Describe The Four Types Of Solid Structures Environmental Sciences Essay

Describe The quad Types Of Solid Structures Environmental Sciences Essay in that location ar three take a hops of substances subsist liquid, firm and gas in which solid is one of the major realm of matter. The solid building bonds the ingredients unneurotic by different chemical substance animal(prenominal) attraction. Chemical bonds ar the result of interactions of negatrons by various forces of attraction. This attraction idler persuade atoms together in a s add-in instalment. Atoms may permute or sh ar atoms to form molecules and compounds. When atoms bond together by chemical bonds, they will pass away more stable. Different types of chemical bonds determine solids properties, much(prenominal) as warminging signalise, persuadeivity and solubility (Lister and Renshaw, 2000).Electron transferring form noggin bonds turn electron sharing and joining molecules form covalent bonds. Linus Pauling came up with a scale, a value for each element called the electr onegativity (E.N.) value. from each one element has different desire wanting, ability to attract electrons. The sinewy electron attractions were given richly values and nearly atoms entertain actually natural depression ability to attract were given a low value. These values ar relative-comparison values and have no social social units. The value of difference electronegativity between two atoms less than 1.8 be defined as covalent bonds while the value of difference electronegativity between two atoms more than 2.0 argon defined as noodle bonds.This essay will describe quaternion-spot-spotsome types of solid social organizations dome and auriferous which contains of unit jail cubicle, giant covalent which is held by network and elementary molecular which be small molecules with weak forces of attraction. noodle StructureFirst of all, ionic bonding comm besides lasts in vitreous silica solid buildings. Ionic bonding electrons are transferred from mental a toms to non-metallic element atoms which result in each ion obtaining a full outer shell of electrons to become stable. Commonly, metals form cation by losing valence electrons while non-metals form anions by gaining valence electrons. atomic number 11 chloride (NaCl) is a well known ionic compound. sodium loses one electron from its outer shell while the chlorine gains one electron to occupy its outer most shell. When sodium (Na+) ions bond with chloride (Cl-) ions they form common table salt, sodium chloride (NaCl) (Lister and Renshaw, 2000).In addition, Sodium chloride (NaCl) is made up of giant wicket gate of ions. at that place are a large amount of sodium ions and chloride ions jam-packed together which depends on how big the crystal is. get word 1 (Adapted Steinberg, 2000) shows how does a bit of sodium chloride lattice arranged.Figure 1 Ionic adhere in Sodium Chloride (Adapted from Steinberg, 2000)Each sodium ion is at a meat surrounded by 6 chloride anions. Each chl oride ion is besides in the centre, it is also surrounded by 6 sodium cations. So sodium chloride is set forth 6 co-ordinated. The pattern in this way will be repeat countless times in sodium chloride crystal and ensure the uttermost stability in sodium chloride. Because when each ion is touched by 6 opposite bear downd ions, there is more attraction between the ions which makes the structure more stable (Clark, 2010). Figure 2 (Adapted from Clark, 2010) shows clearly the unit cell of sodium chloride.Figure 2 Unit Cell of Sodium Chloride (Adapted from Clark, 2010)Commonly, the atoms arrange in a regular way, but sometimes this is non the case. on the whole metal atoms consist of a lot of crystal grains which are regions of regularity. At grains boundaries atoms become inconformity.There are various properties in ionic compounds. Firstly, ionic compounds have a utmost melting point and boiling point. There are strong attractions between the decreed and negative ions which ta ke a lot of energy to overcome them. Secondly, one of the main properties of ionic compounds is they conduct electricity when molten, because when the compound is in the liquid state, the ions provide carry the charge loosenly. Ionic compounds are brittle which resulting from an applied stress. The ions will be go sufficiently to make contact between ions. Ions of the same charged are brought side-by-side leading to repulsion forces within the crystal. Many ionic compounds dissolve in the water. pissing molecules have unbonded electrons, called alone(predicate) pairs. They attract positive ions and negative ions in the compounds form dative bonds and arctic water forms electrostatic attractions between the ions. Water molecules also produce energy by hydration to break up the lattice and reduce their attraction (Clark, 2010).covalent bondsAtoms sharing electrons form covalent bonds which the electronegativity difference between two atoms are less than 1.8.Giant Covalent Struct ureIn giant covalent structures, all atoms are bonded together by covalent bonds which directly have an influence on precise atoms in a regular extended network. The electrostatics forces hold other structures together to act equally in all directions. Diamond is best ensample of giant covalent structure (Lister and Renshaw, 2000).Diamond has a tetrahedral shape in three-dimensions, with four covalent bonds from each carbon atom. According to VSEPR theory which do-nothing explain the levels of repulsion between chemical bonds (Lane, 2009), to reduce the repulsion four pairs of covalent bonds form and covalent bonds repel