Chemistry Unit Project By: Stephanie Do 707

Matter Everything in the universe is made up of matter. Matter is anything that has mass and volume or that takes up space. There are three types of matter solid, liquid, and gas. In solids the atoms are packed together, the atoms vibrate, and its shape is definite. In liquids the atoms move freely, the atoms are farther apart, and it takes the shape of its container. In gases the atoms bounce off of each other and it fills the shape of its container.

Examples of Matter Liquids Solids Gases Water Ice Juice Chairs Soda Milk Saliva Smoke Steam Water vapor Carbon dioxide Oxygen Ice Chairs Tables Glass Wall

Physical and Chemical Properties Physical properties are when the matter is being observed or measured without it being changed. And they are to describe the matter that is being observed. Examples: Color, size, mass, shape, boiling point, etc. Chemical properties are when a substance reacts to acids or another substance in which it creates a new substance. Examples: Rust forming on iron, burning wood, frying an egg, reaction to acid, heating the substance, etc.

Physical and Chemical Changes Physical changes are changes that does not make a new substance. Examples: Snow melting, ripping paper, chopping wood, cutting apples, freezing Kool-Aid, etc. Chemical changes are two substances mixed together in a result of a new substance. Examples: Burning wood, magnesium reacting with oxygen, rotting fruit, roasting marshmallows, frying an egg, etc.

Atoms An atom is the smallest particle that an element can be divided into. There are 3 parts of an atom. Protons, neutrons, and electrons, Protons have a positive charge. Neutrons have a neutral charge. Electrons have a negative charge.

Elements It is a substance that builds up matter. Also an element is made up of the same type of atom. They are organized in the periotic table. Examples: Carbon dioxide, oxygen, nitrogen, aluminum, sodium, etc. They are organized on the periodic table.

Compounds Matter that contains two or more elements in it. And the elements are chemically bonded. That means that it can only be separated chemically. Examples: Water, table salt, table sugar, baking soda, alcohol, etc. Compound of water.

Periodic Table It is a chart were all the elements are organized on. And they are grouped by their properties. Which is by metals, metalloids, nonmetals, noble gases, then unknown elements. And you read it from left to right. The number on top of the letter is the atomic number. The letter is the element symbol. The following is the element name. And the last number is the atomic mass.

Substances and Mixtures A substance is a component of a mixture. A mixture is a combination of two or more substances. And the elements are physically bonded in mixtures. Which means that they can only be separated physically. A mixture of molecules.

Heterogeneous and Homogeneous Mixtures Heterogeneous mixtures are unevenly mixed mixtures. Examples: Salads, oatmeal, soil, soups, orange juice with pulp, etc. Homogeneous mixtures are evenly mixed mixtures. Examples: Apple juice, alcohol, orange juice, salt water, sugar water, etc.

Solutions A solution is a homogeneous mixture of 2 or more substances that are evenly mixed together. And there are two parts of solution. One is a solute and the other one is a solvent. A solute is the substance that is being dissolved. Examples: Sugar, salt, baking soda, food coloring, iodine, etc. A solvent is the substance that dissolves the solute. There are a lot of solvents but the universal solvent is water. Examples: Water, nitrogen, silver, sulfuric acid, hydrochloric acid, etc.

Solubility Solubility is how easily a solute dissolves in a solvent. The solubility of a material is described as the material that can be dissolved in 200g of solvent at a given temperature. And some ways to make it easier to dissolve faster are heating the solute, stirring it, adding more pressure, and increasing the surface area.

References Science notebook Science saurus http://www.elmhurst.edu/~chm/vchembook/104Aphysprop.ht ml http://www.elmhurst.edu/~chm/vchembook/105Achemprop.ht ml http://www.iun.edu/~cpanhd/C101webnotes/matter-and- energy/properties.html