Chemistry: Ionic Bonds and Electronic Structures

A chemical reaction where two or more reactants combine to form a single, more complex product.

A chemical reaction where a single complex reactant breaks down into two or more simpler products.

A chemical reaction where a more reactive element displaces a less reactive element in a compound, resulting in a new compound and a new element.

A chemical reaction where elements in different compounds exchange places, resulting in two new compounds.

Group I or 1 on the periodic table. They have one valence electron and readily lose it to form a +1 charge. They are very reactive metals.

Group II or 2 on the periodic table. They have two valence electrons and readily lose them to form a +2 charge. They are reactive, but less so than alkali metals.

Group VII or 17. They have seven valence electrons and readily gain one electron to form a -1 charge, making them highly reactive.

Group VIII or 18. They have a full outer shell of electrons, making them stable and unreactive. They are known for their lack of reactivity.

A bond formed by the transfer of electrons from a metal atom to a non-metal atom. This creates a positive metal ion (cation) and a negative non-metal ion (anion). The oppositely charged ions are attracted to each other, forming the ionic bond.

A bond formed by the sharing of electrons between two non-metal atoms. In this sharing, both atoms gain a stable electron configuration.

A compound formed when a metal and a non-metal react. The metal atom loses electrons to form a positive ion (cation) and the non-metal atom gains electrons to form a negative ion (anion). These ions are held together by electrostatic attraction, forming the ionic compound.

A compound formed when two or more non-metals share electrons. These shared electrons form a covalent bond, which holds the atoms together.

A chemical reaction that releases energy into the surroundings, often in the form of heat or light.

A chemical reaction that absorbs energy from the surroundings, often in the form of heat or light.

A measure of how fast or slow a reaction proceeds.

A factor that affects the rate of a reaction, such as temperature, concentration, surface area, and the presence of a catalyst.

A substance that changes color depending on whether it is placed in an acid or a base.

A substance that changes color depending on whether it is placed in an acid or a base. Often used to determine the pH of a solution.

A numerical scale ranging from 0 to 14 that is used to compare the acidity of solutions. A pH of 0 is the most acidic; a pH of 7 is neutral; and a pH of 14 is the most basic.

A solution with a pH value between 0 and 6. Stronger acids have a pH closer to 0, while weaker acids have a pH closer to 6.

A solution with a pH value between 8 and 14. Stronger bases have a pH closer to 14, while weaker bases have a pH closer to 8.

A solution with a pH of 7. It is neither acidic nor basic.

A compound that begins with H and usually has a state symbol of (aq). For example, HCl(aq) is the formula for hydrochloric acid.

Acids can react with carbonates to produce CO2(g). For example, HCl(aq) + NaHCO3 → CO2 + H2O + NaCl

A reaction where a hydrocarbon reacts with oxygen to produce carbon dioxide (CO2) and water (H2O), releasing energy. This occurs when there's enough oxygen for the reaction to complete.

A reaction where a hydrocarbon reacts with oxygen to produce carbon dioxide (CO2), water (H2O), carbon monoxide (CO), and carbon (C) due to insufficient oxygen. This can be dangerous as CO is toxic.

A chemical change where an acid and a base react to form water (H2O) and a salt. The pH of the final solution is closer to neutral (pH=7).

Chemical reaction where hydrogen ions (H+) from an acid and hydroxide ions (OH-) from a base react to form water (H2O).

A chemical reaction where elements of two reactants switch places, forming two new compounds.

The mass of the reactants is equal to the total mass of the products. This is why the mass of the zinc chloride solution plus the missing product must equal the initial mass of the reactants.

In the reaction of zinc metal with hydrochloric acid, hydrogen gas (H2) is produced. The reaction can be written as: Zn + 2HCl → ZnCl2 + H2

The reaction of zinc with hydrochloric acid is an example of a single displacement reaction. In this reaction, a more reactive element (zinc) displaces a less reactive element (hydrogen) from a compound (hydrochloric acid).