11970365
Description
Mind Map by Dominic Weston, updated more than 1 year ago
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Created by Dominic Weston
about 6 years ago
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Atomic Stucture
- Ions
- Ions have different numbers of protons and electrons
- Ions formed by gaining or losing electrons from the atom
- Positive ions have lost electrons
- Negative ions have gained electrons
- Negative Ions repel
- Negative Ions repel
- Negative ions have gained electrons
- Positive ions have lost electrons
- Ions formed by gaining or losing electrons from the atom
- Ions have different numbers of protons and electrons
- Isotopes
- Same element with different numbers of neutrons
- Number and arrangement of electorns decide the chemical properties of an element
- Isotopes have the same electrons / config so same chemical porperties
- Slightly different physical properties due to different mass of atom
- Slightly different physical properties due to different mass of atom
- Isotopes have the same electrons / config so same chemical porperties
- Same element with different numbers of neutrons
- ToF Mass Spectrometer
- Ionisation
- Electron Impact
- Sample is vaporised
- High energy electrons fired at sample from an electron gun
- Forms +1 ions that are attracted to -ve plate
- Forms +1 ions that are attracted to -ve plate
- High energy electrons fired at sample from an electron gun
- Sample is vaporised
- Electrospray
- Sample dissolved in volatile solvent
- Injected through fine needle
- Tip of needle attached to +ve end of high-voltage supply
- Forms +1 ions by gaining a proton from solvent
- Forms +1 ions by gaining a proton from solvent
- Tip of needle attached to +ve end of high-voltage supply
- Injected through fine needle
- Sample dissolved in volatile solvent
- Electron Impact
- Detection
- Positive ions discharged
- By gaining electrons when hit detector
- Generates a current from the movement of electrons
- Size of current indicates number of ions hitting plate
- Mass spectrum
- Data used to produce graph
- mass to charge ratio (m/z) against abundance
- used to work out relative atomic mass of element
- = mass of isotopes / abundance
- = mass of isotopes / abundance
- used to work out relative atomic mass of element
- mass to charge ratio (m/z) against abundance
- Greatest m/z value
- Tells us the relative mass of sample
- small signal may be above it
- this is due to ions having higher mass on a single atom
- Signals below are due to fragmentation of molecular ions
- this is due to ions having higher mass on a single atom
- small signal may be above it
- Tells us the relative mass of sample
- Data used to produce graph
- Size of current indicates number of ions hitting plate
- Generates a current from the movement of electrons
- By gaining electrons when hit detector
- Positive ions discharged
- Flight Tube
- Low mass, faster
- Fastest meets detector first
- Fastest meets detector first
- Low mass, faster
- Acceleration
- +1 ions accelerated using electric field
- So that they all have the same kinetic energy
- Velocity depends on mass
- low mass, faster
- low mass, faster
- Velocity depends on mass
- So that they all have the same kinetic energy
- +1 ions accelerated using electric field
- Instrumental method of analysis
- Used to find abundance and mass of each isotope of an element
- This allows us to find its relative atomic mass
- Used to find relative molecular mass of substances of molecules
- This allows us to find its relative atomic mass
- Used to find abundance and mass of each isotope of an element
- Ionisation
- Electronic Structure
- Electron shells made up of sub-shells and orbitals
- Electrons move around nucleus in regions of an atom - shells or energy levels
- Shells are divided into sub-shells which have slightly different energies
- Sub-shells have different numbers of orbitals which can each hold 2 electrons
- Two electrons in each orbital spin in opposite directions due to repulsion
- 1s^2 - 1 orbital, 2e-
- 2p^6 - 3 orbitals, 6e-
- 3d^10 - 5 orbitals, 10e-
- 4f^14 - 7 orbitals, 14e-
- Two electrons in each orbital spin in opposite directions due to repulsion
- Sub-shells have different numbers of orbitals which can each hold 2 electrons
- Shells are divided into sub-shells which have slightly different energies
- Electrons move around nucleus in regions of an atom - shells or energy levels
- Further the shell is from the nucleus, the higher its energy
- Number of outer shell electrons decide chemical properties
- Group 1 and 2 easily lose electrons from outershell to from positive ion
- Group 5, 6 ,7 can gain 1, 2, 3 electrons form negative ions
- Group 4, 7 share electrons to form covalent bonds
- Group 0 have filled sub-shells, dont react making them inert
- Transition metals lose s, d electrons forming positive ions
- Transition metals are unusual
- Copper and Chromium fill their 4s sub shell singly
- Energetically more favourable to fill 3d sub shell first
- They also lose the 4s electron before 3d when becoming ions
- They also lose the 4s electron before 3d when becoming ions
- Energetically more favourable to fill 3d sub shell first
- Copper and Chromium fill their 4s sub shell singly
- Transition metals are unusual
- Transition metals lose s, d electrons forming positive ions
- Group 0 have filled sub-shells, dont react making them inert
- Group 4, 7 share electrons to form covalent bonds
- Form inert gas configuration
- Group 5, 6 ,7 can gain 1, 2, 3 electrons form negative ions
- Group 1 and 2 easily lose electrons from outershell to from positive ion
- Electron shells made up of sub-shells and orbitals
- Ionisation Energy
- Ionisation - removal of electrons from atoms or molecule
- Factors
- Nuclear Charge
- more protons in nucleus, stronger the attaction to electrons
- more protons in nucleus, stronger the attaction to electrons
- Shielding
- More electrons between nucleus and outer electron, less attaction between the two
- More electrons between nucleus and outer electron, less attaction between the two
- Nucleus Radii
- Attraction falls off rapidly with distance, larger the radii, less attaction
- Attraction falls off rapidly with distance, larger the radii, less attaction
- Nuclear Charge
- Trends
- Across any period
- Increase harder to remove outer electron
- Across period increasing nuclear charge, more protons
- Shielding the same across
- More attaction between the electrons and protons
- More attaction between the electrons and protons
- Shielding the same across
- Across period increasing nuclear charge, more protons
- Increase harder to remove outer electron
- Down a group
- Extra electron shells
- Less attraction between positive nucleus and outer electron
- Furthest electron far away
- Furthest electron far away
- Less attraction between positive nucleus and outer electron
- Extra electron shells
- ALM
- Despite increase in nuclear charge,
- Outer Al electron in a higher energy sub-shell
- increase shielding
- Less energy needed to remove the electron
- Less energy needed to remove the electron
- increase shielding
- Same shielding, same orbital
- Phosphorus has 1 fully occupied orbital
- Repulsion in the electron orbital
- Repulsion in the electron orbital
- Phosphorus has 1 fully occupied orbital
- Outer Al electron in a higher energy sub-shell
- Despite increase in nuclear charge,
- SLP
- Across any period
- Ionisation - removal of electrons from atoms or molecule
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