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Electrons in Atoms Name: ___________________ INTRO: Periodic Table of the Elements metals -comprise most of the periodic table (________) -lose electrons to form ___________________ called ___________ -properties; ___________________________________________________________ __________________________________________________________________ nonmetals -located in the upper right “______________” and ______________ -gain electrons to form ____________________ called ___________ -properties; ___________________________________________________________ _____________________________________________________________________ semimetals – called ____________________ - have properties of both ______________________________ (for instance, they are often _________________________) - located on either side of the “____________” noble gases – called “inert” gases (unreactive) - don’t react with other elements because their outermost energy level is filled - located in the far right column group – vertical column of elements (____________________________________) - for group A elements: group # = __________________________ The arrangement of the Periodic Table is such that elements with similar chemical and physical properties appear within a column. It is the configuration of the outer shell electrons that determines how an element will react (bond). Common Group Names: 1A (1); _______________________________ 2A (2): _______________________________ 7A (17) _______________________________ 8A (18) _______________________________ period - horizontal row of elements - period # = # energy levels energy level 1 2 3 4 5 max. # e2 8 18 32 32 8 * The outermost energy level of an atom can hold a maximum of ____________________. stable octet – ____________________________________________________________________ - this is the configuration of ____________________ and is the most ____________ Atoms react to try and attain a stable octet when they combine to form compounds. Law of Definite Proportions – _____________________________________________________ _______________________________________________________________________________ Group A Elements – called _____________________ elements - show entire range of _____________________________ - energy levels beneath the _________________________ Group B Elements – called the _____________________________ - may have more than one _____________________ - energy levels beneath the outermost have more than __________________ and may get ___________________________ - Inner Transitional Metals ________________________________________ 1. lanthanides _______________________________________________ 2. actinides _________________________________________________ A. LIGHT AND THE QUANTUM CONCEPT light – Electromagnetic Spectrum radio waves radar microwaves infrared visible light ultraviolet x-rays gamma rays cosmic rays ROYGBIV Low frequency wavelength ( frequency ( High frequency ) (lamda) – ) (nu) – hertz (Hz) – wavelength and frequency are inversely related: Quantum or photon – The energy of a quantum, where h is Plank’s Constant The amount of radiant energy absorbed or emitted Therefore, B. ATOMIC EMISSION SPECTRA (c = speed of light : ) When an element is heated by passing electricity through its vapor : . When an atom absorbs energy: . Atomic emission spectrum – ( line spectra each element (like a fingerprint - C. DEVELOPMENT OF ATOMIC MODELS 1. JJ Thompson – 2. Ernest Rutherford – Electrons around a dense nucleus; atom mostly empty space 3. Niels Bohr - energy levels – Quantum of energy – 4. Schrodinger – D. ATOMIC STRUCTURE ) ) Atoms contain . nucleus – electrons – energy levels (shells) – - 1 max # e- : ( ) 2 3 ( ) ( 4 ) ( ) stable octet E. SUBDIVISIONS OF ENERGY LEVELS period # on the periodic table = Within each energy level, energy level # = energy level 1 2 3 4 F. ATOMIC ORBITALS . = sublevels 1 2 3 4 Within each sublevel, orbital – sublevel max # e- orbitals ( ) ( ) ( ) ( ) s orbitals are p orbitals are d orbitals are f orbitals are s orbitals p orbitals x y z y d orbitals y z z 2s x 1s x px px equal probability of finding 1st or 2nd “p” electron in either of the 2 lobes or both electrons within 1 lobe At higher energy levels When all orbitals of a sublevel are filled G. ELECTRONS IN ORBITALS . = : One e- spin ( ) and the other opposite e- spin H. IMPORTANT RULES