Module 3: Periodic Table and Qualitative Analysis V2 Flashcards
Define the term first ionisation energy
The first ionisation energy is the energy needed to remove 1 mole of electrons ✓
from 1 mole of gaseous atoms ✓
to form 1 mole of gaseous 1+ ions ✓
Write an equation, with state symbols, to represent the first ionisation energy of Magnesium
Don’t forget that they are gaseous
Write an equation, with state symbols, to represent the fourth ionisation energy of sodium
Don’t forget that they are gaseous
Define what is meant by the “second ionisation energy”
The second ionisation is the energy needed to remove 1 electron from each ion ✓
in 1 mole of gaseous 1+ ions ✓
to form 1 mole of gaseous 2+ ions ✓
Explain why the first ionisation energy, is an endothermic process
Energy is required to overcome electrostatic attraction between positive nucleus and negative electron ✓
Describe and explain the trend in first ionisation energy going down the group
First ionisation energy decreases ✓
Number of shells increases, so shielding increases ✓
Atomic radius increases down the group ✓
Nuclear charge increases down the group, but is outweighed by increase in atomic radius and shielding ✓
Nuclear attraction for outer electron decreases, so electron more easily lost ✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron
Describe and explain the trend in first ionisation energy going across the period.
First ionisation energy increases ✓
Nuclear charge increases ✓
Shielding is similar, outermost electron is being removed from the same shell ✓
Atomic radius decreases. ✓
Greater nuclear attraction for outer electron ✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron
Explain why first ionisation energy decreases between groups 2 to 3 (Mg to Al)
Mg has outer electron in 3s sub-shell and Al has outer electron in 3p sub-shell ✓
3p sub-shell has higher energy than 3s sub-shell. ✓
There is a slight increase in shielding which outweighs the increase in nuclear charge. ✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron. It may be helpful to draw stuff out.
Explain why first ionisation energy decreases between groups 5 to 6 (P to S)
Shielding is identical in phosphorous and sulfur atoms and electron is being removed from 3p-subshell. ✓
In sulfur, the electron is easier to remove – lower ionisation energy. ✓
Orbital has 2 electrons – repulsion between the two electrons. ✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron. It may be helpful to draw stuff out.
Sketch a graph to show how ionisation energy changes across period 3.
Predict where you would expect lithium to be by adding an additional cross above Sodium.
Li would be much higher compared to the rest, as it has one less shell. Li is much greater in ionisation energy due to having less shielding and being closer to the nucleus.
Describe and explain the trend in successive ionisation energies
Increases as more electrons are removed. ✓
Electrons are removed from a more positive ion ✓
Attraction between remaining electrons and nucleus increases. Radius also decreases. ✓
more energy is needed to remove the next electron. ✓
Same number of protons, same nuclear charge attracting fewer electrons. ✓
The successive ionisation energies of element X is shown below. State and explain what group element X belongs to.
Group 5
Big jumps are caused when a new shell is broken into ✓
Electron removed from a shell closer to the nucleus ✓
Describe and explain the trend in reactivity going down the group for group 1 and 2 metals.
Increases down the group ✓
Number of shells increases, so shielding increases ✓
Atomic radius increases down the group ✓
Nuclear charge increases down the group, but is outweighed by increase in atomic radius and shielding ✓
Nuclear attraction for outer electron decreases, so less is energy is required to remove electrons✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron. It may be helpful to draw stuff out.
Write a balanced equation for the reaction of calcium with water and state what observations you would observe.
Fizzing ✓
Solid dissolves ✓
Write an equation for the reaction of Calcium with oxygen.
Write an equation to show how the product above can react with water to produce calcium hydroxide.
State and explain a use of calcium hydroxide
Used in agriculture ✓
to neutralise acidic soils ✓
State and explain a use of magnesium hydroxide and calcium carbonate
Antacids ✓
Neutralises excess stomach acid ✓
State and explain a use of barium sulfate
Barium meals ✓
barium sulfate is insoluble ✓
Describe and explain the trend in atomic radius going across the period.
Decreases across a period ✓
Number of protons / nuclear charge increases ✓
Outer electrons are in the same shell and have similar shielding ✓
Stronger nuclear attraction and electrons are drawn in more ✓
Remember, NANCARS: When talking about how easy it is to lose or gain an electron. It may be helpful to draw stuff out.
Describe and explain the trend in atomic radius going down the group
Increases down the group ✓
Number of shells increases ✓
Describe and explain the trend in melting and boiling points going down group 7
Increases down group 8 ✓
Number of electrons and atomic radius increases ✓
Strength of induced dipole-dipole interactions between atoms increases ✓
which require more energy to overcome ✓
Could use “London forces”
Sketch a graph to show how boiling points change across period 3
Explain why the melting points increases from sodium to aluminum.
Number of delocalised electrons increases ✓
Charge on positive ion increases ✓
Metallic bonding, electrostatic attraction between the positive metal ion and delocalised electrons, gets stronger ✓
Explain why the conductivity increases in period 3, from Na to Al.
Number of delocalised electrons increases ✓