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Mass
amount of matter
Volume
amount of space an object occupies
Plasma
4th state of matter, ionized gas
Atom
smallest unit of matter
Element
a pure substance made of one type of atom that cannot be broken down to simpler, stable substances
Compound
a substance made up of two or more elements chemically bonded together
Molecule
a group of atoms bonded together, representing the smallest unit that can take part in a chemical reaction
Diatomic element
two atoms of the same element bonded together
Mixture
a blend of two or more kinds of matter, each of which retains its own identity and properties
Homogenous mixture
a mixture in which the composition is the same throughout (ex. Solution)
Heterogeneous mixture
a mixture in which the composition is not the same throughout
Extensive property
does depend on the amount of matter
Extensive property examples
mass, volume, amount of energy
Intensive property
does not depend on the amount of matter
Intensive property examples
density, b.p., m.p., conductivity
Metals
solids at room temp, luster, malleable, ductile, conductors
Nonmetals
liquids and gases at room temp, brittle, poor conductors
Metalloids
solids at room temp, luster, semi-conductors
Distillation
separating liquids based on boiling point
Decanting
separating a solid and a liquid by pouring off the liquid after the solid settles
Filtering
separating a solid and a liquid by pouring the mixture into a filter - the liquid will pass through but the solid will remain
Evaporation
a method to separate water from a dissolved liquid
Chromatography
passing a mixture a medium where the compounds move at different rates
Accuracy
closeness of a measurement to the accepted value
Precision
closeness of a group of measurements
Percent error
used to determine accuracy
Percent error formula
[(experimental - accepted) / accepted] x 100
Significant figures
all the digits known with certainty plus an estimated digit
Sig Fig Rules
All nonzero integers are significant; Captive zeroes are always significant; Leading zeroes are never significant; Trailing zeroes are significant if there is a decimal point.
add/sub whole number sig fig rule
the final sig fig is in the same place value as the left most uncertain digit
add/sub decimal sig fig rule
as many decimal places as the least precise piece of data
multiply/divide sig fig rule
as many total sig figs as the least precise piece of data
Scientific method
a logical approach to solving a problem
Quantitative data
numerical data
Qualitative data
observations made using senses
Control
the standard used for comparison in an experiment
Theory
hypothesis that has withstood many tests
Density
ratio of mass to volume (m/V)
Law of Conservation of Mass
mass is neither created nor destroyed during ordinary chemical reactions or physical changes
Law of Definite Proportions
A single chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound
Law of Multiple Proportions
if two or more compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers
Dalton's Atomic Theory
All matter is composed of small particles called atoms; Atoms of an element are identical in size, mass, and other properties; Atoms cannot be subdivided, created, or destroyed; Atoms of different elements combine in simple whole number ratios to form compounds.
Thompson's Atomic Theory
concluded that negatively charged particles called electrons existed - atoms are electrically neutral, so atoms must contain a positive charge to balance the negative electrons
Cathode ray tube experiment
rays were deflected away from negatively charged objects
Millikan's conclusions
used the charge to mass ratio to determine the mass of an electron (so small it's considered negligible), concluded that other particles must be present to account for the mass
Oil drop experiment
measured the charge of an electron
Rutherford's conclusions
the alpha particles hit something small and dense, called a nucleus
Gold Foil experiment
1 in 8000 alpha particles were deflected back
Isotopes of hydrogen
protium (no neutron), deuterium (1 neutron), tritium (2 neutrons)
Alpha emission
least penetrating, blocked by a sheet of paper
Alpha particle
42He
Beta emission
more penetrative, blocked by aluminum foil
Beta symbol
0-1e- OR 0-1β
Positron emission
more penetrative, stopped by aluminum foil
Positron symbol
0+1e- OR 0+1β
Gamma emission
electromagnetic radiation, stopped by lead
Gamma symbol
00Ƴ
Symbol for an isotope
hyphen notation (ex. Hydrogen-1)
Extensive property
Does depend on the amount of matter.
Extensive property examples
Mass, volume, amount of energy.
Intensive property
Does not depend on the amount of matter.
Intensive property examples
Density, boiling point (b.p.), melting point (m.p.), conductivity.
Metals
Solids at room temperature, luster, malleable, ductile, conductors.
Nonmetals
Liquids and gases at room temperature, brittle, poor conductors.
Metalloids
Solids at room temperature, luster, semi-conductors.
Distillation
Separating liquids based on boiling point.
Decanting
Separating a solid and a liquid by pouring off the liquid after the solid settles.
Filtering
Separating a solid and a liquid by pouring the mixture into a filter - the liquid will pass through but the solid will remain.
Evaporation
A method to separate water from a dissolved liquid.
Chromatography
Passing a mixture through a medium where the compounds move at different rates.
Accuracy
Closeness of a measurement to the accepted value.
Precision
Closeness of a group of measurements.
Percent error
Used to determine accuracy.
Percent error formula
[(experimental - accepted) / accepted] x 100.
Significant figures
All the digits known with certainty plus an estimated digit.
Sig Fig Rules
Rules that determine which digits are significant in a number.
Scientific method
A logical approach to solving a problem.
Quantitative data
Numerical data.
Qualitative data
Observations made using senses.
Control
The standard used for comparison in an experiment.
Theory
Hypothesis that has withstood many tests.
Density
Ratio of mass to volume (m/V).
Law of Conservation of Mass
Mass is neither created nor destroyed during ordinary chemical reactions or physical changes.
Law of Definite Proportions
A single chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound.
Law of Multiple Proportions
If two or more compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers.
Dalton's Atomic Theory
All matter is composed of small particles called atoms.
Thompson's Atomic Theory
Concluded that negatively charged particles called electrons existed.
Cathode ray tube experiment
Rays were deflected away from negatively charged objects.
Millikan's conclusions
Used the charge to mass ratio to determine the mass of an electron.
Oil drop experiment
Measured the charge of an electron.
Rutherford's conclusions
The alpha particles hit something small and dense, called a nucleus.
Gold Foil experiment
1 in 8000 alpha particles were deflected back.
Isotopes of hydrogen
Protium (no neutron), deuterium (1 neutron), tritium (2 neutrons).
Alpha emission
Least penetrating, blocked by a sheet of paper.
Beta emission
More penetrative, blocked by aluminum foil.
Positron emission
More penetrative, stopped by aluminum foil.
Gamma emission
Electromagnetic radiation, stopped by lead.
Symbol for an isotope
Hyphen notation (ex. Lithium - 7).
Heterogeneous mixture
a mixture in which the composition is not the same throughout (ex. Milk, blood, trail mix)
Dalton's Atomic Theory
All matter is composed of small particles called atoms; Atoms of an element are identical in size, mass, and other properties; Atoms cannot be subdivided, created, or destroyed; Atoms of different elements combine in simple whole number ratios to form compounds
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