Aufbau Principle – Hund’s Rule – Pauli Exclusion Principle – ( ) 2n2 Rule – How many sublevels, orbitals and electrons could be contained in the 8th energy level? n = n = n2 = energy level n = sublevels n = orbitals n2 = 2(n2) = electrons How many sublevels, orbitals and electrons could be contained in the 11th energy level? I. ELECTRON CONFIGURATIONS & ORBITAL NOTATIONS 1 2 3 4 2(n2) = 1 H 11 Na 2 He 12 Mg 3 Li 13 Al 4 Be 14 Si 5 B 15 P 6 C 16 S 7 N 17 Cl 8 O 18 Ar 9 F Compare Neon and Argon: 10 Ne electron configuration – the arrangement of e- around the nucleus of an atom in its ground state orbital notation – shows the distribution of electrons (as arrows) in the orbital boxes of a sublevel shorthand electron configuration – the e- config. of an atom using the previous noble gas as a starting point condensed electron configuration – the e- config. of an atom that shows the number of electrons present in each energy level (listed vertically) electron dot formula or Lewis Dot diagrams: shows the arrangement of valence (outer shell) electrons around an atomic symbol.Take into account the electrons from the highest energy levels s and p sublevels. Write the symbol for the element use dots to represent electrons. Place the dots one on each side before you pair them up (just like filling in orbitals). Bonding: When elements bond, combine to form compounds, only the electrons in the outer shell (energy level) are involved. Chemists use __________________ to show these outer shell electrons. Write the shorthand electron configuration N: He 2s2 2px1y1z1 e- dot structures: Write the condensed electron configuration Mg: N F: Mg 2 7 P: F P All transitional metals and inner transitional metals have a completed s sublevel so their Lewis Dot Diagrams all look the same. Shorthand electron configuration Ex: Fe Lewis Dot Fe Pm Pm **Because electrons want to be in the orbital with the lowest energy, (AUFBAU PRINCIPLE), There are some exceptions to how the electrons fill up. Orbital Energy Highest part full Lowest Chromium - Cr ½ full Molybdenium -Mo full Copper – Cu empty Silver – Ag J. USING THE PERIODIC TABLE FOR ELECTRON CONFIGURATIONS Energy sublevels overlap because s block – 2 p block – 6 d block – 10 f block – s 14 p d f Remember: Using the periodic table write the complete electron configuration for the following elements: cond. e- cofig for I: Ni (#28) I (#53) Au (#79) K. QUANTUM NUMBERS OF ELECTRONS The energy state of electrons in atoms can be described by a set of four numbers that describe a) distance from the nucleus b) shape c) position in 3D space, and d) spin. Quantum number symbol description values a) Principal n b) Orbital l c) Magnetic ml d) Spin ms Principal quantum n = 1 Orbital quantum l =0 Principal quantum n = 2 Orbital quantum l =1 Principal quantum n = 3 Orbital quantum l =2 Principal quantum n = 4 Orbital quantum l =3 Spin quantum ms = +½ Magnetic quantum ml = 0 (s) Spin quantum ms = -½ 0 Magnetic quantum ml = 1 Magnetic quantum ml = 2 (p) x -1 0 +1 -1 0 +1 +2 (f) -3 -2 Principal Energy level 1: n = z (d) -2 Magnetic quantum ml = 3 y -1 0 +1 orbital l= possible electron sites:1s1 = 1s2 = +2 +3 magnetic ml = spin ms = Principal Orbital Magnetic l= Energy level 2: n = ml = ml = 0 (sublevel s 1 orbital) Spin ms = ml = -1 0 +1 (sublevel p 3 orbitals) 2s 2px 2py 2pz 2s1 = 2px1 = 2py1 = 2pz1 = 2s2 = 2px2= 2py2 = 2pz2 = Principal Orbital Magnetic l= Energy level 3: n = ml = ml = 0 (sublevel s 1 orbital) Spin ms = ml = -1 0 +1 (sublevel p 3 orbitals) 3s 3px 3py 3d energy level 3 n = sublevel d l= (sublevel d 5 orbitals) ml = -2 -1 0 +1 +2 3pz Principal Orbital Magnetic l= Energy level 4: n = ml = 4s Spin ms = 4p possible electron sites: 4d 4f What are the quantum numbers for the last placed electron in each of these atoms? 1. S (#16) 2. Ag (#47) 3. Ba (#56) 4. U (#92) When drawing the electron dot structure for an atom of an element, the diagram shows the VALENCE electrons, that is, the electrons in the HIGHEST energy level of that atom. When writing the quantum numbers for an atom of an element, the numbers are written for LAST placed electron, that is, the LAST ITEM in the electron configuration. For each of the following elements: a. Give the shorthand e- configuration b. Give the orbital notation 1. Na (#11) 2. Ru (#44) 3. Eu (#63) 4. At (#85) c. Give the electron dot formula (valence e-) d. Give the quantum #s for the last placed e-