Periodicity Exam Question
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The reaction of barium with bromine is more vigorous than the reaction of calcium with bromine explain why (barium is further down group 2) ?
*Ba has a greater atomic radius than Ca *Nuclear attraction is less in Ba *Ionisation energy of Ba is less so it is easier to remove outer electron in Ba
Exam question model on a question on metallic simple molecule and ionic ?
• Magnesium(metallic ) • Structure: giant lattice • Metallic bonding • Delocalised electrons Bromine(simple molecule) • Structure: simple molecular • induced dipole dipole forces (London forces) • (Between) molecules DO NOT ALLOW (between) atoms Magnesium bromide(ionic ) • Structure: giant lattice • Ionic bonding • (Between) oppositely charged ions Comparison of bond strengths • Metallic and ionic bonds are stronger than London forces OR Metallic and Ionic bonds need more energy to break than London forces Conductivity • Magnesium: conducts due to delocalised electrons can move/mobile. IGNORE ‘Carry’ charge for movement • Magnesium bromide: In solid IONS cannot move; in solution IONS can move.
Explain why an element would be classified as a p block element?
Highest energy electrons are in a p orbital or p sub shell
Referring to the first 3 period which element has the highest first ionisation energy ?
Helium
Referring to the first 3 period which element reacts with water to form an acidic solution and which one firms a computer with fluorine that has octahedral molecules ?
Compound with fluorine - sulfur Acidic solution- fluorine
Reactivity of group 2 elements?
*atomic radius increases *nuclear attraction decreases *ionisation energy decreases so less energy needed to remove electrons
Explain the trend and effect on the reactivity of groups containing metal (1 and 2) - first ionisation energies ?
*first ionisation energies decreases down the groups *larger atomic radius (more shells ) *increased electron shielding *reactivity increases and less nuclear attraction
State how and explain why the attraction between nucleui and outermost electron in gaseous atoms varies across period 3 ?
*the attraction between nucleui and outermost electron increases *nuclear charge increases *same number if shells *atomic radius decreases
State and explain the trend in period 2 ?
*atomic radius decreases across the period *nuclear charge increases *same electron shielding *greater nuclear attraction
Give a reason why potassium is placed immediately after argon in the periodic table ?
Potassium have one more proton than argon
Why do successive ionisation energies increase with ionisation number ?
*radius decreases *attraction between electrons and nucleus increases
Explain how the first ionisation energies of magnesium and aluminium gives further details of electron structure? Mg - 738 Al - 578(less energy needed as p subshell is higher )
*Mg has outer electron in 3s sub shell *Al has outer electron in 3p sub shell *3p sub shell has higher energy than 3s sub-shell
Explain why nitrogen has a larger first ionisation energy than oxygen ?
N atoms have less repulsion between p orbital electrons than O atoms