Exam 3

Question 1

Covalent Bond

Answer 1

Bond where atoms share electrons

Question 2

Bond lengths - = ≡

Answer 2

triple(≡) = shortest
single(-) = longest

Question 3

Bond energy (lowest to highest)

Answer 3

single(-) = lowest
triple(≡) = highest

Question 4

Electronegativity trend

Answer 4

increases up and to the right

Question 5

Ionic bond

Answer 5

atoms lose and gain electrons and are bonded by pos/neg attraction

Question 6

Polar bond

Answer 6

Electrons are not shared equally (one atom pulls the electron more than the other because it is more electronegative)

Question 7

Atoms greater than or equal to what atomic number can break the octet rule

Answer 7

15

Question 8

Formal charge

Answer 8

of electrons around the atom in a lewis structure (- bond = 1) compared to the # of valence electrons that atom brings

Question 9

Resonance structures

Answer 9

A lewis structure that represents the possibility of different locations where bonds can exist

Question 10

Sum of individual formal charges =

Answer 10

Total charge of the molecule

Question 11

VSEPR

Answer 11

Valence Shell Electron Pair Repulsion (Electrons want to get as far away from each other as possible)

Question 12

Geometry (in lewis structures)

Answer 12

Structure represented by bonds and lone pairs

Question 13

Shape (lewis structure)

Answer 13

Structure represented by only the bonds

Question 14

2 Bonds (find geometry, bond angle, and hybridization)

Answer 14

Geometry = Linear
Bond angle = 180
Hybridization = sp

Question 15

3 bonds (find geometry, bond angle, and hybridization)

Answer 15

Geometry = trigonal planar
Bond angle = 120
Hybridization = sp2

Question 16

4 bonds (find geometry, bond angle, and hybridization)

Answer 16

Geometry = tetrahedral
Bond angle = 109.5
Hybridization = sp3

Question 17

5 bonds (find geometry, bond angle, and hybridization)

Answer 17

Geometry = trigonal bipyramid
Bond angle = 90 120
Hybridization = sp3d

Question 18

6 bonds (find geometry, bond angle, and hybridization)

Answer 18

Geometry = octahedron
Bond angle = 90
Hybridization = sp3d2

Question 19

Lone pairs, double bonds, and triple bonds do what to bond angles

Answer 19

They all repel more than single bonds which will make the bond angles smaller depending on how you look at it

Question 20

Axial plane

Answer 20

Up and down/side-to-side linear AXIS

Question 21

Equitorial plane

Answer 21

Flat plane, similar to an equator

Question 22

Pi bond

Answer 22

Double or triple bond where orbitals overlap side to side

Question 23

Sigma bond

Answer 23

Single bond where orbitals overlap head to head