The three divisions for the type of bonding are Ionic, Covalent, and Metallic.

The Ionic bond means that electorons are completly transferred from one atom to another. During this it is either gaining or losing negativly charged electrons. The oppisitly charged ions are attracted to each other by electrostatic forces which makes up Ionic Bonding. They form between nonmetals and metals, ionic componds dissolve easily in water, they can easily conduct electricity, and usually for crystalline structures with a high melting point. Some examples of ionic bonds include Table Salt, Calcium Chloride, Magnessium Oxide, and Potassium Bromide.

The Covalent bond is a chemical formed by sharing one or more electrons. Covalent bonding does not require two atoms to be the same element, but they have to compare with electronegativty. The stength of covalent bonds depends on the angular relation between atoms in polyatomic molecules. Some examples of Covalent bonds are Carbon, Carbon to hydrogen, and hydrogen to oxygen.

In a Metallic bond the atom has a more stable configuration by sharing the electrons in the in its outer shell. They happen in in elements in which the valence electrons are not tightly bound with the nucleus, mainly metals. They have to ability to conduct heat and electricity very easily. Some exapmles include Zinc, Copper, Tin, Aluminum, and Gold.

Alyssa Cadena

The Three Chemical Bonds-Cal Hatton

A bond is formed when electrons from two atoms interact with each other and their atoms become joined. The electrons that interact with each other are VALENCE ELECTRONS, the ones that reside in the outermost electron shell of an atom. There are two main types of bonding discussed here. A COVALENT BOND results when two atoms "share" valence electrons between them. Covalent bonds involve a complete sharing of electrons and occurrs most commonly between atoms that have partially filled outer shells or energy levels. Thus if the atoms are similar in negativity then the electrons will be shared. Carbon forms covalent bonds. The electrons are in hybrid orbitals formed by the atoms involved as in this example: ethane. Diamond is strong because it involves a vast network of covalent bonds between the carbon atoms in the diamond. An IONIC BOND occurs when one atom gains a valence electron from a different atom, forming a negative ion (ANION) and a positive ion (CATION), respectively. These oppositely charged ions are attracted to each other, forming an ionic bond. Ionic bonds arise from elements with low electronegativity(almost empty outer shells) reacting with elements with high electronegativity (mostly full outer shells). In this case there is a complete transfer of electrons. A well known example is table salt, sodium chloride. Sodium gives up its one outer shell electron completely to chlorine which needs only one electron to fill its shell. Thus, the attraction between these atoms is much like static electricity since opposite charges attract. 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.

Emily Jaska

There are 3 different types of bonds: Covalent bonds, Ionic bonds, and

Covalent Bonds:

Covalent bonding is a form of chemical bonding characterized by the sharing of one or more pairs of electrons between atoms, in order to produce a mutual attraction, which holds the resultant molecule together. Atoms tend to share electrons in such a way that their outer electron shells are filled. Such bonds are always stronger than the intermolecular hydrogen bond and similar in strength to or stronger than the ionic bond.

Characteristics of Covalent Bonds:

• Covalent molecules exist as true molecules.
• Formed between two or more nonmetals.
• Covalent bonds usually have low melting points.
• The molecules in the bonds are not strongly attracted to each other and can move freely about in the physical states of matter such as solid, liquid, or gas.

Ionic Bonds:

Electrostatic attraction between oppositely charged ions in a chemical compound. Such a bond forms when one or more electrons are transferred from one neutral atom (typically a metal, which becomes a cation) to another (typically a nonmetallic element or group, which becomes an anion). The two types of ion are held together by electrostatic forces in a solid that does not comprise neutral molecules as such; rather, each ion has neighbours of the opposite charge in an ordered overall crystalline structure.

Characteristics of Ionic Bonds:

• In solutions ionic bonds easily conduct electricity.
• Bonds formed between metal and nonmetal.
• Dissolve easily in water and other polar solvents.

Metallic Bond:

Most metallic elements contain only one to three electrons in the outer shell. When an element has only one, two or three valence electrons, the bond between these electrons and the nucleus is weak. Sometimes an electron cloud can be formed; in this arrangement, the valence electrons have considerable mobility and are able to conduct heat and electricity easily. Also, the delocalized nature of the bonds, make it possible for the atoms to slide past each other when the metal is deformed instead of fracturing like glass or other brittle material.

Characteristics of Metallic Bonds:

• Conduct heat and electricity
• Ductile and malleable

Dane Lovejoy

There are 3 different types of chemical bonding.

1. Ionic-

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.

Characteristics of Ionic Bonds:

• In solutions ionic bonds easily conduct electricity.
• Bonds formed between metal and nonmetal.
• Dissolve easily in water and other polar solvents.

2. Covalent-

When atoms share - 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. This 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 .

Characteristics of Covalent Bonds:

• Covalent molecules exist as true molecules.
• Formed between two or more nonmetals.
• Covalent bonds usually have low melting points.
• The molecules in the bonds are not strongly attracted to each other and can move freely about in the physical states of matter such as solid, liquid, or gas.

