What can an electron be thought of as ?
A negatively charged cloud with the shape of an orbital, called an electron cloud
Shells are regarded as what ?
Energy levels
What happens to energy as the shell number increases ?
Energy increases
What is the shell number referred to as ?
Principal quantum number (n)
What are shells made up of ?
Atomic orbitals
What is an orbital ?
- An orbital is an area around the nucleus where electrons with opposite spin are likely to be found
What are the different orbitals ?
- S orbitals
- P orbitals
- D orbitals
- F orbitals
How many electrons can be held in an orbital ?
One or two, no more
How many orbitals does each type contain ?
- S - one
- P - three
- D - five
- F - seven
How many electrons can be held in each type of orbital ?
- S - two
- P - six
- D - ten
- F - fourteen
What is the shape of an s orbital ?
Spherical
What is the shape of a p orbital ?
- Dumbbell
- Theres three types, one in each plane (x,y and z)
What are the rules of orbital fillings ?
- Orbitals fill in order of increasing energy
- Electrons pair with opposite spins
- Orbitals with the same energy are occupied singly first
Explain the rule of orbitals filling in order of increasing energy
- 1s is filled first
- Then 2s and 2p
- Then 3s, 3p, 4s and then 3d
Where does this rule cause confusion ?
- The 3d sub-shell has higher energy than the 4s.
- So the 4s fills before the 3d
State the orbital filling until the 4th shell
- 1s
- 2s, 2p
- 3s, 3p, 4s, 3d
- 4p, 4d, 4f
Explain the rule of electrons pair with opposite spins
- Electrons are negatively charged and repel one another
- Electrons can have spin up or spin down
- If electrons have opposite spin, the charge repulsion is counteracted enough for both to be in the orbital, they cancel out
Explain the rule of orbital filling when the same energy subshells are occupied singly first
- Within a sub shell, the orbitals have the same energy
- One electron occupies each orbital before pairing begins.
- This prevents repulsion until no unoccupied orbitals remain
How can electron configuration be shortened ?
- 1s2 can be expressed as [He]
- 1s2 2s2 2p6 can be expressed as [Ne]
- 1s2 2s2 2p6 3s2 3p6 can be expressed as [Ar]
What is this format called ?
Shorthand notation
What happens in terms of energy sub-shells when forming ions ?
The highest energy sub shells lose or gain electrons
What is ionic bonding ?
The electrostatic attraction between oppositely charged ions
In what directions are ions attracted to other ions ?
In all directions
What is the result of ions attracting oppositely charged ions in all directions ?
Giant ionic lattice
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Chapter 2 - Atomic structure and isotopes18
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Chapter 3 - Amount of substance44
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Chapter 4 - Acids and Redox36
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Chapter 5 - Structure and Bonding43
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Chapter 6 - Bonding and structure39
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Chapter 7 - Periodicity35
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Chapter 8 - Reactivity trends43
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Chapter 9 - Enthalpy28
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Chapter 10 - Reaction rates and equilibrium35
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Chapter 11 - Basic concepts of organic chemistry43
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Chapter 12 - Alkanes24
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Chapter 13 - Alkenes63
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Chapter 14 - Alcohols32
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Chapter 15 - Haloalkanes27
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Chapter 16 - Practical techniques12
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Organic synthesis reactions10
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Chapter 17 - Spectroscopy19
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Chapter 18 - Rate of reactions82
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Chapter 19 - Equilibrium35
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Chapter 20 - Acids, Bases and pH35
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Chapter 21 - Buffers and Neutralisation35
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Chapter 22 - Lattice enthalpy54
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Chapter 23 - Redox and electrode potentials54
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Chapter 24 - Transition metals105
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Chapter 25 - Aromatic compounds69
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Chapter 26 - Carbonyls92
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Chapter 27- Amines, Amino Acids and Polymers44
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Chapter 28 - Organic synthesis15
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Chapter 29 - Chromatography and Spectroscopy88
