Chapter 6Chapter 6The Periodic TableThe Periodic Table

Mr SamaniegoMr Samaniego

Lawndale High SchoolLawndale High School

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?

Which one does not belong?Which one does not belong?

Which one does not belong?Which one does not belong?

Section 6.1 - Organizing the ElementsSection 6.1 - Organizing the Elements

By the 1700’s, only about 13 elements By the 1700’s, only about 13 elements had been identifiedhad been identified

The discovery of elements has been an The discovery of elements has been an ongoing process since ancient timesongoing process since ancient times

In the 1800’s, there were only 31 In the 1800’s, there were only 31 known elementsknown elements

By 1865, that number had more than By 1865, that number had more than doubled to 65 known elementsdoubled to 65 known elements

History of the Periodic TableHistory of the Periodic Table

In 1869, Dmitri Mendeleev published a In 1869, Dmitri Mendeleev published a classification scheme of all the classification scheme of all the currently known elementscurrently known elements

Mendeleev insisted that Mendeleev insisted that elements with similar elements with similar characteristics be listed characteristics be listed in the same familyin the same family

He also left blank spaces in his table He also left blank spaces in his table for undiscovered elementsfor undiscovered elements

Mendeleev’s Periodic TableMendeleev’s Periodic Table

From 1829 to 1869, many other From 1829 to 1869, many other scientists proposed different systems, scientists proposed different systems, but none gained wide acceptancebut none gained wide acceptance

In 1869, Dmitri Mendeleev arranged In 1869, Dmitri Mendeleev arranged the elements in his periodic table in the elements in his periodic table in order of increasing atomic mass AND order of increasing atomic mass AND repeating propertiesrepeating properties

Chemists used the properties of elements Chemists used the properties of elements to sort them into groupsto sort them into groups (columns) (columns)

Mendeleev’s Periodic Table (1869)Mendeleev’s Periodic Table (1869)

Albert Tarantola’s

Orbital Table

                                                                    

       

Timothy Stowe – Table for Physicists

                                                

     

Theodor Benfey

                                                                   

        

Emil Zmaczynski

                                                  

     

Vocational Exile Periodic Table

The Periodic LawThe Periodic Law

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

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

About 40 years later, Henry Moseley About 40 years later, Henry Moseley determined atomic numbers for each determined atomic numbers for each known element so…known element so…

Metals, Metalloids and NonmetalsMetals, Metalloids and Nonmetals(Red or Black “Ladder” on the periodic table aka zigzag line)(Red or Black “Ladder” on the periodic table aka zigzag line)

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

MetalsMetalsNonmetalsNonmetalsMetalloidsMetalloids

Metals: elements that are generally Metals: elements that are generally solid at room temperature, have a solid at room temperature, have a grayish color and shiny surface, and grayish color and shiny surface, and conduct heat and electricityconduct heat and electricity

Nonmetals: elements that have Nonmetals: elements that have varying properties but are varying properties but are generally poor conductors of generally poor conductors of heat and electricityheat and electricity

Metalloids: elements with Metalloids: elements with some properties of metals some properties of metals and nonmetalsand nonmetals

Section 6.2 - Classifying the ElementsSection 6.2 - Classifying the Elements(Page 162-163)(Page 162-163)

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

Groups and Periods on the PTGroups and Periods on the PT

Element that are solid at R.T. are usually Element that are solid at R.T. are usually printed in black, liquid at R.T. printed in printed in black, liquid at R.T. printed in blue, and gases at R.T. are printed in greenblue, and gases at R.T. are printed in green

Periodic Table at Different TemperaturesPeriodic Table at Different Temperatures

1.1. HydrogenHydrogen2.2. Alkali Metals (Group 1A)Alkali Metals (Group 1A)3.3. Alkaline Earth Metals (Group 2A)Alkaline Earth Metals (Group 2A)4.4. Chalcogens (Group 6A)Chalcogens (Group 6A)5.5. Halogens (Group 7A)Halogens (Group 7A)6.6. Noble Gases (Group 8A)Noble Gases (Group 8A)7.7. Transition Metals (Group B)Transition Metals (Group B)8.8. Inner Transition Metals Inner Transition Metals

(Lanthanides and Actinides)(Lanthanides and Actinides)

