Question detail
Describe the relationship between the electronic configuration of elements in Period 3 and their first ionisation energies.
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
Question
Type
exam_style
Style
Topic
Periodicity
Question
Describe the relationship between the electronic configuration of elements in Period 3 and their first ionisation energies.
Answer
Elements in Period 3 have increasing first ionisation energies as their electronic configurations show an increase in the number of protons and electrons. As the number of electrons increases, the outermost electrons experience greater effective nuclear charge, leading to higher ionisation energies.
Explanation
This answer is strong because it links electronic configuration directly to ionisation energy, demonstrating an understanding of how atomic structure influences chemical properties. The question assesses the ability to connect concepts in periodicity.
Common mistake
Misunderstanding Ionisation Energy Trends
Students often confuse the trend in first ionisation energy across Period 3 with atomic radius, thinking that ionisation energy decreases as atomic radius increases.
To clarify, remember that first ionisation energy increases across Period 3 due to increased nuclear charge attracting electrons more strongly. Use the formula for ionisation energy trends: as atomic number increases, ionisation energy increases because of greater effective nuclear charge. Therefore, the correct trend is that first ionisation energy increases across Period 3.
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