Bonding Flashcards

1
Q

each type has a specific shape, which describes the probability of finding an electron in a given region of space

A

atomic orbitals

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2
Q

spherical and symmetrical orbital , centered around nucleus

A

s-orbital

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3
Q

orbital composed of two lobes located symmetrically around nucleus and contains a node at the nucleus, like a dumbbell; x, y, or z axis

A

p-orbital

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4
Q

area where the probability of finding an electron is zero

A

node

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5
Q

orbital with four symmetrical lobes and two nodes

A

d-orbital

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6
Q

formed when two atomic orbitals combine

A

molecular orbitals

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7
Q

produced when sign of wave functions is the same, lower energy, more stable

A

bonding orbitals

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8
Q

produced when signs of wave functions are different, higher energy, less stable

A

antibonding orbitals

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9
Q

molecular orbital formed by head-to-head or tail-to-tail overlap; includes all single bonds (accommodating two electrons)

A

sigma (σ) bond

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10
Q

molecular orbital formed when two p-orbitals line up in parallel and their electron clouds overlap

A

pi (π) bond

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11
Q

individual pi bonds are _____ than sigma bonds

A

weaker

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12
Q

one π bond on top of an existing σ bond

A

double bond

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13
Q

a σ bond and two π bonds

A

triple bond

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14
Q

formed by mixing different types of orbitals

A

hybrid orbitals

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15
Q

atom with all single bonds; 25% s character, 75% p character

A

sp^3

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16
Q

atom with one double bond; 33% s character, 67% p character

A

sp^2

17
Q

atom with one triple bond or two double bonds; 50% s character, 50% p character

A

sp

18
Q

alignment of unhybridized p-orbitals down the backbone of a molecule, requires alternating single and multiple bonds; π electrons delocalize through p-orbital system; increases stability

A

conjugation