What is the term given to teo electrons shared by the same atom?
452327
Not exactly sure what you're asking here either, but perhaps a better answer is that electrons that are shared equally between two atoms in a bond are covalent, while electrons that spend more time with one atom than with the other form an ionic bond.\n\nHope that helps.
740938
If a bond has ionic nature, the electrons have a tendency to hang out by one of the atoms in the bond more than the other... On the other hand if the bond is completely covalent in nature, the electrons are shared equally by both bonded atoms.
263276
You mean the electron configuration?\n\n1s2\n2s2 2p6\n3s2 3p4
430202
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 :-)
795345
Same number of protons\n\ndifferent number of neutrons
261105
Better than what?\n\n\nHere's a description of the result:\n\nEach successive "shell" has the capacity to store one more group of paired electrons in a new kind of orbital.\n\nPrincipal quantum number 1:\n1 s-orbital\n- will hold one pair.\n\nPrincipal quantum number 2: \n1 s-orbital\n- will hold one pair.\n3 p-orbitals\n- will hold 3 pairs.\n\nPrincipal quantum number 3: \n1 s-orbital\n- will hold one pair.\n3 p-orbitals\n- will hold 3 pairs.\n5 d-orbitals\n- can hold 5 pairs, but due to "crowding" wait until the 4th S orbital is filled. Are available to help form double bonds for elements like P, S and Cl though.\n\nFor principal quantum number 4 there is the addition of 7 f-orbitals, which insert themselves after the first d-orbital of the next higher principal quantum number is filled.\n\nAs a result, there are lots of rare metals which form 3+ ions...\n\n\nNow why is this so?\n\nThere is no easy way to explain this with classical mechanic and electrostatic. It has to do with standing waves, elimination by interference, and the wave/matter duality. In short, quantum mechanics. If you don't want to start with that topic, just accept that this is how it works...
151430
A proton, neutron, and electron is what makes up an atom.  a molecule however is defined as two or more atoms linked by chemical bonds which are linked atom.  Covalent bonds consist of shared pairs of electrons Electronegativity: unequal sharing of electrons...U can find more info on askjeeves.com
979155
alright. Electron configurations. I had the exact same problem three weeks ago. I was SO confused. But i got it in the end.\n\nLet me explain.\nThere are two types of electron configurations. One is the simple electron shell configuration. Let's say 2-8-16 and the other is called spdf notation like 1s2 2s2(i can' t type the two after the s like an exponent so bear with me)\n\nNow the first one is simple. Shell notation. An atoms outer shells are divided into shells that each have a maximum limit for the number of electrons that they can contain. the first can hold 2, the second 8 and so on. They all follow a rule. It is always 2 time the shell number squared. lets say level 1. Square it. You get 1. Multiply it by 2. You get 2. Therefore 2 is the maximum # that level one can hold. You said 15. So fill each level so that each contains the max. It would be 2-8-5. (The last one is five so that the all ad up to 15). Got it?\n\nNext, we have spdf notation. This takes a lot of time to explain so i'll just give you a site to go to. \n\nhttp://www.fordhamprep.org/gcurran/sho/sho/lessons/lesson36.htm\n\nGood luck!
889275
Covalent bonding is a description of chemical bonding that is characterized by the sharing of one or more electrons between two atoms. In general bonds are defined by a mutual attraction that holds the resultant molecule together. Often bonding occurs in such a way that the the outer electron shells of the participating atoms become filled. In contrast to electrostatic interactions labeled as "ionic bonds," the strength of covalent bond depends on the angular relation between atoms in polyatomic atoms. Covalent bonding is most important between atoms with similar electronegativities. Covalent bonding is often delocalized.
1163298
in covalent compounds, the two ions being bonded share electrons.  these are called covanlence electrons.  in an ionic bond, they share the electrons in a different way.
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
44394
1. The Aufbau principle: Orbitals are occupied in order of increasing energy. 1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d<6p<7s<5f<6d\n\n2. The Pauli exclusion principle: Only two electrons can ocoupy an orbital and they must have opposite spin.\n\n3. Hund's rule: When there are degenerate orbitals, one electron is added to each with their spins parallel until all are half full. Then a second electron with opposite spin is added to each degenerate orbital. (See below)\n\n(Basically every space/box/circle must have an arrow pointing up before any space/box circle can have one pointing down.)\n(Everyone gets one before anyone gets two.)
816025
b) the electronegativities of both atoms involved in the bond are identical.
887107
B.the electron subshell
932025
You mean the Valence Shell Configuration?\n\nIt is easy to find this by simply looking at the Group # (these are the column numbers). \n\nElements in Group 1 all have 1 electron in their valence shell, Elements in group 2 have 2 and so on...\n'\nIf you mean how many shells there are then look at the Period #  this is the horizontal groups) the Period # corresponds with the number of electron shells.\n\nElements in Period 2 have 2 electron shells, elements in Period 3 have 3 and so on...
797271
they are the same.  orbitals on an atom are atomic orbitals.
965248
The atomic number (the big number in the middle or on top of the square) represents the number of protons in the atom, but since an atom is by definition neutral, the number of electrons is the same.  For an ion, you would take the atomic number and subtract the charge, so for instance, carbon (atomic # 12) with a +1 charge would have 11 electrons.