IB Chemistry HL Structure 1 Models of the Particulate Nature of Matter Questions

Practise IB Chemistry HL 1 Particulate Matter with HL questions on atomic structure and spectra.

Exam points

Classify matter and use particle models, state symbols and Kelvin temperature to explain physical behaviour.
Use nuclear symbols, isotopic data and mass spectra to determine particle counts and nuclide information.
Interpret emission spectra, electron configurations, orbitals and ionization-energy data using quantized energy levels.
Convert between amount of substance, particles, mass, formulae and concentration, and apply gas-quantity relationships.
Use the ideal-gas equation and molar-volume relationships, and explain deviations from ideal behaviour.

Covered syllabus points

1.1 Introduction to the particulate nature of matter 1.2 The nuclear atom 1.3 Electron configurations 1.4 The mole 1.5 Ideal gases

Learn this topic

Study Structure 1. Models of the particulate nature of matter conceptsOpen the corresponding Concept lesson for explanations, examples and exam connections.

[Maximum number: 5]

Iron(II) sulfide can be produced by heating powdered iron and sulfur together.

(a)

Describe the difference between an element and a compound.

[ 2 ]

(b)

Calculate the wavelength, in m , for the limit of convergence observed in the line spectrum of iron. Use sections 1, 2 and 9 of the data booklet.

[ 3 ]

$\begin{array}{ll} \left\langle<I E(\mathrm{Fe})=762 \mathrm{~kJ} \mathrm{~mol}^{-1} \|\right. E \text { for } 1 \text { atom } \ll=\frac{762 \times 10^{3} \mathrm{~J} \mathrm{~mol}^{-1}}{6.02 \times 10^{23} \mathrm{~mol}^{-1}}> =1.266 \times 10^{-18} \langle\mathrm{~J}\rangle \mathrm{f}\left\langle<=\frac{E}{h}=\frac{1.266 \times 10^{-18} \mathrm{~J}}{6.63 \times 10^{-34} \mathrm{Js}} \|=1.91 \times 10^{15} \ll \mathrm{~S}^{-1}>\right. \lambda<=\frac{c}{f}=\frac{3.0 \times 10^{8} \mathrm{~m} \mathrm{~s}^{-1}}{1.91 \times 10^{15} \mathrm{~s}^{-1}}>= \end{array}$

Award [3] for correct final
answer.

[Maximum number: 5]

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:

Table for Question (a) — IB Chemistry HL

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 ]

(c)

State the full electron configuration of the ${ }_{22}^{48} \mathrm{Ti}^{2+}$ ion.

[ 1 ]

$1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 3 \mathrm{~d}^{2}$

(d)

Sketch a graph of the first six successive ionization energies of vanadium on the axes provided.

Figure for Question (d) — IB Chemistry HL

[ 1 ]

[Maximum number: 2]

Carbon is produced by fusion reactions in stars.

(a)

Outline how the spectra of light from stars can be used to detect the presence of carbon.

[ 1 ]

(b)

The main fusion reaction responsible for the production of carbon is:

\mathbf{X}+{ }_{2}^{4} \mathrm{He} \rightarrow{ }_{6}^{12} \mathrm{C}

[ 1 ]

(i)

Deduce the identity of X.

[ 1 ]

${ }_{4}^{8} \mathrm{Be}$

[Maximum number: 1]

How much ethanol contains $1.20 \times 10^{24}$ atoms of carbon?

Avogadro's constant, L or $N_{\mathrm{A}}: 6.02 \times 10^{23} \mathrm{~mol}^{-1}$

$0.333 \mathrm{~mol}$

$0.500 \mathrm{~mol}$

$1.00 \mathrm{~mol}$

$2.00 \mathrm{~mol}$

All question bank results loaded

Covered syllabus points

Learn this topic

Question 1

Question (a)

Question (b)

Question 2

Question (a)

Question (b)

Question (c)

Question (d)

Question 3

Question (a)

Question (b)

Question (i)

Question 4