chem final

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speed of light: c = wavelength ( frequency )
Gay-Lussac's Law: p1/t1 = p2/t2
monatomic ions: ions consisiting of only one atom, charges can be determined using the periodic table
physical property: quality of a substance that can be observed or measured without changing the substance's composition example color
stoichiometry: the calculations of quantities in a chemical reaction (when you know one substance, you can calculate the quantity of any other substance in the reaction)
compounds: 2 or more elements chemically combined
noble gases: only elements that exist as isolated atoms (monatomic)
distillation: a liquid is boiled to produce a vapor which is condensed back into a liquid. Solid substances originally dissolved in the liquid are left behind when the liquid turns to vapor.
ions: atoms or groups of atoms with a positive or negative charge, formed when electrons are lost or gained
density: measured in grams per cubic cm (g/cm^3) or grams per mililiter (g/mL)
spectator ions: ions not directly involved in a reaction
atomic number: number of protons in the nucleus of an atom, identifies the element, equals the number of electrons
incomplete combustion: occurs when there is insufficient O2. Could also be a combination reaction.
qualitative measurements: gives results in a descriptive, nonnumerical form "it's warm out"
mass: measure of the amount of matter in a substance, never changes
skeleton equations: doesn't show the amount of the reactants and products
formula unit: used to represent an ionic compound, shows the ratio of ions in the compound
calculating molecular formulas from empirical formulas: calculate the mass of the empirical formula, divide the molar mass by this, and use this number to multiply the empirical formula
mass: amount of matter in an object
pauli exclusion principal: each orbital can only hold two electrons, and they spin in opposite directions
hypothesis: a proposed reason for the observation ("educated guess")
precision: how close a series of measurements are to one another
mili: 1000 times smaller
excited state: takes a quantum of energy to raise an electron to its excited state, and as it drops back a quantum of energy is emmitted in light
sublevels: electrons occupy these within the principal energy levels... same as the quantum number of the energy level
tenary compounds: composed of three different elements, usually contain a polyatomic ion (KNO3)
tetra: 4
diatomic molecule: molecule that consists of 2 atoms
mixture: physical blend of 2 or more substances
percent yield: precent yield = actual yield / theoretical yield x 100. Should not be greater than 100, but might be less than for many reasons.
gas: matter with neither a definite shape nor volume, compressible, takes shape and volume of container
scientific method: observation, hypothesis, experiment, and then theory
periodic law: when elements are arranged in order of increasing atomic number there is a periodic repetiton of their physical and chemical properties. Elements with similar properties end up in the same column.
hund's rule: one electron enters each orbital before any enter 2
gas pressure: depends on the number of gas particles in a given volume and their average kinetic energy... does not depend on type of particles
amplitude: hieght of wave
Kinetic theory of gases: the volumes of gas particles are insignifigant, they are compressible, there are no forces of attration between particles, and they move rapidly in constant motion
molecular compounds: compounds composed of molecules, have low boiling points, are gases or liquids at room temperature (bond covalently)
homogeneous mixture: uniform composition (ex: salt water)
aufbau principal: electrons enter orbitals of lowest energy level first
liquid: matter with a definite volume but no definite shape, particles in close contact but NOT rigid, takes shape of container, expands when heated
Heisenberg Uncertainty Principle: It is impossible to know both the velocity and the position of a particle at the same time
decompostition reaction: 1 compound is broken down into two or more products. Usually requires energy in the form of heat, light, or electricity.
signs that a chemical reaction may have occured: energy is obsorbed or given off, change in color, change in odor, production of gas or solid from liquid, irreversibility
chemical property: ability of a substance to undergo a chemical reaction
anions: negatively charged ions
anions: atoms of nonmetals tend to gain 1 or more electrons
mega: 1 million times larger
theory: thoroughly tested model that explains why experiments give certain results
mass: measured in kilograms (kg)
dissociation: ionic compound breaks into seperate anions and cations in water
deci: 10 times smaller
combined gas law: p1 x v1/ t1 = p2 x v2/ t2
metals: found on left side of table, ductible, malleable, solid at room temperature
weight: measure of the pull of gravity on an object, can change with location
atomic mass: weighted average of the mass of the atoms in a naturally occuring sample of an element
binary molecular compounds: composed of two nonmettalic charges, no ionic charges are involved. When naming, use prefixes to identify how many atoms of each element are present
atomic mass unit: unit created to compare the masses of atoms, equal to the mass of one proton
binary compounds: composed of two different elements, positive cation must balance the charge of the negative anion
phase: part of a system with uniform composition
prinicipal energy level: distance of the electron from the nucleus with increasing values
volume: space occupied by a sample of matter, measured in cubic meters (m^3) or liters (L), 1 cm^3 = 1 mL
micro: 1 million times smaller
Group 1A: alkali metals
chemical reaction: 1 or more substances change into new substances (chemical change)
theoretical yield: maximum amount of product that could be formed from given amounts of reactants.
molecule: 2 or more atoms that act as a single unit, smallest unit of a substance that has the properties of the substance
pressure: measured in pascals (Pa), atmospheres (atm),
Group A elements: Groups 1A-7A and 0
chemical equations: formulas of reactants and products used
exceptions to aufbau rule: chronium (24 electrons) and copper (29 electrons)
temperature: measured in kelvins (K) or degrees Celsius (oC), measure of the average kinetic energy of particles in matter
chemical formula: shows the kinds and numbers of atoms in the smallest unit of a substance
Dalton's atomic theory: 1) all elements are made of atoms 2) atoms of the same element are identical 3) atoms of different elements can combine in whole number ratios to form compounds 4) Chemical reactions occur when atoms are seperated, joined, or rearranged.
