Matter, Measurement, and Problem Solving
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| Properties of Matter | The properties of matter are determined by the properties of atoms and molecules
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| Atoms | Submicroscopic particles that constitute the fundamental building blocks of ordinary matter
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| Molecules | Specific geometrical arrangements of atoms
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| Chemistry | The science that seeks to uderstand the behavior of matter by studying the behavior of atoms and molecules
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| Empirical | Based on observations and experiment
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| Qualitative | Noting or describing how a process happens
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| Quantitative | Measuring or quantifying something about the process
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| Hypothesis | A tentative interpretation or explanation of observations
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| Experiments | Highly controlled procedures designed to generate observations that may confirm or refute a hypothesis
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| Scientific Law | A brief statement that summarizes past observations and predicts future ones
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| Law of Conservation of Mass | In a chemical reaction, matter is neither created nor destroyed
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| Theory | A scientific theory is a model for the way nature is and tries to explain not merely what nature does but why
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| Atomic Theory | Matter is composed of small, indestructible particles called atoms
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| Matter | Anything that occupies space and has mass
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| Substance | A specific instance of matter. Ex: air, water, sand
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| State of Matter | Its physical form
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| Composition | The basic components that make it up
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| Matter's 3 States | Solid, Liquid, and Gas
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| Solid Matter | Atoms or molecules pack close to each other in fixed locations. Fixed volume, fixed shape
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| Crystalline Solid Matter | Atoms of molecules are in patterns with longe-range, repeating order. Ex: table salt and diamond
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| Amorphous Solid Matter | Atoms of molecules do not have any longe-range order. Ex: glass and plastic
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| Liquid Matter | Atoms or molecules pack about as closely as they do in solid matter, but are free to move relative to each other. Fixed volume, not fixed shape
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| Gaseous Matter | Atoms or molecules have a lot of space between them and are free to move relative to one another. Gases are compressible.
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| Pure Substance | Matter that is made up of only one component and its composition is invariant(it does not vary from one sample to another)
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| Mixture | Matter that is composed of two or more components in proportions that can vary from one sample to another
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| Element | A substance that cannot be chemically broken down(decomposed) into simpler substances
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| Compound | A substance composed of two or more elements(in this case hydrogen and oxygen) in a fixed, definite proportion
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| Heterogeneous Mixture | A mixture in which the composition varies from one region of the mixture to another
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| Homogeneous Mixture | A mixture with the same composition throughout
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| Decanting | Carefully pouring off
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| Distillation | A process in which the mixture is heated to boil off the more volatile(easily vaporizable) liquid. Often used for homogeneous mixtures
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| Filtration | Mixture is poured through filter paper in a funnel
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| Physical Changes | Changes that alter only state or appearance, but not composition
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| Chemical Changes | Changes that alter the composition of matter
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| Physical Property | A property that a substance displays without changing its composition
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| Chemical Property | A property that a substance displays only by changing its composition via a chemical change
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| Energy | The capacity to do work
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| Work | The action of a force through a distance
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| Total Energy | Sum of kinetic energy(the energy associated with its motion) and its potential energy(the energy associated with its position or composition)
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| Thermal Energy | The energy associated with the temperature of an object
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| Law of Conservation of Energy | Energy is neither created not destroyed
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| Summarizing Energy | Energy is always conserved in a physical or chemical change, it is neither created nor destroyed. Systems with high potential energy tend to change in a direction that lowers their potential energy, releasing energy into the surroundings
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| Units | Standard quantities used to specify measurements
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| Meter | The standard unit of length
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| Kilogram | The standard unit of mass
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| Second | The standard unit of time
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| Kelvin | Standard unit of temperature
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| SI Base Units | 1. Length -- Meter -- m
2. Mass -- Kilogram -- kg
3. Time -- Second -- s
4. Temperature -- Kelvin -- K
5. Amount of Substance -- Mole -- mol
6. Electric Current -- Ampere -- A
7. Luminous Intensity -- Candela -- cd
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| Mass | The measure of the quantity of matter within an object
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| Weight | The measure of the gravitational pull on an object
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| Absolute Zero | The temperature at which molecular motion virtually stops
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| Fahrenheit Scale(°F) | Water Boils(212 °F)..
Water Freezes(32 °F)..
Absolute Zero(-459 °F)
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| Celsius Scale(°C) | Water Boils(100 °C)..
Water Freezes(0 °C)..
Absolute Zero(-273 °C)
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| Kelvin Scale(Absolute Scale)(K) | Water Boils(373 K)..
Water Freezes(273 K)..
Absolute Zero(0 K)
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| Temperature Scale Conversion Formula | °C=(°F - 32) / 1.8..
K=°C + 273.15
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| Prefix Multipliers | 1. Tera
2. Giga
3. Mega
4. Kilo
5. Deci
6. Centi
7. Milli
8. Micro
9. Nano
10. Pico
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| Tera | T -- 1,000,000,000,000 -- 10^12
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| Giga | G -- 1,000,000,000 -- 10^9
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| Mega | M -- 1,000,000 -- 10^6
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| Kilo | k -- 1000 -- 10^3
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| Deci | d -- 0.1 -- 10^-1
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| Centi | c -- 0.01 -- 10^-2
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| Milli | m -- 0.001 -- 10^-3
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| Micro | |U -- 0.000001 -- 10^-6
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| Nano | n -- 0.000000001 -- 10^-9
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| Pico | p -- 0.000000000001 -- 10^-12
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| Derived Unit | Combination of other units. Ex: speed, volume, density
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| Volume | A measure of space
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| Density(d) | Ratio of a substance's mass(m) to its volume(V).
D=M/V
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| Intensive Property | A property that is independent of the amount of the substance. Ex: density
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| Extensive Property | A property that is dependent on the amount of the substance. Ex: mass
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| Scientific measurements | Scientific measurements are reported so that every digit is certain except the last, which is estimated
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| Significant Figures(Digits) | The non-place-holding digits(those that are no simply marking the decimal place). The greater the number of significant figures, the greater the certainty of the measurement
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| 1. Significant Figures Rule | 1. All nonzero digits are significant..
2. Interior zeroes(zeroes between nonzero digits) are significant..
3. Leading zeroes(zeroes to the left of the first nonzero digit) are not significant. They locate the decimal point..
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| 2. Significant Figures Rule | 4. Trailing zeroes(zeroes at the end of a number) are categorized as follows:
Trailing zeroes after a decimal point are always significant..
Trailing zeroes before a decimal point(and after a nonzero number) are always significant..
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| 3. Significant Figures Rule | Trailing zeroes before an implied decimal point are ambiguous and should be avoided by using scientific notation
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| Exact Numbers | Numbers that have no uncertainty and thus do not limit the number of significant figures in any calculation. They have unlimited significant figures
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| Accuracy | How close the measured value is to the actual value
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| Precision | How close a series of measurements are to one another or how reproducible they are
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| Random Error | Error that has equal probability of being too high or too low. Random error can, with enough trails, average itself out
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| Systematic Error | Error that tends toward being either too high or too low. Systematic error does not average itself out with repeated trials
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Created by:
TimChemistry1
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