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)

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.: HeArXe

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.:_______________________________________

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.: –Fe 2 S 3  Charge on sulfur is ALWAYS 2- Fe & S 2- Formula indicates that Fe has gotta be Fe 3+  iron (III) sulfide –FeS  Charge on sulfur is ALWAYS 2- Fe & S 2- Formula indicates that Fe has gotta be Fe 2+  iron (II) sulfide

More Examples: calcium & iodine AlF 3 Iron 3+ & oxygen CoF 2