Question

part ii: fill in the chart with the missing information about the given isotopes. name notation notation mass number atomic # protons neutrons electrons boron - 14 14 5 b 14 5 5 9 5 135 55 x 135 53 55 80 55 134 54 y 134 54 54 80 54

Explanation:

Step1: Recall atomic - related concepts

The atomic number is equal to the number of protons. For a neutral atom, the number of electrons is equal to the number of protons. The mass number is the sum of the number of protons and neutrons. The notation for an isotope is $_{Z}^{A}X$, where $A$ is the mass number, $Z$ is the atomic number, and $X$ is the chemical symbol.

Step2: Analyze Boron - 14

Boron has an atomic number ($Z$) of 5. The mass number ($A$) is 14. The number of protons is equal to the atomic number, so there are 5 protons. The number of neutrons is $A - Z=14 - 5 = 9$. For a neutral atom, the number of electrons is equal to the number of protons, so there are 5 electrons. The notation is $_{5}^{14}B$.

Step3: Analyze the second isotope

The mass number $A = 135$, the number of protons is 55, so the atomic number $Z = 55$. The number of neutrons is $A - Z=135 - 55 = 80$. For a neutral atom, the number of electrons is 55. The element with atomic number 55 is Cesium (Cs), and the notation is $_{55}^{135}Cs$.

Step4: Analyze the third isotope

The mass number $A = 134$, the number of protons is 54, so the atomic number $Z = 54$. The number of neutrons is $A - Z=134 - 54 = 80$. For a neutral atom, the number of electrons is 54. The element with atomic number 54 is Xenon (Xe), and the notation is $_{54}^{134}Xe$.

Answer:

Name Notation	Notation	Mass Number	Atomic #	Protons	Neutrons	Electrons
Cesium - 135	$_{55}^{135}Cs$	135	55	55	80	55
Xenon - 134	$_{54}^{134}Xe$	134	54	54	80	54