Li if LOSE one negative electron then becomes larger/ smaller Li +

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1 Periodic Table Notes (Summary) Periodic Trends: Define the periodic trends. Atomic Radius:_ _ size of an atom_ Electronegativity: an atom's ability to attract an electron Electron Affinity: energy released when an electron is picked up by an atom Ionization Energy: energy required to remove an electron from an atom Note: Valence Electrons influence the trends. Label the trends using the rectangle below, use arrow to show direction. IONS:_ _Charged atoms Are positive and negative ions larger or smaller than their neutral states? Li if LOSE one negative electron then becomes larger/ smaller Li + F if GAIN one negative electron then becomes larger /smaller F - Cations are _positive ions which means they lose electrons and therefore they are _ smaller then their atoms. Cations: Metals that tend to lose electron and become cation (positive) Anions are _negative ions which means they _gain electrons and therefore they are larger _then their atoms. Anions: Nonmetals that tend to gain electron and become anion (negative) Valence Electrons: Electrons in the outermost energy level of an atom. Important because: They are used in bonding with other atoms Show chemical properties of an element Can be related to an element s position on the PT. 1

2 Octet Rule: Atoms always try to reach stability by having a full_ _ shell_. When outermost shell is filled with _8_ electrons ( like Noble gases ) it s considered full. Hydrogen single proton and a single electron, simplest and most abundant element in the universe. 'burn' to produce energy. combines with other elements to form numerous compounds. Alkali Metals always 1+ (lose the electron in s subshell) strong metals unusually soft, silverish color, tarnishes(dull) quickly in air Very reactive toward Halogens to make salts. Alkali Earth Metals always 2+ (lose both electrons in s subshell) Not as soft as Group 1 metals. Shiny, crystalline. react more mildly with Oxygen to produce oxides of the metals Only react with water at temperatures where the water is steam. Transition Metals Metalloids 2+ is common, and 1+ and 3+ observed Not as predictable Ductile, malleable, solids (except Mercury) Conductors of Electricity between metals and nonmetals Sometimes lose and sometimes gain electrons Ex: Si appears lustrous, is brittle, not malleable or ductile. Poorer conductor of heat and electricity than transition metals. Useful in the semiconductor industry. Ex: computers... Halogens None metals, very reactive Produce salts Gases Noble Gases Noble gas group (inert gas group). Only a handful of compounds (mostly involving Xenon) Non reactive Full (8 valence electrons ) outermost shell. 2

3 Actinides & Lanthanides Diatoms Special inner transition state metals first rearranged by Dr. Glen Seaborg of Univ. of Calif. at Berkeley in the 1950's. Seemed to predict the properties of several newly synthesized man-made elements. 7 diatomic molecules : (HOClBrIFN = Huckleberry Finn!) Hydrogen(H 2 ), Oxygen(O 2 ), Chlorine(Cl 2 ), Bromine(Br 2 ), Iodine(I 2 ), Fluorine(F 2 ), Nitrogen(N 2 ) Bohr Model of Oxygen Atomic Weight: 16_ Atomic #: 8_ _ P + = 8 e - = 8_ n 0 = 8_ _ Li Lewis Dot Structure Be Ionic Lewis Dot Structure P B N O F Covalent Bonding: Bonding between nonmetals. They share electrons Ionic Bonding: Between a nonmetal and metal. They exchange electrons. Give or take Periodic Table Notes continued Electron Configuration: Electrons are arranged energy levels known as n=1,n=2,n=3 n=4, and so on. Each energy level further divided into subshells know as s, p,d and f. Each subshell can hold certain # of electrons. Shell (Energy Level) Subshells & # of e -- # of Electrons 3

4 1 s (s =2)= p (s=2 p=6)= d (s=2 p=6 d= 10)= f (s=2 p=6 d= 10 f= 14)= Label the s, p, d, & f block. 4

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