Chemical Bonding Flashcards
What is an ionic bond?
Electrostatic forces of attraction between oppositely-charged ions
Ionic bonds are non-directional.
What is a covalent bond?
Electrostatic forces of attraction between a shared pair of electrons and positively charged nuclei.
What is a metallic bond?
Electrostatic forces of attraction between a lattice of positive ions and a sea of delocalised electrons.
Metallic bonds are non-directional.
What determines the strength of an ionic bond?
Charge density, which affects Lattice energy
What determines the strength of a metallic bond?
Charge density of cations
What determines the strength of a covalent bond?
4 factors
1) Effectiveness of atomic orbital overlap (how diffuse orbital is)
2) Number of bonds
3) Polarity
4) Presence of neighbouring lone pairs
What is a coordinate/dative bond? What are the requirements for one to form?
A bond where the shared pair of electrons is only provided by one of the bonding atoms.
The donating atom must have a lone pair of electrons, and the receiving atom must have a vacant, low-lying orbital to accept the electrons.
Determine and explain the shape of SF4
State its bond angle.
Since SF4 has four bond pairs of ELECTRONS and one lone pair OF ELECTRONS, it has
Trigonal bipyrimidal
See-saw, since it has one lone pair.
107 degrees.
Determine and explain the shape of PCl5
State its bond angle.
Trigonal bipyrimidal, since it has five regions of electron density and no lone pairs.
120 degrees on equatorial plane, 90 degrees from axial to equatorial.
Determine and explain the shape of SF6
State its bond angle.
Octahedral, since it has six regions of electron density and no lone pairs.
90 degrees.
Bond angle of tetrahedral
109.5 degrees
Draw IF2-
Linear with two lone pairs and a -1 charge.
Bond angle of trigonal planar
120 degrees
Determine and explain the shape of H2O
State its bond angle.
Tetrahedral, four regions of electron density.
Bent, two lone pairs.
105 degrees.
Draw SO3
Trigonal planar shape with every bond being S=O