IB Chemistry HL 1.2 The Nuclear Atom Questions

Practise IB Chemistry HL 1.2 by reading nuclear symbols, comparing isotope behaviour and using m/z peak patterns to calculate relative masses.

Exam points

Use nuclear notation to find proton, neutron and electron counts, mass number and ionic charge.
Identify isotopes from nuclear notation and calculate relative atomic mass from isotope-abundance data.
Read m/z peaks and intensities to identify isotopes, explain diatomic patterns and calculate relative molecular mass.

[Maximum number: 3]

Titanium and vanadium are consecutive elements in the first transition metal series.

(a)

Titanium exists as several isotopes. The mass spectrum of a sample of titanium gave the following data:

Calculate the relative atomic mass of titanium to two decimal places.

[ 2 ]

$\frac{(46\times7.98)+(47\times7.32)+(48\times73.99)+(49\times5.46)+(50\times5.25)}{100} =47.93$

Answer must have two decimal places with a value from 47.90 to 48.00.

(b)

State the number of protons, neutrons and electrons in the ${ }_{22}^{48} \mathrm{Ti}$ atom.

Protons:

......

Neutrons:

......

Electrons:

......

[ 1 ]

[Maximum number: 3]

Magnesium is a group 2 metal which exists as a number of isotopes and forms many compounds.

(a)

State the nuclear symbol notation, ${ }_{Z}^{A} X$ , for magnesium-26.

[ 1 ]

${ }_{12}^{26} \mathrm{Mg}$

(b)

Mass spectroscopic analysis of a sample of magnesium gave the following results:

Calculate the relative atomic mass, $A_{\mathrm{r}}$ , of this sample of magnesium to two decimal places.

[ 2 ]

$A_r=\frac{24(78.60)+25(10.11)+26(11.29)}{100} =24.3269 =24.33$

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