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Pregunta | Respuesta |
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 |
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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 |
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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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