Chemistry group 2

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  • Created by: I.m
  • Created on: 24-12-12 23:43
State the observations made when magnesium ribbon is burned.
Bright white light and white solid formed.
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What is formed when group 2 metals react with oxygen and give a general formula for this product?
Group 2 elements react with oxygen to form oxides whose general formula can be written as MO (M being the group 2 metal).
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Give the general equation for the reaction between a group 2 metal and oxygen. Include state symbols.
2M (s) + O₂ (g) = 2MO (s)
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Write the balanced equation, including state symbols, for the reaction of magnesium with oxygen.
2Mg (s) + O₂ (g) = 2MgO (s)
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The equation for the reaction between magnesium and oxygen is 2Mg (s) + O₂ (g) = 2MgO (s). State the oxidation state of each reactant/product.
Mg(s) = 0, O₂(g) =0, Mg in MgO(s) = +2 and O in MgO(s) = +2.
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The equation for the reaction between magnesium and oxygen is 2Mg (s) + O₂ (g) = 2MgO (s). State what has been oxidised and reduced in this reaction.
Mg has been oxidised because it has lost 2 electrons (0---+2). Oxygen has been reduced because it has gained 2 electrons (0--- -2).
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State the observations made when magnesium reacts with water.
No observation/change at the start. Little effervescence - bubbles
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State the observations made when calcium reacts with water.
Effervescence and white precipitate formed.
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Which reaction is fastest when magnesium and calcium both react with water?
Calcium reaction with water is fastest.
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Explain the general trend in reactivity down group 2 elements with water in terms of ionisation energies.
Reactivity incrs dwn group2.This is bec metals lose e-s whn they react.Going dwn the group,outer e-s r frther frm nuc.Thre is mre shielding so attraction btwn nucl+outer e-s dcrs.Thfre les enrgy needed to remve outer e-s so reactions become faster
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What products are produced when group 2 elements react with water and give a general formula for this product?
Group 2 elements react with water to form hydroxides whose general formula can be written as M(OH)₂ (M being the group 2 metal). Hydrogen gas is also produced.
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Give the general equation for the reaction between a group 2 metal and water. Include state symbols.
M (s) +2 H₂0 (l) = M(OH)₂ (aq) + H₂ (g)
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How soluble are the metal hydroxides in water?
The metal hydroxides are only slightly soluble in water.
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Write a balanced equation for the reaction of calcium with water. Include state symbols.
Ca (s) + 2H₂O (l) = Ca(OH)₂ (aq) +H₂ (g)
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The equation for the reaction between calcium and water is Ca (s) + 2H₂O (l) = Ca(OH)₂ (aq) +H₂ (g). State the oxidation state of each reactant/product.
Ca (s) = 0, H in H₂O(l) = +1, O in H₂O(l) = -2, H in H₂(g) = 0, Ca in Ca(OH)₂ (s) = +2, H in Ca(OH)₂ (s) = +1 and O IN Ca(OH)₂ (s) = -2
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The equation for the reaction between calcium and water is Ca (s) + 2H₂O (l) = Ca(OH)₂ (aq) +H₂ (g). State what has been oxidised and reduced in this reaction.
Ca has been oxidised because it has lost 2 electrons (0---+2). H has been reduced because it has gained 1 electron (+1-----0)
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What is the general formula given to group 2 metal carbonates?
MCO₃ (M being the group2 metal).
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What two products are formed when a group 2 metal carbonate decomposes by heat?
Group 2 metal carbonate are decomposed to for the metal oxide MO and carbon dioxide gas CO₂.
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Give the general equation of the decomposition of group 2 metals. Include state symbols.
MCO₃ (s) = MO (s) + CO₂ (g).
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Describe the trend in decomposition down group 2.
The carbonate become more difficult to decompose on heating as you go down the group. MgCO₃ is easiest to decompose/ decomposes at the lowest temperature/least thermally stable. BaCO₃ is most diffiuclt to decompose/decomposes at highest temp/ most th
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What observations are made when CaCO₃ is decomposed?
CaCO₃ chip is glowing. The chalk crumbles slightly.
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Write the balanced equation for the thermal decomposition of CaCO₃. Include state symbols.
CaCO₃ (s) = CaO (s) +CO₂(g)
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What if anything is oxidised when CaCO₃ decomposes.
Nothing has been decomposed as this is not a redox reaction. It is thermal decomposition.
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What product is formed when group 2 metal oxides react with water?
An aqueous solution og the metal hydroxide is formed.
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Give the general equation of the reaction of group 2 metal oxides and water. Include state symbols.
MO (s) + H₂O (l) = M(OH)₂ (aq).
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What observations are made when universal indicator is added to CaO (from the thermal decomposition of CaCO₃) and what is it pH and what does this indicate?
It turns blue and has an approximate pH of 9/10 so it is weakly alkali.
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Write the balanced equation for when calcium oxide reacts with water. Include state symbols.
CaO (s) + H₂O (l) = Ca(OH)₂ (aq).
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What is a solution of Ca(OH)₂ in water called?
A solution of Ca(OH)₂ in water is called lime water Ca(OH)₂ (aq).
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Write the balanced equation for when you add carbon dioxide to calcium hydroxide?
Ca(OH)₂ + CO₂ = CaCO₃.+ H₂O
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What are the uses of Ca(OH)₂? Give a reason for your answer.
Ca(OH)₂ is use by famers as ‘lime’ to neutralise acidic soil. It is used to reduce soil acidity and restore pH balances to soils.
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What is a common name given to Mg(OH)₂?
Milk of magnesia.
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What are the uses of Mg(OH)₂? Give a reason for your answer.
It is used to relieve indigestion in tablets e.g. antacid. It works by neutralising any excess stomach acid in the stomach.
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What is the ionic equation for neutralisation?
H+ (aq) + OH- (aq) = H₂O (l).
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Other cards in this set

Card 2

Front

What is formed when group 2 metals react with oxygen and give a general formula for this product?

Back

Group 2 elements react with oxygen to form oxides whose general formula can be written as MO (M being the group 2 metal).

Card 3

Front

Give the general equation for the reaction between a group 2 metal and oxygen. Include state symbols.

Back

Preview of the front of card 3

Card 4

Front

Write the balanced equation, including state symbols, for the reaction of magnesium with oxygen.

Back

Preview of the front of card 4

Card 5

Front

The equation for the reaction between magnesium and oxygen is 2Mg (s) + O₂ (g) = 2MgO (s). State the oxidation state of each reactant/product.

Back

Preview of the front of card 5
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