the periodic table chapter 5. alchemy & diderot's alchemical chart of affinities (1778):

The Periodic Table

Chapter 5

Alchemy & Diderot's Alchemical Chart of Affinities (1778):

Dalton's elements and symbols (1808):

The Bayley Pyramid Periodic Table

Mohammed Abubakr's circular periodic table is one alternative to the standard periodic table of the elements.

A Spiral Periodic Table by Prof. Thoedor Benfey

Spiral Periodic Table

The Dufour Periodictree

AtomFlowers A periodic table that gives a representation of the electron orbitals that look like flowers

Chinese periodic table

Chapter 5 section 1pg 126-129

Organizing the Elements

• 1750 = 17 elements known– Mostly common metals

• After 1750, more chemists begin to study elements many more elements discovered faster

• Needed a way to organize elements– 1789 Antoine Lavoisier grouped

elements based on type• Metals, nonmetals, gases & earths

– 1860 Mendeleev

• What was going on in history during this time?

• Why is this organization limited?

Mendeleev’s Periodic Table• Organized elements like

a deck of cards– 1st order by mass– 2nd property patterns

• esp. rxns with O & H

• Draw an example of ordering strategy

A 2 4 5 6

8

7

9 10 QJ K

A 2 43

5 6 87

9 10 QJ

K

Mendeleev’s Periodic Table• Organized elements like

a deck of cards– 1st order by mass– 2nd property patterns

• esp. rxns with O & H

– Rows (called periods)• Mass increases from left to

right

– Columns (called groups)• Mass increases from top to

bottom• Similar properties

• Draw an example of ordering strategy

• Draw a small periodic table to illustrate rows and columns

groups

periods

groupspe

riods

Mendeleev’s Periodic Table

• Left blanks for elements not discovered yet

• Why remember Mendeleev if he wasn’t the first to come up with a P.T.?– Best organization strategy– Used to make accurate predictions about

what elements were yet to be discovered

Mendeleev’s Periodic Table• EX: Gallium

– Predicted similar properties to aluminum» Soft metal» Low melting point» Density ~ 5.9 g/cm3

– Truth about gallium:» Soft metal» Melting pt 29.7˚C» Density 5.91 g/cm3

• Further proof his PT was good:– Discovery of scandium and germanium

Would gallium be a solid, liquid or gas at room temperature (20-22˚C)?

Check your understanding

• Pg 126 reading strategy

• Pg 127 figure 3

• Pg 129 figure 4 (already done )

• Pg 129 assessment, #1-8

REMINDER!!!

• Open note reading quiz

WARNING

Chapter 5 section 2pg 130-138

5.2

• More on Mendeleev (note: 1860)– Did not know about protons– Did not know that all atoms in an

element have the same # of protons– His PT arranged by mass, ours by atomic

#

5.2

• Periods– Rows (side-to-side)– # of periods = # of electron energy

levels

• Groups – Columns (up-and-down)– Similar properties– Similar electron configuration

• Determines chemical properties

5.2

• Atomic mass– # given on PT is an average of the element’s

isotope masses

• Weighted avg.s– Atomic mass = avg. mass of isotopes

compared to how common they are

• AMU– Atomic Mass Unit– Unit of mass for atoms (like grams but much

smaller!)

5.2

• Classes of Elements– Solid, liquid, gas dependant on temp.

– Occur naturally vs. those that do not (man-

made)

– Metals, nonmetals, metalloids

5.2

• Metals– Most elements are metals (+75%!)– Physical properties

• Good conductors• Solids at room temp. (except for Hg)• Malleable• ductile

– Chemical properties• Some are reactive, others are not

(to rust or not to rust?)

5.2

• Special Metals– Transition metals

•Chemical properties–Form compounds with distinctive

colors•Lanthanide & actinide series

5.2

• Nonmetals– Physical properties

• Poor conductors• Brittle • Most are gasses at room temp. (low bp)

– Chemical properties• Vary some very reactive, others not at all• Most reactive = group 17• Least reactive = group 18

5.2

• Metalloids– Physical properties

• Conductivity varies with temp.

• Semi-conductors computer chips “Silicon Valley”

Chapter 5 section 3pg 139-149

Part I: pg 139 & ionsPart II: pg 140-145Part III: pg 146-149

5.3 Part I

• Valence electrons– Electrons in the outermost energy level– Chemical properties depend on the

number of valence electrons– What does this mean after learning

about the organization of the PT?

Groups have similar properties so they must also have similar #s of valence electrons

5.3 Part I

• Octet– magic # in chemistry =

– Valence orbitals can hold no more than 8 e-

– All atoms want a full valence (8 e-) or none (all or nothing)

– Exceptions: H & HeWhy?

5.3 Part I• Ions

– Atoms that gain or loose e- to fill or empty the valence orbital

1p+ +1

5.3 Part I• Ions

– Atoms that gain or loose e- to fill or empty the valence orbital

2p+ Ø

5.3 Part I• Ions

– Atoms that gain or loose e- to fill or empty the valence orbital

3p+ +1

5.3 Part I• Ions

– Atoms that gain or loose e- to fill or empty the valence orbital

4p+ +2

5.3 Part I• Ions

– Atoms that gain or loose e- to fill or empty the valence orbital

5p+ +3

5.3 Part I• Ions

– Atoms that gain or loose e- to fill or empty the valence orbital

6p+ +4

`

5.3 Part I• Ions

– Atoms that gain or loose e- to fill or empty the valence orbital

6p+ -4

`

5.3 Part I• Ions

– Atoms that gain or loose e- to fill or empty the valence orbital

7p+ -3

`

5.3 Part I• Ions

– Atoms that gain or loose e- to fill or empty the valence orbital

8p+ -2

`

5.3 Part I• Ions

– Atoms that gain or loose e- to fill or empty the valence orbital

9p+ -1

`

5.3 Part I• Ions

– Atoms that gain or loose e- to fill or empty the valence orbital

10p+ Ø

`

5.3 Part I• Ions

– Atoms that gain or loose e- to fill or empty the valence orbital

11p+ +1

`

5.3 Part II

• Groups– Alkali Metals– Alkaline Earth

Metals– Transition Metals– Boron Family– Carbon Family– Nitrogen Family– Oxygen Family– Halogens– Noble Gases

• Group #– 1– 2– 3-12– 13– 14– 15– 16– 17– 18

5.3 Part II

• For each group:– List the elements in that group– How many valence electrons do they

have?– What kind of ions do they form?– Are they reactive?– What are some of their physical and

chemical properties?– Where are they found?– What are they used for?

5.3 Part III

• Elemental Friends & Foes

– Add to your group list

Transition Metals

Groups 3-12

Transition Metals

• 1st elements discovered• Make colorful compounds

– Often used to tint/color glass

• Metals– Good conductors– Malleable– Ductile– Solids at room temp. (exception Hg)

Transition Metals

• All ions are positively charged

• Valence electron #s vary Type of ion

formed varies

• Example: Iron – Fe2+ and Fe3+

Transition Metals

• Most mined

• Many uses:– Wires– Construction– Decoration