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| Equation for working out maximum amount of electrons in a shell. |
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Definition
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| How many maximum electrons could there be in the first four shells. |
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| Why do electrons spin around the nucleus? |
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Definition
| Electrons are always trying to get away from the nucleus but they are attracted to the proton so it goes around (orbits) the nucleus. |
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Term
| When you head to the right of the periodic table, what happens to the size of the atoms. |
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Definition
| The atom becomes smaller because there are more protons and electrons which means there is a bigger attraction and therefore the atom in more closely bunched together and it makes a smaller atom. |
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| Known as 'A'. Total number of Protons and Neutrons in the element's atom. |
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| Known as 'Z'. The periodic table number as well as the number of protons in the nucleus. |
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| Means the amount of protons and electrons are the same |
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| Consist of only one type of atom |
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| Consists of different types of elements chemically bonded together. |
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Term
| Who discovered the periodic table and when? |
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Definition
| Mendeleev created the first periodic table in 1869. He has the element Mendeleev named after him. |
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Term
| What are the natural elements? |
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Definition
| The first 92 elements are natural. The ones after 92 man made often named after famous scientists or planets. |
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Definition
Known as groups and each group 1-8 has different numbers of valence electrons.
1 - Alkali
2 - Earth Alkali
3 - Halogens
4 - Noble Gases |
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Definition
| Known as periods, when periods go down in the table the elements increases in orbitals. |
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| Names of the electron shells |
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Definition
1st shell - K
2nd shell - L
3rd Shell - M
4th Shell - N |
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Definition
Within each shell there are sub shells with different energy levels and these fill according to these energy levels.
1st Shell - 1 shell
2nd Shell - 2 sub shells
3rd Shell - 3 sub shells
4th Shell - 4 sub shells |
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Term
| What are the names of the blocks on the periodic table |
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Definition
S block (Alkali and Earth Alkali)
D block (Transition Metals)
P block (Far right)
F block (Man-made bottom block) |
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Term
| How many maximum valence electrons can each block carry? |
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| Variation of an element with different amount of electrons. |
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| The average mass of a certain element's atom as it varies due to different isotopes with different masses. |
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Definition
| The total mass of a compound. Find the atomic mass of the elements in that compound (multiply the atomic mass of an element if there is more than one atom of that element in the compound). Then add the total mass of each elements together to get the relative formula mass. RFM. |
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Definition
| Calculating the percentage of mass for a certain element within a compound. |
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Definition
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| Get the total mass of an element within in a compound and divide it by the total mass of the compound (relative formula mass). |
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| Calculating Relative Abundance |
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Definition
| X/100 (x Atomic Mass) + 100-x/100 (x Atomic Mass) = RAM |
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Definition
| The amount of an element or isotope within a compound or element. |
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Definition
The approximate amount of each element within a compound where the quantity of an atom is written on the bottom right of the atom's symbol.
Eg. H20, C6S12P4 |
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Term
| How do you work out the empirical formula for a compound? |
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Definition
| First you must have either the percentage of each of the elements to the compound or the masses (weight) of the elements. Then divide them each by their atomic masses and have them as a ratio. Then divide each number by the lowest number in the ratio. After that round the ratios to whole numbers. Then right the element's symbols and quantities together to form the compound's symbolic name. |
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Term
| What is the order of the electron sub-shell structure across the first four rows of the periodic table? |
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Definition
| 1s2 , 2s2, 2p6 , 3s2, 3p6 , 4s2 , 3d10 , 4p6. |
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Term
| What is the bohr configuration? |
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Definition
The basic form of writing electron structure.
E.g.
2,8,1
2,8,6
2,6 etc. |
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Term
| When does the elements stop filling according and start filling out over different shells even though a previous shell isn't yet full? |
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Definition
| After element 18 (Argon). After argon it then goes 2,8,8,1 instead of 2,8,9. This is because of an overlap in electron orbits causing electrons to fill out different and not in order. |
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Term
| Who developed the idea of the atom and when |
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Definition
| Democritus in 360 BC. He called it ATOMA. |
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| In 1808 he suggested that all matter was made up of tiny spheres that could bounce around with perfect elasticity and called them atoms. |
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| In 1898 he Found that atoms could sometimes eject a far smaller negative particle which he called an electron. He developed the plum pudding model in 1904 where electrons were scattered unevenly with an elastic sphere surrounded by a soup of positive charge to balance the electrons. |
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Oversaw Geiger and Marsden carrying out his famous experiment.
they fired Helium nuclei at a piece of gold foil which was only a few atoms thick.
they found that although most of them passed through. About 1 in 10,000 hit
They found that while most of the helium nuclei passed through the foil, a small number were deflected and, to their surprise, some helium nuclei bounced straight back. |
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Term
| Rutherford's new evidence: |
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Definition
Rutherford’s new evidence allowed him to propose a more detailed model with a central nucleus.
He suggested that the positive charge was all in a central nucleus. With this holding the electrons in place by electrical attraction
However, this was not the end of the story. |
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| studied under Rutherford at the Victoria University in Manchester. Bohr refined Rutherford's idea by adding that the electrons were in orbits. Rather like planets orbiting the sun. With each orbit only able to contain a set number of electrons. |
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Term
| Why does an element have +2 etc. |
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Definition
| Because it had lose two electrons to get a full shelled and gains a charge of +2. All periodic table elements are uncharged forms so the protons and electron amounts are the same. |
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| In 1932: studied under Rutherford and Geiger in 1913 at the Technical University of Berlin In 1932, while working at Cambridge University, discovered the neutron by bombarded beryllium with alpha particles and noticed that a non-ionising radiation was emitted |
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| Made by Glenn Seaborg and his research team at Berkley Univeristy in California |
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