Lecture 10 - Molecular Shape Flashcards

1
Q

what makes up covalent bonds?

A

2 nonmetals or a nonmetal + metalloid

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2
Q

what is special about metals?

A

they don’t combine, instead mix into alloys

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3
Q

atoms with 1, 2 or 3 valence electrons form…

A

1, 2, or 3 bonds

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4
Q

atoms with 4 or more valence electrons form…

A

enough bonds to make an octet

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5
Q

why is boron an exception to the octet rule?

A

it only wants 6 valence electrons, only taking on 3 bonds

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6
Q

why are elements in group 3A exceptions to the octet rule?

A

they do not have enough valence electrons to form octets in natural molecules.

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7
Q

what is VSEPR?

A

Valence Shell Electron Pair Repulsion. molecules are most stable when its lone pairs and bonds are as FAR from each other as possible

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8
Q

what is a linear lewis dot shape?

A

any atom surrounded by only 2 groups, bond angle of 180 degrees (AX2)

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9
Q

what is a trigonal planar lewis dot shape?

A

any atom surrounded by 3 groups, bond angles of 120 degrees (AX3)

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10
Q

what is a tetrahedral lewis dot shape?

A

any atom surrounded by 4 groups, bond angles of 109.5 degrees (AX4)

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11
Q

what is a trigonal pyramid lewis dot shape?

A

if the 4 groups around an atom include 1 lone pair, bond angles of ~109.5 degrees (AX2E)

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12
Q

what is a bent lewis dot shape?

A

if the 4 groups around the atom include 2 lone pairs, bond angle is 105 degrees (AX2E2)

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13
Q

when drawing lewis structures for polyatomic ions…

A

add one electron for each negative charge, subtract one electron for each positive charge

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14
Q

what are resonant structures?

A

2 lewis structures with the same atoms but different arrangements of electrons

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