CHEMISTRY Flashcards
is the physical material
of the universe.
Matter
is a measure of how closely
individual measurements agree with
one another.
Precision
refers to how closely
individual measurements agree with
the correct, or “true” value.
Accuracy
1005 kg
4 significant figures
7.03 cm
3 significant figures
0.02g
1 significant figures
0.0026 cm
2 significant figures
0.0200 g
3 significant figures
3.0 cm
2 significant figures
consists of the principal energy
level (n value), the letter designation of the sublevel (l
value), and the number of electrons (#) in the sublevel,
written as a superscript: nl .
Electronic Configuration
consists of a box (or just a line) for each
orbital in a given energy level, grouped by sublevel (with nl
designation shown beneath), with an arrow representing
an electron and its spin: ↑ is +1⁄2 and ↓ is -1⁄2.
Orbital Diagram
Every atomic orbital within a sublevel is singly occupied
before it is doubly occupied and that all singly occupied
orbitals possess electrons with the same spin.
Hund’s Rule
the number of
complete waves, or cycles, that pass a
given point per second; expressed by
the unit 1/s [also called hertz (Hz)].
Frequency (v)
the
distance between two adjacent peaks
(or between two adjacent troughs).
Wavelength (lambda)
the distance it moves per unit time (meters per
second), the product of its frequency (cycles per second)
and wavelength (meters per cycle):
Speed
2.99792458 x 10 ^8
Speed of Light
the height of the
crest (or depth of the trough).
Amplitude
objects emit electromagnetic radiation
from their surfaces in a temperature-dependent manner.
Blackbody Radiation
h= Planck’s constant
6.626 x 10^-34
a beam of light falling on a metal
surface in a vacuum ejects electrons from the surface causing
an electric photocurrent to flow.
Photoelectric Effect
R= Rydebergs Constant
1.096776 x 10^7 m^-1
when a high voltage or flame is
applied to gases at low pressures, atoms absorb and emit a
discrete array of light frequencies, rather than a continuous
spectrum, after passing through a prism.
Atomic Emision Spectra
RYDEBERGS EQUATION
(1913) linked the three
discoveries of Planck and Einstein
and developed a mathematical
model that explained the behavior
of an electron in a hydrogen atom,
including its atomic line emission
spectrum.
Bohr model
(1913) linked the three
discoveries of Planck and Einstein
and developed a mathematical
model that explained the behavior
of an electron in a hydrogen atom,
including its atomic line emission
spectrum.
Bohr model
proposed that an electron moving about the
nucleus of an atom behaves like a wave and therefore has a
wavelength. The wavelength of the electron, or of any other
particle, depends on its mass, m, and on its velocity, v:
De Broglie
De Broglie’s Equation
lambda = h/mv
p=h/lambda
states that it is
impossible to measure or calculate exactly, both the
position and the momentum of a particle.
Heisenberg Uncertainty Principle
Defines the size and energy
Increased n correlates to
increasing and quantized energy
and radius in the Bohr model.
of an orbital.
Principal Quantum Number (n)
Defines the shape of the orbital.
A value of the angular momentum quantum number can
indicate either an s, p, d, or f subshell which vary in shape.
Angular Momentum Quantum Number (l)
Defines the orientation of the orbital in space.
An orbital with l = 1 can have one of three ml values,
-1, 0,
or +1; that is, there are three possible orbitals with l = 1,
each with its own orientation.
Magnetic Quantum Number(ml)