3. Metallic-

In the metallic bond, an atom achieves a more stable configuration by sharing the electrons in its outer shell with many other atoms. Metallic bonds prevail in elements in which the valence electrons are not tightly bound with the nucleus, namely metals, thus the name metallic bonding. In this type of bond, each atom in a metal crystal contributes all the electrons in its valence shell to all other atoms in the crystal.

Characteristics of Metallic Bonds:

• Conduct heat and electricity
• Ductile and malleable

Andy Sanchez

There 3 main types of divisions for bonding. There is ionic bonds, covalent bonds, and metallic bonds.
Ionic Bonds-
An ionic bond is a bond with an element with a positive and negative charge usually a metal and nonmetal. Anions are atoms with negative charges .Cations are atoms with positive charge . In ionic bonding the electrons are transferred from one atom to the other by either gaining or losing electrons; the purpose of the elements gaining or losing electrons is so that they can have a full octet like that of a noble gas. Group 1 to 3 will lose electrons and groups 5 to 7 will gain electrons. The oppositely charged atoms are attracted by electrostatic forces.
Covalent Bonds-
Covalent Bonds share electrons this type of bond can occur between two or more elements share electrons. A covalent bond occurs because the elements in the compound have similar tendencies for electrons usually to gain electrons. The most common thing for a covalent bond is when two nonmetals come together to bond because the nonmetals will want to gain electrons; therefore, the elements will share their electrons to fill the orbital.
Metallic bonds-
Metallic bonding is the electromagnetic interaction between delocalized electrons, called conduction electrons, and the metallic nuclei within the metals they gather in the “electronic sea”. Zinc and copper is an example of metallic bond that forms brass because of the negative charge of the electronic cloud pull on the positive atoms causing them to form a metallic bond. The electronic cloud moves freely in a direction and when voltage is applied an electronic current is formed where thermal energy is released allowing this to bond a good conductor of heat.

Mat Groh

Ionic

Ionic bonding occurs between charged particles, metal atoms and nonmetal atoms. Metals usually have 1, 2, or 3 electrons in their outermost shell. Nonmetals have 5, 6, or 7 electrons in their outer shell. Atoms with outer shells that are only partially filled are unstable. To become stable, the metal atom wants to get rid of one or more electrons in its outer shell. Losing electrons will either result in an empty outer shell or get it closer to having an empty outer shell. It would like to have an empty outer shell because the next lower energy shell is a stable shell with eight electrons.

Covalent

Where a compound only contains nonmetal atoms, a covalent bond is formed by atoms sharing two or more electrons. Nonmetals have 4 or more electrons in their outer shells (except boron). With this many electrons in the outer shell, it would require more energy to remove the electrons than would be gained by making new bonds. Therefore, both the atoms involved share a pair of electrons. Each atom gives one of its outer electrons to the electron pair, which then spends some time with each atom. Consequently, both atoms are held near each other since both atoms have a share in the electrons.

Metallic

Most metallic elements contain only one to three electrons in the outer shell. When an element has only one, two or three valence electrons, the bond between these electrons and the nucleus is weak. Sometimes an electron cloud can be formed; in this arrangement, the valence electrons have considerable mobility and are able to conduct heat and electricity easily. Also, the delocalized nature of the bonds, make it possible for the atoms to slide past each other when the metal is deformed instead of fracturing like glass or other brittle material.

Cole Payne


There are three different types of chemical bonds. They are as follows: Covalent, Ionic, and Metallic.

1. Covalent Bonds -
Covalent chemical bonds involve the sharing of a pair of valence electrons by two atoms and these covalent bonds lead to stable molecules if they share electrons in a way to create a noble gas configuration for each atom. Covalent bonding can be shown through the Lewis Dot System. However, covalent bonds in which the sharing of the electron pair is unequal, with the electrons spending more time around the more nonmetallic atom, are called polar covalent bonds. Covalent bonded chemicals have low melting and boiling points, they cannot conduct electricity, and they are not soluble. Covalent bonds usually happen between nonmetals.
Examples can be: Hydrogen, Nitrogen, Oxygen, and Chlorine… As well as many others.

2. Ionic Bonds -
In chemical bonds, atoms can transfer or share valence electrons. In the event where one or more atoms loses electrons and other atoms gain them in order to produce a noble gas electron configuration, the bond is called an ionic bond. Ionic bonds contain positive and negatively charged ions. Ionic bonds can also be displayed through the Lewis Dot System. When chemicals bond ionically, they form a negative ion (Anion) and a positive ion (Cation), depending on the amount of valence electrons either lost or gained. Characteristics ionic bonded chemicals have are high melting points, the ability to conduct electricity, easily soluble, and they have well-defined crystals.Examples are: Most alkali halides such as sodium chloride, NaCl.

3. Metallic Bonds -
Metallic bonds are formed when two metallic atoms share valence electrons. As the name hints, metallic bonds are formed between metals. Metallic bonded substances have the ability to easily conduct heat and electricity. They are also ductile and malleable. Valence electrons are able to freely move around the metallic substance.
Examples are: Zinc, Copper, Aluminum, Tin, Gold