Do Oxygen atoms always covalently bond with each other when they join to become molecules?
817547
yes, they always covalently bond with each other under any normal type conditions\n\neven if you were to conveniently have an oxygen cation and anion that you combined, they would lose their ionic nature and bind in a covalent fashion
763539
In the Lewis structure, dots left alone want to pair up with those of another atom.  If there are 5-6-7 dots all around, the atom will accept electrons to fill it last layer.  If there are 1-2-3 dots, the atom will want to give those electrons away.\n\nSo you look at your Lewis structures, and try to pair up alone dots from one giving atom to a receiving atom. \n\nFor your peroxyde, you would get H.   and :.O.: twice so one link between and H and a O, another link between the other O and the other H, and then the two O's link together.\n\nFor you chlorine, there are 7 dots all around each atom, so they will share their un-matched electron in a covalent bond.  \n\nFor the CH4O, their are 4 dots all around the carbon, so you would think that one H will bond to each (that's 4 H then) but to add the oxygen, you have to insert it between a H and the C (that the hydroxyde radical).  It is written CH3H usually to show the -OH polyatomic ion.\n\nFor the C2H4, the carbon has 4 dots all around it, and they will bond to each other.  Each will link to two hydrogen (to make up the four in the molecule), leaving two dots on each C, so this means that there will be one double bond between the two carbon atoms.\n\nFinally, the CH2O os trickyer.  That carbon, with its four dots, will have one H bond to each one dot, so there are two free electrons left.  That oxygen has six dots, two pairs and two free.  This means that each free electron of the O will link up to one of the free electrons on the C, which means that there is one double bond between the carbon and the oxygen.  You'll have H-C-H for the first part and C=O for the second part.\n\nIt's kinda hard to type these :-)  Hope this helps anyway
812476
The bonding of what? The individual atoms to eachother........ The bonding of each sugar unit to the next..............
758383
Since the central atom, C, does not have any lone pair electrons on it, and it is bonded to 3 oxygen atoms, the general shape around the central atom is trigonal planar.  The hydrogen atom is bonded to one of the oxygen atoms.\n\nTrigonal planar indictates that all 4 atoms, C and three O, lie in a plane and that the O-C-O bond angle is 120o for all bonds.
976900
Chemical bonds form when electrons are shared, like in covalent bonds.  The atoms in the bond share a certain number of electrons between them usually so they both have a complete octet of electrons.  Another type of bond is ionic.  This is when one atom completely pulls off an electron from the other atom.  This results in a negative charge on the taker and a positive charge on the giver.  The bond is formed by the electromagnetic force acting between these two dissimilar charges.
1146263
Molecular bonding.\n\nThis is a function of the atomic weight (protons in the nuclei) and the distrobution of the electron shell.  Give me three years and I will explain it fully.
800097
Yes 1 is correct. Oxygen and Hydrogen have very strong bonds. Also known as hydrogen bonding. That's why water, for example, has such a high surface tension. You are correct!
46564
VTNomad is right.  Hydrogen gas is H:H (two hydrogen atoms sharing a covalent bond) and molecular oxygen is O=O (two oxygen atoms sharing two covalent bonds).\n\nOxidation results from electronegativity, or the affinity of atoms for electrons.  Oxygen is very electronegative, which means it really, really wants to have it's own electrons, and it hates to share them (metaphorically speaking, of course).  Hydrogen is not very electronegative, and its pretty content to walk around as a positive ion with no electrons at all.  It is the weakling on the school playground who will get beaten up and have its electrons stolen by the big kids, like oxygen and chlorine.\n\nTwo oxygen atons don't like having to share electrons, but they can't take them from one another.  But if an oxygen molecule sees two hydrogen molecules, then the two oxygen atoms will part ways, and each will beat up the hydrogen weakling and take both of its electrons.  The "fight" that ensues is fire, where the rapid loss of energy (O=O bonds and H-H bonds have a lot of energy, while H-O-H bonds are low in energy) becomes heat and light, aka fire.\n\nAn oxygen atom, though it likes electrons, will have a negative charge of -2 if it has the eight total electrons needed for Nobel configuration.  Likewise, Hydrogen will have a positive charge if denied its electrons.  So oxygen will let two little hydrogens tag along, and the H2O molecule is charge neutral.  But in water, the electrons are almost always around the oxygen, while the hydgrogen has very little chance of any electrons being around it for very long.  These bonds are low energy.\n\nOther things that burn--coal, gas, methane--these are things where carbon shares electrons with either more carbon or with hydrogen.  O2 will come along and steal electrons.  But O2 can't steal electrons from water, because the oxygen atom in water is just as tough (electronegative) as the oxygen in O2, so it won't win that fight.  But oxygen can take electrons from carbon (giving CO2, or carbon dioxide) or hydrogen, and it does.
11021
covalent bonds are called the directional bonds.because the orbitals involved in bonding have specific direction where they bond.
525685
You can approach this is one of two ways:\n\n1)  By analogy with H2O (because O and S are both in the same group)\n\n2) From first principles ie octet rule, Lewis diagram, hybridisation, shape. \n\nNow S has 6 electrons in outer shell, while H has 1 each, therefore, S will share 1 e- from each H to complete its octet and each H will share an e- with S so H (which is too small to have 8e-s in outer shell) will have a full outer shell. So S is now covalently bonded to to H atoms, accounting for 4 e-s, with 2 non-bonding pairs. That makes 4 pairs of electrons around S all together, so hybridisation is sp3. Shape is tetrahedral minus two vertices ie bent (just like H2O).\n\nI hope this helps.
750581
Covalent single bonds.\nYou'll find carbon - oxygen\noxygen - hydrogen\ncarbon - hydrogen\ncarbon - carbon
571040
Oxygen is the element. O2 is a MOLECULE.. a diatomic molecule!!
183750
One molecule of Oxygen is referred as Oxygen atom.  When two of these are fused together (by reaction), it is called Oxygen (exists in gas phase but can also exist as liquid under high pressure).  When three atoms are fused together, it is called Ozone.  Yes, the same one you hear about making hole in the atomosphere.  I am assuming that you are a bigginer chemist so I will not go through scientifc discussions regarding this chemical reaction.  If you are interested, post me anote and I will explain in details.
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.
950288
1)  Only the valence orbitals matter, and all the valence orbitals count (more complicated version: all valence orbitals which are of the correct symmetry to hybridize to form MO.  If you don't know what that means then you're in a lower level class and it doesn't matter).  # of atomic orbitals = # of molecular orbitals, and the molecular orbitals may be bonding, nonbonding, or antibonding.  Not depending on the particular class you're taking your teacher may or may not want you to draw the non-valence orbitals, but they don't matter at all.\n\n2)  You start filling all the MOs with electrons, starting with the lowest energy and moving up.\n\n3)  You wouldn't determine that for C2 because that's not correct.  The bonding and antibonding orbitals formed from the 2s atomic orbitals would both be filled (net bond order of zero) the lowest bonding (sigma) MO from the 2p AO would be filled, and each of the higher bonding (pi) MO from the 2p AO would have one electron.  None of the antibonding orbitals from the 2p AO would be filled.\n\nThis predicts that C2 would have 2 unpaired electrons, whereas a Lewis structure would predict a quadruple bond between the carbons.  One guess as to which one is right....
537794
Okay, to begin with; the molecular orbital theory is based on the "octet rule."  This means that, with exceptions of hydrogen and helium of course, an atom is most stable with 8 electrons (the octet) in its outer shell.  \n\nA diatomic molecule is a pair of identical atoms forming a small molecule.  The most common diatomic molecules are in the halogens; Cl, F, I, Br.  These atoms each lack one electron from a full octet, and will covalently bond in pairs to each gain a full octet.  Oxygen gas (O2) will bond in a double pair, sharing four electrons to gain an octet on each atom.  \n\nBeryllium contains 4 electrons in total.  The electronic configuration is 2:2 or if you use the other method is 1s2 2s2.  A full octet would be 2:8 or 2:0 to gain the most stability, and the Be2+ is actually in use in labs (2:0).  \n\nBecause it would need to gain electrons from or donate them to some other element with a greater number or greater need, beryllium can't form a diatomic molecule or a pair with another of itself.  \n\nIt is difficult to explain without pictures, but there are a few shell pictures available at Chemical Elements which will let you compare these elements.
467694
When atoms combine by covelant or ionic bonds, the resulting compound has properties that are different from those of the atoms.  For example, Sodium is a soft and very reactive metal, and Chlorine is a yellow-green poisonous gas, but when they combine ionically, the result is table salt: neither reactive nor poisonous.  This has to do with how the electrons are situated at the atomic level.  Often, bonding stabilizes the electrons and makes the resulting compound less reactive, which is why water will not react the way Hydrogen or Oxygen do.