Atomic Definitions

• Electrons are negatively charged particles that orbit around the nucleus of an atom.
• Isotopes are atoms with different numbers of neutrons but the same number of protons.
• Atoms are neutral, meaning they have an equal number of positive charges (protons) and negative charges (electrons).
• The number of protons is equal to the atomic number.
• The number of electrons is equal to the atomic number, which determines the chemical properties of an element.
• Neutrons do not carry any electrical charge (0).
• Protons have a positive charge (+1) and are located in the nucleus of an atom.
• The atomic mass is calculated by adding up the masses of all the protons, electrons, and neutrons in an atom.
• Atoms can gain or lose electrons to form ions.
• Ions have a net charge due to having more or fewer electrons than protons.
• The mass number is the total number of protons and neutrons in an atom.
• What is an atomic number and why is it useful?

  Proton number and can determine the chemical properties of an element and its place in the periodic table.
• What is the mass number of an atom?

  Number of the neutrons and protons added together.
• What is the definition of an isotope?

  Atoms of the same element with the same atomic number but with a different number of neutrons, resulting in a different mass number. 
• What are the sub-atomic particles in an atom and their charge/mass/location

  Table:

  
• What is the main difference between isotopes of an element?

  Number of neutrons
• Which subatomic particle has a zero charge?

  Neutron
• What is the charge of electrons?

  Negative
• What is the relative mass of electrons compared to protons and neutrons?

  1 over 2000
• Which subatomic particle has a positive charge?


  Proton
• How do protons, neutrons, and electrons contribute to the composition of an atom?

  Protons and neutrons are located in the nucleus, with protons carrying a positive charge and neutrons having no charge. Electrons orbit the nucleus in shells and carry a negative charge.
• Why is it crucial to understand the differences between isotopes of an element?

  Understanding isotopes is important because they have the same number of protons but different numbers of neutrons, leading to variations in mass. This impacts chemical behavior and physical properties of elements.
• Why is the relative atomic mass measured with respect to carbon-12 significant in understanding atomic structure?

  The measurement of relative atomic mass relative to carbon-12 provides a standardized scale for comparing the masses of atoms, aiding in the understanding of atomic weights and compositions across different elements.
• Why is it essential to understand the relative masses of electrons, protons, and neutrons in the context of atomic structure?

  Understanding the relative masses of subatomic particles helps in determining the overall mass and composition of atoms, providing insights into their physical properties and behaviour.
• How does the concept of ions differ from that of neutral atoms in terms of electron and proton numbers?

  Ions have an unequal number of electrons and protons, leading to a net positive or negative charge, unlike neutral atoms where the number of protons equals the number of electrons.
• Why are protons and neutrons referred to as nucleons in the context of atomic structure?

  Protons and neutrons are called nucleons because they are the subatomic particles found in the nucleus of an atom, contributing to its mass and stability.
• How do the charges of protons, neutrons, and electrons influence the overall charge of an atom?

  The positive charge of protons balances the negative charge of electrons, while neutrons have no charge, resulting in an overall neutral charge for an atom.
• What impact do additional neutrons in isotopes have on the atom's chemical properties?

  Additional neutrons in isotopes result in a greater mass for the atom.Neutrons do not significantly affect chemical properties because they do not change the electron configuration.