What is an inorganic molecule?
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First of all, do you know what a molecule is?\n\nA molecule is the smallest particle of a substance (that still has the same chemical and physical properties of the substance) that is composed of 2 or more atoms.  Atoms are held together by a number of chemical forces, including a wide variety of bonds.\n\nAn inorganic molecule is a molecule from a substance that is non-living.  It is not composed of organic (living) matter, and often times that means it will not contain carbon, as carbon (C) is the main element of organic molecules.
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The molecular mass of a substance (less accurately called molecular weight and abbreviated as MW) is the mass of one molecule of that substance, relative to the unified atomic mass unit u (equal to 1/12 the mass of one atom of carbon-12).\n\nThe molecular mass can be calculated as the sum of the atomic masses of all the atoms of any one molecule. The molecular mass can also be measured directly using mass spectrometry. In mass spectrometry, the molecular mass of a small molecule (< ~200 atoms of a given element) is exact, that is, the sum of the most common isotopes of each element. Of larger molecules, it is average, or calculated using the elemental mass number or the periodic table, since there is likely to be a statistical distribution of atoms representing the isotopes throughout the molecule.
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A chemical element, often called simply an element, is a substance that cannot be decomposed or transformed into other chemical substances by ordinary chemical processes. All matter consists of these elements and as of 2006, 117 unique elements have been discovered or artificially created. The smallest particle of such an element is an atom, which consists of electrons centered about a nucleus of protons and neutrons.
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A biomolecule is a chemical compound that naturally occurs in living organisms. Biomolecules consist primarily of carbon and hydrogen, along with nitrogen, oxygen, phosphorus and sulfur. Other elements sometimes are incorporated but these are much less common.\n\nBiomolecules are necessary for the existence of all known forms of life. For example, humans possess skin and hair. The main component of hair is keratin, an agglomeration of proteins which are themselves polymers built from amino acids. Amino acids are some of the most important building blocks used, in nature, to construct larger molecules. Another type of building block is the nucleotides, each of which consists of three components: either a purine or pyrimidine base, a pentose sugar and a phosphate group. These nucleotides, mainly, form the nucleic acids.\n\nBesides the polymeric biomolecules, numerous small organic molecules are absorbed or synthesised by living systems. Many biomolecules may be useful or important drugs.
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There are two broad classifications:  physical properties and chemical properties.  Physical properties include the solid, liquid, and gaseous phases (mostly).  Chemical properties, on the other hand, are many and varied.  There's organic and inorganic, biochemical, petrochemical, there are some based on a particular anion (nitride, oxide, phosphate, etc.); it all really depends on how specific one wants to be and what one is attempting to do or study.  \n\nThe analysis of matter is also broad:  there is structural analysis of both atoms and molecules (how is it put together?), there is quantitative analysis (how much is present?), and there is qualitative analysis (what is it?).
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In chemistry, a metal (Greek: Metallon) is an element that readily forms ions (cations) and has metallic bonds. Metals are sometimes described as a lattice of positive ions (cations) surrounded by a cloud of delocalized electrons. The metals are one of the three groups of elements as distinguished by their ionisation and bonding properties, along with the metalloids and nonmetals. On the periodic table, a diagonal line drawn from boron (B) to polonium (Po) separates the metals from the nonmetals. Elements on this line are metalloids, sometimes called semi-metals; elements to the lower left are metals; elements to the upper right are nonmetals.
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Figure 21: Heteropolymolybdate structures. (A) The structure of [Mo< ...  \n  \nchemical compound\n\nCrystal field, ligand field, and molecular orbital theories \n\nConsiderable success in understanding certain coordination compounds also has been achieved by treating them as examples of simple ionic or electrostatic bonding. The German theoretical physicist Walther Kossel's ionic model of 1916 was revitalized and developed by the American physicists Hans Bethe and John H. Van Vleck into the crystal field theory (CFT) of coordination, used by physicists as early as the 1930s but not generally accepted by chemists until the 1950s. This view attributes the bonding in coordination compounds to electrostatic forces between the positively charged metal ions and negatively charged ligands--or, in the case of neutral ligands (e.g., water and ammonia), to charge separations (dipoles) that appear within the molecules. Although this approach meets with considerable success for complexes of metal ions with small electronegative ligands, such as fluoride or chloride ions or water molecules, it breaks down for ligands of low polarity (charge separation), such as carbon monoxide. It also requires modification to explain why the spectral (light-absorption) and magnetic properties of coordinated metal ions generally differ from those of the free ions and why, for a given metal ion, these properties depend on the nature of the ligands. Thus, the complex ion hexafluoroferrate(III) (FeF63-) has magnetic properties to be expected from a substance with five unpaired electrons, as does the free iron(III) ion (Fe3+), whereas the magnetic properties of the closely related hexacyanoferrate(III) ([Fe(CN)6]3-) correspond to only one unpaired electron.\n\nSince 1950 it has been apparent that a more complete theory, which incorporates contributions from both ionic and covalent bonding, is necessary to give an adequate account of the properties of coordination compounds. Such a theory is the so-called ligand field theory (LFT), which has its origin in the more general, but more complicated, theory of chemical bonding called the molecular orbital (MO) theory. (Molecular orbitals describe the spatial distributions of electrons in molecules, just as atomic orbitals describe the distributions in atoms.) This theory accounts with remarkable success for most properties of coordination compounds.\n\nAn important conclusion from LFT is that two types of bonds, called sigma () bonds and pi () bonds, occur in coordination compounds just as they do in ordinary covalent (organic) compounds. The more usual of the two are  bonds, and they are symmetrical about the axis of the bond;  bonds, which are less common, are unsymmetrical with regard to the bond axis. In coordination compounds,  bonding may result from donation of electrons from ligands, such as fluorine or oxygen atoms, to empty d orbitals of the metal atoms (the designation d merely being a way of indicating the particular orbitals involved). An example of this type of bonding is the chromate ion, (CrO4)2-, in which the oxygen atoms donate electrons to the central chromium ion (Cr6+). Alternatively, electrons from d orbitals of the metal atom may be donated to empty orbitals of the ligand. This is the case in the compound tetracarbonylnickel, Ni(CO)4, in which empty  orbitals in the carbon monoxide molecules accept d-orbital electrons from the nickel atom.
