Briana Lina

The three types of bonds are ionic, covalent(nonpolar and polar), and metallic bonding.

In ionic bonding, electrons are completely transferred from one atom to another. In the process of either losing or gaining negatively charged electrons, the reacting atoms form ions. The oppositely charged ions are attracted to each other by electrostatic forces, which are the basis of the ionic bond. The second major type of atomic bonding occurs when atoms share electrons. As opposed to ionic bonding in which a complete transfer of electrons occurs, covalent bonding occurs when two (or more) elements share electrons. Covalent bonding occurs because the atoms in the compound have a similar tendency for electrons (generally to gain electrons). This most commonly occurs when two nonmetals bond together. Because both of the nonmetals will want to gain electrons, the elements involved will share electrons in an effort to fill their valence shells. A good example of a covalent bond is that which occurs between two hydrogen atoms.There are, in fact, two subtypes of covalent bonds. The H2 molecule is a good example of the first type of covalent bond, the nonpolar bond. Because both atoms in the H2 molecule have an equal attraction (or affinity) for electrons, the bonding electrons are equally shared by the two atoms, and a nonpolar covalent bond is formed. Whenever two atoms of the same element bond together, a nonpolar bond is formed. A polar bond is formed when electrons are unequally shared between two atoms. Polar covalent bonding occurs because one atom has a stronger affinity for electrons than the other (yet not enough to pull the electrons away completely and form an ion). In a polar covalent bond, the bonding electrons will spend a greater amount of time around the atom that has the stronger affinity for electrons. A good example of a polar covalent bond is the hydrogen-oxygen bond in the water molecule. There is a third type of bonding, called metallic bonding. As the name implies, metallic bonding usually occurs in metals, such as copper. A piece of copper metal has a certain arrangement of copper atoms. The valence electrons of these atoms are free to move about the piece of metal and are attracted to the positive cores of copper, thus holding the atoms together.

The three divisions of bonds that occur: Covalent, ionic, and metallic bonds. A covalent bonds a chemical bond that involves sharing a pair of electrons between atoms in a molecule. A metal plus a nonmetal can form a covalent bond. They are nuetral molecules which do not conduct electricity, and have low melting and boiling points. A few examples of covalent bonds are HCl, SO2, and CO2. An ionic bond is a chemical bond in which one atom loses and electron to form a positive ion and the other atom gains an electron to form a negative ion. They are easily polar, conductable to electricity, have high melting points, dissolve easily in water, and have well-defined crystals. One atom has a high electronegativity vaule, while the other is relatively low; and one atom is a metal, while the other is nonmetal. An example of an ionic bond is magnesium oxide. Metallic bonds are the electromagnetic interaction between delocalized electrons, and the metallic nuclei within metals. Metallic bonding accounts for many physical properties of metals such as strength, malleability, ductility, thermal and electrical conductivity, opacity, and luster. An example of a metallic bond is the mercurous ion (Hg2+2).

There are 3 different types of bonds. There are ionic bonds, covalent bonds, and metallic bonds.
In ionic bonds an atom loses an electron to form a positive ion and the other atom gains an electron to form a negative ion. An example is magnesium oxide. There are two different types of ionic bonds. They are cations and anions. A cation is an atom or group of atoms with a positive charge. An anion is any amtom or group of itoms that a have negative charge. Some characteristic of ionic bonds are: they have high melting points, they can conduct electricty, they dissolve in water, and they have well defined crystals. They attract by electrostatic forces. Usually ionic bonds are metals. The next type of bond is Covalent bonds. Covalent bonds share a pair of elctrons between atoms in a molecule (non-metals). An example is hydrogen chloride. There is one type of covalent bonding and it is polar covalent. Polar covalent simply means its a chemical bond that unequally shares electrons but one side is positive while the other is negative. An example of this is water. Some characteristics of covalent bonds are: they are neutral, do not conduct electricty, and low melting and boiling points. The next type of bonding is a metallic bond. A metallic bond is a chemical bond in which electrons are shared over many nuclei and electronic conduction occurs. An example is copper.

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There are three divisions for the types of bonds that occur. Explain the three types of bonds and their characteristics. Then explain the reason for their characteristics by use of concepts such as ,metal, nonmetal, metalloid as well as forces of bonding (notice i did not give you the name for that). Make sure that you explain all the characteristics and you give examples.