Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
17 Cards in this Set
- Front
- Back
|
Angular momentum of an electron
|
nh/2pi
where h is Planck's constant and n is the quantum number |
|
|
Energy of an electron
|
E= -RH/n^2
RH= 2.18E-18 |
|
|
Electromagnetic energy of a photon
|
E= hc/lamda
h= Plancks constant and c= 3.00E8, speed of light |
|
|
Principal quantum number (n)
|
Can take on any positive integer value and the larger the value of n, the higher the energy level and radius of the electron's orbit
|
|
|
Angular momentum quantum number (l)
|
Refers to the subshells or sublevels that occur within each principal energy level. For any given n, the value of l can be any integer in the range 0 to n-1.
|
|
|
Magnetic quantum number (ml)
|
Specifies the particular orbital where an electron is likely to be found. Ml can range from -l to +l.
|
|
|
Spin quantum number (ms)
|
Values of either +1/2 or -1/2
|
|
|
Hundt's Rule
|
Within a given subshell, orbitals are filled such that there are a maximum number of half-filled orbitals with parallel spins. (Electrons prefer empty orbitals to half-filled ones)
|
|
|
Valence electrons
|
Those electrons in the outer energy shell available for bonding.
|
|
|
Atomic radii
|
Decreases across a period, increases down a group. Thus, atoms with the largest atomic radii are at the bottom of Group 1
|
|
|
Ionization energy
|
Energy required to remove an electron (energy is required, endothermic) from a gaseous atom or ion. Ionization energies grow increasingly large as multiple electrons are removed.
Increases from left to right and decreases down a group. Thus, the highest IE are in the top right of the periodic chart. |
|
|
Electron affinity
|
The energy change that occurs when an electron is added to a gaseous atom. The stronger the pull of the nucleus for electrons, the greater the electron affinity will be.
Increases from left to right and also up a group, but Group VIII elements have electron affinities of zero (already possess a stable octet) |
|
|
Alkali metals
|
Elements of Group IA. They have most of the properties of metals but have lower densities. Also only have one loosely bounded electron in the outermost shell which is easily lost (thus, they have low IE values)
|
|
|
Alkaline earths
|
Elements of Group IIA. They possess many characteristics of metals. They have two electrons in their outer shell and thus have smaller atomic radii than Group IA metals. The electrons are not held very tightly and can be easily removed.
|
|
|
Halogens
|
Group VIIA, highly reactive nonmetals with seven valence electrons. Different physical properties... liquid or gaseous. All have high EN values.
|
|
|
Noble gases
|
Group VIII, inert gases that are fairly nonreactive because they have a complete valence shell. They have no tendency to gain or lose electrons. Also have low boiling points and are gases at room temp.
|
|
|
Transition elements
|
Groups IB to VIIIB, all considered metals. Very hard with high boiling points and melting points. Can exist in a variety of forms.
|
