DP Chemistry Questionbank

State the full electron configuration of the chlorine atom.

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.

State the number of protons, neutrons and electrons in each species.

State the number of protons, neutrons and electrons in each species.

Natural uranium needs to be enriched to increase the proportion of ²³⁵U. Suggest a technique that would determine the relative abundances of ²³⁵U and ²³⁸U.

Subsequent experiments showed electrons existing in energy levels occupying various orbital shapes.

Sketch diagrams of 1s, 2s and 2p.

State the electron configuration of a bromine atom.

What is represented by A in ${}_{\text{Z}}^{\text{A}}{\text{X}}^{2-}$?

A. Number of electrons

B. Number of neutrons

C. Number of nucleons

D. Number of protons

When calcium compounds are introduced into a gas flame a red colour is seen; sodium compounds give a yellow flame. Outline the source of the colours and why they are different.

When calcium compounds are introduced into a gas flame a red colour is seen; sodium compounds give a yellow flame. Outline the source of the colours and why they are different.

Sketch the orbital diagram of the valence shell of a bromine atom (ground state) on the energy axis provided. Use boxes to represent orbitals and arrows to represent electrons.

Mass spectrometry analysis of a sample of iron gave the following results:

Calculate the relative atomic mass, A_r, of this sample of iron to two decimal places.

State the nuclear symbol notation, ${}_{\text{Z}}^{\text{A}}\text{X}$, for iron-54.

Which is correct for ${}_{16}^{34}{\text{S}}^{2-}$?

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

(i) Explain the convergence of lines in a hydrogen emission spectrum.

(ii) State what can be determined from the frequency of the convergence limit.

Which representation would be correct for a species, Z, which has 31 protons, 40 neutrons and 28 electrons?

A. ${}_{31}^{71}{\mathrm{Z}}^{3+}$

B. ${}_{31}^{71}{\mathrm{Z}}^{3-}$

C. ${}_{40}^{71}{\mathrm{Z}}^{3+}$

D.  ${}_{28}^{71}{\mathrm{Z}}^{3+}$

State the full electron configuration of the chlorine atom.

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

A sample of magnesium has the following isotopic composition.

Calculate the relative atomic mass of magnesium based on this data, giving your answer to two decimal places.

State the condensed electron configurations for Cr and Cr3⁺.

State one analytical technique that could be used to determine the ratio of ¹⁴N : ¹⁵N.

What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?

A. [Ar]3d⁶

B. [Ar]4s²3d⁴

C. [Ar]4s¹3d⁵

D. [Ar]4s²4p⁴

What is the ground state electron configuration of an atom of chromium, Cr (Z = 24)?

A. [Ar]3d⁶

B. [Ar]4s²3d⁴

C. [Ar]4s¹3d⁵

D. [Ar]4s²4p⁴

What is the relative atomic mass, $A_{\mathrm{r}}$, of an element with this mass spectrum?

A.  $24.0$

B.  $24.3$

C.  $24.9$

D.  $25.0$

What is the maximum number of electrons that can occupy the 4th main energy level in an atom?

A.  $8$

B.  $14$

C.  $18$

D.  $32$

State the full electron configuration of the sulfide ion.

State the full electron configuration of the sulfide ion.

Describe how the relative atomic mass of a sample of calcium could be determined from its mass spectrum.

Which species has two more neutrons than electrons?

${}_3{}^{6}L{i}^{+}$             ${}_4{}^{9}B{e}^{2+}$             ${}_{11}{}^{23}N{a}^{+}$             ${}_{20}{}^{42}C{a}^{2+}$

A.  ${}_3{}^{6}L{i}^{+}$

B.  ${}_4{}^{9}B{e}^{2+}$

C.  ${}_{11}{}^{23}N{a}^{+}$

D.  ${}_{20}{}^{42}C{a}^{2+}$

State the electron configuration of copper.

Naturally occurring gallium consists of the isotopes ⁷¹Ga and ⁶⁹Ga. What is the approximate percentage abundance of ⁶⁹Ga?

M_r(Ga) = 69.72.

A.  40 %

B.  50 %

C.  60 %

D.  75 %

State the nuclear symbol notation, ${}_{\text{Z}}^{\text{A}}\text{X}$, for iron-54.

State the electron configuration of the Cu⁺ ion.

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

Calculate the relative atomic mass, A_r, of this sample of magnesium to two decimal places.

The mass spectrum of chlorine is shown.

NIST Mass Spectrometry Data Center Collection © 2014 copyright by the U.S. Secretary of Commerce on behalf of the United States of America. All rights reserved.

Outline the reason for the two peaks at $m/z=35$ and $37$.

Which is the electron configuration of a chromium atom in the ground state?

