QQuestionChemistry
QuestionChemistry
"Arrange the following elements in order of decreasing ionization energy:
Cl, Si, P, Ar"
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Answer
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Step 1:I'll solve this problem step by step, focusing on the periodic trends of ionization energy.
Step 2:: Understand Ionization Energy
Ionization energy is the energy required to remove the outermost electron from a neutral atom in its gaseous state. It depends on two main factors: - Atomic size - Nuclear charge (number of protons)
Step 3:: Analyze the Periodic Table Positions
Let's look at the periodic table locations for these elements: - Cl: Group 17 (Halogen), Period 3 - Si: Group 14 (Metalloid), Period 3 - P: Group 15 (Nonmetal), Period 3 - Ar: Group 18 (Noble Gas), Period 3
Step 4:: Compare Atomic Sizes
As we move from left to right in a period, atomic size decreases due to increased nuclear charge. This means ionization energy generally increases.
Step 5:: Analyze Electron Configurations
- Ar: $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6}
- Si: 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{2}
Step 6:: Determine Ionization Energy Order
Comparing the electron configurations and periodic trends: - Ar has a full outer shell (noble gas configuration), which makes it very stable - Cl is a halogen with high electronegativity - P and Si have partially filled outer shells
Step 7:: Rank in Order of Decreasing Ionization Energy
From highest to lowest ionization energy:
Step 8:
Ar (highest)
Step 9:
Cl
Step 10:
P
Step 11:
Si (lowest)
Final Answer
Ar > Cl > P > Si
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