density: how much matter is in a given amount of space, D=M/V (Density = mass/volume)
mass number: total number of protons and neutrons in an atom
analytical chemistry: study of the composition of substances
products: substances formed, written on the left of the arrow
amount of a substance: measured in moles
heterogeneous mixture: not uniform in composition (ex: salad)
nonmetals: found in upper right corner, poor conductors, nonlustrous, some are gases at room temp
mass-mass calculations: 1. balance equation 2. convert mass to moles. 3. use mole ratio to find moles of other substances 4. convert moles back to mass
(aq): aqueous, substance dissolved in water
quantum mechanical model: estimates the probabilty of finding an electron in a certain place... electron clouds show where the electron is 90% of the time
polyatomic ions: tightly bound groups of atoms that act as one and carry a charge
ground state: lowest energy level of an electron in an atom
heterogeneous mixtures: has two or more phases
error: accepted value - experimental value
scientific law: concise statement that summarizes the results of many experiments, describes a natural phenomenon without attempting to explain it
Charles's Law: v1/t1 = v2/t2
solid: matter with a definite shape and volume, rigidly packed particles, expands only slightly when heated
complete combustion: produces CO2 and H2O
Dmitri Mendeleev: created the first periodic table, arranged elements by increasing atomic mass
7 diatomic elements: H, F, O, N, Cl, Br, I
specific gravity: comparison of the density of a substance with the density of a reference substance, = density of a substance/ density of water
shorthand notation for elements: mass number above atomic number
combination reaction: 2 or more substances combine to form a single substance. Product is always a compound.
biochemistry: study of the chemistry of living organisms
electron configuration: the way electrons are arranged around the nucleus
law of conservation of mass: in any physical change or chemical reaction, mass is neither created nor destroyed
accuracy: how close a measurement comes to the true value
nano: 1 billion times smaller
spectrum: colors produced when sunlight passes through a prism
quantum: amount of energy nessesary for an electron to jump to the next higher energy level
Boyles law: p1 x v1 = p2 x v2
Group 2A: alkali earth metals
length: measured in meters (m)
cations: when atoms of metals tend to lose 1 or more electrons
ideal gas law: P X V = n X R X T
nona: 9
excess reagant: reagant not completely used up in a reaction
limiting reagant: the reactant that limits the amount of product that can be made in a reaction... the reaction can no longer occur after this has been used up
frequency: number of waves to pass a given point per unit of time
empirical formula: gives the lowest whole number ratio of the atoms in the compound... tells you the kinds and numbers of atoms in a compound
penta: 5
inorganic chemistry: study of substances that do not contain carbon
International System of Units: "SI", revised version of the metric system, used by worldwide science community
single-replacement reaction: 1 element replaces a second element in a compound. Need to use Activity Series of Metals to tell whether one will replace the other. Any metal on the series will replace the metal below it.
kilo: 1000 times larger
Avagadro's hypothesis: equal volumes of gases at the same temperature and pressure contain equal numbers of particles
percent error: IerrorI/accepted value x 100
isotopes: atoms with the same number of protons but different numbers of neutrons (same atomic numbers but different mass numbers)
ionic compounds: compounds made of anions and cations, usually composed of metal cations and nonmetal anions, usually solid crystal at room temperature
ideal gas: gas that follows gas laws at all temperatures and pressures, conforms to all part of the kinetic theory, do not exisit, cant be liquified or solidified
physical chemistry: study of the behavior of chemicals, relies on math and physics
Henry Moseley: created a periodic table arranging the elements in order of increasing atomic number
hexa: 6
triatomic molecule: molecule that consists of 3 atoms
Group 7A: halogens
energy level: region around the nucleus where electron is likely to be moving... the higher the energy level, the easier it is for an electron to escape the atom
observation: the use of the senses to obtain information directly
centi: 100 times smaller
time: measured in second (s)
double-replacement reaction: 2 reacting compounds exchange cations. A percipitate usually forms, or a gas bubbles out, or a molecular compound like water forms.
experiment: a test of the hypothesis and results should be the same no matter how many times experiment is performed
catalyst: substance that speeds up reaction but is not part of the reaction... niether reactant or product (written above the arrow)
ideal gas constant (R): 8.31 or .0821 if atmospheres are used for pressure
combustion reaction: an element or compound reacts with oxygen
organic chemistry: study of substances that contain carbon
factors affecting gas pressure: amount of gas particles, volume, temperature
hepta: 7
actual yield: the amount of product that actually forms
reactants: starting substances, written left of the arrow
atomic emission spectrum: produced by passing the light emitted by an element through a prism
significant figures: digits in a measurement that are known plus a last digit that is estimated (addition and subtraction: round answer to the same number of decimal places as the least number of decimal places) (multiplication and subtraction: same thing, but with sig figs instead of decimals)
homogeneous mixtures: has one phase
conversion factor: ratio of equivalent measures
variables that describe a gas: pressure, volume, temperature, number of moles
molecular formula: chemical formula of a molecular compound
pico: 1 trillion times smaller
physical change: a change in material that doesn't involve a change in composition; examples: cutting, bending, change in state (freezing, melting)
mole-mole calculations: use mole ratios to find the number of moles of a different substance
quantitative measurements: give results in a definite form (usually as numbers and units) "its 98.4"
matter: anything that has mass and occupies space
elements: cannot be separated into simpler substances by chemical means, building blocks for all other other substances
substance: contains only 1 kind of matter and all samples have the same physical properties
cations: positively charged ions
balancing equations: 1. Count the number of atoms of each element in reactants and products. 2. use coefficiants to balance elements one at a time. 3. Make sure all coefficiants are in lowest ratio
wavelength: distance between crests

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