Matter : anything that has mass and takes up space
Mass : amount of matter in an object. Calculate by placing on a balance (g)
Weight : The downward pull of an objects due to gravity
Volume : how much space an object takes up
- Solids: Length x Width x Height (cm 3 )
- Liquids: Use a beaker/graduated cylinder (mL)
-Irregular shaped objects: displacement
Displacement – process used to find the volume of irregular shaped objects, using a graduation cylinder and water.
Density : the mass per unit volume of a substance. Calculate density = mass
/ volume (g/cm 3 )
Element – a substance that contains only one type of atom (Eg. Carbon atom) Elements cannot be broken down into other substances by physical or chemical means.
Compound – a substance that consists of two or more different types of atoms bonded together. (E.g. Water molecules is a compound of hydrogen and oxygen)
Atom : smallest basic unit of matter
Molecule : two or more atoms bonded together
Atoms and Molecules are always in motion!

Move rapidly in a gas

Can slide freely in a liquid

Close together and vibrate in solids

Expansion and Contraction when energy is gained or lost
States of Matter : different forms in which matter can exist

Solid – fixed volume and fixed shape

Liquid – fixed volume but does not have a fixed shape

Gas - no fixed volume or shape
States of matter change when heat energy is lost or gained. When energy is gained, the molecules expand and move faster. When energy is lost, the molecules contract and slow down movement.

Characteristic property – properties that never change and can be used to identify a substance (for example, the density of iron (7.71 g/cm 3 ) will stay the same no matter if the iron is a small iron nail or a massive statue)
Characteristics properties are independent of mass, volume, and shape. (e.g.
Density, Solubility)
Solubility –ability to dissolve
Solute – the smaller proportion of a solution
Solvent – the larger proportion of a solution
Solution – a mixture so well mixed that it can look like a pure substance
Aqueous solution – a mixture where water is the solvent
Chemical Reaction - a reaction that produces new substances by changing the way in which the atoms are arranged. Chemical reactions form new substances (ex. Iron + Oxygen formed Iron Oxide.) You can tell a chemical reaction has occurred if you there is
1.
Change in temperature
2.
Change in color
3.
Production of a gas
Metalloid – share properties of both metals and nonmetals. Metalloids are located on the dark zigzag line of the periodic table. They are semiconductors of electricity.
Alloy – mixture of two metals
Atomic Number – the number of protons in the nucleus of the atom. The atomic numbers of elements increase as the elements move towards right on the periodic table.
Atomic Mass Number – The average number of protons and neutrons in an atoms nucleus. It represents the mass of one atom of that element.
Period – each row of the periodic table. As read from left to right, one proton and one electron are added from one element to the next.
Group (aka family) – each column of the periodic table. Elements in a group share similar properties.
Use your periodic table flip chart to know about reactive metals, transition metals, rare earth metals, metalloids, halogens, and noble gases.

Essay Topics

Be able to draw the structure of an atom, label its parts, and describe the associated charges o Proton – positively charged particle located in the atoms nucleus o Neutron
– particle in the atoms nucleus that has no charge o Electron – negatively charged particle that move around the outside of the nucleus o Nucleus - combination of protons and neutrons in the middle of an atom

Know the differences between physical and chemical changes o Physical Change : Changes that can be undone and do not create new substances (E.g. Ripping up paper) o Chemical Change : Changes that cannot be undone. Chemical changes form new substances. The chemical reaction rearranges the atoms, which causes a completely new product to form (E.g. Burning paper) – see the chemical reaction description on the previous page

How could you differentiate between a mixture and a pure substance
(element or compound)? Why would this work? o Think about our pure substance vs. mixtures lab. What did you do to determine if the substances were pure or mixtures? (Used various properties to test if substances were mixtures or pure – You tested the magnetism, solubility, and density of materials. If one material was soluble and the other was not, you knew it was a mixture. If put materials in water and one material is dense and sinks while the other is less dense and floats, what can you tell? You also used observations to compare the appearance of certain substances).

 o Mixture - a combination of different substances that remain the same individual substances (are not chemically combined) and can be separated by physical means. (E.g. Fruit salad / Kool-Aid) o Pure substance : either an element or a compound (only has one type of atom)
Know how to use the periodic table o You will be asked to pick an element and describe its characteristics based on its location on the table (including reactivity, uses, etc.) Include its location (group and family), number of protons, and mass. You may want to study from your lab where you studied the Element Cards.

Metals vs. Nonmetals o Metal – Good conductors of electricity

Most are solid and shiny

Able to be hammered or rolled into a shape (malleable)

Able to form into a wire (ductile)

Take up most of the periodic table (groups 1, expect hydrogen through group 12)
 Some metals are more reactive than others (group 1 is
VERY reactive!) o Nonmetals : elements to the right of the periodic table

Many are gases at room temperature

Solid nonmetals have dull surfaces and are not malleable
 Poor conductors of electricity
 The reactive nonmetals are in Group 17