7.6 Metals, Nonmetals, & Metalloids
We have looked at properties of individual atoms (IE, EA, radius).
Only the ________________ ___________________ exist as individual atoms in nature.
Review properties of metals & nonmetals (Table 7.3, p. 264)
Ge is a ________________ , Sn is a ________________ even though they are in the same group. How can you explain
this difference?
Metallic character ________________ down a group and ________________ across a period.
Metals
All metals are solid except for ________________ ; Cs and Ga melt just above room T
Metals tend to have ________________ ionization energies and tend to form ________________ relatively easily.
Since metals lose e- in reactions, they are ________________ .
First ionization energy is the best indicator whether an element behaves as a metal or a nonmetal.
Sn forms either a 2+ or 4+ ion. Why?
Soluble metallic oxides react with water to form hydroxides:
Na2O(s) + H2O 
CaO(s) + H2O 
Metallic oxides react with acid to produce a salt and water:
NiO(s) + HNO3 
p. 267 SE (a) Would you expect scandium oxide to me a solid, liquid, or gas at room T?
(b) Write the net ionic equation for scandium oxide reacting with nitric acid:
When the name of an acid
has no prefix and ends in
–ic (like sulfuric acid), the
formula is H+ + the –ate
ion (H+ combines with
SO42- to make H2SO4).
PE: copper(II) oxide and sulfuric acid
Nonmetals
________________ , ________________ , or gas at room T. Melting points tend to be ________________ than
metals.
Nonmetals tend to ________________ e- to fill the outer p sublevel when they react with metals.
Compounds of nonmetals tend to be __________________________ substances that are ________________ ,
________________ , or ________________ with low ________________ ________________ .
Nonmetallic oxides react with water to produce an acid
CO2 + H2O 
This is why carbonate beverages are acidic and is one factor in acid rain. SO2 and SO3 produced from burning fuels are
also responsible for acid rain.
P4O10 + H2O 
Nonmetallic oxides react with bases to produce a salt and water
CO2 + NaOH 
A compound, XCl3, has a melting point of -112oC. Would you expect the compound to me molecular or ionic? If you
were told that X is either scandium or phosphorus, which do you think is the more likely choice?
Write net ionic equations:
SeO2 (s) + H2O 
SeO2(s) + NaOH(aq) 
P4O6(s) + H2O 
Read Metalloids on page 268
7.7 Trends for Group 1A and Group 2A Metals
Read Group 1A: The Alkali Metals on page 269
Alkali metals combine directly with most nonmetals.
When hydrogen combines with a metal, it forms the hydride ion (H-)
Na + H2 
K+S
Alkali metals react with water to produce a metallic hydroxide (base) and hydrogen
Li + H2O 
(this is an __________________________ reaction)
Why are alkali metals stored in oil or kerosene?
Write the balanced equations and net ionic equations for cesium metal reacting with (a) Cl2 (b) H2O (c) H2