What is the chemical structure for NaCl?
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NaCl IS NOT TWO ATOMS (sodium and chlorine) BONDED TOGETHER!\n\nNaCl is what is known in chemistry as an ionic salt.  That means that a very positively charged Na+ ion met up with a very negatively charged Cl- ion, and because opposite charges attract, they got close to each other in what is known as an ionic bond, which isn't really a bond, just two particles hanging out together.
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Well it's tough because on one hand, an ionic compound is really likely to be a salt of somekind (CaCO3, NaCl).  But, on the other hand, you could have metals such as aluminum which forms an oxidized coating (Al2O3), which itself is ionic.  So you are looking at a brittle and maleable material.  In addition, not all salts are as soluble as NaCl.  Hmm... tough... good luck.
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Na+ Cl-\nC +4 O-2 each\nK+ Br-\nN-3 H+1 each\nMg+2 O-2
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Ionic compound\n\n The crystal structure of NaCl, a typical ionic compoundIn chemistry, an ionic compound is a chemical compound in which ions are held together in a lattice structure by ionic bonds. The positively charged ion is usually a metal ion and the negatively charged ion is non-metallic element or molecule.\n\nIons can be single atoms, as in common table salt sodium chloride, or more complex groups such as calcium carbonate. But to be considered ions, they must carry a positive or negative charge.\n\nThus, in an ionic bond, one 'bonder' must have a positive charge and the other a negative one. By sticking to each other, they resolve, or partially resolve, their separate charge imbalances. Positive to positive and negative to negative ionic bonds do not occur. (For a real world analogy, experiment with a pair of bar magnets.)\n\nIonic compounds have strong bonds between particles and thus generally have high melting and boiling points. They have good electrical conductivity when molten or in aqueous solution. While ionic inorganic compounds are solids at room temperature and will usually form crystals, organic ionic liquids are increasingly of interest.\n\nIonic compounds also dissolve in polarised liquids, of which water is an example, while they do not dissolve in organic liquids, such as Petrol. This is the opposite of covalent compounds.\n\nWhen an ionic compound is named, the cation is named first and then the anion. When an elemental anion is named, the suffix, -ide, is added to the name of the element. There are two common types of cations: Type I and Type II. Type I cations have only one charge and their name is simply listed when the compound is named. Type II cations have more than one charge and when the ionic compound is named, a Roman numeral is used to denote the charge of the cation. In addition, there are common polyatomic anions which do not have suffixes in their name such as hypochlorite (ClO–).\n\nRetrieved from "http://en.wikipedia.org/wiki/Ionic_compound"
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sodium & chlorine to make NaCl, table salt
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Determining structure of molecules.\nIonic structures- The Alkali metal halides are ionic compounds e.g NaCl. Na has a positive charge whereas Cl has a negative charge.\n\nMolecular solids- are held by weak bonds called Van Der waals forces. \n\nMacromolecular structures or giant molecular- have covalent bonds between atoms, these bind all the atoms into a giant molecule e.g Diamond
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I believe it's sodium chloride
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Binary: NaCl  (sodium chloride)\nPolyatomic cation:  NH4Cl  (ammonium chloride)\nPolyatomic anion:  Li2SO4  (lithium sulfate)\nPolyatomic complexed:  (NH4)3PO4  (ammonium phosphate)\nThey might be broken down differently to include inorganic and organic.  Their are also compounds called Zwitterions which contain both cation and anion.
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Glass:\namorph structure (not cristaline)\ncasant\nan melted mixture of Na2O, SiO2, K20\ntransparent\ninsipide\n\nSalt:\ncristaline structure - cubic system\nNaCl - natrium chloride\ntranslucid\nsalty taste
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Sodium fluoride is an ionic compound, so you can't really say that you have one "molecule" of sodium fluoride. Instead, what you have is an alternating arrangement of sodium and fluoride ions in a 6-coordinate ocathedral pattern in a crystal lattice. A nice picture of this is at the website listed below.
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Here you have the heat of solution of sodium hydroxide. LOL, it may help you with your work:\n\nhttp://chemlab.byu.edu/worksheets/0cb1f0c84fee4d6cda5d5f99832e9513.pdf\n\nand you can find the heat of solution for ammonium chloride here:\n\nhttp://www.brynmawr.edu/Acads/Chem/Chem103/swhite/exam2answersfall99.html\n\nThe heat of solution of NH4Cl is + 14.7 kJ/mol.
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The salt sodium chloride will dissociate into sodium ions and chloride ions as it dissolves in water. The solution is an elecrolyte.\nStarch is insoluble but can be persuaded to make a colloidal solution in water. Starch molecules do not dissociate, but remain suspended in the water. If left undisturbed for a while, the starch and water will separate into two layers.
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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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It is lithium Chloride i.e. LiCl\nIt is an covalent compound rather than being an ionic compound. It is define by FAJAN's rule
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salt.\n\n(Sodium Chloride)
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The formula for table salt is NaCl (Sodium Chloride). It exists in face-centred crystal lattices.
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NaCl is sodium chloride, that's chemistry! LOL!\nall i know is good chemistry and bad chemistry\nThe good is when you get the fluttering in your stomach when you look at them and your heart beats faster, \nthe bad chemistry is when you look at them and you feel your stomach turning over and your bile rising into your throat, then you make a beeline for the bathroom.