An element of group 14 has an atomic number of 14 . State whether this element will have metallic properties or not. (2024)

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An element of group 14 has an atomic number of 14 . State whether this element will have metallic properties or not.? ›

Silicon has 14 electrons and its electron configuration is 2,8,4. Losing or gaining 4 electrons to gain octet is equally difficult for Si. Hence it is classified as a metalloid. It does exhibit some metallic properties but also exhibits non-metallic properties.

Silicon, represented by the symbol 'Si', is a chemical element with the atomic number 14. This places it in group 14 (IV-A) and period 3 of the periodic table, among other metalloids—a class of elements with properties in between those of metals and nonmetals.

Silicon is a chemical element; it has symbol Si and atomic number 14.

Although tin has an even more metallic character than germanium, lead is the only element in the group that behaves purely as a metal.

Physical properties of group 14 elements

Melting and boiling points: Carbon, silicon and germanium have extremely high melting and boiling points because of their stable structures. The inner pair effect causes tin and lead to have lower boiling points as they can form only two bonds instead of four.

Silicon has 14 electrons and its electron configuration is 2,8,4. Losing or gaining 4 electrons to gain octet is equally difficult for Si. Hence it is classified as a metalloid. It does exhibit some metallic properties but also exhibits non-metallic properties.

The carbon family consists of one nonmetal (carbon), two metalloids (silicon and germanium), and two metals (tin and lead).

Silicon is a chemical element with symbol Si and atomic number 14. Classified as a metalloid, Silicon is a solid at room temperature.

Group 14 is the carbon family. The five members are carbon, silicon, germanium, tin, and lead.

Aluminum has an atomic number and is a good heat and electrical conductor. In nature, it is hard, ductile, malleable, and lustrous with a high melting and boiling point. Hence it is considered as a metal.

What is the metallic element in Group 14? ›

Metallic properties increase down the group. Carbon is a non-metal, silicon and germanium are metalloids, and tin and lead are poor metals (they conduct heat and electricity less effectively than other metals such as copper).

carbon is least metallic because metallic character increases down the group due to increase in size of atom and metallic character decreases along the period due to decrease in atomic radii.

The metallic character of group 14 elements increases from top to bottom because removal of electron becomes easier on moving down the group.

Among the Group 14 elements, carbon (C) is a typical nonmetal, silicon (Si) and germanium (Ge) are classified as metalloids or semimetals, while tin (Sn) and lead (Pb) are metals, exhibiting metallic properties such as malleability and electrical conductivity.

Because group 14 elements contain 4 electrons in their valence shell i.e. half-filled shell which is stable too. Now it is difficult to remove 4 electrons or to add 4 electrons to attain the next noble gas configuration. hence, it doesn't form ions instead they form a covalent bond.

(b)The elements of group 14 have 4 valence electrons. Therefore, the oxidation state of the group is +4. However, as a result of the inert pair effect, the lower oxidation state becomes more and more stable and the higher oxidation state becomes less stable. Therefore, this group exhibits +4 and +2 oxidation states.

Carbon is a chemical element with the symbol C and atomic number 6. It is nonmetallic and tetravalent-making four electrons available to form covalent chemical bonds. It belongs to group 14 of the periodic table.

Group 14 elements have 4 valence electrons in their outer shell. The lighter of these elements can form both cations with a +4 charge, and anions with a -4 charge.

Silicon. Silicon (symbol Si) is a group 14 metalloid. It is less reactive than its chemical analog carbon, the nonmetal directly above it in the periodic table, but more reactive than germanium, the metalloid directly below it in the table.