each other equally. There are no intermolecular forces of attraction only, between the carbon atoms.Figure 4 (Adapted from Chemcases, 2010) shows the structure of baseball fieldFigure 4 shows the structure of diamond (Adapted from Chemcases, 2010).Diamond is well known as the hardness natural substance, and results from four strong covalent bonds giving diamond a strong exacting extended and continuous structure, so diamond just stern be cut by other diamond. In addition, diamond has a very high melting point of around 4000K, because to break up the four strong covalent bonds requires a lot of energy. Next, the electrons which are held tightly are not free to move, resulting in the diamond having neither conduct electricity nor heat. At Last, diamond is insoluble in water because the covalent bonds are much stronger than the attraction of water molecules (Clark, 2000).Simple Molecular StructureThe simple molecular substances are non-metal compounds which are made up of atoms by strong covalently bond and relatively weak intermolecular forces. Water is taken as a typical type of the simple molecular structure (Lower, 2010). In water, each hydrogen atom is bound to the central oxygen atom by a pair of sharing electrons. group O has four free electrons in its outer second level to form two lone pairs to reduce the repulsions between clouds of negative charge, leaving two of the outer electrons overlap with hydrogen to form covalent bonds. This rule leads to a tetrahedral structure in which the angle between electron pairs is 104.5. In addition, water molecules forms hydrogen bonding.Oxygen likes electrons more than hydrogen and electrons spend more time near the oxygen, resulting in oxygen is part negative charge while the hydrogen is positive charge. Electrons are distributed leading to water form a negative structure of hydrogen bonds. Dipole-dipole attractions occur between two water molecules, due to its polar nature (Lane, 2009). Figure 5 (Adapted from Google, 2010) shows the structure of water molecule.Figure 5 Hydrogen Bonding Between Water Molecules (Adapted from Google, 2010)As the weak forces exist in simple molecular substances, they are not very leaden or strong nor solid resulting in it having a low melting point and boiling point. Simple molecular substances can easily become gas or liquid. There are no ions existing in these substances, so they are insoluble in the water and can not conduct electricity (Lower, 2010).metallic elementlic StructureMetals are giant structures which hold the atoms together by metallic bonding transferring the electrons. All elements of metal can easily lose electrons forming positive ions which are in a freely moving sea and electrons. How many electrons have been lost by each metal determine the number of electrons in the sea (Lister and Renshaw, 2000).Most ions in metals pack as close as they can. However, sodium in root word one is more open and less dense and forms a unit called the body-centred cubic (BCC) structure which is a common packing geometry for some metals. This structure is not a close-packed arrangement, just 68% of the space beingness filled (Lister and Renshaw, 2000). There is an atom located in the centre of a cube which is surrounded by eight other spheres. Figure 3 (Adapted from Clark, 2007) shows the structure of sodium a co ordination of eight and a unit cell containing two atoms.Figure 3 The Structure of Sodium (Adapted from Clark, 2007)There are several properties about metals. Most of metals tend to have a high melting point and boiling point due to the strength of the metallic bonding. The strength of metallic bonding is not only different from metal to metal, but also depends on the number of electrons which each atom can delocalise in the sea of electrons and by the packing. Transition metals have a high melting point and boiling point because they form a unit called hexagonal close packing. Group one such as Sodium is an exception and has a low melting point and boiling point, because it only has one electron to contribute to the bond and it is 8 co-ordinated which can not form strong enough bonds as other metals. Secondly, metals are secure conductors of electricity. The electrons in the sea are free to move throughout the structure even cross the grain boundaries. The metallic bonding still e xists as long as atoms are touching each other. In addition, these electrons are also responsible for the high thermal conductivities of metals. Electrons of the metals can pick up heat energy which is transferred to the rest of metal by moving electrons (Clark, 2007).In conclusion, electrons are transferred forming ionic bonding in ionic crystal solid structure. As giant lattice of ions exist in ionic solids, the ionic solids not only have a high melting point and boiling point but also conduct electricity well. Metal hold the atoms together by metallic bonding which determines that metal compounds have a high melting point and boiling point and are good conductors of electricity and heat. Although both of giant covalent structures and simple molecular structures have electron sharing covalent bonding, they have different properties. unfaltering covalent network bonding is involved in giant covalent structures holding the atoms together, with the result that giant covalent compoun ds are easily to melt and can not conduct electricity. In contrast, there are some weak intramolecular forces in simple molecular structures which lead to this human body of structure having a low melting point and boiling point, and ineffective to conduct electricity.