Types of Bonding

Flashcards covering the types of bonding, detailed explanations of ionic bonding, rules for writing ionic formulae, and the characteristic properties of ionic compounds including their physical state and electrical conductivity.

Valence Shells

The outermost electron shells of atoms.

Valence Electrons

Electrons in the outermost shell involved in chemical bonding, which can be lost, gained, or shared.

Ionic Bonding

A type of bonding that occurs between a metal atom and a non-metal atom, involving the transfer of electrons.

Covalent Bonding

A type of bonding that occurs only between non-metal atoms, involving the sharing of electrons.

Metallic Bonding

A type of bonding that occurs only between metal atoms.

Ions

Electrically charged particles formed when an atom either loses or gains electrons.

Electron Transfer

The process in ionic bonding where electrons are moved from a metal atom to a non-metal atom.

Electrostatic Attraction

The attractive force between negative anions and positive cations after electron transfer, holding ions tightly together in ionic compounds.

Anions

Negatively charged ions.

Cations

Positively charged ions.

Ionic Compound Charge

The overall charge of an ionic compound, which is neutral.

Crystal Structure

The regular, strong attraction between positive and negative ions forming an organized lattice in ionic compounds.

Octet Rule

The principle that atoms generally seek to have 8 electrons in their valence shell (or 2 for the first shell) to achieve stability.

Group 2 Metal Atoms

Metal atoms with two valence electrons they tend to donate during ionic bonding.

Subscript '2'

In a chemical formula, denotes a ratio of two ions for every one of another ion (e.g., 2 Chlorine ions for every 1 Calcium ion in CaCl2).

Electrovalencies Table

A table that lists cations, anions, and their respective charges, crucial for writing ionic formulae.

Polyatomic Ions

Ions composed of two or more atoms covalently bonded together that carry an overall charge (e.g., OH-, NO3-, CO32-).

Criss-Cross Rule

A method to write ionic compound formulae by using the numerical value of each ion's charge as the subscript for the other ion.

Superscript

A symbol, usually representing charge, written above and to the right of an elemental symbol.

Subscript

A number written below and to the right of an elemental symbol, indicating the ratio of atoms or ions.

Subscript '1' Rule

The convention that the subscript '1' is never explicitly written in chemical formulas.

Brackets in Formulae

Used in chemical formulae when there are two or more of the same polyatomic ion.

Equal Valencies Rule

If both ions have equal valencies, no subscript is required as they simplify (e.g., NaCl instead of Na1Cl1).

High Melting Points (Ionic Compounds)

A property of ionic compounds due to strong bonds requiring significant energy to separate particles.

High Boiling Points (Ionic Compounds)

A property of ionic compounds, even higher than melting points, due to the intense energy needed to overcome strong ionic bonds.

Hard (Ionic Compounds)

A property resulting from a uniform, repeating lattice structure with strong attractions between ions.

Brittle (Ionic Compounds)

A property indicating they will shatter upon striking, as disruption to the lattice causes like-charges to align and repel.

Solubility in Water (Ionic Compounds)

Most ionic compounds dissolve in water to form solutions.

Electrical Conductivity (Solid Ionic Compounds)

Ionic compounds do NOT conduct electricity in solid form because ions are fixed in a lattice and cannot move.

Electrical Conductivity (Molten or Dissolved Ionic Compounds)

Ionic compounds DO conduct electricity when molten or dissolved because their ions are free to move.

Requirements for Electrical Conductivity

A substance must have charged particles (electrons or ions) that are free to move.