Chapter 2: Structure And Properties Of Organic Molecules

Front 1

Acid Chloride

Back 1

- An acid derivative with a chlorine atom in place of the hydroxyl group

Front 2

Alcohol

Back 2

- A compound that contains a hydroxyl group bonded to a carbon atom

- R-OH

Front 3

Aldehyde

Back 3

- A carbonyl group with one alkyl group and one hydrogen

Front 4

Alkanes

Back 4

- Hydrocarbons containing only single bonds

Front 5

Alkenes

Back 5

- Hydrocarbons containing one or more C=C double bonds

Front 6

Alkyl group

Back 6

- A hydrocarbon group with only single bonds

- An alkane with one hydrogen removed, to allow bonding to another group

- Symbolized by R.

Front 7

Alkynes

Back 7

- Hydrocarbons containing one or more carbon carbon triple bonds

Front 8

Amide

Back 8

An acid derivative that contains a nitrogen atom instead of the hydroxyl group of the acid

Front 9

Amine

Back 9

- An alkylated analogue of ammonia

- R-NH2, R2NH, or R3N

Front 10

Aromatic Hydrocarbons

Back 10

- Arenes

- Hydrocarbons containing a benzene ring

- A six-membered ring with three double bonds

Front 11

Bond Dipole moment

Back 11

- A measure of the polarity of an individual bond in a molecule

Front 12

Carbonyl Group

Back 12

- A functional group with a carbon double bonded to an oxygen

- Ketone

- Aldehyde

Front 13

Ketone

Back 13

- Two alkyl groups bonded to the carbonyl group

- "one" suffix

Front 14

Aldehyde

Back 14

- One alkyl group and a hydrogen atom bonded to the carbonyl group

- "al" or "aldehyde" suffix

Front 15

Carboxyl Group

Back 15

- The -COOH functional group, as in a carboxylic acid

Front 16

Carboxylic Acid

Back 16

- A compound that contains the carboxyl group

-COOH

Front 17

Cis-Trans Isomers

Back 17

- Geometric Isomers

- StereoIsomers that differ in their cis-trans arrangement on a double bond or on a ring.

- The cis isomer has similar groups on the same side, and the trans isomer has similar groups on opposite sides

Front 18

Constitutional Isomers

Back 18

- Structural Isomers

- Isomers whose atoms are connected differently; they differ in their bonding sequence

Front 19

Cyano Group

Back 19

- Nitrile

- A functional group with a carbon triple bonded to a nitrogen

Front 20

Dipole-Dipole forces

Back 20

- Attractive intermolecular forces resulting from the attraction of the positive and negative ends of the permanent dipole moments of polar molecules

Front 21

Bond Dipole Moment

Back 21

- The measure of the polarity of an individual bond

Front 22

Molecular Dipole Moment

Back 22

- The vector sum of the bond dipole moments (and any nonbonding pairs of electrons) in a molecule

- A measure of the polarity of a molecule

Front 23

Double Bond

Back 23

- A bond containing four electrons between two nuclei

- One pair of electrons forms a sigma bond, and the other pair forms a pi bond

Front 24

Ester

Back 24

- An acid derivative with an alkyl group replacing the acid proton

Front 25

Ether

Back 25

- A compound with an oxygen bonded between two alkyl (or aromatic) groups; R-O-R'

Front 26

Functional Group

Back 26

- The reactive, nonalkane part of an organic molecule

Front 27

Geometric Isomers

Back 27

- Cis-trans isomers

- Differ in the geometry of the groups on a double bond

Front 28

Hybrid Atomic Orbital

Back 28

- A directional Orbital formed from a combination of s and p orbitals on the same atom

- sp, sp2, sp3 hybrid orbtials

Front 29

sp Hybrid Orbitals

Back 29

- Give two orbitals with a bond angle of 180 degrees

Front 30

sp2 Hybrid Orbitals

Back 30

- Give three orbitals with bond angles of 120 degrees

Front 31

sp3 Hybrid Orbitals

Back 31

- Give four orbitals with bond angles of 109.5 degrees

Front 32

Hydrocarbons

Back 32

- Compounds composed exclusively of carbon and hydrogen

- Alkanes, Alkenes, Alkynes, Cycloalkanes, Cycloalkanes, Cycloalkanes, Aromatic hydrocarbons

Front 33

Alkanes

Back 33

- Hydrocarbons containing only single bonds

Front 34

Alkenes

Back 34

- Hydrocarbons containing one or more carbon carbon double bonds

Front 35

Alkynes

Back 35

Hydrocarbons containing one or more carbon carbon triple bonds

Front 36

Cycloalkanes, Cycloalkanes, Cycloalkynes

Back 36

- Alkanes, alkenes, and alkynes in the form of a ring

Front 37

Aromatic Hydrocarbons

Back 37

- Hydrocarbons containing a benzene ring

Front 38

Benzene ring

Back 38

- A six-membered ring with three double bonds

Front 39

Hydrogen bond

Back 39

- A particularly strong attraction between a nonbonding pair of electrons and an electrophilic O-H or N-H hydrogen

Front 40

Hydroxyl group

Back 40

- An alcohol

- The -OH functional group

Front 41

Isomers

Back 41

- Different compounds with eh same molecular formula

Front 42

Consistituaional Isomers

Back 42

- Structural Isomers

- Connected differently

- Differ in their bonding sequence.

