What’s the Matter foldable

Chemistry Chemistry is the study of matter and the changes matter undergoes.

Matter Matter is anything that takes up space and has mass.

General Properties mass weight shape volume color density texture

Properties of Matter How It Looks (Shiny ,Dull, Color, etc.) How It Feels (Hard, Soft, Rough , Smooth, etc.) How It Smells (Sweet, Sharp, Terrible, No Smell, etc.) How It Sounds (Loud, Soft, Echo, No Sound, etc.) What It Does (Bounce, Stretch, Tear, Break, Magnetism etc.)

SOLIDS

Solids Characteristics definite shape definite volume objects do not pass through easily Examples: paperclip, bones, desk, car, chair, etc…

Solids Molecules are very close molecules move very slowly in place.

Liquids

Liquids Characteristics no definite shape definite volume takes shape of container has surface tension example: water, soda, glue, oil, etc…

Liquids molecules have some space between them. molecules move around a bit faster.

GAS

GAS Characteristics no definite shape no definite volume expands to fill container examples: oxygen, hydrogen, steam, air, carbon dioxide, etc…

GAS Molecules have lots of space. molecules very fast.

Metals Characteristics Most are solid at room temp. Except Mercury. Most elements are metals Located to the left of the zigzag line. Shiny, conduct heat & electricity, and Malleable.

Non-Metals Located on the right side of the zigzag line. Characteristics Located on the right side of the zigzag line. More then ½ are gases at room temperature. dull, DO NOT conduct heat or electricity.

Metalloids Characteristics Border the zigzag line Have properties of both metals and non-metals. Called “semi-conductors”.

Compound Molecule made of more then one type of atom, chemically combined in a fixed proportion. CAN NOT be separated easily by physical means. Properties of the compound are much different than the elements that make them up.

Sodium + Chlorine Na=Cl= NaCl Compound Example Sodium + Chlorine Na=Cl= NaCl greenish gas Soft shiny metal Salt

Mixture Made up of different types of particles, they are NOT chemically combined. tossed salad CAN BE separated easily by physical means. 2 Types of mixtures Homogeneous-the same appearance and composition throughout.

Mixtures Heterogeneous-made up of different visible substances. Example oil and vinegar Example; Chocolate chip cookie recipe Recipe ingredients+ baking=cookie

Molecules made up of only one type of atom Element Molecules made up of only one type of atom

Solutions Special Mixture where a substance dissolves in another. particles are not big enough to be seen. Particles spread out evenly Example + = H2O

Physical Property Characteristic of matter that can be seen through direct observation without changing the identity of the substance.

Density: mass/volume. Brittleness: cracks/breaks. Transparency: light passes through. Boiling point: temperature liquid to gas. Freezing point: temp from liquid to solid. Melting Point: temp from solid to liquid. Ductility: bends without breaking. Elasticity: how much it can be stretched.

Physical Change Change in which the identity of the substance does not change! Atoms do not rearrange only physical properties change, chemical do not change No energy is produced. Physical changes are generally easy to reverse.

Chemical Property Characteristics of a substance indicating that it can change chemically. It changes one substance into another.

properties Flammability- ability to burn Combustible- explode Rust- reacts with oxygen React with Vinegar-produce new substance. Oxidation- produces something new All chemical changes include physical change

Chemical Change How the particles of matter react with other kinds of matter and change. color temperature bubble formation can not be reversed ex burning eggs

Chemical Change Atoms are rearranged into different molecules Both physical and chemical properties have changed. Energy is often produced (heat) CHANGES ARE NOT REVERSIBLE WITHOUT ANOTHER REACTION!

ENDOTHERMIC reaction Absorbs energy solid to liquid- melting ex-ice-water hot

Exothermic releases energy liquid to solid- freezing water to ice cold

Condensation GAS Evaporation Liquid Sublimation Melting Sublimation Freezing Freezing Solid

Solid  liquid melting (ICE to water) Solid  gas- Sublimation ex: Dry ice CO2 Liquid  Gas – Evaporation H2O steam Liquid  Solid- Freezing H2O  ice Gas  Liquid- Condensation Steam H2O Gas  Solid- Sublimation freezing CO2 dry ice

pH Scale A range showing the strength of acids and bases 1 Acid 7 Neutral 14 Base

Acid- A substance that is sour, reacts with metals has H+ ions Examples: lemon juice, orange juice, vinegar, perfume, Alcohol , pineapple. (picture) Base- A substance that is bitter, slippery, and has OH¯ ions. Examples- Hairspray, furniture polish, bleach, (non-scented) soap. (picture)

Solubility= The ability of one substance to dissolve in another at a given temperature & pressure.

Solubility Soluble- able to dissolve in another substance Insoluble- Not able to dissolve in another substance

Solubility Insoluble can equal a precipitate. a substance formed when two or more substances are mixed and a solid “falls” out of the liquid and settles on the bottom.

Balancing Chemical Equations Reactants Product Yields 2Mg + O2 2MgO Coefficient Subscript Coefficient

Balancing Chemical Equations Steps 1. Determine number of atoms on each side. 2. If not equal pick one element you need to work with. 3. Add a coefficient in front of formula adjust counts to see if balanced. 4. If not keep adding to get each side equal.

Examples: 2H2 + O2 H2O H= H= O= O= Na + O2 Na2O Na= Na= O= O=

Examples: H2O2 H2O + O2 H= H= O= O=