1. 7.6 Metals, Nonmetals, and Metalloids
By: Monique Briones, Marie Leibfreid, Bryanne Vollmer, Richard Wang

2. In the Periodic Table
No elements exist naturally as individual atoms EXCEPT noble gases
Metals—left and middle
Nonmetals—top right
Metalloids—between metals and nonmetals
Hydrogen nonmetal
Increase
Increase

3. Characteristic Properties
Metals
Nonmetals
Luster, various colors (silver)
Solids malleable and ductile
Good conductors heat and electricity
Oxides are basic ionic solids
Form cations aqueous solution
Corrode
Dense
High melting point
No luster, various colors
Solids brittle, hard and soft
Poor conductors heat and electricity
Oxides molecular substances form acidic solutions
Anions or oxyanions in aqueous solution
Cannot change shape without breaking
Low melting point
Metallic Character—the extent to which an element exhibits the physical and chemical properties of metals
Nonmetallic Character— “the extent…” nonmetals

4. Metals Solids room temp. (except Hg, Cs 28.4C, Ga 29.8C)
Low ionization energies
Oxidized
Form positive ions easily
Noble Gas Electron Configuration (Alkali 1+, Alkaline Earth 2+)
Transition metals more than one positive ion
Alkali, Alkaline Earth, Transition, and Other

5. Metals Cont. Compounds with nonmetals are ionic (Ex: oxides)
Metal oxides basic, dissolve in water to form metal hydroxides (due to oxide ion)
React with acids to form salt and water
High melting point

6. Alkali Group 1A Reactive Do not occur naturally on their own
Bond with other elements since there is only one e- in outer shell
Soft
Explode in water

7. Alkaline Earth Oxidation number: +2 Reactive
Not naturally found uncombined in nature
I.E.
Beryllium
Calcium
Radium

8. Transition Groups 3-12 Valence e- in more than shell
Several oxidation states
I.E.
Titanium
Iron
Cobalt

9. Other Metals Groups 13-15 Solid High density
Opaque (light cannot get through)
Oxidation numbers: +3,+/- 4, -3
I.E.
Aluminum
Tin
Lead

10. Metal Chemical Reactions
Metal + Nonmetal ––––> Ionic substance
Ex: 2Ni(s) + O2(g) ––––> 2NiO(s)
Metal Oxide + Water ––––> Metal Hydroxide
Ex: Na2O(s) + H20(l) ––––> 2NaOH(aq)
Ex: CaO(s) + H20(l) ––––> Ca(OH) 2(aq)
Basicity Due to Oxide Ion
Ex: O2-(aq) + H2O(l) ––––> 2OH-(aq)
Metal Oxide + Acid ––––> Salt + Water
Ex: NiO(s)+ 2HCl(aq)––––> NiCl2 (aq) + H2O(l)

11. Nonmetals Vary greatly in appearance
7 Diatomic (Gas: H2, N2, O2, F2, Cl2; Liquid: Br2; Solid: I2)
Gain electrons when react with metals to form noble gas electron configuration
Completely nonmetal compounds are molecular substances
Oxides acidic, dissolve in water to form acids (acid rain)
Dissolve in basic solution to form salts

12. Nonmetal Chemical Reactions
Tend to gain electrons when react with metals
Ex: 2Al(s) + 3Br2(l) ––––> 2AlBr3(s)
Nonmetal Oxide + Water ––––> Acid
Ex: CO2(g) + H2O(l) ––––> H2CO3(aq)
Ex: P4O10(s) + 6H2O(l) ––––> 4H3PO4(aq)
Nonmetal Oxide + Base ––––> Salt + Water
Ex: CO2 (g) + 2NaOH(aq) ––––> Na2CO3(aq)+ H20(l)

13. Metalloids Have metal and nonmetal properties
Found in stair shaped section of periodic table
Used in computers & calculators
Shiny or dull depending on element
Shape can be changed easily
Ex: Silicon
Looks like metal
Brittle
Poorer conductor of heat and electricity than metal
Electrical semiconductors

14. Additional Research

15. Chemical Behavior Metals Nonmetals Reducing Agents
Form oxides that react with water to give hydroxides
Form basic hydroxides
React with O, F, H, and other nonmetals, giving ionic compounds
React with other metals, giving metallic compounds
Lower electronegativities
Have 1-5 electrons in valence, usually not more than 3
Low ionization potentials, form cations by loss of electrons
Oxidizing agents (except noble gases)
Form oxides that react with water to give acids
Form acidic hydroxides
React with O, F, H, and other nonmetals, giving covalent compounds
React with metals, giving ionic compounds
Higher electronegativities
Usually have 4-8 electrons in valence
High electron affinities, form anions by accepting electrons in valence (except noble gases)

16. Physical Behavior Metals Nonmetals
Good conductors of heat and electricity
Malleable and ductile in solid state
Metallic luster
Opaque
High density
Mostly solids
Crystal structure in which each atom surrounded by 8-12 nearest neighbors (metallic bonds between atoms)
Poor conductors
Brittle and nonductile in solid state
Show no metallic luster
May be transparent or translucent
Low density
Gases, liquids, or solids
Form molecules that consist of atoms covalently bonded; noble gases monatomic

17. Metalloids Has both properties
Has appearance of metal, but behaves chemically like nonmetal
Boron (B), Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te), Polonium (Po), Astatine (At)
Not Aluminum
Semiconductors of electricity
Conductivity increases with temp. (metals decrease)
Ex: Silicon
Metallic luster
Forms weak acid

18. Periodic Trends
Consistent with trends of ionization energy, electron affinity, and electronegativity
Effective nuclear charge increase across period (left to right) and decrease down group (top to bottom)
Atomic Radius (decrease)
Ionization Energy (increase)
Electron affinity (general increase)
Electronegativity (increase)
Polarizability (Decrease)

19. Dependence Oxidation Number
As oxidation number of element increases, metallic behavior decreases, nonmetallic behavior increases
HOCl (+1) is weak acid, HClO4 (+7) is strong acid
TlCl (+1) is ionic,
TlCl3 (+3) is covalent

20. Acidic and Basic Properties
Basic oxide—oxide that reacts with acids
Acidic oxide—oxide that reacts with bases
Amphoteric oxide—oxide with both basic and acidic properties
MgO(s)+ 2HCl(aq) ––––> MgCl2 (aq) + H2O(l)
CO2 (g) + NaOH(aq) ––––> NaHCO3(aq)
Al2O3(s) + 6HCl(aq) ––––> 2AlCl3(aq) + 3H20(l)
Al2O3(s) + 2NaOH(aq) ––––> 2Na[Al(OH)4](aq)

21. Helpful Websites:
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