Consider that a sample of a compound is decomposed and the masses of its constituent elements is as follows: 1.443 g se, 0.5848 g o what would be the empirical formula for this compound?

The empirical formula is .

Explanation:

So, the mass of each element is given:

Mass of Se = 1.443 g

Mass of O = 0.5848 g

Step 1 : convert given masses into moles.

Moles of Se=

Moles of O =

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For Se =

For O =

The ratio of Se: O = 1: 2

Hence the empirical formula is .

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.