BY molecular orbital theory the bond order of both are same.\n& hence stabbility by relation, stability directly proportional to bond order -they have same stability.but some theory say bcoz bonding electron in nitrogen molecule is more so it is more stable & other theory say bcoz the co molecule dont have antibonding electron so it is more stable........?  so which is more stable.
218386
YOU WOULD HAVE TO USE THE BOND ENTHALPIES TO WORK OUT WHICH ONE. SEEING THOUGH N2 MAKES UP 78%OF THE EARTHS ATMOSPHERE ITS SEEMS VERY INERT SO MOST PEOPLE WOULD ASSUME THAT IS THE ONE
530500
the previous answer is deficient on the following points...\nelemental C has the atoms held together by covalent bonding\nNa, being a metal, has metallic bonding, not ionic. Ionic bonds occure BETWEEN a metal and a non metal such as Na with Cl.\nMetallic character decreases as you cross the periodic table, and increases as you go down the periodic table, so Na is more metallic than Fe\nnon metallic character does the opposite..\nSo from the list above, metallic character would be Na > Fe >C  > S > O\nNa is a metallic lattice while O2 exists as discrete molecules\nHope that helps
449065
its because N only has 3 avalbile electrons to bond but P on it's outer has 3 but also contains more electrons at a lower orbit
249095
a) 1\n2) depends on if the outer shell is full or not. If it's full, they probably bounce off of each other, if not full, they can create a bond with each other.\n3) stable, noble\n4) becasue it has an electrical charge since the protons (positive) and electrons (negative) are unequal.
339718
B and C.  Molecules with H bonded to N, O, or F can form hydrogen bonds.  Others cannot.  In molecules A and D, all the H's are bonded to C's, so they are not capable of hydrogen bonding.  In molecules B and C, there is an O-H bond, so they are capable of hydrogen bonding.\n\nAlthough all four structural formulas have H written next to O, that doesn't necessarily indicate that there is an O-H bond.\n\nMolecule A is an ether, so the oxygen is between two carbons.  Specifically, it's dimethyl ether, so there's a methyl group (CH3) on each side of the oxygen.  You can find a picture of it here: http://en.wikipedia.org/wiki/Dimethyl_ether\nThe oxygen in an ether doesn't allow for hydrogen bonding because none of the hydrogens are attached to it.\n\nMolecule B a carboxylic acid.  Specifically, it's acetic acid.  It consists of a methyl group attached to a carboxyl group, which is a carbon double bonded to an oxygen and also single bonded to an OH group.  The O-H bond in the carboxyl group allows the molecule to form hydrogen bonds.\nYou can find a picture of its structure here:\nhttp://en.wikipedia.org/wiki/Acetic_acid\n\nMolecule C is ethanol.  It consists of a methyl group, a methylene group (CH2), and an OH groupl.  Like with carboxylic acid, the O-H bond is capable of hydrogen bonding.\nHere's it's structure:\nhttp://en.wikipedia.org/wiki/Ethanol\n\nMolecule D might be a bit misleading at first glance, but it's actually an aldehyde, specifically acetaldehyde.  It consists of a methyl group bonded to a second carbon that is bonded to a hydrogen and double-bonded to an oxygen.  That last hydrogen is attached to the carbon, rather than the oxygen, so it can't do hydrogen bonding.  Here's a picture of it's structure:\nhttp://en.wikipedia.org/wiki/Acetylaldehyde
530377
Okay, it's been a looooooong time since I had to use my chemistry skills, so lets see what I have:\n\nCopper is more magnetic with electrons than silver is because it's electrons (with fewer of them) are close to the nucleus (or whatever you call it) of the element.  Silver is more apt to lose its electrons with them being so far away.  \n\nCopper is more often found in a +2 state.  So I'd say that's a safe bet to go with.  I'd only assume a +1 state if your teacher said so.\n\nSo therefore:  2AgNO3 + Cu -> Cu(NO3)2 + 2 Ag would probably be your best bet.\n\nBut once again, it's been a long time since I used this so I don't know how right I might be.
355031
Well if it's stable, there will be the same amount of protons as electrons. If it has a charge add or subtract. \n(If you have a plus charge, that means there's 1 more proton than electron... if you have a -2 there are two more electrons than protons etc.)
360425
Electron cloud of N-F bonds will pull closer to N as you reasoned... However -- this will reduce the overall repulsion between the N-F bonds!  Thus, the repulsion from the lone pair-bond e will (in essence) be greater)and will tend to push N-F bonds closer togehter -- thereby reducing the bond angle for NF3.
