Chapter 8

Question 1

No lone pair atoms name their geometries

Answer 1

ABx

Question 2

Lone pairs name their geometries

Answer 2

ABEx

Question 3

Rules for applying VSEPR:

Answer 3

DRAW LEWIS STRUCTURES

Determine A, B, & E lone pairs

The Predict Geometry

Question 4

BeCl2

Answer 4

Linear AB2

Cl—Be—Cl 180degrees each

Cl gets 8 but incomplete octet on Be

Question 5

AB3

Answer 5

Trigonal Planar
120 degrees

Question 6

AB4
AB3e1
AB2e2

All look the same geometry just
e1 has lone pairs on top
E2 has lone pairs on top & bottom left

Answer 6

Tetrahedral 109.5 degrees
Trigonal Pyramidal 107.3 degrees <109.5
Bent 104.5 <109.5

Question 7

AB5

Answer 7

Trigonal bipyramidal

90
120

Question 8

AB5

Answer 8

Trigonal pyramidal
90 degrees
120degrees

Question 9

3 Bs make it Trigonal
2 Bs = bent

Answer 9

Trigonal pyramidal 1LP <109

Bent 1 LP <120

Bent 2LP <90

Question 10

Electronegativity

Answer 10

The ability of an atom to attract electrons and a chemical bond towards itself

Question 11

A covalent bond is made up of?

Answer 11

2 of the same atoms

H—H F—F

Electrons are shared equally

Question 12

If a covalent bond is made up of two different atoms, how are the electrons shared and what is it called?

Answer 12

H—F electrons are not shared equally POLAR COVALENT BOND

Question 13

Pure covalent

Answer 13

Electrons are equidistance from the atoms

Question 14

In an ionic bond

Answer 14

ELECTRONS are TRANSFERRED to each other from positive to negative

Question 15

Polar covalent bond

Answer 15

Electrons are not shared equally

Question 16

Dipole moment is?

Answer 16

Quantitative measure of the polarity of the bond

Symbol is Greek letter u

Units dipoles are measured in are Debyes D

Question 17

Vectors show?

Answer 17

Direction & magnitude

Question 18

Diatomic molecules made up with the same element are

Answer 18

Nonpolar covalent

Question 19

Diatomic molecules made up of different elements are

Answer 19

Polar covalent

Question 20

For molecules made up of three or more elements we must take into account
-POLARITY of the Bond
-and MOLECULAR GEOMETRY

Answer 20

Vectors point from least electronegative to most electronegative

-VECTORS point from LEFT to RIGHT on PT (periodic table)

Question 21

Each single vector is called a

Answer 21

Bond Moment

Question 22

Dipole Moment is the SUM of the individual BOND MOMENTS

Answer 22

I——->
<——I

Cancelled vectors = non polar covalent molecule MEANS NO DIPOLE MOMENT

Question 23

Bent structure 2 vectors that don’t cancel but gives a sum

Answer 23

Bent=Vectors reinforce with a third arrow creating a triangle 🔺

-Representing a polar covalent molecule

= DIPOLE MOMENT - 2 polar bonds of same polarity in different directions connect with a trianglular 3rd side sum

Question 24

Cl Cl
C==C
H H

Figure Dipole Moment

Answer 24

This does have a dipole moment bc we don’t end where we started creating a box that cancels each other or a double line

Dipole Moment

Question 25

Sample Cancel Moment = no dipole moment

Answer 25

Non polar molecule

Question 26

Valence bond theory

Answer 26

—Assumes electrons occupy atomic orbitals of individual atoms; —individual atoms, participate, informing bonds Atomic Orbitals are the 1s2p stuff

Question 27

Molecular orbital theory (MO)

Answer 27

- Atomic orbitals form molecular orbitals

Question 28

Valance Bond theory involves

Answer 28

Hybridization- mixing of atomic orbitals to form hybrid orbitals

Question 29

Hybrid orbitals

Answer 29

Atomic orbitals obtained when two or more non-equivalent orbitals of the same atom combine for covalent bonding Non-equivalent - mixing a 2s & 2p

Question 30

LEWIS STRUCTURE IS

Answer 30

The KEY TO EVERYTHING IN THIS UNIT

Question 31

Hybridization is

Answer 31

The mixing of atomic orbitals to form hybrid orbitals

Question 32

Hybrid orbitals are

Answer 32

Atomic orbitals obtained when two or more non-equivalent orbitals of the same atom combine for covalent bonding

Question 33

How does an electron move from one orbital to another?

Answer 33

We energetically excite the electron to the next higher level

Question 34

CH4 hybridization

Answer 34

1 electron moves from 1s to be the third upward pointing electron in 2p — these 4 filled orbitals represent the four bonds It makes to the carbon atom and CH4. = SP3 hybridization (used 4 atomic orbitals) s, p, p, p were used

Question 35

Incomplete Octet exception & Hybridization

Answer 35

BeCl2 SP hybridization 2 atomic orbitals used, 2 hybrid orbitals 1 in 2s moved to 2p leaving 2 spots available for bonding to the 2 Cl atoms

Question 36

BF3 incomplete octet

Answer 36

Question 37

Do we count full orbitals in our hybridization declaration?

Answer 37

No only the orbitals that have unpaired electrons or moved electrons are counted If there is a full D orbital with 10 electrons in it in the middle, it’s not counted in the SP3D designation

Question 38

If the central atom form the double bonds, what is it automatically as far as hybridization?

Answer 38

SP2

Question 39

At the central atom forms, a triple bond what hybridization is that automatically?

Answer 39

Sp

Question 40

A single bond is represented by?

Answer 40

Sigma

Question 41

A double bond is represented by?

Answer 41

1 sigma 1 pie

Question 42

A triple bond is represented by?

Answer 42

1 sigma 2 pies