Give the definition of the Dash Method and the Dot Method in regards to Ionic Bonding?
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If you're referring to Lewis structures, dashes represent pairs of electrons being shared between 2 atoms and dots represent one electron (see link below).  When there is more than one line connecting atoms, that means they are sharing more than one pair of electrons.  Ionic bonds aren't usually represented this way. But to do this, each atom is surrounded by dots representing the electrons present after they are transferred to bond, surrounded by brackets individually (brackets can be left off if there are no electrons after bonding), and the charge is marked in the upper right corner.  The second link shows an example with salt (NaCl).
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It tells you when you're at the end point, and the end point is where ever you want it to be, hopefully past but not too far from the equivalence point. \n\nThis isn't always used for pH. Let's say you wanted to know the concentration Sodium in a Na2C2O4 solution. You could use standardized KMnO4 (which is purple) and do a redox reaction which would make CO2 and a bunch of cations (K, Mn, Na). This would be a redox titration, which is different from acid base. This redox titration is actually pretty interesting because a reagent is the indicator, so the end point is when the solution changes to the color of the reactant (this particular reaction is also self catalyzing, which is kinda neat as well).
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See if these help\n\nhttp://www.rit.edu/~pac8612/webionex/website/\n\nhttp://www.dartmouth.edu/~chemlab/chem3-5/ionx1/overview/procedure.html\n\nhttp://www.culliganmiami.com/pf7.html\n\nhttp://www.wqa.org/sitelogic.cfm?id=1085
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Ionic compounds are basically defined as compounds where two or more ions are held next to each other by electrical attraction. One of the ions has a positive charge (called a "cation") and the other has a negative charge ("anion"). Cations are usually metal atoms, and anions are either nonmetals or polyatomic ions (ions with more than one atom).\n\nA molecular compound is made up of all non-metals. The bond that forms between the atoms is by the sharing of electrons, unlike ionic compounds, which are made by the transfer of electrons.\n\nIn the case of NaH, this is a ionic compount and this is a strong base. \n\nAcid is defined as a compound which donates a hydrogen ion (H+) to another compound (called a base). You can also see it this way: An acid is a proton donor and a base is a proton acceptor. The acid is said to be dissociated after the proton is donated.\n\nAbout naming of compounds, read the book. It's a long discussion.
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It is not a reaction because the bond formed is ionic, not covalent.  Extraction is a better term for the process you are describing.
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To put it very simply,\nin a covalent bond, the atoms share electrons,\nin an ionic bond, electrons from one atoms are totally removed and added to the other atom, forming ions.\n\nBut in all bonds, there is some degree of sharing, even ionic.  Atoms of different elements "pull" on electrons with different strengths, the stronger the pull (larger electron negativity), the more time the electron will be found around that atom as opposed to the other.\n\nHydrogen gas (H2) is a good example of a covalent bond between two of the same elements, in this case, they share the electrons perfectly since they both have the same electron negativity.\n\nHF, or Hydrogen Floride is an example of a very ionic bond, with an electronegativity difference of 2.0 (4.1 - 2.1).  In this case, the electrons being shared spend almost all of thier time around the Floride ion, making that side develop a negative charge whereas the Hydrogen develops a positive charge.
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You need to split the ionic compounds apart to find the individual ions you would find in these structures.\n\nMgO would produce Mg^2+ & O^2- ions.\n\nK2S would produce K^+ & S^2- ions.\n\nYou can find the charge values directly from the periodic table trends for the charges atoms assume when they are ionized.
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Ionic bonds are created by attraction of separated charges or differences in electronegativity.  This results in a dipole moment, which is a vector property, hence it is directional.
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The chemical forces of attraction that hold atoms or ions together in chemical compounds are called chemical bonds. All chemical bonds result from the simultaneous attraction of one or more electrons by two or more.\n       You can give me your email address then i will prepare notes for you.\n  My email address is:\n\n\n                           masterpee_006@yahoo.co.uk\n\n\n\nOkay.Have a nice day and stay blessed.\n\n\nDo not forget to choose my answer as best answer.\nThank you.
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In Ionic bond, elements looses or gains electron(s) and become ions and the electrostatic potential of these ions bind them\n\nIn covalent, the participating elements are bound by sharing electrons between them.
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There are a lot of sites that have info.  Search for "formula writing polyatomic ions".\nIf you have a list of polyatomic ions like "SO4", "SO3", "PO4", etc. you will see that they have specific charges associated with them.  SO4 and SO3 both have a negative 2 charge.  Hydrogen has a +1 charge.  A compound must be neutral so you need 2 H to pair with one SO4.  +2-2=0.\nPO4 has a negative 3 charge, so you'd need 3 H+ to offset the 3 negatives.  H3PO4.\n\nAs far as naming them, search for "naming chemical compounds"  The examples you are asking about are actually acids, so you might need to look up "naming acids".
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these arent elements... they are compounds. you have to separate them first. then look at ur P.T. (periodic table) and if u look at the 8 tallest rows (the first 2 and last 6). from left to right, number the columns 1-8. whatever column number an element is in, that is how many dots are used. i hope this helped!
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H2SO4 + 2NaOH ----> 2H2O + Na2SO4\n\nYOU MUST SEPARATE AND CANCEL THE COMMON IONS (AQUEOUS ONES)
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OK....You need to understand how this is all working, and why.  So, the formula equation for this reaction would be something like:\n\nKOH(aq) + HNO3(aq) --> H2O(l) + KNO3(aq)\n\nSince KOH, HNO3 and KNO3 are all strong electrolytes, they are totally ionized when they're dissolved in water.  So, written in complete ionic form, that equation would be:\n\nK+(aq) + OH-(aq) + H+(aq) + NO3-(aq) --> H2O(l) + K+(aq) + NO3-(aq)\n\nTo get to the net ionic equation, you just cross out the things that are the same on both sides of the arrow.  K+(aq) and NO3-(aq) are on both sides, so the net ionic equation is:\n\nH+(aq) + OH-(aq) --> H2O(l)
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An ionic compound is dissolved with an appropriate solvent, or otherwise melted by heat, so that its ions are available in the liquid. An electrical current is applied between a pair of inert electrodes immersed in the liquid. The negatively charged electrode is called the cathode, and the positively charged one the anode. Each electrode attracts ions which are of the opposite charge. Therefore, positively charged ions (called cations) move towards the cathode, while negatively charged ions (termed anions) move toward the anode. The energy required to separate the ions, and cause them to gather at the respective electrodes, is provided by an electrical power supply. At the probes, electrons are absorbed or released by the ions, forming a collection of the desired element or compound.
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u do, ionic bonds results not from a sharing of electrons but from a transefer of one of more electrons from one atom to another
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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"