Identify and describe the states of matter.
Solid: particles in a solid are closely packed and held tightly in place.
Liquid: particles are still close together but can move past each other, allowing the liquid to flow.
Gas: Particles are well separated and move freely.
Identify and classify matter.
Pure Substances: have distinct properties and composition. - two types of substances:
Elements: cannot be decomposed into simpler substances (represented by a symbol on the periodic table).
Compounds: can be decomposed into simpler substances (is a combination of elements - multiple symbols) EX: H2O
Mixtures: Exhibit the properties of the substances that make them up (multiple substances). Homogeneous: Have the same composition throughout a sample (AKA: liquid). Heterogeneous: vary in composition throughout a sample (EX, dinner salad).
Compare and contrast physical property vs. a chemical process. Give and identify examples of each.
Physical Properties:
can be observed w/ senses.
can be determined w/o destroying matter
Ex: boiling point, density, mass, or volume
Chemical Properties”
indicates how a substance reacts (changes chemically) with something else.
Matter will be changed into a new substance after the reaction
Ex: flammability, corrosiveness, or reactivity with acid
Compare and contrast physical changes vs. chemical changes.
Signs of a chemical change: a new odor, color change, gas production, precipitate (formation of a solid), temp. change (without explicitly adding/removing energy), evolution of gas (bubbles).
Apply conservation of mass to any chemical or physical change. List various forms of energy, explain the role of energy in a chemical change.
In a chemical change…
Law of Conservation of Mass: matter cannot be created or destroyed it can only change form (rearrange).
Law of Conservation of Energy: energy can not be created or destroyed. - many chemical changes either cause energy to be released (heats up) or absorbed (cools down)
Forms of energy: chemical, genetic, nuclear
Describe the properties and units of length, mass, volume, density, temperature, and time.
length - mesures distance - meter (m)
mass - amount of matter - kilogram (kg)
volume - space an object occupies - liter or cubic meter (mL, L, or m3)
density - mass per unit volume (g/mL)
temperature - measure of avg. kinetic energy - Kelvin, Fahrenheit, or Celsius (K, °F or °C)
time - duration of evets - second (s)
Identify the proper unit for matter and the way in which it changes.
Proper Unit: mole (mol)
Ways Matter Changes:
- Physical change – alters form/appearance
- Chemical change – produces new substances
Identify the three basic parts of a measurement
Units, Significant figures, magnitude (the overall value)
Define accuracy and precision.
???
Steps for Writing a Conclusion
Restate Hypothesis/Objective – Briefly restate what the experiment was testing or aiming to find.
Summary of Results – Give the main results and state if they supported or refuted the hypothesis. (specific evidience)
Analysis/Interpretation – Explain patterns or trends in the data, often with an R² value:
0.90–1.00 = strong correlation
0.70–0.89 = reasonable correlation
0.60–0.69 = weak correlation
0.59 or lower = no correlation
Limitations – Note errors or weaknesses in the experiment, including percent error if applicable.
Further Research – Suggest next steps, new experiments, or ways to improve the design.
