How does valence electrons revolve around the nucleus in a simple covalent bonds?
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The electrons form a standing wave surrounding both nuclei in a bond. The exact shape of this three-dimensional standing wave depends on the number of electrons in either element and the main quantum number.\n\nMost common are "hybrids" of S and P orbitals, for heavier elements also S and D and P orbitals. Those hybridized orbitals usually seek maximum distance from one another, leading to a rather small set of bond symmetries.
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I'm very surprised your book doesn't have information on VSEPR.  The acronym "VSEPR" stands for "valence shell electron pair repulsion".  Please double-check the list of topics in the back of your text.  \n\nA dipole moment in the context that you're considering is an incomplete sharing of electrons. In a covalent bond, one of the atoms involved is better at attracting & holding electrons than the other (more electronegative), so that instead of the covalent bond being perfectly shared it gets distorted to one side.  If a molecule has a dipole moment, it has more electrons (higher electron density) in one direction than in others.  One example of this is the covalently bonded acid, H-Cl.  Hydrogen is not very electronegative, but chlorine is very electronegative, so the chlorine atom does a better job holding onto the two shared electrons in the H-Cl bond.  \n\nI hope this gets you started in the right direction.  If you really can't find the info in your text, please go to a library and look at another chemistry book.
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The answer is simple. All elements (whose basic units are atoms) except the noble gases, have less than 8 electrons in their valence shells.  The rule that states that atoms should have 8 electrons to achieve stability is called The Octet Rule.\n\nhttp://en.wikipedia.org/wiki/Octet_rule\n\nThe way that they can attain 8 electrons is by forming BONDS: by either sharing electrons (covalent bond) or by gaining/losing electrons (ionic bond).   This is the main reason why atoms react: to attain 8 valence electrons.\n\nIf we look at it at another angle, we can say that atoms react in order to decrease energy.  This comes from the principle that bond formation results in loss of energy, and that stability comes from decreased energy.\n\nHope that helps.
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well i cant help you with the lewis structure cuz i dunno what that is. but the bohr diagram is   um hard to explain without drawing it out. ill try. \nfirst you draw a circle and the number of protons and neutrons in them (#protons is atomic number and #neutrons is mass=#protons). and then you draw an orbital around that circle and draw 2 dots on that orbital (corresponding to 2 electrons, there is a max of 2 electrons in the first orbital). then you draw another orbital around it and you can put up to 8 electrons (dots) on it. and then if you need another one, then you can put up to 8 on it and so on. the number of electrons you have to put is the same as the number of protons. and dont draw the empty orbitals.\n\nhope that helps. let me know if u need more help. later
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CaC2, it's not about the valency of either atom, the thing is the carbide carbons have a triple bond that joins them together, it's rather an organic chemistry question.
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dobereiner's like that mendeleev guy right? if my memory is right, all  of the elements above have similar chemical properties, that's why he placed them in his "triads". This means that all of them act similarly. Remember that it is the VALENCE electrons that causes the specific reaction of an element. So, as all three elemnts have the same number of valence electrons, they act similarly.
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Atoms become more stable with a full valence shell of electrons (usually 8 electrons).  Therefore, if an atom has 7 electrons, it is going to try to gain 1 more electron to gain a full valence shell.  Likewise, an atom with 1 electron on it's outer shell is likely to lose that electron, since the shell beneath it is full.  Since these atoms are losing or gaining electrons, they give themselves a positive or negative charge as a result and become ions.\n\nThe transition metals are a completely different story however, because these deal more with the d-orbitals rather than just the s- and p-orbitals.
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neon has eight valence electrons..and how u determine the is u look at a periodic table and Looking at the periodic table at the top of the table to the far right, neon has eight valence electrons.(All of the elements below neon in the same column have eight valence electrons.)(Ne=neon)below explains how to determine how to find valence in elements.\nThe periodic table shows how elements can be grouped into families. Elements with atoms that have one valence electron are in Group I; elements with two valence electrons are in Group II; elements with six are in Group VI; and elements with seven are in Group. http://lgfl.skoool.co.uk/content.aspx?id=767\nabove is the periodic table link.....
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An electron in an s orbital has zero angular momentum.\n\nViewed classically it is in Simple Harmonic Motion (SHM) passing through the nucleus of the atom.\n\nThe restoring force in the SHM is the electrical attraction between the electron and the positively charged nucleus.  The attraction is  an inverse square law which enables you to derive the equation of motion of the electron.\n\n  (Some "proton rich" isotopes undergo a type of radioactivity where this electron is captured by a proton in the nucleus which changes to a neutron which makes the atomic Number of the atom decrease by 1)
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Valence Shell Electron Pair Repulsion theory (VSEPR) is a set of rules whereby the chemist may predict the shape of an isolated molecule. It is based on the premise that groups of electrons surrounding a central atom repel each other, and that to minimize the overall energy of the molecule, these groups of electrons try to get as far apart as possible. Groups of electrons can refer to electrons that participate in a bond (single, double, or triple) to another atom, or to non-bonding electrons (e.g. lone pair electrons).
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If you mean the chemisty term like I think you so as in valence electrons, its the elcetrons on the outer most part of the atom which does all the bonding and reacting.
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to attain an octet electron config.\n\nzinc has 10 electrons in its valence shell. it gives up 2 when it ionises so it can form the magic 8 that is stable. fyi, many atoms in the the table strive to attain this 8, and this principle drives the understanding of many compounds formed from the elements.
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Filling its valence shell with paired electrons.
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Atoms don't get pulled around by electrons. The electrons orbit around the nucleus of an atom. The electrostatic attraction between the protons in the nucleus and the electrons is what keeps the electrons orbiting. When atoms form molecules, it is electrons that hold the atoms bonded to one another... electrons are "shared" by the various nuclei in the molecule. In other words, the electron orbits (orbitals) from neighboring atoms overlap, and the electrons can move freely within the system of overlapped orbitals.
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The Relationship of Electrons and Valence\n\nFor purposes of describing chemical behavior, an atom can be considered as a positively charged nucleus surrounded by negatively charged electrons orbiting in concentric spherical shells. The number of positive charges in the nucleus determines how many electrons normally surround the nucleus; as atomic number increases, the electron shells are filled, starting with those nearest the nucleus.\n\nThe valence of an atom is determined by the number of electrons in the outermost, or valence, shell. The atom exists in its most stable configuration when its outermost shell is completely filled; in combining with other atoms, it thus tends to gain or lose valence electrons in order to attain a stable configuration. If the valence shell of the atom is nearly complete, as in chlorine and other nonmetals, the atom will tend to accept electrons to complete it; if the valence shell has few electrons, as in potassium and other metals, the atom will tend to lose these electrons, so that the next shell below the valence shell becomes a completed outermost shell.\n\nThe valence of many elements is determined from their ability to combine with hydrogen or to replace it in compounds. For example, one oxygen atom combines with two hydrogen atoms to form water and the valence of oxygen is thus determined to be 2. Similarly, chlorine accepts one electron in combining with a single atom of hydrogen to form hydrogen chloride, HCl, and chlorine's valence is 1. Zinc does not combine with hydrogen but does replace it in compounds; in a typical replacement reaction, one zinc atom replaces two hydrogen atoms, as in the equation Zn+H2SO4→ZnSO4+H2, so that zinc has a valence of 2.
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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...
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It only has 7 valence electrons :)\n\nRival