Bonding, equations and formula Flashcards
What does bonding do
They invole changes in the outermost electron shells of the atom
What are the three types of bonding
Ionic, Covalent, Metallic
What is ionic bonding
A metal and a non metal bonding
What is covalent bonding
2 non metals bonding
What is metallic bonding
Two metals bonding
What happens to metals when they react in ionic bonding
They lose their outermost electrons to leave a full electron shell. This produces a charged atom/ion with a positive charge called cation. This process is called oxidation.
What happens when non metals react in ionic bonding
The non metal gains electrons to achieve a full electron shell. The atom becomes negatively charged and is called an anion. This process is called reduction.
Are the atoms involved in ionic bonding more stable
Yes
What happens to the oppositly charged atoms.
Millions of pairs attract and form a lattice
What does column 1 show
The ions with 1 extra electron
What does column 2 show
The elements which have 2 extra atoms
What does column 3 show
The elements with 3 extra electrons
What does column 6 show
The elements with two electrons missing to achieve a full shell
What does column 7 show
The elements which have 1 electron missing to achieve a full shell
What do transition metals show
The number of electrons can change
What is a complex ion
A ion made out of more than 1 element
Simple ions
Ions only made of 1 type of atom
When working out formulae, when would you use brackets
In compound ions
How would you balance equations
Count the number of atoms on each side. And add big numbers before a compound to change it. Never change the small numbers in a compound
Covalent bonding
Two non metals share pairs of electrons
Strong attraction between bonding pair of electrons and nuclei
Metallic bonding
Metals are held together by metallic bonding
All electrons are delocalised
Attraction between positive ions and electrons
Giant ionic structure characteristics
Crystalline High melting point and boiling point Brittle Soluble in water Do not conduct electricity when solid Electrolyte
Crystalline
Regular arrangement of lattice
Crystals can be seen by microscope
High melting and boiling point
Strong electrostatic forces
Large amount of energy needed to overcome them
Brittle
Distorted crystal will bring together like ions, repel and split crystal
Soluble in water
Electrostatic forces in water overcome electrostatic forces in ion
H+ and -
O2- and +
Insulator of electricity
No free electrons
Electrolyte
Ions are free to move
Simple molecule characteristics
Solid, liquid or gas with low melting point Strong covalent bonds Insulator Non electrolyte Soluble in organic solvents
Low melting point
Small amount of energy breaks weak intermolecular bonds
Insulators
No free delocalised electrons that can move aroun
Not soluble in water unless reacted with
Covalent molecules are not attracted to water molecules enough to break intermolecular forces
Soluble in organic solvents
Solvent molecules are stronger than covalent compounds and break them apart
Giant covalent structure
Diamond, graphite
Diamond
Attached to 4 ions No intermolecular forces High melting point Hard Insulator Insoluble in water
Graphite
Attached to 3 other ions Free delocalised electrons Weak intermolecular forces High melting point Soft and slippery Conductor Insoluble in water
High melting point
Strong covalent bonds have to be overcome by lots of energy
Hard
No intermolecular forces
Strong covalent bonds
Soft and slippery
Layers of weak intermolecular forces broken easily
Insulator
No free electrons
Conductor
1 free delocalised electrons per carbon atom
Insoluble in water
Covalent bonds too strong
Metallic bonding
High melting and boiling points
Conductors of heat
Malleable
Ductile
High melting and boiling point
High attraction between ions
Large amount of energy needed to overcome attraction
Conductors of heat
Delocalised electrons move through lattice
Malleable, ductile
Electron can take shape of object
Electrostatic forces keep metal together
Ions move in layers by sliding over each other
Uses of diamond
Cutting
Uses of graphite
Lubrication
