Table of contents

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1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

2. Atoms & Elements

Ions

General Chemistry

2. Atoms & Elements

Ions

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Multiple Choice

A neutral phosphorus atom has 15 electrons. How many electrons are present in a phosphide ion (P^{3-})?

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Identify the number of electrons in a neutral phosphorus atom. Since phosphorus has an atomic number of 15, it has 15 protons and, in its neutral state, also 15 electrons.

Understand that a phosphide ion, denoted as $P^{3-}$, has gained 3 extra electrons compared to the neutral atom.

Calculate the total number of electrons in the $P^{3-}$ ion by adding the 3 extra electrons to the 15 electrons of the neutral phosphorus atom.

Express this calculation as an equation: $\text{Number of electrons in } P^{3-} = 15 + 3$.

Conclude that the phosphide ion has more electrons than the neutral atom due to the negative charge, which corresponds to the number of electrons gained.