Indium has only two naturally occurring isotopes. the mass of indium-113 is 112.9041 amu and the mass of indium-115 is 114.9039 amu . part a use the atomic mass of indium to calculate the relative abundance of indium-113.

Isotopy is a phenomenon where by two or more atoms have the same atomic number but different mass number due to the difference in the neutron number of the atoms involved.

We can obtain the abundance of indium–113 as illustrated below:

Let indium–113 be isotope A

Let indium–115 be isotope B

From the question given above, the following data were obtained:

isotope A (indium–113):

Mass of A = 112.9041 amu

Isotope B (indium–115):

Mass of B = 114.9039 amu

Abundance of B (B%) = 100 – A%

Atomic mass of indium = 114.818 amu

Atomic mass = [(mass of A × A%)/100] +  [(mass of A × A%)/100]

114.818 = [(112.9041 × A%)/100] + [(114.9039 × (100 – A%)/100]

114.818 = 1.129041A% + 114.9039 – 1.149039A%

Collect like terms

114.818 – 114.9039 = 1.129041A%  – 1.149039A%

–0.0856 = –0.019998A%

Divide both side by –0.019998

A% = –0.0856 / –0.019998

Therefore, the relative abundance of indium–113 is 4.28%

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a chemical reaction

explanation:

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.