857655
Description
Mind Map by brandon.fletcher, updated more than 1 year ago
|
Created by brandon.fletcher
over 10 years ago
|
|
Unit 1 - Chapter 2
- Limestone & its Uses
- Its Uses
- Neutralising
- Buildings
- Toothpaste
- Concrete
- Glass
- Neutralising
- Calcium Carbonate: CaCO3
- Found in the ground
- A pale white-ish rock
- Thermal Decomposition:
When a substance is
heated it will break down
into simpler substances
- Metal Carbonate --> Metal Oxide + Carbon dioxide
- This happens with similar effects with all metals in group 2
e.g Magnesium Carbonate --> Magnesium Oxide + Carbon dioxide
- This happens with similar effects with all metals in group 2
e.g Magnesium Carbonate --> Magnesium Oxide + Carbon dioxide
- CaCO3 --> CaO + CO2
- Metal Carbonate --> Metal Oxide + Carbon dioxide
- Its Uses
- Reactions of Carbonates
- Limestone Statues are
affected by acid rain
- Testing for Carbon Dioxide
- Limewater is a solution
of Calcium Hydroxide.
It is alkaline!
- Carbon Dioxide is a weak acidic
gas so it reacts with the Limewater.
- Tiny particles of insoluble Calcium Carbonate
are formed. This makes it look cloudy.
- Limewater + Carbon Dioxide = Calcium Carbonate + Water
- Ca(OH)2 + CO2 = CaCO3 + H2O
- Limewater is a solution
of Calcium Hydroxide.
It is alkaline!
- Carbonate + Acid = Salt + Water + Carbon Dioxide
- Calcium Carbonate + Hydrochloric Acid =
Calcium Chloride + Water + Carbon Dioxide
- CaCO3 + 2HCl = CaCl2 + H2O + CO2
- CaCO3 + 2HCl = CaCl2 + H2O + CO2
- Limestone Statues are
affected by acid rain
- The Limestone Cycle
- Step 2 is important - If we add water
to Calcium Oxide we get limewater!
- Nuetralizing Acids
- Calcium Hydroxide is an alkali. It can neutralise
acids to create calcium salt and water.
- is used to neutralise soil and harmful
acidic gases given of by factories.
- Calcium Hydroxide is an alkali. It can neutralise
acids to create calcium salt and water.
Media attachments
Want to create your own Mind Maps for free with GoConqr? Learn more.