Chemical Bonding Flashcards
List the type of chemical bonds
-ionic
-covalent
-metallic
List the type of forces
-intermolecular(van der Waals)
-London dispersion forces
-dipole-dipole forces
Define Ionic bonds
These are bonds formed between metals and non metals where the electronegativity difference is at least 1.67 leading to a loss and gain of electrons.
Briefly define a Covalent bond
This is a bond that results due to similarity in electronegativity values in non metals leading to sharing of electrons.The electronegativity difference is less than 0.4.
Give an example of elements that can form ionic bonds
Oxygen and Magnesium
Sodium and Chlorine
Give examples of proper covalent bonds
N2(Nitrogen) , O2(Oxygen ),Cl2 (Chlorine)
(diatomic molecules)
Give examples of polar covalent bonds
Water
(Because the hydrogen has a partially positive charge and the oxygen has a partially negative charge) so it is polar
What is meant by polar?
It means that there is an uneven distribution of charge
Briefly define a polar Bond
This is a bond that results due to electronegativity difference between 0.4 and 1.67 in non-metals leading to unequal sharing of electrons. For example the bond between oxygen and hydrogen.
Briefly define a metallic Bond
This is a bond that occurs between a sea of delocalized electrons and ions.
Define intermolecular bonds
These are bonds that occur due to weak forces or bonds that occur between different molecules or compounds.
What causes dipole-dipole forces?
These occur as a result of different charges on molecules.
What causes hydrogen bonding?
This is a result of forces between hydrogen and either flourine ,oxygen or nitrogen.
What causes London dispersion forces?
This occur as a result of unequal distribution of electrons.
What do forces have an effect on when it comes to compounds?
Forces have an effect on melting points and boiling points and the ability to dissolve a substance in another.