Chemistry Test 2 Ch 5

Front 1

In forming bonds, main group elements gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons.

Back 1

Octet Rule

Front 2

A measure of the relative tendency of an atom to attract electrons to itself.

Back 2

Electronegativity

Front 3

An atom or group of bonded atoms that has a negative charge.

Back 3

Anion

Front 4

An atom or group of bonded atoms that has a positive charge.

Back 4

Cation

Front 5

A representation of a molecule, ion, or formula unit by atomic symbols with the valence electrons shown as dots.

Back 5

Lewis dot symbol

Front 6

The attraction between positive and negative ions.

Back 6

Ionic bond

Front 7

Compounds composed of positive and negative ions.

Back 7

Ionic compounds

Front 8

In ionic compounds, the simplest ratio of oppositely charged ions that gives an electrically neutral unit

Back 8

Formula Unit

Front 9

Chemical compound composed of two elements

Back 9

Binary compound

Front 10

A positive or negative ion composed of two or more atoms.

Back 10

Polyatomic ion

Front 11

A bond in which two atoms share electrons

Back 11

Covalent bond

Front 12

Pairs of electrons shared between two atoms, frequently represented by lines (instead of dots) for convenience in Lewis structures

Back 12

Bonding pairs

Front 13

Pairs of valence electrons that are not shared between to atoms in the Lewis structure but instead are associated with a single atom in the structure; should always be shown as dots in lewis structures.

Back 13

Lone Pairs

Front 14

Compounds containing only carbon and hydrogen

Back 14

Hydrocarbons

Front 15

Hydrocarbons with carbon-carbon single bonds

Back 15

Alkanes

Front 16

Different compounds with the same formula but different structures

Back 16

Isomers

Front 17

Hydrocarbons that are alkanes

Back 17

Saturated hydrocarbons

Front 18

A bond in which two pairs of electrons are shared between two atoms

Back 18

Double bond

Front 19

A bond in which three pairs of electrons are shared between two atoms

Back 19

Triple bond

Front 20

Two or more possible Lewis dot representations of a molecule or ion in which the only difference is the position of the valence electrons.

Back 20

Resonance Structures

Front 21

Amount of energy required to break one mole of bonds between a specified pair of atoms

Back 21

Bond Energy

Front 22

Hydrocarbons with one or more carbon-carbon double bonds

Back 22

Alkenes

Front 23

Hydrocarbons that contain fewer than the maximum number of hydrogen atoms; alkenes and alynes

Back 23

Unsaturated hydrocarbons

Front 24

Describes a bond or molecule which is not polar because it has no polar bonds or because its polar bonds are oriented symmetrically so that they cancel each other

Back 24

Nonpolar

Front 25

Describes a bond or molecule in which charge is unevenly distributed, creating positive and negative regions

Back 25

Polar

Front 26

A compound that conducts electricity when melted or dissolved in water

Back 26

Electrolyte

Front 27

A compound that does not conduct electricity when melted or dissolved in water

Back 27

Nonelectrolyte

Front 28

Attractive forces that act between molecules; weaker than covalent bonds

Back 28

Intermolecular forces

Front 29

Attraction between a hydrogen atom bonded to a highly electronegative atom (O, N, F) and the lone pair on an electronegative atom in another or the same molecule.

Back 29

Hydrogen bonding

Front 30

The change of molecules from the gaseous state to the liquid state

Back 30

Condensation

Front 31

A state of matter that is capable of flowing; a gas or a liquid

Back 31

Fluid

Front 32

Force per unit area

Back 32

Pressure

Front 33

Ability to mis in all proportions

Back 33

Miscibility

Front 34

Easily vaporized

Back 34

Volatile

Front 35

The pressure above a liquid caused by molecules that have escaped from the liquid surface

Back 35

Vapor pressure

Front 36

The temperature at which the vapor pressure of a liquid equals the atmospheric pressure and boiling occurs.

Back 36

Boiling Point

Front 37

If the atmospheric pressure is 1 atm

Back 37

Normal boiling point

Front 38

In a solution, the substance present in the greater amount

Back 38

Solvent

Front 39

In a solution, the substance dissolved in the solvent

Back 39

Solute

Front 40

The maximum quantity of a solute that will dissolve in a given amount of a solvent at a specified temperature

Back 40

Saturated Solution

Front 41

Solution in which less than the maximum amount of solute is dissolved at a given temperature

Back 41

Unsaturated Solution

Front 42

Describes a substance that will not dissolve in a given solvent

Back 42

Insoluble

Front 43

The temperature at which a solid substance turns into a liquid

Back 43

Melting point

Front 44

Formation of a crystalline solid from a melt or a solution

Back 44

Crystallization (solidification)

Front 45

The process whereby molecules escape from the surface of a solid into the gas phase

Back 45

Sublimation