Unit 3: Periodic Table Notes Packet

Unit 3: Periodic Table

Notes Packet

You will be expected to always have your

notebook for diagrams and note taking that is

supplementary to the note sheets.

Name: ___________________________________________Date: ___________________ Introduction to the Periodic Table, Metals, Nonmetals and Metalloids

1

Aim: How is the Periodic Table arranged and what patterns emerge among the elements? Do Now: Please examine how the periodic table is arranged and with the person next to you, find as many patterns as you can. Periodic Law: ________________________________________________________________________

_____________________________________________________________________________________

_____________________________________________________________________________________

Organization of the Table

Groups 1-18: ___________________ Periods 1-7: ____________________

Groups

Elements in the same group have the:

• __________________________________________________________________________________

_________________________________________________________________________________

• _________________________________________________________________________________

__________________________________________________________________________________

Periods

Elements in the same period have the ____________________________________________________

___________________________________________________________________________________


2

Dmitri Mendeleev: Father of the Periodic Table

●Mendeleev organized the periodic table by listing elements in rows by increasing atomic mass. ●He also put them in groups by reactivity. Mendeleev’s table was close to the table we use today.

Mendeleev’s Table Modern Table

●Arranged elements by mass ● ____________________________________________

● Ordered elements in groups by ● ____________________________________________

reactivity ______________________________________

The boron staircase is the dividing line for metals and nonmetals.

Metals, Nonmetals and Metalloids

• Metals_____________________________________________________________________________

_____________________________________________________________

• ___________________________________. IT IS ONLY IN GROUP 1 BECAUSE IT HAS 1 VALENCE ELECTRON.

• Nonmetals_________________________________________________________________________

__________________________________________________________________________________

• Metalloids _________________________________________________________________________

• Metalloid elements: ________________________________________


3

Properties of Metals, Nonmetals and Metalloids

Aim: How do the properties of metals and nonmetals differ?

Metal Properties

All metals are solids except for mercury which is a liquid.

1._________________________________________________________

2._________________________________________________________

3._________________________________________________________

_________________________________________________________

4._________________________________________________________

_________________________________________________________

5. ________________________________________________________

________________________________________________________

Nonmetal Properties

The nonmetals exist as mostly gases, some solids and 1 liquid (Bromine)

1.__________________________________________________________

2.__________________________________________________________

3.__________________________________________________________

__________________________________________________________

4.__________________________________________________________

__________________________________________________________

5. __________________________________________________________

__________________________________________________________

Metalloid Properties

Metalloids can behave as a metal or a nonmetal, depending upon what type of element they are reacting with.

1._________________________________________________________

2._________________________________________________________

3._________________________________________________________

4._________________________________________________________

5. ________________________________________________________


4

Metallic and Nonmetallic Character

5

Aim: What are the properties of the representative element groups in the periodic table? Do Now:

1. Write the electron configuration for ATOM of the element below.

2. Write the electron configuration for its ION form.

3. Identify the noble gas electron configuration it matches when forming its’ ion.

Atom Ion symbol Atom’s e- configuration Ion’s e- configuration after Noble gas matchsymbol w/ charge from periodic table e- were lost/gained Mg Mg2+

___________________________ __________________________ _________________

Sr Sr2+ __________________ _________________ ___________

Why do elements in the same group have similar physical and chemical properties?

Groups of the Periodic Table

● The representative elements are found in groups 1,2 and 13-18.

• _______________________________________________________________________

• The transition metals are a shorter block of columns.

• These elements stand out from the other groups because they do not follow the same patterns and trends with their valence electrons and reactivities.

Properties of Transition Metals Groups 3-12

Electrons: ___________________________________

Ions: ________________________________________________________________________________

_____________________________________________________________________________________

Reactivity: ___________________________________________________________________________

6

Properties of the Representative Element Groups of the Periodic Table

Group 1: __________________________

Properties:

Electrons and Ions: ___________________________________

Ionization energy and Electronegativity: __________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

Reactivity: ___________________________________________________________________

_____________________________________________________________________________

General Reactivity of Metals

• ___________________________________________________________________

_____________________________________________________________

Group 2: __________________________

Properties:


Ionization energy and Electronegativity: __________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

Reactivity: ___________________________________________________________________

_____________________________________________________________________________

7

Group 17: __________________________________

Properties:


Ionization energy and Electronegativity: ___________________________________

______________________________________________________________________

______________________________________________________________________

Reactivity: ____________________________________________________________

______________________________________________________________________

______________________________________________________________________

Phases: ______________________________________________________

General Reactivity of Nonmetals

• ___________________________________________________________________

__________________________________________________________________

Group 18: __________________________

Properties:

Electrons and Ions: ____________________________________________________

Ionization energy and Electronegativity: ___________________________________

______________________________________________________________________

_______________________________________________________________________

Reactivity: ______________________________________________________________

________________________________________________________________________

________________________________________________________________________

8

Aim: To explain the trends in atomic radius, electronegativity and ionization energy in terms of nuclear charge and nuclear shielding. Definitions:

1. Electronegativity: ___________________________________________________

______________________________________________________________________

2. Ionization energy: __________________________________________

_____________________________________________________________

_____________________________________________________________

3. Atomic radius: ________________________________________

________________________________________________________

________________________________________________________

4. Nuclear charge: ____________________________________________________________________

_____________________________________________________________________________________

5. Nuclear shielding: _____________________________

________________________________________________

________________________________________________

9

Answer the following questions using your reference tables and knowledge of chemistry.

A. Trends across a period:

Complete the missing information for the elements below:

Lithium Fluorine

Ionization Energy

Electronegativity

Atomic Radius

Electron Configuration

# of Occupied PEL’s

Nuclear Charge

1. In general, state what happens to each of the following properties as you move across period 2

(indicate if it increases or decreases)

a. Ionization energy: _____________________________

b. Electronegativity: _____________________________

c. Atomic Radius: _______________________________

2. Why is the nuclear charge of Fluorine greater than the nuclear charge of Lithium?

3. Explain, in terms of nuclear charge, why Fluorine has a greater electronegativity AND ionization energy than Lithium?

4. Explain, in terms of nuclear charge, why Fluorine pulls it’s 2 principle energy levels in closer and has a SMALLER atomic radius than lithium?

10

B. Trends down a Group:

Complete the missing information for the elements to the left:

5. In general, state what happens to each of the following properties as you move down Group 1 (indicate if it increases or decreases) a. Ionization energy: _____________________________

b. Electronegativity: _____________________________

c. Atomic Radius: _______________________________

6. Explain, in terms of atomic structure, why Francium has a larger atomic radius than Lithium?

7. What happens to the amount of nuclear shielding (electrons blocking the nucleus) for an element when you move down a group? Explain in terms of number of electrons and principle energy levels.

8. Why is it easier to remove a valence electron from Francium than from Lithium? Explain your answer in terms of nuclear shielding and electron shells.

9. Why does Francium have a lower electronegativity than Lithium? Explain your answer in terms of nuclear shielding and electron shells.

11

Electronegativity, ionization energy and atomic radius down a Group

Atomic radius ________________________________________

____________________________________________________

The electronegativity and ionization energy ________________

____________________________________________________

____________________________________________________

____________________________________________________

____________________________________________________

Electronegativity, ionization energy and atomic radius across a Period

The electronegativity and ionization energy____________________________________________

__________________________________________________________________________________

__________________________________________________________________________________

Atomic radius______________________________________________________________________

__________________________________________________________________________________

Unit 3: Periodic Table Notes Packet

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