By Maya Seaforth

Matter  What is matter?  Matter is objects that take up space and everything around you is made up of matter.

States of Matter Solid – Solid is one of the three classical states of matter. It is characterized by structural rigidity and resistance to changes of shape or volume. The particles stay tied together.

Liquid  Liquid – Liquid is a form of matter with a definite value but no fixed shape. Like a gas, liquid is able to flow and take the shape of a container. The particles have room to move around.

Gas  Gas – Near absolute zero, a substance exists as a solid. It boils into gas at it’s boiling point. The particles move around freely in the absence of an applied electric field.

Physical & Chemical Properties  Physical – are properties that do not change the chemical nature of matter.  Chemical – are properties that do change the chemical nature of matter.  The difference between chemical and physical properties are that they are both opposite from one another.

Physical & Chemical Changes  Physical – A physical change does not produce a new substance, the changes in state or phase are physical changes.  Example: Melting an ice cube, breaking a bottle, crushing a can, crumpling a paper, car crash.  Chemical – Chemical change produces a new substance.  Example of chemical changes include: combustion, cooking an egg, rusting an iron pan, mixing hydrochloric acid, and sodium hydroxide to make salt and water.

Atoms  What is an atom?  An atom is a basic piece of matter. An atom itself is made up of three tiny particles called subatomic particles; protons; neutrons; and electrons.

Element  What is an element?  In chemistry, an element is a pure substance that cannot be broken down into any simpler substance by chemical methods.  Example: Iron (Fe) Gold (Au), Hydrogen (H), Carbon (C), and Oxygen (O)

Compound  What is a compound?  Compound are pure substances made of atoms of two or more elements chemically combined in fixed ratios.  Example: Carbon Dioxide (Co2), Water (H2O), Hydrogen Peroxide (H2O2), Table Salt (NaCl), and Carbon Monoxide (Co)

What is a Periodic Table?  The periodic table is a tabular display of the chemical elements, organized on the basis of their properties.  How do you read/use the periodic table?  Step 1 – The element symbol. Symbols are the abbreviations of the elements name.  Step 2 – The elements atomic number. It’s the number of protons and atoms of the elements contained.  Step 3 – The elements name. Many tables will include the names to help those who do not remember.

Substance/Mixture  Mixture – Made of more than one kind of material  Substance – Made of one kind of material.  What is the difference between them?  A mixture can have more than one material and the substance can have only one material.

Heterogeneous & Homogenous Mixtures  What is the difference between them?  A homogeneous mixture has the same uniform appearance and composition throughout. Many homogeneous mixtures are commonly referred as solutions. A heterogeneous mixture consists of visibly different substances or phases. The three phases or states of matter are gas, liquid, and solid.  Example for heterogeneous – salad dressing, strawberry shortcake, fruit salad, and party mix chips.  Example of homogenous – juice, soda, milk, tea, and lemonade.

Solutions  What is a solution?  A homogeneous mixture of two or more substances, which may be solids, liquids, gases, or a combination of these.  Solute - A substance dissolved in another substance, usually the component of a solution present in the lesser amount.  Solvent - A substance in which another substance is dissolved, forming a solution.  Examples: Solvent - Water Solute - Sugar Solution - Sugar water Solvent - Milk (hot) Solute - Cocoa powder Solution - Hot Cocoa Solvent - Water Solute - Kool-Aid powder Solution - Kool-Aid

Solubility  The maximum quantity of a substance that may be dissolved in another. The maximum amount of solute that may be dissolved in a solvent.