Bonding

Question 1

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

Answer 1

atomic orbitals

Question 2

spherical and symmetrical orbital , centered around nucleus

Answer 2

s-orbital

Question 3

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

Answer 3

p-orbital

Question 4

area where the probability of finding an electron is zero

Answer 4

node

Question 5

orbital with four symmetrical lobes and two nodes

Answer 5

d-orbital

Question 6

formed when two atomic orbitals combine

Answer 6

molecular orbitals

Question 7

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

Answer 7

bonding orbitals

Question 8

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

Answer 8

antibonding orbitals

Question 9

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

Answer 9

sigma (σ) bond

Question 10

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

Answer 10

pi (π) bond

Question 11

individual pi bonds are _____ than sigma bonds

Answer 11

weaker

Question 12

one π bond on top of an existing σ bond

Answer 12

double bond

Question 13

a σ bond and two π bonds

Answer 13

triple bond

Question 14

formed by mixing different types of orbitals

Answer 14

hybrid orbitals

Question 15

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

Answer 15

sp^3

Question 16

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

Answer 16

sp^2

Question 17

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

Answer 17

sp

Question 18

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

Answer 18

conjugation