147468
As above, chemical bonds hold atoms together, making molecules.  Molecules make up the vast majority of the stuff everything is made of.  Knowing all we can know about chemical bonds enables us to break existing bonds and make new ones.  That's how we make different kinds of things (from new drugs to artificial diamonds).  It's what makes chemistry soooo cool.  \n\nThere are 4 kinds of bonds (covalent, ionic, metallic, and hydrogen), but I've never heard of 4 kinds of hydrogen bonds.  Hydrogen bonds, strictly speaking, are different from the other three and are the attractive force between a polar hydrogen atom in one molecue and an exposed, unshared pair of electrons on another atom (like oxygen or nitrogen) on another molecule.
531836
all aelements in the same group have same number of electrons in their outermost orbit. but as you go down the group the number of orbits go on increasing and so there will be change in properties like ionization energy, electron affinity etc.\n\nnoble gases have got 8 electrons in their outermost shell or orbit. as we know that 8 electrons are required to complete octet, they have already a stable octet, so they don't require to loose or gain electrons to become stable as they are already stable, so they are unreactive\n\nthe period in which the element is present represent the number of shell of that element. for eg Mg has atomic number 12 so it will have 3 orbits or shell so it will appear in period III. all elements in same period will have same outermost orbit but number of electrons will go on increasing as their atomic number goes on increasing.\n\ni hope this will help you out
652170
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.
351568
If the ligands lie in the x-y plane, then the d-orbitals on the central atom that have all their electron density *out* of this plane will have the lowest energies.  These are the d-xz and d-yz orbitals. \n\nThe d-z^2 orbital has its density mostly out of the x-y plane, but there is a ring of electron density in the x-y plane, so this orbital will have a somewhat higher energy than the d-xz and d-yz orbitals.\n\nThe d-xy and d-(x^2-y^2) orbitals have their electron density concentrated in the x-y plane so their energies will be the highest.  They have the same energy.\n\nSummary, highest energy at the top:\n\nd-xy, x-(x^2-y^2)\nd-z^2\nd-xz, d-yz
192287
They have the same number of electrons and protons *relative to each other*.  \n\nFor example: carbon has 6 protons in it's nucleus, and therefore has 6 electrons to be neutral.  It's atomic number also happens to be 6 :-)
234477
H2 because it will be electronically more like Helium. It will have an electron with 1/2 spin up and 1/2 spin down. It will therefore have a happy orbital. You can also say that the bonding orbitals are occupied, and the antibonding orbitals aren't.
5305
It's because of the number of valence electrons they have. They are both willing to give 3 electrons away (which is why the have a negative three charge), so they also share the same affinity for electrons.
27961
Here, this question asks you for three things: Bond order, unpaired electron, and whether each is paramagnetic or diamagnetic. I figure that you already know what molecular orbital model is? Right? If you do, this problem is very very easy to approach. Look in your text book or google it for more info. Anways, I'll list the asnwer like this:\n--Bond Order:--Unpaired electron:--Dia-/Para:\nF2+ has  1.5;          1;                  P\nF2 has    1;           0;                  D\nF2- has   0;           1;                  P\n\nRemember the + means there is one less electron and - means there's one more. Also, I'm doing the Bond Order in my head so check again to make sure. Ask me any question regarding on this problem. It's very simple so I don't think you have much problem here.
620655
A covalent bond is a bond in which the atoms making up the resulting molecule "share" the electrons in the form of covalent bonds.\nAn ionic bond is an extremely one sided "sharing" of electrons, so one sided, one atom is said to have completely stripped of an electron from another atom.\n\nWhat determines if the bond is covalent or ionic is the difference in the electronegativities of the two atoms bonding.  If the electronegativity difference is high enough, the bond is said to be ionic.  If the difference in electronagativities is significant, but not quite to the level of a full ionic bond, the bond is said to be polar (which may or may not mean that the resulting molecule is polar, this depends on several things).\n\nLooking at a chart of [Pauling] electronegativities,\nhttp://www.psigate.ac.uk/newsite/reference/plambeck/chem1/p01244a.htm\none can see that most elements are somewhere in the 1 to 2 range, with only a few elements getting much lower or higher than this value.  Unless the difference is high enough (usually a difference of about 1.5 is considered ionic), then the bond will just be polar, or less so.\n\nSo, all elements have the potential to theoretically bond ionically, but only in certain combinations with other elements.\nFor example, you will never see an ionic bond between Carbon and Hydrogen since the difference is just .4, but an ionic bond between Lithium and Fluorine is easy to make with a huge difference of 3.0.