Electron Configurations Through Neon (8.1.3) Flashcards
• By the Pauli exclusion principle, each orbital can only hold two electrons.
• By the Pauli exclusion principle, each orbital can only hold two electrons.
• For a given energy level in an element other than hydrogen, the s orbital is lower in energy than the p orbitals.
• For a given energy level in an element other than hydrogen, the s orbital is lower in energy than the p orbitals.
• By Hund’s rule, one electron enters each degenerate orbital before any pairing occurs.
• By Hund’s rule, one electron enters each degenerate orbital before any pairing occurs.
The Pauli exclusion principle states that each
electron in an atom must have a unique set of
quantum numbers describing it.
By the Pauli exclusion principle, each orbital can
only hold two electrons. The two electrons in an
orbital differ only in their electron spin quantum
numbers (ms).
The Pauli exclusion principle states that each
electron in an atom must have a unique set of
quantum numbers describing it.
By the Pauli exclusion principle, each orbital can
only hold two electrons. The two electrons in an
orbital differ only in their electron spin quantum
numbers (ms).
For a given energy level in an element other than
hydrogen, the s orbital is lower in energy than the p
orbitals. For example, in helium (He), the 2s orbital
is lower in energy than the 2p orbital.
This difference in energy is because p orbitals
experience more electron shielding than s orbitals.
This shielding causes the p orbitals to experience a
lower effective nuclear charge, and therefore to be
higher in energy. Electrons fill lower energy orbitals
before higher energy orbitals.
For a given energy level in an element other than
hydrogen, the s orbital is lower in energy than the p
orbitals. For example, in helium (He), the 2s orbital
is lower in energy than the 2p orbital.
This difference in energy is because p orbitals
experience more electron shielding than s orbitals.
This shielding causes the p orbitals to experience a
lower effective nuclear charge, and therefore to be
higher in energy. Electrons fill lower energy orbitals
before higher energy orbitals.
Degenerate orbitals (such as the three 2p orbitals) have equal energy.
By Hund’s rule, one electron enters each
degenerate orbital before any pairing occurs. These
electrons tend to have aligned electron spins.
Electron configurations are expressed in forms
such as 1s^2 2s^2 2p^6. Understanding electron
configurations allows for a better understanding of
the properties of the elements.
Degenerate orbitals (such as the three 2p orbitals) have equal energy.
By Hund’s rule, one electron enters each
degenerate orbital before any pairing occurs. These
electrons tend to have aligned electron spins.
Electron configurations are expressed in forms
such as 1s^2 2s^2 2p^6. Understanding electron
configurations allows for a better understanding of
the properties of the elements.
What is the ground state electron configuration for boron?
1s^2 2s^2 2p^1 (D)
Which of the following is the best explanation of why it is harder to remove an electron from an atom of neon than an atom of fluorine?
It is harder to remove an electron from neon than fluorine because of increased nuclear charge (Z = 10). (B)
Which of the following represents the electron configuration for carbon?
C
This is the correct number of electrons and in the correct orientation. This diagram shows that the electrons in the 2p orbital are entering separate orbitals and have parallel spins.
Which of the following is not a consideration in the placement of electrons in an atom?
Heisenberg uncertainty principle (D)
The Heisenberg uncertainty principle states the location and the momentum of an electron cannot be known simultaneously. This in not a consideration in the placement of the electron in orbitals of an atom.
What is the ground state electron configuration for oxygen?
1s^2 2s^2 2p^4 (A)
This is the correct ground state electron configuration for oxygen.
What is the ground state electron configuration for fluorine?
1s^2 2s^2 2p^5 (C)
This is the correct ground state electron configuration for fluorine.
Though Neon is a relatively small atom with a relatively high nuclear charge, it is difficult to add an electron to a neon atom. Which of the following is the best explanation of this phenomenon?
The next electron added to neon would have to be placed in a higher energy level (the n = 3 level). (C)
Because the next electron added to the neon atom would have to be added to a higher energy level (n = 3), it is very energetically unfavorable to do. This is partially the reason that neon is an unreactive element.
Which of the following is a correct statement of Hund’s Rule?
Electrons will occupy separate degenerate orbitals and maintain parallel spins before pairing up. (B)
By occupying different orbitals, the electrons maintain a maximum distance from each other and thus create the lowest possible electron-electron repulsion interaction.
There are no known compounds of neon, a noble gas. Which of the following is the best explanation of the inert nature of neon?
It is both harder to add an electron to and remove an electron from neon, thus no compounds readily form. (A)
The reactivity of an element depends on the ability to add or lose electrons. Neon does not easily gain or lose an electron.
