Term
| What didn't Rutherford's model of the atom explain? |
|
Definition
| How electrons filled in the spaces surrounding the nucleus, opposite charges attract |
|
|
Term
| Light behaves as what and has what type properties? |
|
Definition
|
|
Term
| What did the photoelectric effect reveal about light? |
|
Definition
| that it acts as a particle |
|
|
Term
| Form of energy;travels through space;properties of waves |
|
Definition
| electromagnetic radiation |
|
|
Term
| All forms of elecromagnetic radiation |
|
Definition
|
|
Term
| whichtypes of electromagnetic radiation have long wavelengths (4)? |
|
Definition
| Infrared, radiowaves, TV, and microwaves |
|
|
Term
| Which types of electromagnetic radiation have short wavelengths (3)? |
|
Definition
|
|
Term
| Which of visible light is the shortest, which is the longest? |
|
Definition
|
|
Term
| All forms of electromagnetic radiation travel at the same speed, what is that speed? |
|
Definition
|
|
Term
| the distance between corresponding points on adjacent waves(cm, m or nm) |
|
Definition
|
|
Term
| Defined number of waves that pass a given point in a specific time, usually 1 second (waves/second aka hertz) |
|
Definition
|
|
Term
| how wavelength and frequency are related in realtion to the speed of light |
|
Definition
| speed of light=wavelength x frequency |
|
|
Term
| the emission of electrons from a metal when light shines on the metal |
|
Definition
|
|
Term
| of energy is the minimum quantity of energy that can be lost or gained by an atom |
|
Definition
|
|
Term
| what is the value of 1 hertz? |
|
Definition
|
|
Term
| how are hertz and frequency related in relation to energy? |
|
Definition
|
|
Term
| higher frequency= ___________ |
|
Definition
|
|
Term
| a particle of electromagnetic radiation having zero mass and carrying a quantum of energy |
|
Definition
|
|
Term
|
Definition
|
|
Term
| higher potential energy than ground state |
|
Definition
|
|
Term
| when a narrow beam of the emitted light was shined through a prism, it was seperated into four specific colors of the visible spectrum |
|
Definition
|
|
Term
| what types of electromagnetic radiation is the Lyman;Balmer;Paschen series? |
|
Definition
lyman=UV
Balmer=Visible
Paschen=Infrared |
|
|
Term
| emission of continuos range of frequencies of electromagnetic radiation |
|
Definition
|
|
Term
| electron can circle nucleus only in allowed paths(orbits); definate fixed energy |
|
Definition
|
|
Term
| electron falls to lower energy level and a photon is emitted |
|
Definition
|
|
Term
| energy added to an atom in order to move an electron from lower level to higher level |
|
Definition
|
|
Term
| bending of a wave as it passes by the edge of an opening or through a small opening |
|
Definition
|
|
Term
|
Definition
|
|
Term
| states that it is impossible to determine aimultaneously both the position and velocity of an electron or any other particle |
|
Definition
| heisenberg uncertainty principle |
|
|
Term
| describes mathematically the wave properties of electrons and other very small particles |
|
Definition
|
|
Term
| 3d region around the nucleus that indicates the probable location of an electron |
|
Definition
|
|
Term
| specify the properties of atomic orbitals and the properties of electrons in orbitals |
|
Definition
|
|
Term
| indicates the main energy level occupied by the electron |
|
Definition
| principal quantum number (n) |
|
|
Term
|
Definition
| the total number of orbitals that can exist in a given shell(main energy level) |
|
|
Term
| orbitals of different shapes |
|
Definition
|
|
Term
| indicates shape of orbital |
|
Definition
| angular momentum quantum number(l) |
|
|
Term
|
Definition
orbital shapes possible
angular momentum number |
|
|
Term
shape of:
s orbital
p orbital |
|
Definition
|
|
Term
|
Definition
|
|
Term
| indicates the orientation of an orbital around the nucleus |
|
Definition
Magnetic quantum number(m)
n-2 |
|
|
Term
| only two possible values(1/2 or -1/2) which indicate the fundamental spin states of an electron in an orbital |
|
Definition
|
|
Term
|
Definition
| total number of electrons |
|
|
Term
| the arrangement of electrons in an atom |
|
Definition
|
|
Term
| the electron configuration is _______ for each element |
|
Definition
|
|
Term
| an electron occupies the lowest-energy orbital that can recieve it |
|
Definition
|
|
Term
| no two electrons in the same atom can have the same set of four quantum numbers |
|
Definition
| pauli exclusion principal |
|
|
Term
| orbitals of equal energy are each occupied by a second electron and all electrons in singly occupied orbitals must have the same spin state |
|
Definition
|
|
