Question

select the subatomic composition of a strontium ion (sr²⁺) with a mass number of 88. refer to a periodic table. 38 protons, 50 neutrons, 36 electrons 38 protons, 50 neutrons, 38 electrons 50 protons, 38 neutrons, 38 electrons 50 protons, 38 neutrons, 36 electrons

Explanation:

Step1: Determine the atomic number of strontium

From the periodic table, the atomic number of strontium (Sr) is 38. The atomic number is equal to the number of protons, so the number of protons in Sr is 38.

Step2: Calculate the number of neutrons

The mass - number formula is $Mass\ number=Number\ of\ protons + Number\ of\ neutrons$. Given the mass number is 88 and the number of protons is 38. So, $Number\ of\ neutrons=Mass\ number - Number\ of\ protons=88 - 38=50$.

Step3: Determine the number of electrons in the ion

A $Sr^{2 + }$ ion means that the strontium atom has lost 2 electrons. A neutral strontium atom has 38 electrons (equal to the number of protons). So, the number of electrons in $Sr^{2+}$ is $38 - 2=36$.

Answer:

38 protons, 50 neutrons, 36 electrons