Part 1: name the type of chemical reaction that occurs when aluminum (al) reacts with copper nitrate (cu(no3)2).
part 2: explain why aluminum does not react with potassium nitrate (kno3) although it reacts with copper nitrate.

Part 1: Single displacement or redox

Part 2: Al is above Cu but below K in the activity series

Explanation:

Part 1

2Al + 3Cu(NO₃)₂ ⟶ 3Cu + 2Al(NO₃)₃

(a) You could call this a single displacement reaction, because aluminium is displacing copper from its salt.

(b) You could also call this a reduction-oxidation reaction, because Al is oxidized to Al³⁺ and Cu²⁺ is reduced to Cu.

Part 2

Al reacts with Cu(NO₃)₂ because Al is above Cu in the activity series.

Al does not react with KNO₃ because Al is below K in the activity series.

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.

there are two significant figures.