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Questions and Answers
What are the alkali metals collectively known as?
What are the alkali metals collectively known as?
Alkali metals
What are the alkaline earth metals commonly known as?
What are the alkaline earth metals commonly known as?
Alkaline earth metals
Which of the following are true about the alkali metals? (Select all that apply)
Which of the following are true about the alkali metals? (Select all that apply)
- They are all highly reactive. (correct)
- They are all silvery white, soft and light metals. (correct)
- They all form hydroxides on reaction with water. (correct)
What is the general electronic configuration of s-block elements for alkali metals?
What is the general electronic configuration of s-block elements for alkali metals?
What is the general electronic configuration of s-block elements for alkaline earth metals?
What is the general electronic configuration of s-block elements for alkaline earth metals?
Why are lithium and beryllium anomalous compared to the other alkali and alkaline earth metals?
Why are lithium and beryllium anomalous compared to the other alkali and alkaline earth metals?
The ionization enthalpy of alkali metals increases as you move down the group from Lithium to Caesium.
The ionization enthalpy of alkali metals increases as you move down the group from Lithium to Caesium.
The hydration enthalpy of alkali metal ions increases as you move down the group from Lithium to Caesium.
The hydration enthalpy of alkali metal ions increases as you move down the group from Lithium to Caesium.
What color does lithium impart to a flame?
What color does lithium impart to a flame?
Lithium has the most negative Eº value among all the alkali metals.
Lithium has the most negative Eº value among all the alkali metals.
Lithium's reaction with water is more vigorous than sodium, which has the least negative Eº value.
Lithium's reaction with water is more vigorous than sodium, which has the least negative Eº value.
LiCl is deliquescent and crystallises as a hydrate LiCl.2H₂O whereas other alkali metal chlorides do not form hydrates.
LiCl is deliquescent and crystallises as a hydrate LiCl.2H₂O whereas other alkali metal chlorides do not form hydrates.
Lithium hydrogencarbonate cannot be obtained in the solid form while all other alkali metals form solid hydrogencarbonates.
Lithium hydrogencarbonate cannot be obtained in the solid form while all other alkali metals form solid hydrogencarbonates.
Lithium nitrate when heated gives lithium oxide, Li₂O, whereas other alkali metal nitrates decompose to give the corresponding nitrite.
Lithium nitrate when heated gives lithium oxide, Li₂O, whereas other alkali metal nitrates decompose to give the corresponding nitrite.
LiF and Li₂O are more soluble in water than the corresponding compounds of other alkali metals.
LiF and Li₂O are more soluble in water than the corresponding compounds of other alkali metals.
Both lithium and magnesium are harder and lighter than other elements in the respective groups.
Both lithium and magnesium are harder and lighter than other elements in the respective groups.
The oxides and hydroxides of lithium and magnesium are much less soluble in water and decompose on heating.
The oxides and hydroxides of lithium and magnesium are much less soluble in water and decompose on heating.
The hydroxides of lithium and magnesium are amphoteric.
The hydroxides of lithium and magnesium are amphoteric.
Beryllium and magnesium are kinetically inert to oxygen and water because they are not reactive.
Beryllium and magnesium are kinetically inert to oxygen and water because they are not reactive.
Beryllium is more electropositive than magnesium.
Beryllium is more electropositive than magnesium.
The reactivity of alkaline earth metals towards the halogens increases as you move down the group.
The reactivity of alkaline earth metals towards the halogens increases as you move down the group.
All alkaline earth metals combine with hydrogen upon heating to form their hydrides.
All alkaline earth metals combine with hydrogen upon heating to form their hydrides.
Beryllium hydroxide is amphoteric.
Beryllium hydroxide is amphoteric.
Beryllium halides are ionic in nature.
Beryllium halides are ionic in nature.
The fluorides of alkaline earth metals are more soluble than the chlorides.
The fluorides of alkaline earth metals are more soluble than the chlorides.
The carbonates of alkaline earth metals are insoluble in water.
The carbonates of alkaline earth metals are insoluble in water.
The sulphates of alkaline earth metals are all white solids and stable to heat.
The sulphates of alkaline earth metals are all white solids and stable to heat.
The nitrates of alkaline earth metals are soluble in water.
The nitrates of alkaline earth metals are soluble in water.
The atomic radii of alkaline earth metals are smaller than the atomic radii of the corresponding alkali metals.
The atomic radii of alkaline earth metals are smaller than the atomic radii of the corresponding alkali metals.
The ionization enthalpies of alkaline earth metals are higher than the ionization enthalpies of the corresponding alkali metals.
The ionization enthalpies of alkaline earth metals are higher than the ionization enthalpies of the corresponding alkali metals.
