Lecture 2: Orbital theory, electron configurations and hybridisation

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14 Terms

1
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what was john daltons assumption that was proved incorrect?

particle of an atom was indivisible

2
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what are the main types of atomic orbitals?

s, p, d, and f orbitals

  • lowest energy shells first

  • the more full the shell the less reactive

3
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how many electrons can be found in each orbital?

s=2 p=6 d=10

4
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what are S orbitals?

  • sphere of electron denisty centered on the nucleus

  • electron can be found anywhere in orbital

<ul><li><p>sphere of electron denisty centered on the nucleus</p></li><li><p>electron can be found anywhere in orbital</p></li></ul><p></p>
5
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what are P orbitals

  • dumbell looking

  • have a node at the centre so no chance of finding e there

<ul><li><p>dumbell looking</p></li><li><p>have a node at the centre so no chance of finding e there</p></li></ul><p></p>
6
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what is valency?

the number of bonds needed to complete the outer shell

7
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what is Sp3 hybridisation?

1s orbital + 3 p orbitals

  • tetrahedral

  • 109.5

  • all sigma bonds(single)

<p>1s orbital + 3 p orbitals </p><ul><li><p>tetrahedral </p></li><li><p>109.5 </p></li><li><p>all sigma bonds(single)</p></li></ul><p></p>
8
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what is Sp2 hybridisation?

1s orbital and 2 p orbitals

  • trigonal planar

  • 120

  • sigma and pi bonds

<p>1s orbital and 2 p orbitals </p><ul><li><p>trigonal planar</p></li><li><p>120 </p></li><li><p>sigma and pi bonds </p></li></ul><p></p>
9
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what is Sp hybridisation?

1 s orbital and 1 p orbital

  • linear

  • 180

<p>1 s orbital and 1 p orbital </p><ul><li><p>linear </p></li><li><p>180</p></li><li><p></p></li></ul><p></p>
10
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what are sigma bonds?

strongest type of covalent bond(single bond)

  • formed when atomic orbitals overlap head on

  • release energy

  • free rotation

<p>strongest type of covalent bond(single bond)</p><ul><li><p>formed when atomic orbitals overlap head on</p></li><li><p>release energy</p></li><li><p>free rotation</p></li></ul><p></p>
11
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sigma bond with 1s and 1p orbital

  • lobe opposite new orbital, involved in substitution reactions

<ul><li><p>lobe opposite new orbital, involved in substitution reactions</p></li></ul><p></p>
12
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sigma bond with 1s and sp orbital

  • lobe opposite new orbital, involved in substitution reactions

<ul><li><p>lobe opposite new orbital, involved in substitution reactions</p></li></ul><p></p>
13
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what are pi bonds?

covalent bonds formed from overlap of 2 orbital lobes laterally

  • the node has no electron density

  • there is a plane w no electron density

  • fixed( no free rotation)(leads to isomers)

<p>covalent bonds formed from overlap of 2 orbital lobes laterally</p><ul><li><p>the node has no electron density</p></li><li><p>there is a plane w no electron density</p></li><li><p>fixed( no free rotation)(leads to isomers)</p></li></ul><p></p>
14
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what is the influence of lone pairs?

  • lone pairs are held closer to the atom than bonding e- so exert repulsion on other e-

  • this compreses bond angles, -2.5 for every lp

<ul><li><p>lone pairs are held closer to the atom than bonding e- so exert repulsion on other e-</p></li><li><p>this compreses bond angles, -2.5 for every lp</p></li></ul><p></p>