Table with the electron configuration until you get to the element on the table.

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Noble Gas Configuration

Bromine

Bromine is in Period 4

The noble gas in Period 3 is argon

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[Ar] 4s² 3d¹⁰ 4p⁵

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Write the Noble Gas Configuration for the following elements.

• Magnesium
• Chromium
• Selenium
• Cesium
• Silver
• Xenon

• [Ne] 3s²
• [Ar] 4s¹ 3d⁵
• [Ar] 4s² 3d¹⁰ 4p⁴
• [Xe] 6s¹
• [Kr] 5s¹ 4d¹⁰
• [Kr] 5s² 4d¹⁰ 5p⁶

• Silicon
• Tellurium

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• [Ne] 3s² 3p²
• [Kr] 5s² 4d¹⁰ 5p⁴

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Family Names

Family IA Alkali Metals

Family IIA Alkaline Earth Metals

Family IIIA Mixed Group – Boron Family

Family IVA Mixed Group – Carbon Family

Family VA Pnictogens (Mixed Group) –

Nitrogen Family

Family VIA Chalcogens - Oxygen Family

Family VIIA Halogens

Family VIIIA Noble Gases

IB – VIIIB Transition Metals

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9

s-Block:

Hydrogen and Helium

• Special Cases
• Not members of Alkali Metals or Alkaline Earth Metals
• Hydrogen does not share properties with Group IA
• Helium has full outer shell and is placed above the Noble Gases even though it does not have an octet.

s-Block: Group IA

• Alkali Metals
• Ion Charge (+1)
• Silvery luster, soft enough to cut with a knife, malleable, ductile, low density
• Extremely reactive, combine with water to release hydrogen gas and aqueous alkalis
• Stored under kerosene to prevent reaction with air
• From top to bottom of the periodic table, they melt at successively lower temperatures
• Good conductors of heat and electricity

Lithium

Reactivity of Alkali Metals

s-Block: Group IIA

• Alkaline Earth Metals
• Ion Charge (+2)
• Silvery luster, ductile and malleable
• Good conductors of heat and electricity
• Harder, denser and stronger than alkali metals
• Higher melting points than alkali metals
• Too reactive to be found pure in nature
• React with water to form bases and hydrogen gas

Calcium

d-Block Elements

Groups IB-VIIIB

• Transition Metals
• Typical metallic properties
• Good conductors of heat and electricity
• Harder and more brittle than Groups IA and IIA
• Less reactive and can be found pure in nature

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• Gold, palladium, platinum are the least reactive of all non-noble gas elements

p-Block Elements

Groups IIIA - VIIIA

• s and p blocks constitute the Main Group Elements
• Contains metals, metalloids and all non-metals
• Metals – harder and denser than s-block but softer and less dense than d-block, usually found combined in nature but stable when pure in contact with air
• Metalloids – semiconductors
• Brittle solids, some properties of both metals and nonmetals
• Nonmetals - solids, liquids, and gases
• Halogens are most reactive nonmetals

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Bromine

f-Block Elements

• Actinides are all radioactive
• Only first four are natural, the rest are synthetic
• Lanthanides are shiny metals similar in reactivity to Group II alkaline earth metals

Fin

• Review Questions p. 149

• How are the blocks of the periodic table related to electron configurations?
• Name the families and groups on the Periodic Table.
• Use electron configuration to locate an element on the periodic table.
• Write electron configurations from the periodic table.

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Bromine