Difference between revisions of "Relative Atomic Mass"
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| style="height:20px; width:200px; text-align:center;" |[[Boron]] has eleven [[nucleon]]s so it has an '''atomic mass''' of 11 and [[Avagadro Constant|6.02x10<sup>23</sup>]] (or 1 [[mole]] of) [[atom]]s of [[Boron]] have a [[mass]] of 11g. | | style="height:20px; width:200px; text-align:center;" |[[Boron]] has eleven [[nucleon]]s so it has an '''atomic mass''' of 11 and [[Avagadro Constant|6.02x10<sup>23</sup>]] (or 1 [[mole]] of) [[atom]]s of [[Boron]] have a [[mass]] of 11g. | ||
|} | |} | ||
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| + | ===References=== | ||
| + | ====Edexcel==== | ||
| + | :[https://www.amazon.co.uk/gp/product/1292120193/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=1292120193&linkCode=as2&tag=nrjc-21&linkId=572df39392fb4200db8391d98ae6314e ''Ar (relative atomic mass), page 167, GCSE Combined Science, Pearson Edexcel ''] | ||
| + | :[https://www.amazon.co.uk/gp/product/1292120215/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=1292120215&linkCode=as2&tag=nrjc-21&linkId=8f96ddb76196848bafdb124354e4cf77 ''Ar (relative atomic mass), page 23, GCSE Chemistry, Pearson, Edexcel ''] | ||
Revision as of 11:29, 29 October 2019
Contents
Key Stage 3
Meaning
An element tile showing the mass number.
The Atomic Mass or mass number is the number of nucleons (protons + neutrons) in an atom.
About The Atomic Mass
- Two atoms of the same element may have the same Atomic Number but a different Atomic Mass depending on the number of neutrons in the nucleus. Elements with different mass numbers are called isotopes.
- The atomic mass is not affected by the number of electrons.
- Only the particles in the nucleus affect the atomic mass.
Examples
| Hydrogen | Helium | Lithium | Beryllium |
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| Hydrogen has one nucleon so it has an atomic mass of 1. | Helium has four nucleons so it has an atomic mass of 4. | Lithium has seven nucleons so it has an atomic mass of 7. | Beryllium has nine nucleons so it has an atomic mass of 9. |
Key Stage 4
Meaning
An element tile showing the mass number.
The relative atomic mass or mass number of an element is the number of nucleons (protons + neutrons) in an atom.
The relative atomic mass in grams is also the mass of one mole or 6.02x1023 atoms of the element.
About Relative Atomic Mass
- The relative atomic mass in grams on the Periodic Table tells the mass of a mole of the element. A mole of the element is 6.02x1023 atoms of that element.
- Two atoms of the same element may have the same Atomic Number but a different Relative Atomic Mass depending on the number of neutrons in the nucleus. Elements with different mass numbers are called isotopes.
- The relative atomic mass is not affected by the number of electrons.
- Only the particles in the nucleus affect the relative atomic mass.
Examples
| Hydrogen | Deuterium | Tritium | Boron |
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| Hydrogen has one nucleon so it has an atomic mass of 1 and 6.02x1023 (or 1 mole of) atoms of Hydrogen have a mass of 1g. | Deuterium has two nucleons so it has an atomic mass of 2 and 6.02x1023 (or 1 mole of) atoms of Deuterium have a mass of 2g. | Tritium has three nucleons so it has an atomic mass of 3 and 6.02x1023 (or 1 mole of) atoms of Tritium have a mass of 3g. | Boron has eleven nucleons so it has an atomic mass of 11 and 6.02x1023 (or 1 mole of) atoms of Boron have a mass of 11g. |