group 1 Flashcards
(22 cards)
What happens to size down group 1
Increases down group as electrons in shells further from the nucleus
What happens to reactivity down group 1?
Increases as ionisation energy decreases
What is the bonding like in group 1?
Metallic bonding, they aren’t very electronegative
What happens to basicity in group 1 hydroxides down the group?
Basicity increases down the group because increased metallic character (down group atoms aren’t as electronegative)
Are group 1 hydroxides Acidic or Basic?
Basic
What is the bonding between group 1 and the oxides?
strong Ionic lattice. smaller ions can get closer together and therefore have really strong bonds
Why do larger group 1 cations usually form superoxides and not stronger ionic lattices with smaller anions?
The ionic lattices with large ions are weaker and therefore it isn’t favourable for the peroxide to undergo an energy cost reaction into a smaller oxide.
N2 is a very stable gas, but it reacts with Li, none of the other group 1 metals do this, why?
Lithium can become such a small densely charged cation which can form a really strong ionic lattice making the energy cost of breaking the N2 bond favourable
Why does only Li react with N2 and not the other group 1 atoms?
They are too big, the ionic lattice would not be favourable and wouldn’t offset the energy used to break the N2 bond
Why is Li similar to Mg
The diagonal relationship, they both have very high charge density small cations
What bonding is in group 1 hydrides?
Ionic lattices as a big difference in electronegativity, group 1 electropositive
As metal ions get bigger down group one what happens to the ionic lattice?
Gets weaker as the ions are further apart from each other, therefor the thermal stability is also weaker.
What bonds are in the group 1 halides?
Ionic as big electronegativity difference. Strength is greatest between smallest ions
What is this O^2- called?
Oxide
What is O2^2- called?
Peroxide
what is O2- called?
Superoxide
Products of group 1 metals with oxygen are?
Basic
What structure does Na form with halides?
Rocksalt crystal structure
Why is solubility of group 1 halides complex?
There are two competing factors, hydration enthalpy and lattice enthalpy. As the halide ion gets bigger the dominant factor changes from lattice energy to hydration enthalpy.
For group 1 halides why does the dominant solubility factor shift from lattice energy to hydration enthalpy as the halide ion gets bigger?
As the ion gets bigger it cant overlap as well with the group 1 elements, therefore the lattice enthalpy isn’t as high. This weak lattice energy doesn’t change much with the cation size if anion is small so hydration becomes dominant factor
What happens to the solubility of group 1 halides if the anion is large?
Decreases down the group 1. As hydration enthalpy is the dominant factor over lattice enthalpy. Hydration E decreases as cation gets bigger it is less favourable to hydrate.
What happens to the solubility of group 1 halides if the anion is small?
Increases down group 1. Small anion means the lattice energy could be strong, as the cation gets bigger this energy rapidly decreases meaning it can get broken easier.
