Ionic Bonding

Definition: electrons being transferred between atoms specifically between the non metal and metal where the metal is always the electron donor and the non metal is the electron acceptor

• they attain their nearest inert noble gas configuration

• atoms with greater electronegativity difference

• the higher energy electrons leave the less electronegative element

• all ionic compounds dissolve in water

• forms crystalline structure

Chemical Formulas

*like a reduced fraction, instead of saying 6/8 you can say ¾

Ionic compound: an array of cations and anions (can vary from sample from sample)

• formed from a cation and an anion (negatively charged ion)

• have electrically neutral formulas ( same number of gain and loss of electrons )

• subscripts tells to balance the charges to get the electrically neutral compound

Monoatomic: one atom in ions

Polyatomic: many atom ions (charged groups of covalently bound atoms)

https://www.studystack.com/flashcard-907510

Main group ions: First two and last six group

Oxidation States, Polyatomic ions

Ion formtaion:

Metals

• small ionization energy lose electrons and become cations

Non Metals

• large electronegativity

• low energy open orbitals

• gain electrons often by taking the electrons away from metals forming anions

Driving forces:

• system wants to lower its energy by leaving metals and joining metals

• atoms of the main group want to become isoelectronic with the noble gas

Oxidation States: electron accounting system (treat most bonds as ionic bonds)

follow in order

1) Pure elements have an oxidation state of 0

2) A compound with fluorine and a different type of element: Fluroine has an oxidation sttae of 1-

3) Metals: 1A are +1, 2A are +2 and AL are +3

a) alkali earth metals

a) 1A: Li, NA, K, Rb

2A: Be, Mg, Ca

4) H is usually +1 (which is a proton) (can be -1 with a metal if it encounters the metal like sodium)

because hydrogen has an open orbital inner energy H^-1 = hydride w two electrons

5) O is usually -2 but it can be -1

6) Halogens are usually -1

• oxidation states should result in a net charge of 0

• Ions: overallcharge on ion = sum

• Neutral molecules: sum = zero

F2 = molecule in elemental state

oxidation state=0

• needs to add up to -3 since it’s the overall charge

Naming ionic compounds

1. Naming Ions (combination of cation + anion)

   1. monoatomic cation: no change in name

   2. monoatomic anion: change the ending of the name of the element to -ide

      1. fluorine F1- fluoride

2. 2 cases for compounds

   1. Cation can only assume a single oxidation state - true for alkaline earth metals, a few of transition metals and aluminium

      1. sodium +1 charge sodium ion or sodium anion

      2. alkaline earth metals: calcium (metallic calcium calcium 0) or lose its valence electron for charge +2

      3. transition metal: silver has plus one oxidation state, zinc +2, aluminum +3

   2. Name: cation anion (ide)

3. Some instances where there’s groups of non metals that make a cation (ammonium) & still have an ionic compound

second case (when metals adopt more than one oxidation state (most transition metals and larger Group 3A and 4A metals)

• oxidation states indicated in roman numerals in parantheses after the metal

  • applies to transition metals (3-12)

    • exceptions: silver and zinc

• Name: metal (oxidation state) anion

  • Examples: FeBr2 is iron(II) bromide

    

• More electrons in the same level, gets closer Cl is smaller than NA.

Particle diagram of Hallite and Mica: