Unit+6+-+Periodic+Table

= Periodic Table = = = __Wavelength__:distance between 2 consecutive crests (lamda) meters, nm= 10(-9) __frequency:__ number of wave cycles that pass a given point in unit time (v) __hertz:__ represents one cycle per second (Hz) __speed of light__: 2.998x10(8)meters (c)=lamda x hertz __Photon__: an individual particle of light radiant energy (E) joules. E= hv= (hc/lamda) __Joule:__ __Atomic Spectra__: produced when an electron moves from a higher energy to a lower energy level, giving off light in the process __Spectrum__ __Delta E__ __Bohr Model__: Bohr postulated that e-s move about the nucleus in a circular orbit of fixed radius. By absorbimg energy, it moves to a higher orbit of greater energy, energy is given off as the e- returns __Rydberg Constant__: 2.180 x 10(^-18) __Quantum Mechanical Level:__ can only refer to the probability of finding an e- in a region; cannot specify path. The kinetic energy of the e- in an atom is inversely related to teh volume. 4 quantun numbers are required to describe completely the energy of an e- in an atom. __Quantum Number__: to give the probable location of an electron. __PEL__: principal energy level, n= 1,2,3,4; value of n is the main factor that determines the energy of an e- and its distannce from the nucleus 2n(^2) __Sublevel__ __orbital:__ the region where there is a high probability of finding e-'s within an atom (ml) __Electron Spin__ __Pauli Exclusion Principle__ __Electron Configuration__ __Hund's Rule__ __Orbital Diagram__ __Monatomic Ion:__ EX:) 24Cr(3+): 1s(^2)2s(^2)2p(^6)3s(^2)3p(^6)4s(^2)3d(^4) remove 3e-s to form Cr(3+)= 21 e-s get rid of ^ 4s(^2) first [{1s(^2)2s(^2)2p(^6)3s(^2)3p(^6)}3d(^3)] abbreviated notation: [Ar]3d(^3) __Periodic Law__ __Atomic Radius__ __Atomic Radius trends__ __Ionic Radius Trends__ __Ionization Energy__ __Ionization Energy Trends__ __Electronegativety:__ __Electronegativity Trends:__
 * //The power of an atom in a molecule to attract electrons to itself//**

Quantum Number: gives the probable location of an electron 1st q#: (n) principal energy level 2nd q#: (l) sublevels s,p,d,f 3rd q#: (ml) orbitals 4th q#: (ms) electron spin

maximum # of e- in PEL: 2n(2) if n=1: l=0 (one sublevel) if n=2: l=0,1 if n=3: l=0,1,2 Sublevel Designations: s,p,d,f __Orbital Diagrams__ each can hold 2 elctron and are represented by arrows. Fill in first with up arrows in each group and then fill in the down arrows.
 * n || 1 || 2 || 3 || 4 ||
 * e- || 2 || 8 || 18 || 32 ||
 * value of l || 0 || 1 || 2 || 3 ||
 * letter || s || p || d || f ||
 * e- capacity || 2 || 6 || 10 || 14 ||

SOOO Basically.... 0, 1, 2, 3 || -1,0,+1=p -2,-1,0,+1,+2=d -3,-2,-1,0,+1,+2,+3=f ||
 * Quantum # || Description || Symbol || Value ||
 * 1 || PEL || n || n= 1,2,3,4 ||
 * 2 || sublevels || //l// || s, p, d, f
 * 3 || orbital || m//l// || 0=s
 * 4 || direction of spin || m//s// || +1/2, -1/2 ||

media type="google" key="-2158222101210607510 Sodium Explosion! this is how it works: (credit to answers.com) Sodium (Na; Atomic number: 11) is a higly reactive element belonging to the alkali group. Since sodium has valency 1 ie it has one lone electron in its outermost orbital, it is highly reactive in nature. When sodium is added to water, the lone electron of sodium reacts with the hydroxyl group of water and displaces H+ ion, thus forming NaOH (sodium hydroxide). Since this is a highly exothermic reaction, the sudden release of energy during bond reformation results in explosion.

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