Multiple Choice
Which electron configuration represents the element carbon (atomic number 6)?
4
views
10. Periodic Properties of the Elements
The Electron Configuration
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Which of the following is true about the electron configurations of the noble gases?
A
They have partially filled d orbitals in their outermost energy level.
B
They have unpaired electrons in their outermost shell.
C
They have completely filled s and p orbitals in their outermost energy level.
D
They have the same electron configuration as alkali metals.
Verified step by step guidance1
Recall that noble gases are elements in Group 18 of the periodic table, known for their chemical inertness due to stable electron configurations.
Understand that the outermost energy level (valence shell) of noble gases is characterized by completely filled s and p orbitals, which makes them very stable.
Recognize that noble gases do not have partially filled d orbitals in their outermost energy level because their valence shell consists only of s and p orbitals (the d orbitals belong to inner shells or transition metals).
Note that noble gases have no unpaired electrons in their outermost shell since all their valence orbitals are fully occupied, leading to paired electrons.
Compare noble gases to alkali metals: alkali metals have a single electron in their outermost s orbital, so their electron configurations are quite different from the fully filled configurations of noble gases.
Related Videos
Related Practice
The Electron Configuration practice set
Problem sets built by lead tutorsExpert video explanations