Chemistry Flashcards
Molecular ions
Ammonium
NH4 (1+)
Molecular ions
Carbonate
CO3 (2-)
Molecular ions
Hydroxide
OH (1-)
Molecular ions
Hydrogen carbonate
HCO3 (1-)
Molecular ions
Nitrate
NO3 (1-)
Molecular ions
Sulfate
SO4 (2-)
Quicklime
CaO
Slaked lime
Ca(OH)2
Testing for cations using sodium hydroxide
Ammonium
Ammonia gas produced; turns red litmus blue
Testing for cations using sodium hydroxide
Calcium
White percipitate insoluble in excess
Testing for cations using sodium hydroxide
Copper (II)
Light blue percipitate insoluble in excess
Testing for cations using sodium hydroxide
Iron (II)
Green percipitate insoluble in excess
Testing for cations using sodium hydroxide
Iron (III)
Red-brown percipitate insoluble in excess
Testing for cations using sodium hydroxide
Zinc (II)
White percipitate soluble in excess
Testing for cations using ammonia
Calcium
No percipitate or very slightly white ppt
Testing for cations using ammonia
Copper (II)
Light blue ppt, soluble in excess
Testing for cations using flame
Lithium
Red
Testing for cations using flame
Sodium
Yellow
Testing for cations using flame
Potassium
Lilac
Testing for cations using flame
Copper (II)
Blue-green
Testing for anions
Carbonate
Add dilute acid to see effervescence (CO2 produced)
Testing for anions
Chlroide
Acidify with dilute nitric acid then add silver nitrate (White ppt)
Testing for anions
Bormide
Acidify with nitric acid then add silver nitrate (Cream ppt)
Testing for anions
Nitrate
Add sodium hydroxide then aluminium foil (ammonia gas produced)
Testing for anions
Sulfate
Acidify then add barium nitrate or barium chloride (white ppt)
Trends in periodic table
Trends in Group 1
- Density increases down the group
- Melting point decreases down the group
- React with water to produce metal hydroxide or hydrogen gas
Trends in periodic table
Trends in Group 7 - halogens
- When reacted with metals, produces salts
- Exist as diatoms
- Non-metallic
- Color increases in darkness down the group
- Density increases down the group
- Reactivity decreases down the group
Molten lead bromide
Product at cathode: Lead
Product at anode: Bromide
Observations: Silvery solid at the cathode, brown gas at the anode
Concentrated aqueous sodium chloride
Product at cathode: Hydrogen
Product at anode: Chloride
Observations: Colourless gas at the cathode, pale yellow green gas at the anode which bleaches damp litmus paper
Acid + metal
Observation:
* Effervescence
* Heat evolved
* Hydrogen gas formed
Reaction occurring:
Acid + Metal -> Salt + Hydrogen
Acid + Base
Observation:
Indicator goes green
Reaction occurring:
Neutralisation
Acid + Base -> Salt + Water
Bronze
Copper and tin
Mild steel
Iron and about 0.25% carbon
High carbon steel
Iron and up to 2.5% carbon
Brass
Copper and zinc
Stainless steel
Iron, carbon, chromium and nickel
General formula of alkanes
CnH2n+2
General formula of alkenes
CnH2n
Thermal decomposition
A process where a compound breaks down when heated. New products are formed. These are usually endothermic.
Redox reaction in catalytic converters
2NO + 2CO → N2 + 2CO2