72009
Description
Flashcards by snowred-orange, updated more than 1 year ago
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Created by snowred-orange
over 11 years ago
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| Question | Answer |
| Amphoteric oxides | exhibit both acidic and basic properties e.g. aluminium oxide (Al2O3) + H2O and BeO |
| Covalent Chlorides which form white fumes of HCl when in water? | AlCl3 (aluminium chloride), SiCl4 (silicon chloride), PCl3 (phosphorus chloride), SCl2 (sulphur chloride) |
| Hydrides | NaH - strong alkaline MgH2 - alkaline SiH4 - neutral H2S - weak acidic HCl - strong acid |
| Electrolysis of hydrides | electrolysis of molten hydrides produces Hydrogen gas at +VE electrode |
| Oxidation States rules : | #Uncombined element = 0 #Ions have O-number of charge #Fluorine always = -1 #Hydrogen mostly = +1 #Oxygen usually = -2 |
| Ligands | negative ions or uncharged molecules with one or more lone pairs of electrons. & electron donors, forming dative covalent bonds |
| Naming complexes e.g. [Fe(CN)6]2- | -ligands first, alphabetical order:(ammine, aqua, cyano, chloro) - If complex -ve, ion name ends in 'ate' (ferrate, cuprate) e.g. hexacyanoferrate (II) ion |
| Degenerate | of equal energy (degenerate E levels) |
| Colours of light |
Image:
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| Why do metal compounds absorb light? | e-'s in lower E d-orbitals absorb E and move to higher E orbitals. If energy in d-d transitions corresponds to colour in visible spectrum, we see complementary colour |
| Catalysts | Lower the activation energy --> alternative reaction pathway. Aren't used up. Homogenous, heterogenous (same/different states to reactants) |
| Ground state | The lowest E level an electron can be in. |
| Lyman Series | within UV light spectrum e-'s fall to n=1 energy level |
| Balmer series | within Visible light spectrum excited electron falls to energy level of n=2 |
| Principal Quantum number | n corresponds to the electron shell e.g. n=2 |
| Heisenberg's Uncertainty Principle | "impossible to define with absolute precision, the position & momentum of an electron simultaneously" |
| Pauli Exclusion Principle | atomic orbitals hold a max of 2 electrons with opposite spins. e.g. no two electrons in an atom can have the same four quantum numbers |
| S orbital | spherical like a ball max no. of electrons = 2 |
| P orbital | dumbbell shaped px, py or pz aligned along one of the 3 perpendicular axes' |
| D orbitals | degenerate with each other higher energies then s and p orbitals in same shell |
| Aufbau Principle | Electrons fill orbitals in order of inc. E lowest subshell filled first |
| Hund's Rule | electrons fill each degenerate orbital singly with parallel spins before pairing occurs |
| Electronic arrangements | show only no. of electrons in each shell |
| Electronic configurations | show the subshell that electrons are in |
| Atomic Emission Spectra | colour spectrum + black lines |
| Electronegativity differences (Δ EN ) | use to predict type of bond: same EN = non-polar covalent ΔEN is 0.8ish = polar covalent ΔEN is 3.2+ = ionic |
| Lewis Dot Cross diagrams or electron dot diagrams | |
| Resonance Structures |
Image:
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| Linear | Two bonding e- pairs e.g. BeCl2 |
| Trigonal | 3 bonding pairs (flat triangle shape) e.g. BCl3 |
| Tetrahedral | 4 bonding pairs (pyramid shape, triangle bottom) e.g. CH4 |
| Trigonal Bipyramid | 5 bonding pairs (3D diamond shape) e.g. PCl5 |
| Octahedral | 6 bonding pairs (90 degree angle between each atom) e.g. SF6 |
| Ionic lattice structure types | common : NaCl structure 6:6 co-ordination rarer : CsCl structure 8:8 co-ordination |
| Superconductors | zero electrical resistance at temperatures close to absolute zero (0K or -273 degrees) |
| Semiconductors | higher conductivity than covalent, lower conductivity than metals. as temp increases, conductivity increases. |
| N-type semiconductor | N-type = negative electrons carry charge e.g. silicon doped with arsenic or phosphorus |
| P-type semiconductor | positive holes main current carrier e.g. silicon doped with boron/aluminium |
| Wavelength | distance between adjacent crest in a wave -lambda |
| Frequency | number of wavelengths passing a fixed point in one second v = symbol |
| Unit of wavelength | nanometres - nm - (1x10-9) |
| Unit of frequency | Hertz - Hz |
| Unit and symbol of Velocity | symbol = c (ms-1) |
| Properties of IR light | long wavelength + low frequency |
| Properties of UV light | Short wavelength + High frequency |
| Planck's constant | 6.63 x 10 - 34 Js |
| Avogadro's constant | 6.02 x 10^23 mol-1 |
| Emission Spectra | Black spectrum + coloured lines Lines correspond to E given out when excited electron moves to a lower E level. |
| Excited state | when an electron absorbs the appropriate quantity of E to move from ground state to higher E level. |
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