Atomic mass is the weighted average mass of an atom of an element based on the relative abundance of its isotopes, measured in atomic mass units (amu). It reflects the mass of the nucleus and is crucial for understanding the chemical and physical properties of elements.

Atomic Mass

Atomic mass

weighted average mass

mass of an atom

Relative abundance refers to the proportion of a particular species within an ecological community, compared to the total number of individuals across all species in that community. It is a crucial metric for understanding biodiversity, community structure, and ecosystem health, providing insights into species dominance and ecological balance.

relative abundance

Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons, resulting in different atomic masses. These differences in neutron count can lead to variations in stability and radioactive properties, making isotopes useful in fields like medicine, archaeology, and nuclear energy.

isotopes

atomic mass units

mass of the nucleus

Chemical properties of elements

physical properties of elements

Understanding Atomic Mass: The Role of the Nucleus

Atomic Mass Explained: How Isotopes Affect Element Weight

Understanding Relative Atomic Mass in Chemistry

Understanding Relative Atomic Mass and Its Importance in Chemistry

Understanding Relative Atomic Mass: An Analogy with Apples

What is Atomic Mass? Understanding the Contribution of Neutrons

Exploring Atomic Mass: How Neutrons and Protons Contribute

Atomic Number and Mass

Decoding Atomic Mass

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