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  LiveWire / Teen Forums / School & Homework Connection / Viewing Topic

Can someone explain this please? (science)
Replies: 11Last Post Sep. 14, 2008 9:18pm by MrIndigo
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( ukichik )


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I don't need you to do my homework so explain something. So we're learning compounds in class and we have to write a chemical formula when given a chemical name. I understand that but I don't understand how do you know when an electron "leaves" or "comes" to form an ion (a complete circle of 8 electrons in outer shell)
Can someone explain please?

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2:07 pm on Sep. 14, 2008 | Joined: Aug. 2007 | Days Active: 32
Join to learn more about ukichik Ontario, Canada | Straight Female | Posts: 79 | Points: 404
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Ancient Rights


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When an electron leaves or comes it is an ionic bond. Generally ionic bonds form between metals and nonmetal.

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1, 2, 4, 8, 16, 32, 64, 128, 256, 512, 1024, 2048, 4096, 8192, 16384,
32768, 65536, 131072, 262144, 524288, 1048576, 2097152, 4194304, 8388608,
16777216, 33554432, 67108864, 134217728, 268435456, 536870912, 1073741824,
2147483648, 4294967296

2:08 pm on Sep. 14, 2008 | Joined: May 2006 | Days Active: 821
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Angel Star


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im doing the same thing in science
i think that the electrons are always there cause a atom (ion) is made up of neutrons, electrons and protons.

2:10 pm on Sep. 14, 2008 | Joined: July 2006 | Days Active: 38
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Arcarius


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I think it's that metals want to give away electrons and non-metals want to take them

Electro negativity and ionization energy

Post edited at 2:12 pm on Sep. 14, 2008 by Arcarius

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2:10 pm on Sep. 14, 2008 | Joined: June 2008 | Days Active: 147
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( ukichik )


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nooo
i mean how do you know when if for example you need 5 electrons (because theres only 3 in the outer shell) , how do you know if you ADD 5 or SUBTARCT 3?

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2:11 pm on Sep. 14, 2008 | Joined: Aug. 2007 | Days Active: 32
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Arcarius


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Quote: from ukichik at 5:11 pm on Sep. 14, 2008

nooo
i mean how do you know when if for example you need 5 electrons (because theres only 3 in the outer shell) , how do you know if you ADD 5 or SUBTARCT 3?

Well non-metals take electrons, so I guess you add to them.

Metals give them away so you subtract?

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2:12 pm on Sep. 14, 2008 | Joined: June 2008 | Days Active: 147
Join to learn more about Arcarius New York, United States | Straight Male | Posts: 2,562 | Points: 5,377
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ok
thanks:D:D:D

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2:15 pm on Sep. 14, 2008 | Joined: Aug. 2007 | Days Active: 32
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icecalay


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Okay, the groups 1, 2, and 3 will need to loose a certain number of electrons. The groups 5, 6, and 7 will need to gain electrons for a full outer shell. Get it? Just say if you need more explaination.

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2:15 pm on Sep. 14, 2008 | Joined: Sep. 2008 | Days Active: 1
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marshmellowman


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An element in it's normal state doesn't always have a full outer shell, in fact it rarely does. Those that do are called the halogens and are in group 8 (or 0).

An element always tries to reach it's most stable state, and it can achieve this by having a full outer shell. To do this an element can either gain electrons or lose electrons. For those with less than 4 electrons in its outer shell, it is simpler and takes less energy to lose the electrons and get a full outer shell (it being the second outer shell - now the first) than it would to gain electrons and get a full outer shell.

Conversely it takes less energy for elements with more than four electrons in their outer shell to gain electrons and get a full shell than it does for them to lose the electrons. Elements with exactly 4 electrons can go either way.

When an element loses or accepts electrons it forms an ion, because the number of protons are not the same as the number of electrons. When it loses electrons it forms a positive charge, when it gains electrons it forms a negative charge.

For example Magnesium contains 2 electrons in its outer shell (being in group 2), so it loses two electrons to form its ion - Mg2+. Chlorine however has 7 electrons in its outer shell, so it gains one electron to become the ion Cl-.

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2:16 pm on Sep. 14, 2008 | Joined: Feb. 2007 | Days Active: 763
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thanks everyone
even though yuo all gave different explanations
:P

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2:32 pm on Sep. 14, 2008 | Joined: Aug. 2007 | Days Active: 32
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MrIndigo


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" I understand that but I don't understand how do you know when an electron "leaves" or "comes" to form an ion (a complete circle of 8 electrons in outer shell) "

"a complete circle of 8 electrons in outer shell" wrong definition.. don't use that.

Draw the electron configuration diagram is a much better way to determine a molecule is electron deficient or not.

If a bond forms, then the electron will be close to the more ELECTRONEGATIVE element. ionic and covalent is simply made up by people to simply the bond types for beginners. Ionic bonds are when the electronegativity of the two bonding atoms are so great that the electron is just really close to the other atom.
Also.. ionic atoms can dissociate:P

Basically, you put the negative charge on the more electronegative atom... if they are not in the ionic range, then just put the partial negative charge on the more electronegative  atom.


9:18 pm on Sep. 14, 2008 | Joined: May 2008 | Days Active: 90
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