why is a negtivly charged ion larger than its corresponding neutral atom?
371324
Negatively charged ion has one/some extra electrons than the corresponding neutral atom. so, deu to repulsion they stay more apart.\n\nthat is what i think is the reason why -ve ions have greater radious than neutral atom.
634552
an ion with both acidic and basic part
758851
This is because the nuclear attraction over the electrons increases.\nRemember Coulombs law of electro_nuclear forces.
943097
I think it's false. If the ionisation energy is increased, it's more difficult achieve ionisation, therefore less likely to be reactive. This is why those at the top of the group are more reactive.
679382
Jaleesa, I think that you can use the same principle that I explained in the earlier question. The Sodium ion has fewer electrons and fewer shells, and is thus smaller than the potassium ion. But I think you should do the rest of your homework yourself.
570227
Na is larger than Na+.\nF is larger than F+.\nCations are always smaller than the parent atom as the effective nuclear charge acting on an electron increases as the total number of electrons decreases.\nIn the case of Na&Na+,Na+ has one whole shell lesser than Na.
36755
An atom has no charge because it likes to be stable and to be stable it has the same number of protons (positively charged particles)as it has electrons (negatively charged particles) therefore they cancel each other out of course sometimes they are not stable and are called ions which are charged atoms
285366
well if by terminal you mean, like a hub.  it would probably be due to the larger number of electrons inside the valence shell, not the valence shell itself. the ones give them their strong electro negetivity,combined with the fact that as the atom gets larger there is more distance between the center(+) and the surrounding (-).  these cause coordinate bonds, basicly like static electricity attracts things. the bonds are weaker than covalent or ionic cause the moleceles already stable(this is where the valence shell comes in, stability), a good example of this example is take a hard natural magnet and try sticking a piece of steel note the force that is required to seperate the two. then exert that same amount of force toward breaking the magnet itself.  you'll surely notice that the bonds in the magnet are far stronger than the bonds that the magnet makes with other substances.  ok do you see now how a strong negtive force within a atom has the ability to attract weaker positively charged atoms/molecules?  i noticed one answer had the valence shell mentioned, and true they have a valence configuration which has a deficency of one electron.  this is a factor ivolved in the formation of ionic and covalent bonds.  the coordenate bonds are more like magnets attracting one another. the difference in electro negetivity is what determines the type of bond techniclly.  the ionic bonds are the strongest. now the covalent bonds actually share electrons and these bonds are not as strong, and the coordenate bonds are weaker still.  there are other even weaker bonds such as hydrogen bonds (i.e. in water the hydrogen bonds account for the face that water expands right before it freezes). these bonds are the result of the attraction of the positive charge that is present with the electron of the hydrogen affects the magnetic field within the oxygen atom causing a slightly more negetive charge in a 180 deg. position relevent to the hydrogen. anyway i had a little more time tonight.
246818
Here is the easy answer:\nCations are formed by losing electrons.  When comparing the relative numbers of electrons to protons, there will be more protons (because electrons were lost).  Protons are positively charged... since there are more of them compared to electrons, the cation will have a positive charge.
298345
The Sodium (Na) atom is much larger by comparison to the Chlorine (Cl) atom.\nThe periodic trend of atomic radii gets smaller as you move accross a row.  Since Sodium is at the start of the row and Chlorine at the end, Sodium is larger.\nThis has to due to with the largest shell holding electrons, both Na and Cl's largest shell is the 2S orbital, but since Chlorine has many more protons in its nucleus, those electrons are held more closely than those of Sodium.\n\nOn the other hand, when an atom becomes an ion, it either gains or looses an electron (protons dont change).  When Sodium becomes an ion, it looses 1 electron to become Na+ and because of this, it looses the electron in its outer shell which is making it so big (ion is smaller than the atom).\nWhen Chlorine becomes an ion, it gains an electron which goes into completing its Octet and the ion is larger than the atom.\nWhen all is said and done, the Chloride ion (Cl-) is much larger than the Sodium ion (Na+).
129718
its due to their spin, and actually protons are composed of quarks (which due to their spin properties give it a positive charge).\n\nYou can do a search on quarks and learn more about sub-atomic particles
493143
Considering the conflicting answers, perhaps I should add something:\n\na sodium *atom* carries 11 electrons and has a neutral charge, therefore having a configuration of 2:8:1 as one person wrote -- 2 electrons in the first (ground) level, 8 electrons at the second level, and 1 (valence electron) in the third level.  As a configuration written 1s2 2s2 2p6 3s1 -- 2 electrons in the first (ground) level, 8 electrons total at the second level (2 in s, 6 in p), and 1 electron in the third level.  These are the two possible ways of writing the electron configuration -- remembering of course the superscript that we don't have here!  \n\nThe other answers that I saw were describing sodium as having 10 electrons.  These with 10 electrons are not sodium atoms but sodium *ions.*  If sodium becomes ionized it loses an electron and becomes positively charged -- in that case losing the valence electron in the third level.
462594
As you go down, the electrons occupy energy levels whose energy is greater. That is, they are farther away from the nucleus. For example an element in period 6 has its outtermost electrons in the n=6 energy level. These electrons have a greater potential energy than those in the n=2 level because they are farther away from the nucleus. This is similar to an object that is higher up: It has a greater gravitational potential energy. The size of the atom increases because as more electrons are present in an atom, the more energy levels they fill. The outtermost occupied energy level of an atom is what determines size.
1075073
well it depends, but generally they don't stay that way for long. They react with other atoms that are charged opposite of whatever they are. This is how chemical bonds are formed. It can either be a covalent bond in which they atoms are "sharing" electrons in order for both to be neutrally charged or they form an Ionic bond.
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+
252404
An element is reactive because it is unstable.By reacting with other substances it tries to become stable.\nin case of metals or as u say positively charged elements,say,Li,Na,K...the atomic size is increasing on going down.As the size increases the the nuclear pull for the valence shell decreases,thereby making it easier to lose electrons.Thus,K easily loses electrons as compared to Na or Li and is therefore more reactive.\nin case of negatively charged atoms or non metals,the atomic size is again increasing for eg in case of F,Cl,Br..\nbut the case is opposite here.\nthe atom has to gain one electron in order to become stable.\nthe smaller the atom the more is the nuclear pull for the incoming electron and more readily it is accepted.\nthus in this case,reactivity decreases down the group.
1058444
Mg2+ < Na+ < Br-\n\nIon size depends first on the main quantum number. Na and Mg both strip down to the Ne configuration, while Br takes up the Xe configuration, two main quantum numbers higher.\n\nMg2+ is smaller than Na1+ because the remaining electrons are subject to a stronger electrostatic field.\n\nThe above is true for ions in crystal lattices.\n\nNote that in watery solutions ion size has to be calculated differently when you take the hydrate shell into account. Na+ becomes Na(H2O)6(1+), and Mg2+ becomes Mg(H2O)6(2+). Bromide won't take up a regular hydrate shell.