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Chem 130 > ch6 > Flashcards

ch6 Flashcards

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1
Q

why do elements make hybrid orbitals

A

because they form bigger overlap than regular orbitals

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2
Q

what process can predict hybridization of orbitals

A

VsPR

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3
Q

What is sigma bond

A

any bond that is isn’t double bonded

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4
Q

pi bond

A

bond only between two p orbitals
can form

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5
Q

what is constructive interference

A

when two orbitals are in phase

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6
Q

destructive interference

A

two orbitals are out of phase and there is a node

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7
Q

symbol for anti bonding orbitals

A

star

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8
Q

why does antibonding exist

A

orbitals are constantly changing phase

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9
Q

what is bond order of stable molecule

A

greater than 1

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10
Q

formula for bond order

A

sum bonding orbitals - sum anti bonding orbits / 2

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11
Q

paramagnetic

A

unpaired electrons (magnetic)

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12
Q

diamagnetic

A

fully paired, non magnetic

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13
Q

what happens to unpaired electrons when near magnet

A

they orient

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14
Q

does a double bond count as more than one electron group

A

double and triple bonds are 1 electron group

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15
Q

what does electron group determine

A

shape of particle

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16
Q

which bonds are stronger pi or sigma

A

sigma

17
Q

isomer

A

same chem formula with different structures and have different properties

18
Q

molecular orbital

A

function that represents the state of electron in orbital

19
Q

bonding orbital

A

orbital power in energy than atomic orbitals it was formed from

20
Q

molecular orbital diagram

A

diagram that determines binding energy and whether or not something is paramagnetic or diamagnetic

21
Q

What does electronegativity magnitude mean in regard to bonding

A

when orbital is more electronegative it means the total energy is lower

22
Q

Which contibutes more to bonding something more electronegative or something less

A

more electronegative wants electron more

23
Q

what row can expand its octets

A

row 3 and beyond

24
Q

are loan pairs included in hybridization

A

yes

Chem 130 (20 decks)

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