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STRUCTURE AND BONDING
10/03/2023
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structure AND bonding Tonic bonding → the electrostatic attraction between two oppositely charged ions Type of atom: metal and a non-metal STRONG IONIC BONDS How is it formed: Metal loses electron to form +ve ion, non metal gains electron to form -ve coralent bonding A shared pair of electrons diamond graphite Giant covalent lattice Atomi Strong covalent bonds. Type of atom: Between non-metal atoms simple molecule moleculer How it is formed: Atoms share electrons weak intermolecular forcer. Metallic bonding Type of atom within a metal. strong metallic bonds How is it formed Metal loser outer most elections to form - ve and a sea of delocalised elections. co-ordinate bonding •special type of covalent bond. Shapes of MOLECULES nº bonding pairs BASIC shapes Electron Bonding Pairs Pairs 3 3 4 NH₂ 4 H₂O 4 Electron Bonding Lone Pairs Pairs Pairs 5 5 Behave the same way as normal covalent bonds 3 5 2 5 4 4 3 3 2 0 Electron Bonding Lone Pairs Pairs Pairs 1 2 Lone pairs have greatest repulsion Lone Pairs Shape 0 0 1 2 2 1 1198 - (no electrons in outer + atoms bonded) nº lone pairs - bonded - atoms bonded. pairs 120 120° 118° 120° 109.5° 107° o 120 Basic shape Trigonal planar 104.5° i_89° The electrostatic attraction between a tve metal ion and-ve delocalised election. C 90° Shape Shape Bent (V-shape) -90-0 Basic shape Tetrahedral Pyramidal Bent (V-shape) A shared pair of electrons where both elections come from the same atom Basic Shape Trigonal bipyramidal Triangle based pyramid or see-saw Trigonal planar or T-shape Electron Bonding Lone Pairs Pairs Pairs 6 6 6 6 5 4 0 1 2 O o O Shape ° 90° 9 89° O 90° Explaining shape and bond angle ↓ state nº electron pairs + Give basic shape + bond angle t Lone pairs ? Basic Shape Octahedral Distorted Square based pyramid Square planar tha YES Lone pairs repel more bond pairs A Bond angle reduced by 2⁰ for each lone pair No Bond pairs repel equally. State bond angle...
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Alternative transcript:
The ability of an atom to pull election density towards electronegativity → itself, across a COVALENT BOND Depends on 3 things : -Nuclear charge shielding -Atom radius Electronegativity increases across a period nuclear charge increases Amount of shielding is the same. Atomic radius increases → • Stronger attractions Electronegativity decreaser down a group. FLUORINE MOST ELETRONEGATIVE Inuclear charge increases Amount of shielding increases Atomic radiur increases Diatomic moleauer are perfect covalent bonds. Intermolecular FORCES van der Waals → dipole-dipole · VON only. + Hydrogen strongest weakest van der Waals Act on all moleculer at all times (monoatomic too). VDW forces are the attraction between opposite charger on temp + induced dipole More electrons stronger forcer Branched chains reduce VDW's as moleculer can't sit as close together. Permanent dipole-dipole forces Occurs between moleculer with an overall dipole. Differences in electronegativity lead to polar Covalent bonds symmetrical - → has a basic shape and all atoms bonded are the same. symmetrical moleculer have no dipole because election density is evenly spread. HYDROGEN bonding Acts between molecules that have a I atom bonded to a f, 0 or N atom. Large difference in electronegativity. I atom 8+ and F,0 or N 8. Hydrogen is attracted to lone pair of elections on F,0 or N atom. Melting + boiling point. small size + higher charge The stronger the IMF the 4 the melting + boiling point. When simpe covalent substancer melt IMF are broken Stronger IMF more energy needed to break them. If type of IMF is the same consider size + shape of the molecule For conic + metallic consider size and charge of cons < attraction Stronger bond.