Topic 3- Bonding Flashcards
What does covalent bonding consist of (exam answer)?
What does covalent bonding consist of (full answer)?
How are the atoms held together in covalent bonding?
What are the four different types of formations in covalent bonding and give examples?
What is the full general rule of covalent bonding?
What is the only metal that bonds in covalent bonding?
What is formed in covalent bonding?
A shared pair of electrons
A shared pair of electrons with one electron being supplied by each atom either side of the bond
Because their nuclei which have an overall positive charge are attracted to the shared electrons
- Between atoms of the same element (eg N2, O2, diamond, graphite)
- Between atoms of different elements on the right-hand side of the periodic table (eg CO2, SO2)
- When one of the elements is in the middle of the table (eg CCl4, SiCl4)
- With head of the group elements with high ionisation energies (eg BeCl2)
That covalent bonding is between non metals- either themselves or another non-metal
Beryllium (Be)
In covalent bonding, a molecule is formed.
What pairs are formed in covalent bonding when an element shares only a few of its electrons?
What is formed in the covalent bonding of oxygen and why?
What are the following properties of simple covalent molecules like:
Bonding
Electrical
Solubility
Boiling Point
What are intermolecular forces?
What happens as a result of the intermolecular forces being weak in simple covalent molecules?
Why are some boiling points higher than expected for a given mass?
Lone pairs
A double covalent bond is formed because each oxygen shares 2 of its electrons
Bonding: Atoms are joined together within the molecules by covalent bonds
Electrical: Do not conduct electricity as they have no mobile ions or electrons
Solubility: Tend to be more soluble in organic solvents than in water; some are hydrolysed
Boiling Point: Low- intermolecular forces are weak; they increase as molecules get a larger surface area
Forces between molecules
Little energy is required to separate molecules from each other so boiling points are low
Because you can get additional forces or attraction.
How does a co-ordinate bond differ from covalent bond?
What happens in a co-ordinate bond (full detail)?
What happens to the donor species?
What happens to the acceptor species?
What happens to an ammonium ion in its co-ordinate bonds?
What are the four types of crystal structures?
Only in its formation
Both electrons of the shared pair are provided by one species- or atoms- (donor) and it shares the electrons with the acceptor
Donor species will have lone pairs in their outer shells
Acceptor species will be short of their “octet” or maximum
The Nitrogen now has a positive charge as it is now sharing rather than owning two electrons
- Giant ionic lattice
- Simple covalent compounds (molecular)
- Giant covalent structures (macromolecular)
- Giant metallic lattice.
What is the definition of an ionic bond?
What do dot-cross diagrams show?
What do metals do to non-metals and what two things does this then produce?
What is a giant ionic lattice?
What are the melting and boiling points like of giant ionic lattices?
Why is this?
What don’t giant ionic lattices do when solid and why?
What do giant ionic lattices do when molten or dissolved in water?
What is the solubility like of giant ionic lattices (full description)?
Why are giant ionic lattices brittle (full description)?
An electrostatic attraction between oppositely charged ions
Outer electrons only (eg NaCl)
Metals transfer electrons to non-metals producing positive metal ions and negative non-metal ions
Lattice of oppositely charged ions
High melting and boiling points
Because of strong forces of attraction between ions that need to be broken
Do not conduct electricity when solid (because ions not free to move)
Conduct electricity when molten or dissolved in water (because ions then free to move)
- Soluble in water
- Insoluble in non polar solvents (water is a polar solvent and stabilises the separated ions)
If you move a layer of ions, you get ions of the same charge next to each other. The layers repel each other and the crystal breaks up.
What happens in giant ionic crystal lattice?
What does the arrangement of ions in a crystal lattice depend on?
What do ionic compounds exist as in their solid state?
What happens to the forces in these compounds when in solid state?
What is the ionic symbols for the following ionic compounds:
Ammonium
Carbonate
Hydroxide
Nitrate
Sulfate
What are compound ions?
Oppositely charged ions held in a regular 3-dimensional lattice by electrostatic attraction
The relative sizes of the ions
In their solid state, ionic compounds exist as giant lattices
Attractive and repulsive forces are balanced
NH4 +
CO3 2-
OH -
NO3 -
SO4 2-
Ions made up of a group of atoms with an overall charge.
What is and describe the melting point of silica?
What is and describe the strength of silica?
What is and describe why silica is a non-conductor of electricity?
What is an example of monatomic?
What is the conductivity of the following types of structure in solid, liquid and aqueous solution:
Monatomic
Simple Covalent (molecular)
Giant Covalent (macromolecular)
Ionic
Metallic
Very high due to many covalent bonds that must be broken into separate atoms
Strong due to each silicon atom being joined to four oxygen’s and each oxygen atoms are joined to two silicon’s
Non-conductor as there are no mobile electrons
Noble gases
No for solid, liquid and aqueous solution
No for solid and liquid and no for aqueous solution (but may react)
No for solid, liquid and aqueous solution
No for solid and yes for liquid and aqueous solution
Yes for solid and liquid and no for aqueous solution (doesn’t dissolve; but may react).
What are and describe what the particles are like for:
Solid
Liquid
Gas
Particles close together, vibrating about a fixed point
Particles move freely and randomly within the liquid
Particles move about freely with little attraction between them.
