Chapter 6The Periodic Table

Stylish Shoes

What is in common with all the pictures below?

Which one does not belong?

Which one does not belong?

Which one does not belong?

Which one does not belong?

History of the Periodic Table 1869 - Mendeleev published a

classification scheme of all the currently known elements

Organized elements based on similar characteristics.

Left blank spaces in table for undiscovered elements.

Mendeleev’s Periodic Table (1869)Mendeleev arranged the elements on his table in order of increasing atomic mass.

Many scientist suggested other periodic tables.

Albert Tarantola’s

Orbital Table

                                                                    

       

Timothy Stowe – Table for Physicists

                                                

     

Theodor Benfey

                                                                   

        

Emil Zmaczynski

                                                  

     

Vocational Exile Periodic Table

The Periodic Law

In the modern periodic table, elements are arranged in order of increasing atomic number

Periodic Law – when elements are arranged in order of increasing atomic number, there is a trend in their physical and chemical properties

Metals, Metalloids and Nonmetals

Elements can be grouped into three broad classes based on their general properties

MetalsNonmetalsMetalloids

Metals: Generally solid at room temp. Ductile – drawn into wires. Malleable – hammered into sheets Shiny surface Conduct heat and electricity

Metals

• Nonmetals: • Varying properties, but are generally

poor conductors of heat and electricity

• Brittle

Non-metals Nonconductors

• Metalloids: • some properties of metals and nonmetals

• Intermediate

Metalloids or Semimetals Properties of both

Practice

Tell me all you can about the following elements:

1. Titanium (Ti)2. Germanium (Ge)3. Calcium (Ca)4. Fluorine (F)

Section 6.2 - Classifying the Elements

The periodic table displays the symbols and names of the elements, along with information about the structure of their atoms (# of protons, neutrons, and electrons)

Black symbol = solid Green = gas Blue = liquid

Electron Configurations in Groups Elements can be sorted into 4 different

groupings based on their electron configurations:

1) Noble gases

2) Representative elements

3) Transition metals

4) Inner transition metals

Representative

Noble Gases

Transition

Inner Trans.

Electron Configurations in Groups

1) Noble gases elements in Group 8A

2) Very stable = do not react• Noble gases have an electron

configuration that has the outer s and p sublevels completely full

Ci

Circle the Noble Gases

Electron Configurations in Groups2) Representative Elements

are in Groups 1A through 7A• Display wide range of

properties, thus a good “representative”

• Include metals, nonmetals, metalloids, solids, gases, or liquids

• Their outer s and p electron configurations are NOT filled

Ci

Circle the Representative Elements

Electron Configurations in Groups

3) Transition metals are in the “B” columns of the periodic table

• Electron configuration has outer s sublevel full

• Elements in the “d” sublevel• A “transition” between the metal area and

the nonmetal area

Ci

Circle the Transition Metals

Electron Configurations in Groups

4) Inner Transition Metals are located below the main body of the table, in two horizontal rows

• Electron configuration has the outer s sublevel full

• Elements in the f sublevel

Ci

Circle the Inner Transition Metals

1A

2A 3A 4A 5A 6A 7A

8A Elements in the 1A-7A groups

are called the representative elements

outer s or p filling

The group B are called the transition elements

These are called the inner transition elements, and they belong here

Groups of elements - family names Group 1A – alkali metals

Forms a “base” (or alkali) when reacting with water Exception is Hydrogen

Group 2A – alkaline earth metalsAlso form bases with water; do not

dissolve well, hence “earth metals” Group 7A – halogens

Means “salt-forming”

Group 1A - alkali metals (but NOT H)

Group 2A - alkaline earth metalsH

Group 8A are the noble gases Group 7A is called the halogens

Groups of the periodic table: Representative Elements Noble Gases Transition Metals Inner Transition Metals

Family names: Alkali metals Alkaline earth metals Halogens

The Groups of the Periodic Table

Practice

Tell me all you can about the following elements:

1. Titanium (Ti)2. Germanium (Ge)3. Calcium (Ca)4. Fluorine (F)

Section 6.3 – Periodic Trends

Properties of elements are related to their location on the periodic table

We will be studying 3 periodic trends:–Atomic Radius–Ionization Energy–Electronegativity

1. Atomic Radius or Atomic Size

One-half the distance from center to center of two atoms

Atomic Radius

Atomic Radius or Atomic SizeWhat do you notice about the atomic radii of the elements on the periodic table?

Atomic Radius increases towards the bottom left corner of the PT

Which element has a greater atomic radius? F or Cs Ga or K Kr or Rb Ba or Si Fr or W O or Ag

Atomic Radius/Size Practice

Ions

When elements combine in compounds, they transfer electrons.

Ions are atoms that have a positive or negative charge.

Normally, atoms are neutral because they have the same number of protons and electrons

Transfer of an electron forms two ions: a cation and anion

Na+

Cations Cation – an ion with a

positive charge (lost electrons)

Na+

Circle the cation

AnionsAnion – an ion with a

negative charge gained electrons)

Na+

Circle the anion

Ionic SizeCations are always

smaller than the atoms from which they form

Anions are always larger than the atoms from which they form

Before

After

• Does this make sense?• Where are electrons located in the

atom?• Around the nucleus

• The more electrons around the nucleus, the larger the atom will be.

Practice

Which of the following is larger? Na or Na+

Al or Al3+

I or I-

Ca2+ or Ca S or S2-

O2- or O

2. Ionization Energy The energy required to

remove an electron from an atom

Ionization Energy What trend do you notice about the ionization

energy of the elements on the periodic table?

Ionization Energy increases towards the top right corner of the PT

• Does this make sense?• Which elements are the most

stable?• Elements with full orbitals

• The more stablethe elements is, the harder it will be to remove an electron.

Which of these elements has a greater ionization energy? Kr or Ar Al or Na S or Rb Si or Cs He or Ca P or O

Ionization Energy Practice

3. Electronegativity (EN) The ability of an atom to

attract electrons to itself when in a compound

ElectronegativityWhat trend do you notice about the electronegativity of

the elements on the periodic table?

Electronegativity increases towards the top right corner of the PT

• Does this make sense?• Which elements want electrons?

• Elements closest to filling their orbitals

• The closer the elements is to filling its orbital, the more it will attract electrons.

Which element has greater electronegativity? Na or F Ca or C Al or Mg Sr or Al Ca or K Cl or F

Electronegativity Practice

Draw a diagonal arrow showingincreasing atomic size

Draw a diagonal arrow showingincreasing ionization energy

Draw a diagonal arrow showingincreasing electronegativity