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 Groups
Team Alkali Metals
Anthony C
Donald C
Noah S
Team Alkaline Earth Metals
Tatyana K
Isaiah F
Bethany L
Team Halogens
Tyler H
JadiAnn H
Jorge M
Team Transition Metals
Team Noble Gases
Tim B
Autumn S
JaQuona R
Metals, Metalloids & Nonmetals:
Metals, Metalloids & Nonmetals:
Property
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
METAL
SEMIMETAL
NONMETAL
Property
LOCATION
LUSTER – SHINY?
CONDUCTIVE OF
HEAT & ELECTRICITY?
MALLEABLE – can bend without breaking?
PHYSICAL STATE at RT?
Important examples:
Ionization Energy
Electronegativity
TENDENCY TO LOSE OR TO GAIN
ELECTRONS?
# OF
VALENCE ELECTRONS
METAL
SEMIMETAL
NONMETAL
right & above
staircase line
bordering the
staircase line
left & below the
staircase line
yes - luster
maybe
no - dull
yes
maybe
no
yes – malleable &
ductile
maybe
no- brittle & hard
solids,
Mercury (Hg) is
only liquid metal
solids
Solids – I2
Liquid – Br
Gas – N2, O2, F2, Cl2
Au, Ag, Fe, Ni, Cr,
Na, K , Fr, Ca, Mg,
Pt
Al, Si, Ge
C, S, P, Br2, I2,N2,
O2, F2, Cl2
Lo IE & lo EN
N/A
Hi IE & Hi EN
Lose,
forming cations
Gain or Lose
Gain,
Forming anions
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 (IIA)
13 (IIIA)
14(IVA)
15 (VA)
16 (VIA) 17 (VIIA) 18 (VIIIA)
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 270
X-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 1350
X-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
IA
1
2
3 Na
4 K
5
6
7 Fr
2
IIA
13
14
15
16
17
IIIA IVA VA VIA VIIA
F
Mg
Ca
3
4
5
6
7
8
9
10
11
12
18
VIIIA
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.
Na
K
Physical properties of group IA & IIA metals
IA (1)
IIA (2)
Mg
Ca
Observe the reactions of each metal as the
instructor places it in water. Record your
observations below.
Na
K
Reactivity of group IA (1) & IIA (2) metals in water
IA (1)
IIA (2)
Mg
Ca
Video demos of alkali metals
Video of sodium in water
Video if potassium in water
Video of Cesium in water
Video 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 & electronegativity
lose 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 & electronegativity
lose 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/ F
BP increases with increasing size
Never found free in nature: groups 1, 2, 17
Colored ions due to multiple oxidation states: transition metals