Which of the following best describes the atomic emission spectra?

A. A continuous spectrum of all wavelengths of light.

B. A spectrum showing only specific wavelengths of light emitted by an atom.

C. A spectrum showing the absorption of light by an atom.

D. A spectrum showing the reflection of light by an atom.

The limit of convergence in an atomic emission spectrum is directly related to:

A. The atomic radius.

B. The atomic mass.

C. The first ionisation energy.

D. The electron affinity.

Which factor primarily influences the variation of ionisation energy across periods in the periodic table?

A. Atomic size.

B. Nuclear charge.

C. Electron shielding.

D. Both B and C.

Which of the following trends is observed for atomic size as we move from left to right across a period in the periodic table?

A. Increases due to increased nuclear charge.

B. Decreases due to increased nuclear charge.

C. Increases due to increased electron shielding.

D. Remains constant.

What can be inferred about an element if there is a large jump in energy between its first and second ionisation energies?

A. The element is likely a noble gas.

B. The element is likely a metal.

C. The element is likely a non-metal.

D. The element has a full valence shell.

a) Explain the significance of atomic emission spectra in understanding the electronic structure of atoms. [3]

b) The limit of convergence in the hydrogen spectrum is related to the ionisation energy of hydrogen. Describe this relationship. [2]

a) As one moves across a period in the periodic table, how does the first ionisation energy typically change? Explain the reason for this trend. [3]

b) Discuss the influence of nuclear charge and electron shielding on the ionisation energy of an atom. [2]

a) Describe the trend in atomic size as one moves across a period in the periodic table and relate it to ionisation energy. [3]

b) How do successive ionisation energies of an element provide insights into its electron configuration? [2]

a) Describe the basic principles behind atomic emission spectra. [2]

b) How can atomic emission spectra be used to determine the atomic structure of an element? [3]

c) Why are the emission spectra of elements unique and distinct from one another? [2]

a) Explain the relationship between the limit of convergence in a spectrum and the first ionisation energy of an element. [3]

b) How does electron shielding affect the ionisation energy of an atom? [2]

c) Why does ionisation energy generally increase across a period in the periodic table? [3]