Question

part d
an atom of sulfur is represented by $\ce{^{33}_{16}s}$. how many neutrons are in the nucleus of this atom?
express your answer as an integer.
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neutrons in $\ce{^{33}_{16}s} = $
submit

part e
give the nuclear symbol for the isotope of argon for which $a = 38$ ?
enter the nuclear symbol for the isotope (e.g., $\ce{^4_2he}$) using the stacked super/subscript template.
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Explanation:

Part D

Step1: Recall neutron calculation formula

The number of neutrons ($N$) in an atom is given by $N = A - Z$, where $A$ is the mass number (top number in the nuclear symbol) and $Z$ is the atomic number (bottom number in the nuclear symbol).

Step2: Identify $A$ and $Z$ for $\ce{^{33}_{16}S}$

For $\ce{^{33}_{16}S}$, $A = 33$ and $Z = 16$.

Step3: Calculate number of neutrons

Substitute $A = 33$ and $Z = 16$ into the formula: $N = 33 - 16 = 17$.

Step1: Recall nuclear symbol format

The nuclear symbol is written as $\ce{^{A}_{Z}X}$, where $X$ is the element symbol, $A$ is the mass number, and $Z$ is the atomic number.

Step2: Determine $Z$ for argon

Argon has an atomic number $Z = 18$ (from the periodic table).

Step3: Determine $A$ for the isotope

Given $A = 38$ for the argon isotope.

Step4: Write the nuclear symbol

Using the format $\ce{^{A}_{Z}X}$ with $X = \ce{Ar}$, $A = 38$, and $Z = 18$, the nuclear symbol is $\ce{^{38}_{18}Ar}$.

Answer:

17

Part E