NEON has 2 ISOTOPES of differing mass and in different proportions shown below. Which option demonstrates how we calculate its relative atomic mass (A_(r)) in g/mol {}^20Ne:91% {}^22Ne:9% ((91+9)times (20+22))/(100)=42 ((91times 9)+(20times 22))/(100)=12.6 ((91+20)times (9+22))/(100)=7.11 ((91times 20)+(9times 22))/(100)=20.2

Question

NEON has 2 ISOTOPES of differing mass and in different proportions shown below. Which option demonstrates how we calculate its relative atomic mass (A_(r)) in g/mol {}^20Ne:91% {}^22Ne:9% ((91+9)times (20+22))/(100)=42 ((91times 9)+(20times 22))/(100)=12.6 ((91+20)times (9+22))/(100)=7.11 ((91times 20)+(9times 22))/(100)=20.2

Answer 1

20.18 g/molThe relative atomic mass of Neon (Ne) is 20.18 g/mol. Among the options given, the correct calculation is \(\frac{(91 \times 20)+(9 \times 22)}{100}=20.2\), which is approximately equal to our calculated value.

Answer 2

## Step 1: Understand the problemThe problem is asking us to calculate the relative atomic mass of Neon (Ne). Neon has two isotopes, Ne-20 and Ne-22, with respective abundances of 91% and 9%. The relative atomic mass is calculated as the weighted average of the atomic masses of the isotopes, with the weights being the abundances of the isotopes.## Step 2: Identify the correct formulaThe correct formula for calculating the relative atomic mass is to multiply the atomic mass of each isotope by its abundance (expressed as a decimal), and then sum up these results.### Formula: \(A = (m_1 \times p_1) + (m_2 \times p_2)\)where:-

and

are the atomic masses of the isotopes,-

and

are the abundances of the isotopes (expressed as decimals).## Step 3: Substitute the values into the formulaSubstitute the atomic masses and abundances of the isotopes into the formula:### \(A = (20 \times 0.91) + (22 \times 0.09)\)## Step 4: Perform the calculationsMultiply the atomic masses by their respective abundances, and then add these results:###

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