what is the lewis structure of H2O2? can you pleasetell me the # of electrons it has, the molecule nand the?
925613
The oxygens are bonded together with the one hydrogen bonded to each oxygen.  It hydrogen peroxide and has 18 electrons
677445
A water molecule contains two elements: hydrogen and oxygen. Both elements have different electronegativities, which is a fancy word meaning how well they can attract electrons. Since oxygen has a higher electronegativity, it forces the electrons of the water molecule toward itself, giving the oxygen element a slight negative charge and the hydrogen atoms slight positive charges.\nBasically speaking, water itself is somewhat charged. This makes water what is called a polar molecule and allows it to conduct electricity. This also accounts for how well water adheres to itself (cohesion).\nHowever, this polarity is relatively small.
726228
It is hydrogen (H). Hydrogen must always exist as a compound, forming a covalent bond with another hydrogen atom (H2).\n\nAtoms such as this are called 'diatomic'. There are others (N, O, F, Cl, Br, and I), however, only H is the stuff of the sun.\n\nUse the extra info to dazzle your teacher.\n\n. . .  and if you didn't know, now you do . . .
601089
Actually, H2O2 is a very strong oxidizing agent. \nNaClO + H2O2 ---> O2 + H2O + NaCl\nNet ionic equation:\nClO- + H2O2 ---> O2 + H2) + Cl-
479725
H2O is Hydrogen (2) Oxygen, which is two hydrogen atoms bound to one oxygen atom to form water. \nYahoo! is an internet company, which specializes in e-mail and search technology.
108641
if you want to know the number of electrons for a sample, you need to calculate the molarity of the substance and then multiply by the number of electrons that that element has. \n\nFor example:  you have 18 grams of water.  I picked that amount since the molecular weight of water is 18grams/mol.  (the mol weight of oxygen is 16 and 1 for hydrogen H2O =18grams of water is one mol of water)  A mol of sample is 6.02214199 × 10^23.  Yes thats a big number but its just like saying I have a dozen of something, a mol is a quantity of something.  I could have a mol of cars which would be 6.02x10^23 cars.  The reason we use such a big number is that there are so many atoms in even a tiny sample.  \n\nAnyways, 18 grams of water is one mol of water which is 6.02x10^23 molecules of water.  Now we need to figure out how many electrons are in one molecule of water and multiply it by the number of water molecules.  Oxygen has 8 protons and thus 8 electrons, hydrogen has 1 electron each, so a water molecule has 10 electrons.  So 6.02x10^23 times 10 more would equal 6.02x10^24 electrons in 18 grams of water.  (lots)
673911
If you could shrink 'way down and look at a single water molecule, you\nwould find that it is made of two hydrogen atoms and one oxygen atom.\nThey are arranged in a V-shape, with the oxygen at the point.  The result\nof this shape is that there is more negative charge at one end of the\nmolecule than the other (oxygen likes to have negative charge).  We call \nthis a POLAR molecule.\n\nOther polar molecules like salt and sugar and Kool-aid will dissolve in\nwater because the water molecule will be attracted to their charged ends.\nThe water molecule likes their charges so much that it will actually\nsurround the salt or sugar molecules, so that each one looks like a ball\nof water molecules.  We call this SOLVATION.  Since the salt molecule\nis surrounded now by water, it can't stick to other salt molecules, so\nit just sort of floats away.
753982
You have some errors there:\n\nSO4 with the -2 charge has 4 bonded pairs and no lone pairs (unbonded pairs) on the sulfur (but three on each of the four oxygens, which I assume you are not counting).\n\nH2 is correct with 1,0\n\nH2O2 is correct with 3, 4 (two lone pair on each oxygen)\n\nCH2O has 4 bonded pairs (four between the carbon and the oxygen for a double bond) and 0 non bonded pair.\n\nCO2 has 4, 0, with double bonds between each oxygen and the central carbon\n\nHF, is 1,3\n\nCl2 is 1, 6, if you count the lone pairs on the two chlorine like you are doing with F in HF but not the O in SO4 with the -2 charge.\n\nSO2 has a resonance structure where three bonded pair are smeared over two bonds between the S and O.  There are six unbonded pair (3 per oxygen) on the two oxygen.\n\nCH4O, (methyl alcohol?, CH3OH?) has four bonded pair between the carbon and three hydrogen and the one oxygen.  The oxygen has another bonded pair for its hydrogen and two unbonded pair.  This is 5, 2 as you have it.
