OK, both metals and nonmetals start off with neutral charges. When they're ionized, nonmetals tend to gain electrons because the nonmetals easiest to ionize tend to be halogens--fluorine, chlorine and points south--and they only need one electron for a full octet. (I'm assuming you know about the octet rule, but for nonchemists, the short version is, the stablest ions have the same numbers of electrons as a noble gas. For instance, F- has the same number of electrons as Ne.)
The alkali and alkaline earth metals only have one or two valence electrons, so if they lose them, they end up with the electron configuration of the next-lower noble gas. For instance, Li+ is isoelectronic with He.
The tricky part, and the part you seem to be having trouble with, is the transition metals. They are right in the middle of the periodic table, with too many electrons to lose enough for noble gas configurations and too few to gain enough. They are also large enough to have a d-subshell of electrons. So instead of trying to get the whole shell full or empty, they just try to stabilize the d-subshell. It's most stable if it is empty or half-full, so the metal ions tend to lose electrons to get to that state.
I'm not sure why transition metals always form positive ions and not negative ones, except that it's pretty difficult to get more than one extra electron on a single atom, whereas many transition metal ions can lose multiple electrons.
2006-12-18 12:56:53
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answer #1
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answered by Amy F 5
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number of protons will always be the same. It is all about the electrons and electrons have negative value so let me give you example...
lithium atom has 3 protons and 3 electrons charge = 0
but lithium ion has 3 protons and 2 electrons so the charge =+1 because of that missing that one electron
It works the other way around chlorine atom has 17 protons and 17 electrons so the charge =0
but chlorine ion has 17 protons and 18 electrons charge will=-1
Just remember protons are positive charge and electrons are negative charge so when atom gains electron(s) it becomes negatively charge and vice versa
2006-12-18 12:59:29
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answer #2
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answered by krucha 2
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I think you should look into the concept of electronegativity. Basically, metals don't hold onto their electrons as strongly and nonmetals can attract these electrons. Very simplified version, but check out a textbook for a full explanation of ionization energies and electron affinities.
2006-12-18 12:47:07
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answer #3
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answered by Phil 5
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Each atom has a tendency to reach the most stable state, which is to have a completely filled outer shell of electrons. It is energetically more favorable to lose electrons to reach that state for metals, and gaining electrons are also more energetically favorable for non-metals to reach that state.
2006-12-18 12:48:31
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answer #4
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answered by yungr01 3
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i will see the place they're coming from. destructive ions can %. up the advantageous H+ ions, which ability they're effortless. although, this does not inevitably neutralise them; that relies upon on the backside capability of the anion. additionally, it makes me ask your self what the counterion is going to be, seeing as ions won't be able to usually exist on their very own. by choosing up H+, besides, you create acidic compounds. What result might they have, and how are you able to scrub the necklace from them? I surely have my doubts with regard to the applications of this component.
2016-12-30 15:13:00
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answer #5
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answered by ? 4
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They don't have extra protons, they have less electrons. That's all.
2006-12-18 12:45:46
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answer #6
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answered by Anonymous
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well its doesn't seem like you are convfused. i don't understna dwhat you are asking. you seem to understnad it. i am learning about that too in scince. i actually have my exam tomorrow
2006-12-18 12:51:14
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answer #7
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answered by emile 2
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