Chemistry - Elements, Isotopes & Relative Atomic Mass

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What are isotopes?

Q: What are isotopes?A: Isotopes are variants of the same chemical element that have the same number of protons but different numbers of neutrons. This results in different atomic masses. For example, carbon-12 and carbon-14 are isotopes of carbon.

What is the structure of an atom?

An atom has a central nucleus containing protons (positively charged) and neutrons (neutral), with electrons (negatively charged) orbiting in shells around it. The number of protons defines the element, and the electron arrangement affects chemical behavior.

What is the structure of an atom?

Q: What is the basic structure of an atom?A: An atom consists of a nucleus containing protons and neutrons, surrounded by electrons in orbitals.

How do you calculate relative atomic mass?

To calculate relative atomic mass, follow these steps:

1. Identify Isotopes: Determine the isotopes of the element and their respective abundances.

2. Find Atomic Masses: Obtain the atomic mass of each isotope (usually from a periodic table).

3. Calculate Weighted Average: Use the formula:

   [ \text{Relative Atomic Mass} = \frac{\sum (\text{isotope mass} \times \text{abundance})}{\sum \text{abundance}} ]

4. Express as a Decimal: Ensure the final value is expressed as a decimal.

This gives the average mass of an atom of the element relative to 1/12th the mass of carbon-12.

What are protons?

Protons are positively charged particles found in the nucleus of an atom.

What are neutrons?

Neutrons are neutral particles located in the nucleus of an atom.

What are electrons?

Electrons are negatively charged particles that orbit the nucleus of an atom