The second ionization enthalpies of the alkaline earth metals are higher than the second ionization enthalpies of the corresponding alkali metals.
The second ionization enthalpies of the alkaline earth metals are higher than the second ionization enthalpies of the corresponding alkali metals.
The hydration enthalpy of alkaline earth metal ions decreases as you move down the group from Beryllium to Barium.
The hydration enthalpy of alkaline earth metal ions decreases as you move down the group from Beryllium to Barium.
The alkaline earth metals are all silvery white, lustrous, and soft.
The alkaline earth metals are all silvery white, lustrous, and soft.
The melting and boiling points of the alkaline earth metals are lower than the corresponding alkali metals.
The melting and boiling points of the alkaline earth metals are lower than the corresponding alkali metals.
The oxide and hydroxide of beryllium are amphoteric, unlike the hydroxides of other elements in the group.
The oxide and hydroxide of beryllium are amphoteric, unlike the hydroxides of other elements in the group.
The ionic radius of Be²⁺ is estimated to be 31 pm; the charge/radius ratio is nearly the same as that of the Al³⁺ ion.
The ionic radius of Be²⁺ is estimated to be 31 pm; the charge/radius ratio is nearly the same as that of the Al³⁺ ion.
Beryllium hydroxide dissolves in excess of alkali to give a beryllate ion, [Be(OH)4]² just as aluminium hydroxide gives aluminate ion, [Al(OH)4]²⁻.
Beryllium hydroxide dissolves in excess of alkali to give a beryllate ion, [Be(OH)4]² just as aluminium hydroxide gives aluminate ion, [Al(OH)4]²⁻.
The chlorides of both beryllium and aluminium have Cl bridged chloride structure in vapour phase.
The chlorides of both beryllium and aluminium have Cl bridged chloride structure in vapour phase.
Beryllium and aluminium have a strong tendency to form complexes, BeF₂²⁻, AlF₃³⁻.
Beryllium and aluminium have a strong tendency to form complexes, BeF₂²⁻, AlF₃³⁻.
Calcium oxide is manufactured by heating limestone (CaCO3) in a rotary kiln at 1070-1270 K.
Calcium oxide is manufactured by heating limestone (CaCO3) in a rotary kiln at 1070-1270 K.
Calcium oxide is a white amorphous solid with a melting point of 2870 K.
Calcium oxide is a white amorphous solid with a melting point of 2870 K.
Calcium hydroxide is prepared by adding water to quick lime, CaO.
Calcium hydroxide is prepared by adding water to quick lime, CaO.
The aqueous solution of calcium hydroxide is known as lime water.
The aqueous solution of calcium hydroxide is known as lime water.
The suspension of slaked lime in water known as milk of lime will turn milky when carbon dioxide is passed through it.
The suspension of slaked lime in water known as milk of lime will turn milky when carbon dioxide is passed through it.
Calcium carbonate is a white fluffy powder and is almost insoluble in water.
Calcium carbonate is a white fluffy powder and is almost insoluble in water.
Calcium oxide is an important primary material for manufacturing cement and is the cheapest form of alkali.
Calcium oxide is an important primary material for manufacturing cement and is the cheapest form of alkali.
Calcium oxide is used in the manufacture of sodium carbonate from caustic soda.
Calcium oxide is used in the manufacture of sodium carbonate from caustic soda.
Calcium oxide is employed in the purification of sugar and in the manufacture of dye stuffs.
Calcium oxide is employed in the purification of sugar and in the manufacture of dye stuffs.
Calcium hydroxide is used in the preparation of mortar, a building material.
Calcium hydroxide is used in the preparation of mortar, a building material.
Calcium hydroxide is used in white wash due to its disinfectant nature.
Calcium hydroxide is used in white wash due to its disinfectant nature.
Calcium hydroxide is used in glass making, in tanning industry, for the preparation of bleaching powder and for purification of sugar.
Calcium hydroxide is used in glass making, in tanning industry, for the preparation of bleaching powder and for purification of sugar.
When heated to 1200 K, Calcium carbonate decomposes to evolve carbon dioxide.
When heated to 1200 K, Calcium carbonate decomposes to evolve carbon dioxide.
Calcium carbonate is used in the manufacture of quick lime, marble and as a building material in the form of marble.
Calcium carbonate is used in the manufacture of quick lime, marble and as a building material in the form of marble.
Plaster of Paris (CaSO4⋅1/2 H2O), is obtained when gypsum (CaSO4⋅2H2O), is heated at 393 K.
Plaster of Paris (CaSO4⋅1/2 H2O), is obtained when gypsum (CaSO4⋅2H2O), is heated at 393 K.
