Name:††††††††††††††††††††††††††††††††††††††††††††††††††††††††††††††††††††††††† Date:††††††††††††††††††††††††††† Quan/Chem

 

 

Exploring the Coolness of the Periodic Table

 

Directions:Print out a copy of this lab sheet for you to write your answers on.

 

Background:The periodic table is arranged according to the Periodic Law which states that when elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern.The properties you will be examining in this lesson are atomic radius, ionic radius, first ionization energy, and electronegativity.Use your book to define those terms

 

*Atomic Radius:

 

 

 

*Ionic Radius:

 

 

 

*Shielding:

 

 

 

*First Ionization Energy:

 

 

 

 

Use the online periodic table at www.webelements.com to assist you in answering these questions (in case you donít know the answers off the top of your head.)

 

  1. For the first three elements in rows 2 and 3 (Li, Be, B then Na, Mg, Al) find the Atomic Radius and fill in the table below

 

Li

Be

B

Na

Mg

Al

 

  1. What appears to be the trend in atomic radius as you move from left to right?

 

 

  1. What explains that trend?

 

 

 

  1. What appears to be the trend in atomic radius as you move down a column?

 

 

  1. What explains that trend?

 

 

 

  1. Predict the CHANGE in atomic radius of the next elements in a row (C, N, O, F, Ne and Si, P, S, Cl, Ar) then click the button to check those predictions.How close were your predictions?†††

PREDICTIONS

C

N

O

F

Ne

Si

P

S

Cl

Ar

 

Fill in the master table for atomic radius.

  1. Is the pattern of atomic radius always true or generally true?

 

 

 

Fill in the table for ionic radius.

  1. What appears to be the trend in ionic radius as you move from left to right in a row?

 

 

  1. What explains that trend?

 

 

  1. What appears to be the trend in ionic radius as you move down a column?

 

 

  1. What explains that trend?

 

 

Fill in the table for 1st ionization energy.

  1. What appears to be the trend in 1st ionization energy as you move from left to right in a row?

 

 

  1. Why is it easier to remove that first electron from Lithium than fluorine?

 

 

 

  1. What appears to be the trend in 1st ionization energy as you move down a column?

 

 

  1. Why is it easier to remove that first electron from sodium than lithium?

 

 

 

Use the links below to examine the same properties graphically

 

††††††††††† Atomic Radius:†††††††††††† www.webelements.com/webelements/properties/text/image-balls/atomic-radius-emp.html

 

††††††††††† Ionic Radius:†††††††††††††††† www.webelements.com/webelements/properties/text/image-balls/radius-ionic-pauling-1.html

 

††††††††††† 1st Ionization:††††††††††††††† www.webelements.com/webelements/properties/text/image-balls/ionization-energy-1.html

 

 

 

 

 

Element Name

 

Li

Be

B

C

N

O

F

Ne

Atomic Radius

Unit:

 

 

 

 

 

 

 

 

 

Ionic Radius

Unit:

 

 

 

 

 

 

 

 

 

 

1st Ionization Energy

Unit:

 

 

 

 

 

 

 

 

 

 

 

 

Element Name

 

Na

Mg

Al

Si

P

S

Cl

Ar

Atomic Radius

Unit:

 

 

 

 

 

 

 

 

 

Ionic Radius

Unit:

 

 

 

 

 

 

 

 

 

1st Ionization Energy

Unit: