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The energy (kJ mol⁻¹) required to remove the first five electrons from an atom of element X is shown in the table: Electron number 1 2 3 4 5 Energy 495 4560 6910 9550 13420 Element X is most likely to be located in the periodic table in group A - VCE - SSCE Chemistry - Question 10 - 2004 - Paper 1
Question 10
The energy (kJ mol⁻¹) required to remove the first five electrons from an atom of element X is shown in the table: Electron number 1 2 3 4 5 Energy 495 4560 6910 95... show full transcript
Worked Solution & Example Answer:The energy (kJ mol⁻¹) required to remove the first five electrons from an atom of element X is shown in the table: Electron number 1 2 3 4 5 Energy 495 4560 6910 9550 13420 Element X is most likely to be located in the periodic table in group A - VCE - SSCE Chemistry - Question 10 - 2004 - Paper 1
Step 1
Identify the trend in ionization energy
Answer
As seen in the provided energy values, there is a noticeable trend in the increase of energy required to remove each successive electron. The relatively small increase from the first to the second electron (495 kJ mol⁻¹ to 4560 kJ mol⁻¹) indicates that the first electron is removed from a less stable state, likely to be an outermost electron.
Step 2
Analyze the large jump in ionization energy
Answer
The substantial increase between the second and third electrons (from 4560 kJ mol⁻¹ to 6910 kJ mol⁻¹) suggests that upon removing the second electron, the remaining electron configuration has achieved a more stable noble gas configuration. This indicates that element X likely has 2 valence electrons, characteristic of Group II elements.
Step 3