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103 Cards in this Set

  • Front
  • Back
Matter
anything that has mass and occupies space
energy
the capacity to do work or to transfer heat
kinetic energy
represents the capactiy for doing work directly
potential energy
energy an object possesses because of its position
Law of Conservation of Matter
there is no observable change in the quantity of matter during a chemical reaction or during a physical change
Law of Conservation of Energy
energy cannot be created or destroyed in a chemical reaction or in a physical change. It can only be converted from one form to another
Law of Conservation of Matter and Energy
The combined amount of matter and energy available in the universe is fixed
Daltons Atomic Theory
1. An element is composed of extremely small, indivisible particles called atoms
2. All atoms of a given element have identical properties that differ from those of other elements
3. Atoms cannot be created, destroyed, or transformed into atoms of another element in chemical or physical changes
4. Compounds are formed when atoms of different elements combine with one another in small whole-number ratios
5. The relative numbers and kinds of atoms are constant in a given compound
atoms
the smallest particle of an element that maintains its chemical identity through all chemical and physical changes
molecules
smallest particle of an element or compound that can have a stabe independent existence
Which elements exist in nature as diatomic molecules?
Hydrogen, nitrogen, fluorine, chlorine, bromine, and iodine
Chemical properties
undergoes change in composition
physical properties
absence of any change in composition
Mixtures
combination of two or more substances in which each substances retains its own composition and properties
variable composition, components retain their characteristic properties,

may be separated into pure substances by physical methods
pure substances
fixed composition, cannot be separated into simpler substances by physical methods, can only be changed in identity properties by chemical methods, under identical conditions, properties do not vary
homogeneous
(solution) kind of mixture that has uniform properties throughout
heterogeneous
mixture in which different portions of the sample have recognizably different properties
compounds
substance that can be decomposed by chemical means into simpler substances
element
substance that cannot be decomposed into simpler substances by chemical changes
Law of Definite Proportions( Law of Constant Composition)
different samples of any pure compound contain the same elements in the same proportions by mass
length
meter
mass
kg
time
s
temp
K
mass
measure of quantity of matter a body contains
weight
measure of the gravitational attraction of the earth for the body
Most common temperatures
C, F, K
Solids
have molecules that are packed together tightly
Liquids
made of molecules that are close but can still move around
gases
made up of free-moving molecules
Fluids are:
liquids and gases because they flow freely
Solids and liquids are referred to:
condensed states because they have much higher densities then gases
miscible
they mix completely unless they mix with one another
pressure
force per unit area
barometer
measures atmospheric pressure
manometer
measures the pressure of a gas
What are the two main gases in clean, dry, air? What are their approximate %'s?
N_2 - 78%, 0_2 - 20.94%, Ar - .93%
What is the typical pressure of the atmosphere in our classroom in pounds per square inch? atmospheres? torr? mm of mercury? inches of mercury?
14.69 PSi
What is the greenhouse effect?
CO_2 and H_2O absorb the heat from the earth and keep it trapped in the atmosphere, warming the earth
What are the primary greenhouse gases?
CO_2 and H_2O
What is the relationship between the greenhouse effect and global warming?
because the energy from the earth is trapped, the world warms up and then it disturbs the ecosystems
What are some possible problems from global warming?
