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Metals are good conductors of heat and electricity, and are malleable they can be hammered into sheets and ductile they can be drawn into wire. Most of the metals are solids at room temperature, with a characteristic silvery shine except for mercury, which is a liquid.
Nonmetals are usually poor conductors of heat and electricity, and are not malleable or ductile; many of the elemental nonmetals are gases at room temperature, while others are liquids and others are solids.
The metalloids are intermediate in their properties. In their physical properties, they are more like the nonmetals, but under certain circumstances, several of them can be made to conduct electricity.
These semiconductors are extremely important in computers and other electronic devices.
On many periodic tables, a jagged black line see figure below along the right side of the table separates the metals from the nonmetals. The metals are to the left of the line except for hydrogen, which is a nonmetalthe nonmetals are to the right of the line, and the elements immediately adjacent to the line are the metalloids.
When elements combine to form compounds, there are two major types of bonding that can result. Ionic bonds form when there is a transfer of electrons from one species to another, producing charged ions which attract each other very strongly by electrostatic interactions, and covalent bonds, which result when atoms share electrons to produce neutral molecules.
In general, metal and nonmetals combine to form ionic compounds, while nonmetals combine with other nonmetals to form covalent compounds molecules.
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Since the metals are further to the left on the periodic table, they have low ionization energies and low electron affinitiesso they lose electrons relatively easily and gain them with difficulty. They also have relatively few valence electrons, and can form ions and thereby satisfy the octet rule more easily by losing their valence electrons to form positively charged cations.
The main-group metals usually form charges that are the same as their group number: The metals which follow the transition metals towards the bottom of Groups 4A and 5A can lose either their outermost s and p electrons, forming charges that are identical to their group number, or they can lose just the p electrons while retaining their two s electrons, forming charges that are the group number minus two.
Most of the transition metals can form more than one possible charge in ionic compounds. Nonmetals are further to the right on the periodic table, and have high ionization energies and high electron affinitiesso they gain electrons relatively easily, and lose them with difficulty.
They also have a larger number of valence electrons, and are already close to having a complete octet of eight electrons.
The nonmetals gain electrons until they have the same number of electrons as the nearest noble gas Group 8Aforming negatively charged anions which have charges that are the group number minus eight. That is, the Group 7A nonmetals form 1- charges, the Group 6A nonmetals form 2- charges, and the Group 5A metals form 3- charges.
The Group 8A elements already have eight electrons in their valence shells, and have little tendency to either gain or lose electrons, and do not readily form ionic or molecular compounds. Ionic compounds are held together in a regular array called a crystal lattice by the attractive forces between the oppositely charged cations and anions.
These attractive forces are very strong, and most ionic compounds therefore have very high melting points. Ionic compounds are typically hard, rigid, and brittle. Ionic compounds do not conduct electricity, because the ions are not free to move in the solid phase, but ionic compounds can conduct electricity when they are dissolved in water.
When nonmetals combine with other nonmetals, they tend to share electrons in covalent bonds instead of forming ions, resulting in the formation of neutral molecules. Keep in mind that since hydrogen is also a nonmetal, the combination of hydrogen with another nonmetal will also produce a covalent bond.
Molecular compounds can be gases, liquids, or low melting point solids, and comprise a wide variety of substances. See the Molecule Gallery for examples. When metals combine with each other, the bonding is usually described as metallic bonding you could've guessed that.
In this model, each metal atom donates one or more of its valence electrons to make an electron sea that surrounds all of the atoms, holding the substance together by the attraction between the metal cations and the negatively charged electrons. Since the electrons in the electron sea can move freely, metals conduct electricity very easily, unlike molecules, where the electrons are more localized.
Metal atoms can move past each other more easily than those in ionic compounds which are held in fixed positions by the attractions between cations and anionsallowing the metal to be hammered into sheets or drawn into wire.
Different metals can be combined very easily to make alloys, which can have much different physical properties from their constituent metals. Steel is an alloy of iron and carbon, which is much harder than iron itself; chromium, vanadium, nickel, and other metals are also often added to iron to make steels of various types.
Brass is an alloy of copper and zinc which is used in plumbing fixtures, electrical parts, and musical instruments. Bronze is an alloy of copper and tin, which is much harder than copper; when bronze was discovered by ancient civilizations, it marked a significant step forward from the use of less durable stone tools.The principles and their application for the synthesis of some of the naturally occurring compounds will be described in this note.
Major topics covered includes: Formation of Aliphatic Carbon-Carbon Bonds: Base Catalyzed Reactions and Acid Catalyzed Reactions, Organometallic Reagents, Nucleophilic Aromatic Substitution, Aromatic Diazonium Salts, Molecular Rearrangements, eagents Containing.
Chemical compound, any substance composed of identical molecules consisting of atoms of two or more chemical elements..
All the matter in the universe is composed of the atoms of more than different chemical elements, which are found both in pure form and combined in chemical compounds.A sample of any given pure element is composed only of the atoms characteristic of that element, and .
with ionic compounds called solutes and dissolve them. Negative oxygen regions of polar water molecules are attracted to sodium cations (Na+). + + +. If you use this Internet site regularly and if you don't feel the need for the printed textbook, I ask that you pay $20 for using the electronic text and tools on this site.
Ionic compounds are between metals and non-metals. Molecular (covalent) compounds are between only non-metals.
(Metallic compounds are between metals and other metals.) An ionic compound is a pure. Molecular solids are mild compared to ionic compounds, although the latter is a little more fragile and susceptible to breakage.
Because the covalent bond is much weaker than the ionic bond, the molecular compounds change state to the liquid or gas at low temperatures.