Periodicity Experiment #7

Determine the number of atoms in 10.03g of Copper

From last lab

Cu of atoms 9.51X10

Cu of 1mol

Cu of atoms6.02X10

Cu of 63.55g

Cu of 1mol

1

Cu of 10.03g

22

23

The Periodic Table:

MetalsNon-metals Metalloids

Valence Electrons Electronegativity Ionization EnergyAtomic Radius

1

2

3

Periods ↔ Columns or Groups ↕

Metals •Found to the left of the periodic table.•75% of the elements are metals. •Good conductors of heat and electricity•Malleable and good reflectors of light •Metals tend to lose electrons•Almost all are solid at room temperature

Metals Non-Metals and Metalloids

Non-metals Found to the right of the periodic table. Poor conductors of heat and electricity

Most are gases at room temperature Non-metals tend to gain electrons

Metalloids Found adjacent to the “stair case”. Metalloids exhibit properties of both metals and nonmetals.

Ionization energy and Electronegativity

Ionization energy/ Electronegativity

Increase

Electronegativity Vs. Ionization Energy

• Electronegativity - the attraction an atom has for its Valence electrons.

• Ionization energy - the amount of energy that is needed to remove an electron from its Valence shell.

• They both increase traveling across the table from left to right, and decrease traveling down the table.

Atomic Radius

atomic radiusIncreases going down Atomic radius

decreases going to the right

Reactivity Group #1 very reactive metal1 Val e-

Atomic Radius?Ionization Energy? Electronegativity?

Group #2 reactive metal 2 Val e-Atomic Radius?Ionization Energy? Electronegativity?

Group # 7Very reactive non-metal 7 Val e-Atomic Radius?Ionization Energy? Electronegativity?

Why is group # 1more reactive then group # 2?

Why is group # 8 Nobel gases uncreative?

Why is it easier for elements in group 1 to loose 1e- then to gain 7e-? Why is it easier for element in group 7 to gain 1e- then to loose 7e-?

Amphoteric Properties # 4 pg 98

•Test NaOH for basic behavior with addition of acid •Add 9 drops of H2O and 1 drop of NaOH to a test tube•Add 2 drops phenolpthalein (indicator) to same test tube.•Add dropwise Hydrochloric acid (HCL)

•Test NaOH for acidic behavior with addition of a base•Add 9 drops of H2O and 1 drop of NaOH to a test tube•Add 2 drops phenolpthalein (indicator) to same test tube.•Add 2 drops of NH4 OH ( a base)•Record results

Second Test Tube

Due Next Lab

• Pg 101 & 103 Sections 1-4; use your amphoteric trial data to complete 4a-4d pg103.

• Pg 104 Questions 1-8 • For question # 5 Graph all elements 1-36• Atomic # (X-axis) Ionization energy (Y-Axis)• Graphs made by hand will not be accepted. • Ionization energy data found in Lab • pg 106 observations from lab # 7

Atomic Number Vs. Ionization Energy

He

Ne

Ar

Kr

Li NaK

0

500

1000

1500

2000

2500

0 10 20 30 40

Atomic Number

Ioniz

ation E

nergy (kJ/m

ol)

Lou Tisone Chem. 116-01

Fall 06

• Metal + Oxygen Metal Oxide

• 2Mg + O2 2MgO

• Metal Oxide + Water Base

• MgO+ 2H2O Mg(OH)2

• Metal + Water Base + H2

• Mg+ 2H2O Mg(OH)2 + H2

Reactions With Metals

Non-Metal + Oxygen Non-Metal OxideS + O2 SO2

Non-Metal Oxide + Water Oxy-AcidSO3 + H2O H2S04

Metalloids – May act as an acid or base (Amphoteric)

Reactions with Non-Metals