Question

1. differences in which subatomic particles are responsible for ions and isotopes? a. ions → protons, isotopes → electrons b. ions → electrons, isotopes → neutrons c. ions → neutrons, isotopes → protons d. ions → protons, isotopes → neutrons 23. boron - 10’s abundance is 19.8%, boron - 11’s is 80.2%. what is boron’s atomic mass? ave. atomic mass = \frac{(mass of isotope 1)(% abundance)+(mass of isotope 2)(% abundance)+(mass of isotope 3)(% abundance)}{100} a. 10.0 amu b. 10.2 amu c. 10.8 amu d. 11.0 amu

Explanation:

Step1: Recall ion and isotope concepts

Ions form when atoms gain or lose electrons. Isotopes are atoms of the same element with different numbers of neutrons.

Step2: Answer question 22

Based on the above - mentioned concepts, ions are related to electrons and isotopes are related to neutrons. So the answer to question 22 is B.

Step3: Calculate boron's atomic mass

The formula for average atomic mass is $A=\frac{(m_1\times p_1)+(m_2\times p_2)}{100}$, where $m_1$ and $m_2$ are the masses of isotopes and $p_1$ and $p_2$ are their percentages. Boron - 10 has a mass of 10 amu and an abundance of 19.8%, and boron - 11 has a mass of 11 amu and an abundance of 80.2%.
\[

$$\begin{align*} A&=\frac{(10\times19.8)+(11\times80.2)}{100}\\ &=\frac{198 + 882.2}{100}\\ &=\frac{1080.2}{100}\\ & = 10.802\approx10.8\text{ amu} \end{align*}$$

\]
So the answer to question 23 is C.

Answer:

1. B. Ions → electrons, Isotopes → neutrons
2. C. 10.8 amu