Question

Explain each term as it applies to the element nitrogen. (a) atomic mass; (b) molecular mass; (c) molar mass.

Short answer

The summarized definitions and applications for the element nitrogen are: (a) Atomic mass is the mass of a single atom, for Nitrogen it's roughly 14.01 amu. (b) Molecular mass is the total mass of all atoms in a molecule, for Nitrogen molecule (\(N_2\)) it's around 28.02 amu. (c) Molar mass is the mass of one mole of a substance, for Nitrogen this value is approximately 28.02 g/mol.

Step-by-step solution

Define and Apply the Term 'Atomic Mass'

Atomic mass refers to the mass of a single atom of an element. It's usually expressed in atomic mass units (amu), where 1 amu is approximately equal to the mass of a single nucleon (a proton or a neutron). The atomic mass of nitrogen is approximately 14.01 amu.

Define and Apply the Term 'Molecular Mass'

Molecular mass is the sum of the atomic masses of all the atoms in a molecule. Nitrogen usually exists as a diatomic molecule (\(N_2\)). Therefore, the molecular mass of nitrogen is approximately \(2 \times 14.01\) amu = 28.02 amu.

Define and Apply the Term 'Molar Mass'

Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). The molar mass is numerically equal to the molecular mass, but expressed in different units. For nitrogen (\(N_2\)), the molar mass is approximately 28.02 g/mol.

Key concepts

Atomic Mass

Atomic mass is a fundamental concept in chemistry that refers to the mass of a single atom of a chemical element. This measurement is reported in atomic mass units (amu). Specifically, 1 amu is defined as one-twelfth of the mass of a carbon-12 atom, and this standard allows scientists to compare the mass of different atoms in a consistent manner.
When we consider nitrogen, its atomic mass is modestly around 14.01 amu. This value reflects the average mass of nitrogen atoms, accounting for its natural isotopic composition, mainly including isotopes like nitrogen-14.
Understanding atomic mass is essential as it helps in predicting how different atoms might combine. It sets the ground for further discussions on molecular and molar masses, especially in complex reactions and compound formations.

Molecular Mass

Molecular mass, sometimes called molecular weight, represents the collective mass of all the atoms forming a single molecule. It adds up the individual atomic masses of the atoms involved.
For nitrogen, which typically bonds as a diatomic molecule, represented by the formula \(N_2\), the molecular mass is calculated by summing the atomic masses of two nitrogen atoms: \(2 \times 14.01\, \text{amu} = 28.02\, \text{amu}\).
This notion is crucial because it allows us to understand the scale and magnitude of molecules, predicting their behaviors in chemical reactions. When molecules interact, their mass and proportion determine how they will change states, bond with other molecules, or break apart.
Highly helpful in lab environments, knowing the molecular mass guides chemists in measuring out precise amounts of chemicals, ensuring reactions occur as intended.

Molar Mass

The concept of molar mass plays a pivotal role in chemistry, conveying the mass of 6.022 x \(10^{23}\) entities (atoms, molecules, or other particles), known as one mole of a substance. Molar mass is given in grams per mole (g/mol), highlighting its practical utility in laboratory settings.
For the nitrogen molecule \(N_2\), its molar mass is equivalent to its molecular mass, however expressed in grams: \(28.02\, \text{g/mol}\).
Moles offer a bridge between the atomic world and the human scale, making it conceivable to weigh out substances easily in the lab.

• It simplifies calculations in chemical reactions, allowing one to predict how much product one will yield from a given reactant.
• It serves as a stepping-stone to convert between atoms/molecules and grams. Therefore, understanding molar mass is a vital skill for chemists and students alike, providing insight into both micro-level and measurable phenomena in the real world.