Which element is oxidized in the following reaction: cuo(s) + h2 (g) → cu(s) + h2o (l)

Start by determining the oxidation numbers of each element on both sides of the equation CuO(s) + H2 (g) → Cu(s) + H2O (l)

Let's start with the reactants.

In the compound CuO(s), the oxidation number of O is -2 and the oxidation number of Cu is +2. (Remember, oxygen's oxidation number is -2 unless it's in a peroxide)

In H2(g) the oxidation number of H is 0 because it is in its elemental form.

Now onto the products

The oxidation number of Cu(s) is 0 because it is in its elemental form

In H2O(l) the oxidation number of oxygen is -2, and the oxidation number of H is +1.

Now let's summarize the change in the oxidation numbers of each element.

Cu: started as +2 and became 0

O: started as -2 and became -2 (didn't change)

H: started as 0 and became +1

To determine which element was oxidized, we look at which element lost electrons, and thus became more positive. So, we can determine that H was oxidized in this reaction, because it started with the oxidation number 0 and became +1.

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Explanation:

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.

each chemical family is represented as a group or column on the periodic table. based on chemical properties, there are 6 types of chemical families. group 1 represents alkali metals, group 2 represents alkaline earth metals, groups 3 to 12 represent transition metals, groups 13 to 16 represent non-metals and other metals, group 17 represents halogens and group 18 represents noble gases.