Table of contents

1. The Chemical World9m
- The Scientific Method
  9m
2. Measurement and Problem Solving2h 19m
3. Matter and Energy2h 15m
4. Atoms and Elements2h 33m
5. Molecules and Compounds1h 50m
6. Chemical Composition1h 23m
7. Chemical Reactions1h 43m
8. Quantities in Chemical Reactions1h 8m
9. Electrons in Atoms and the Periodic Table2h 32m
10. Chemical Bonding2h 10m
11 Gases2h 7m
12. Liquids, Solids, and Intermolecular Forces1h 11m
13. Solutions3h 1m
14. Acids and Bases2h 14m
15. Chemical Equilibrium1h 27m
16. Oxidation and Reduction1h 33m
17. Radioactivity and Nuclear Chemistry53m

9. Electrons in Atoms and the Periodic Table

Periodic Trend: Ionization Energy (Simplified)

Introduction to Chemistry

9. Electrons in Atoms and the Periodic Table

Periodic Trend: Ionization Energy (Simplified)

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Multiple Choice

Which element from Group 7A has lowest ionization energy.

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Verified step by step guidance

Understand the concept of ionization energy: Ionization energy is the energy required to remove an electron from an atom in the gaseous state. It generally increases across a period and decreases down a group in the periodic table.

Identify the elements in Group 7A (also known as Group 17 or the halogens): The elements listed are Iodine (I), Bromine (Br), Chlorine (Cl), and Fluorine (F). Neon (Ne) is not a halogen; it is a noble gas from Group 8A.

Recall the trend in ionization energy within a group: As you move down a group in the periodic table, the ionization energy decreases. This is because the outer electrons are further from the nucleus and are shielded by more inner electron shells, making them easier to remove.

Apply the trend to the halogens: Among the halogens listed, Iodine (I) is the furthest down the group, meaning it has the lowest ionization energy compared to Bromine (Br), Chlorine (Cl), and Fluorine (F).

Conclude that Iodine (I) has the lowest ionization energy among the halogens listed, based on its position in the periodic table and the trend of decreasing ionization energy down a group.