WIM - Acids, Bases and Bonding Flashcards
Define an acid using the BrØnsted - Lowry theory
A proton donor
Define a base using the BrØnsted - Lowry theory
A proton acceptor
How, in terms of protons do acids and bases react together?
By the transfer of protons from acid to base
What are ionic bonds, how are they formed and what structures do they form?
Ionic bonding is the electrostatic attraction which holds positive and negative ions together in a lattice, and is caused when electrons are transferred from one atom to another to achieve a full outer shell
How do metallic atoms bond and what structures do they form?
Metal elements exist as giant metallic lattice structures of positively charged metal ions in a ‘sea’ of delocalised electrons
Define dative covalent bonding
Where both electrons come from one atom
Give 2 example of covalently bonded substances with giant structures
Diamond and Graphite
Explain how the Arrhenius definition and Bronsted-Lowry definition of a base agree with each other
The Arrhenius definition states that a base releases OH⁻ ions in solution. This agrees with the Bronsted-Lowry definition that bases accept protons (since OH⁻ accepts H⁺ ions) but, Arrhenius’ definition would mean that a substance could not be a base unless in solution.
Name the product for the reaction between gaseous Hydrochloric acid and Ammonia
HCl (g) + NH₃ (g) → NH₄Cl (s)
Hydrochloric Acid + Ammonia → Ammonium Chloride
Give the structure and type of intramolecular bonds for the bonding between ions of a metal and a non-metal
Ionic Bonding held by electrostatic attraction
Ionic Lattice Structure
According to some acid-base theories, aluminium chloride (AlCl₃) is an acid.
Could AlCl₃ be an acid according to the Bronsted-Lowret theory? Explain your answer.
No, because it has no protons to donate
Give the following physical properites for Ionically bonded substances
i) Melting and Boiling points
ii) Typical state at STP
iii) Electrical conductor when solid?
iv) Electrical conductor when liquid?
v) Is it water soluble?
i) High
ii) Solid
iii) No (ions are held firmly in place)
iv) Yes (ions are free to move)
v) Yes
Give the following physical properites for simple molecular (covalently bonded) substances
i) Melting and Boiling points
ii) Typical state at STP
iii) Electrical conductor when solid?
iv) Electrical conductor when liquid?
v) Is it water soluble?
i) Low (have to overcome Van der Waals forces or hydrogen bonds, not covalent bonds)
ii) Sometimes solid, usually liquid or gas (water is lqiuid due to its Hydrogen bonds)
iii) No
iv) No
v) Depends on how polarised the molecule is
Give the following physical properites for giant molecular (covalently bonded) substances
i) Melting and Boiling points
ii) Typical state at STP
iii) Electrical conductor when solid?
iv) Electrical conductor when liquid?
v) Is it water soluble?
i) High
ii) Solid
iii) No (except graphite)
iv) - (will generally sublime)
v) No
Give the following physical properites for metallicaly bonded substances
i) Melting and Boiling points
ii) Typical state at STP
iii) Electrical conductor when solid?
iv) Electrical conductor when liquid?
v) Is it water soluble?
i) High
ii) Solid
iii) Yes (delocalised electrons)
iv) Yes (delocalised electrons)
v) No
