How do I find the outer electron configuration of ion Se and the formula for the ion?
921437
Se is in Group VI, hence it has 6 valence electrons, and most likely will taken in 2 more electrons to gain stability with an octet. Thus ion of Se should have a charge of -2 and the electronic configuration should be 2,8,18,8.\n\nHope this helps :)
1050318
With any ion - you can look at the charge it has to determine how many extra electrons it has.\n\nFor example -  elemental Sulfur has 16 electrons. To have a negative 2 charge it must have gained an additional 2 electrons. So it has a total of 18. \n\nBut since 18 is not one of the answers I assume the answer is 2 because it gained 2 electrons to get the negative 2 charge.\n\nHope this helped!
199009
The full electronic configuration of mercury is:\n1s2\n2s2 2p6\n3s2 3p6 3d10\n4s2 4p6 4d10 4f14\n5s2 5p6 5d10\n6s2
446055
Electrons per shell 2, 8, 18, 3
603525
Selenium element is located in Group 6A of the periodic table. This in dicates that it has 6 electron in its valence or outermost shell. The Lewis dot structure of Selenium shoulde be written with Se surrounded by six dots. These six dots don't have to be an all four sides but if you do then that is the conventional way of doing it.
961493
You need to know more than just the electron configuration.  There is contraction from left to right on the periodic table, plus additional periodic trends that must be considered.   \n\nEven more importantly, you need to define whether you are looking for the largest element IN ITS NATURAL  STATE (i.e. Cl2, Hg metal, etc) or AS THE ION.   Atomic and ionic radii differ.\n\nMore clarity is needed here.
192380
http://www.webelements.com/webelements/elements/media/kossel-pics/Xe.jpg\nYou can find that:\n1st shell: 2 electrons\n2nd shell: 8 electrons\n3rd shell: 18 electrons\n4th shell: 18 electrons\n5th shell: 8 electrons\nGround state electron configuration:  [Kr].4d10.5s2.5p6 \nShell structure:  2.8.18.18.8 \nTerm symbol:   1S0
697038
This is kinda hard to draw on here...\n......_\nK--Br|\n......_\n\nThe lines around Br represent 2 electrons, and the -- represents a bond...ignore the periods
561926
XeF  + e-  ============> Xe  + F-      E°/V = 3.4 with reference to the standard hydrogen electrode
917414
You apparently know what the diagonal rule looks like, but the link below gives a quite nice picture of it.\n\nBasically it is a summary of the order in which electron shells will be filled up. Follow the arrows round to discover where the electrons will go, starting at the 1s level.\n\nSo for 15:\n2 electrons will go into 1s, filling that up\n1s2\nthe next electrons will go into 2s2, 2p6, 3s2 and then the remaining 3 electrons into the 3p orbital, giving us a structure of:\n1s2 2s2 2p6 3s2 3p3\nRemeber, on your diagram, the first two characters (2p, 4d etc) are the names of the orbital, and the final digit is the number of electrons in that orbital. On your diagram the final digit shows the maximum number of electrons on the orbital; when you write out the structure the first few orbitals will be full (1s2 2s2 2p6 3s2) and the last one will be part full of however many electrons you have left (3p3.)
831018
http://www.chemicalelements.com/elements/be.html\n\nthis website may help you!!!!!! ( hope you get an A)
981192
http://periodic.lanl.gov/default.htm\n\nClick on the element, and it's in the top section of information. To write out the electron configuration for every element would take quite a while, so if you need it for a specific element or a few elements, I'd reccomend asking just for the few.
454535
Try drawing it yourself.  Here's the electrons per shell\n\n2.8.18.32.18.8.1 note they add up to 87, the Atomic Number for Fr.  Its Relative Atomic Mass is 223.\n\nWith this information you've got all you need.
1043428
Yeah - its in the second group of the periodic table therefore the ion will be 2+\n\nSome more information which may aid understanding or may just be useful at some stage \n\nAn atom in group one will have an ion which is +1\nAn atom in group 7 will have an ion which is -1\nAn atom in group 6 will have an ion which is -2\nThey are the general rules for all the ions which you you will probably come across most often
191934
Two in the first shell. 10 in the second shell. 10 in the third shell. 5 in the 4th shell for neutral Manganese. Mn 2+ is missing 2 electrons, so it would only have 3 in the outer shell. The rest will stay the same.\n\nHere's a cool interactive periodic table that may help you with your homework. \n\nhttp://www.webelements.com/\n\nYou can click on the the element you are interested in, then in the column on the left you can go to electronic properties and it will show you how the electrons are distributed. You can add or remove electrons to configure the electron arrangement of various ions of the substance you are interested in.
64224
All of the answers are in the periodic table. The atomic number is the number above the symbol. The number of protons is the atomic number. The number of electrons is the number of protons (if there's no charge). To find the number of valence electrons, look at the number of the column it's in (as in, Fluorine is in column #7, so it has 7 valence electrons).\n\nAs for the type of ion formed, everything to the left of the "staircase" (diving non-metals from metals) makes cations. Everything to the right makes anions.
954162
1.  they are the outer most electrons \n2.  8 because that is a full orbital and a octet.. they want to get a noble gas notation\n3. Covalent shares electrons Ionic bonds donate electrons due to low electronegativity