Section 1-3 Objectives

1) Identify some of the more important metals from the

alkali and alkaline earth groups.

2) Describe the differences in characteristics between the

metals of the alkali and the alkaline earth groups.

3) Locate the transitional metals on the periodic table.

4) Name some of the important transitional metals and

describe some of their uses.

5) Define the term alloy and name several important alloys

of transition metals.

6) Locate the inner transition metals on the periodic table.

7) Describe the general properties of the lanthanide and

actinide series of elements.

6-1 Reactive Metals: The s-block Elements

• The most reactive metals.

• s-block elements is located of the 1A and 2A groups.

• Alkali metals and alkaline earth metals.

• Most abundant elements include:

• Alkali metals: sodium (Na) and potassium (K)

• Alkaline earth metals: calcium (Ca) and magnesium

(Mg)

6-1 Reactive Metals: The s-block Elements

Alkali Metals

• Properties:

• Shiny solids that are malleable, ductile, and good

conductors of electricity.

• Low density and low melting points.

• Very soft and can be cut with a knife.

• Very reactive and tarnish rapidly with exposure to

oxygen in the air.

• Single valence electron causes reactivity with

moisture which increases down the group.

Alkali Metals: Sources and Uses

• All alkali metals react with halogens (7A): ex. NaCl

• Alkali metals = 1 valence electron

• Halogens = 7 valence electrons

• Create a full outer electron shell

• Sources:

• Alkali metals are never found in an elemental state in

nature because they are very reactive.

• Compounds made with alkali metals are very soluble

in water

• Common compounds: table salt (NaCl), Lye (NaOH),

bleach (NaClO), baking soda (NaHCO3)

Alkaline Earth Metals: Properties

• Group 2A = 2 valence electrons

• React strongly with group 6A Oxygen group

• Also react with halogens to form compounds (MgCl2)

• Not quite as reactive as the alkali metals but are still

considered reactive.

• Higher densities and melting points than alkali metals.

• Alkaline earth metals will form ions with a 2+ charge

Alkaline Earth Metals: Sources and Uses

• Because of reactivity, they are not found in an elemental

state in nature.

• They can be found in compounds such as limestone

(CaCO3) and magnesite (MgCO3)

• Alloy: when one metal is added to another metal.

• Alloys of magnesium and aluminum is an important

structural metal.

• Used to make aircraft, tools and car rims.

• Light and strong

• Beryllium is slightly different: strong and high melting

point – component of emeralds.

6-2 Transition Metals: the d-block Elements

• These elements are located in the middle of the periodic

table.

• Composed of groups 1B- 8B

• Transition metal properties:

• High densities and high melting points

• Strong and structurally useful

• Other properties vary across the periodic table

• Important transitional metals include Chromium, Iron,

Copper, Silver and Gold

6-2 Transition Metals: the d-block Elements

Chromium

• Source: found in deposits located in

Russia, the Phillipines, and southern

Africa.

• Properties: hard, silvery metal that is

very resistant to corrosion (reaction

with water, oxygen or acids)

• Uses:

• Forms many useful alloys: ex.

Stainless steel

• Compounds with chromium exhibit a

wide range of colors: ex.

Gemstones, paint pigments

Iron

• Source:

• 4th most abundant element found in the Earth’s crust.

• Usually found as rust (Fe2O3) because of its reactivity

to oxygen

• Properties: Produces alloys that are strong, durable and

resistant to corrosion.

• Uses:

• Forms compounds that are red in color

• Iron attaches to hemoglobin and carries oxygen

throughout the body.

Coinage Metals: Gold, Silver and Copper

• Sources:

• Found in compounds and elemental states in nature.

• Properties: resistant to corrosion, shiny and malleable

• Uses: Used throughout history to make coins, wires and

strong alloys (bronze) to make weapons

Copper, Silver and Gold

• Copper: soft metal used to make bronze.

• Slightly resistant to corrosion but will react with

oxygen and CO2 to create a patina (greenish coating).

• Silver: lustrous, white metal that is very ductile and

malleable.

• Used in coinage, jewelry, silverware and wiring.

• Silver will react with sulfide ions to create a tarnish.

• Gold: dense, soft, yellow metal.

• Usually found in an alloy because it is so soft.

• Used in jewelry and coinage.

6-3 Inner Transition Metals: the f-block

Elements

• Composed of the Lanthanides and Actinides.

• Located at the bottom of the periodic table, detached

from the other groups.

• These elements belong between the s- and d- block

elements.

• Electron configurations of f-block elements are

complicated and do not follow a regular pattern.

6-3 Inner Transition Metals: the f-block

Elements

Lanthanides

• Source: Widely distributed in nature but are found

together because their properties are so similar.

• Properties:

• Form 3+ ions

• Soft, silvery metals

• Too reactive to be used in structural materials.

• Uses: making special steel alloys and compounds that

create the color in televisions

Actinides

• Source: Found in nature and man-made

• Properties: Often radioactive

• Common elements: Uranium and Thorium

• Uses: fuel for nuclear power plants and other radioactive

processes.