C4 Summary
- Created by: Arron murray
- Created on: 02-04-13 17:35
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- C4 Summary
- Atomic structure and atomic bonding
- Isotopes are elements that have atoms of the same atomic number but different mass numbers
- Dot and cross models can be used to represent the ionic bonding in compounds
- Sodium chloride and magnesium oxide form giant ionic lattices as their ions attract
- The electron is made up of protons and neutrons
- Metals form positive ions as they lose electrons
- The periodic table and convalent bonding
- Non-metals combine by sharing electrons
- Carbon dioxide and water have low melting points as the inter-molecular forces are weak
- The period to which an element belongs is the same as the number of occupied electron shells
- Groups
- The group number is the same as the number of electrons in the outer shell
- Rubidium and caesium are group 1 metals which react violently with water to give of hydrogen and make an alkaline solution
- Group 1 metals have similar properties as they all need to lose one electron from their outershell
- Flame tests can be used to identify the presence of lithium,sodium and potassium
- if a group 1 metal reacts with a group 7 non-metal the word equation for the formation of a metal halide can be constructed
- Metals and water
- Copper compounds are often blue,iron (II) compounds are often green and iron (III) compounds are often orange/brown
- The thermal decomposition of transition metal carbonates results in the metal oxide and carbon dioxide being made
- Cu^2+ ions react with sodium hydroxide to make a blue solid in a precipitation reaction
- Metals have high melting points due to their strong metallic bonding
- Super conductors conduct electricity with little or no resistance
- Drinking water is purified by filitration,sedimentation and chlorination
- Sulfates in water can be tested using barium chloride, Halides, can be tested using silver nitrate
- Atomic structure and atomic bonding
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