Atoms Combining Flashcards
Ionic Bonds
Metal+ Non Metal
Loss and gain of electrons takes place
Contains Charged particles
Strong bonds- Strong electrostatic forces of attration between charged particles
High melting and boiling points as it takes a lot of heat energy to overcome the electrostatic forces of attraction
Can conduct electricity in liquid form as ions are free to move
They are water soluable
Covalent Bonds
Non Metal+ Non Metal
Sharing of electrons
No charged particles
Weaker bonds- Low melting and boiling points
Can’t conduct electricity as there are no charged particles
They are insoluable in water
Metallic Bonds
It is a bond between positively charged ions and negatively charged delocalised electrons
Properties of Metals:
They are hard and strong- Strong forces of attraction between positively charged ions and negatively charged delocalised electrons
Malleable and Ductile
High Melting and Boiling Points
Good conductors of heat and electricity- Sea of free electrons
Polar and Non- Polar Covalent Bonds
Polar Covalent Bonds: Difference in Electro Negativity Partial + or - charge Conduct electricity Soluable in water
Non- Polar Covalent Bonds: No or barely any difference in Electronegativity No charge Cant conduct electricity Insoluable
Diamond
Tetrahedral structure
Every carbon is bonded to four other carbons
Hard and Strong- Every carbon has all the bonds complete and hence strong covalent bonds between C-C
MP and BP- Strong covalent bonds between C-C hence more energy required
Cant Conduct Electricity- All the electrons of C are shared and it has no free electrons
It is used for cutting and drilling tools
Graphite
Hexagonal ring
Every carbon is bonded to only three other carbons
Low MP and BP- They are weak forces of attraction between the layers hence less energy is required to break them
Soft- Weak forces of attraction between layers
Good conductor of electricity- Every carbon has a free electron
Used in lubricants and pencils
Silcon (IV) Oxide and Silicon Dioxide
Each Si is bonded to four O and each O is bonded to 2 Si
Hard and Strong- All bonds of Si and O are complete
High MP and BP- Strong covalent bonds betweeen Si and O and hence more energy is required
Poor conductor of electricity- Doesnt have free electrons