what are metal carbonyls?
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Metal carbonyls are organometallic complexes of transition metals with carbon monoxide.
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An acid anhydride is an organic compound of the formula\n\nR-CO-0-CO-R\n\nwhere CO is a carbonyl, or a carbon double bound to an oxygen. They are quite reactive, as the presence of 2 oxygens on the carbon with no resonance structures makes the carbon quite electrophilic.
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Nail polish is mostly water, but the effective ingredient is acetone, a ketone with the formula:\n\nCH3 - CO - CH3\n\nwhere CO is a carbon double-bound to an oxygen (a carbonyl).
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carbon monoxide = CO\nIron (II) Chlorate= Fe(ClO3)2\nLead (IV) oxide = PbO4\nNitric acid = HNO3\nSulfuric Acid = H2SO4\n\nall numbers are subscripts.
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Silver carbonate, Ag2CO3.
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Hydroxyl,any compound that has OH is an alcohol,like CH3OH, or CH3CH2OH,etc....)\n\nCarboxyl,is a group that has c=o (carbon double bondedwith oxygen)\n\nHalide: Any element from group 7 like chlorine or iodine
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2Ag+ + CO_33-2 -> Ag_2CO_3
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Oxygen - Water, that should be easy to talk about.\n\n"Among the relatively few gold compounds of practical importance are gold(I) chloride, AuCl; gold(III) chloride, or gold trichloride, AuCl3; and chlorauric acid, HAuCl4. All three are involved in the electrolytic refining of gold. "\nhttp://www.britannica.com/eb/article-2770\n\nCarbon - Carbon Dioxide http://www.ch.ic.ac.uk/vchemlib/mol/simple/gases/carbon_dioxidebak.html\n\nHydrogen or carbon  - methane, natural gas.\nhttp://en.wikipedia.org/wiki/Methane\n\nIts salts, especially silver nitrate and silver halides, are also widely used in photography (which is the largest single end use of silver). http://en.wikipedia.org/wiki/Silver\n\nCalcium Carbonate\n"Calcium carbonate is a chemical compound, with chemical formula CaCO3.\n\nIt is commonly used as an antacid, and is the active ingredient in agricultural lime."\nhttp://en.wikipedia.org/wiki/Calcium_carbonate\n\nNitrous Oxide\nhttp://en.wikipedia.org/wiki/Nitrous_Oxide
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copper, silver, aluminum, lead, magnesium, platinum and tungsten
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calcium carbonate...\n\ncalcium and carbon....
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the acids are carboxalic acid and  carbonic acid
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Covalent single bonds.\nYou'll find carbon - oxygen\noxygen - hydrogen\ncarbon - hydrogen\ncarbon - carbon
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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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It's pentanal, because it's a terminal carbonyl. It's certainly not pentanol, because otherwise you'd have a carbon missing 2 bonds, or a carbon missing 1 bond and an oxygen missing 1.
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Carbon monoxide has a triple bond between the two elements, and has a LINEAR electron geometry.  Although, there IS a fairly large electronegativity difference between the carbon and oxygen, lone-pair distribution makes up for it.  Therefore, a carbon monoxide molecule is still a little polar.  It does have a small dipole moment.
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There are several.  Most are non-metalic oxides.\n\nCarbon dioxide:\nCO2 + H2O --> H2CO3 (carbonic acid)\n\nSulfur trioxide\nSO3 + H2O  -->  H2SO4 (sulfuric acid)\n\nSulfur diodixe\nSO2 + H2O  -->  H2SO3 (sulfurous acid)\n\nNitrogen dioxide\n3NO2 + H2O --> 2HNO3 (nitric acid) + NO\n\nThere are many others.
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Carboxyl\nand that's the last one I'm answering, I shouldn't be doing your homework for you...