EL8:1 Spectacular Metals Flashcards
What are the most reactive metals in the periodic table?
Group 1 and 2.
What are group 1 metals called?
Alkali metals.
What are group 2 metals called?
The alkaline earth metals.
What happens as you go down groups in the periodic table?
Elements get more metallic and therefore get more reactive.
What happens as you go across a periods in the periodic table?
Elements become less metallic.
What block are groups 1 and 2 in?
The s block.
What do s block metals tend to be like?
Soft, weak metals with low boiling points but very reactive with water and oxygen.
Why don’t metals in elemental form in groups 1 and 2 have many uses?
They are too reactive.
What compounds are common and useful?
S block compounds.
What is similar within groups in the periodic table?
Electron arrangements in their atoms.
What is the cause of differences between groups in the periodic table?
The size of the atom, it increases down the group.
What happens if sufficient energy is given to an atom (in group 1 and 2)?
An electron is lost and the atom becomes a positive ion.
What is needed to remove electrons and why?
Energy, because the electrons are attracted to the nucleus.
What is the first ionisation enthalpy of an element?
The energy needed to remove one electron from every atom in one mole of isolated gaseous atoms forming one mole of gaseous ions.
What is the general equation for first ionisation enthalpy?
X(g)-X^+(g)+e^-
What is the first ionisation enthalpy equation for oxygen?
O(g)-0^+(g)+e^-
What is the first ionisation enthalpy for oxygen?
+1320 kJ/mol
What electron does the first ionisation enthalpy remove and why?
One of the outer shell electrons, they are the most loosely held.
What do group 0 have?
High first ionisation enthalpies.
What does it mean if groups have a high first ionisation enthalpy?
They are hard to ionise.
Why are group 0 elements hard to ionise?
They have full outer shells.
What does it mean if groups have a low first ionisation enthalpy?
They are easy to ionise.
What do group 1 have?
A low first ionisation enthalpy.
Why are group 1 elements easy to ionise?
They have one electron in their outer shell.
What are the peaks and troughs in a first ionisation enthalpy graph and why?
Peaks are group 0 as they are hard to ionise and troughs are group 1 as they are easily ionised.
What is the electron shield theory?
Electron shielding from the nucleus increases as the number of shells increase, so less energy is needed to remove an outer shell electron.
Why does it become harder to remove an outer shell electron as you go across the period?
The number of protons increases so nuclear charge increases.
What causes variation of first ionisation enthalpy across periods?
The different energies and paired repulsions in sub-shells.
What happens to the first ionisation enthalpies as you go down a group and why?
They decrease as the attraction between the nucleus and outer electrons decreases.
What do group 1 and 2 metals first ionisation enthalpy correspond to?
It’s reactivity.
What factors effect ionisation energy?
The size of the nuclear charge, the distance of the outer electrons to the nucleus, and the shielding effect on inner electrons.
Why is it easier to remove an electron from a p-subshell than a s-subshell?
The p-subshell is further away from the nucleus and the s-subshell is shielding the electron so there is less attraction.
Why is it easier to remove an electron from group 6 than group 5?
The p orbital starts to double fill in group 6 so there is a repulsion making it easier to remove the electron.
What are the second, third, fourth and so on ionisation enthalpies?
The energy required to remove further electrons.
What is the general equation for second ionisation enthalpy?
X^+(g)-X^2+(g)+e^-
