Multiple Choice
How many valence electrons does neon (Ne) have?
3
views
10. Periodic Properties of the Elements
Valence Electrons of Elements
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Which characteristic of metal atoms helps explain why valence electrons in a metal are delocalized?
A
Metals have small atomic radii, resulting in strong attraction between nucleus and valence electrons.
B
Metals have low ionization energies, allowing their valence electrons to move freely.
C
Metals have high electronegativity, causing their valence electrons to be tightly held.
D
Metals have completely filled valence shells, making their electrons stable and localized.
Verified step by step guidance1
Understand that in metals, valence electrons are not tightly bound to any single atom but are free to move throughout the metal lattice, creating a 'sea of electrons.'
Recognize that the key factor allowing this delocalization is the energy required to remove an electron from an atom, known as the ionization energy.
Recall that metals generally have low ionization energies, meaning their valence electrons can be removed or shared with relative ease compared to nonmetals.
Connect the low ionization energy to the ability of valence electrons to become delocalized, as they are not held strongly by the nucleus and can move freely between atoms.
Conclude that this characteristic explains why metals conduct electricity and heat well, as the delocalized electrons act as charge carriers.
2:32mWatch next
Master Main Group Elements Valence Electrons with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Valence Electrons of Elements practice set
Problem sets built by lead tutorsExpert video explanations