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The reaction of group 2 metals with oxygen follows the following general equation: 2M (s) + O2 (g) → 2MO (s) Where M is any metal in group 2. We can see this is a redox reaction by looking at the changes in oxidation number of the metal, M, and oxygen. M = 0 → +2 so the metal has been oxidised. O = 0 → -2 so the oxygen has been reduced.
Group 2 Reactivity. As a result of the deceases in ionisation energy, the elements become more reactive going down the group as it gets easier for the atoms to lose two electrons and become 2+ ions. This trend is shown by looking at reactions of the Group 2 metals: With dilute hydrochloric acid: bubbles of hydrogen gas are given off much faster ...
Group 2. Group 2 elements, known as alkaline-earth metals, include Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), and Radium (Ra). These elements are s-block elements as their outer electrons are in s-orbitals. Alkaline-earth metals have two electrons in their outermost s orbital.
CIE A-Level Chemistry Study Notes. 10.1.4 Physical and Chemical Trends in Group 2 Elements. Group 2 elements, commonly known as the alkaline earth metals, encompass Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), and Radium (Ra). These elements showcase distinct trends in their physical and chemical properties, which ...
Group 2 elements are s-block elements because their outermost electrons are in the s-orbital. They have two electrons in their outermost shell, leading to their tendency to lose two electrons in reactions to achieve a stable electron configuration. Group 2 elements are all metallic and shiny. They are generally harder than Group 1 metals, but ...
Medium. Hard. 1a 3 marks. i) State how many electrons a Group 2 element has in its outermost principal quantum shell. ii) State how a Group 2 element forms an ionic bond with nonmetals. iii) State whether Group 2 elements act as oxidising or reducing agents.
Solution: A The group 2 elements are in the s block of the periodic table, and as group 2 elements, they all have two valence electrons. Beginning with beryllium, we see that its nearest preceding noble gas is helium and that the principal quantum number of its valence shell is n = 2. B Thus beryllium has an [He] s2 electron configuration.
