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Chem 1 - Atomic Stru
Chem 1 - Atomic Structure
Question | Answer |
---|---|
Proton | A nucleon of an Atom. Relative Mass of 1, Relative Charge of +1. Defines the ATOMIC NUMBER of an Element. |
Neutron | A nucleon of an Atom. Relative mass of 1, relative charge of 0. Together with Protons defines MASS NUMBER. |
Electron | An atomic Particle that surrounds the Nucleus of an atom. Relative mass of 1/2000, Relative charge of -1. The major component of bonding. |
Atomic Number | The number of Protons in an Atom of an Element. |
Mass Number | The number of Protons and Neutrons in an atom of an element. |
Nucleons | Protons and Neutrons of an Atom. |
Formulae for MAX number of electrons in a shell: | 2n(squared), where n is the shell number. |
energy level 1 sub shells: | 1s / |
energy level 2 sub shells: | 1s / 2s, 2p / |
energy level 3 sub shells: | 1s / 2s, 2p / 3s, 3p, 3d / |
Energy Level 4 Sub Shells: | 1s / 2s, 2p / 3s, 3p, 3d / 4s, 4p, 4d, 4f / |
Write out, in order, the subshells that are filled first up to 4f. | 1s - 2s - 2p - 3s - 3p - 4s - 3d - 4p - 4d - 4f. (remember the special diagonal diagram!) |
Isotopes | Isotopes are atoms of an element that have the same number of protons but different number of Neutrons. |
Ions | Ions are atoms that have a different amount of electrons to the amount of protons. |
Mass Spectrometry | Is an analytical technique used to determine the mass of particles. |
Name the four stages in Mass spectrometry: | Ionisation, Acceleration, Deflection, Detection. |
Mass Spec: Ionisation: | |
Mass Spec: Acceleration: | |
Mass Spec: Deflection: | |
Mass Spec: Detection: | |
First Ionisation Energy | The amount of energy required to remove one mole of electrons from one mole of atoms in a gaseous state to give a charge of +1. Measured in kJ mol-1. |
Why is the second Ionisation Energy always higher than the first? | Because removing an electron from an ion that is already positively charged requires a much greater amount of energy. |
What is the trend in first Ionisation Energies going along a period? | They generally increase because of increasing nuclear attraction, until you change sub-shell or the spin of electrons changes direction. |
What is the trend in Ionisation Energies going down a Group? | They decrease because of a large increase of Nuclear Radius and increasing electron shielding. |
Atomic Radius | The distance from the Nucleus to the outer electron shell. |
Electron Shielding. |