Investigate the reactions of Group-2 elements
Title: Investigate the reactions of Group-2 elements.
Objective:
To be able to describe the redox reactions of Group-2 elements with oxygen and water
To be able to identify trends of reactivity down the Group-2
Equipment required:
2 x250 cm3 beaker
Funnel
2x boiling tubes
Crucible tongs
Calcium granules
Magnesium ribbon
Magnesium powder
Spatula
Universal Indicator
Thermal mat
Filter paper
Safety:
Wear eye protection.
Magnesium and calcium are highly flammable.
Calcium hydroxide is an irritant.
Group 2 elements
Calcium
Strontium
Magnesium
Beryllium
Barium
Radium
Introduction: The Group 2 elements are all metals with a shiny, silvery-white colour having 2 electrons in their outermost shell. The alkaline earth metals are high in the reactivity series of metals, but not as high as the alkali metals of Group 1. The metals of Group 2 are harder and denser than sodium and potassium, and have higher melting points. These properties are due largely to the presence of two valence electrons on each atom, which leads to stronger metallic bonding. In the nature, they are mainly found in their compounds and it is very difficult to separate its bonding with other elements. All react with halogens and, except for beryllium; with water and oxygen (magnesium at temperatures higher than those of living things) all oxidizes to the +2 state that represents an ion in the stable configuration of an inert gas. Beryllium is the least reactive; it is the hardest of these elements. Its oxide is amphoteric; it reacts with both strong acids and bases.
Atomic and ionic radii increase smoothly down the Group. The chemical properties of Group 2 elements are dominated by the strong reducing power of the metals. The elements become increasingly electropositive on descending the Group. All the metals except beryllium form oxides in air at room temperature which dulls the surface of the metal. Barium is so reactive it is stored under oil. All the metals
Objective:
To be able to describe the redox reactions of Group-2 elements with oxygen and water
To be able to identify trends of reactivity down the Group-2
Equipment required:
2 x250 cm3 beaker
Funnel
2x boiling tubes
Crucible tongs
Calcium granules
Magnesium ribbon
Magnesium powder
Spatula
Universal Indicator
Thermal mat
Filter paper
Safety:
Wear eye protection.
Magnesium and calcium are highly flammable.
Calcium hydroxide is an irritant.
Group 2 elements
Calcium
Strontium
Magnesium
Beryllium
Barium
Radium
Introduction: The Group 2 elements are all metals with a shiny, silvery-white colour having 2 electrons in their outermost shell. The alkaline earth metals are high in the reactivity series of metals, but not as high as the alkali metals of Group 1. The metals of Group 2 are harder and denser than sodium and potassium, and have higher melting points. These properties are due largely to the presence of two valence electrons on each atom, which leads to stronger metallic bonding. In the nature, they are mainly found in their compounds and it is very difficult to separate its bonding with other elements. All react with halogens and, except for beryllium; with water and oxygen (magnesium at temperatures higher than those of living things) all oxidizes to the +2 state that represents an ion in the stable configuration of an inert gas. Beryllium is the least reactive; it is the hardest of these elements. Its oxide is amphoteric; it reacts with both strong acids and bases.
Atomic and ionic radii increase smoothly down the Group. The chemical properties of Group 2 elements are dominated by the strong reducing power of the metals. The elements become increasingly electropositive on descending the Group. All the metals except beryllium form oxides in air at room temperature which dulls the surface of the metal. Barium is so reactive it is stored under oil. All the metals