Question

element name,isotopic notation,mass # (whole numbers only),atomic mass (comes from pt),atomic #,# of protons,# of electrons,# of neutrons; lead,\ce{^{208}_{82}pb},208,207.2,82,82,82,26

Explanation:

Step 1: Recall Isotope Basics

For an isotope \( ^{A}_{Z}\text{X} \), \( A \) is mass number (protons + neutrons), \( Z \) is atomic number (protons = electrons in neutral atom), atomic mass is from periodic table, neutrons = \( A - Z \).

Step 2: Analyze Lead Isotope \( ^{208}_{82}\text{Pb} \)

• Mass #: Given as \( 208 \) (whole number from notation).
• Atomic Mass: From PT, lead (Pb) has atomic mass \( 207.2 \).
• Atomic # (\( Z \)): From notation, \( Z = 82 \) (bottom number).
• # of protons: \( = Z = 82 \) (protons = atomic number).
• # of electrons: In neutral atom, electrons = protons = \( 82 \).
• # of neutrons: \( = \text{Mass #} - \text{Atomic #} = 208 - 82 = 126 \).

Answer:

Element Name	Isotopic Notation	Mass #	Atomic Mass	Atomic #	# of protons	# of electrons	# of neutrons

(Note: The original "26" for neutrons was incorrect; correct calculation gives 126.)