A large majority of substances around us are solids. The distinctive features of solids are:
They have a definite shape.
They are rigid and hard.
They have fixed volume.
These characteristics can be explained on the baisi of following facts:
The costituent units of solids are held very close to each other so that the packing of the costituents is very efficient. Consequently solids have high densities.
Since the constiuents of solids are closely packed, it imparts rigidity and hardness to solids.
The costituents of solids are held toghetes by strong forces of actraction. This results in their having define shape and fixed volume.
Information regarding the nature of chemical forces in solids can be obtained by the study of the structure of solids, i.e. arrangements of atoms in space.
2 Classsification of solids
Solids are classified into categories:
Amorphous solids
Crystalline solids
The two types of solids have different characteristics.
Amorphous Solids. An amporphous solidd is a substance whose constituents do not possess an orderly arangement. Important examples of amorphous solids are glass and plastics. Although amorphous solids consist of microcrystalline substance but the orderly arrangement is restricted to very short distances. These distances are of the same order of magnitude as the interatomic distances.
Crystalline Solids. A crystalline solid is a substance whose constituents possess an orderly arrangement in a definite geometric pattern. Some very common examples of crystalline substances are sodium chloride, sugar and diamond. The main characteristica of crystalline substances are:
Orderly arrangement. The costituent units of crystalline solids are arranged in an orderly fashion which repeats itself over very long distances as compared to interatomic distances. The arrangement of bricks in a wall can be considered as an example. The arrangement is so well defined that the entire pattern can be repeated provided the arrangement of a few atoms is known.
Crystals are always bounded by plane faces.
The faces of crystals always meet at some fixed angles.
Crystalline solids exibit anisotropy in many of their properties. It means all those properties wich depend upon direction or angular orientation of crystals. These show different behaviour in non-parallel directions. One such consequence of anisotropy is the phenomenon of cleavage. In crystals the splitting is easier in some directions than others
The transition from the solid to liquid (i.e. melting point) for crystalline solids is sharp and distinct. An amorphous substance, on the other hand, has no sharp melting point. The transition fron solid to liquid in an amorphous solid does not take place at a define point but extends over a long range. The absence of sharp melting point suggests that most of amorphous solids may be best thought of as liquids.
Crystalline solids exhibit definite heats of fusion.
Crystalline – periodic arrangement of atoms: definite
repetitive pattern
Non-crystalline orAmorphous – random arrangement of
atoms
.
The periodicity of atoms in crystalline solids can be
described by a network of points in space called lattice
Atomic arrangement Space lattice
A space lattice can be defined as a three dimensional array
of points, each of which has identical surroundings.
If the periodicity along a line is a, then position of any point
along the line can be obtained by a simple translation, ru = ua.
Similarly ruv = ua + vb will repeat the point along a 2D plane,
where u and v are integers.
The Seven Crystal Systems
First notice: The intention of the following listing is to give you an overview rather than making you feel required to learn them by heart!
However, this is not yet the best solution for a classification with respect to symmetry. Consider for example the unit cells (a) and (b) presented before: While cell (a) is the actual unit cellspanned by the primitive translation vectors, it does not show the symmetry of the latticeproperly whereas cell (b) clearly shows the two axes of rotation.
So sometimes it makes sense not to use a primitive unit cell but one which fits better to the symmetry of the problem. This idea leads to the 14 Bravais Lattices which are depicted below ordered by the crystal systems:
There are two tetragonal Bravais lattices with a=b≠c and α=β=γ=90∘. One is primitive and the other body centered.
Orthorhombic
There are four orthorhombic Bravais lattices with a≠b≠c and α=β=γ=90∘: Primitive, body centered, face centered and base centered.
Hexagonal
When two sides are of equal length with an enclosed angle of 120∘ the crystal has a hexagonal structure and thus a 6-fold rotary axis.
Monoclinic
As in the orthohombric structure, all edges are of unequal length. However, one of the three angles is ≠90∘.
Trigonal and Triclinic
The trigonal (or rhombohedral) lattice has three edges of equal length and three equal angles (≠90∘). In the triclinic lattice, all edges and angles are unequal.
The simple structures come from the arrangement of the anions (though sometimes the cations) in the positions of the spheres in the fcc or hcp lattices, and the cations go into some or all of the octahedral and tetrahedral holes within the lattices. Structures based on face centered cubic lattices The Rock Salt structure This the structure adopted by Sodium Chloride , NaCl. It is based on the fcc array of the large chloride anions, and the sodium cations occupy all the octahedral holes in the fcc lattice . However, it could also be seen as an fcc array of sodium ions, with the anions in all the octahedral holes. Each ion is octahedrally coordinated by six counterions, and so this structure has so-called (6,6)-coordination , where the first number refers to the coordination of the cation and the second to the anion . The structure beyond the first coordination sphere can also be visualized. The Rock Salt, or NaCl, structure The sodium cations (green) occupy the oct
Oxides are chemical compounds with one or more oxygen atoms combined with another element (e.g. Li 2 O). Oxides are binary compounds of oxygen with another element, e.g., CO 2 , SO 2 , CaO, CO, ZnO, BaO 2 , H 2 O, etc. These are termed as oxides because here, oxygen is in combination with only one element. Based on their acid-base characteristics oxides are classified as acidic, basic, amphoteric or neutral: An oxide that combines with water to give an acid is termed as an acidic oxide. The oxide that gives a base in water is known as a basic oxide. An amphoteric solution is a substance that can chemically react as either acid or base. However, it is also possible for an oxide to be neither acidic nor basic, but is a neutral oxide. Defferent type of oxides;- Acidic Oxides Acidic oxides are the oxides of non-metals ( Groups 14-17 ) and these acid anhydrides form acids with water: Sulfurous Acid SO 2 + H 2 O → H 2 SO 3 (1.1) (1.1) SO 2 + H 2 O → H 2
Heme Protien :- Porphyrin+Iron-----Hemeprotein A hemeprotein (or haemprotein ; also hemoprotein or haemoprotein ), or heme protein, is a protein that contains a heme prosthetic group . They are a large class of metalloproteins . The heme group confers functionality, which can include oxygen carrying, oxygen reduction, electron transfer, and other processes. Heme is bound to the protein either covalently or noncovalently bound or both. [1] The heme consists of iron cation bound at the center of the conjugate base of the porphyrin, as well as other ligands attached to the "axial sites" of the iron. The porphyrin ring is a planar dianionic, tetradentate ligand. The iron is typically Fe 2+ or Fe 3+ . One or two ligands are attached at the axial sites. The porphyrin ring has 4 nitrogen atoms that bind to the iron, leaving two other coordination positions of the iron available for bonding to the histidine of the protein and a divalent atom. Roles
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