Organic Chemistry Chapter 2

Front 1

What is a functional group

Back 1

common and specific arrangements of atoms that impart predictable reactivity and properties to a molecule

Front 2

What do all alcohol's contain?

Back 2

An OH (Hydroxyl) functional group attached to a saturated carbon bearing nothing else but carbon or hydrogen

Front 3

What are hydrocarbons?

Back 3

compounds that contain only carbon and hydrogen. They are Alkanes, Alkenes, Alkynes and Aromatic Compounds

Front 4

Methane (CH4) and Ethane (C2H6) are examples of which hydrocarbon group?

Back 4

Alkanes

Front 5

Which hydrocarbon group does not have multiple bonds between carbon atoms

Back 5

Alkanes (compounds ending in
-ane

Front 6

Which hydrocarbon group has at least one carbon-carbon double bond

Back 6

Alkenes (compounds ending in
-ene

Front 7

Which hydrocarbon group has at least one carbon-carbon triple bond

Back 7

Alkynes (compounds ending in
-yne

Front 8

Which hydrocarbon group contains a special type of ring, the most common example of which is benzene

Back 8

Aromatic Compound

Front 9

What's a saturated compound?

Back 9

Compounds such as alkanes, whose molecules contain only single bonds are referred to as saturated because these compounds contain the maximum number of hydrogen atoms that the carbon compound can posses.

Front 10

What's an unsaturated compound?

Back 10

Compounds with multiple bonds such as alkenes, alkynes and aromatic hydrocarbons because they possess fewer than the maximum number of hydrogen atoms. They are capable of reacting with hydrogen under the proper conditions

Front 11

What is the primary source of alkanes?

Back 11

gas and petroleum. Smaller alkanes are methane and butane

Front 12

Methanogens take in what gases and produce what gas.

Back 12

Take in carbon dioxide and hydrogen and produce methane. They are believed to be earth's oldest organisms. They can only survive in anaerobic environments

Front 13

What is a polar covalent bond?

Back 13

If the electronegativity difference existing between two bonded atoms is small, the electrons are not being shared equally, and example is hydrogen chloride, where the hydrogen bears a partial positive charge and the chorine atome bears a partial negative charge.

Front 14

The polar covalent bond of Hydrogen Chloride can also be referred to as a

Back 14

dipole moment

Front 15

Atoms such as Oxygen, Nitrogen and Sulfur that form covalent bonds and have unshared electron pairs are called

Back 15

heteroatoms

Front 16

Any diatomic molecule of two different atoms will have a

Back 16

dipole moment.

Front 17

A molecule with a dipole moment is

Back 17

polar

Front 18

Does carbon tetrachloride (CCl4) have a dipole moment? Why or why not?

Back 18

It does not because it is simmetrical and the bond moments are vectors of equal magnitude arranged tetrahedrally, their effects cancel out.

Front 19

Which has a higher melting point / boiling point, A cis or trans isomer? Which has a dipole moment

Back 19

Generally, Cis have higher melting points and boiling points and dipole moments, trans do not have dipole moments, they have lower melting and boiling points.

Front 20

What is the melting point

Back 20

The melting point of a substance is the temperature at which an equilibrium exists between
the well-ordered crystalline state and the more random liquid state.

Front 21

What is the melting point

Back 21

The melting point of a substance is the temperature at which an equilibrium exists between
the well-ordered crystalline state and the more random liquid state.

Front 22

What are the ion-ion forces?

Back 22

the ion–ion forces that hold the ions
together in the crystalline state are the strong electrostatic lattice forces that act between
the positive and negative ions in the orderly crystalline structure.

Front 23

List the Intermolecular Forces (van der Waals Forces) in order of Strongest to Weakest

Back 23

Hydrogen Bonds
Dipole-Dipole forces
Dispersion Forces

Front 24

How do dipole-dipole forces cause molecules to align themselves

Back 24

dipole–dipole attractions cause the molecules to orient themselves so that
the positive end of one molecule is directed toward the negative end of another

Front 25

What is a Hydrogen Bond

Back 25

Very strong dipole–dipole attractions occur between hydrogen atoms bonded to
small, strongly electronegative atoms (O, N, or F) and nonbonding electron pairs
on other such electronegative atoms.

Front 26

What is the boiling point?

Back 26

The boiling point of a liquid is the temperature at which the vapor pressure of the liquid
equals the pressure of the atmosphere above it.

Front 27

What can happen to a molecule when passing from a liquid to a gaseous state? (boiling)

Back 27

In passing from a liquid to a gaseous state, the individual molecules (or ions) of the substance
must separate. Because of this, we can understand why ionic organic compounds
often decompose before they boil. The thermal energy required to completely separate
(volatilize) the ions is so great that chemical reactions (decompositions) occur first.

Front 28

What can happen to a molecule when passing from a liquid to a gaseous state? (boiling)

Back 28

In passing from a liquid to a gaseous state, the individual molecules (or ions) of the substance
must separate. Because of this, we can understand why ionic organic compounds
often decompose before they boil. The thermal energy required to completely separate
(volatilize) the ions is so great that chemical reactions (decompositions) occur first.

Front 29

What is solubility?

Back 29

The orderly
crystal structure of the solid is destroyed, and the result is the formation of the more disorderly
arrangement of the molecules (or ions) in solution.

Front 30

Why is water a good solvent?

Back 30

Because water is highly polar, and because water is capable of forming strong hydrogen
bonds, the ion–dipole forces of attraction are also large. The energy supplied by the
formation of these forces is great enough to overcome both the lattice energy and interionic
attractions of the crystal.

Front 31

Why is water a good solvent?

Back 31

Because water is highly polar, and because water is capable of forming strong hydrogen
bonds, the ion–dipole forces of attraction are also large. The energy supplied by the
formation of these forces is great enough to overcome both the lattice energy and interionic
attractions of the crystal.

Front 32

What is Infrared (IR) spectroscopy

Back 32

is a simple and rapid instrumental technique that can give evidence
for the presence of various functional groups.