Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
57 Cards in this Set
- Front
- Back
|
Acid + Base |
Salt + Water |
|
|
Acid + Metal |
Salt + Hydrogen |
|
|
Acid + Metal Carbonate |
Salt + Water + Carbon Dioxide |
|
|
Acid + Metal Hydrogencarbonate |
Salt + Water + Carbon Dioxide |
|
|
An acid is a |
proton donor. |
|
|
A base is a |
proton acceptor |
|
|
What are alkalis? |
Hydroxide Ions (OH-) |
|
|
When is HCl an acid? |
When it is dissolved in water so it turns to H+ and Cl- ions. |
|
|
When is HCl not an acid? |
When it is in methybenzene. |
|
|
What colour is Methy Orange in an acid? |
Red |
|
|
What colour is Methy Orange in an alkali? |
Yellow |
|
|
What colour is Phenolpthalein in an acid? |
Colourless |
|
|
What colour is Phenolpthalein in an alkali? |
Purple |
|
|
What colour is Litmus in an acid? |
Red |
|
|
What colour is Litmus in an alkali? |
Light Blue |
|
|
What colour is universal indicator in an acid? |
Red |
|
|
What colour is universal indicator in an alkali? |
Purple |
|
|
What pH is H2SO4? |
Less than 1 |
|
|
What pH is ethanoic acid? |
3 |
|
|
What is the ionic equation for Neutralisation? |
H+(aq) + OH-(aq) -> H2O(l) |
|
|
What makes an acid strong? |
It dissociates completely to give H+ ions in water. |
|
|
What makes a base strong? |
It ionises completely to give OH- ions. |
|
|
What are two examples of strong bases? |
NaOH and KOH |
|
|
What's a weak base? |
Ammonia (NH3) |
|
|
What's the difference between Hydrogen Chloride gas and acid? |
When HCl is in water it dissociates to give H+ and Cl- ions but as a gas it stays as HCl molecules. |
|
|
Hydrochloric Acid + Metal |
Metal Chloride + Hydrogen |
|
|
Sulphuric acid + Metal |
Metal Sulphate + Hydrogen |
|
|
Hydrochloric acid + Metal oxide |
Metal chloride + Water |
|
|
Nitric acid + Metal oxide |
Metal Nitrate + Water |
|
|
Sulphuric Acid + Metal Oxide |
Metal Sulphate + Water |
|
|
Hydrochloric acid + Metal Carbonate |
Metal Chloride + Water + Carbon Dioxide |
|
|
Nitric acid + Metal Carboante |
Metal nitrate + Water + Carbon dioxide |
|
|
Sulphuric acid + Metal Carbonate |
Metal Sulphate + Water + Carbon Dioxide |
|
|
Why are elements metals? |
Because they conduct electricity and they form metal-oxides which are alkali. |
|
|
Why are elements non-metals? |
Because they do not conduct electricity and they form non-metal-oxides which are acidic. |
|
|
Why do elements in the same group have similar chemical properties? |
They have the same number of electrons in their outer shell so they react and bond in similar ways. |
|
|
Why are the noble gasses unreactive? |
They have a full outer shell? |
|
|
How does lithium react in water? |
It fizzes, the metal moves to the surface and the metal gets smaller and dissappears. |
|
|
How does sodium react in water? |
The metal melts into a ball, it fizzes, the metal moves to the surface and the metal gets smaller and disappears. |
|
|
How does potassium react in water? |
It makes a lilac flame, The metal melts into a ball, it fizzes, the metal moves to the surface and the metal gets smaller and disappears. |
|
|
Why do group 1 metals get more reactive as you go down the group? |
The outer shell is further from the nucleus and it is being shielded by the inner electrons so it is less strongly held by the nucleus. |
|
|
What does fluorine look like? |
It is a pale yellow gas |
|
|
What does chlorine look like? |
It is a grey gas |
|
|
What does Bromine look like? |
It is a brown liquid |
|
|
What does iodine look like? |
It is a grey solid |
|
|
What happens to halogens as you go down the group? |
They become less reactive because of more electon shells which make the molecule bigger and therefore the intermolecular bonds get stronger. |
|
|
Halogens exist as what? |
Diatomic molecules. |
|
|
Why are Halogens boiling points low? |
They exist as diatomic molecules and the intermolecular forces are weak so easy to be broken. |
|
|
What 4 factors affect the rate of reaction? |
Surface Area, concentration, temperature, catalysts. |
|
|
What experiment would you use to test how surface area affects the rate of reaction? What considerations would you take? |
Calcium Carbonate chips and HCl. Cotton wool stops the HCl or CaCO3 spraying out.` |
|
|
What experiment would show the effects of concentration on rate of reaction? |
Mg with HCl. |
|
|
Why does a higher concentration acid make the rate of reaction faster? |
The higher concentration means there are more H+ ions so the frequency of collision is higher? |
|
|
How would you see the effects of temperature on rate of reaction? |
By using Sodium thiosulphate with HCl and a cross underneath the beaker. |
|
|
What is the relationship of temperature and rate of reaction? |
Non-linear |
|
|
How do catalysts affect rate of reaction? |
They create an alternative pathway with lower activation energy. |
|
|
Describe diamond |
Covalent carbon-carbon bonds High melting and boiling point Extremely hard Insoluble |
|
|
Describe Graphite |
Covalent carbon-carbon bonds Weak forces between layers so they can slide over each other. Used as a lubricant. Electrons can flow between layers so it conducts electricity. |
