| What happens when Non-Metals Combine with each other? | They make Covalent Bonds, this is Sharing a Pair of Electrons |
| Why do Atoms use Covalent Bonding? | Both of the Atoms can have a Full Outer Shell, Its Stable |
| Are the Covalent Bonding Strong? Why? | This is Strong, because of the Electrostatic Attraction between the Positive Nucleus and the Negative Electron in the Shared Pair. |
| Explain why H20, Hydrogen Gas and Carbon Dioxide use Covalent Bonding | -Water [H2O] has the Oxygen Atom wanting 2 More electrons [Its Group 6] and what happens is the Hydrogen shares its Only Electron with it, and in return Oxygen allows to share one of its Own.
Both have a Full Outer Shell [Oxygen and Hydrogen] 2 Covalent Bonds is used [Because 2 Electrons is used]
-Hydrogen Gas [H2] has the Hydrogen Atoms wanting a Single Electron, and since there is 2 of them, they Share their Only Electron, Which creates 2 Electrons being Shared for both of them [1 Covalent Bond is used because 1 Electron is Shared]
-CO2 has the Carbon wanting 4 Electrons to Fill the Outer Shell, and Oxygen wanting 2 to Have. Simple maths can say that having 2 Oxygen would provide 4 Electrons needed, which Carbon can give. So 2 Double Covalent bonds are created [4 Covalent Bonds] |
| What is a Simple Molecule | This is simply a Substance created via Covalent Bonds [Water, Carbon Dioxide] |
| Are they Hard to Pull the Atoms in the Molecule Apart? Is it hard to Separate the Molecules? | -It is very hard to Split up the Molecule it self, because of the Strong Attraction of Forces for that Electron
-But the Molecules Forces with Other Molecules in the Simple Molecule have a Weak Force of Attraction [Known as Intermolecular Forces] and these forces determine how Easy it is to Change the State
-So the Melting and Boiling Point is very low, compared to Ionic Bonding. That's why most of the Simple Molecules are Gases or Liquids. |
| Can Simple Molecules Conduct Electricity? | No, there is no Free Electrons or Ions to move Around. No movement of Charge means no Electricity can Flow |
| Are Ball and Stick Models Good? | Mix of Both.
-It can really show the Structure of the Molecule as it shows in 3D
-It makes it look like there is Massive Gaps between the Atoms. Reality says that's where the Electrons Clouds come to play |
| Can the Giant Covalent Structures be acute to Giant Ionic Lattices? | Almost, they just have no Charged Ions |
| Explain the Giant Covalent Structure | -So, the Atoms involved makes Strong Covalent Bonds with each other, creating a need for more energy to Break them apart [High Melting/Boiling Points.]
-These Structures Don't conduct Electricity, at all [Exceptions]
-Carbon is an Excellent Example, as the Atom can make 4 Covalent Bonds, and can also go with other Carbon Atoms with ease. This can make Chains and Rings. |
| Explain the Diamond in terms of Covalent Structure | -Sparky and Colourless
-The Carbon atoms here make the 4 Covalent Structures, in a Rigid Format. This Formation makes the Material Tough.
-A lot of Energy is needed to break these bonds, and makes it have a High Melting Point.
-No Electricity is Conducted, because there is no Free Electrons or Ions |
| Explain Graphite and Graphene in terms of Covalent Structure | -Graphite is black, and opaque.
-The Carbon atoms hear only create 3 Covalent Bonds, which means the 4th Electron that isn't used can be Delocalised [Free] and with it creating an Electric Charge
-Sheet Formation happens also, that can Slide on each other
-Those layers are held Weakly, so that they can be broken off and leave a Black Mark. That is how you can write with a pencil.
-Like with the Diamond, it has a High Melting/Boiling Point because of the Covalent Bonding
-Graphene is the Single Sheet, and its Very Strong, Thin, Transparent and Light. The Delocalised Electrons here are even more 'Freeer' than the Graphite's ones, so it can conduct better |
| Explain Fullerenes | -Also made from Carbon, but not using Covalent Bonding.
-They are formed as a Hollow Ball, or a Tube. The amount of Carbon atoms are from the Fullerenes
-They too have Delocalised Electrons [Electricity] and have High Melting/Boiling Points, but its too notice they Don't compare with the Diamond or Graphite.
This Melting Point comes from the fact they have Big Molecules, which in turn boost the Intermolecular Force |
