Flashcards
CHEM1100 mid sem
Cards in this deck (25)
- 1The two natures of lightLight has a dual wave and particle nature
- 2Heisenberg theory and equationWe can never know momentum and position of an e-, we can find the probability of those positions.
delta(x).delta(p) = h/4(pi)
delta(x) is the uncertainty of position
delta(p) is the uncertainty of momentum - 3Wave functions; quantum numbers,values and meaningn-> energy level, distance from the nucleus
l-> angular momentum, speed of e- related to shape. 0<= n-1
m(l) -> magnetic, its orientation in space = +l to -l - 4The corresponding l values to letters0 = s
1 = p
2 = d
3 = f - 5Penetration and sheilding theoryIn non hydrogen orbitals e- of a lower orbit repel the outer e- due to opposing charges. Therefore atoms with more than 1e- have shielding and penetration acting upon them. Penetration is how some l shapes get closer to the nucleus.
- 6Ionisation Energy (IE)Energy required to completely remove e- from species. Energy of orbital measured through this.
- 7Hybridisation theoryThe fusion of atomic orbitals that influences the molecular geometry and bonding properties.
- 8What are the two hybrid bonds (that we've learned)Sigma and Pi bonds
- 9What are the exceptions to the Afbau principleCr: 3d(5)4s(1)
Cu: 3d(10)4s(1)
Half full/full - 10What is an ionic bondBonding when atoms that lose electrons relatively easily bond with atoms that have high electron affinity. Ionic bonds are formed when the electronegativity difference (Dc) between the atoms is > 1.7.
- 11Covalent bondThe sharing of valence electrons by nuclei with an overlap of orbitals. Covalent bonds are formed when the electronegativity difference (Dc) between the atoms is < 1.7.
- 12Formal charge: definition and ruleThe charge on an atom in a bond (typically lewis structure).
= valence electrons - lone pair electrons - 1/2 bonded electrons - 13When are resonant structure present, and what is it about themOccur there are multiple bonds present. When combined are a representation of the forms that the molecule 'flips' between, as the bond is always changing positions or whatnot.
- 14What would tell you to find resonant structures in a questionOther than when there is a multiple bond, it may say that all bonds are of equal length, when it is known that double bonds are shorter than single bonds.
- 15Sigma bonds shape/formationFrom the side on bonding of two orbitals (either p or s)
- 16Pi bond forms froms
- 17What are the bonds for single, double and triple bondsc-c = 1 sigma
c=c 1 sigma 1 pi
c(triple bond)c = 1 sigma 2 pi - 18Number of atoms and angles: Linear bond Trigonal planar Tetrahedral Trigonal Bipyrimidal OctahedralLinear: 3 atoms, 180 degrees
Trigonal planar: 4 atoms, 120 degrees
Tetrahedral: 5 atoms, 109.5 degrees
Trigonal bipyrimidal: 6 atoms, 90 degrees and 120 degrees
Octahedral: 7 atoms, 90 degrees - 19What is molecular orbital theorysigma and pi bonds forming without hybridisation taking place. DO NOT MIX WITH VSEPR.
- 20What are bonding molecule orbitalsbonding molecular orbitals are constructive, or in phase, and end up having a consistent oval of electron density.
- 21What are anti bonding molecular orbitalsAnti bonding molecular orbitals have destructive interference, hence they have two small electron densities with a node in the middle of them.
- 22Bond order; what it means and equation
- 23Tetrahedral hybridisationsp3
4 sigma bonds - 24Trigonal planar hybridisationsp2
3 sigma 1 pi bond - 25Linear hybridisationsp
2 sigma 2 pi bonds
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- Flashcards on CHEM1100 mid sem, created by courtney_houston on 03/04/2016.
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