Chemistry /Edexcel A Level Chemistry: Inorganic Chemistry and the Periodic Table Part 1
Edexcel A Level Chemistry: Inorganic Chemistry and the Periodic Table Part 1
This flashcard deck covers key concepts from the Edexcel A Level Chemistry syllabus, focusing on inorganic chemistry and the periodic table. It includes questions on ionisation energy, reactivity, reactions of group 2 elements, solubility trends, thermal stability, and flame tests.
How does ionisation energy change down group 2?
It decreases
Tap or swipe ↕ to flip
Swipe ←→Navigate
SSpeak
FFocus
1/45
Key Terms
Term
Definition
How does ionisation energy change down group 2?
It decreases
Why does ionisation energy decrease down Group 2?
The extra inner shells shield electrons. Nucleus is further away from outer electrons due to more shells
How does reactivity change down group 2?
Reactivity increases
Why does reactivity increase down group 2?
It becomes easier for the outer electrons to be lost, as they have lower ionisation energies
What do group 2 elements react with?
Water, oxygen and chlorine
What are the group 2 elements?
Beryllium, Magnesium, Calcium, Strontium, Barium (Radium)
Related Flashcard Decks
Study Tips
- Press F to enter focus mode for distraction-free studying
- Review cards regularly to improve retention
- Try to recall the answer before flipping the card
- Share this deck with friends to study together
Term | Definition |
---|---|
How does ionisation energy change down group 2? | It decreases |
Why does ionisation energy decrease down Group 2? | The extra inner shells shield electrons. Nucleus is further away from outer electrons due to more shells |
How does reactivity change down group 2? | Reactivity increases |
Why does reactivity increase down group 2? | It becomes easier for the outer electrons to be lost, as they have lower ionisation energies |
What do group 2 elements react with? | Water, oxygen and chlorine |
What are the group 2 elements? | Beryllium, Magnesium, Calcium, Strontium, Barium (Radium) |
What do group 2 elements produce when they react with water? | Hydroxides and hydrogen |
Which group 2 elements react with water? | All except Be, Mg reacts very slowly |
What do group 2 elements produce when they react with oxygen? | Oxides |
What colour are group 2 oxides? | White |
What do group 2 elements produce when they react with chlorine? | Chlorides |
What colour are group 2 chlorides? | White |
Oxides and hydroxides are… | …bases |
What happens when group 2 oxides dissolve in water? | They form a strongly alkaline solution due to OH- |
What happens when beryllium oxide is added to water? | It doesn’t dissolve, it is insoluble |
What happens when magnesium oxide is added to water? | It reacts slowly and isn’t very soluble |
When oxides and hydroxides are added to acid, what do they form? | They neutralise the acid to form salts |
What is the equation for the reaction between MgO and H2O? | MgO + H2O —-> Mg(OH)2 |
What is the equation for the reaction between MgO and HCl? | MgO + 2HCl —-> MgCl2 + H2O |
Solubility trends of group 2 depend on… | …the anion |
If a group 2 compound has a singly charged anion (OH-) how does the solubility change down the group? | It increases |
If a group 2 compound has a doubly charged anion (SO4 2-) how does the solubility change down the group? | It decreases |
Which group 2 sulfate is insoluble? | Barium Sulfate |
How does thermal stability change down group 1 and 2 carbonates and nitrates? | It increases |
Why do carbonates and nitrates become more stable down the group? | Large ions have less polarising power so distort the electron cloud less and have a lower charge density. Therefore, they distort the carbonate or nitrate less |
Which of group 1 and group two compounds are more thermally stable? | Group 1 |
Why are Group 1 compounds more stable than group 2? | They have a lower charge, so a lower charge density and therefore less polarising power |
What do group 2 carbonates decompose to form? | An oxide and carbon dioxide |
What is the equation for thermal decomposition of CaCO3? | CaCO3 ----> CaO + CO2 |
Do group 1 carbonates decompose? | No |
What do group 1 nitrates decompose to form? | The Nitrite (NO2) and oxygen |
What is the equation for decomposition of Potassium nitrate? | 2KNO3 ----> 2KNO2 + O2 |
What is the exception to the group 1 nitrate decomposition? | Lithium |
What does lithium nitrate decompose to form? | LiO2, NO2 and O2 |
What doe group 2 nitrates decompose to form? | The oxide, nitrogen dioxide and oxygen |
What is the equation for the decomposition of Ca(NO3)2? | 2Ca(NO3)2 ----> 2CaO + 4NO2 + O2 |
How can the thermal stability of nitrates be tested? | Measuring how long it takes for a certain amount of oxygen to be produced |
How can the thermal stability of carbonates be tested? | Measuring how long it takes for a certain amount of CO2 to be produced using lime water |
What is the flame colour for Lithium? | Red |
What is the flame colour for Sodium? | Orange/Yellow |
What is the flame colour for Potassium? | Lilac |
What is the flame colour for Rubidium? | Red |
What is the flame colour for Caesium? | Blue |
What is the flame colour for Calcium? | Brick red |
What is the flame colour for Strontium? | Crimson |