3) How rainbow forms &

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1 Glen CP Chem Chap. 5 Electrons (e - ) I) Light & Quantized Energy A) Rutherford s nuclear model B) Wave Nature of Light 1) electromagnetic radiation form of (= ) that exhibits behavior as it thru. Includes 2) waves have primary characteristics: (a) (= ) (b) (= nu ) (c) (d) Speed of all electromagnetic wave is 3) : As wavelength, freq. & vice versa.138 (Fig. 5-3) How rainbow forms & of light breaks it up into component colors. Sunlight contains a range of wavelengths and frequencies. 4) Electromagnetic (EM) spectrum = all forms of electromagnetic. 139 (Fig 5-5) C) Particle Nature of Light not everything about light is explained by wave model 1) Quantum concept: quantum min amt of that can be / by an. Small, specific amt of. 1

2 2 2) effect electrons from a metal s when light of certain frequency shines on surface ( ) 3) photon particle of EM w/ no that carries a of. 4) 1905 Einstein proposed that (EM radiation) has properties of both and. Said photon s dep on its. D) Atomic Emission Spectra Consists of several individual lines of, not. 1) Each element s at. Emission spectrum is ; used to element 2) Flame tests explain II) Quantum Theory & the Atom A) Bohr Model of the Atom 1) - lowest allowable state of an atom 2) state - atom has gained 3) Bohr proposed that e - move only in around the. Smaller orbit, lower atom s or level; larger orbit, higher atom s 4) Orbits are numbered from outward. 5) e - that gains amt of moves to next level. When it drops back to orbit,

3 gives off, as light. B) Heisenberg Uncertainty Principle: 1) Impossible to make a on an object w/o changing the object can never know velocity & position of a particle at the same time. 2) Schrodinger wave equation - model of atom: model (a) atomic = region around nucleus; e - s most location (b) e - cloud model C) Hydrogen s Atomic Orbitals 1) quantum no. = ; indicates relative & of orbitals. As n, orbital becomes 2) energy sublevels = III) Electron Configurations A) Martian apartments 3 B) Ground-State e - Configurations 1) e - config

4 4 2) Low- systems more than high- system 3) principle each e- occupies the orbital available. All orbitals in an energy sublevel are of energy. Order of orbitals is. 4) Pauli exclusion principle max may occupy an atomic 5) orbital. They must have 6) Hund s rule e- must occupy each equal- orbital before 2 e- can occupy any orbital. C) Orbital Diagrams & e- Configuration Notations 1) orbital notation 2) shorthand notation 3) shorthand w/ noble gas D) e- = e- in atom s outermost level 1) Counting valence e- from e- config. 2) structure = element s symbol surrounded by dots representing electrons - format

5 Glen CP Chem Chap. 6- Periodic Table 5 I) Dev of Modern Periodic Table A) History of Per. Table 1) known elements - 2) John Newlands (layout not accepted) 3) Dmitri Mendeleev laid out elements by, into columns. Predicted unknown elements & left space for them ( ) 4) Henry Moseley Discovered way to determine. Rearranged elements by. Everything fell into place. 5) Periodic law there is a periodic of chem & phys of elements when they are arranged by at. no. B) Modern Per. Table 1) Organization (a) groups (b) periods (c) representative elements (d) transition elements 2) Metals left of stairstep : (a) Characteristics (1) (2) (3) (4)

6 (b) Groups (1) metals (2) metals (3) metals (4) metals 3) Nonmetals right of stairstep (a) most are / solids/ is only one liquid at room temp. (b) poor (c) (d) 4) Metalloids border stairstep: (a) have & props. of both & ; (b) Ex.-- II) Classification of Elements A) Elements in same group have same to. Atoms in the same group have chem properties b/c they have the same no. of. Valence e-: group numbers tell valence e-. B) Energy level of element s valence e- = in which it is found. C) s-, p-, d-, & f-blocks 1) s-block = Groups. Filling sublevel. 6

7 7 2) p-block = Groups. Filling sublevel; Group elements ( gases) have sublevels, therefore very 3) d-block = Groups ( metals). Filling sublevel. Pushed down by quake Principal energy level =. 4) f-block = metals. Filling sublevels. III) Periodic Trends A) Atomic Radius (size): 1) Moving left to right across period, atom size. 2) Moving top to bottom, atom size. B) Ionic Radius 1) ion atom/group of atoms w/ a ; lose or gain 2) Positive ions are than original atoms. 3) Neg. ions are than original atoms. 4) Moving down group, size same reason as atoms. C) Ionization Energy Energy required to an from a atom. 1 st = 1 st ionization energy. Indicates how an atom holds its. 2 nd, 3 rd ionization energies will be much than 1 st. D) Octet Rule atoms tend to,, or e- in order to acquire a full set of e-. Nonmetals e- and

8 8 form ions. Metals e- & form ions. E) Electronegativity ability of an atom to in a chem bond. most electroneg. Element. least electroneg.