Explain what is implied by most alpha particles passing straight through the foil.

Explain what is implied by a very small proportion of alpha particles being deflected through angles greater than $90^\circ$.

Calculate the ratio of the diameter of the atom to the diameter of the nucleus.

Explain why a diagram showing a visible nucleus inside an atom is not to scale.

State where most of the mass of an atom is found.

State why these atoms are isotopes of copper.

Determine the number of neutrons in each atom.

Explain why these isotopes have very similar chemical properties but may have slightly different physical properties.

Calculate the relative atomic mass, $A_r$, of element Y using these data.

Explain why the relative atomic mass is not a whole number.

State why the $m/z$ values correspond to the mass numbers of the magnesium isotopes.

The peaks occur at $m/z$ values 24, 25 and 26 with relative abundances $78.6\%$, $10.1\%$ and $11.3\%$, respectively. Calculate the relative atomic mass of magnesium.

Identify the most abundant isotope in the sample.

State what is represented by the height or area of each peak in an elemental mass spectrum.

The two peaks are at $m/z = 79$ and $m/z = 81$, with relative abundances $50.5\%$ and $49.5\%$, respectively. Calculate the relative atomic mass of bromine.

Explain what the two similar peak heights indicate about naturally occurring bromine.

State the most common outcome for the alpha particles.

Explain how the data support the nuclear model of the atom.

Suggest why increasing the foil thickness would increase the number of deflected alpha particles.

Deduce the number of protons, neutrons and electrons in ${}^{65}_{29}\text{Cu}^{2+}$.

Deduce the nuclear symbol for the species with 17 protons, 20 neutrons and 18 electrons.

Convert the atomic diameter of $2.0\times 10^{-10}\ \text{m}$ into picometres.

Calculate the ratio of the atomic diameter to the nuclear diameter, using $2.0\times 10^{-15}\ \text{m}$ for the nuclear diameter.

Explain why the student's drawing is not to scale and what this implies about atomic structure.

Let $x$ be the percentage abundance of the isotope with mass number 69. Write an expression for the relative atomic mass in terms of $x$.

Calculate the percentage abundance of each isotope.

State which isotope is more abundant and justify your answer.

The peaks are at $m/z = 35$ and $m/z = 37$ with relative abundances $75.8\%$ and $24.2\%$, respectively. Calculate the relative atomic mass of the unknown element.

Identify the unknown element using the data booklet values given.

Explain why the relative atomic mass is closer to 35 than to 37.

Explain why the intensities must be normalised before calculating the relative atomic mass.

Calculate the relative atomic mass of silicon from these data.

Define the term fragment ion.

Suggest the formula of the fragment ion at $m/z = 15$.

Explain how fragment ion peaks can help determine the structure of a compound.

Calculate the relative atomic mass, $A_r$, of element M using the data.

Explain why the value of $A_r$ is closest to 88.

Suggest why the calculated value may differ slightly from a value in a data booklet.

Identify the product that contains most of the $^{18}\text{O}$ label.

Suggest what the tracer result shows about the fate of the oxygen atom originally in $P-OH$.

Explain why an oxygen isotope can be used as a tracer in this experiment.

Describe the relationship shown in the graph.

Calculate the percentage decrease in relative rate from the lightest to the heaviest isotopic molecule.

Explain why isotopic molecules can have different physical properties but very similar chemical properties.

State what each peak in the spectrum represents.

Calculate the relative atomic mass of X from peaks at $m/z=79$ and $m/z=81$ with relative abundances of $50.5\%$ and $49.5\%$, respectively.

Explain why the peak positions can be treated as isotope mass numbers in this calculation.

Calculate the relative atomic mass from peaks at $m/z=28$, 29 and 30 with percentage abundances $92.2\%$, $4.7\%$ and $3.1\%$, respectively.

Identify the element if the data table lists aluminium, silicon and phosphorus with approximate $A_r$ values 26.98, 28.09 and 30.97.

Explain why there are three peaks in the elemental mass spectrum.

The lower and higher peaks occur at $m/z = 10$ and $m/z = 11$, respectively. Determine the percentage abundance of each isotope.

Calculate the relative atomic mass of the element in this sample.

Suggest one reason why this value may differ slightly from a data booklet value for the same element.

Convert the relative intensity of the peak at $m/z=24$ to a percentage abundance.

Calculate the relative atomic mass of Y using peaks at $m/z=24$, 25 and 26 with relative intensities 315, 40 and 45.

State why the most intense peak does not by itself give the relative atomic mass.

Calculate $A_r$ for sample A, which contains $75.0\%$ $^{35}\text{Cl}$ and $25.0\%$ $^{37}\text{Cl}$.

Calculate $A_r$ for sample B, which contains $60.0\%$ $^{35}\text{Cl}$ and $40.0\%$ $^{37}\text{Cl}$.

Compare the isotope composition of the two samples using the spectra.

Explain why the mass number of an atom is determined by the nucleus rather than by the electrons.

Compare the roles of protons, neutrons and electrons in determining the identity and charge of these particles.

Explain why ${}^{86}\text{Sr}^{2+}$ and ${}^{88}\text{Sr}^{2+}$ have very similar chemical properties.

Explain why the nucleus contains almost all the mass of a silicon atom but occupies only a tiny fraction of the atom's volume.

Deduce the mass numbers of the two isotopes if the observed peaks are at $m/z=32.0$ and $m/z=33.0$.

Calculate the relative atomic mass of Z if the relative abundances of the two peaks are $69.1\%$ and $30.9\%$, respectively.

Suggest the error in calculating $A_r$ directly from the observed $m/z$ values.

Calculate $A_r$ using the peak areas for isotopes with masses 10 and 11. The integrated areas are 40 and 60, respectively.

The student used peak heights of 40 and 30 for the same two isotopes. Calculate the value of $A_r$ the student would obtain.

Evaluate the student's method for this spectrum.

Calculate the relative atomic mass, $A_r$, of X using the data in the table.

Another sample contains only ${}^{50}\text{X}$ and ${}^{52}\text{X}$ and has $A_r = 51.70$. Calculate the percentage abundance of ${}^{50}\text{X}$ in this sample.

Suggest why a sample enriched in ${}^{53}\text{X}$ could have a slightly different density from a natural sample of X.

Explain why ${}^{18}\text{O}$-labelled water can be used as a tracer in this experiment.

Evaluate the conclusion that the oxygen atoms in the oxygen gas product come from water rather than carbon dioxide.

Explain why the relative atomic mass of chlorine is not a whole number and why a value calculated using mass numbers may differ slightly from a data booklet value.

Discuss whether ${}^{35}\text{Cl}$ and ${}^{37}\text{Cl}$ have identical chemical and physical properties.

Identify the element using the calculated relative atomic mass and the isotope pattern.

Discuss three limitations or assumptions involved in using this mass spectrum to determine a data booklet value of $A_r$.

Compare the spectra of samples A and B and evaluate whether the samples have the same isotopic composition.

Explain why the two boron samples can have different mass spectra but very similar chemical reactions.

Calculate the average relative molecular mass of $\text{CH}_3\text{Br}$ using $A_r(\text{C})=12.01$, $A_r(\text{H})=1.01$ and $A_r(\text{Br})=79.90$.

Discuss how the fragment ion peaks support the proposed composition of the compound.

Explain why the calculated $A_r$ is not exactly equal to the $m/z$ value of either peak.

A second copper sample has a higher calculated $A_r$ than this sample. Suggest one change in isotopic composition that could explain this.