A. [Ne]3s²3p⁶4s¹3d⁴

B. [Ar]3d³

C. 1s²2s²2p⁶3s²3p⁶4s²3d⁴

D. [Ar]4s¹3d⁵

What is the relative molecular mass of bromine, according to the following mass spectrum?

NIST Mass Spectrometry Data Center Collection © 2014 copyright by the U.S. Secretary of Commerce
on behalf of the United States of America. All rights reserved.

A.  $\frac{158\times 52+160\times 100+162\times 48}{52+100+48}$

B.  $\frac{158\times 52+160\times 100+162\times 48}{158+160+162}$

C.  $\frac{79\times 11+81\times 11+158\times 52+160\times 100+162\times 48}{11+11+52+100+48}$

D.  $\frac{79\times 11+81\times 11}{11+11}$

Calculate the wavelength, in m, for the electron transition corresponding to the frequency in (a)(iii) using section 1 of the data booklet.

State the electron configuration of copper.

State the full electronic configuration of Fe²⁺.

The stable isotope of rhenium contains 110 neutrons.

State the nuclear symbol notation ${}_{\text{Z}}^{\text{A}}\text{X}$ for this isotope.

State the electron configuration of the Cu⁺ ion.

Explain the presence and relative abundance of the peak at $m/z=74$.

State the electron configuration of the Ca²⁺ ion.

Draw the first four energy levels of a hydrogen atom on the axis, labelling n = 1, 2, 3 and 4.

Copper is widely used as an electrical conductor.

Draw arrows in the boxes to represent the electronic configuration of copper in the 4s and 3d orbitals.

State the electron configuration of a bromine atom.

Which transition in the hydrogen atom emits visible light?

A. n = 1 to n = 2

B. n = 2 to n = 3

C. n = 2 to n = 1

D. n = 3 to n = 2

What is the condensed electron configuration of the Fe²⁺ ion? 

A. [Ar]3d⁶
B. [Ar]3d⁴4s²
C. [Ar]3d⁵4s¹
D. [Ar]3d⁶4s²

Explain the presence and relative abundance of the peak at $m/z=74$.

The mass spectrum of chlorine is shown.

NIST Mass Spectrometry Data Center Collection © 2014 copyright by the U.S. Secretary of Commerce on behalf of the United States of America. All rights reserved.

Outline the reason for the two peaks at $m/z=35$ and $37$.

Naturally occurring silver is composed of two stable isotopes, ¹⁰⁷Ag and ¹⁰⁹Ag.

The relative atomic mass of silver is 107.87. Show that isotope ¹⁰⁷Ag is more abundant.

Outline the model of electron configuration deduced from the hydrogen line emission spectrum (Bohr’s model).

What is represented by ^“2−” in ${}_{\mathrm{Z}}{}^{\mathrm{A}}\mathrm{X}^{2-}$?

A.  loss of electron

B.  gain of electron

C.  loss of proton

D.  gain of proton

[Cr(OH)₆]³⁻ forms a green solution. Estimate a wavelength of light absorbed by this complex, using section 17 of the data booklet.

State the condensed electron configurations for Cr and Cr3⁺.

Subsequent experiments showed electrons existing in energy levels occupying various orbital shapes.

Sketch diagrams of 1s, 2s and 2p.

What is the maximum number of electrons that can occupy a p-orbital?

A.  2

B.  3

C.  6

D.  8

Sketch the orbital diagram of the valence shell of a bromine atom (ground state) on the energy axis provided. Use boxes to represent orbitals and arrows to represent electrons.

Deduce the full electron configuration of Fe²⁺.

A sample of gas was enriched to contain 2 % by mass of ¹⁵N with the remainder being ¹⁴N.

Calculate the relative molecular mass of the resulting N₂O.

Which is correct for ${}_{16}^{34}{\text{S}}^{2-}$?

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

What does ${}_{12}^{24}M{g}^{2+}$ represent?

A.     An ion with 12 protons and 24 neutrons

B.     An ion with 14 protons and 24 neutrons

C.     An ion with 12 protons and 12 neutrons

D.     An ion with 12 protons and 22 neutrons

Draw the lines, on your diagram, that represent the electron transitions to n = 2 in the emission spectrum.

Which of the following is the electron configuration of a metallic element?

A.  [Ne] 3s² 3p²

B.  [Ne] 3s² 3p⁴

C.  [Ne] 3s² 3p⁶ 3d³ 4s²

D.  [Ne] 3s² 3p⁶ 3d¹⁰ 4s² 4p⁵

Mass spectrometry analysis of a sample of iron gave the following results:

Calculate the relative atomic mass, A_r, of this sample of iron to two decimal places.

A sample of gas was enriched to contain 2 % by mass of ¹⁵N with the remainder being ¹⁴N.

Calculate the relative molecular mass of the resulting N₂O.

State one analytical technique that could be used to determine the ratio of ¹⁴N:¹⁵N.