Chemical Bonding (Intramolecular) Flashcards
Ionic Bonding is between ____________ &____________________
Ionic Bonding is between METALS & NON-METALS
In an Ionic Bond Metals ________electrons, giving it a __________ charge
In an Ionic Bond Metals LOSE electrons, giving it a POSITIVE charge
In an Ionic Bond Non- Metals ________electrons, giving it a __________ charge
In an Ionic Bond Non- Metals GAIN electrons, giving it a NEGATIVE charge
What is a Cation?
Positive Ion
What is a Anion?
Negative Ion
What is the Ionic Lattice?
Positive and negative ions attract each other to form a three dimensional continuous lattice structure.
The _______ is written first in the ionic formula
Cation (Metal)
Ionic Bonding- Boiling Point
High. The is a large amount of thermal energy required to separate the ions which are bound by strong electrostatic forces.
Ionic Bonding- Electro conductivity in Solid
No- there are no mobile charge particles to conduct an electric current
Ionic Bonding- Electro conductivity in Liquid
Yes- the cations and anions are able to move and conduct electricity
Ionic Bonding- Hardness
Very Hard- The surface of crystals are not easily scratched as the ions are strongly bound and not easily displaced
Ionic Bonding- Brittleness
Very Brittle- Shatter if you try to distort is. Distortion causes ions of like charges to come together and repel sharply
Covalent Bonding is between ________
Covalent Bonding is between NON-METALS
Covalent Bonding is the __________ of electrons
Covalent Bonding is the SHARING of electrons
Ionic Bonding is the ____________ of electrons
Ionic Bonding is the TRANSFER of electrons
In covalent Bonding electrons are shared according to ______________
In covalent Bonding electrons are shared according to ELECTRONEGATIVITY
Covalent Bonding- Electroconductivity
No- there are no mobile charged particles as the electrons are bound tightly to the atoms or are shared by atoms in covalent bonds
Covalent Bonding- Melting and Boiling Points
Low- the forces of attraction between molecules are weak, requiring a small amount of thermal energy to seperate
Covalent Bonding- Hardness
Soft- The molecules are weakly attracted to each other and are easily displaced
What is Covalent Network?
Do not form separate discrete molecules but a continuous network
Covalent Network- Electrical Conductivity
Poor- electrons are held tightly together on atoms or within covalent bonds, preventing electrons from moving through the lattice. Graphite is the exception as it has a free electron
Covalent Network- Melting Point
Very High- the atoms are bound by strong covalent bonds. In order to break the many covalent bonds a large amount of thermal energy is required
Covalent Network- Hardness
Strong- the atoms are strongly bound and not easily displaced
Covalent Network- Brittleness
Very Brittle- when a sufficient amount of force is applied to break the covalent bond, the lattice is distorted.
Covalent Networks shatter rather than deform
What is Metallic Bonding?
A Metallic Bonds are the delocalised electrons moving over tightly packed metal cations
Metals- Density
Very Dense- the particles present in Metals are tightly packed in a lattice
Metals- Melting & Boiling Points
High- a large amount of thermal energy is required to overcome the strong electrostatic attraction between the positive ions and delocalised electrons
Metals- Heat and Electricity Conductors
Very Good- the delocalised electrons transmit the energy through vibrations from one positive ions to its neighbour
Difference between Metals and Covalent Network
Metals have conduct electricity well, whereas Covalent Networks do not.
Explain the difference in the Melting Points of different Metals.
E.g Potassium +1 is 64 degrees whereas Calcium Ca+2 is 850 degrees.
Metallic Ca+2 has twice as many delocalised electrons which create an electrostatic attraction that is twice as strong between the electrons and positive ions.
