a) Define: i) Atomic number ii) Mass number. b) Calculate the relative atomic mass of element X. c) Define…

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a) Define: i) Atomic number ii) Mass number. b) Calculate the relative atomic mass of element X. c) Define the term isotopes.

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6. a) Define: i) Atomic number The atomic number (Z) is the number of protons in the nucleus of an atom. It determines the chemical identity of an element. ii) Mass number The mass number (A) is the total number of protons and neutrons in the nucleus of an atom. 6. b) Calculate the relative atomic mass of element X. Step 1: Identify the mass numbers and abundances of the isotopes. Isotope X1: Mass number = 35, Abundance = 75%; Isotope X2: Mass number = 37, Abundance = 25% Step 2: Use the formula for relative atomic mass. Relative atomic mass is the weighted average of the mass numbers of its isotopes. Relative atomic mass = (mass of isotope 1 × fractional abundance 1) + (mass of isotope 2 × fractional abundance 2); Relative atomic mass = (35 × 0.75) + (37 × 0.25) Step 3: Perform the calculation. Relative atomic mass = 26.25 + 9.25; Relative atomic mass = 35.5 The relative atomic mass of element X is 35.5. 6. c) Define the term isotopes. Isotopes are atoms of the same element that have the same number of protons (atomic number) but different numbers of neutrons, resulting in different mass numbers.

A) Define: i) Atomic number ii) Mass number. b) Calculate the relative atomic mass of element X. c) Define the term isotopes.

Answer

Step-by-step solution

Part i

Part ii· 3 steps
$\text{35.5}$

Identify the mass numbers and abundances of the isotopes.

Use the formula for relative atomic mass.

Perform the calculation.

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