The largest use of Plaster of Paris is in the building industry as well as plasters.
The largest use of Plaster of Paris is in the building industry as well as plasters.
Cement is referred to as Portland cement because it resembles the limestone quarried in the Isle of Portland, England.
Cement is referred to as Portland cement because it resembles the limestone quarried in the Isle of Portland, England.
When clay and lime are strongly heated together they fuse and react to form 'cement clinker'.
When clay and lime are strongly heated together they fuse and react to form 'cement clinker'.
When mixed with water, the setting of cement takes place to give a hard mass due to the hydration of the molecules of the constituents and their rearrangement.
When mixed with water, the setting of cement takes place to give a hard mass due to the hydration of the molecules of the constituents and their rearrangement.
An adult body contains about 25 g of Mg and 1200 g of Ca compared with only 5 g of iron and 0.06 g of copper.
An adult body contains about 25 g of Mg and 1200 g of Ca compared with only 5 g of iron and 0.06 g of copper.
The main pigment for the absorption of light in plants is chlorophyll which contains magnesium.
The main pigment for the absorption of light in plants is chlorophyll which contains magnesium.
The calcium concentration in plasma is regulated at about 100 mgL-¹ by the hormones, calcitonin and parathyroid hormone.
The calcium concentration in plasma is regulated at about 100 mgL-¹ by the hormones, calcitonin and parathyroid hormone.
A typical 70 kg man contains about 90 g of Na and 170 g of K compared with only 5 g of iron and 0.06 g of copper.
A typical 70 kg man contains about 90 g of Na and 170 g of K compared with only 5 g of iron and 0.06 g of copper.
Sodium ions are located primarily on the outside of cells, being located in blood plasma and in the interstitial fluid which surrounds the cells.
Sodium ions are located primarily on the outside of cells, being located in blood plasma and in the interstitial fluid which surrounds the cells.
Sodium and potassium are similar chemically but differ quantitatively in their ability to penetrate cell membranes, in their transport mechanisms and in their efficiency to activate enzymes.
Sodium and potassium are similar chemically but differ quantitatively in their ability to penetrate cell membranes, in their transport mechanisms and in their efficiency to activate enzymes.
There is very considerable variation in the concentration of sodium and potassium ions found on the opposite sides of cell membranes.
There is very considerable variation in the concentration of sodium and potassium ions found on the opposite sides of cell membranes.
Flashcards
s-block elements definition
s-block elements definition
Elements where the last electron enters the outermost s-orbital
Alkali metals group
Alkali metals group
Group 1 elements: Lithium, Sodium, Potassium, Rubidium, Caesium, Francium
Alkaline Earth metals group
Alkaline Earth metals group
Group 2 elements: Beryllium, Magnesium, Calcium, Strontium, Barium, Radium
General electronic configuration of alkali metals
General electronic configuration of alkali metals
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General electronic configuration of alkaline earth metals
General electronic configuration of alkaline earth metals
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Diagonal relationship definition
Diagonal relationship definition
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Diagonal relationship example
Diagonal relationship example
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Atomic radii trend in alkali metals
Atomic radii trend in alkali metals
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Ionization enthalpy trend in alkali metals
Ionization enthalpy trend in alkali metals
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Hydration enthalpy trend in alkali metals
Hydration enthalpy trend in alkali metals
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Flame test for alkali metals
Flame test for alkali metals
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Reactivity of alkali metals trend
Reactivity of alkali metals trend
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Reactivity of alkali metals towards air
Reactivity of alkali metals towards air
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Reactivity of alkali metals towards water
Reactivity of alkali metals towards water
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Sodium carbonate formula (washing soda)
Sodium carbonate formula (washing soda)
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Solvay process
Solvay process
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Sodium chloride uses
Sodium chloride uses
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Sodium hydroxide (caustic soda) manufacturing
Sodium hydroxide (caustic soda) manufacturing
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Biological importance of sodium
Biological importance of sodium
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Biological importance of potassium
Biological importance of potassium
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Study Notes
Alkali Metals
- Collectively known as alkali metals
- General electronic configuration: ns¹
- Lithium is anomalous due to its small size and high ionization enthalpy
- Lithium has the most negative Eº value among all alkali metals
