Karteikarten
Atomic Structure
Karten in diesem Stapel (18)
- 1What are Isotopes?Isotopes are atoms of the same element but they have a different number of neutrons e.g. B can have a mass number of 10 or 11
- 2Isotopes (2)On the periodic table the number usually quoted is not the mass number as they are different but instead the Relative atomic mass
- 3How do you work out R.A.M? (Relative Atomic Mass)the sum of each elements
(Mass No. x Abundance /(divide by) 100)
e.g. Boron
(10 x 20/100) + (11x 80/100)
=2.0+8.8
= 10.8 - 4History of the Atom Start of the 19th Century John Dalton 1stAtoms are solid Spheres and said that different spheres made up the different elements.
- 5History of the Atom 1897 J J Thompson (Plum Pudding Model)A positive Atom surrounded by negative charged Particles
- 6History of the Atom 1909 Ernest Rutherford (Rutherford's Model)A tiny positively charged nucleus at the centre however there is a cloud of negative electrons surrounding the nucleus
- 7History of the Atom Bohr ModelBohr suggested that the electrons were contained in shells and that electrons were in a fixed orbit around the nucleus in fixed shells and each shell is a fixed distance from the nucleus
- 8Formation of the shells and how many electrons can fit in them!
- 9Shells and Electron Configuration1st = 2 electrons = 2e- Max
2nd = 8 electrons = 8e- Max
3rd = 8 electrons (but can expand) = 8e- Max
They fill up from Inner Shell
Electrons can pair up when forced to! - 10More about ShellsThere is a Maximum number of electrons that can fit in each shell as was shown in the last Card
The number of Electrons in an Atom = Number of Protons (which = the Atomic Number) - 11More Shells!!!!!!An electron will occupy the lowest energy shell available!
That's enough about shells - 12Types of Atom and Formation of Ions A typical Metal Atom:Has a large radius
Has one or two or three outer electrons
These electrons are a long way from the nucleus so are weakly held
This means that the outer electron can easily be lost....... - 13Types of Atom and Formation of Ions A typical Metal Atom (2):This means that when a metal reacts it always does so by losing electrons, thus forming a positive ion* (a cation)
*an atom or molecule with a net electric charge due to the loss or gain of one or more electrons. - 14Types of Atom and Formation of Ions A typical Non-Metal Atom:Has a small radius
With a nearly full outer shell of electrons (a full outer shell in the case of noble gases [Group 8])
These electrons are relatively close to the nucleus so they are strongly held.
These electrons are not easily lost....... - 15Types of Atom and Formation of Ions A typical Non-Metal Atom (2):However the gaps in the outer shell allow electrons from elsewhere to be gained
So when a non-metal atom reacts with a metal atom, the non-metal atom will gain electrons, thus forming a negative ion (an Anion) e.g. O + 2e- = O2-
The ion becomes 'stable' when it has a full outer shell of electrons - 16The Fundamental ParticlesParticle-where found?-Relative mass- Relative charge
Proton-Nucleus-1-+
Neutron-Nucleus-1-none
Electron-In orbit around the nucleus-1/2,000- negative charge - 17Modern Model of the Atom
- 18Things about The Atom:An Atom is the smallest part of an element that still has the properties of the element itself
The Idea of the "Atom" originated in Ancient Greece
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- CE Science (Chemistry) Karteikarten am Atomic Structure, erstellt von Dan Carpenter am 16/02/2017.
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- Dan Carpenter
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