Chapter 13: Types Of Chemical Reactions

Front 1

Electronegativity

Back 1

Is the ability of an atom to attract shared pairs of electrons to it.

So, the more electronegative the atom is, the more it will attract electrons.

Smaller atoms (non-metals located on the top right of the periodic table -- least electronegative located on the bottom left) have greater electronegativity.

Front 2

Nonpolar Covalent Bond

Back 2

Is a covalent bond in which the shared electrons are shared equally

Front 3

Polar Covalent Bond

Back 3

Is a covalent bond in which the shared electrons are more attracted to one of the atoms than the other, thereby forming a polar molecule

The shared electrons are more likely to be near the atom whose electronegativity is higher

Front 4

Ionic Character

Back 4

Refers to the percentage of difference between the electronegativity of two covalently bonded atoms

The greater the electronegativity the higher the ionic character

Front 5

Valence Shell Electron Pair Repulsion (VSEPR Theory)

Back 5

Helps predict the shape of any molecule given its Lewis dot structure.

Front 6

Intermolecular Forces

Back 6

Are the forces that exist between molecules

Effects

• Boiling point
• Evaporation
• Solubility
• Evaporation

Front 7

Hydrogen Bond

Back 7

Is an attraction between a slightly positive hydrogen on one molecule and a slightly negative atom on another molecule

It is a dipole-dipole attraction

Strongest among intermolecular forces

Front 8

Dipole-Dipole Force

Back 8

Is when the positive side of a polar molecule attracts the negative side of another polar molecule.

Molecules need to be close together

Front 9

Ion-Dipole Force

Back 9

Is a force between an ion and a polar molecule

Front 10

London Dispersion Force

(Van der Walls)

Back 10

Is the weak intermolecular force that results from the motion of electrons that creates temporary dipoles in molecules.

When the electrons are concentrated more at one end of a molecule, that end becomes slightly negative. The other end, where the electrons are not as concentrated, becomes slightly positive -- all atoms experience this

A London dispersion force works because of the movement of electrons. As you can imagine, the more electrons in the atoms, the stronger the force

London dispersion force increases with increasing atomic mass.

Front 11

Sigma Bond

Back 11

Is when two orbitals directly overlap but there is only one bonding interaction

Front 12

Pi Bond

Back 12

Is weaker than the sigma bond.

This overlap occurs when two orbitals overlap and there are two bonding interactions.

It looks like two dumbbells put side-by-side and overlapped.

Front 13

Hybridization

Back 13

Is the mixing of two or more atomic orbitals to form new orbitals that describe the covalent bonding in molecules

The number of hybrid orbitals is the same as the number of atomic orbitals that participate in the process.

Front 14

Molecular Orbital Theory

Back 14

Describes how the orbital shapes combine when atoms combine into molecules.

It makes the assumption that electrons don't belong to any individual atom, but are under the influence of the entire molecule and belong to the entire molecule as a whole.

Front 15

Metal Bonds

Back 15

Most metals have very few electrons in their outermost energy shells, and some have vacant outer electron orbitals.

What this means for the metal is that its valence electrons are decentralized and free to move around.

Metals do not form; ionic, compound, or molecular bonds

Front 16

Properties of Metal

Back 16

Metal is shiny because it reflects incoming light photons.

It is malleable because the structure and uniform bonding in all directions of the metal allow the atoms to slide past each other without breaking.

Metal conducts electricity well because all of the mobile electrons are free to move towards any attraction.

Front 17

Organic Macromolecules Include Four Classes

Back 17

1. Proteins
2. Carbohydrates
3. Lipids
4. Nucleic Acids

Front 18

Proteins

Back 18

Are formed through a condensation reaction between amino acid monomers

A condensation reaction is when two molecules combine to form a larger molecule but lose a small molecule, kind of like a waste product

Front 19

Lipids

Back 19

Lipids are hydrophobic, meaning they hate water, and contain a lot of C-H bonds

Front 20

Carbohydrates

Back 20

These polysaccharides are made up of monomer monosaccharides, or simple sugars, like fructose and glucose.

Carbohydrates contain only C, H and O.

Front 21

Nucleic Acids

Back 21

Are made up of nucleotide monomers

A nucleotide has three parts - a phosphate group, a five-carbon sugar and a nitrogen base.

Front 22

Saturated Hydrocarbon

Back 22

Are hydrocarbons that contain no rings and contain only single bonds between the different atoms

Makes up what we call "natural gas"

Methane

Front 23

Saturation Formula

Back 23

Saturated hydrocarbons have 2N + 2 hydrogen atoms, where N is the number of carbon atoms in the molecule

Front 24

Alkane

Back 24

A hydrocarbon that contains no double bonds, or hydrocarbon containing only single bonds

Front 25

Alkene

Back 25

Is a hydrocarbon that contains a carbon-carbon double bond

Front 26

Alkynes

Back 26

Hydrocarbons that contain carbon-carbon triple bonds

Front 27

Isomers

Back 27

Molecules that have the same chemical formula but different structures

Front 28

Aromatic Hydrocarbons

Back 28

These hydrocarbons that contain rings consisting of alternating single and double carbon-carbon bonds were initially called this because of their strong smells

Front 29

Functional Groups

Back 29

Atoms or groups of atoms that are responsible for particular chemical properties and reactions of organic compounds.

• Alcolohol
• Alkyl Halides
• Ketone/Aldehydes
• Ethers
• Carboxylic Acids
• Esters

Front 30

Esters

Back 30

Esters are derivatives of carboxylic acids. The -OH of the carboxyl group gets replaced by an -OR from an ether

R-COOR

Front 31

Carboxylic Acids

Back 31

Is a compound with a carboxyl group. A carboxyl group is -COOH

RCOOH

Front 32

Ethers

Back 32

Is an organic compound where oxygen is bonded to two carbon atoms

ROR

Front 33

Aldehydes

Back 33

Is a compound in which the carbon of a carbonyl group shares bonds with two other carbons. A carbonyl group is an oxygen double-bonded to a carbon

RCHO

Front 34

Ketones

Back 34

Is a compound in which the carbon of a carbonyl group shares bonds with two other carbons. A carbonyl group is an oxygen double-bonded to a carbon

RCOR

Front 35

Alkyl Halides

Back 35

An alkyl halide is an organic compound where a halogen atom - F, Cl, Br or I (fluorine, chlorine, bromine or iodine) - takes the place of one or more hydrogens in a hydrocarbon

RX

Front 36

Alcohols

Back 36

Is an organic compound that contains one or more hydroxyl groups

ROH