Advanced Physical Science 1 st Semester Exam Review December ~ 2009

Know #2: SI units of measurement  Mass – grams (g)  Volume – milliliters (mL)  Density – grams per cubic cm (g/cm³)  Distance – meters (m)  Speed – meters per second (m/s)  Velocity - meters per second South (m/s South)  Acceleration – m/s² South  Force – Newtons (N)

#3: Three types of scientific models  Physical  Mathematical  Conceptual

#4 Examples of physical properties of matter  Solubility  State of matter (solid, liquid, gas)  Density  Ductility  Malleability  Thermal conductivity  Shape, texture, etc.  Odor  Color  Back Back

#5 Viscosity and an example  Physical property of a liquid which is its level of resistance to flow  High viscosity – stronger attraction of molecules, flow is slower  Honey has a high viscosity compared to water

#6: The states of matter…  Solid – Definite shape, definite volume  Liquid – Definite volume, no definite shape  Gas – No definite shape or volume  Plasma – (gas) No definite shape of volume

#6 Continued – Changes of State  Liquid to gas – evaporation  Gas to liquid – condensation  Solid to liquid – melting (endothermic)  Liquid to solid – freezing (exothermic)  Sublimation – solid to gas

#7: What sublimation is  Solid becoming a gas without going through the liquid state.  Example – Dry Ice

# 8: Properties of metals…  Hard  Shinny  Malleable – can be pounded, pressed  Ductile – can be pulled into wire  Good conductors of heat

#9: Properties of non- metals…  Dull  Not malleable/ductile  Poor conductors

#10: The parts of an atom and their charges  Protons – positive, in nucleus  Neutrons – no charge, in nucleus  Electrons – negative charge, move in all directions at various levels around the nucleus

#11: How the periodic table is arranged…  By increasing atomic number from left to right  Family / groups in columns  Periods in horizontal rows

#13: Reference point…  Place or object used for comparison to determine if something is in motion

#14: Balanced, unbalanced forces and net force  Balanced – forces acting on an object are equal; no movement/ motion  Unbalanced – forces acting on an object are not equal; results in motion  Net force – Combination of all forces acting on an object  Force can be a push or a pull

#15: Examples of Acceleration and what would not be an example  Speeding up – or slowing down  Changing direction  Spinning around  Orbiting NOT Examples:  Going in one direction at a steady rate  Not moving at all

Understand 1: The Scientific Method  Ask question or state problem  Gather info  Form a hypothesis  Test the hypothesis  Observe  Analyze  Draw a conclusion

Scientific Method, continued  Independent variable – The one you’re testing; the one that’s changing  Dependent variable – the one that changes as a result of the experiment; what you’re measuring.

#2: The difference between scientific law and theory  Scientific Theory - Explains / an explanation based on hypothesis and observations  Scientific Law – Summarizes/ a summary of many results; Will predict or tell what will happen every time.

#4: Examples of chemical properties and what they mean  Flammability – ability to burn  Reactivity– Ability to chemically combine

#5: The difference between a physical and chemical property  Physical property – can be observed or measured without changing identity See slide #4 under “Know”slide #4 under “Know”  Chemical property – ability to change into a new substance

# 6: Difference between mass and weight  Mass is the amount of matter in an object  Weight is the measure of gravitational force on an object

#7: The particles in solids, liquids and gases  In solids they vibrate in place ( strong attractions of particles)  Liquids – Are close but slide past one another  Gases – Move apart independently and randomly

#8: The difference between compounds and mixtures  Compounds – a chemical combination of elements  Mixtures – combination of 2+ substances not chemically combined  Compound examples – H 2 O, CO 2  Mixture examples – dirt, pizza, salad, blood, oil & vinegar

#9: Difference between elements and compounds  Elements are pure substances that can’t be broken down by physical or chemical means (particle – atom)  Compounds are pure substances made of 2+ elements combined chemically (particle – molecule)

Difference between solvent and solute  The solvent is the substance in which the solute is dissolved.  Salt water- Water is the solvent, salt is the solute

# 11: Difference between metals, non-metals and metalloids  Metals are shiny, malleable, ductile and good conductors of heat  Non-metals are dull and poor conductors  Metalloids are semi-conductors; properties of both

#12: Difference between mass number and atomic number  Atomic number is the # of protons in an atom  Mass number is the sum of protons and neutrons  Atomic mass is how much mass is contained in all the particles of an atom. On the Periodic Table it is the average mass of the isotopes.

# 13: Motion vs. Speed  Motion is an object’s change of position relative to a reference point  Speed is the distance traveled over the time it takes to get there; D/T

#14: Speed vs. Velocity  Speed is D/T (m/s)  Velocity is D/T in a certain direction - North, South, East, West (m/s East)  When you know speed and direction, you can determine velocity  Acceleration is the change in velocity over time (m/s ² South) V 2 – V 1 T 2 - T 1

#15: Static vs. Kinetic friction  Static friction – friction that does not allow movement  Kinetic friction – friction that allows movement  Static – Trying to move a ton of concrete blocks  Kinetic – Sliding a book

#1 Be able to… A pure substance is the smallest sample of matter where there is only one type of particle (an atom or molecule). Elements and compounds are both considered the smallest samples of matter. A single element or a single compound (elements combined chemically) have definite physical and chemical properties.

#4: Be able to….  Compounds are the chemically combined atoms of elements whose smallest particle is a molecule

#5: Be able to…  By spinning around, orbiting or changing direction

#6 & 7: Be able to…  Exothermic – heat out. For example, freezing  Endothermic – heat in. For example, melting

#8: Be able to calculate…  Density – M/V – 1 st you have to calculate volume – L x W x H (or by water displacement cm³), then divide mass by your answer  Speed – D/T  Acceleration – V 2 – V 1 T 2 - T 1  Net Force 5 N East and 8 N West Net Force = 3 N West