Matter anything that has mass and takes up

Matter: anything that has mass and takes up space Mass: the amount of matter an object has Weight: the force applied to an object by gravity Substance: a sample that contains only one kind of matter

States of matter Solid: matter that has - Definite shape and volume - Particles packed tightly together - No compressibility (incompressible) - Particles that move in a fixed position (vibrate)

Liquids: matter that - Particles are close but not in a fixed position - Flows - Takes the shape of its container - Has a definite volume - No compressibility (incompressible)

Gas: matter that - Take the shape of its container - Particles are farther apart - Has no definite volume or shape - Is easily compressed

Physical Property: a property that can be observed or measured without changing the substance’s composition Ex: Color, Temperature Density Odor Hardness State of matter

Physical Change: a change in a substance which does not alter its chemical composition - Freezing - Melting - Boiling - Cutting - Grinding - Crumpling

Chemical Property: the ability of a substance to react and form a new substance (observed only when there is a chemical change) (most chemical changes are not easily reversed) Ex. Burning, rusting, rotting, corroding

Chemical Reactions Chemical Reaction: one or more substances change into a new substance Ex. Iron and oxygen react or make rust Reactants: the starting substances in a chemical reaction Products: What you end up with in a chemical reaction HCl + Na. OH → Na. Cl + H 2 O

How do you know if a chemical reaction is happening? There are four indications of a chemical reaction. (not all indicators will be easy to see during every chemical reaction) 1. 2. 3. 4. The production of a gas A change in energy A change in color The production of a precipitate

Mixtures: a physical blend of two or more substances Heterogeneous Mixtures: mixtures that are not uniform throughout or have more than one phase Ex. Oil and water, paint, chocolate chip cookies, and salad

Homogeneous Mixtures: a mixture that is uniform throughout and only has one phase Ex. Lemonade, Koolaid, and Salt water ALL MIXTURES CAN BE SEPERATED INTO THEIR INDIVIDUAL COMPONENTS!

Elements and Compounds Element: the simplest form of matter - Can NOT be separated into simpler substances through ordinary chemical means - They are the building blocks for all substances - They are represented by one or two letter symbols (C for Carbon, H for Hydrogen)

Compounds: two or more elements combined - They can be separated into simpler substances (the elements) - They are represented chemical formulas Ex. Na. Cl (salt) and H 2 O (water)

The Law of Conservation of Mass - Mass is never created nor destroyed in a chemical or physical change. - The mass of the products always equals the mass of the reactants.

Intensive Properties: properties that do not depend on the amount of matter present. Ex. Melting point Extensive Properties: properties that do depend on the amount of matter present Ex. mass

Qualitative and Quantitative Measurements Qualitative Measurement: descriptive, nonnumerical information Quantitative Measurement: a numerical measurement

How close is your measurement? Accuracy: How close your measurement is to the actual (accepted) measurement Precision: a measure of how close a series of measurements are to each other

Experimental Error: How close the value you got in lab (the experimental value) is to the actual value (accepted value) % Error = (Accept. Value – Exper. Value) x 100% Accepted Value In lab, I found that 1 ml of water has a mass of 1. 32 g. The accepted mass of 1 ml of water is 1 g. What was my percent error? %Error = (AV – EV) x 100% = (1 g – 1. 32 g) x 100% AV 1 g= 32. 0%