When a small piece of copper metal is added to a silver nitrate solution, the following reaction occurs: 2Ag+NO3+Cu → Cu (NO3)2+2Ag

This equation both represents both a single replacement reaction AND a(n) reaction.

A. combustion
B. decomposing
C. neutralization
D. oxidation-reduction

Explanation:

Copper is more reactive than silver.

When copper reacts with AgNO3, Cu displaces Ag from AgNO3, forming Cu(NO3)2.

Chemical reaction -

It's a displacement reaction as well as redox reaction.

Reasons are :

The Oxidation number of Cu changes from 0 to 2 so it's oxidized.

Oxidation number of Ag changes from 1 to 0 so it's reduced.

So, it's also a redox reaction.

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.