section 5.3 electron configuration
in your textbook, read about ground - state electron configurations.
use each of the terms below just once to complete the passage.
aufbau principle electron configuration ground - state electron configuration hunds rule
lowest pauli exclusion principle spins stable
the arrangement of electrons in an atom is called the atoms
(1)____. electrons in an atom tend to assume the arrangement
that gives the atom the (2)____ possible energy. this arrangement
of electrons is the most (3)____ arrangement and is called the
atoms (4)____.
three rules define how electrons can be arranged in an atoms orbitals. the
(5)____ states that each electron occupies the lowest energy
orbital available. the (6)____ states that a maximum of two
electrons may occupy a single atomic orbital, but only if the electrons have opposite
(7)____. (8)____ states that single
electrons with the same spin must occupy each equal - energy orbital before additional
electrons with opposite spins occupy the same orbitals.
complete the following table.

Question

Accepted Answer

# Brief Explanations:
1. The term for the arrangement of electrons in an atom is "electron configuration".
2. Electrons tend to assume the arrangement with the "lowest" possible energy.
3. The lowest - energy arrangement is the most "stable".
4. This stable arrangement is called the "ground - state electron configuration".
5. The rule that each electron occupies the lowest energy orbital is the "Aufbau principle".
6. The principle that a maximum of two electrons may occupy a single atomic orbital (with opposite spins) is the "Pauli exclusion principle".
7. The property that electrons in a single orbital have opposite is "spins".
8. The rule about single electrons with the same spin occupying equal - energy orbitals first is "Hund's rule".

For the table:
- Helium has an atomic number of 2. In the 1s orbital, there are 2 electrons (as per $1s^{2}$).
- For an atomic number of 7 (nitrogen), using the Aufbau principle, Pauli exclusion principle, and Hund's rule:
    - 1s orbital: 2 electrons ($\uparrow\downarrow$)
    - 2s orbital: 2 electrons ($\uparrow\downarrow$)
    - 2p orbitals ($2p_{x}$, $2p_{y}$, $2p_{z}$): 3 electrons (each $2p$ orbital has 1 electron with the same spin, $\uparrow$ in $2p_{x}$, $\uparrow$ in $2p_{y}$, $\uparrow$ in $2p_{z}$), and the electron configuration is $1s^{2}2s^{2}2p^{3}$
- Neon has an atomic number of 10. The electron configuration is $1s^{2}2s^{2}2p^{6}$

# Answer:
1. electron configuration
2. lowest
3. stable
4. ground - state electron configuration
5. Aufbau principle
6. Pauli exclusion principle
7. spins
8. Hund's rule
9. Atomic number: 2; Orbitals: 1s has 2 electrons ($\uparrow\downarrow$), 2s has 0 electrons, $2p_{x}$, $2p_{y}$, $2p_{z}$ have 0 electrons
10. Element: Nitrogen; Orbitals: 1s ($\uparrow\downarrow$), 2s ($\uparrow\downarrow$), $2p_{x}$ ($\uparrow$), $2p_{y}$ ($\uparrow$), $2p_{z}$ ($\uparrow$); Electron configuration: $1s^{2}2s^{2}2p^{3}$
11. Atomic number: 10; Electron configuration: $1s^{2}2s^{2}2p^{6}$

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Answer: