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119 Cards in this Set
- Front
- Back
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atoms
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submicroscopic particles; fundamental building blocks of all matter
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molecules
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two or more atoms attached together (attachments are called bonds and attachments come in different strengths)
molecules come in different shapes and patterns |
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chemistry
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the science that seeks to uderstand the behavior of matter by studying the behavior of atoms and molecules
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the scientific method
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trying to understand the universe through empirical knowledge gained through observation and experiment
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hypothesis
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a tentative interpretation or explanation for an observation
falsifiable can be tested |
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atoms
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submicroscopic particles; fundamental building blocks of all matter
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molecules
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two or more atoms attached together (attachments are called bonds and attachments come in different strengths); molecules come in different shapes and patterns
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chemistry
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the science that seeks to uderstand the behavior of matter by studying the behavior of atoms and molecules
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the scientific method
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trying to understand the universe through empirical knowledge gained through observation and experiment
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hypothesis
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a tentative interpretation or explanation for an observation; falsifiable; can be tested
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scientific law
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occurs when similar observations are consistently made
behavior is always observed summarizes past observations and predicts future ones example: law of conservation of mass |
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theory
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general exlanation for the manifestation and behavior of all nature; models; Nobel Prize worthy; validated or invalidated by experiment and observation
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matter
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anything that has mass and occupies space; we can classify matter based on whether it's solid, liquid, or gas
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solid
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fixed shape, fixed volume, no compress, and no flow
packed close together |
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liquid
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indefinite shape, fixed volume, no compress, and flow
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scientific law
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occurs when similar observations are consistently made; behavior is always observed; summarizes past observations and predicts future ones; example: law of conservation of mass
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theory
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general exlanation for the manifestation and behavior of all nature; models; Nobel Prize worthy; validated or invalidated by experiment and observation
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matter
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anything that has mass and occupies space; we can classify matter based on whether it's solid, liquid, or gas
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solid
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fixed shape, fixed volume, no compress, and no flow
packed close together |
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liquid
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indefinite shape, fixed volume, no compress, and flow
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gas
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indefinite shape, indefinite volume, compress, and flow
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crystalline solids
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solids that have their particles arranged in an orderly geometric pattern (i.e. salt, diamonds)
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amorphous solids
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solids that have their particles randomly distributed without any long-range pattern (i.e. plastic, glass, charcoal)
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pure substances
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made of one type of particle; all samples show the same intensive properties
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mixture
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made of multiple types of particles; samples may show different intensive properties
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gas
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indefinite shape, indefinite volume, compress, and flow
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crystalline solids
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solids that have their particles arranged in an orderly geometric pattern (i.e. salt, diamonds)
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amorphous solids
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solids that have their particles randomly distributed without any long-range pattern (i.e. plastic, glass, charcoal)
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pure substances
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made of one type of particle; all samples show the same intensive properties
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mixture
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made of multiple types of particles; samples may show different intensive properties
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pure substances - element
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made of one type of atom (some elements found as multi-atom molecules in nature); combine together to make compounds
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pure substances - compound
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made of one type of molecule, or array of ions; molecules contain 2 or more different kinds of atoms
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mixtures - heterogenous
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made of multiple substances, whose presence can be seen; portions of a sample have different composition and properties
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mixtures - homogenous
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made of multiple substances, but appears to be one substance; all portions of a sample have the same composition and properties
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separation of mixtures
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physical property : technique
boiling point : distillation state of matter (solid/liquid/gas) : filtration adherence to a surface : chromatography volatility : evaporation density : centrifugation & decanting |
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physical properties
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characteristics of matter that can be changed without changing its composition; directly observable
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chemical properties
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characteristics that determine how the composition of matter changes as a result of contact with other matter or the influence of energy; describe the behavior of matter
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physical changes
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changes that alter the state or appearance of the matter without altering the composition
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chemical changes
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changes that alter the composition of the matter; during the chemical change, the atoms that are present rearrange into new molecules, but all of the original atoms are still present
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energy
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the capacity to do work; changes in matter, result in gaining or releasing energy
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work
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the action of a force applied across a distance; a force is a push or a pull on an object; electrostatic force is the push or pull on objects that have an electrical charge
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energy of matter
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all matter possesses energy; energy is either kinetic or potential; energy can be converted from one form to another; when matter undergoes a chemical or physical change, the amount of energy in the matter changes as well
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kinetic energy
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energy of motion; atoms, molecules, and subatomic particles; thermal (heat) energy is a form of kinetic energy because it is caused by molecular motion
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potential energy
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energy that is stored in matter; due to the composition of the matter and its position in the universe; chemical potential energy arises from electrostatic forces between atoms; molecules, and subatomic particles
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law of conservation of energy
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whatever process you do that converts energy from one type or form to another, the total amount of energy remains the same
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SI units
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international system
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temperature
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measure of the average amount of kinetic energy (higher temperature = larger average kinetic energy)
SI unit - Kelvin = C + 273.15 |
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volume
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measure of the amount of space occupied
SI unit = cubic meter (m^3) |
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density
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ratio of mass:volume (intensive property - value independent of the quantity of matter)
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significant figures
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the non-place-holding digits in a reported measurement; tell us the range of values to expect for repeated measurements
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multiplication and division of significant figures
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the result has the same number of significant figures as the measurement with the fewest number of significant figures
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addition and subtraction of significant figures
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the result has the same number of decimal places as the measurement with the fewest number of decimal places
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accuracy
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an indication of how close a measurement comes to the actual value of the quantity
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precision
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an indication of how reproducible a measurement is
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Which philosophers believed that matter was infinitely divisible?
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Plato and Aristotle
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Scanning Tunneling Microscope
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movement of tip is used to create an image with atomic resolution; tunneling current is extremely sensitive to distance; tip is scanned across surface and moved up and down to maintain constant tunneling current
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law of conservation of mass
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in a chemical reaction, matter is neither created nor destroyed; total mass of reactants = total mass of products
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Who created the Law of Conservation of Mass?
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Antoine Lavoisier (1743 - 1794)
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law of definite proportions
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all samples of a compound have the same proportions of their constituent elements (i.e. water)
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Who created the Law of Definite Proportions?
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Joseph Proust (1754 - 1826)
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law of multiple proportions
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when two elements, (call them A and B), form two different compounds, the masses of B that combine with 1 g of A can be expressed as a ratio of small, whole numbers
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Who created the Law of Multiple Proportions?
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John Dalton (1766 - 1844)
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Dalton's Atomic Theory
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1. each element is composed of tiny, indestructible particles called atoms
2. all atoms of a given element have the same mass and other properties that distinguish them from atoms of other elements 3. atoms combine in simple, whole-number ratios to form molecules of compounds 4. in a chemical reaction, atoms of one element cannot change into atoms of another element |
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J.J. Thomson's Experiment
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purpose: investigate the effect of placing an electric field around tube
1. charged matter is attracted to an electric field 2. light's path is not deflected by an electric field conclusions: charge of electron; atom is not unbreakable |
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electrons
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particles found in all atoms; cathode rays are streams of electrons
charge: -1.60 x 10^19 C mass: 9.1 x 10^-28 g |
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Thomson's Plum Pudding Atom
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electrons are held in the atom by their attraction for a positively charged electric field within the atom
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Plum Pudding Atom Predictions
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the mass of the atom is due to the mass of the electrons within it > electrons are the only particles in Plum Pudding atoms; the atom is mostly empty space > cannot have a bunch of negatively charged particles near each other as they would repel
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Rutherford's Experiment
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"how can you prove something is empty?" > put something through it; bullet = alpha particles, target atoms = gold foil; alpha particles have a mass of 4 amu & charge of +2 c.u.; gold has a mass of 197 amu & is very malleable
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Rutherford's Results
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over 98% of the alpha particles went straight through; about 2% went through but were deflected by large angles; about .01% bounced off the gold foil > the atom is mostly empty space; contains a dense particle that was small in volume compared to the atom but large in mass; this dense particle was positively charged
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Rutherford's Interpretation - the Nuclear Model
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1. the atom contains a tiny dense center called the nucleus
2. the nucleus has essentially the entire mass of the atom 3. the nucleus is positively charged 4. the electrons are dispersed in the empty space of the atom surrounding the nucleus |
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protons
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positively charged particles found in the nucleus of atoms
charge = 1.60 x 10^19 C mass = 1.67262 x 10^-24 g |
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neutron
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particle found in the nucleus of atoms with no charge
mass = 1.67493 x 10^-24 g (slightly heavier than a proton) = 1 amu |
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atomic number
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the number of protons in the nucleus of an atom; defines each element
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isotopes
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atoms of the same elements with different masses (more or less neutrons)
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natural abundance
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the percentage of an element that is 1 isotope
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qualities of isotopes
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chemically identical > undergo the exact same chemical reactions; same number of protons (Z); different masses; different numbers of neutrons; identified by their mass numbers (A) > protons + neutrons; abundance = relative amount found in a sample
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ions
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charged particles (formed when atoms gain or lose electrons); behave much differently than the neutral atom
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anions
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negatively charged atoms (that have gained electrons)
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cations
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positively charged ions (that have lost electrons)
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nonmetals form _ _ _ _ _ _
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anions
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anions are named by changing the ending of the name to -_ _ _
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ide
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metals for _ _ _ _ _ _ _
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cations
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cations are named the same as the _ _ _ _ _
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metal
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Mendeleev
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order elements by atomic mass; saw a repeating pattern of properties; periodic law; put elements with similar properties in the same column; made predictions for undiscovered elements
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Periodic Law
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when the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically
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metals
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solid at room temperature, except Hg; reflective surface (shiny); conduct heat and electricity; malleable (can be shaped); ductile (drawn or pulled into wires); lose electrons and form cations in reactions
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nonmetals
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found in all 3 states; poor conductors of heat & electricity; solids are brittle; gain electrons in reactions to become anions; upper right on the table (except H)
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metalloids
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show some properties of metals and some of nonmetals; also known as semiconductors
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alkali metals
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group 1A, except H; soft, low melting points; low density; very reactive; tend to form water-soluble compounds (colorless)
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alkali earth metals
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group 2A; harder, higher melting, and denser than alkali metals; reactive; form stable, insoluble oxides from which they are normally extracted
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halogens
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group 7A; nonmetals, F2 and Cl2 gases; Br2 liquid; I2 solid; diatomic; very reactive; HX all acids
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noble gases
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group 8A; all gases at room temperature; very unreactive; very hard to remove electron from or give an electron to
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Mendeleev
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order elements by atomic mass; saw a repeating pattern of properties; periodic law; put elements with similar properties in the same column; made predictions for undiscovered elements
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Periodic Law
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when the elements are arranged in order of increasing atomic mass, certain sets of properties recur periodically
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metals
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solid at room temperature, except Hg; reflective surface (shiny); conduct heat and electricity; malleable (can be shaped); ductile (drawn or pulled into wires); lose electrons and form cations in reactions
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nonmetals
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found in all 3 states; poor conductors of heat & electricity; solids are brittle; gain electrons in reactions to become anions; upper right on the table (except H)
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metalloids
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show some properties of metals and some of nonmetals; also known as semiconductors
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alkali metals
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group 1A, except H; soft, low melting points; low density; very reactive; tend to form water-soluble compounds (colorless)
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alkali earth metals
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group 2A; harder, higher melting, and denser than alkali metals; reactive; form stable, insoluble oxides from which they are normally extracted
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halogens
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group 7A; nonmetals, F2 and Cl2 gases; Br2 liquid; I2 solid; diatomic; very reactive; HX all acids
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noble gases
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group 8A; all gases at room temperature; very unreactive; very hard to remove electron from or give an electron to
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atomic mass
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the average mass of all the isotopes of an element
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mass spectrometer
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used to measure the masses and abundances of isotopes
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mass spectrum
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a graph that gives the relative mass and relative abundance of each particle
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mole
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the number of atoms: 6.033 x 10^23 (things)
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Avogadro's Number
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6.0221421 x 10^23
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molar mass
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the mass of one mole of atoms
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1 amu = 1 _ / mol
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gram
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chemical bonds
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bonds that hold together compounds
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bonds
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forces of attraction between atoms (the bottom attraction comes from attractions between protons and electrons)
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ionic bonds
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when electrons have been transferred between atoms, resulting in oppositely charged ions; generally found when metal atoms bond with nonmetal atoms
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covalent bonds
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when two atoms share some of their electrons; generally found when when nonmetal atoms bond together
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empirical formula
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describe the kinds of elements found in the compound and the ratio of their atoms
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molecular formula
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describe the kinds of elements found in the compound and the numbers of their atoms
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structural formula
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describe the kinds of elements found in the compound, the numbers of their atoms, order of atom attachment, and the kind of attachment
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atomic elements
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elements whose particles are single atoms
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molecular elements
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elements whose particles are multi-atom molecules
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molecular compounds
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compounds whose particles are molecules made of only nonmetals
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ionic compounds
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compounds whose particles are cations and anions
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