Electron Configuration
The electron configuration of sulfur.
What is 1s2 2s2 2p6 3s2 3p4?
This principle states that no two electrons in an atom can have the same four quantum numbers.
What is the Pauli Exclusion Principle?
Atomic radius generally does this moving left to right across a period.
What is decrease?
Coulomb’s Law describes the force of attraction between these two types of particles.
What are charged particles?
These electrons are primarily involved in chemical bonding.
What are valence electrons?
This subshell begins filling immediately after 4s according to the Aufbau principle.
What is 3d?
Hund’s rule states that electrons occupy orbitals singly before this occurs.
What is electron pairing?
Ionization energy generally does this moving up a group.
What is increase?
According to Coulomb’s Law, increasing distance between charges causes electrostatic attraction to do this.
What is decrease?
The number of valence electrons in phosphorus.
What is 5?
Write the electron configuration for Fe³⁺.
What is
[Ar] 3d5?
According to the Aufbau principle, electrons fill orbitals in order of increasing this quantity.
What is energy?
Cations are smaller than their neutral atoms because they have this reduced feature.
What is electron-electron repulsion and often fewer occupied energy levels?
This trend explains why ionization energy increases across a period.
What is increasing nuclear attraction for valence electrons?
Metals tend to have low ionization energies because they do this with electrons easily.
What is lose them?
Chromium is an exception to expected filling patterns because one electron is promoted to produce this especially stable arrangement.
What is a half-filled d subshell?
Explain why nitrogen is more stable than oxygen in terms of electron configuration.
What is because nitrogen has a half-filled 2p subshell?
Explain why fluorine has a smaller atomic radius than lithium.
What is fluorine has greater effective nuclear charge pulling electrons closer?
Using Coulomb’s Law, explain why Mg has a higher ionization energy than Na.
What is magnesium has greater nuclear charge with similar shielding, increasing attraction to valence electrons?
Nonmetals generally have high electron affinities because they tend to do this.
What is gain electrons?
Determine the element represented by the configuration: [Kr] 5s2 4d105p3
What is antimony (Sb)?
Draw the orbital diagram for carbon and explain why the two 2p electrons occupy separate orbitals.
What is due to Hund’s rule minimizing electron-electron repulsion?
Rank the following from largest to smallest radius: Na⁺, Mg²⁺, Ne, F⁻.
What is F⁻ > Ne > Na⁺ > Mg²⁺?
Explain why electron affinity becomes more negative moving across a period toward halogens.
What is increasing nuclear attraction stabilizes added electrons more strongly?
Compare sodium and chlorine in terms of metallic character.
What is sodium has metallic character, while chlorine has nonmetallic character?