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The IUPAC nomenclature of inorganic chemistry is a systematic way of naming inorganic chemical compounds as recommended by the International Union of Pure and Applied Chemistry (IUPAC). Ideally, every inorganic compound should have a name from which an unambiguous formula can be determined. There is also a IUPAC nomenclature of organic chemistry.\n\nThe names "caffeine" and "3,7-dihydro-1,3,7-trimethyl-1H-purine-2,6-dione" both describe the same chemical. The systematic name encodes the structure and composition of the caffeine molecule in some detail, and provides an unambiguous reference to this compound, whereas the name "caffeine" just names it. These advantages make the systematic name far superior to the common name when absolute clarity and precision is required. However, even professional chemists will use the non-systematic name almost all of the time, because caffeine is a well-known common chemical with a unique structure. Similarly, the chemical water is always known as such, never as "dihydrogen monoxide."\n\nSingle atom anions are named with an -ide suffix: for example, H− is hydride. \nCompounds with a positive ion (cation), the name of the compound is simply the cation's name (usually the same as the element's), followed by the anion. For example, NaCl is sodium chloride, and CaF2 is calcium fluoride. \nCations able to take on more than one positive charge are labeled with Roman numerals in parentheses. For example, Cu+ is copper(I), Cu2+ is copper(II). An older, deprecated notation is to append -ous or -ic to the root of the Latin name to name ions with a lesser or greater charge. Under this naming convention, Cu+ is cuprous and Cu2+ is cupric. For naming metal complexes see the page on complex (chemistry). \nOxyanions (polyatomic anions containing oxygen) are named with -ite or -ate, for a lesser or greater quantity of oxygen. For example, NO2− is nitrite, while NO3− is nitrate. If four oxyanions are possible, the prefixes hypo- and per- are used: Hypochlorite is ClO−, Perchlorate is ClO4−, \nThe prefix bi- is a deprecated way of indicating the presence of a single hydrogen ion, as in "sodium bicarbonate" (NaHCO3). The modern method specifically names the hydrogen atom. Thus, NaHCO3 would be pronounced "sodium hydrogen carbonate". \nPositively charged ions are called cations and negatively charged ions are called anions. The cation is always named first. Ions can be metals or polyatomic ions. Therefore the name of the metal or positive polyatomic ion is followed by the name of the non-metal or negative polyatomic ion. The positive ion retains its element name whereas for a single non-metal anion the ending is changed to -ide.\n\nExample: sodium chloride, potassium oxide, or calcium carbonate.\n\nWhen the metal has more than one possible ionic charge or oxidation number the name becomes ambiguous. In these cases the oxidation number of the metal ion is represented by a Roman numeral in parentheses immediately following the metal ion name. For example in uranium(VI) fluoride the oxidation number of uranium is 6. Another example is the iron oxides. FeO is iron(II) oxide and Fe2O3 is iron(III) oxide.\n\nhehe.. this is what i've found... sorry if it doesn't help...
