Set: Chemistry Chapter 3

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All 117 Terms

Term Definition
atomic theory the theory that all matter is composed of indivisble particles called atoms
law of definite proportions any sample of a compound always has the same compostition
law of multiple proportions the mass ratio for one of the elements in a compound that combines with a fixed mass of another element can be expressed in small whole numbers
atomic mass the mass of an atom in atomic mass units
mole the SI unit for measuring the amount of a substance
Avogadro's constant the number of particles in 1 mol, 6.00221367*10^23/mol
Carbon-12 atom used as standard for atomic mass scale (1 amu= 1/12 the mass of...)
no does every atom of an element have the exact same mass?
False True or False: Einstein's equation of E=mc^2 disproves the law of conservation of mass
anode an electrode through which electrons enter a metal
cathode an electrode through which electrons leave a metal
electron small negatively charged particle found in atoms
alpha particle a positively charged particle produced by some nuclear disintegrations
nucleus the central region of an atom made up of protons and neutrons
proton a particle with a positive charge found in atomic nuclei
neutron a particle with no electric charge found in atomic nuclei
atomic number (what number?) the number of protons in the nucleus of an atom
mass number the total number of protons and neutrons in the nucleus of an atom equals the...
Coulomb's law (whose law?) the force between two charged particles is inversely proportional to the square of the distance between them
isotope one of two or more atoms of the same element w/ different numbers of neutrons
radioisotope an unstable atom that undergoes radioactive decay
coulombs SI unit for electric charge
electrons cathode rays are made of...
true (but it's soooo small that it doesn't matter when calculating atomic mass) true/false electrons have mass
they originated at the negatively charged cathode why did scientists reason that the particles in a cathode ray had a negative charge
yes does every atom contain electrons
Rutherford _____________ discovered that atoms had a massive, positively charged nucleus and were mostly empty space in his gold foil experiment.
neutrons Irene Joliot-Curie and James Chadwick proved the existence of...
number of neutrons mass number - atomic number =
the number of electrons the number of protons in an atom must equal...
the atomic number when expressing an atomic structure in a symbol, this is always to the lower left of the element's symbol
(the) mass number when expressing an atomic structure in a symbol, this is always to the upper left of the element's symbol
strong the ______ force allows protons and neutrons to form a stable nucleus despite the repulsive force between protons
observations of electrical experiments like the cathode ray experiment this led scientists to propose the existence of subatomic particles
Rutherford's gold foil experiment (shot a-particles at gold foil, most went through empty space but some bounced off/ were repelled by positively charged nucleus) what showed atoms are mostly empty space and have a positively charged nucleus
isotopes ______ of the same element are different in stability, properties, number of neutrons
electromagnetic spectrum the total range of electromagnetic radiation, ranging from the longest radio waves to the shortest gamma waves
line-emission spectrum distinct lines of colored light that are produced when the light produced by excited atoms of an element is passed through a prism
ground state the lowest energy state of a quantized system
excited state the condition of an atom in a higher energy state than ground state
quantum number a number with certain definite values
orbital a region of an atom in which there is a high probability of finding one or more electrons
Pauli exclusion principle (What principle?) a maximum of two electrons can occupy each orbital, and these electrons must have different spin quantum numbers
electron configuration a description of the occupied electron orbitals in an atom
aufbau principle (what principle?) electrons in an atom will occupy the lowest energy orbitals available
Hund's rule the most stable arrangement of electrons is that with the maximum number of unpaired electrons, all with the same spin quantum number
electrons the most important part of an atom in chemistry becausue they occupy most of an atoms volume and determine virtually all of its chemistry
studying the light they emit how we gain much of our knowledge of electrons
as frequency increases wavelength decreases
red light low frequency, long wavelength
violet (light) (what color light has) high frequency, short wavelength
frequency number of waves that pass a stationary point in one second
wavelength distance between two consecutive peaks or troughs of a wave
wavelength property of a wave that is measured in meters
frequency property of a wave that is measured in hertz
speed of light frequency*wavelength=
speed, wavelength, and frequency three characteristics by which waves can be described
light an electromagnetic wave
false (t/f) the Rutherford model of the atom could explain line-emission spectra
lavender glow excited hydrogen atoms emit a ---
