🫧reactivity unit🫧

• All matter consists of particles called atoms, which cannot be divided using chemicals.
• Throughout time, there have been many different theories of the atom as science has further developed our understanding of them.
• All matter is composed of atoms, which have different parts including protons, neutrons, and electrons, but an atom is a basic chemical building block of matter.
• The atomic model evolves over time as science further develops our understanding of them.
• Elements in the periodic table are arranged according to atomic number.
• Elements in a column on the periodic table share physical and chemical properties.
• The physical and chemical properties of the elements in groups 1,2,3,6,7 and 8 are described.
• An element is a material that cannot be broken down into anything simpler, for example, a piece of pure gold only contains gold particles.
• The formula for water molecule is H2O.
• A covalent bond is a type of bond that involves the sharing of electrons between atoms.
• Group 1 metals react with water to produce hydrogen gas and a metal hydroxide.
• Alkali metals are shiny silver which dull by oxidation, are soft enough to be cut with a knife, have low melting and boiling points, have low density, react with water to form alkaline compounds, and are stored under oil due to their high reactivity.
• When group 1 metals react with water, they produce hydrogen gas and a metal hydroxide.
• Alkali metals all have one electron in their outer shell.
• Group 1 metals have to be kept in oil to not react with oxygen and water.
• Elements in a column share physical and chemical properties.
• Group 1 metals are also known as alkali metals due to their reaction with water.
• Group 1 metals are stored under oil to prevent them from reacting with oxygen and water.
• The physical and chemical properties of the elements in group 1 can be described.
• As you go down Group 1, the atoms become larger and the outer electron is further from the nucleus, which makes the outer electron more easily lost.
• Group 1 metals can be used in real life, for example, as a component in batteries.
• As group 1 metals begin to react with oxygen in the air, they begin to dull, forming a metal oxide.
• Cordy's Golden Rules for Ionic Bonding can be used to determine how atoms can bond together by transferring electrons.
• If an ion gains 3 electrons, it gets a 3- charge.
• A positive cation and a negative anion can combine in a chemical reaction to form an ionic compound.
• Cations are electrostatically attracted to the oppositely charged anions when forming an ionic compound.
• Ions will gain or lose electrons, depending on what takes the least amount of energy.
• If an ion gains 1 electron, it gets a - charge.
• The formula for ionic compounds is written by writing the cation and its charge first, the anion and its charge, drawing an arrow, and showing the product.
• Electrons are transferred from one atom to another to form ions.
• If an ion loses negative electrons, it becomes positive.
• The Sodium ion loses 1 electron and the oxygen ion needs to gain 2 electrons in an ionic compound.
• Ions form when elements try to get full outer shells.
• Two Sodium ions transfer their electrons to one oxygen ion to make an ionic compound.
• If an ion gains 2 electrons, it gets a 2- charge.
• If the charges are different, the charges are swapped and dropped below.
• Cations lose electrons and anions gain electrons in ionic compounds.
• The magnesium ion loses two electrons and the chloride ion gains 1 electron in an ionic compound.
• If an ion loses 1 electron, it gets a + charge.
• If students have a cation (positive) and an anion (negative), they write the ionic compound it would form.