Valence Electrons - Ionic Bonding | Eastern Kentucky University

University:
Eastern Kentucky University
Course:
CHE 111 | General Chemistry
Academic year:

2023
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200

Pages:

1
Author:

Accinkiquicpqw

1.8 - Valence electrons - Ionic bonding != covalent bonds, not electron sharing but transfer metal & nonmetals (except 8A) NA = 6.022*10^23 Transition metals lose valence electrons before losing group d Ionic substances: - Hard, high melting point - Brittle - Crystalline increase from left to right, except 2A 5A 8A n = m/M n = moles electron affinity (energy released when + e-) electronegativity same trend, no exception (no noble gases) M = grams/mole MOLES decides bond type atomic radius increase down a group (more shells) decrease to the right (+ nucleus charge) decrease when down a group (+ distance) increase when to right of a period (- distance, + nucleus charge) m = grams Same element (proton, electron); different weight (neutron) explained by Coulomb’s law and Z eff cation/anion 1.1 Mass spectroscopy Isotopes 1.7 - Periodic trends mass * % for all isotopes => avg atomic mass Relative abundance in nature 1.2 First ionization energy ionization energy “jump” => group (exceptions: p0 -> p1; p3 -> p4) L. o. definite proportions directly correlate with e- config AP Chemistry Unit 1 Review highest binding energy = closest to nucleus => 1s2 1.3 - Elemental composition Empirical formula 1.6 - Photoelectric simplest whole number combination of elements in a compound ex. C6H12 O6 empirical formula is CH2O 1.4 - Mixtures Spectroscopy Distillation Typ es Filtration see increasing or decreasing attraction force constant pure sample always same ratio of constituent elements based on boiling point differenc NaCl from H2O heterogeneous solid - liquid m sand from water product of charges Chromatography Aufbau principle: lowest subshell first, then build up Mass percentage in mixtures: substance mass/total mass Hund’s rule: each subshell should have one electron before doubling up based on polarity: mixture of ink colour Coulomb’s law RULES Pauli’s exclusion: all e- have at least 1 quantum No. diff electron configuration radius/distance 1.5 - Atomic subshells (1, 3, 5, 6): 2 electrons each structure s, p, d, f Most likely to find electrons orbitals Quantum mechanical model Main topic Examples