Butler Chemistry Unit 4

Front 1

Chemical Bond

Back 1

The force that holds two atoms together

Front 2

Cation

Back 2

A positively charged ion

Front 3

Anion

Back 3

A negatively charged ion

Front 4

Ionic Bond

Back 4

The electrostatic force that holds oppositely charged particles together in an ionic compound

Front 5

Electrolyte

Back 5

An ionic compound whose aqueous solution conducts an electrical current

Front 6

Lattice Energy

Back 6

The energy required to separate one mole of the ions of an ionic compound

Front 7

Formula Unit

Back 7

The simplest ratio of the ions represented in an ionic compound

Front 8

Formula Unit

Back 8

The simplest ratio of the ions represented in an ionic compound

Front 9

Monatomic Ion

Back 9

An one-atom ion

Front 10

Oxidation Number

Back 10

The charge of a monatomic ion

Front 11

Polyatomic Ion

Back 11

Ion made up of more than one atom

Front 12

Oxyanion

Back 12

A polyatomic ion composed of an element usually nonmetals, bonded to one or more oxygen atoms

Front 13

Electron Sea Model

Back 13

Proposes that all the metal atoms in a metallic solid contribute their valence electrons to form this

Front 14

Delocalized Electrons

Back 14

Electrons free to move from one atom to another

Front 15

Metallic Bond

Back 15

The attraction of a metallic cation for delocalized elements

Front 16

Alloy

Back 16

A mixture of elements that have metallic properties

Front 17

Covalent Bond

Back 17

The chemical bond that results from the sharing of valence electrons

Front 18

Molecule

Back 18

Formed when two or more atoms bond covalently

Front 19

Lewis Structures

Back 19

Use electron-dot diagrams to show how electrons are arranged in molecules

Front 20

Sigma Bonds

Back 20

Single covalent bonds; symbolized by greek letter sigma (σ)

Front 21

Pi Bond

Back 21

Formed when parallel orbitals overlap to share electrons; symbolized by greek pi (π)

Front 22

Endothermic

Back 22

Reaction that occurs when a greater amount of the existing bonds in energy is required to break the reactants than is released when the new bonds form in the product molecules

Front 23

Exothermic

Back 23

Reaction that occurs when more energy is released forming new bonds than is required to break bonds in the initial reactants

Front 24

Oxyacid

Back 24

Any acid that contains hydrogen and an oxyanion

Front 25

Structural Formula

Back 25

Uses letter symbols and bonds to show relative positions of atoms

Front 26

Resonance

Back 26

A condition that occurs when more than one valid Lewis Structure can be written for a molecule or ion

Front 27

Coordinate Covalent Bond

Back 27

When one atom donates a pair of electrons to be shared with an atom or ion that needs two electrons to become stable

Front 28

VSEPR (Valence Shell Electron Pair Repulsion) Model

Back 28

The model used to determine the molecular shape in a Lewis Structure

Front 29

Hybridization

Back 29

A process in which atomic orbitals are mixed to form new, identical hybrid orbitals

Front 30

Polar Covalent

Back 30

Results from unequal sharing of electrons in a covalent bond