Orbitals, shapes of molecule and polarity

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Orbital region of high chance of finding an electron each orbital can hold 2 electrons IS 2p 2s - Cu to 3d 1⁰ 45' exceptions to remember: - 45 filled BEFORE 3d. - Chromium → normally LINEAR NON-LINEAR H: 0:H 3d 3p 35 zü: B: üz U-B-C 2 bonding pairs, no lone pairs. ft H¹" £+ o=C² = 0 N ZA HS * 1 HS 180° GH Is this molecule polar? -filled with increasing order of energy. electrons prefer to occupy orbitals on their own (not pairs) F → but write it after, and remove electrons. from it first 3d"45² but changes to 3d5 4s¹ 77777 Iso each electron has own orbital 104.5 reduce degree lone pairs repel by 2.5° r 2 bonding pairs, 2 love pairs. F - SIMF OCTA HEDRAL F F TRIAGONAL PLANAR F F covalent bonds. (outer shell of electrons) 290° F B 31 √ 1200 F Shapes of molecules 3 bonding pairs no lone pairs 6b.p TETRAHEDRAL H H.HC M I more than bonding pairs. H&N H H 109.5 H PYRAMIDAL H "IN 4 bonding pairs no lone pairs. H Н. С.Н H H H 107.5 J Oxygen more electronegative than carbon has polar bonds molecule is non-polar 2 dipole moments CANCELOUT 7 dipole moments don't cances out :: molecule is polar CI CI 1 ↑ VC CL CI dipole moments cancel out (all leaving C at same angle) • non-polar ( Electronegativity - the ability of an atom to attract the bonding electrons in a covalent bond across a period → proton no. ↑ (nuclear charge) → bonding electrons experience → electronegativity → occupied shells the same. GREATER attraction to nucleus increases down a group : → Sheilding increases a층 a HC → proton number increases no. of electrons on outer shell Stays the same →nuclear charge negated →less attraction between bonding. electrons and nucleus CNOF Ne SCI Flourine most...

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