1.3 Bonding Flashcards
Which element is most electro positive and why?
Caesium.
Has a large atomic radius with comparatively low nuclear charge.
How does electronegativity change across a period and why?
Electronegativity increases. Because... Nuclear charge increases The number of energy levels remains the same Atoms contract so get smaller
Name the three main types of intermolecular force from weakest to strongest.
Van der Waals
Dipole-dipole
Hydrogen bonding
What is the shape and bond angle for a molecule with:
3 bonding pairs
1 lone pair
Pyramidal
107 degrees
What is the shape and bond angle for a molecule with:
3 bonding pairs
No lone pairs
Trigonal planar
120 degrees
What is the shape and lone pair for a molecule with:
4 bonding pairs
2 lone pairs
Square planar
90 degrees
What is the shape and bond angle for a molecule with:
4 bonding pairs
No lone pairs
Tetrahedral
109.5 degrees
What is the shape and bond angle for a molecule with:
6 bonding pairs
No lone pairs
Octahedral
90 degrees
What is the shape and bod angle for a molecule with:
2 bonding pairs
2 lone pairs
Bent
104.5 degrees
What is the shape and bond angle for a molecule with:
2 bonding pairs
No lone pairs
Linear
180 degrees
What is the shape and bond angle for a molecule with:
5 bonding pairs
No lone pairs
Trigonal bipyramid
120 degrees
Which element is most electronegative and why?
Fluorine.
Has a small atomic radius with a comparatively large nuclear charge.
What is Electronegativity?
Electronegativity is the relative ability of an atom to attract electrons in a covalent bond.
What is Dative bonding?
A Dative covalent bond is a pair of electrons shared between two atoms, one of which provides both electrons to the bond.
What is Polar bonding?
A Polar covalent bond is a pair of electrons that are shared unequally between two atoms.
Name 4 types of crystal structure
- Ionic
- Metallic
- Macromolecular (giant covalent)
- Molecular
What’s the structure, type of bonding and properties of DIAMOND.
Giant Molecular Covalent Shiny and hard High melting point High boiling point
What’s unusual about graphite?
It conducts electricity due to having delocalised electrons
What happens to iodine when heated and why?
It sublimes(goes from solid to gaseous) Due to the fact only VdW forces are holding iodine atoms together so it's very easy to overcome these forces resulting in a low boiling point.
Explain why does ice float?
Water molecules are held together by weak hydrogen bonds.
These hydrogen bonding forces a rather open structure on the ice leaving gaps in the structure. This means that when water freezes it expands which occupies more space becoming less dense that water.
Define metallic bonding
Metallic bonding involves attraction between delocalised electrons and positive ions arranged in a lattice.
Define ionic bonding
Ionic bonding involves electrostatic attraction between oppositely charged ions in a lattice
