Ch 1 - Matter, Measurement, and Problem Solving Flashcards
Atom
submicroscopic particles that constitute the fundamental building blocks of ordinary matter.
Molecule
bound together atoms in specific geometric arrangements.
Chemistry
the science that seeks to understand the behavior of matter by studying the behavior of atoms and molecules.
Scientific Approach
Observation, Hypothesis, Experiments, and Law(or Theory). Circular for deeper understanding of the issue.
Observation
Qualitative(describing a process) or quantitative(measuring) review of something in the physical world.
Hypothesis
A tentative interpretation or explanation of the observation. Must be falsifiable.
Experiment
Highly controlled procedures designed to generate observations that may confirm or refute a hypothesis.
Law
A Truth. A brief statement that summarizes past observations and predicts future ones.
Theory
A speculations. One or more well-established hypothesis which become a model for the way nature is and tried to explain both what nature does and why.
The Law of Conservation of Mass
“In a chemical reaction, matter is neither created or destroyed.” -Antoine Lavoisier.
Atomic Theory
John Daltons expansion on Law of Conservation of Mass. Matter is composed of small, indestructible particles called atoms. Atoms are rearranged in chemical changes so no matter is created or destroyed.
Matter
Anything that occupies space and has mass.
Substance
A specific instance of matter.
State
Matters physical form(Solid, liquid, gas)
Composition
the basic components that make up matter.
Solid
atoms closely packed together in fixed positions
Crystalline(solid)
Atoms arranged in patterns with long-range and repeating order. Example: Table salt and Diamond
Amorphous(solid)
Atoms have no long-range order. Example: glass and plastic
Liquid
atoms or molecules pack closely like a solid but are free to move relative to each other. A fixed volume but no fixed shape.
Gas
atoms and molecules have a lot of space between them and are free to move relative to each other.
Compressible(gas)
Gases assume the shape and volume of their container.
Pure Substance
Made of one component and composition is invariant.(100% identical samples) Elements and Compounds.
Mixture
Composed of two or more components in proportion that can vary from one sample to another.
Element
Pure Substance. A substance that can not be broken down into simpler substances.
Compounds
Pure Substance. A substance composed of two or more elements in a fixed definite proportion. Example: Water.
Heterogeneous Mixture
One in which the composition varies from one region of the mixture to another. Example: Wet Sand(not the same everywhere)
Homogeneous Mixture
One with the same composition throughout(uniform composition within the sample). Example: Tea with Sugar.
Decanting(Separating Mixtures)
carefully pouring off a liquid to separate another substance.
Distillation(Separating Mixtures)
Boiling a homogeneous mixture to boil off the more volatile liquid which transfer to a separate flask via a condenser.
Volatile(distillation)
An easily vaporizable liquid which re-condenses in a condenser and collected in a separate flask.
Filtration(Separating Mixtures)
Insoluable solid and a liquid can be separated by pouring the liquid through a filter paper in a funnel(pulls solid out).
Physical Change
Any change that only alters the state or appearance but not composition. Example: Water boiling.
Chemical Change
Any change that alters the composition of matter. Example: Iron rusting.
Physical Property
a property that a substance displays without changing its composition. Example: The smell of gas.
Chemical property
a property that a substance displays only by changing its composition. Example: Flammability of gasoline.
Energy
the capacity to do work.
Work
the action of a force through distance.
Total Energy
Sum of kinetic(motion) and potential(held position) energy.
Kinetic Energy
the energy associated with its motion.
Potential Energy
the energy associated with its position or composition. Higher PE is more unstable.
Thermal Energy
A type of kinetic energy. Energy associated with the temperature of an object.
Law of Conservation of Energy
Energy can change from one type to another however energy is neither created or destroyed in the process.
Unit
Standard quantities used to specify measurements.
Metric System
Used almost everywhere.
English System
Used in the U.S.
International System of Units(SI)
Scientist use this. Based on metric system.
Meter(m)
The standard unit of length.
Kilogram(kg)
the standard unit of mass.
Second(s)
the standard unit of time.
Kelvin(K)
The standard unit of temperature.
Mole(mol)
Standard unit for amount of a substance.
Ampere(A)
Standard unit for electric current.
Candela(cd)
Standard unit for luminous intensity.
Meter(m)/Yard Conversion
Yard=36in. Meter=39.37in.
Mass
The amount of matter in an object.
Weight
The gravitational pull on matter.
Kelvin/Celsius Conversion
K = C + 273.15
Celsius/Fahrenheit Conversion
C = (F - 32) / 1.8 OR F = 1.8(C) + 32
Derived Unit
a combination of other units. Example: m/s.
Volume
A measure of space. Any unit of length when cubed becomes volume. Example: cubic centimeter(cm^3)
Liter(L)
A common unit of volume.
Milliliter(mL)
A common unit of volume. 1 mL = 1cm^3.
Liter(L)/Gallon Conversion
3.785L = 1gal
Length: Kilometer(km)/Mile(mi)
1km = 0.6214mi
Length: Meter(m)/Inches(in)/Yard(yd)
1m = 39.37in = 1.094yd
Length: Foot(ft)/Centimeter(cm)
1ft = 30.48cm
Length: Inch/Centimeter(cm)(exact)
1in = 2.54cm
Mass: Kilogram(kg)/Pound(lb)
1kg = 2.205lb
Mass: Pound(lb)/Gram(g)
1lb = 453.59g
Mass: Ounce(oz)/Gram(g)
1oz = 28.35g
Volume: Liter(L)/Milliliter(mL)/Centimeter^3(cm^3)
1L = 1000mL = 1000cm^3
Volume: Liter(l)/Quart(qt)
1L = 1.057qt
Volume: Gallon(gal)/Liter(L)
1gal = 3.785L
Density
the ratio of its mass(m) to its volume(v). d = m/v
Intensive Property
a property that is independent of the amount of a substance. Example: the density of a substance is constant no matter the amount.
Extensive Property
a property that depends on the amount of a substance. Example: the mass of a substance may change so it can not tell you the type of substance on mass alone.
Density Calculation
d = m/v. 3.15g/0.233cm^3 = 13.5g/cm^3 = Mercury
Significant Figures(digits)
Used to match the precision of a measurement before and after calculations. In a reported measurement the non place holding digits.
Exact Number
numbers with no uncertainty and thus an unlimited amount of significant figures. Example: 3 atoms = 3.0000000… atoms.
Accuracy
how close a measurement is to the actual value desired.
Precision
how close a series of measurements are to one another.
Random Error
error with equal probability of being too high or too low from the target value. may average to the target value but still bad!
Systematic Error
error that tends toward being either too high or too low. Will never average to the target value and needs to be re-calibrated.
Dimensional Analysis
Using units as a guide to solving problems. Include units in the math problem.
Conversion Factor
a fractional quantity with the units we are converting from on the bottom and the units we are converting to on the top. used to cancel out unit symbols and get the value into the appropriate unit.
General Problem-Solving Strategy
Sort information, use strategy to plan the unit conversions, Solve the problem, check the answer.
