Question

1. use the mass spectrum below to fill out the information in the table about each isotope.

Explanation:

To solve this, we analyze the mass spectrum and table:

Step 1: Identify Isotopes (m/z values)

From the spectrum, the \( m/z \) (mass) values are 86, 87, 88, and 92 (assuming the tallest peak is 88 with 82.58% abundance, 86 with ~0.59%, 87 with ~7.06%, and 92? Wait, the table and spectrum show:

• Isotope 1: \( m/z = 86 \), Relative Abundance ≈ 0.59%
• Isotope 2: \( m/z = 87 \), Relative Abundance ≈ 7.06%
• Isotope 3: \( m/z = 88 \), Relative Abundance = 82.58%
• (Maybe 92? But focus on visible peaks.)

Step 2: Protons (Atomic Number)

Assume the element is Strontium (Sr, atomic number 38) (common for these masses). So protons = 38 for all isotopes.

Step 3: Neutrons (Mass Number − Protons)

• For \( \text{Mass} = 86 \): Neutrons = \( 86 - 38 = 48 \)
• For \( \text{Mass} = 87 \): Neutrons = \( 87 - 38 = 49 \)
• For \( \text{Mass} = 88 \): Neutrons = \( 88 - 38 = 50 \)

Step 4: Mass (amu) and Relative Abundance

• Isotope \( ^{86}\text{Sr} \): Mass = 86 amu, Abundance ≈ 0.59%
• Isotope \( ^{87}\text{Sr} \): Mass = 87 amu, Abundance ≈ 7.06%
• Isotope \( ^{88}\text{Sr} \): Mass = 88 amu, Abundance = 82.58%

Filling the Table (Example for \( ^{88}\text{Sr} \)):

Isotope	Protons	Neutrons	Mass (amu)	Relative Abundance (%)

(Repeat for other isotopes using \( \text{Neutrons} = \text{Mass} - 38 \) and given abundances.)

Answer:

For the isotope with mass 88 amu (most abundant):

• Protons: 38
• Neutrons: 50
• Mass: 88 amu
• Relative Abundance: 82.58%

(Adjust for other isotopes using the same logic.)