Question

Given the following information regarding the masses and relative abundances for the isotopes of an element, determine its atomic mass and its atomic symbol. (5 pts) Isotope mass amu) Relative abundance 57.9353 58.9332 60.9310 61.9283 63.9280 68.274% 26.095% 1.134% 3.593% 0.904%

Answer 1

Average atomic mass = 58.51047 amu

The symbol is
`Ni`

Step-by-step explanation:

The formula for the calculation of the average atomic mass is:

`Average\ atomic\ mass=(\frac {\%\ of\ the\ first\ isotope}{100}* {Mass\ of\ the\ first\ isotope})+(\frac {\%\ of\ the\ second\ isotope}{100}* {Mass\ of\ the\ second\ isotope})+(\frac {\%\ of\ the\ third\ isotope}{100}* {Mass\ of\ the\ third\ isotope})+(\frac {\%\ of\ the\ fourth\ isotope}{100}* {Mass\ of\ the\ fourth\ isotope})+(\frac {\%\ of\ the\ fifth\ isotope}{100}* {Mass\ of\ the\ fifth\ isotope})`

Given that:

For first isotope:

% = 68.274 %

Mass = 57.9353 amu

For second isotope:

% = 26.095 %

Mass = 58.9332 amu

For third isotope:

% = 1.134 %

Mass = 61.9283 amu

For fourth isotope:

% = 3.593 %

Mass = 63.9280 amu

For fifth isotope:

% = 0.904 %

Mass = 63.9280 amu

Thus,

`Average\ atomic\ mass=(68.274)/(100)* {57.9353}+(26.095)/(100)* {58.9332}+(1.134)/(100)* {61.9283}+(3.593)/(100)* {63.9280}+(0.904)/(100)* {63.9280}`

`Average\ atomic\ mass=39.55474 +15.37861854+0.702266922+2.29693304+0.57790912`

Average atomic mass = 58.51047 amu

The symbol is
`Ni`