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Magazine Chapter 28: Problem 23
Draw schematic diagrams for the electrons in the subshells of (a) sodium (Na) and (b) argon (Ar) atoms in the ground state.
Short Answer
Expert verified
Sodium: 1s虏 2s虏 2p鈦� 3s鹿; Argon: 1s虏 2s虏 2p鈦� 3s虏 3p鈦�.
Step by step solution
01
Identify the Number of Electrons
Sodium (Na) has an atomic number of 11, meaning it has 11 electrons. Argon (Ar) has an atomic number of 18, meaning it has 18 electrons. These electrons will be distributed among different subshells in the schematic diagrams.
02
Understand Electron Configuration Notation
Electron configuration shows the distribution of electrons among the orbitals in an atom. This notation helps identify how many electrons are in each subshell, such as 1s, 2s, or 2p. Each letter and number combination (like 3p) corresponds to one specific subshell.
03
Distribute Electrons for Sodium
For sodium (Na) with 11 electrons, distribute the electrons as follows: 1s虏, 2s虏, 2p鈦�, 3s鹿. Start filling from the 1s subshell, then 2s, 2p, and finally 3s. The configuration terminates at 3s鹿, indicating one electron in the 3s subshell.
04
Draw Schematic Diagram for Sodium
Using the electron configuration in Step 3, the schematic diagram for sodium shows filled orbitals for each subshell completed. Each subshell is filled as 1s with 2 electrons, 2s with 2 electrons, 2p with 6 electrons, and 3s with 1 electron.
05
Distribute Electrons for Argon
For argon (Ar) with 18 electrons, distribute them in these subshells: 1s虏, 2s虏, 2p鈦�, 3s虏, 3p鈦�. Similar to sodium, start with the 1s, then 2s, filling each subsequent subshell (2p, 3s, 3p) until all electrons are allocated.
06
Draw Schematic Diagram for Argon
Using the electron configuration from Step 5, draw the schematic diagram for argon with filled subshells. The diagram illustrates 1s with 2 electrons, 2s with 2 electrons, 2p with 6 electrons, 3s with 2 electrons, and 3p with 6 electrons.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Sodium Electron Configuration
When we talk about sodium, we're focusing on an element with an atomic number of 11. This means sodium has 11 electrons moving around its nucleus in shells or orbitals. To understand how these electrons are spread out, we use the electron configuration notation.
Sodium's electrons are arranged in this order: 1s虏 2s虏 2p鈦� 3s鹿. This sequence reflects how the electrons are added to the orbitals:
Sodium's electrons are arranged in this order: 1s虏 2s虏 2p鈦� 3s鹿. This sequence reflects how the electrons are added to the orbitals:
- 1s虏 means the first energy level's s subshell is fully filled with 2 electrons.
- 2s虏 shows the second energy level's s subshell is filled with 2 electrons.
- 2p鈦� represents the p subshell within the second energy level holding 6 electrons, which maxes out the p subshell's capacity.
- Finally, 3s鹿 illustrates that there is 1 lonely electron in the third energy level's s subshell.
Argon Electron Configuration
Argon is a noble gas with an atomic number of 18 and, consequently, has 18 electrons. Its electron configuration reflects the complete filling of its energy levels, giving it stability.
The electron configuration of argon is 1s虏 2s虏 2p鈦� 3s虏 3p鈦�. This breakdown indicates:
The electron configuration of argon is 1s虏 2s虏 2p鈦� 3s虏 3p鈦�. This breakdown indicates:
- 1s虏 - The first energy level's s subshell holds 2 electrons, fully occupied.
- 2s虏 - The second energy level's s subshell contains 2 electrons.
- 2p鈦� - Argon's second energy level p subshell can comfortably house 6 electrons, filling this subshell entirely.
- 3s虏 - The third energy level's s subshell is maxed out with 2 electrons.
- 3p鈦� - Finally, the p subshell in the third energy level has room for 6 electrons, which completes its capacity.
Subshell Diagrams
Subshell diagrams give us a visual way to see how electrons occupy an atom's subshells. These diagrams are vital in understanding electron configurations. They help depict how electrons fill various subshells from lowest to highest energy, following rules like Aufbau principle, Hund's rule, and Pauli exclusion principle.
Here鈥檚 how you can imagine the filling of subshells:
Here鈥檚 how you can imagine the filling of subshells:
- Aufbau principle: Electrons start filling the available orbitals with the lowest energy first (1s is filled before 2s, and so on).
- Pauli exclusion principle: Each orbital can hold a maximum of 2 electrons, and they must have opposite spins.
- Hund鈥檚 rule: For orbitals of the same energy (like p, d, or f orbitals), one electron goes into each orbital until all are half-full, before pairing starts.
