Chapter 7 Chemistry Study Guide
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. ▪ coordination
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. ▪ coordination