It's the TRANSFER of electrons FROM a METAL atom TO a NON-metal atom.
ionic bonding
The METAL atom LOSES electrons to be a POSITIVELYcharged ion, while the NON-METAL atom GAINS THOSE electrons to become a negatively charged ion.
All ionic bonds has strong electrostatic forces holding each other, which is why they have highmelting points - they need a lot of energy to break the forces.
Lithium has ONE outer shell electron, and Fluorine has SEVEN.
For BOTH atoms to get stability and a full outer shell is LITHIUM to TRANSFER ONE electron to FLUORINE.
Lithium LOSESONE electron and forms a positiveion and Fluorine gainsone electron and forms a negativeion.
Both ions are OPPOSITELY CHARGED.
The Li+ and F- join to give the final formula for Lithium Fluoride as LiF.
Lithium has ONE outer shell electron, but Oxygen has SIX.
Lithium LOSESONE electron, but Oxygen GAINsTWO, so twoLithiumatoms react with oneoxygenatom to form ions with fulloutershells.
The Li+ and O2- join to give the final formula for Lithium Oxide as Li2O.
calcium loses 2 outer electrons to oxygen atoms and forms Ca2+
oxygen gains 2 outer electrons to form O2-.
Electrostatic forces of attraction pulls the ions together to form CaO.
Magnesium losestwoelectrons and chlorine gainsoneelectrons, so there's onemagnesium and twochlorines and formsionicbonds.
Ionic compounds
known for their GIANTIONICLATTICE structure, which consists of a 3D arrangement where ions are held together by strong ELECTROSTATICFORCES of attraction in ALLDIRECTIONS.
Metals and Non-Metals that combine with IONICBONDING form IONICCOMPOUNDS.
Key Properties of Ionic Compounds
HIGH MELTING AND BOILING POINTS:
since they have lattice structure that are held together by STRONG ELECTROSTATIC FORCES of attraction between the OPPOSITELY CHARGED ions, it will need a lot of energy to break.
Key Properties of Ionic Compounds
ELECTRICALCONDUCTIVITY when molten or aqueous:
When ionic compounds are MOLTEN or AQUEOUS, the IONS are FREETOMOVE, meaning they can CARRYACHARGE and conductelectricity.
MOLTEN
MELTED to liquid.
AQUEOUS
DISSOLVED in water to make a SOLUTION.
Key Properties of Ionic Compounds
ELECTRICALCONDUCTIVITY when SOLID:
IONS in the solid are FIXED meaning the IONS are NOT free to move, so they CAN’T carry a charge and conduct electricity.
Key Properties of Ionic Compounds
SOLUBILITY:
Many ionic compounds CANDISSOLVE in water, allowing the ions to separate and movefreely.
Determining the Formula of an Ionic Compound:
You can do this by SWAPPING the numbers of their charges and the amount of each element.
Calcium has a charge of +2 because it is in group 2.
Chlorine has a charge of -1 because it is in group 7.
State how you can tell from a dot and cross diagram that the particles in a compound are held together by ionic bonds.
The particles in a compound are oppositely charged ions. The bonds is formed by electrons transfer.
Advantages of dots and cross diagrams:
charge of the ions
the arrangement of electrons in an atom or ion
which atoms the electrons in an ion originally come from
empirical formula (correct ratio of ions)
disadvantages of dots and cross diagrams:
show the structure of the compound
correctly represent the size of the ions
describe the structure of a crystal of sodium chloride.
Sodium chloride crystal consists of sodium ions (Na+) and chloride ions (Cl-) arranged in a repeating 3Dpattern with strong electrostatic forces holding them together.
Ions
Atoms that has gained or lost electrons.
DOT AND CROSS DIAGRAMS
represents the ARRANGEMENT of electrons in atoms or ions where each electron is a dot or a cross and shows where the electrons originally came from.
Chemical bonds:
ionic bonds
covalent bonds
metallic bonds
ionic bonds are the attraction between positive and negative ions.