Question

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

• For an isotope \(S - 34\):
• The atomic number of sulfur (\(S\)) is \(16\). In a neutral atom, the number of electrons equals the atomic number. So, a neutral \(S\) atom has \(16\) electrons, not \(18\).
• The symbol \(S\) stands for sulfur, not sodium (\(Na\)).
• The atomic number (\(Z\)) of sulfur is \(16\) (number of protons). The mass number (\(A=34\)). The number of neutrons \(N=A - Z=34 - 16 = 18\) only if the atom is neutral and we are talking about the most common isotope - but the problem does not specify it's a neutral atom. If it is an ion (e.g., \(S^{2-}\)), the electron number changes. Also, the question is about general properties of the isotope \(S - 34\) (the notation \(X - A\) where \(X\) is the element symbol and \(A\) is the mass number). The key is that just from \(S - 34\) (assuming it's a neutral atom for neutron - proton - electron relations, but the first three options are factually wrong in their general statements).

Answer:

none of the above