The 8 Groups of the Periodic TableThe 8 Groups of the Periodic Table

PracticePractice

Which group are the following elements in?Which group are the following elements in?1.1. FluorineFluorine2.2. CalciumCalcium3.3. IronIron4.4. OxygenOxygen5.5. KryptonKrypton6.6. LithiumLithium7.7. UraniumUranium8.8. HydrogenHydrogen

Electron Configurations in GroupsElectron Configurations in Groups Elements can be sorted into Elements can be sorted into

different groups based on their different groups based on their electron configurationelectron configuration

Noble Gases Noble Gases always have their always have their s and p orbital s and p orbital completely filled completely filled with electrons, with electrons, which makes which makes them relatively them relatively inactiveinactive

Representative ElementsRepresentative Elements Representative Elements are Groups Representative Elements are Groups

1A through 7A 1A through 7A because they display a because they display a wide range of physical and chemical wide range of physical and chemical propertiesproperties

Section 6.3 – Periodic TrendsSection 6.3 – Periodic Trends

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

We will be studying 3 periodic trends:We will be studying 3 periodic trends:–Atomic RadiusAtomic Radius–Ionization EnergyIonization Energy–ElectronegativityElectronegativity

1. Atomic Radius or Atomic Size1. Atomic Radius or Atomic Size

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

Radius

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

Atomic Radius increases towards the Atomic Radius increases towards the bottom left corner of the PTbottom left corner of the PT

Which element has a greater atomic Which element has a greater atomic radius?radius?– F or CsF or Cs– Ga or KGa or K– Kr or RbKr or Rb– Ba or SiBa or Si– Fr or WFr or W– O or AgO or Ag

Atomic Radius/Size Practice

IonsIons

When elements combine in When elements combine in compounds, they do not have the compounds, they do not have the same number of protons and same number of protons and electrons anymoreelectrons anymore

Ions are atoms that have a positive Ions are atoms that have a positive or negative charge.or negative charge.

Remember that neutral atoms have Remember that neutral atoms have the same number of protons and the same number of protons and electronselectrons

CationsCations

Positive and negative ions form when Positive and negative ions form when electrons are transferred between electrons are transferred between atoms (given up or stolen away)atoms (given up or stolen away)

Cation – an ion with a positive charge Cation – an ion with a positive charge (lost electrons)(lost electrons)

AnionsAnions Anion – an ion with a negative charge Anion – an ion with a negative charge

(gained electrons)(gained electrons)

Ionic SizeIonic Size Cations are always smaller than the Cations are always smaller than the

atoms from which they formatoms from which they form Anions are always larger than the Anions are always larger than the

atoms from which they formatoms from which they form

PracticePractice

Which of the following is larger?Which of the following is larger?– Na or NaNa or Na++

– Al or AlAl or Al3+3+

– I or II or I--

– CaCa2+2+ or Ca or Ca– S or SS or S2-2-

– OO2-2- or O or O

2. Ionization Energy2. Ionization Energy The energy required to remove an The energy required to remove an

electron from an atomelectron from an atom

Ionization EnergyIonization Energy What trend do you notice about the ionization What trend do you notice about the ionization

energy of the elements on the periodic table?energy of the elements on the periodic table?

Ionization Energy increases towards the Ionization Energy increases towards the top right corner of the PTtop right corner of the PT

Which of these elements has a Which of these elements has a greater ionization energy?greater ionization energy?– Kr or ArKr or Ar– Al or NaAl or Na– S or RbS or Rb– Si or CsSi or Cs– He or CaHe or Ca– P or OP or O

Ionization Energy Practice

3. Electronegativity3. Electronegativity The ability of an atom to attract electrons to The ability of an atom to attract electrons to

itself when in a compounditself when in a compound

ElectronegativityElectronegativityWhat trend do you notice about the electronegativity of What trend do you notice about the electronegativity of

the elements on the periodic table?the elements on the periodic table?

Electronegativity increases towards the Electronegativity increases towards the top right corner of the PTtop right corner of the PT

Which element has greater Which element has greater electronegativity?electronegativity?– Na or FNa or F– Ca or CCa or C– Al or MgAl or Mg– Sr or AlSr or Al– Ca or KCa or K– Cl or FCl or F

Electronegativity Practice