Write the full electron configuration for a neutral fluorine atom. full electron configuration: 1s 2s22p Draw the Lewis dot symbol for a neutral fluroine atom Identify the subshells in the full electron configuration whose electrons are included in the Lewis dot symbol for the neutral fluorine atom ?? 3p 1x 1 FIF: 23 Predict the ground-state electron configuration of each ion. Use the abbreviated noble gas notation. Cr2+ [Ar]3d1450 Incorrect Cu2+ [Ar]3d9450 , Incorrect Co3+ [Ar]3d4 Incorrect
The Correct Answer and Explanation is :
Here’s a step-by-step breakdown and explanation to address all parts of your question:
1. Full Electron Configuration for Neutral Fluorine Atom
The atomic number of fluorine is 9, meaning it has 9 electrons. The full electron configuration is:
1s² 2s² 2p⁵
2. Lewis Dot Symbol for Neutral Fluorine
The Lewis dot symbol represents the valence electrons around the atom. For fluorine:
- Valence shell: ( n = 2 ), containing 2s² and 2p⁵ subshells.
- Total valence electrons: ( 2 + 5 = 7 ).
- Lewis symbol: The symbol for fluorine (( F )) with seven dots around it, one for each valence electron.
..
:F:
.3. Subshells Included in Lewis Dot Symbol
Electrons in the 2s and 2p subshells (i.e., the valence shell) are represented in the Lewis dot symbol. The 1s subshell electrons are core electrons and are not shown.
4. Predicting the Ground-State Electron Configurations for Ions
a. Cr²⁺ (Chromium ion):
Neutral chromium: ( [Ar] 4s¹ 3d⁵ ).
For Cr²⁺: Remove two electrons starting from the ( 4s ) orbital.
Correct configuration: ( [Ar] 3d⁴ ).
b. Cu²⁺ (Copper ion):
Neutral copper: ( [Ar] 4s¹ 3d¹⁰ ).
For Cu²⁺: Remove two electrons starting from the ( 4s ) orbital.
Correct configuration: ( [Ar] 3d⁹ ).
c. Co³⁺ (Cobalt ion):
Neutral cobalt: ( [Ar] 4s² 3d⁷ ).
For Co³⁺: Remove three electrons (first two from ( 4s ), then one from ( 3d )).
Correct configuration: ( [Ar] 3d⁶ ).
5. Explanation (300 Words)
Electron configurations describe the distribution of electrons in an atom’s orbitals. Neutral atoms fill orbitals according to the Aufbau principle, Hund’s rule, and the Pauli exclusion principle. When forming ions, electrons are removed starting from the highest energy orbital.
- Fluorine: Its ground-state electron configuration is ( 1s² 2s² 2p⁵ ). The ( 1s ) electrons are core electrons, while ( 2s² 2p⁵ ) are the valence electrons. These seven valence electrons are depicted in the Lewis dot symbol, where dots are placed around the atomic symbol to indicate the electron count in the outermost shell.
- Transition Metal Ions (Cr, Cu, Co): Transition metals often involve ( 3d ) and ( 4s ) orbitals. While ( 4s ) is filled before ( 3d ), the ( 4s ) electrons are removed first when forming cations because ( 4s ) electrons are at a higher energy level once ( 3d ) starts filling. Thus, for Cr²⁺, ( 4s¹ ) and one ( 3d ) electron are removed, yielding ( [Ar] 3d⁴ ). Similarly, Cu²⁺ loses its ( 4s¹ ) and one ( 3d ) electron, resulting in ( [Ar] 3d⁹ ). Finally, Co³⁺ removes two ( 4s ) and one ( 3d ) electron to yield ( [Ar] 3d⁶ ).
Understanding these principles ensures accurate predictions of electron configurations and chemical behavior.