How do you find the number of vibrational modes in a molecule?
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The number of vibrational modes (different types of vibrations) in a molecule is 3N-5 for linear molecules and 3N-6 for nonlinear molecules, where N is the number of atoms. So the diatomic molecule we just discussed has 3 x 2 - 5 = 1 vibration: the stretching of the bond between the atoms. Carbon dioxide, a linear molecule, has 3 x 3 - 5 = 4 vibrations.
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The Lewis Dot diagram shows the number of electrons in the outer shell of an atom. These are also known as valence electrons. You simply determine the number of outer electrons an atom has, write the chemical symbol of the atom and by twos, place the same number of dots as there are outer electrons around the chemical symbol. Place the dots at the top, bottom, left, and right of the symbol.\n\nHow do you determine the number of outer electrons? Look at the periodic table. \n1. All the elements in the first column from Hydrogen to Francium all have 1 outer electron.\n2. All the elements in the second column from Beryllium to Radium have 2 outer electrons.\n3. Skip all the way to Boron. All the elements in that column have 3 outer electrons.\n4. Carbon's column has 4 outer electrons\n5. Nitrogen's column has 5. Oxygen's has 6. Fluorine's has 7\n6. Helium only has two, but the rest of the column under Helium has 8.
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1\nThere are 2 Hydrogen atoms, 1 Sulfur atom (as idicated by the absence of any subscript) and 4 Oxygen atoms.
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first of all write the molecular orbital configuration.then count the number of electrons with sigma bonds i.e., no. of bonding orbital electrons and then count the number of electrons with pi bonds i.e., no. of antibonding orbital electrons .Then\n\n bond order = 1/2[(No. of  bonding orbital  electrons) -(No.of antibonding orbital electrons)]
74671
a two attom molecule. molecule=more than one attom
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You can use Aldrich, which will give you a sample spectra of the compound. It would be very useful for identification based on a comparison of the fingerprint region (<900 cm-1)\n\nAny Organic book worth its salt will have typical vibrational frequencies. You can also do a yahoo search to get them.
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pv=nrt\nmeasure pressure, volume, and temperature to find the number of moles, n\n\nfind the mass of the gas\n\nmass of gas/ moles of gas= molecular mass (g/mol)
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There are several steps used to do Lewis Dot Structures.\n1) Determine the number of electrons required ( in this example there are 40 electrons required)\n2) Determine the number of valence elestrons ( there are 6 +6+6+6+6 = 30 ), however since you have a -2 formal charge there are 2 extra electrons, which means you have 32\n3) Determine the number of bonds (subract the number of valence electrons from the total required and then divide by 2) ie: 40 - 32 = 8/2 = 4 bonds\n4) write the atom symbols on this page ( in this example you're going to write Se in the center with one Oxygen on every side)\n5) connect with the number of bonds that were calculated\n6) fill in electrons until all the atoms have conformed to the octet rule except for hydrogen\n7) then count the number of electrons shown to check your work\nAnswer: 1 bond connects each Oxygen to the one Selenium and each Oxygen is going to have six dots on the outside and Selenium is going to have four dots.
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http://www.chemistrycoach.com/periodic_tables.htm#Periodic%20Table%20Songs\n I hope it helps you
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i think there is a formula like 13.6/n^2.where n=state.find out for n=1 and n=6 states and the difference of these two energies will give u the answer u require.
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This is kinda hard to draw on here...\n......_\nK--Br|\n......_\n\nThe lines around Br represent 2 electrons, and the -- represents a bond...ignore the periods
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Here is one : http://en.wikipedia.org/wiki/Periodic_table
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HBr, -1\nHOBr, +1\nBr2, 0\nHBrO4,  +7\nBrF3  +3\n\nThere is nothing to explain.  There are rules, and you need to learn them and follow them.\n\nHere is a site with a good set of rules\nhttp://www.science.uwaterloo.ca/~cchieh/cact/c123/oxidstat.html
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Use the periodic table of the elements.  The "weights" are in grams per mol.  Just use algebra and solve for the number of mols.  Then you know how many atoms there are by the number of mols which is a definite number.
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6.37 moles of any molecular substance just contains 6.37 times Avogadro's number of molecules, because a mole of matter always contains a mole of particles, that is, Avogadro's number many.  6.37*6.022 x 10^23 = 3.84 x 10^24.
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Let's assume that the energy of the Cl - Cl bond is 328 kJ/mol.\nSo that's how much energyis needed to break it.\n\n328 kJ/mol = 5.49 x 10^ -19 J/molecule\n\nUse E = hf  (E = energy, h = Planck's constant) \nto find the frequency (f) of the light with that much energy.\n\nThen, use the universal wave equation v= f(lambda) where v is the speed of light, and lamba is the wavelength, in metres.\n\nGood luck !
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Or . . . 6.023 X 10 to the 23rd atoms.\n\nGet an "A".