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→Calculating the number of Neutrons
{| class="wikitable"
| style="height:20px; width:300px; text-align:center;" |Calculate the number of [[neutron]]s in an [[isotope]] of [[Titanium]] with a [[Atomic Nucleus|nucleus]] of '''specific charge''' 4.58x10<sup>7</sup>Ckg<sup>-1</sup>.
| style="height:20px; width:300px; text-align:center;" |Calculate the number of [[neutron]]s in an [[isotope]] of [[Neon]] with the '''specific charge''' of -2.46x10<sup>6</sup>Ckg<sup>-1</sup> for a [[Selenium|Selenium 2-]] [[ion]].
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| style="height:20px; width:300px; text-align:left;" |'''1. State the known quantities in [[SI Unit]]s.'''
| style="height:20px; width:300px; text-align:left;" |'''1. State the known quantities in [[SI Unit]]s.'''
<math>S.C. = -2.46\times10^{6}</math>Ckg<sup>-1</sup>
A 2- [[ion]] has two more [[electron]]s than [[proton]]s giving it a [[Negative Charge|negative charge]].
<math>Q = -2\times1.60\times10^{-19}</math>C
<math>m = (z + n)\times1.67\times10^{-27}+(z+2)\times9.11\time10^{-31}</math>kg
Where z is the number of [[proton]]s, n is the number of [[neutron]]s, (z+n) is the [[Relative Atomic Mass|relative atomic mass]] and (z+2) is the number of [[electron]]s since there are two more [[electron]]s than [[proton]]s.
Therefore
<math>m = (34 + n)\times1.67\times10^{-27}+36\times9.11\time10^{-31}</math>kg
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| style="height:20px; width:300px; text-align:left;" |'''2. [[Substitute (Maths)|Substitute]] the numbers and [[Evaluate (Maths)|evaluate]].'''