Learning objectives:After completing this unit of study, you should be able to: • An element’s location on the periodic table gives an indication of its physical and chemical properties.• Elements on the Periodic Table are arranged in order of increasing atomic number.• Elements are classified as metals, nonmetals and metalloids based on their properties and location on

the periodic table.• Groups 1, 2, and 13-18 have the same number of valence electrons in the group, and therefore have

similar chemical properties. Helium is the exception to this. • Each group shows trends in atomic radius, ionic radius, Electronegativity, first ionization energy, and

metallic and nonmetallic properties.• Each period shows trends in atomic radius, Electronegativity, first ionization energy, and metallic and

nonmetallic properties.• When an element becomes an anion by gaining electrons, the radius increases.• When an element becomes a cation by losing electrons, the radius decreases.• Some elements exist as two or more forms in the same phase due to differences in molecular or crystal

structures, and therefore have different chemical and physical properties. These are called Allotropes. Carbon has the allotropes coal, graphite, diamond, and fullerenes. Oxygen has the allotropes O2 & O3.

Element song

• SpongeBob sings it!• So do the Chipmunks!

Cooperative GroupsTeam Alkali Metals

Anthony CDonald CNoah S

Team Alkaline Earth MetalsTatyana KIsaiah FBethany L

Team HalogensTyler HJadiAnn HJorge M

Team Noble GasesTim BAutumn SJaQuona R

Team Transition Metals

Metals, Metalloids & Nonmetals:

Metals, Metalloids & Nonmetals:

Property METAL SEMIMETAL NONMETAL  LOCATION 

     

 LUSTER – SHINY? 

     

 CONDUCTIVE OF HEAT & ELECTRICITY? 

     

 MALLEABLE – can bend without breaking? 

     

  PHYSICAL STATE at RT?  

     

  Important examples:   

     

GENERAL ATOMIC STRUCTURE 

     

TENDENCY TO LOSE OR TO GAIN ELECTRONS? 

     

# OF VALENCE ELECTRONS

  

   

Property METAL SEMIMETAL NONMETAL  LOCATION 

 right & above staircase line

 bordering the staircase line

 left & below the staircase line

 LUSTER – SHINY? 

 yes - luster  maybe  no - dull

 CONDUCTIVE OF HEAT & ELECTRICITY? 

 yes  maybe  no

 MALLEABLE – can bend without breaking? 

 yes – malleable & ductile

 maybe  no- brittle & hard

  PHYSICAL STATE at RT?  

 solids, Mercury (Hg) is only liquid metal

 solids Solids – I2Liquid – BrGas – N2, O2, F2, Cl2

  Important examples:   

 Au, Ag, Fe, Ni, Cr, Na, K , Fr, Ca, Mg, Pt

 Al, Si, Ge  C, S, P, Br2, I2,N2, O2, F2, Cl2

Ionization EnergyElectronegativity 

Lo IE & lo EN   N/A  Hi IE & Hi EN

TENDENCY TO LOSE OR TO GAIN ELECTRONS? 

 Lose, forming cations

 Gain or Lose  Gain, Forming anions

# OF VALENCE ELECTRONS  1-3 valence e-  3-5 val e-  5-7 val e-

Shielding

• Kernel electrons interfere with the nuclear attraction for valence electrons.

• More energy levels mean that it is easier to remove an e- and harder to gain an e-, because protons are shielded by the kernel e- in between them.

Nuclear Charge

• The charge of the nucleus

• The number of protons = atomic number

• Greater nuclear charge means greater attraction of nucleus on the electrons

• Means smaller radius, harder to lose e- (IE)easier to gain e- (e-neg)

Bohr models of 3Li, 9F, 87Fr

Periodicity:

• FOLLOWS A PATTERN

• There are general trends in properties as you move left to right across a period.

• There are general trends in properties as you move top to bottom down a group.

Periodic Trend in Number of Valence Electrons

1 (IA) 2 (I IA) 13 (I I IA) 14(IVA) 15 (VA) 16 (VIA) 17 (VIIA) 18 (VII IA)

Periodic Trend in Number of Valence Electrons

1.) What is the trend in valence electron number as you go from left to right across any period on the table?   2.) What is the trend in the valence electron number as you go down any group from top to bottom?   3.) What is the trend in the number of energy levels as you go down any group from top to bottom?    4.) Use your answers to #2 & 3 to write a statement explaining the relationship between number of valence electrons and the number of energy levels.

Chem Do 3 graph

Y-axis: start at 50, increase by 10, stop at 220

X-axis : start at 10, count by .5, stop at 18

Chem Do 3b graphs“Trend in atomic radius down group 2”

Y-axis: start at 100, increase by 10, stop at 270X-axis : start at 0, count by 5, stop at 90

“Trend in ionization energy down group 1” Y-axis: start at 350, increase by 50, stop at 1350X-axis : start at 0, count by 5, stop at 90

Reactivity of Metals Demo (pg 14)

You have learned that trends occur in the physical & chemical properties of elements both horizontally & vertically on the periodic table. In this lab demonstration you will observe trends down groups 1 & 2, and the trends across periods 3 & 4.

1 2 13 14 15 16 17 18IA IIA VIIIA

1 II IA IVA VA VIA VIIA2 F3 Na Mg 3 4 5 6 7 8 9 10 11 124 K Ca567 Fr

Complete the following data table by making observations about the physical appearance of the metals shown by the instructor. Include luster(shine), hardness or softness, reaction with air.

Physical properties of group IA & IIA metals IA (1) IIA (2) Na

Mg

K

Ca

Observe the reactions of each metal as the instructor places it in water. Record your observations below.

Reactivity of group IA (1) & IIA (2) metals in water IA (1) IIA (2)

Na

Mg

K

Ca

Video demos of alkali metals

Video of sodium in waterVideo if potassium in waterVideo of Cesium in waterVideo of Francium in water

Groups/Families of the Periodic Table

Alkali Metals

Location: group 1

Characteristic Elements: Na, K, Rb, Cs, Fr

Reactivity: most active metals (Fr is THE most active metal), never found free in nature, electrolysis of fused salts.

lo IE & electronegativitylose e-, IR<AR

Alkaline Earth Metals

Location: group 2

Characteristic Elements: Be, Mg, Ca, Sr, Ba, Ra

Reactivity: very hi, but less than group 1. Also never found free in nature, electrolysis of fused salts

lo IE & electronegativitylose e-, IR<AR

Transition Metals

Location: groups 3-12

Characteristic Elements: Fe, Cu, Cr, Au, Ag, Pt, Pb, Mn, Co…

Special Characteristics: hard solids with hi MP, less reactive than groups 1 & 2

multiple oxidation states due to more than one energy level being filled at a time

colored solutions in water

Why do transition metals produce colored solutions?

MULTIPLE OXIDATION STATES!

Look at: Fe Cr Ni Cu

Halogens

Location: group 17

Characteristic Elements: F, Cl, Br, I, AS

Reactivity: most reactive NONMETALS, Also never found free in nature, electrolysis of fused salts or chemically

hi IE & electronegativity (F is highest of 4.0)gain e-, IR>AR

Exhibit all 3 states of matter (F & Cl (g), Br (l), I & As (s))

Noble Gases

Location: group 18

Characteristic Elements: He, Ne, Ar, Kr, Xe, Rn

Reactivity: monatomic because full valence shell of 8 e- (He is full w/ 2 e-) therefore, do not react

exception: Xe & Ar w/ FBP increases with increasing size

Never found free in nature: groups 1, 2, 17Colored ions due to multiple oxidation states: transition metals