C2 | Flashcards

Question	Answer
Describe Ionic Bonding	Transferring electrons. Atoms lose or gain electrons to form charged particles called ions, which are strongly attracted to one another.
Explain the bonding between group 1 & 7 element	Elements from group 1, the alkali metals, react with elements from group 7, the halogens to form ionic bonds. The group 1 metals lose one electron from their outer shell to elements in group 7 that gain the electron.
Describe Covalent Bonding	Sharing electrons. For example, in chlorine, the atoms both share one electron each so that they both have full outer shells.
Explain Metallic Bonding	Metallic bonding occurs between the metal ions and the delocalised electrons. Each metal atom donates outer electrons from their outer shell. These become delocalised and are free to move and carry charge.
Do simple molecules have high or low melting and boiling points?	They have low melting and boiling points.
Explain the role of inter molecular forces when a substance melts/boils.	Simple molecules are gases or liquids as room temperature. Each atoms provides one shared electron as part of the covalent bond. They have low melting and boiling points because there are weak intermolecular forces between the molecules.
Explain why simple molecules do not conduct electricity.	Simple molecules such as hydrogen are gases at room temperature as they have low melting and boiling points. The simple covalent structures contain no overall charge and so do not conduct electricity.
Explain the structure and properties of ionic compounds (salt)	Salts form a giant ionic lattice. Each sodium ions bonds with a chlorine ion, forming strong ionic bonds. They have a high melting point as they need a lot of energy to break bonds, they conduct electricity when molten or dissolved and the ions are free to move and carry charge.
Why are simple molecules gases or liquids and room temperature?	Simple molecules such as water and carbon dioxide are liquids or gases at room temperature because they have weak intermolecular forces between the molecules.
The Bonding of Diamond	Each carbon atoms forms covalent bonds in a very rigid giant covalent structure. This makes diamond the hardest natural substance, so its used for drill tips.
Graphite - conductivity	Each carbon atom is connected to three other atoms with strong covalent bonds. One electron from each carbon is delocalised meaning it is free to move and carries charge.
Structure and use of fullerenes - graphene	Graphene has delocalised electrons that are free to move and carry charge. It is made up of strong covalent bonds which need a lot of energy to break (giant covalent lattice).
Structure and properties of Metals	Metals donate electrons from each metal atom's outer shell. These form a sea of delocalised electrons that form the bond with the metal ion. The opposite charges attract each other to form a giant lattice.
How metals conduct heat - copper in saucepans	Copper conducts heat. Each metal ion is very close to each other in the lattice. They can pass their vibration energy to their neighbours. It has a high melting point, bonds are strong and a lot of energy is needed to break them.
Shape memory alloys	Alloys that remember their original shape and can be bent. An example is nitinol which is used in braces.
Properties of Polymers	The properties of polymers depend on what they are made from ans the conditions under which they are made. For example, low density and high density poly(ethene) is produced using different catalysts and reaction conditions. Two types of polymers are thermosetting and softening.
Thermosetting vs Thermosoftening polymers	Both are made of monomers. Setting - strong covalent bonds, lots of energy needed to break, don't melt when heated. Softening - long polymer chains, allows them to melt when heated.
RAM	Relative atomic mass is a way of saying how heavy an element is compared to carbon 12. The AR of carbon is exactly 12. In reality the relative atomic mass for an element is their mass number.
Moles	One mole of a substance is equal to its MR in grams.
Paper chromatography	Artificial colours can be separated.
Gas chromatography	Identifies substances- separates out a mixture of compounds.
Percentage of an element	Ar/Mr = percentage.
Empirical Formula	Write percentages Write in grams Divide by the RAM Divide by the smallest if necessary
Calculate masses	Mass/RFM = Moles Ratio Moles * RFM = Answer
Percentage yield	Actual yield/theoretical yield * 100
Reversible reactions	Products of the reaction can themselves react to produce the original reactants.

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	Created by Abbie Goffin over 7 years ago