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Determined by the number of regions of electron density around an atom. (bonding and nonbonding). Polar covalent bond. Electronegativity. F O N and Cl S.
Typology: Lecture notes
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Shape of SF 2 Shape of HCl^ Shape of CO 2 Shape of F^2 O
V shaped or bent Linear Linear V shaped or bent
Shape of NCl (^3) Shape of PBr 3 Shape of SO^2 Shape of CCl^4
Trigonal pyramid Trigonal pyramid V shaped or bent Tetrahedral
Shape of CH 2 Cl 2 Shape of PCl^3 Shape of PH (^3) Shape of H 2 O
Tetrahedral Trigonal pyramid Trigonal pyramid V shaped or bent
Shape of CCl (^4) Shape of H 2 S Shape of CH^3 Br^ Shape of SO (^2)
Tetrahedral V shaped or bent Tetrahedral V shaped or bent
Shape of COCl (^2) Shape of H 2 CO Shape of O 2 Shape of O^3
Trigonal planar Trigonal planar Linear V shaped or bent
Definition: Uneven sharing of electrons, where one atom in bonding pair is more electronegative
Definition: Ability of an atom in a bond to attract electrons towards itself
The 5 most electronegative elements
Determined by the number of regions of electron density around an atom (bonding and nonbonding)
Polar covalent bond Electronegativity F O N and Cl S Shape of molecule
NaCl
Type of particles? Type of bond?
Type of particles? Type of bond?
SiO (^2)
Type of particles? Type of bond?
MgO
Type of particles? Type of bond?
Ions Ionic bond
Molecules Weak intermolecular
Atoms Covalent
Ions Ionic bond
Type of particles? Type of bond?
SCl (^2)
Type of particles? Type of bond?
C (diamond)
Type of particles? Type of bond?
SiCl (^4)
Type of particles? Type of bond?
Molecules Weak intermolecular
Molecules Weak intermolecular
Atoms Covalent
Molecules Weak intermolecular
Temperature at which (l) →(g); its value reflects the strength of bonds between particles
Nonpolar solutes will dissolve in ______ solvents e.g.
Polar solutes will dissolve in ______ solvents e.g.
Type of solid: Consists of large covalently bonded molecules with strong attractions between atoms
Boiling point Nonpolar Cyclohexane
Polar Water
Covalent network
Type of solid: A 3D crystal lattice made up of alternating + and - ions
Definition: Charged particles formed when atoms have lost or gained electrons
Name for a positively charged ion
Name for a negatively charged ion
Ionic Ions Cation Anion
Most ionic solutes e.g. NaCl will dissolve in ______ solvents
Attractive force between molecular dipoles
Type of solid: Consists of metal cations in a sea of delocalised electrons
Definition: Electrostatic attraction between oppositely charged ions
Polar e.g. water
Weak intermolecular attraction
Metallic Ionic bond
Definition: Attraction between positively charged nuclei of metal atoms and loosely held valence electrons
Definition: Bond formed by the sharing of a pair of electrons
Trend in bonding types moving across a period L to R e.g. NaCl AlCl 3 PCl 3 Cl (^2)
Definition: Diagram showing bonding between atoms in a molecule and any lone pairs of electrons in the molecule
Metallic bond Covalent bond Ionic to covalent Lewis diagram
Bond between two atoms containing 4 electrons (2 pairs)
Bond between two atoms containing 6 electrons (3 pairs)
Type of solid: Crystal lattice of ions held together by electrostatic attractions
Type of solid: Molecules held together by weak intermolecular attractions
Double bond Triple bond Ionic solid Covalent molecular
Type of solid: Atoms held together by nondirectional attractions between delocalised electrons and metal ions
Type of solid: Many atoms in a regular 3D lattice held together by covalent bonds
Shape of molecule & bond angle:
Shape of molecule & bond angle:
Metallic solid Covalent network solid
Linear 180 o
Trigonal planar Approx. 120o
Shape of molecule & bond angle:
Shape of molecule & bond angle:
Shape of molecule & bond angle: Shape of molecule & bond angle:
Tetrahedral Approx. 109o
V shaped / bent Approx. 109o
Trigonal pyramid / pyramidal Approx. 109o
Linear Bond angle n/a
Identity of this covalent network solid
Identity of this covalent network solid
Identity of this covalent network solid
Diamond, C
Silicon dioxide / silica / SiO 2 Graphite, C^ No Brain Too Small