- Lithium's reaction with water is less vigorous than sodium
- LiCl is deliquescent and crystallizes as a hydrate LiCl.2H₂O
- Lithium hydrogencarbonate cannot be obtained in solid form
- Lithium nitrate when heated gives lithium oxide, Li₂O, while other alkali metal nitrates decompose to give their corresponding nitrite
- LiF and Li₂O are more soluble in water than the corresponding compounds of other alkali metals
- Both lithium and magnesium are harder and lighter than other elements in their respective groups
- The oxides and hydroxides of lithium and magnesium are less soluble in water and decompose on heating
- The hydroxides of lithium and magnesium are amphoteric
Alkaline Earth Metals
- Commonly known as alkaline earth metals
- General electronic configuration: ns²
- Beryllium is anomalous due to its small size, high ionization enthalpy, and high polarizing power
- The reactivity of alkaline earth metals towards halogens increases down the group
- All alkaline earth metals combine with hydrogen upon heating to form their hydrides
- Beryllium hydroxide is amphoteric
- Beryllium halides are ionic in nature
- The fluorides of alkaline earth metals are more soluble than the chlorides
- The carbonates of alkaline earth metals are insoluble in water
- The sulphates of alkaline earth metals are white solids and stable to heat
- The nitrates of alkaline earth metals are soluble in water
- The atomic radii of alkaline earth metals are smaller than the atomic radii of their corresponding alkali metals
- The ionization enthalpies of alkaline earth metals are higher than the ionization enthalpies of their corresponding alkali metals
- The second ionization enthalpies of alkaline earth metals are higher than their corresponding alkali metals
- The hydration enthalpy of alkaline earth metal ions decreases down the group from Beryllium to Barium
- Alkaline earth metals are silvery white, lustrous, and soft
- The melting and boiling points of alkaline earth metals are lower than those of their corresponding alkali metals
- The oxide and hydroxide of beryllium are amphoteric, unlike the hydroxides of other elements in the group
- The ionic radius of Be²⁺ is estimated to be 31 pm; the charge/radius ratio is nearly the same as that of the Al³⁺ ion
- Beryllium hydroxide dissolves in excess of alkali to give a beryllate ion, [Be(OH)4]²⁻, just as aluminium hydroxide gives aluminate ion, [Al(OH)4]²⁻
- The chlorides of both beryllium and aluminium have Cl bridged chloride structure in the vapour phase
- Beryllium and aluminium have a strong tendency to form complexes, BeF₂²⁻, AlF₃³⁻
Calcium
- Calcium oxide is manufactured by heating limestone (CaCO3) in a rotary kiln at 1070-1270 K.
- Calcium oxide is a white amorphous solid with a melting point of 2870 K.
- Calcium hydroxide is prepared by adding water to quick lime, CaO.
- The aqueous solution of calcium hydroxide is known as lime water.
- The suspension of slaked lime in water known as milk of lime will turn milky when carbon dioxide is passed through it.
- Calcium carbonate is a white fluffy powder and is almost insoluble in water.
- Calcium oxide is an important primary material for manufacturing cement, and is the cheapest form of alkali.
- Calcium oxide is used in the manufacture of sodium carbonate from caustic soda.
- Calcium oxide is employed in the purification of sugar and in the manufacture of dye stuffs.
- Calcium hydroxide is used in the preparation of mortar, a building material.
- Calcium hydroxide is used in white wash due to its disinfectant nature.
- Calcium hydroxide is used in glass making, in tanning industry, for the preparation of bleaching powder and for purification of sugar.
- When heated to 1200 K, Calcium carbonate decomposes to evolve carbon dioxide.
- Calcium carbonate is used in the manufacture of quick lime, marble and as a building material in the form of marble.
Plaster of Paris
- Plaster of Paris (CaSO4⋅1/2 H2O), is obtained when gypsum (CaSO4⋅2H2O), is heated at 393 K.
- The largest use of Plaster of Paris is in the building industry as well as plasters.
Cement
- Cement is referred to as Portland cement because it resembles the limestone quarried in the Isle of Portland, England.
- When clay and lime are strongly heated together they fuse and react to form 'cement clinker'.
- When mixed with water, the setting of cement takes place to give a hard mass due to the hydration of the molecules of the constituents and their rearrangement.
Magnesium
- An adult body contains about 25 g of Mg and 1200 g of Ca compared with only 5 g of iron and 0.06 g of copper.
- The main pigment for the absorption of light in plants is chlorophyll which contains magnesium.
Calcium
- The calcium concentration in plasma is regulated at about 100 mgL-¹ by the hormones, calcitonin and parathyroid hormone.
Sodium and Potassium
- A typical 70 kg man contains about 90 g of Na and 170 g of K compared with only 5 g of iron and 0.06 g of copper.
- Sodium ions are located primarily on the outside of cells, being located in blood plasma and in the interstitial fluid which surrounds the cells.
- Sodium and potassium are similar chemically but differ quantitatively in their ability to penetrate cell membranes, in their transport mechanisms and in their efficiency to activate enzymes.
- There is considerable variation in the concentration of sodium and potassium ions found on the opposite sides of cell membranes.
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