1.5 Hybrid Orbitals

Question 1

what creates stronger bonds in orbitals

Answer 1

the better overlap between the orbitals the stronger the bond

Question 2

what do bond involve

Answer 2

the sharing of spin-paired electrons

Question 3

in organic chem what is the most common valence orbitals available

Answer 3

S and P

Question 4

what is hybridization

Answer 4

it is a simple theory that can help explain why geometry can be linear, trigonal plainer, or tetrahedral

Question 5

what is hybridization orbitals

Answer 5

S and P orbitals overlapping

Question 6

if we have a carbon (valence e is 2S2, 2P2) and hybridization occurs what happens to the configuration

Answer 6

it becomes sp3 this means one s + 3p (25% s and 75% p) and all _ _ _ _s get filled with electrons and moved to the same heights. and we call this atom 3 P hybridized

Question 7

if we combine 2s orbitals with the 2p, 2p, 2p orbitals we get…

Answer 7

four sp3 orbitals distributed in a tetrahedral

Question 8

how many lobes do SP3 orbitals have

Answer 8

the combination of the s and the p orbitals cause it to has 2 lobes like p orbitals but one is smaller then the other

Question 9

what kind of hybridization can pi bonding be explained

Answer 9

by sp2 hybridization

Question 10

if a atom is sp2-hybridized how many orbitals does it have and what are they made from

Answer 10

it has 3 orbitals made from one s and two p orbitals

Question 11

what is the precent compisition of sp2-hybridized orbitals

Answer 11

they are 33.3% s and 66.6% p

Question 12

what has more energy sp3 or sp2

Answer 12

sp3

Question 13

explain how the electrons fill when there is a sp2 hybridization

Answer 13

there is sp2 _ _ _ with one arrow (these are hybridized
and there is a 2p _ with a arrow (this is not hybridized)

Question 14

in a sp2 hybridization are all orbitals hybridized

Answer 14

no there is one unhybridized p orbital

Question 15

what kind of bonds does sp2-hybridized allow for

Answer 15

the formation of double bonds if 2 p orbitals each with electron are on atoms connected by a sigma bond

Question 16

if we combine the 2s orbitals with the 2px, 2py we get…

Answer 16

three sp2 orbitals (and keep 2pz)

Question 17

for the sp2 hybridization what do the orbitals look like

Answer 17

the three sp2 have two lobes (one bigger, one smaller) and they are distributed in a trigonal planer

the un hybridized p orbital does not change (2 same sized lobes)

Question 18

what is they hybridization of methane (CH4)

Answer 18

sp3

Question 19

what is the hybridization of ethylene (C2H4)

Answer 19

sp2

Question 20

in ethylene (C2H4) explain how the structure creates double bonds

Answer 20

there is 2 tetrahedral shape of hybridized sp2 carbon orbitals and they over lap creating a sigma bond

there is 2 un hybridized p bonds that hover electrons causing pi bonds

these two bonds create double bonding

Question 21

if we combine the 2s orbital and the 2px orbital we get…

Answer 21

two sp orbitals (and keep the 2py and 2pz)

Question 22

describe the shape of a sp orbital

Answer 22

the two sp hybrids would have two lobes one bigger then the other

the un hybridized 2py and 2pz will have two same sized lobes

Question 23

what are the anges between the new sp hybridized orbitals

Answer 23

they are 180 degrees so the geometry is linear

Question 24

list the charictrisitc of an orbital with 2 groups

Answer 24

-it (can/has?) have a triple bond
-its linear
-it is sp hybridized
-2=1+1

Question 25

list the characteristics of an orbital with 3 groups

Answer 25

-it (can/has?) have a double bond
-its trigonal planar
-it is sp2 hybridized
-3=1+2

Question 26

list the characteristics of an orbital with 4 groups

Answer 26

_