How does the electron configuration of an element relate to it's position in the periodic table ?
829372
this web-site expains the relation very clearly:\nhttp://wine1.sb.fsu.edu/chm1045/notes/\nStruct/EPeriod/Struct09.htm\n\n(please copy/paste two address lines together, don't click directly on the first line)
48721
The periodic table elements atomic number will tell the number of protons found in the atom.  The number electrons will be same as the number of protons.\n\nHowever, if the atom is an "ion", it could more or fewer electrons than there are protons.  These are refered to as anions and cations (cat-eye-ons) respectively.\n\nThe net electric charge of N+ or N- written as a superscript to the atom will reflect the number of additional or fewer electrons for the ion.
178046
the s is the orbital in which 2 electrons can occupy\nthe orbitals are the s which can hold 2 electrons, the p which can hold 6 electrons, the d which can hold up to 10 electrons and so on \nhydrogen has an electron configuration of 1s1\nhelium has its elec. conf. of 1s2\nLithium has its elec. conf. of 1s2 2s1\nkeep adding \nNeon has its elec. conf of 1s2 2s2 2p6 \n\nTHOSe two 2s u add the elctrons which are 2 & 6 and u get get which makes the octect of NEON (noble conf.)
575353
That is simple- Just write down the the electronic configuration of the atomic number of that element. And the number of electrons in the last shell are the valence electrons.\n\nFor eg: Na(Sodium) has the atomic number 11, now there are four shells in which the distribustion takes place- namely- K,L,M,N.These shells are also known as energy levels. \n\nThe max no of electrons in K is 2, In L is 8, M is 16 and finally in N its 32.\nAnd you cant fill the next shell till the total number is completed in one shell.\n\nThere fore for Na the configuration is: K= 2 L= 8 M= 1\nAnd hence the valence electron is 1. That is only one electron partcipates in bond formation and in chemical reactions.
181377
The electronegativity generally increases as you go from left to right across the periodic table. It decreases as you go down the periodic table.\n\nI think you can see that the reason for this is going to depend on those same factors that we used to explain the trends in atomic size, ionization energy, and electron affinity. \n\nFirst, the horizontal comparison. As you go across a period from left to right, the atoms of each element all have the same number of energy levels and the same number of shielding electrons. Thus the factor that predominates is the increased nuclear charge. When the nuclear charge increases, so will the attraction that the atom has for electrons in its outermost energy level and that means the electronegativity will increase. \n\nThus the Periodic chart will not only tell you which metal has the most electronegetivity , but the order of all metals
56343
The Periodic Table of Elements organizes all the elements known to man. There are certain characteristics of each elements that they are grouped by. For example, the last column on the right is called the "Noble Gasses" becase they are all gasses in their natural state, and they're atoms have every electron in each orbital making them the most stable elements.
295219
It looks like a stable atom. The protons, neutrons, and electrons are all equal so they do not need to take away from other atoms. The maxium number of protons, neutrons, and electrons vary for each element. For example some elements on the periodic table can only contain 8 protons on the outer shell. Etc. And this question would get better answer if it was in Physics or Chemistry.
693223
Yes an atom is the same as an element.  A single atom is the smallest particle of an element.  There are 118 different elements in the periodic table. For example, a Hydrogen atom is one proton and one electron.  The next element in the periodic table is Helium, it has one proton, one neutron and one electron.  Each of these atom examples represent their own element.  So you see a single atom does represent it's own particular element, as discussed in the Hydrogen and Helium examples.
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The atomic radii for Cr, Mn, Fe, Co, Ni, and Cu are\n\nCr: 125 pm\nMn: 137 pm\nFe: 124 pm\nCo: 125 pm\nNi: 125 pm\nCu: 128 pm\n\nSo, you can see, there is a bit difference between their sizes. Although among them, Cr, Co, Ni, and Cu do have very similar atomic radius. \n\nThe reason that these elements have similar radius is due to their electron configurations. So, let's look at their corresponding electron configuration first (hope you know what I am referring to) :\n\nCr: [Ar] 3d5 4s1\nMn: [Ar] 3d5 4s2\nFe: [Ar] 3d6 4s2\nCo: [Ar] 3d7 4s2\nNi: [Ar] 3d8 4s2\nCu: [Ar] 3d10 4s1\n\nAs you may realize, the major difference between their electron configuration is mainly in the "3d" orbital, which has a quantum number (n) of 3; this 3d orbital has a smaller radius than the next orbital, 4s. The reason why 4s orbital is filled BEFORE 3d is due to the lower energy level of 4s compared to 3d.\n\nIn short, the major reason why these elements have similar radii is because the newly added electrons are not added to the "outermost electron shell", instead, they are added to the "inner electron shell". Therefore, no SIGNIFICANT changes to their radius.
