Question

1. complete the following chart: isotope name atomic # mass # # of protons # of neutrons # of electrons 92 uranium-235 92 235 92 92 uranium-238 92 92 5 boron-10 5 10 5 3 5 5 boron-11 5 10.81 5 4 6

Explanation:

Step1: Recall neutron - proton relationship

The mass number ($A$) is the sum of the number of protons ($p$) and neutrons ($n$), i.e., $A=p + n$. The number of electrons in a neutral atom is equal to the number of protons.

Step2: Calculate neutrons for uranium - 235

For uranium - 235 with atomic number $Z = 92$ (number of protons) and mass number $A=235$, the number of neutrons $n=A - p=235 - 92 = 143$. The number of electrons is equal to the number of protons, so it is 92.

Step3: Calculate neutrons for uranium - 238

For uranium - 238 with atomic number $Z = 92$ (number of protons) and mass number $A = 238$, the number of neutrons $n=A - p=238 - 92=146$. The number of electrons is 92.

Step4: Correct boron - 10 values (if wrong)

For boron - 10 with atomic number $Z = 5$ (number of protons) and mass number $A = 10$, the number of neutrons $n=A - p=10 - 5 = 5$. The number of electrons is 5.

Step5: Correct boron - 11 values (if wrong)

For boron - 11 with atomic number $Z = 5$ (number of protons) and mass number $A = 11$, the number of neutrons $n=A - p=11 - 5 = 6$. The number of electrons is 5.

Answer:

Isotope name	atomic #	mass #	# of protons	# of neutrons	# of electrons
92 uranium - 238	92	238	92	146	92
5 boron - 10	5	10	5	5	5
5 boron - 11	5	11	5	6	5