State the electron configuration of the Ca²⁺ ion.

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.

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

A.  2

B.  3

C.  6

D.  8

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

State the electron configuration of the Cu⁺ ion.

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.

State the full electronic configuration of Fe²⁺.

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.

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.

State the electron configuration of a bromine atom.

State the electron configuration of a bromine atom.

Deduce the full electron configuration of Fe²⁺.

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

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

A. [Ne]3s²3p⁶4s¹3d⁴

B. [Ar]3d³

C. 1s²2s²2p⁶3s²3p⁶4s²3d⁴

D. [Ar]4s¹3d⁵

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

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

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

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

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

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

State the electron configuration of the Cu⁺ ion.

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

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

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

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

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

State the full electron configuration of the sulfide ion.

State the full electron configuration of the sulfide ion.

State the condensed electron configurations for Cr and Cr3⁺.

State the condensed electron configurations for Cr and Cr3⁺.

State the full electron configuration of the chlorine atom.

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 chlorine atom.

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 electron configuration of copper.

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

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