Chapter 7 Chemistry Study Guide

Topics: Ion, Electric charge, Atom Pages: 3 (561 words) Published: December 21, 2012
Chapter 7

same number of valence electrons=behave similarly(chemical properties)
neon gases (neon, argon) unreactive in chemical reactions(stable)
Gilbert Lewis-octet rule(atoms tend to achieve electron configuration of gas)
atoms of metallic atoms lose electrons, atoms of nonmetal atoms lose or share electrons with another nonmetal elements to achieve a complete octet
to achieve octet, change electrons to ge ns2 np6 configuration
remove electrons=ionization
metals in group 1A and 2A always have charge of 1+ and 2+ (loses enough electrons to attain electron configuration of noble gas)
transition metals- cations vary
pseudo noble-gas electron configuration=18 electrons in outer level and all orbitals filled.
pseudo noble-gas electron configuration= silver, copper, gold, cadmium, mercury
name of anion ends with -ide
cations-> take noble electron configuration of group before, anion takes noble gas electron configuration of same group
Halide ions- ions produced when atoms of chlorine and other halogens gain electrons

ionic compounds= compounds composed of cations and anions
ionic compounds are electrically neutral
anions and cations attract one another by means of electrostatic force
ionic bonds= electrostatic forces that hold ions together in ionic compounds
chemical formula=shows the kinds and numbers of atoms in the smallest representative unit of a substance. (ex: NaCl) ▪ formula unit= lowest whole number ratio of ions in an ionic compound. (In sodium chloride, it is 1:1, one to Na+ to each Cl-)

Most ionic compounds are crystalline solids at room temperature
component ions in such crystals are arranged in repeating 3D patterns.
In NaCl, each sodium ion is surrounded by six chloride ions, and each chloride ions is surrounded by six sodium ions.
Large attractive forces of ionic compounds result in stable structures, high melting points.
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