How do you find the electron configuration of an Ion?
154287
for example:\n\nCl-1: has 18 electrons = 17+1\nif u are talking about simple configuration: then ok:\nelectron config: 2,8,8\n\nif u want the SPDF configuration: then:\n1s2 2s2 2p6 3s2 3p6
811889
No concrete way to work it out. Groups one and two take positive charges equal to their group number (Mg2+, Li1+ etc). Groups 3, 4, 5, 6 and 7 ionise to a negative charge of 8 minus their group number (Cl1-, O2- etc), though 3, 4, and 5 tend to resist ionisation and are much more commonly found bonded covalently. The Transition elements ion charges are virtually impossible to predict without an extensive knowledge of d orbitals etc..
764097
Find the atomic number of elements.\n\nFind other data about the elements (molar mass, electronegativity, etc).\n\nPredict the properties of elements based on know properties of other elements in the same column or row.\n\nPredict the properties that have not been discovered yet.
691296
use that at equilibrium : n.p = ni^2\nand from charge neutrality: \n\nn + NA = p + ND
258486
This is a more complicated question than it appears.  You didn't include to what degree you were seeking this information, so rather than go into a great deal of explanation I have included a link that explains and tabulates the basics of electron energy levels.  Hope this helps.
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.
1090457
a the number of outer electron that will bond with other atoms to fill thei valence shells
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.)
266069
Every atom has two unique numbers: Atomic Number (Z) and mass number (A). Atomic number Z represents the number of protons in the nucleus of an atom. Mass number A represents the number of neutrons and protons in the nucleus of an atom. When atoms are expressed on a periodic table, they are written with a number on the top and a number on the bottom. Z is written on the top and A is written on the bottom. Also when elements are represented with the name and a number on the upper lefthand side corner. This number represents the electrical charge of the atom. This is the number that tells us if the atom gained or gave away electrons.\n\nTo calculate the number of protons: Simply just look at the atomic number and it is the number of protons. For example Number of protons in a sodium atom is 11.(Z=11)\n\nTo calculate the number of electrons: Subtract electrical charge of the atom from the atomic number. For example Na+1 tells us that sodium atom gave an electron away. So 11-1=10 electrons present.\n\nBut the number of electrons is equal to the number of protons when the atom is not charged.\n\nTo calculate the number of neutrons: Subtract the atomic number from the mass number. For example, to find the number of neutrons in the nucleus of a sodium atom 23-11=12 neutrons.
235740
Use toothpicks and colored gumdrops.\n\nChoose a color for: protons, neutrons, and electrons.\n\nThen use the colored gumdrops to represent them. for example, use 2 blue gumdrops for the protons, 2 red gumdrops for the electrons.\n\nthen connect them using the toothpicks- so end result is it looks lke an atom with te protons in the middle (nucleus) and electrons on the outside.
1164545
It's easy. I'de do it for you, but I'm about to leave work.\n\nIf you know the order of electron configuration, and how many electrons go into each sublevel, all you have to do is know how many electrons you've got. Whatever atomic number it has, that's how many electrons the atom has. Use the electron configuration model to place all the electrons in their proper energy level, and if you have it right, you'll know how many valence electrons you have. \n\nIf your clueless, then I can't help you. Research electron configuration. You should be able to find a chart showing you the order. \n\nThe levels go all the way up to 7, and within each one, is a sublevel, s, p, d, and f. s has 2 electrons, p has 6, d has 10, and f has 14. Helium for example has two electrons. \n\nHe = 1s^2\n\nHelium has only one level, and two valence electrons. \n\nOxygen = 1s^2, 2s^2, 2p^4\n\nOxygen has 6 valence because on the two outermost levels, there are 6 electrons, and also you see the ground state.
829932
Take radium and subtract two from its atomic number. Then find the element with that result as its atomic number. I'm too lazy to see what that is right now.
844991
Potassium is number 19. That means it has 19 protons. If it is an atom and not an ion, it has the same nimber of electrons as protons. Since protons are positive + and electrons are negative - , they have to balance. You find the neutrons by subtracting the atomic number from the atomic mass, since both the protons and neutrons weigh 1 and make up the mass. The electrons in the energy levels can move to another atom in compound formation.(ions)
712728
choose the noble gas that comes before the element.   in Mn(2+)'s case, that's Ar\n\nwrite the noble gas down in brackets, and continue on with the electron config. as normal\n\n[Ar}4s23d3\n\nFor O(2-), it turns into Neon so it would just be [Ne]
199009
The full electronic configuration of mercury is:\n1s2\n2s2 2p6\n3s2 3p6 3d10\n4s2 4p6 4d10 4f14\n5s2 5p6 5d10\n6s2
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!
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.