how to find the particular atom is in particular hybridisation in a molecule?
435560
you determine the hybridization of a particular atom by seeing how many electron pairs there are around a particular atom.  For example, if you draw the structure for ethylene (C2H4) you get \n\nH3C=CH3\n\nthis means that there are 3 electron pairs around both C atoms and they are both show sp2 hybridization.  \n\nIn another example, d2sp3 hybridization, you will have 6 electron pairs around the d2sp3 hybridized atom.  \nIn dsp3 hybridization, you will have 5\nin sp3 hybridization, you will have 4, etc...
88971
Force holding atoms in a molecule together as a specific, separate entity (as opposed to, e.g., colloidal aggregates; see bonding).\n\nIn covalent bonds, two atoms share one or more pairs of valence electrons to give each atom the stability found in a noble gas. In single bonds (e.g., H-H in molecular hydrogen), one electron pair is shared; in double bonds (e.g., O=O in molecular oxygen or H2C=CH2 in ethylene), two; in triple bonds (e.g., HCºCH in acetylene), three. In coordinate covalent bonds, additional electron pairs are shared with another atom, usually forming a functional group, such as sulfate (SO4) or phosphate (PO4). The number of bonds and the atoms participating in each (including any additional paired electrons) give molecules their configuration; the slight negative and positive charges at the opposite ends of a covalent bond are the reason most molecules have some polarity (see electrophile; nucleophile). Carbon in organic compounds can have as many as four single bonds, each pointing to one vertex of a tetrahedron; as a result, certain molecules exist in mirror-image forms (see optical activity). Double bonds are rigid, leading to the possibility of geometric isomers (see isomerism). Some types of bonds, such as the amide linkages that join the amino acids in peptides and proteins (peptide bonds), are apparently single but have some double-bond characteristics because of the electronic structure of the participating atoms. The configurations of enzymes and their substrates, determined by their covalent bonds (particularly the peptide bonds) and hydrogen bonds, are crucial to the reactions they participate in, which are fundamental to all life
801830
molecules of a compound are not pure and may contain more than one element however molecules of an element are pure and are only one type\n\nfor example:\nin a block of pure gold all the molecules are gold molecules nothing else\nin carbon dioxide the molecules are carbon and oxygen\n\nhope this will help u understand sweetie
78348
The answer has to do with symmetry of the molecule and hydrogen bonding.  That should get you going in the right direction
1082916
Atoms are the smallest pieces of an element that still exhibit that element's properties.  They consists of a nucleus (protons and neutrons) and  electrons.  A hydrogen atom doesn't even have a neutron.\nA molecule is a combination of atoms of at least two different elements.  These atoms share at least one electron through a covalent bond.  The molecule will exhibit some of the properties of each of its ingredient elements, as well as some of its own unique properties.\nA neutral atom or group of atoms has no charge. It is neither a positive nor negative ion.\nAn ion is an atom or group of atoms that has either more or less electrons than it has protons.  If its number of electrons is greater that its number of protons, then it has a negative ionic charge, in the amount of the difference.  If its number of protons is greater than its number of electrons, then it has a positive ionic charge, in the amount of the difference.
937266
1)electron ...(also negative meson)\n2)the atom is the basic (many atoms make molecule and so on)\n3)polymer (the most famous are protiens)
860814
In Carbon Carbon bonding:\n\nC-C is  sp3 hybridization, C=C is sp2 and C triple bond C is sp hybridisation. more s character is more strong covalent nature. Covalent character is increasing when moving multiple bonds in carbon. Covalent bond means sharing of pair of electrons (common pair) in bonding by both atoms(mutual) and hence both atoms come closer, that is lowering of bond length.
