An element X has four naturally occurring isotopes, with natural abundances and masses outlined in the table below. Mass (a.m.u) Natural Abundance (%)21.00 45.50 %23.00 32.00 %24.00 12.60 %26.00 9.90 %Calculate the atomic mass of element X, to two decimal places.

A fictional element has two naturally occurring isotopes with the natural abundances shown here: ATOMIC MASS (AMU) ABUNDANCE1650.0%1850.0% Which statement is TRUE for this element?Group of answer choicesThe atomic mass would be 16.The atomic mass would be less than 16.The atomic mass would be 18.The atomic mass would be more than 18.The atomic mass would be 17.

lement X has two isotopes. Their mass numbers are 69 and 71 The percentage abundance of each isotope is: • 60% of 69 X • 40% of 71 X Estimate the relative atomic mass of element X. [1 mark] Tick one box. < 69.5 Between 69.5 and 70.0 Between 70.0 and 70.5 > 70.5

A fictional element named Schwartzium is found to have two naturally occurring isotopes with the natural abundances shown here:          Mass (amu)         % Abundance           32.3456                   65%           31.7812                   35% The calculated atomic mass (in amu) of Schwartzium is (place only a numerical answer, no units, in the following box):Group of answer choices32.3456 amu31.7812 amu31.9787 amu32.1481 amuinsufficient information provided to answer question

The Atomic  of an element indicates the average mass number for an atom and its isotopes and will therefore include one or more  places.

Define the terms mass number (A), atomic number (Z) and isotopes of an element