Calculate the number of atoms in a 1.94 x 10^3 g sample of calcium

1.94 *10^3 grams calcium contains 2.9*10^25 calcium atoms

Explanation:

Step 1: Data given

Mass of Calcium = 1.94 *10³ grams = 1940 grams

Molar mass of Calcium = 40.08 g/mol

Number of Avogadro = 6.022 * 10^23 / mol

Step 2: Calculate moles of Calcium

Moles Calcium = mass calcium / molar mass Calcium

Moles Calcium = 1940 grams / 40.08 g/mol

Moles Calcium = 48.40 moles

Step 3: Calculate number of atoms

Number of Calcium atoms = moles calcium * Number of Avogadro

Number of Calcium atoms = 48.40 moles * 6.022 *10^23 / mol

Number of Calcium atoms = 2.9 *10^25 atoms

1.94 *10^3 grams calcium contains 2.9*10^25 calcium atoms

i have know clue i guess aluminum

i think lol

the electronic configuration of an atom with eight electrons is 1s²2s²2p⁴. the orbital diagrams are shown in the figure.

as per the hunds rule:

1. electrons tend to avoid being in the same orbital as per as practicable.

2. electrons in different orbitals of the same energy will have their spin parallel.

this can be illustrated from the multiplicity of the orbitals of the atom. as there are four electrons in the p orbital and p orbital has 3 sub-shells. the electrons can be fed in different ways as shown in the figure but the correct orbital diagram will be as per the hunds rule.