Bonding Flashcards
What is an ionic bond?
lonic bonding involves electrostatic attraction
What is a metallic bond?
The attraction between delocalised electrons and cations
Draw trigonal bipyramidal
[Draw it]
Draw an octahedral
[Draw it]
What is a covalent bond
The attraction between a pair of electrons and the nucleus it lies between
Draw tetrahedral
[Draw it]
Draw trigonal pyramidal
[Draw it]
what is the bonding angle in a linear molecule
the bonding angle in linear is 180 degrees
what is the bonding angle in trigonal planar
the bonding angle in trigonal planar is 120 degrees
what is the bonding angle in tetrahedral
the bonding angle in tetrahedral is 109.5 degrees
what is the bonding angle in trigonal pyramidal
the bonding angle in trigonal pyramidal 107
what is the bonding angle in bent
the bonding angle in bent 104.5 degrees
what is the bonding angle in trigonal bipyramidal
the bonding angle in octahedral is 90 degrees down and 120 degrees accross
what is the bonding angle in octahedral
the bonding angle in octahedral is 90 degrees
which simple molecular shape has
2 electron groups
2 bonding electron groups
0 lone pairs
Linear
which simple molecular shape has
3 electron groups
3 bonding electron groups
0 lone pairs
trigonal planar
which simple molecular shape has
4 electron groups
4 bonding electron groups
0 lone pairs
tetrahedral
which simple molecular shape has
4 electron groups
3 bonding electron groups
1 lone pairs
trigonal pyramidal
which simple molecular shape has
4 electron groups
2 bonding electron groups
2 lone pairs
Bent
which simple molecular shape has
5 electron groups
5 bonding electron groups
0 lone pairs
trigonal bipyramidal
which simple molecular shape has
6 electron groups
6 bonding electron groups
0 lone pairs
octahedral
what is a free radical
a species that has one unpaired electron
why is NH4 (for example) tetrahedral
applies to similar questions
- There are 4 bonding pairs that repel each other equally as far away as possible,
- the bond angle is 109.5, the shape is tetrahedral
why is H3O trigonal pyramidal
-There are 3 bonding pairs of electrons and 1 lone pair of electrons that repel each other as far away as possible
- lone pairs repel more than bonding pairs
-the bonding angle is 107 the shape trigonal pyramidal
How is a dative bond formed in ammonium ion
Ammonia donates its lone pair of electrons to a H+ ion making it NH4 +
What is electronegativity
Ability of an atom to withdraw electrons density towards itself
In a covalent bond
Properties of diamond
giant covalent structures
diamond is hard because of 3d structure
Diamond carbon atoms joined to 4 other carbon atoms
Properties of graphite
Carbon atoms in graphite joined to 3 other carbon atoms
Graphite is soft because has layers that can Slide Over each other because of weak intermolecular forces
Why is the melting point high for carbon and diamond
Covalent bonds must be broken
Which requires a lot of energy
What is the difference between graphite and diamond
Diamond is a not a conductor of electricity and has no delocalised electron
Graphite has delocalised electron and can conduct electricity
Name 3 types of bondings
Van der Waals
Hydrogen
Dipole dipole
Why is the energy needed to vaporise sodium chloride is much more than the energy needed to melt sodium chloride
Because vaporisation breaks all the bonds
Ionic compound conduct what when they are molten?
Electricity
Why to ionic compounds dissolve in water
Water molecules are polar- part of water molecules have a small negative charge and others have positive so the charged parts pill ions away from the lattice
What molecule shape has 5 electron pairs and 1 lone pair
Seesaw
What molecule shape has 5 electron pairs and 2 lone pairs
T-Shaped
What molecule shape had 6 electron pairs and 2 lone pairs
Square planar
What is the bonding angle of seesaw
102 degrees and 87 degrees
What are the bonding Angie of T-shaped
88 degrees
What is the bond angle of square planar
90 degrees
What is a dipole
A difference in charge between two atoms caused by an uneven shift in electron density
What causes a permanent dipole
In polar bonds the shift in electronegativity between two atoms causes a permanent dipole.
Explain van der waals
At any moment electrons are more likely to be on one side of an atom called an instantaneous dipole
This dipole can cause an induced dipole and the two dipoles are now attracted to each other
The second dipole caused another dipole in another atom
Electrons are always moving so dipoles are constantly created and destroyed
Name properties of ionic substances
- high mp and bp
- typical state solid
- can’t conduct electricity in solid state
- can conduct electricity in liquid state
- is soluble in water
Name properties of simple covalent substances
- Low melting and boiling points
- is usually a liquid or gas
- can’t conduct electricity in solid
- can’t conduct electricity in liquid
- is soluble in water depending on polarity of molecules
Giant covalent substance properties
-high melting and boiling point
- typically solid at room tem
- solid cannot conduct electricity except for graphite
- does not melt, it sublimes
-is not soluble in water
Metal is substance properties
High melting and bp
Typically solid
Can conduct electricity in solid and liquid state
Not soluble in water
Explain why Nickle high mp
- contains positive metal ions
- delocalised electron
- strong attraction between metallic bonds