1125360
H2O2 can exist in many forms at pH = 7, \n\nH3O2+, H3O3- are among the possibilities.
837857
Because in the H2 and O2 molecules, the atoms are the same, and so there is no separation of charges within the molecules. In the H2O molecule, which is H-O-H, the electrons are unequally shared, leading to a slight + charge on each H and a slight - charge on each O. The H's of one molecule are attracted to the O's on other molecules. This attraction of molecules for one another is so strong, that O2, molecular weight 32, boils hundreds of degrees below zero, whereas H2O, molecular weight 18, boils at +100degC.
43551
Most professional papers that I read refer to it as just water ion (in its charged form).  This a water molecule with an over-all positive charge.  I do not believe that its structure is known, but I could be wrong about this.\nSee example reference below:
82769
Specifically the intermolucular forces make up surface tension in water are hydrogen bonds.  A hydrogen bond is a noncovalent interaction between two polar molecules.  In this case one molecule of water lines up with another as shown here:  H2O - HOH.  Where the "-" is indicating an interaction between the relatively postive hydrogen on the right molecule and the negative lone pair of electrons on the oxygen of the left molecule.  As each molecule has two hydrogen atoms and two lone pairs of electrons on the oxygen, each is capable of participating in four separate hydrogen bonds.
697038
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
86157
"water has the molecular formula H2O, indicating that there are two atoms of hydrogen and one atom of oxygen in a molecule of water. Rounded to three decimal places, the atomic weight of hydrogen is 1.008 amu and that of oxygen is 15.999 amu. The molecular weight of water is thus (2×1.008)+(1×15.999)=2.016+15.999=18.015 amu. Since atomic weights are average values, molecular weights are also average values. On the average, a molecule of ordinary water weighs 18.015 amu."
294058
FeCl3 is a Lewis acid, because the Iron loses electron density because of the chlorines. So it complexes with the lone pair in water on the oxygen atom. In doing so, a proton is released from the water, which then complexes with the other water molecules to make H30+
968238
d) Reducing agent. Oxidation is the loss of electrons. The substance getting oxidized donates the electrons to the subnstance getting reduced. For that reason, a) Electron donor is also correct.\n\nI don't know if you're allowed more than one answer to this question. It may be that the teacher did not see that the reducing agent was an electron donor, and thought of electron donation in the Lewis base sense, which does not come up in this question.
446372
You proffered the example of XeF4.  Now the Lewis structure for XeF4 gives an expanded octet, viz: AX4E2, where A represents the central atom (Xe) in this example; X represents a shared pair of electrons; and E represents an unshared pair.  Thus for XeF4 we have 4 shared pairs and 2 unshared pairs, i.e. 6 pairs.  \n\nNow whatever the principal energy level(n), there is 1 s orbital; and for n=2 and higher, there are 3 p orbitals; and for n=3 and higher there are 5 d orbitals. For n=4 and higher there are 7 f orbitals.\n\nNow considering XeF4 hybridization, for the 6 pairs of electrons there will be 6 orbitals [each orbital holds a maximum of two electrons with opposite spin]. That means sp3d2 hybridization.  That is the one s orbital, the three p orbitals and two of the five d orbitals form six sp3d2 orbitals.  Of course, we are talking here about valence shell electrons.  How would these orbitals fill?  Well, electrons are added to orbitals such that electrons with the same spin are added until there are no more empty orbitals, then the orbitals with one electron fill (i.e. add a second electron) by acquiring an electron of opposite spin.\n\nThis gives XeF4 sp3d2 hybrid orbitals and an octahedron orientation. \n\nConsidering the Lewis structure for water, as another example, we obtain a AX2E2 form. Thus sp3 hydrid orbitals and a tetrahedron orientation. The 4 hybrid orbitals come from 1 s and 3 p atomic orbitals.