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: The number of [[electron]] in an [[ion]] can be found using the [[Atomic Number]] (which is the same as the [[Relative Atomic Charge]] of the [[Atomic Nucleus|nucleus]]) and subtracting the [[charge]] of the [[ion]].
{| class="wikitable"
| style="height:20px; width:200px; text-align:center;" |'''A Lithium Ion'''
| style="height:20px; width:200px; text-align:center;" |'''A Fluorine Ion'''
| style="height:20px; width:200px; text-align:center;" |'''A Boron Ion'''
| style="height:20px; width:200px; text-align:center;" |'''An Oxygen Ion '''
|-
|[[File:LithiumIonSymbol.png|center|200px]]
|[[File:FluorineIonSymbol.png|center|200px]]
|[[File:BoronIonSymbol.png|center|200px]]
|[[File:OxygenIonSymbol.png|center|200px]]
|-
| style="height:20px; width:200px; text-align:left;" |This [[atom]] has an [[Atomic Number]] (Z) of 3 and a [[Relative Atomic Charge]] (Q) of +1.
Number of [[electron]]s = A - Q
Number of [[electron]]s = 3 - 1
Number of [[electron]]s = 2
| style="height:20px; width:200px; text-align:left;" |This [[atom]] has an [[Atomic Number]] (Z) of 9 and a [[Relative Atomic Charge]] (Q) of -1.
Number of [[electron]]s = A - Q
Number of [[electron]]s = 9 - (-1)
Number of [[electron]]s = 10
| style="height:20px; width:200px; text-align:left;" |This [[atom]] has an [[Atomic Number]] (Z) of 5 and a [[Relative Atomic Charge]] (Q) of +3.
Number of [[electron]]s = A - Q
Number of [[electron]]s = 5 - 3
Number of [[electron]]s = 2
| style="height:20px; width:200px; text-align:left;" |This [[atom]] has an [[Atomic Number]] (Z) of 8 and a [[Relative Atomic Charge]] (Q) of -2.
Number of [[electron]]s = A - Q
Number of [[electron]]s = 8 - (-2)
Number of [[electron]]s = 10
|}