Explain the relationship between the relative size of an ion to its atom and the charge on the ion?
961921
The first part of your question is not quite accurate. An ion is an atom. Normally, atoms are neutral; that is, they carry no charge.\n\nSo let's imagine you have a hydrogen atom with its single electron. If the hydrogen lost the electron, it would be a positively charged hydrogen ion. If the hydrogen gained an electron, it would be a negatively charged hydrogen ion. It would still be the same size as it was before, but the electrical charge would be different.
59794
i dunno the first one...but sharing electrons is a covalent bond, and charged atoms are ions and they form ionic bonds
52468
it is the charge of an electron 1.602*10^-19 Coulombs, i think that is what you are referring to.
231126
The difference in Pauling's electronegativity\ndetermine percent ionic character\ncovalent and ionic are sort of relative positions on a continuum
798559
positive ions are formed by removing electrons from the atoms and hence the ionic radius for positive ion is always less than that of atomic radius
536511
If you mean atomic radius, the atoms.  The ions will most likely have shed their outer electrons to form the ion, such as Ca +2, while the atoms keep that outer shell, which increases the radius.\n\ndkrgrand:  That's the whole point.  The size of Ca (the metal) is bigger than the size of Ca+2 (the ion) because of the missing shell.  This is what was asked.
976855
Ions are basically charged atoms. The formula of an ion can be found out if you have the valency of the atom. You can figure out the valency of any atom by finding the group at which the atom is located in the periodic table. For example, Sodium (Na) is located in group 1A of the periodic table. Hence the valency is +1. The formula of the sodium ion would be Na+1.\n\nHope that helps!
693553
The atomic number of an element is equal to the number of protons the element has in the nucleus of one atom.\nThe number of protons in the nucleus determine what element it is.\n\nThe atomic mass of an element is equal to the sum of number of protons and the number of neutrons in the nucleus.  The electrons around the atom are neglected since their mass is negligible, as well as the fact that atoms can form ions by gaining and/or loosing electrons even though the element is the same.
854239
I hope this is what you need:\n\nLattice energy is the energy required to completely separate an ionic solid into its gaseous ions. It depends on the ionic charges and on ionic sizes:\n\nE(l) = k * Q1 * Q2 / d\n\nwhere k is a constant (8.99 x 10^9 J·m/C2), Q1 and Q2 are\nthe charges on the ions, and d is the distance between ions.\n\nThe lattice energy increases as distance between the ions decreases and as ionic charges increase.
745401
There are two rules to use:\n1) The lattice energy between ions of opposite charge is strongest when the ions are small.\n2) The lattice energies  increase rapidly as the charge on the ion becomes larger.\n\nThe first rule implies that  LE(PbF2) > LE(PbCl2), in absolute value.\nThe second implies that   LE(PbF4) > LE(PbF2) and  LE(Pb2O3) > LE (PbF4)\nTherefore we have  LE(Pb2O3) > LE (PbF4) > LE(PbF2) > LE(PbCl2)  still in absolute value.\n\nConclusion:  3c 2d 1a 2b
876338
All three of these ions have the same number of electrons, they are "isoelectronic."  The size of the ions thus depends on the number of protons in the nucleus.  As we move to the right across a row on the periodic table, the number of protons in the nucleus, and thus the nuclear charge, increases.  This increase in nuclear charge pulls the electrons in tighter, thus reducing the size of the ions.  Na+ > Mg2+ > Al3+
30976
to explain how two electrons can be near each other
975119
Okay now you're getting into physics or something here, so I have absolutely no idea!\n\nBut it might have something to do with.......oh yeah, ions, that's it! Ions......
881483
cations form when the atoms lose an electron or more and have + valency , so the mass will decrease and the effect of the nuclei on the remaining electrons will be stronger so it attracts them stronger toward the center so the size will decrease .. while in the anions the number of electrons increase so the attraction caused by the nuclei is weaker so the size is larger ..\n\nsize of the cation of an element < size of the atom of that element < size of the anion of that element
740901
You need to split the ionic compounds apart to find the individual ions you would find in these structures.\n\nMgO would produce Mg^2+ & O^2- ions.\n\nK2S would produce K^+ & S^2- ions.\n\nYou can find the charge values directly from the periodic table trends for the charges atoms assume when they are ionized.
812707
The size of the atom increases across the table as more electrons are added to the shell.  Look at it logically.  The size of an atom with 8 electrons in the outer shell compared to an atom with one electron in the outer shell despite the increase in the charge of the nucleus.  Negative charges, (the electrons), repel.
917329
Realllllll Simply:\n\nCovalent molecules (atoms that make up the molecule) each contribute enough electrons (which are shared) to each other so that each atom thinks is has the nearest Noble Gas configuration. \n\nIonic molecules (the atoms that make up the molecule) transfer the electrons. One atom gains them and one atom loses them. Thus the atoms become ions (as in ionic bond), so they have charges.\n\nGet an "A".