Atomic Structure and Bonding Vocabulary

Flashcards about Atomic Structure and Bonding

Groups

Vertical columns of the periodic table.

Periods

Horizontal rows of the periodic table, numbered 1, 2, 3, etc.

Chemical Property

A material's property that becomes evident during, or after, a chemical reaction.

Early Periodic Tables

Arranged elements based on known physical and chemical properties (metals combine with one oxygen per atom).

Periodic Table Structure

The result of the electron configuration of the atoms.

Group Number

For the first 20 elements, it represents the number of electrons in the outer electron shell.

Diatomic Molecules

Simple molecules made of only two atoms.

BrINClHOF

Elements that form diatomic molecules, remembered by the mnemonic BrINClHOF.

Alkali Metals

Group I elements; highly reactive and react with water.

Alkaline Earth Metals

Group II elements; also react with water but more slowly.

Halogens

Group VII or 17 elements; highly reactive.

Noble Gases

Group VIII or 18 elements; unreactive.

Protons

Positively charged particles in the nucleus.

Electrons

Negatively charged particles that move around the nucleus.

Neutrons

Particles with no electric charge, located in the nucleus.

Atomic Number

The number of protons present in each atom.

Bohr’s Model of the Atom

Electrons are arranged in concentric spherical shells and can only occupy the shells.

Innermost Shell

The maximum number of electrons it can hold is 2.

Ions

Atoms that gain or lose electrons.

Ions

Atoms form these to become more stable with a full outer electron shell.

Cations

Positively charged ions.

Anions

Negatively charged ions.

Compound

A substance made from atoms of different elements bonded to each other.

Ionic Compounds

Made of oppositely charged ions held together by electrostatic forces called ionic bonds.

Lattice

A regular, repeated three-dimensional arrangement of atoms or ions.

Polyatomic Ions

Molecules that become ions but do not break apart in reactions (e.g., Carbonate, Sulphate, Nitrate, Hydroxide, Phosphate, Ammonium).

Transition Metal Ions

Roman numerals in brackets after the metal’s name indicate its charge.

Valency

The ‘combining power’ of the atoms with other atoms when it forms chemical compounds or molecules. \nCan be defined as the number of H atoms that can combine with the element.

Valence Electrons

Also known as valence electrons, the electrons in the outer electron shell.

Covalent bonds

Compounds form between the atoms of non-metal elements.

Covalent molecules

Valence electrons are shared so that the atoms get full outer electron shells, which is a more stable state for the atoms involved.

Electron Dot Diagrams

Outer shell or valence electrons are shown (represented by dots).

Double Covalent Bond

A double bond.

Naming Rules For Covalent Molecules

The suffix -ide is then added to the stem of the name of the second atom.