Chem Bonding Essay PDF

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Sofia Ferreira Mr. Baruch Chemistry: Bonding Essay December 14th, 2016 A chemical bond is a lasting attraction between atoms that enables the formation of chemical compounds. The bond may result from a transfer of electrons between metals and nonmetals with opposite charges or through the sharing of electrons between covalent bonds. There can be single(1 pair of electrons), double(2 pairs of electrons), or triple bonds(3 pairs of electrons). The reason for bonding is that all atoms want to stabilize and lower their energy. Atoms can either bond through Intramolecular Bonding or Intermolecular Bonding. Intramolecular Bonding is the bonding between atoms within molecules. There are two types of Intramolecular Bonding: covalent bonding and ionic bonding. A chemical bond results from the sharing of electrons between atoms is known as covalent bonding. Compounds that have Covalent bonds have low melting points, can be either solids, liquids or gases, they are nonconductive, and have no ions. This type of bonding exists between nonmetals. There are three types of covalent bonding; polar, nonpolar, and coordinate covalent. Polar covalent bonding is a type of chemical bond where a pair of electrons is unequally shared between two atoms. Nonpolar covalent bonds are a type of chemical bond where two atoms equally share a pair of electrons with each other. A coordinate covalent bond is a chemical bond between two atoms that is produced when one atom shares a pair of electrons with another atom lacking such a pair. A chemical bond resulting from electrostatic attractions between positive and negative ions is known as ionic bonding. Ionic bonds have high melting points, conduct when they are melted or dissolved, appear to be crystal, brittle, hard, and “salt-like”. This type of bonding exists between

metals and nonmetals. The other form of bonding is known as Intermolecular Bonding or the “Attractive Forces”, which is the bonding between molecules. One type of intermolecular bonding is known as Dipole-dipole attraction. Dipole-dipole attractions are the forces of attraction between polar molecules caused by the attraction of the negative ends of molecules to the positive ends of other molecules of the same type. Another type of intermolecular bonding is known as Hydrogen bonding which is the attraction between a hydrogen atom and an unshared pair of electrons on a strong electronegative atom. Hydrogen bonds have very high boiling points and have very strong attractions. The last type of intermolecular bonding is known as Van der Waals forces or “London Forces” which is the attraction between nonpolar molecules. These forces increase with increasing atomic number. In general, these are considered to be the weakest of all the intermolecular forces. However, there are other attractive forces in substances that don’t form “molecular solids”. There are network solids which are covalently bonded atoms linked in a giant network. They have characteristics such as being hard, poor conductors, and extremely high melting points (unlike other covalently bonded substances). Examples of network solids are diamond and sand. Another attractive force is an ionic solid. Ionic solids are substances formed by the ionic attractions of ionic bonding between many ions. They have characteristics such as high melting points, very strong attractions, crystalline structures, and do not conduct electricity in a solid state, only in liquids or solutions. Another attractive force is through metallic bonds. Metallic bonds are the bonds between positive metal ions surrounded by a sea of mobile electrons. They have characteristics such as strong attractions(solids), and high electrical conductivity. The compound Carbon Monoxide, also known as CO, has an intramolecular force of polar

covalent triple bonds. These polar covalent bonds are also bonded together through dipole-dipole attractions. Polar covalent bonds are stronger than nonpolar bonds, however, they are weaker than ionic and metallic bonds. However, its dipole-dipole attractions are weak because it is a gas and a gas by definition is made up of weak bonds. Carbon Monoxide is not conductive due to the fact that it is a gas. Gases have no ions and ions are needed to conduct electricity so it is not conductive. Since Carbon Monoxide has such weak dipole-dipole attractions, it is a gas at room temperature, so therefore, it has a low boiling point. The compound Sodium Chloride, also known as NaCl, is made up of ionic bonds. It is an ionic solid that is held together by ionic bonds. The bonds in Sodium Chloride are very strong because it is very difficult to break positive-negative bonds. Although Sodium Chloride is a solid, and it is not a conductor of electricity in its solid state, if dissolved in water it will conduct because in order to conduct electricity you need moving ions. Sodium Chloride is a solid at room temperature and has a very high melting point due to its strong attractions. The substance Water, also known as H2O, is made up of polar covalent bonds. This molecule is also bonded through hydrogen bonding. Polar covalent bonds are stronger than nonpolar bonds, but they are far weaker than all other bonds. However, Hydrogen bonding is very strong. In fact, it is the strongest intermolecular force there is. Since water is a liquid, it is not a conductor of electricity because it doesn’t have any ions. At room temperature, water is a liquid and has a very high boiling point because it is held together by such strong hydrogen bonds. The compound Fluorine(as a diatomic molecule), also known as F2, is made up of nonpolar covalent bonds, which is the weakest bond of all the intramolecular forces.. It is nonpolar due to the fact that it is the same atom, therefore they are equal because they have the same pull. It is attracted by London Dispersion Forces which are the weakest of all the intermolecular forces.

Therefore, Fluorine is an extremely weak bond. Since Fluorine does not contain any ions, it is also not a conductor of electricity. At room temperature, Fluorine is a gas, so it has a very low boiling point because its attractive force is so weak. The compound Iron, also known as Fe, is a metallic solid held together by metallic bonds. Metallic bonds are the strongest intramolecular bonds of all. Metallic solids are also extremely strong and stronger than ionic solids, however, they are weaker than network solids. Iron is a very good conductor of electricity because since it is a metal, it is a moving sea of electrons so there are constant moving charges. Iron is a solid at room temperature and has a very high melting point because of its strong bonds and attractions. The substance Diamond, also known as C, is is held together by nonpolar covalent bonds which are the weakest of all the intramolecular forces. However, it is a network solid, which is by definition the strongest of all the attractions. Therefore, diamond is made up of some of the strongest bonds in the world. Diamond doesn’t have any ions, and no mobility so it is not a conductor of electricity. At room temperature, diamond is a solid and has an extremely high melting point because its network solid structure is so strong that it is virtually unbreakable. The bonding unit has taught me a lot about many substances. I now know that every substance on this earth has atoms in it and that they are bonded together in some way. I know that solids have strong attractions, liquids are less strong, and gases are the weakest. I know that ionic bonds are between a metal and a nonmetal and that covalent bonds are between two nonmetals. I know the difference between polar, nonpolar and coordinate covalent bonds. I know that conductors of electricity must have ions. I learned all about what makes network solids so strong and why diamond is the world’s strongest substance even though it is only one molecule. I learned that bonding truly exists in every aspect of our world....