87059
You should consult a chemistry textbook, if possible, or if not, look online for an answer; I'm sure there is information or a guide describing how to do it better than I can in a few short sentences. That said, the basic way to draw a molecule (often abbreviated mlcl) is to use each element's symbol(ie sodium=Na, carbon=C, etc) to denote an atom, and to draw a single, solid line for each bond between elements. This line/bond represents 2 electrons, aka one orbital. Most elements like to have 8 electrons in their valence (outermost) shells in order to be stable, but this doesn't always happen; there are many exceptions, hence my suggestion to look at a textbook or online text/guide.\n\nIt gets more complicated when you're dealing with things like organic chemistry or complexes or chelating agents where sharing of bonds/electrons is pretty common and there are more types of bonds. For a simple example, if you had a 6-carbon atom ring, each carbon has 6 electrons in its valence; it wants 8, so what happens, does it get frustrated with its misfortune and self destruct, destroy our little universe? Of course not... there are a total of (6)(6)=36 electrons, and we need (6)(8)=48. How is this possible? Clearly, 36 is not equal to 48. We can't create more. So what happens? As it turns out, carbon, along with most other elements, passed kindergarten with flying colors- they SHARE them, and since it's a symmetrical hexagon shape of identical atoms, they are shared equally. There are all kinds of crazy combos in which the electrons are shared unequally between atoms because of something called electronegativity, but our rules for drawing those lopsided things aren't very different. However, that's for another 'lesson;' don't worry about it for now.\n\nSo, in order to make the carbon happy, we have to share 12, or 6 pairs, of electrons. ([48 needed]-[36 that we have] = 12) \nSince this carbon ring has multiple resonance structures (atom config the same but electron pairs on different atoms), we draw six carbons in a hexagon, with one solid line bond between each, and a dotted circle in the middle- this accounts for all of its resonance structures and provides us with more info, in addition to only needing one drawing to display that info, than using single bond lines only.\n\nSo in conclusion, I've said way more than I really had to... from the level of generality of your question I assume that you don't know too much about chemistry; if you are confused with what I said, then do as I said- look up the info online or get a book. It's not too easy to understand right away but with some patience you should be able to figure it out just fine; good luck.
92358
Just count the (sigma) bonds and the lone electron pairs and memorize the cooresponding geometric shapes.  Sorry, but it's the only way.
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.
926891
just count how many of each element you have, and make sure they add up\n\n\nC2H6 + 5O2 ---> 2CO2 + 3H2O\n2 carbon 6 hydrogen 2 oxygen----> 1 carbon 2 oxygen 2 hydrogen 1 oxygen\n\n\nso to even it out it would be...\n\nC2H6 + 7O2--->2CO2 + 3H2O\n2 carbon 6 hydrogen + 7oxygen--->2 carbon 4 oxygen + 6 hydrogen 3 oxygen\n\niff you add up each element they are the same on each side
899426
the way i like to look at is... in a given molecule, you usually have one or two (maybe three) central atoms.  for example, in CH3OH, the carbon is your central atom.  in C2H5Cl, two two carbons are your central atoms.\n\nnow, taking a look at the central atom, see if it is bonded to identical atoms an all sides.  For example, if the carbons are bonded to four idental atoms, then it is non-polar.  if the carbons are bonded to different atoms, then it is polar.\n\nIf you take a look at CH4,  there are dipole moments between the bond  between the carbon and hydrogen, but the molecule as whole is considered non-polar because the carbon is bonded to four identical atoms.  \n\nhope that helps.
963196
Many molecules have a lot more than two. You just have to keep counting. Don't forget the green ones.
950410
Mainly H-bonding (intermolecular forces)
829932
Take radium and subtract two from its atomic number. Then find the element with that result as its atomic number. I'm too lazy to see what that is right now.
1120147
Hybridization, in terms of Chemistry, involves the sharing, or overlapping, of orbitals.  Depending on the energy level where electrons are contained within a molecule, different orbitals will be formed.  These orbitals are really just mathematical representations of where electrons may be found.  The commonly studied orbitals are s, p, d and f.  They are different in shape.  Hybridization occurs when electrons of different orbital types overlap, and combine, forming a new orbital.  Hybridized orbitals tend to be more stable.  You may want to look up Molecular Orbital (MO) diagrams to fully understand how bonding among electrons occurs.
1107805
study on intermolecular particals and there behavior