chemistry

• Isotopes are atoms with different numbers of neutrons but the same number of protons, resulting in different masses.
• The number of protons is equal to the atomic number.
• The atomic mass is calculated by adding up the relative abundance of all isotopes present in an element.
• Atoms can gain or lose electrons to form ions.
• Atomic structure consists of electrons orbiting around the nucleus at various energy levels called shells or electron clouds.
• Electron configuration refers to the arrangement of electrons within these shells/clouds.
• Ions have an overall charge due to unequal numbers of protons and electrons.
• Cations (positive) have fewer electrons than protons, while anions (negative) have more electrons than protons.
• Atomic structure includes electrons arranged around the nucleus in shells or energy levels.
• Electron configuration refers to the arrangement of electrons within these shells.
• Ions have a net charge due to having more or fewer electrons than protons.
• Cations (positive) have lost one or more electrons, while anions (negative) have gained one or more electrons.
• Elements have unique electron configurations that determine their chemical properties.
• Ionization Energy (IE) is defined as the minimum amount of energy required to remove one mole of gaseous atoms from their ground state and form one mole of positive ions.
• The number of electrons is equal to the atomic number.
• Ions are formed when atoms either gain or lose electrons, leading to changes in charge and size.
• Metals tend to lose electrons to become cations, while non-metals tend to gain electrons to become anions.
• Cations are positively charged, while anions are negatively charged.
• The periodic table is organized by atomic number, with elements grouped into periods based on their electron configurations.
• Shells are filled with electrons up to their maximum capacity.
• Cations are positively charged ions formed when atoms lose one or more electrons.
• Isotones are atoms with the same number of neutrons but different numbers of protons.
• Ions are formed when atoms either gain or lose electrons.
• Metals tend to lose electrons to become cations, while non-metals tend to gain electrons to become anions.
• Isobars are atoms with the same mass number but different numbers of neutrons.
• Isotopes are atoms with different masses but the same number of protons (atomic number).
• Atomic mass = relative abundance x mass
• Electron affinity refers to the tendency of elements to attract electrons and form negative ions.
• Relative abundance is calculated by dividing the mass of an element by its atomic weight.
• Relative abundance is calculated by dividing the mass of an element by its atomic weight.
• Metals tend to lose electrons to become positively charged cations, while non-metals tend to gain electrons to become negatively charged anions.
• Metals tend to lose electrons to become positively charged cations, while non-metals tend to gain electrons to become negatively charged anions.
• Periodic trends refer to patterns observed when comparing elements across rows or columns of the periodic table.
• Periodic trends refer to patterns observed when comparing elements across rows or columns of the periodic table.
• Electron configuration refers to the arrangement of electrons around the nucleus of an atom.
• Electron configuration refers to the arrangement of electrons around the nucleus of an atom.
• The outermost shell determines chemical properties.
• The outermost shell determines chemical properties.
• The first ionization energy is the energy needed to remove one electron from one atom of an element.
• The first ionization energy is the energy needed to remove one electron from one atom of an element.