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AP Chemistry - Structure of the Atom
Flashcards for the AP exam based off of the first chapter of Barron's 6th edition.
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Chemistry
10th Grade
04/15/2013

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Term
Law of Conservation of Matter
Definition
Antoine Lavoisier - 1774
In chemical reactions matter is neither created nor destroyed.
Term
Law of Constant Composition
Definition
Joseph Proust - 1799
Pure chemical compound always has the same percentage composition of each element by mass.
Term
Dalton's Atomic Theory
Definition
John Dalton - 1803 to 1808
1. All matter is composed of tiny, indivisible particles, called atoms, that cannot be created or destroyed.
2. Each element has atoms that are identical to each other in all of their properties, and these properties are different from the properties of all other atoms.
3. Chemical reactions are simple rearrangements of atoms from one combination to another in small whole-number ratios.
Term
Law of Multiple Proportions
Definition
John Dalton
When two elements can be combined to make two different compounds, and if samples of these two compounds are taken so that the masses of one of the elements in the two compounds are the same in both samples, then the ratio of the masses of the other element in these compounds will be a ratio of small whole numbers.
Term
Michael Faraday
Definition
1834 - showed that electric current could cause chemical reactions to occur, demonstrating the electric nature of the elements.
Term
J.J. Thompson
Definition
Cathode rays are a fundamental part of matter he termed electrons.
He also found the charge to mass ratio of electrons.
Term
Ernest Rutherford
Definition
Gold foil experiment- alpha particles shot at a thin gold foil went straight through - this proved that atoms are mostly empty space.
Term
Johann Balmer
Definition
1885 - empirical mathematical relationship between the wavelengths of light in the visible region of the spectrum.
Term
Johannes Rydberg
Definition
Extended Balmer's equation so that all of the wavelengths could be predicted
Term
Atomic Models
Definition
Solid particle model - 400 BC
Plum pudding model - 1909
Nuclear model - 1910 (Rutherford)
Solar system model - 1913 (Bohr)
Wave-mechanical model - 1927 (Schrödinger)
Term
Niels Bohr
Definition
1913 - solar system model of the atom.
Term
Max Planck
Definition
1900 - described light as packets, or quanta, of energy
Term
Louis de Broglie
Definition
1924 - if light can be considered as particles, then the small particles like electrons may have characteristics of a wave.
Term
Erwin Schrödinger
Definition
1927 - wave-mechanical theory of the atom; the electron doesn't follow a precise orbit.
Term
Werner Heisenberg
Definition
Heisenberg Uncertainty Principle - it is impossible to know the exact momentum and position of a particle.
Term
ground state vs excited state
Definition
ground state - an atom that exists in the lowest possible energy state
excited state - an atom that has more energy than the ground state
Term
wavelength
Definition
the distance between two repeating points on a sine wave
Term
frequency
Definition
the number of waves that pass a point in space each second
Term
λv=c
Definition
(wavelength)(frequency) = speed of light
Term
speed of light (in a vacuum)
Definition
c = 3.0 * 10^8
Term
Planck's constant
Definition
the energy of electromagnetic waves is proportional to the frequency and inversely proportional to the wavelength. The proportionality constant, h, is Planck's constant.
Term
How to find energy emitted when an electron drops back to the original orbit
Definition
The energy emitted from an electron moving to a lower orbit can be determined by subtracting the energy of the lower orbit from the energy of the higher orbit - this results in line spectra.
Term
Bohr radius
Definition
when n (energy level) = 1, it's 53 pm.
when n = 2, it's 106 pm.
Term
Wave-Particle Duality
Definition
there is a relationship between the particle (mass) and wave (frequency) nature of an electron.
Term
The Wave-Mechanical Model
Definition
1. Quantum numbers are crucial
2. This changes the view of the nucleus--cloud instead of orbit.
3. This agrees with the periodic table
4. Bohr was right about the energy change and the Bohr radius
Term
Heisenberg Uncertainty Principle
Definition
Both the position and the momentum of an electron cannot be exactly known at the same time. The more precisely that the position of the electron is known, the more uncertainty exists as to its momentum.
Term
energy order
Definition
1s, 2s, 2p, 3s, etc.
the order is s, p, d, f
can be obtained with the periodic table
Term
valance electrons
Definition
outermost electrons
count columns on the periodic table to find them
Term
Hund's rule
Definition
p, d, or f orbitals must all be filled with one electron before a second is allowed in
Term
orbital diagrams
Definition
arrows, representing electrons, are placed in each orbital. the second electron in each orbital has an arrow facing in the opposite direction.
Term
spin quantum number
Definition
either +1/2 or -1/2
this represents the spin of an electron
Term
Pauli exclusion principle
Definition
no two electrons in the same atom can have the same quantum numbers
Term
principal quantum number
Definition
n
any integer greater than one
represents the size of the principal energy level
Term
azimuthal quantum number
Definition
l
it can be any positive integer less than n-1
represents the shape of an orbtial
Term
magnetic quantum number
Definition
m sub l
it can be any integer from -l to +l
it represents the orientation of each orbital in space
Term
e=hv
Definition
Energy = Plank's constant * frequency
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