Section Four: Electrons, Bonding, and Structure Flashcards

1
Q

how many electrons can fill the first four shells?

A

1st shell= 2
2nd shell= 8
3rd shell= 18
4th shell= 32

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2
Q

what is the atomic orbital?

A

area around the nucleus that can hold up to two electrons with opposite spins

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3
Q

what shape is an s-orbital and a p-orbital?

A

s-orbitals are spherical
p-orbitals are dumbbell and can have 3 separate orbitals

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4
Q

what is the number of orbitals and maximum number of electrons in each sub-shell?

A

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

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5
Q

how do orbitals fill? why does the 4s sub-shell fill first?

A

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

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6
Q

how are electrons configurations shown? practice doing them.

A

sub-shell notation and electrons in boxes

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7
Q

what is ionic bonding?

A

the electrostatic attraction between positive and negative ions

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8
Q

why do lattices have a higher boiling point?

A
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9
Q

why do ionic bonds have high melting and boiling points?

A

a high temperature is needed because a lot of energy is needed to overcome the strong electrostatic attraction between ions

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10
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11
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12
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13
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14
Q

what is covalent bonding?

A

strong electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms

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15
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25
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what is electronegativity?

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the ability of an atom to attract the bonding electrons in a covalent bond

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