Chemistry: 2.2 Group 2 Notes
This flashcard set outlines the physical and chemical characteristics of Group 2 elements, including their high melting points, hardness, and density due to strong metallic bonding. It also explains their consistent reactivity patterns, attributed to the loss of two electrons during reactions.
what are group 2 MP like
high
Key Terms
what are group 2 MP like
high
why are group 2 MP high
metals have strong metallic bnding
are group one or group 2 harder
group 2 are harder and have a higher density than group one elements
why are group 2 elements harder and have a higher density than group 1 elements
ions are smaller and more highly charged therefore ions pack together more closely leading to stronger bonding
what are group 2 elements reactivity’s like
reactive with similar chemical reactions
why are group 2 elements reactive metals with similar chemical reactions
they all lose 2 electrons when they react
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| Term | Definition |
|---|---|
what are group 2 MP like | high |
why are group 2 MP high | metals have strong metallic bnding |
are group one or group 2 harder | group 2 are harder and have a higher density than group one elements |
why are group 2 elements harder and have a higher density than group 1 elements | ions are smaller and more highly charged therefore ions pack together more closely leading to stronger bonding |
what are group 2 elements reactivity’s like | reactive with similar chemical reactions |
why are group 2 elements reactive metals with similar chemical reactions | they all lose 2 electrons when they react |
| white solids/colourless solutions |
trend in atomic radius in group 2 | increases down group 2 |
why does atomic radius increase down group 2 | shells increase |
trend in first IE down group 2 | decreases |
why does first IE decrease down group 2 | shells increase |
trend in melting points down group 2 | decrease |
why do melting points decrease down group 2 |
- as ions increase, charge density decreases- attraction/bonding decreases |
trend in reactivity down group 2 | increases |
why does reactivity increase down group 2 | lose electrons more readily as we go down group because:
|
observations of the reaction of magnesium with cold water | very slow few bubbles of gas |
products of the reaction of magnesium with cold water | magnesium hydroxide and hydrogen |
Products of the reaction of magnesium with steam | Magnesium oxide and hydrogen |
Observations of the reaction between calcium and water | Effervescence Solid Ca dissolves |
Products of the reaction between calcium and water | Calcium hydroxide and hydrogen |
Observations of the reaction between strontium and water | Vigorous fizzing Solid strontium dissolves |
| Strontium hydroxide and hydrogen |
Observations of reaction between barium and water |
- solid barium dissolves |
Products of the reaction between barium and cold water | Barium hydroxide and hydrogen |
What is the general trend in reactivity with water of group 2 element as you go down the group | Reactivity increases |
Why is titanium a useful metal | Strong, high melting point and high corrosion resistance |
Where does titanium have many applications | In the aerospace, marine and motor vehicle industries |
Why is it difficult to extract titanium from its ores | Because reduction with carbon produces a brittle titanium carbide |
How is the production of titanium carbide avoided in the extraction of titanium from its ore | The titanium oxide ore is first reacted with chlorine and carbon to form titanium chloride |
What happens to the titanium chloride to produce titanium | It is reduced with magnesium to produce titanium |
What are group 2 hydroxides | Bases |
What do group 2 hydroxides react with | Acids |
Example of acid base reaction between magnesium hydroxide and hydrochloric acid | Mg(OH)2 + 2HCL > MgCl2 + 2H20 |
What is magnesium hydroxides solubility like and pH of the solution it makes | V sparingly soluble PH 8-9 |
What is calcium hydroxides solubility like and pH of the solution it makes | Not much better than magnesium pH 10-11 |
What is strontium hydroxides solubility like and pH of the solution it makes | Relatively soluble, pH 11-12 |
What is barium hydroxides solubility like and pH of the solution it makes | Pretty soluble, pH 12-14 |
What the trend in water solubility of group 2 hydroxides | Increases down the group |
What is the trend in pH of resultant solutions from reaction of group 2 hydroxides and acids | Increases down the group |
How are relative solubilities of group 2 hydroxides tested | Adding aqueous sodium hydroxide to the solutions of group 2 ions and observing the precipitate formed |
What indicates that magnesium hydroxide is sparingly soluble | The pH of the solution is slightly alkaline, indicating a small amount of hydroxide ions have dissolved- hence a thick white precipitate will be seen |
How is it indicated that barium hydroxide is more soluble than magnesium hydroxide | Very thin white PPT seen |
What is magnesium hydroxide used for | In medicine Milk of magnesium Indigestion medicine- neutralises stomach acid |
How is calcium hydroxide used | To neutralise acidic soil Obtained from limestone- cheap |
What is the trend in solubility of group 2 sulfates | Decreases down the group |
What are calcium and barium sulfates' solubility like | Calcium- sparingly soluble | Barium- insoluble |
How to test the relative solubility of group 2 sulfates | Add sulfuric acid/aqueous sodium sulfates to solutions of group 2 ions and observing the precipitates formed |
What is magnesium sulfate solubility and how would this be seen | Soluble- no precipitate |
What is barium sulfate solubility and how would this be seen | Insoluble so a thick white precipitate would be seen |
What can the solubilities of group 2 hydroxides and sulfates be used to test | The identity of group 2 ions in solution |
Uses of barium salts | Tests for sulfates |
Method for using barium salts to test for sulfates |
|
Interpretation for using barium salts to test for sulfates | White PPT? Sulfate ions present |
Equation for using barium salts to test for sulfates | BaCl2 + Na2SO4 > BaSO4 + 2NaCl |
Uses of barium sulfate | Medicine |
Barium meal | BaSO4- good at absorbing xrays- if ingested provides a good image of the digestive tract via X-ray images |
Why is using barium sulfate in medicine harmless despite it being toxic | Barium sulfate is insoluble so barium ions are not absorbed into the blood |
Uses of calcium compounds | CaO or CaCO3 can be used to remove sulfur dioxide from flue gas |
Equation of neutralisation of sulfur dioxide using calcium oxide | CaO + SO2 > CaSO3 |
Equation for reaction of calcium carbonate with so2 | CaCO3 + SO2 > CaSO3 + CO2 |