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

10. Chemical Bonding

Lewis Dot Structures: Ions (Simplified)

Introduction to Chemistry

10. Chemical Bonding

Lewis Dot Structures: Ions (Simplified)

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Multiple Choice

Draw the Lewis Dot Structure for the following ion:PCl₄⁺.

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Verified step by step guidance

Identify the total number of valence electrons available. Phosphorus (P) has 5 valence electrons, and each Chlorine (Cl) has 7 valence electrons. Since the ion has a +1 charge, subtract one electron from the total.

Calculate the total number of valence electrons: 5 (from P) + 4*7 (from 4 Cl atoms) - 1 (due to the +1 charge) = 32 electrons.

Place the phosphorus atom in the center as it is less electronegative than chlorine, and arrange the four chlorine atoms around it.

Form single bonds between the phosphorus atom and each chlorine atom. Each bond uses 2 electrons, so 4 bonds will use 8 electrons.

Distribute the remaining electrons to satisfy the octet rule for each chlorine atom. Each chlorine should have 6 more electrons to complete its octet, using up the remaining 24 electrons. Ensure the structure reflects the +1 charge by enclosing it in brackets and indicating the charge.