Protons are the representative particles of elements, ionic compounds, and covalent compounds.

Ionic compounds are compounds composed of ions, charged particles that form when an atom (or group of atoms) gains or loses electrons. (A cation is a positively charged ion; an anion is a negatively charged ion.) Covalent or molecular compounds form when elements share electrons in a covalent bond to form molecules.

A representative particle is the smallest unit in which a substance naturally exists. For the majority of elements, the representative particle is the atom. Iron, carbon, and helium consist of iron atoms, carbon atoms, and helium atoms, respectively.

Representative Particle: The smallest part of a substance that retains the properties of the substance. For a molecular compound (H2O), a representative particle is a molecule. For an ionic compound (Na2SO4), a representative particle is a formula unit.

The types of representative particles that chemists generally work with are:

• atoms – the smallest particle of an element.
• ions – atoms with positive or negative charges.
• molecules – two or more covalently bonded atoms.
• formula units – the simplest ratio of ions that make up an ionic compound.

Amedeo Avogadro

The answer is because in chemical reactions there is a conservation of moles, rather than mass. Moles are the total amount of molecules in the system, those remain constant. Naturally using numbers like 6.022×1023 is inconvenient, so moles help with keeping track.

One mole of a substance is equal to 6.022 × 10²³ units of that substance (such as atoms, molecules, or ions). The number 6.022 × 10²³ is known as Avogadro’s number or Avogadro’s constant. The concept of the mole can be used to convert between mass and number of particles.. Created by Sal Khan.

15.998 grams

Avogadro’s number is the number of representative particles in 1 mole. The mass of 6.02 x 10^23 particles of a representative of a substance is the molar mass of the substance. Compare the number of particles and the mass of 1 mole of each.

Because 1 mole = 6.02 x 10 23 atoms and the molar mass of an element is equal to one mole, the mass of a single atom can be calculated by dividing the mass of one mole by Avogadro’s number.

If we have 2 mol of Na atoms, we have 2 × (6.022 × 10 23) Na atoms, or 1

3.77 moles of Fe contain 2.27×1024 atoms Fe .

Avogadro’s Number and the Mole. The mole is represented by Avogadro’s number, which is 6.022×1023 atoms or molecules per mol.

Converting to moles is fairly easy because the conversion is always the same. A mole is 6.022 × 1023 of something, and this number is referred to as Avogadro’s number. In chemistry, this is: # of moles × Avogadro’s number = # of atoms or molecules.

The mole is thus the link between the micro world of atoms, and molecules, to the macro world of grams and litres. 2.5⋅mol×6.022×1023⋅mol−1=15.06×1024⋅nickel atoms .

Since an atom has a finite number of protons and neutrons, it will generally emit particles until it gets to a point where its half-life is so long, it is effectively stable. It undergoes something known as “alpha decay,” and it’s half-life is over a billion times longer than the current estimated age of the universe.

the amount of molecules of carbon dioxide which is found in 5 moles of carbon dioxide and determined by the avogadro’s law. Explanation: 1 mole of carbon dioxide consist of 6.023 x10^23 molecules. Hence 5 mole of carbon dioxide consists of 3.01 x10^24 molecules.

0.5 mole CO2=0. 5×44=22 gm.

There are 4.2×1024 4.2 × 10 24 molecules in 7 moles of CO2 .

Let’s consider the carbon dioxide molecule. We know it has the formula CO2, and this tells us that: 1 mole carbon dioxide contains 6.02 x 1023 molecules.

Thus, if we have 1 mole of a molecule present, we have 6.022*10^23 of those molecules present. If we have 2 moles of a molecule present, we have 2*1.022*10^23 of that molecule present etc.