Final answer:
The particle with an equal number of protons and neutrons and the given electronic structure is none of the options provided.
Step-by-step explanation:
In the given electronic structure 1s² 2s² 2p 3s² 3p6, we can determine the number of protons and neutrons of the particle. The number of protons is equal to the atomic number, which is the number after the element's symbol in the periodic table. The number of neutrons can be calculated by subtracting the atomic number from the mass number of the element. The given electronic structure represents the electron configuration of the element. Now, let's look at the options to find the particle that satisfies both conditions.
A) 18 Ar - Argon has an atomic number of 18, which means it has 18 protons. However, its mass number is 40, which means it has a different number of neutrons.
B) Ca²+ - Calcium has an atomic number of 20, but the calcium ion (Ca²+) loses two electrons, so it does not have the same electronic structure as the given one.
C) ¹60²- - This particle has 60 protons and 62 neutrons, but its electronic structure is not the same as the given one.
D) 16- - This particle has 16 protons and 0 neutrons, but the electron configuration does not match the given one.
Therefore, none of the options match the particle with an equal number of protons and neutrons and the given electron configuration. The correct answer is none of the above.
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