properties of all groups of elements in periodic table
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Explanation:
Alkali Metals:
-less dense than other metals
-one loosely bound valence electron
-highly reactive, with reactivity increasing -moving down the group
-largest atomic radius of elements in their period
-low ionization energy
-low electronegativity
Alkaline Earth Metals:
-two electrons in the valence shell
-readily form divalent cations
-low electron affinity
-low electronegativity
Transition Metals:
-The lanthanides (rare earth) and actinides are also transition metals. The basic metals are similar to transition metals but tend to be softer and to hint at nonmetallic properties. In their pure state, all of these elements tend to have a shiny, metallic appearance. While there are radioisotopes of other elements, all of the actinides are radioactive.
-very hard, usually shiny, ductile, and malleable
-high melting and boiling points
-high thermal and electrical conductivity
-form cations (positive oxidation states)
-tend to exhibit more than one oxidation state
-low ionization energy
Metalloids or Semimetals:
-electronegativity and ionization energy -intermediate between that of metals and nonmetals
-may possess a metallic luster
Nonmetals:
The halogens and noble gases are nonmetals, although they have their own groups, too.
-high ionization energy
-high electronegativity
-poor electrical and thermal conductors
-form brittle solids
-little if any metallic luster
-readily gain electrons
Halogens:
The halogens exhibit different physical properties from each other but do share chemical properties.
-extremely high electronegativity
-very reactive
-seven valence electrons, so elements from this group typically exhibit a -1 oxidation state
Noble Gases"
The noble gasses have complete valence electron shells, so they act differently. Unlike other groups, noble gasses are unreactive and have very low electronegativity or electron affinity.
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