1001402
Do you mean the valence shell?\n\nThe outer shell of an atom is its valence shell. The electron configuration of this shell determines the behavior of the atom.  \n\nFor more information refer to \n1. http://en.wikipedia.org/wiki/Valence_electron \n2. http://www.ndt-ed.org/EducationResources/HighSchool/Electricity/valenceshell.htm
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An element consists of protons, neutrons and electrons. The protons and neutrons are to be found in the nucleus which is a dense ball of energy/mass. The protons are 'positive' and neutrons are 'neutral'. The electrons are to be found within the vicinity of the nucleus in set energy states defined by the quantum properties of the particular element. The electrons can be considered to particles orbiting the nucleus if you haven't done quantum physics or they can be considered to have a probability distribution of appearing at any particular point within one of the clouds around the nucleus if you have some knowledge of quantum mechanics! Elements have the same number of protons and electrons so the charge is balanced. The number of neutrons tend to equal the number of protons in light elements, although this does differ frequently! In heavier atoms there are far more neutrons (this is to maintain the stability of the nucleus - which is made unstable by too many postive charges occupying a very close space).
337603
Here is the answer.. Just remember periodi table...\nElements on left most side are electro positive and elements on right most are electro negative. (The last row is nobel gases..so leave it)\nNow Cl- belongs to right most side... its more electro-ve\nRb, Ca are on left side.... they are electro positive(They will give  electron with out much force)\nSi, S are in middle-- their properties are in between...\n\nThats it!
402942
An atom is stable when it has a full valence (outer) electron shell.  For the first row on the periodic table, the outer (and only) shell can hold up to 2 electrons.  For the next two rows, the atoms' outer shells can hold up to 8 electrons.  The next two can hold up to 18.\n\nAtoms like sodium, in column 1 of the periodic table, have one electron in its valence shell.  It is very reactive, since it wants to get rid of this extra electron so that its outer shell can be full.\n\nAtoms like chlorine, in the second last column, have one electron missing from their valence shells.  They are also very reactive, since they want to accept an electron to fill the outer shell.\n\nNoble gases are almost totally unreactive, since they have the unique property of having full outer shells without having to give away or accept any electrons.
137403
the periodic table is great because it ditinguishes the different shells (s, p, d and f) that are filled as you add electrons. eg. He has 2 s electrons (full shell)\nNe has 1s2, 2s2 and 2p6 (full shell).\nIt gets a little more complicated at d electrons (transition metals) but Mendeleev did a great first shot.
835475
I think ur referring to the chemical definitions.\n\nIn the periodic table, groups are the vertical columns having similar elements... ie. they have the same valencies leading to similar properties.. Example Group 1: has valency 1.. (Na, K etc)\n\nperiods are horizontal rows having elements with the same number of shells.. ie.. 1st period elements have only one shell (H and He - K shell).. 2nd period elements have 2 shells (K,L) and so on..\n\nLook up wikipedia for more info..
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protons is the atomic number\nvalence electrons corresponds to this:\nGroup 1 (I) (alkali metals) :1\nGroup 2 (II) (alkaline earth metals) :2\nGroups 3-12 (transition metals) :1 or 2\nGroup 13 (III) (boron group) :3\nGroup 14 (IV) (carbon group) :4\nGroup 15 (V) (nitrogen group) :5\nGroup 17 (VII) (halogens) :7\nGroup 18 (VIII or 0) (noble gases) :8\n\n\nEvery element in the top row (the first period) has one orbital for its electrons. All of the elements in the second row (the second period) have two orbitals for their electrons. It goes down the periodic table like that. At this time, the maximum number of electron orbitals or electron shells for any element is seven.
15505
"This representation is related to the idea that the electrons are not precisely located around the atomic or molecular nuclei but must instead be described by probability amplitudes or wavefunctions which provides the probability to find electrons in a given region of space (for example along a particular chemical bond)." (from Wikipedia)