ice melting planting seasons, rain cycles
Boyles Law
For a gas at a constant temp, the volume and pressure is always the same number
Charles' Law
at a constant temperature, the volume occupied by a definite mass of a gas is directly proportional to its absolute temperature
Atomic number
the number of protons in the nucleus of an atom
Heat
a form of energy that flows between two samples of matter because of their difference in temperature
Law of Definite Proportions (Law of Constant Composition)
Different samples any pure compound contain the same elements in the same proportions by mass
Mixture
A sample of matter composed variable amounts of two or more substances, each of which retains its identity and properties
Properties
characteristics that describe samples of matter
Specific gravity
the ratio of the density of a substance to the density of water at the same temp
Substance
any kind of matter all specimens of which have the same chemical composition and physical properties
Allotropes
different forms of the same element in the same physical state
Anhydrous
without water
Anion
An ion with a negative charge
Atomic mass unit (amu)
One twelfth of the mass of an atom of the carbon-12 isotope; a unit used for starting atomic and formula weights
Cation
A ion with a positive charge
Chemical formula
Combination of element symbols that indicates the chemical composition of a substance
Composition stoichiometry
describes the quantitative relationships among elements in compounds
Formula
Combination of element symbols that indicates the chemical composition of a substance
Formula unit
the smallest repeating unit of a substance-for non-ionic substances, the molecule
Hydrate
A crystalline sampe that contains water, H20, and another compound in a fixed mole ratio
Ion
An atom or group of atoms that carries an electric charge
Ionic compound
A compound that is composed of cations and anions
Law of Definite Proportions
Different samples of a pure compound always contain the same elements in the same proportions by mass
Law of multiple proportions
when two elements form more than a compound,
Molar mass
the mass, in grams, of one mole of a substance; numerically equal to the formula weight of the substance
Mole
(Avogradro's number) formula units molecules of a substance. The mass, in grams, of one mole is numerically equal to the formula weight of the substance
Molecular formula
A formula that indicates the actual number of atoms present in a molecule of a molecular substance
Molecular weight
the mass, in amu, of one molecule of a non-ionic (molecular) substance
Percent composition
The mass percentage of each element in a compound
Percent purity
The mass percentage of a specified compound or element in an impure sample
Polyatomic
Consisting of more than one atom
Simplest formula
the smallest whole-number ratio of atoms present ina compound
Stoichiometry
description of the quantitative relationships among elements in compounds (composition stoichiometry) and among substances as they undergo chemical changes
Structural formula
A representation that shows how atoms are connected in a compound
Absolute zero
The zero point on the absolute temperature scale
-273.15C or O K
Atmosphere (atm)
A unit of pressure
Avogadro's Law
At the same temperature and pressure equal volumes of all gases contain the same number of molecules
Bar
A unit of pressure
Barometer
A device for measuring atmospheric pressure
Boyle's Law
At constant temp, the volume occupied by a given mass of a gas is inversely proportional to the applied pressure
Charles' Law
At constant pressure, the volume occupied a definite mass of a gas is directly proportional to its absolute temp
Condensed states
The solid and liquid states
Dalton's Law of Partial Pressures
The total pressure exerted by a mixture of gases is the sum of the partial pressures of the individual gases
Diffusion
The movement of a substance into a space or the mixing of one substance with another
Dispersion forces
Weak, short-range attractive forces between short-lived temporary dipoles
Effusion
The escape of a gas through a tiny hole or a thin porous wall
Fluids
Substances that flow freely; gases and liquids
Gay-Lussac's Law of Combining Volumes
At constant temperature and pressure, the volumes of reacting gases (and any gaseous products) can be expressed as ratios of small whole numbers
Ideal gas
A hypothetical gas that obeys exactly all postulates of the kinetic-molecular theory
Ideal gas equation
The product of the pressure and volume of an ideal gas is directly proportional to the number of moles of the gas and the absolute temperature
Kinetic-molecular theory
A theory that attempts to explain macroscopic observations of gases in microscopic or molecular terms
Manometer
A two-armed barometer
Partial pressure
The pressure exerted by one gas in a mixture of gases
Pascal (Pa)
The SI unit of pressure
Pressure
Force per unit area
Standard molar volume
The volume occupied by one mole of an ideal gas under standard conditions
Standard temperature and pressure (STP)
Standard temperature 0C (273.15K) and standard pressure, one atmosphere, are standard conditions for gases
Torr
A unit of pressure
Universal gas constant
The proportionally constant in the ideal gas equation, PV=nRT
van de Waals equation
An equation of state that extends the ideal gas law to real gases by inclusion of two empirically determined parameters, which are different for different gases
Vapor
A gas formed by boiling or evaporation of a liquid or sublimation of a solid; a term commonly used when some of the liquid or solid remains in contact with the gas
Vapor pressure
The pressure exerted by a vapor in equilibrium with its liquid or solid