Front 43

Cis-trans isomers

Back 43

- Geometric Isomers

- Stereoisomers that differ in their cis-trans arrangement on a double bond or ring

Front 44

Stereoisomers

Back 44

- Differ only in how their atoms are oriented in space

Front 45

Linear Combination of Atomic Orbitals (LCAO)

Back 45

- Wave functions can add to each other to produce the wave functions of new orbitals

- The number of new orbitals generated equals the original number of orbitals

Front 46

London Dispersion Forces

Back 46

- Intermolecular forces resulting from the attraction of correlated temporary dipole moments induced in adjacent molecules

Front 47

Molecular Orbital (MO)

Back 47

- When orbitals on different atoms interact

- An orbital formed by the overlap of atomic oribtials on different atoms

- MOs can be bonding or nonbonding, but only the bonding MOs are filled in most stable molecules

Front 48

Bonding Molecular Orbital

Back 48

- Places a large amount of electron density i the bonding region between the nuclei.

- The energy of an electron in a bonding MO is lower than it is in an atomic orbital

Front 49

Antibonding Molecular Orbital

Back 49

- Places most of the electron density outside the bonding region.

- The energy of an electron in an antibonding MO is higher than it is in an atomic orbital

- When two hydrogen 1s orbitals overlap out of phase with each other

Front 50

Nitrile

Back 50

- A compound containing a cyan group

- A carbon triple bonded with a nitrogen

Front 51

Node

Back 51

- In an orbital, a region of space with zero electron density

- The midpoint of the wave function

Front 52

Pi bond

Back 52

- A bond formed by sideways overlap of two p orbitals

- A pi bond has its electron density in two lobes, one above and one below the line joining the nuclei.

Front 53

Sigma bond

Back 53

- Single bonds

- All double or triple bonds contain one sigma bond

- A bond with most of its electron density centered along the ling joining the nuclei

- A cylindrically symmetrical bond

- The most common bonds in organic compounds

Front 54

Stereochemistry

Back 54

- The study of the structure and chemistry of stereoisomers

Front 55

Structural Isomers

Back 55

- Constitutional Isomers

- Isomers who's atoms are connected differently

- Differ in their bonding sequence

Front 56

Triple Bond

Back 56

- A bond containing six electrons between two nuclei.

- One pair of electrons forms a sigma bond and the other two pairs form two pi bonds at right angles to each other

Front 57

Valence-shell Electron-pair Repulsion Theory (VSEPR theory)

Back 57

- Bonds and lone pairs around a central atom tend to be separated by the largest possible angles

- 180 degrees for two

- 120 degrees for three

- 109.5 for four

Front 58

Van Der Waals Forces

Back 58

- The attractive forces between neutral molecules

- Dipole-dipole forces

- London dispersion forces

Front 59

Dipole-Dipole Forces

Back 59

- The forces between polar molecules resulting from the attraction of their permanent dipole moments

Front 60

London Forces

Back 60

- Intermolecular forces resulting from the attraction of correlated temporary dipole moments induced in adjacent molecules

Front 61

Wave function

Back 61

- The mathematical description of an orbital.

- The square of the wave function is proportional to the electron density

Front 62

Traveling Waves

Back 62

- Sound Waves that carry a thunderclap

- Water waves that form the wake of a boat

Front 63

Standing Waves

Back 63

- Vibrate in a fixed location

- Found inside an organ pipe, where the rush of air creates a vibrating air column

- The wave pattern of a guitar string when it is plucked

- An electron in an atomic orbital is like a stationary bound vibration

Front 64

The Plus and Minus Sign of Wave Functions

Back 64

- Not charges

- The instantaneous phase of the constantly changing wave function

Front 65

Hybrid Atomic Orbitals

Back 65

- When orbitals on the same atom interact

- Define the geometry of the bonds

Front 66

The stability of a covalent bond results from what?

Back 66

- The large amount of electron density in the bonding region, the space between the two nuclei

Front 67

Bond Length

Back 67

- The internuclear distance where attraction and repulsion are balanced

- Gives the minimum energy (the strongest bond)

Front 68

What makes a compound stable in terms of bonding orbitals and antibonding orbitals?

Back 68

- In stable compounds, all or most of the bonding orbitals will be filled, and all or most of the antibonding orbitals will be empty.

Front 69

How can the 1s wave functions of hydrogen add?

Back 69

- Constructively so that they reinforce each other

- Destructively so that they cancel out where they overlap

Front 70

When drawing three-dimensional molecules what should you not do when showing perspective?

Back 70

- When showing perspective, do not draw another bond between the two bonds in the plane of the paper.

- This leads to incorrect shape.