Unit 2 #2 Flashcards
gamma
10 to the -12
radio waves
100 meters
frequency
write with letter n, number of waves per second, that pass a given point in space
x ryas
10 to the -10
waves
Greek letter that is upside down, distance between two consecutive peaks (1 full cycle), light is a wave
microwaves
10 to the -2
speed
C, speed of the waves, all electro magnetic waves travel at the speed of light
infared
10 to the -4
visbile light
in between
4 times 10 to the -7 and ….
7 times 10 to the -7
bohr model
1.said there is a nucleus and different levels, 2. electrons confined to these levels, 3. when one passes energy through the tube, it takes it to another level and then drops down, 4. electron moves from high level to low levels, in doing so it releases an energy (photon) of light
see red light
from 1 to 3
see green light
from 4 then 2
see blue light
from 5 to 2
energy =….
photon’s constant times frequency, can use this to make calculations
z
atomic number
ultraviolent
10 to the -8
speed of light
700 miles per hour
electro mangetic radiation
includes light, x rays, micro waves, radio waves, all classified based on wave length
speed of light
wave length (meters) times frequency (1/second)
Rh
riburg constant
always 2.178 times 10 to the -18 Joules
emission of light by excited hydrogen atoms
- sample of hydrogen recieve high energy of spark
- hydrogen molecule absorb energy and bonds are broken
- they then get exicted
- they release extra energy by wavelengths to produce emission spectrum of hydrogen atoms
continous spectrum
white light pass through prism, continas all the wavelengths
line spectrum
visible region passed through prism only see a few, indicates that only certain energies are alowed for the electron in the hydrogen atom
Bohr
developed quantum model for the HYDROGEN atom, believed the electron in a hydrogen atom moves around the nucleus only in certain allowed circular orbits, gave hydrogen atom energy levels consistent with the hydrogen emission spectrum
the negative in the equation (energy levels available to the electron in the hydrogen atom)
energy of the electron is lower than it would be if the electron were at an infinite distance from the nucleus (interation and energy = zero)
ground state
lowest possible energy state
the negative in the equation (the change in energy when the electron falls from one level to another
indicates that the atom has lost energy
aufbau principle
as protons are added on by one to the nucleus to build up the elements, electrons are simply added to these hydrogenlike orbitals
Hund’s rule
the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by Pauli principle in a paritcular set of degenerate orbitals
valence electrons
electrons in the outermost principal quantum level of an atom
core electrons
inner electrons
orbital diagram
ARROWS
transition metals
configurations are obtained by adding electrons to the five 3d orbitals
important points of the periodic table
- (n + 1)s orbitals always fill before nd orbitals 2. lanthaninde series or lanthanides (filling of the seven 4f orbitals) 3.actinide series (filling seven 5f orbitals) 4. group label tells the total number of valence electrons for that gro
inoization energy
required to remove an electron from a gaseous atom or ion, highest energy electron (one bound least tightly) is removed first
first inoization energy
energy required to remove the highest energy of an electron
second inoization energy
energy required to removed the second electron
when you go to the right….
the first ionization energy increasesoo
when you go down a group…..
first innozation decreases (electrons being removed are farther away from the nucleus)
electron affinity
energy charge associated with addition of an electron to a gaseous atom (if addition of energy resutls in lower energy, the electron affinity will carry a negative sign)
when go left to right (electron affinity)
electron affinity began negative
when you go down by group (electron affinity0
electron affinity become positive( (less energy released)
atomic radius
atom size cannot specify exactly
values for atomic radii
obtained distance between atoms in chemical compounds
when left to right (raddi)
atomic radii decreases, valence electrons become closer, decreasing in size
when go down a group (radii)
atomic radii increaes
metals
left side, cations (give up electrons, become postivie)
nometals
right side, gain electrons form anions (negative)
metalloids
have metal and nonmetal properties
alkali metals
group 1A, going down (first inozation energy decreases, radii increaes), very reactive, low inoziation energy