colors of light (that produce a distinctive line-emission spectrum for that element) experiments with elements in the gas phase showed that each element emits characteristic...
Bohr _____ showed that excited atoms emit light
an excited electron falls to its ground state light is emitted when...
line-emission spectra (what does this produce?) emission of characteristic frequencies of light...
400 nm-700nm (violet-red) visible spectrum
n, l, m unique set of quantum numbers each electron in an atom is assigned
false (t/f) every series of three quantum numbers is acceptable
n symbol for principal quantum number (shell) , can take whole # values, in practice, values greater than 7 not encountered
n the farther the orbital from the nucleus, the larger this quantum number is
electrons orbit like planets Rutherford's model
l can take any whole # value from 0 to n-1
m may take whole # values depending on l. for example, if l =1 this equals=any from -1 - 1
false more than 2 elecrtons can occupy an orbital (t/f)
m(subscript)s symbol (letter) representing spin in a set of quantum numbers
direction of spin spin quantum number describes an electrons...
2 possible spin quantum numbers -1/2, +1/2
opposite directions two electrons in the same orbitals spin in...
true electrons occupy low energy orbitals first (t/f)
s _ orbital can hold 2 electrons
p _ orbital can hold 6 electrons
10 electrons d orbital can hold
f orbital can hold 14 electrons
asterisk when referring to elements an ________indicates excited state
definite proportions, conservation of mass, multiple proportions laws that support existence of atoms
mass of carbon-12 12 amu (exactly)
1 amu mass of what ? 1.6605*10^-27 kg
Avogadro's constant Whose constant? 6.022*10^23/mol, number of particles in a mol
protium consists solely of 1 electron and 1 proton
true isotopes are atoms that have the same atomic number but different mass numbers (t/f)
true (t/f) the electromagnetic spectrum includes the wavelengths of radiation of visible light
l symbol (letter) for quantum number for subshells, describes shape of orbital
0,1,2 when describing the quantum number of a subshell of a atom s, p, d equal what numbers (consecutively)
m(subscript)l quantum symbol (letter) for the orbital of an atom, where it is in the subshell
Dalton who came up w/ law or multiple proportions?
5 (ml=-2,-1,0,1,2) number of orbitals 2 subshell has
quantum numbers the 'address' of an electron
Pauli Exclusion Principle This means that no 2 electrons have the same set of quantum numbers
paramagnetic elements that do not have all of their electrons spin paired, are strongly affected by magnetic fields
diamagnetic elements that have all their electrons spin paired and aren't strongly affected by magnetic fields
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2, 4d10 electron configuration of Iron (atomic # 26)
false (t/f) most elements are diamagnetic
true (t/f) Helium is diamagnetic
dumbbell the p orbital is shaped like this piece of workout equipment...
different spins what allows electrons to coexist closely?
2 what is the mass ratio of CO? (know how to make law of multiple proportions table)
radiate energy according to Bohr's theory an excited atom would...
frequency the energy of a photon (quantum) is related to its...
8 number of electrons in highest energy level of an argon atom (#18)...
3 this (n) main energy level can hold 18 electrons
de Broglie his hypothesis means that electrons are like waves confined to the orbit of an atom
Bohr he thought electrons orbiting the nucleus were like planets orbiting the sun
false (t/f) Dalton's atomic theory said the number of protons equals an atom's atomic number
Millikan he calculated the charge on an electron by examining the behavior of charged oil drops in a electric field
Planck who figured out that electron magnetic energy is quantized for a given frequency of radiation (or light)
true (t/f) energy changes occur in small, specific steps
potential electrons farther away from the nucleus of an atom have more ___ energy
false (Mendeleev and Meyer independantly proposed early versions of the periodic table) (t/f) Dalton developed the periodic table
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Set Information

Terms 117
Creator julialt
Created September 1, 2007
Group Honors Chemistry
Tag chemistry
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tommy729 : .
tommy729 : .
tommy729 : wow... how long did it take to make all this..;;??
Annabelle : Changed Plank → who figured out that electron magnetic energy is quantized for a given frequency of radiation (or light) to Planck → who figured out that electron magnetic energy is quantized for a given frequency of radiation (or light)
Last Message: 11 months ago

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Most Missed Words

  1. Bohr → _____ showed that excited atoms emit light - 13 misses
  2. line-emission spectra → (what does this produce?) emission of characteristic frequencies of light... - 11 misses
  3. direction of spin → spin quantum number describes an electrons... - 11 misses
  4. lavender glow → excited hydrogen atoms emit a --- - 10 misses
  5. an excited electron falls to its ground state → light is emitted when... - 10 misses
  6. 2 possible spin quantum numbers → -1/2, +1/2 - 10 misses
  7. the atomic number → when expressing an atomic structure in a symbol, this is always to the lower left of the element's symbol - 9 misses