Illustrating Ionic Bonding

Bonding

• Bonding:– When two or more atoms come together to

form a _______________________________

• In order for bonding to occur, atoms must:– _______ an electron (s) or– _______an electron (s) or– _______ an electron (s)

Basic Bonding Concepts

• Atoms react in such a way as to achieve a STABLE ELECTRON CONFIGURATION (SEC) – A SEC is the result of a ______ outer energy

level known as a __________________– A full valence shell contains a total of __

electrons– It can be referred to as a _______________– The ____________ represent a stable octet or

SEC because they have a full valence shell – - i.e.: He Ar Xe

Bonding Types

• There are two (2) main types of bonds:– 1) Ionic

• Electrons are ________________ between atoms• Electrons are ________________ by atoms

– 2) Covalent• Electrons are ___________ between atoms

Bonding Type 1 – Ionic Bonds

• Ionic bonds are the result of the ___________ of electrons

• Electrons are _____________________ to achieve a SEC

• Form ionic compounds• IONIC compounds form from the attraction

between _________________________. – The resulting compound is electrically

_________, so the charges must balance out.

Examples of Ionic Bonds Illustrated:

• 1) Potassium & Bromine

• 2) Beryllium & Chlorine

• 3) Calcium & Phosphorus

Binary Ionic Compounds: Naming & Formulas

• Binary Ionic Compounds– Ionic compounds consisting of __________________– Bi = ___ – “Binary” = _______– Part 1

• Monoatomic cation– _____________– _____________ charged– Metal _____________ of periodic table

– Part 2 • Monoatomic anion

– _____________– _____________ charged– Non-metal __________ of the periodic table

Naming Binary Ionic Compounds

• Steps for naming binary ionic compounds:– 1: Metal cation is ALWAYS named first

• Keeps its own name• Do not change the cation name

– 2: Non-metal anion is ALWAYS named second• The ending of the anion name changes to the

suffix, “-ide”

Naming Binary Ionic Compounds

• Examples:– Sodium & chlorine

• ____________________________

– Aluminum & chlorine• ____________________________

– Aluminum & oxygen• ____________________________

– Sodium & sulfur• ____________________________

Transition Metals

• Transition metals are found in the ___________ of the periodic table

• They often have ____________________ ionic charge– Can form ___________________ cations

• Indicate the charge using roman numerals in brackets when naming

• Roman numerals:– ____________________________________– i.e. Iron & Oxygen Iron has two possible charges: Fe 2+ and

Fe 3+

__________________________________________

Binary Ionic Formulas

• Formula:– Representation of a chemical compound

using ___________________________

• The formula of an ionic compound must be _________________

• Therefore the “positives” must equal the “negatives”– *Recall the drawing ionic bonding worksheet

we did

Writing Binary Ionic Formulas

• Step 1. Use your periodic table to determine the symbols and the charges of the atoms involved– Write the symbol out EXACTLY as it appears

on the periodic table remember, the letters are case sensitive!

– Indicate the ionic charge as a superscript– i.e.:

• ____________________________________________

• _______________________________________

Writing Binary Ionic Formulas

• Step 2. Make sure that the “positives” equal the “negatives”. – Do this by crossing or switching the charges and

placing them as subscripts– Subscripts then indicate the NUMBER of atoms in the

formula required to balance the charges once the charges are crossed and become subscripts, they no longer have a charge

– i.e.:• _______________________

• ____________________________________

Tricky Rules

• When an ion has a charge of (+1) or (- 1), there is no need to include it as a subscript– i.e.: _______________________________________

• When a compound has two subscripts that are both even numbers, we want to reduce them to the lowest ratio possible– i.e.:_______________________________________– i.e.:_______________________________________

Writing Formulas with Transition Metals• Remember, transition metals have more than one

charge• How can we determine the charge from a formula alone?• Answer: use the charge of the anion as a guide!• The charge of the anion will always be the same, so

determine the charge of the anion and work backwards• i.e.:

– Fe2S3 Charge on sulfur is ALWAYS 2-• Fe & S2-

• Formula indicates that Fe has gotta be Fe 3+ iron (III) sulfide

– FeS Charge on sulfur is ALWAYS 2-• Fe & S2-

• Formula indicates that Fe has gotta be Fe 2+ iron (II) sulfide

More Examples:

• calcium & iodine

• AlF3

• Iron 3+ & oxygen

• CoF2