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Fundamental concepts\nNomenclature\nNomenclature refers to the system for naming chemical compounds. There are well-defined systems in place for naming chemical species. Organic compounds are named according to the organic nomenclature system. Inorganic compounds are named according to the inorganic nomenclature system.\n\nRelated Topics:\nChemical compound - Organic compound - Organic nomenclature - Inorganic compound - Inorganic nomenclature\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nSee also: IUPAC nomenclature\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nAtoms\nMain article: Atom.\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nAn atom is a collection of matter consisting of a positively charged core (the nucleus) which contains protons and neutrons, and which maintains a number of electrons to balance the positive charge in the nucleus.\n\nRelated Topics:\nNucleus - Protons - Neutrons - Electron\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nElements\nMain article: Chemical element.\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nAn element is a class of atoms which have the same number of protons in the nucleus. This number is known as the atomic number of the element. For example, all atoms with 6 protons in their nuclei are atoms of the chemical element carbon, and all atoms with 92 protons in their nuclei are atoms of the element uranium.\n\nRelated Topics:\nProton - Nucleus - Atomic number - Carbon - Uranium\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nThe most convenient presentation of the elements is in the periodic table, which groups elements with similar chemical properties together. Lists of the elements by name, by symbol, and by atomic number are also available.\n\nRelated Topics:\nPeriodic table - By name - By symbol - Atomic number\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nSee also: isotope\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nCompounds\nMain article: Chemical compound\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nA compound is a substance with a fixed ratio of elements which determines the composition, and a particular organisation which determines chemical properties. For example, water is a compound containing hydrogen and oxygen in the ratio of two to one, with the Oxygen between the hydrogens, and an angle of 104.5° between them. Compounds are formed and interconverted by chemical reactions.\n\nRelated Topics:\nElement - Water - Hydrogen - Oxygen - Chemical reaction\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nMolecules\nMain article: Molecule.\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nA molecule is the smallest indivisible portion of a pure compound that retains a set of unique chemical properties. A molecule consists of two or more atoms bonded together.\n\nRelated Topics:\nCompound - Atom - Bonded\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nIons\nMain article: Ion.\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nAn ion is a charged species, or an atom or a molecule that has lost or gained an electron. Positively charged cations (e.g. sodium cation Na+) and negatively charged anions (e.g. chloride Cl-) can form neutral salts (e.g. sodium chloride NaCl). Examples of polyatomic ions that do not split up during acid-base reactions are hydroxide (OH-), or phosphate (PO43-).\n\nRelated Topics:\nCations - Sodium - Anions - Chloride - Salts - Sodium chloride - Polyatomic ion - Acid-base reactions - Hydroxide - Phosphate\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nBonding\nMain article: Chemical bond.\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nA chemical bond is the force which holds together atoms in molecules or crystals. In many simple compounds, valence bond theory and the concept of oxidation number can be used to predict molecular structure and composition. Similarly, theories from classical physics can be used to predict many ionic structures. With more complicated compounds, such as metal complexes, valence bond theory fails and alternative approaches which are based on quantum chemistry, such as molecular orbital theory, are necessary.\n\nRelated Topics:\nAtom - Molecule - Crystal - Valence bond theory - Oxidation number - Classical physics - Metal complexes - Quantum chemistry - Molecular orbital\n\n~ ~ ~ ~ ~ ~ ~ ~ ~ ~\n\nStates of matter\nMain article: Phase (matter)
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A chemical bond is the physical phenomenon of chemical species being held together by attraction to each other through sharing, as well as exchanging, of electrons and is a phenomenon that is fully described by the laws of quantum electrodynamics. In general, strong chemical bonds are found in molecules, crystals or in solid metal and they organize the atoms in ordered structures.
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by molecular bonds.  covalent and ionic.
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isomerism is classified into structural and stereo\nstuctural isomerism arises b/w two compounds when they differ in the structural arrangement of atoms. in organic it is divided into:\nchain\nposition\nfunctional\nmeta\nhowever in inorganic chemistry we have other classifications\n\nfor more and detailed information, u could go to google
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I'm not quite sure what you mean by "H2 molecules form higher elements."  An element is a single atom, such as Br, or Co, so molecules do not form atoms, rather, atoms form molecules.  There are various organic reactions, such as oxidation, fermentation, esterification, polymerization, condensation, and saponifacation, however, when CO2 decomposes, the products would most likely be C and O2, which could be shown by CO2 + heat ---> C + O2, since this is an endothermic reaction.
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NaCl IS A MOLECULE CALLED TABLE SALT!\nNH3 is not a molecule because the nitrogen atom is not bonded to another atom/atoms using all of its valence electrons and is therefore not a molecule, it is an ion.
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A compound contains more than one element (H2O).  A molecule may contain atoms of one element only (O2).
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Elements:\n\nMain constituents are H, C, O, N, with considerable amounts of Ca, Na, P, S, Cl, less Mg, K, Fe, I, and traces of about any common element.\n\nThe most common simple molecule is water.\n\nMost important "inorganic" compounds are CaCO3 (in the bones), NaCl (dissolved in the water) and Ca2(PO4)OH in the teeth.\n\nThe main classes of chemicals are carbohydrates and proteins, which form the main structural elements of our cells as well as most of the functional framework. (DNA for instance has a modified carbohydrate linked by phosphate as its structural basis). Fats (triglycerides of fatty acids) are abundant, but don't participate structurally in most features of human anatomy except as fillers (lower skin, lips, breasts...)
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Try Wikipedia.org...Qualitative inorganic analysis. I was just there.