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Periodic Trend • Horizontal rows are called _________ • Vertical columns are called ________ • There are __ periods, __ groups Element Arrangement • Elements in each ______have different electron energy shell level • Elements in each column of table have same number of __________ in their _________ level – _____________ • Group 1 or 1A– one valence electron • Group 2 or 2A– two valence electron • Group 13 or 3A– has three valence electron and so on. • Groups 3/ 3B to 12 / 12B have different number of valence electron Periodic Table • Periodic Table A. Metallic Character • Metals • Nonmetals • Metalloids – Metals- 80%, ___ of stair-step line, excellent – Nonmetals- ____ of stair-step line, generally poor – Metalloids- ______ stair-step line; » Stair-step line aka. “zig-zag” • We can also look at the periodic table in terms of ________________, the arrangement of electrons in an atom Take a look at Pg 119 • What is the electron configuration of C? • What is the electron configuration of Pb? – s-block elements: chemically reactive metals, • alkali metals- group ___ • alkaline earth metals- group __ – d-Block elements: • transition metals- group ____, – p-Block elements: part of main block • halogens- group ___, • noble gases- group ___, – f-Block elements: To save space the lanthanides and actinides are set off below the main portion of the Table. • inner transition metals-aka ____-____ ________ • Lanthanide Still placed in the 6th and 7th periods, respectively (even • Actinide though 4f and 5f) Periodic Trend • As you go from ____ to ____, the number of _____________. • As you go from ____ to _____, the ____________ in the same energy level ___________. • As you go from _____ to _______, more _______ are added. • As you go from _____ to _______, ______ are farther away. Effective Nuclear Charge • Nucleus is _________. • Positive charge of the nucleus ____________ • Electrons closer are ________ effectively drawn to nucleus • Electrons farther away are _______ drawn to nucleus • Attractive force from the nucleus is canceled out by inner electrons. Outermost shell feel less attraction – _________________ Atomic Radius • Hard to determine- electron clouds • ___________- the length that is half the distance between the nuclei of two bonded atoms. Figure 19. • _________, _________ more pulling closer to the nucleus smaller the bond radius _____________________ • _________, _____________ electrons are farther away ____________ bigger the bond radius __________________ Atomic size increases, (shielding constant across a period) Ionic size increases Ionization Energy • The energy needed to __________ an electron from the shell • ___________, more protons stronger pulling tighter the atom more energy needed to remove an electron _______________ • ____________, more electron shells electron shielding farther electrons feel less attraction less energy to remove an electron _____________________ Ionization energy, Electronegativity, Electron affinity INCREASE Electronegativity • A measure ability to __________ electrons • __________, more protons more pulling from nucleus easier to attract another electron ________________________ • ________, more electron shells farther away less effective pulling ______________________________ Atomic Size } Radius • Atomic Radius = half the distance between two nuclei of a diatomic molecule