Periodic Table

• Elements are arranged into groups (columns) based on their electron configuration
• Atomic mass is the average mass of all atoms of that element
• The periodic table is organised by atomic number, which is the number of protons in an atom.
• The periodic table is divided into periods, which represent the number of electrons in an atom's outer shell.
• Periods increase from left to right across the table.
• Groups contain elements with similar chemical properties due to having the same number of valence electrons.
• The atomic number tells us how many protons an atom has, which determines its identity as an element.
• Mass number = #protons + #neutrons
• Groups contain elements with similar chemical properties due to having the same number of electrons in their outer shell.
• Isotopes have different numbers of neutrons but the same number of protons.
• Metals have high melting points, low densities, good conductors of heat and electricity, shiny surfaces, and can be malleable or ductile.
• Periods contain elements with increasing atomic numbers and increasing atomic masses.
• Groups or columns contain elements with similar chemical properties due to having the same number of valence electrons.
• Metals are found on the left side of the periodic table and have low ionisation energies.
• Non-metals are found on the right side of the periodic table and have high ionisation energies.
• Transition metals are located between non-metals and metals and have partially filled d orbitals.
• Transition metals are located between non-metals and metals and have partially filled d orbitals.
• Atomic mass is calculated by adding up the numbers of neutrons and protons in an atom.
• Atoms can gain or lose electrons to form ions.
• Atoms can gain or lose electrons to form ions.
• Isotopes are atoms of the same element that have different numbers of neutrons.
• Isotopes are atoms of the same element that have different masses because they have different numbers of neutrons.
• Ions are charged particles formed when atoms gain or lose electrons.
• Atomic mass is calculated by adding up the numbers of neutrons and protons in an atom.
• Atomic mass is calculated by adding up the masses of all the particles in the nucleus (protons and neutrons) and dividing it by Avogadro's constant.
• Elements can be represented using symbols or names.
• Non-metals are poor conductors of heat and electricity, brittle solids at room temperature, and do not react with water.
• Relative atomic mass is the average mass of atoms of an element compared to carbon-12.
• Elements on the periodic table are arranged by increasing atomic number (number of protons).
• Non-metals are poor conductors of heat and electricity, brittle solids at room temperature, dull surfaces, and do not react with water.
• Ionic bonding occurs when metals lose electrons to nonmetals, forming positive ions, while nonmetals gain electrons to form negative ions.
• Ionic bonding occurs when metals lose electrons to nonmetals, forming positive ions, while nonmetals gain electrons to form negative ions.
• Ionic bonding occurs when metals lose electrons to form positive ions and nonmetals gain electrons to form negative ions.
• Ionic bonding occurs when metals lose electrons to form positive ions and nonmetals gain electrons to form negative ions.
• The periodic table is organized by atomic mass (atomic weight) and electron configuration.
• The periodic table is organized by atomic mass (atomic weight) and electron configuration.
• Atomic mass is calculated using relative atomic mass (A) and average atomic mass (amu).
• Elements on the left side of the periodic table tend to lose electrons when they form compounds, while those on the right side gain electrons.
• The noble gases (Group 0) are unreactive because they already have full outer electron shells.
• The atomic mass unit (u) is defined as exactly one twelfth of the mass of a carbon-12 atom, which has six protons, six neutrons, and six electrons.