kJ mol-1. The elements of the group contain an s-electron in the outer electron shell. Elements in group seven have a number of similar properties, most importantly they have low melting and boiling … These elements are called salt producers because chlorine, bromine, and iodine are highly electronegative in nature and form anions that constitute the anionic part of salts found in the seawater. The word "alkali" is derived from an Arabic word meaning "ashes". The remaining elements in period 3 do not conduct electricity. These structures are shown below: Aside from argon, the atoms in each of these molecules are held together by covalent bonds. Members of this group include: Unless otherwise noted, LibreTexts content is licensed by CC BY-NC-SA 3.0. Missed the LibreFest? Because of the two different types of bonding in silicon and aluminum, it makes little sense to directly compare the two melting and boiling points. When period 3 elements are reacted with chlorine gas the chlorides X-Cl1-5 are produced in the order Na, Mg, Al, Si, and P. The sodium and magnesium chlorides are ionic structures which have high boiling points. By integrating these comprehensive worksheets into your KS3 Chemistry lessons you can reinforce learning with confidence. Ionization Energy. Aluminium also reacts violently with Iron (III) oxide to produce Iron in the Thermit process. It covers ionization energy, atomic radius, electronegativity, electrical conductivity, melting point and boiling point. They are called s-block elements because their highest energy electrons appear in the s subshell. In sodium, only one electron per atom is involved in the metallic bond, the single 3s electron. Their melting or boiling points are lower than those of the first four members of the period which have complex structures. The diagram below shows how atomic radius changes across Period 3. Compare this with the coloured compounds of most transition metals. Magnesium and aluminum are each 12-coordinated, and therefore packed more efficiently, creating less empty space in the metal structures and stronger bonding in the metal. \n . The structures of the elements vary across the period. The general trend towards smaller atoms across the period is not broken at argon. Across Period 3 of the Periodic Table, the 3s and 3p orbitals fill with electrons. The first ionization energy is the energy required to remove the most loosely held electron from one mole of gaseous atoms to produce 1 mole of gaseous ions each with a charge of +1. Elements that show tripositive ions with electronic configuration of a noble gas (scandium, yttrium, lanthanum, actinium) show a clear trend in their physical properties, such as hardness. As we move down the group (from Li to Fr) we find the following trends: All have a single electron in an 's' valence orbital Apart from boron, the rest of the group 3 elements are poor metals. No group 3 element has any documented biological role in living organisms. gain electrons more readily and increase in nonmetallic character. Legal. The chemical properties of the elements of Group 3 reflect the increasingly metallic characteristics of descending members of the Group. Group 17 elements are also known as: (a) halogens (2) (name still in common use) (b) Group VIIA (name no longer used) Group 17 elements are non-metals; Group 17 elements exist as diatomic molecules (X 2) when not combined with other elements. Crystal_Lee460. Let us now look at some of the trends of atomic properties of these elements. (3) Both group 1 and group 2 elements produce white ionic compounds. And atomic radii as one moves from top to bottom the elements, the ionic,. 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