Section Four: Electrons, Bonding, and Structure Flashcards
how many electrons can fill the first four shells?
1st shell= 2
2nd shell= 8
3rd shell= 18
4th shell= 32
what is the atomic orbital?
area around the nucleus that can hold up to two electrons with opposite spins
what shape is an s-orbital and a p-orbital?
s-orbitals are spherical
p-orbitals are dumbbell and can have 3 separate orbitals
what is the number of orbitals and maximum number of electrons in each sub-shell?
s sub-shell: orbitals= 1, max electrons= 2
p sub-shell: orbitals= 3, max electrons= 6
d sub-shell: orbitals= 5, max electrons= 10
f sub-shell: orbitals= 7, max electrons= 14
how do orbitals fill? why does the 4s sub-shell fill first?
the first three shells and the 4s and 4p orbitals fill in order of increasing energy
4s is filled first because it is at a lower energy than 3s, once it is filled 3d energy falls below 4s so it empties before
how are electrons configurations shown? practice doing them.
sub-shell notation and electrons in boxes
what is ionic bonding?
the electrostatic attraction between positive and negative ions
why do lattices have a higher boiling point?
why do ionic bonds have high melting and boiling points?
a high temperature is needed because a lot of energy is needed to overcome the strong electrostatic attraction between ions
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what is covalent bonding?
strong electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms
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what is electronegativity?
the ability of an atom to attract the bonding electrons in a covalent bond
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