Why some are metals and some are nonmetals?

Answer 1

Metals fill the s, d, and f orbitals. Nonmetals only fill the p orbitals thus giving us more metals on the table of elements. The greater question is why is this so? complicated answer but I will give it a try. Electron attraction to the nucleus obeys the inverse square as is evident in Coulomb's law. As the electron move away from the nucleus by the addition of shells (energy levels) the "pull" it feels to the nucleus drops off as a square of the distance. This means the electron's drop in attraction is an exponential drop. Draw yourself an exponential graph, with the greatest attraction at the top, quickly dropping off toward zero. At the top of the graph (left of the table you drew) are the nonmetals who feel a strong attraction toward the nucleus and so behave as nonmetals. Notice in the graph this represents very few elements along the X-axis. The bulk of elements fall beneath this.................exponentially............s, d, and f blocks flow sorta exponentially away from the nucleus. Leaving the few elements in the p block to behave as nonmetals.

Answer 2

All chemicals elements are contained in the Periodic Table. This table arranges the elements according to their electronic structure. One of the clearest ways to define elements is whether they are metals or non metals. What is the difference? How can we define a metal or a non-metal?

Hard and Shiny?Most people would say that metals are shiny and hard. Some would mention that metals conduct electricity. When you think about metals, however, you soon realise that metals are quite different from one another. Iron is a hard shiny metal. Mercury is a liquid. Lead is a dull grey and easy to bend. Copper is a coppery colour! Poisonous Gases?Non-metals, too, are very different from one another. Some are colourless gases like oxygen or nitrogen. Chlorine is a green gas and poisonous. Carbon has more than one form. Sulphur is a yellow solid. Chemists need to work out what properties put elements in one or other of these categories. Periodic TableA look at the Periodic Table helps with these problems. The metals are all on the left-hand side of the periodic table and in the transition metals section in the middle. To the right of the transition metals a line in the form of steps can be drawn, beginning between boron and aluminum and going down between silicon and germanium and so on. Metal PropertiesMetals in the form of elements are usually good conductors of electricity, are flexible and strong. When they are combined with oxygen to form oxides, they are alkaline compounds. When combined with chlorine to form chlorides they form ionic compoundswhich have giant structures. Non-Metal PropertiesNon-metals as elements are rarely solids, usually they are gases. They are poor conductors of electricity except graphitewhich has a special structure. Their oxides are often gases and are acidic. Their chlorides are covalently bonded and solids or liquids. Electronic ExpalantionThese properties can be simply explained by considering the electronic structure of the atoms of these elements. Metals, on the left hand side of the periodic table, have few electrons in the outer shell. This lends itself to what is called metallic bonding in which many atoms of the elements share their outer electrons in a delocalised cloud which makes a hard structure which conducts electricity. Non-metals have outer electron shells which are nearly full. This means that small numbers of atoms bond covalently to form small molecules which usually are gases. Shared ElectronsAgain, combined with oxygen and chlorine, metals lose electrons and become positive ions, leading to alkaline oxides and ionic chlorides. Non-metals have to share electrons to fill their outer shell and so form small covalently bonded molecules with oxygen and chlorine which again are often gases or liquids.

The classification of elements into metal and non-metal groups is a useful exercise and helps a great deal in understanding the properties of different elements and compounds.

Answer 3

This is a difficult question. It relates to the fuundamental principle of forming a bond which is overlap of orbitals and the population of the molecular orbitals that result. Most elements have orbitals that do not project too far and do not have large numbers of electrons able to partake in bonding. This favours the formation of metallic bonds which are typified by high coordination numbers and partially filled "energy levels" giving rise to electrical conduction. The 2d period elements that are best known in organic chemistry, groups 14-18 have nicely projecting orbitals tand a reasonable number of electrons to populate bonding orbitals which are required to form discrete molecules. As you go down a group the projection is less and the elements get more metallic in nature.

Answer 4

There are more metallic elements than nonmetallic elements due to the configuration of their electrons. Metallic elements are also more likely to lose their electrons to form bonds.

Answer 5

Because many elements are metals and no one can explain. Why don't you ask God?

Answer 6

Nickel, copper, gold, silver are the commonest but just about all the metals have been used somewhere at some time or other.

Answer 7

Metals and nonmetals are equally important. Carbon, phosphorus, oxygen, nitrogen and sulfur are all nonmetals, and life can't exist without them.

Answer 8

Because they have the characteristics of metals: luster, malleability, ductility, ability to conduct heat and electricity.