Bonding Flashcards
What is the bond angle, name of shape and how many electron pairs does this molecule have?
- Linear
- 180˚ Bond Angles
- 2 Electron Pairs
What is the bond angle, name of shape and how many electron pairs does this molecule have?
- Trigonal Planar
- 120˚ Bond Angles
- 3 Electron Pairs
What is the bond angle, name of shape and how many electron pairs does this molecule have?
- Tetrahedral
- 109.5˚ Bond Angles
- 4 Electron Pairs
What is the bond angle, name of shape and how many electron pairs does this molecule have?
- Trigonal Bipyramid(ial)
- 120˚ and 90˚ Bond Angles
- 5 Electron Pairs
What is the bond angle, name of shape and how many electron pairs does this molecule have?
- Octahedral
- 90˚ Bond Angles
- 6 Electron Pairs
What does a thick black wedge show?
The atom “coming out” of the paper.
What does a dashed wedge show?
The atom “going into” the paper.
Define Lone Pair.
A lone pair is a pair of electrons that are not involved in bonding.
What bond angles does water have, what do we call that type of molecule (3) and how many lone pairs does a molecule with this bond angle have?
- 104.5˚ Bond Angles
- We call this:
- Bent
- Angular
- V-shaped
- This has 2 lone pairs.
Why does water have lone pairs on the oxygen atom rather than on the hydrogen atoms?
Oxygen is more electronegative than hydrogen, so the lone pairs go closer to the oxygen than the hydrogen.
Why does water take the shape of a “bent” molecule?
The lone pairs come closer to the oxygen than the bonding pair of electrons, so the lone pairs repel more. In addition, the lone pairs aren’t shared out between atoms, so they are more concentrated areas of charge. Both of these factors contribute to making the hydrogens repel and the molecule “bending”.
Give the repulsion hierachy for lone pairs and bonding pairs.
Lone pair/lone pair > Lone pair/bonding pair > Bonding pair/bonding pair.
Give the bond angles, name of the shape it forms and an example of a molecule with four atoms and one lone pair.
- Pyramidal Shape
- 107˚ Bond Angles
- Ammonia (NH₃)
Explain what forms van der Waals intermolecular forces of attraction.
Electrons form a “cloud” around the atom, which causes temporary δ+ and δ- inducements in opposite ends of the atom as it moves. When non-polar molecules get very close to each other, they induce temporary dipole-dipole inducements. These are polar inducements, therefore the attraction is electrostatic.
What causes an atom to have stronger van der Waals forces of attraction?
- Being larger (so it has more electrons)
- Being in molecules (noble gases can still have van der Waals forces of attraction, but they are very weak; take helium which has a very low melting point (4˚K), it still has van der Waals but very few)
What sort of molecules have van der Waals forces of attraction?
None polar molecules - those with an overall electronegativity of zero (e.g. I2) or that are symmetrical (e.g. CH4). Metals cannot have van der Waals forces of attraction due to delocalised electrons.
What sort of attraction takes place between hydrogen chloride (HCl) molecules?
Permanent dipole-dipole interactions. No van der Waals.
How does a permanent dipole-dipole force take place?
Between two polar molecules, the negative end of one molecule attracts the positive end of another molecule.
Give the 2 factors that influence the strength of permanent dipole-dipole forces.
- More polar (greater difference in electronegativity) makes a stronger dipole force;
- Distance between the atoms/molecules also changes the dipole force (closer = stronger).
Between what elements can hydrogen bonding occur?
Between Hydrogen and the lone pairs of Oxygen, Nitrogen or Fluorine.
What is the strongest intermolecular force of attraction?
Hydrogen bonding.
Can more than one intermolecular force of attraction take place at any one time between molecules?
Yes
What is responsible for making water a liquid at room temperature?
Hydrogen bonding.
What properties do hydrogen-bonded molecules have?
Viscous molecules with high boiling points (most being different from the general trend in their group).
