Question

part a
an isotope represented as s - 34:
is an isotope of sodium.
contains exactly 18 neutrons.
must have exactly 18 electrons.
has 34 protons.
none of the above
submit request answer

Explanation:

Step1: Analyze the symbol S - 34

The symbol S represents sulfur. The number 34 is the mass number.

Step2: Recall the atomic number of sulfur

The atomic number of sulfur (S) is 16. So, the number of protons \(p = 16\).

Step3: Calculate the number of neutrons

The formula for the mass number \(A\) is \(A=p + n\) (where \(n\) is the number of neutrons). Given \(A = 34\) and \(p=16\), then \(n=A - p=34 - 16 = 18\). But this is only for a neutral atom. However, the problem does not specify if it is a neutral atom. If it is an ion (e.g., \(S^{2-}\)), the number of electrons changes.

Step4: Check each option

• Option 1: S is sulfur, not sodium (Na).
• Option 2: Only if it is a neutral atom, but not specified.
• Option 3: Only if it is a neutral atom (for neutral \(S\), electrons \(e=p = 16\)).
• Option 4: Protons \(p = 16

eq34\).

Answer:

none of the above