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Properties of Groups

Properties of Groups. Chapter 7 part II. Metals, Nonmetals & Metalloids. Information from the Periodic Table. The number and type of valence electrons determine the group/chemical reactivity. From the periodic table one can determine the electron configuration.

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Properties of Groups

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  1. Properties of Groups Chapter 7 part II

  2. Metals, Nonmetals & Metalloids

  3. Information from the Periodic Table • The number and type of valence electrons determine the group/chemical reactivity. • From the periodic table one can determine the electron configuration. • Certain groups have specific names.

  4. Group IA • Alkali Metals • Valence electron is s1 • First ionization energy is low. • First ionization energy deceases as atomic radius increases. Why?

  5. Group 2A • Alkaline Earth Metals • Valence electrons are s2. • Higher first ionization energy than group 1A, but much lower second ionization energy.

  6. Group 3A • Group 3A • Form +3 ions upon ionization • Metals and semimetals aka metalloids.

  7. Ionic Compounds • How ionic or covalent a compound is depends on the placement of elements on the periodic table (hence their electron configuration). • Many covalent compounds have ionic characteristics and visa versa.

  8. Halogens • Group 7A, • Form -1 ions upon gaining an electron.

  9. Nobel Gases • Group 8A • Complete s2p6 shell • Tend not to form compounds and were formerly known as the 'inert gases.' • However, a few of them (most notably xenon) have been found to form compounds with fluorine.

  10. Diamagnetic • When all electrons are paired in an atom, ion, or compound - it is said to be diamagnetic and largely unaffected (very weakly repelled) by external magnetic fields. • Examples: • Beryllium

  11. Paramagnetic • When unpaired electrons exist, like the case for Li below, the material is termed paramagnetic and it is attracted to a magnetic field.

  12. This effect can be measured for various elements and compounds with an electrobalance as shown below

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