TOPIC: Metals vs Nonmetals

Classifying the Elements

• 2/3 (75%) of elements are metals• Remaining elements: non-metals & metalloids

(semi-metals)• Metalloids:

– some properties of metals & some properties of nonmetals

• Staircase: – dividing line between metals & nonmetals – elements to left are metals (except H)– elements to right are non-metals

Most elements are solid at room temperature

• Some nonmetals are gases– All the noble gases, of course– Some diatomics (H2 N2 O2 F2 Cl2)

• There are only 2 Liquids at STP (room temp)– Br2 (non-metal) and Hg (metal)

Properties of Metals• Malleable – flattened into sheets• Ductile – drawn into wires & tubes • have Luster• Good Conductors of heat & electricity• Solid at room temperature (except Hg)• Metals lose electrons & form positive ions

“Metals are losers”• Most reactive metal is Fr• Most reactive family is Alkali Metals

So…metals don’t want electrons, they want to get rid of them

Metals also have…

• Low electronegativity (low attraction for electrons)

• Low ionization energy (doesn’t take a lot of energy to remove an electron)

Decreased Electronegativity Decreased Ionization energy

Properties of Nonmetals• generally gases or solids (except Br2)• solids are Brittle• solids are Dull• poor conductors of heat & electricity• Nonmetals gain electrons & form negative ions

“Nonmetals are winners”• Most reactive nonmetal is F

– Properties: OPPOSITE of metals

So…nonmetals love electrons, they want to take electrons

Nonmetals also have…

• high electronegativity (high attraction for electrons)

• high ionization energy (takes a lot of energy to remove an electron)

Increased Electronegativity Increased Ionization energy

Properties of Metalloids

7 metalloids: – 5 on right of staircase: B,Si,As,Te,At– 2 on left of staircase: Ge,Sb

Each metalloid has some metallic and some nonmetallic properties– Example:Si

• shiny like metal but brittle like nonmetalMetalloids are elements touching the stairs (except Al) and have some properties of metals and some of nonmetals

Size of the Atom (Atomic Radius)

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Li: Group 1 Period 2 Cs: Group 1 Period 6

Cs has more energy levels, so it’s bigger

Atomic Radius Gets Bigger

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How about as you go across?!

as go across row size tends to decrease a bit because of greater PPP “proton pulling power”

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Atomic Radius Gets Smaller