Name:Date:

Periodic Table Lab

Purpose: Students will 1) demonstrate an understanding of periodicity; and 2) graph the atomic radius, ionization energy, electronegativity, and density of various atoms to determine any trends in these values.

Pre Lab Question:1. Use your notes or a textbook to define the following: atomic radius, ionization energy, and electronegativity.

Procedures:

Period Trends

1. Using the graphing calculator determine the atomic radii, ionization energy, electronegativity, density, and state of the following elements: Li, Be, B, C, N, O, F, and Ne. Do this by pressing the blue APPS key, scroll to Periodic and press ENTER. Scroll to find Li on the periodic table. When cursor is on Li press ENTER, scroll down past the electron configuration and the next value should be the atomic radius(for Li it should be RADIUS: 152). The next value under the atomic radius is the ionization energy (for Li 1st ION: 520). Under the ionization energy value is the electronegativity (for Li ELECTRONEG: 0.98). The density is listed next (for Li DENSITY: 0.534). Determine the units for atomic radius, ionization energy, electronegativity, and density by selecting HELP. To select HELP press the blue WINDOW key. Once you have determined the units select ESC by pressing the blue GRAPH key. Scroll down past the BOILING PT to find the state of Li (for Li STATE: SOLID). Record these values in Data Table 1 (make sure you include units in your data table).

2. Repeat step 1 for the remaining elements in period 2 and record your data in Table 1.

Groups Trends

3. Repeat step 1 to complete Data Table 2.

Graphing the Trends

4. On your graph paper, under Data and Calculations, construct eightlarge (at least ½ a page per graph)graphs using the following guidelines:

Graph 1: Graph a line graph of the Atomic Radii VS Atomic Number of the elements in Period 2. Place atomic number on the x-axis and atomic radius (in picometers) on the y-axis.

Graph 2: Graph a line graph of the Ionization Energy VS Atomic Number of the elements in Period 2. Place the atomic number on the x-axis and ionization energy (in kJ/mol) on the y-axis.

Graph 3: Graph a line graph of the Electronegativity VS Atomic Number of the elements in Period 2. Place the atomic number on the x-axis and electronegativity on the y-axis.

Graph 4: Graph a line graph of the Density VS Atomic Number of the elements in Period 2. Place theatomic number on the x-axis and density (in g/cm3) on the y-axis.

Graphs 5-8: Follow the same guidelines as graphs 1-4, but use the elements in Group 2 (listed in Data Table 2).

Data:

Data Table 1: / Period / Trends
Name of Element / Period Number / Atomic Number / Atomic Radius / Ionization Energy / Electroneg-ativity / Density / State (solid, liquid, or gas)
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
Data Table 2: / Group / Trends
Name of Element / Group Number / Atomic Number / Atomic Radius / Ionization Energy / Electroneg-ativity / Density / State (solid, liquid, or gas)
Beryllium
Magnesium
Calcium
Strontium
Barium
Radium

Conclusion Questions:

1. Based on your Data Tables and the graphs complete the following with either “increases” or “decreases.”

Overall, what is the trend for following values within a period:

The atomic radius ______as you move across the periodic table from left to right.

The ionization energy ______as you move across the periodic table from left to right.

The electronegativity ______as you move across the periodic table from left to right.

The density of SOLIDS ______as you move across the periodic table from left to right.

2. Based on your Data Tables and the graphs complete the following with either “increases” or “decreases.”

Overall, what is the trend for following values within a group:

The atomic radius ______as you move down a group from top to bottom.

The ionization energy ______as you move down a group from top to bottom.

The electronegativity ______as you move down a group from top to bottom.

The density of SOLIDS ______as you move down a group from top to bottom.

3. Based on its position in the periodic table, which atom is larger: magnesium or sulfur?

4. Based on its position in the periodic table, which has higher ionization energy: nitrogen or phosphorus?

5. Based on its position in the periodic table, which has a greater electronegativity: sodium or cesium?

6. Based on its position in the periodic table, which has the lower density: potassium or nickel?

7. Using your graph for Density vs Atomic Number, try to predict what the density would be for an element with atomic number 40.

8. Calculate the percent error for problem 7 if the accepted density for atomic number 40 is 6.52 g/cm3. % Error = Accepted – Experimental X 100

Accepted