Periodic Trends

Periodic Trends

The periodic table tells us more than just basic information. It's organization can also tell us about properties.

Getting Started

You will need to open your chemistry notebook to the page that says "first ionization energy". This is where our notes will begin.

Practice

On the next few slides will be practice problems dealing with ionization energy.

YOU WILL NEED YOUR PERIODIC TABLE FROM YOUR NOTEBOOK.

Multiple Choice

Based on their positions in the periodic table, predict which has the largest first ionization energy: Mg, Ba, B, O, Te.

• Mg

• Ba

• B

• O

• Te

Oxygen

Oxygen is the further to the right and the closest to the top of the periodic table.

Remember: Ionization energy INCREASES from left to right and DECREASES down a group.

Multiple Choice

Based on their positions in the periodic table, predict which has the smallest first ionization energy: Li, Cs, N, F, I.

• Li

• Cs

• N

• F

• I

Cesium

Cesium is the furthest to the left and down on the periodic table.

Remember: Ionization energy INCREASES from left to right and DECREASES down a group.

Fill in the Blanks

Based on their positions in the periodic table, rank the following atoms in order of increasing first ionization energy: F, Li, N, Rb.

BE SURE TO WRITE IT IN THIS FORMAT:

W, X, Y, Z

Rb < Li < N < F

Rubidium has the lowest ionization energy since it is the furthest left and down.

Lithium is next since it is as far left as rubidium but higher on the table.

Next is nitrogen since it is high on the group and also close to the right side.

The highest ionization energy is fluorine because it is the highest up and furthest right of the listed elements.

Remember: Ionization energy INCREASES from left to right and DECREASES down a group.

Fill in the Blanks

Based on their positions in the periodic table, rank the following atoms or compounds in order of increasing first ionization energy: Mg, O, S, Si

BE SURE TO WRITE IT IN THIS FORMAT:

W, X, Y, Z

Mg < Si < S < O

Magnesium has the lowest ionization energy since it is the furthest left.

Silicon is next since it is further to the right.

Next is sulfur since it is high on the group and also close to the right side.

The highest ionization energy is oxygen because it is the highest up and furthest right of the listed elements.

Remember: Ionization energy INCREASES from left to right and DECREASES down a group.

An our next trend...

is electron affinity. Please open to that page in your chemistry notebook. You will now be taking notes.

Practice

On the next few slides will be practice problems dealing with electron affinity.

YOU WILL NEED YOUR PERIODIC TABLE FROM YOUR NOTEBOOK.

Multiple Choice

Based on their positions in the periodic table, predict which has the largest electron affinity: Mg, Ba, B, O, Te.

• Mg

• Ba

• B

• O

• Te

Oxygen

Oxygen is the furthest to the right on the periodic table of these options.

Remember: Electron affinity INCREASES from left to right and DECREASES down a group.

Multiple Choice

Based on their positions in the periodic table, predict which has the smallest electron affinity: Li, Cs, N, F, I.

• Li

• Cs

• N

• F

• I

Cesium

Cesium is the furthest to the left and lowest down on the periodic table of these options.

Remember: Electron affinity INCREASES from left to right and DECREASES down a group.

Fill in the Blanks

Based on their positions in the periodic table, rank the following atoms in order of increasing electron affinity: F, Li, N, Rb.

BE SURE TO WRITE IT IN THIS FORMAT:

W, X, Y, Z

Rb < Li < N < F

Rubidium has the lowest electron affinity since it is the furthest left and down.

Lithium is next since it is as far left as rubidium but higher on the table.

Next is nitrogen since it is high on the group and also close to the right side.

The highest electron affinity is fluorine because it is the highest up and furthest right of the listed elements.

Remember: Electron affinity INCREASES from left to right and DECREASES down a group.

An our next trend...

is atomic radius. Please open to that page in your chemistry notebook. You will now be taking notes.

Practice

On the next few slides will be practice problems dealing with atomic radius.

YOU WILL NEED YOUR PERIODIC TABLE FROM YOUR NOTEBOOK.

Multiple Choice

Which of the following atoms has the largest atomic radius?

• P

• S

• Se

• As

Arsenic

Arsenic is the furthest left and down on the periodic table of these options.

Remember: Atomic radius DECREASES across the period and INCREASES down the group.

Multiple Choice

Which of the following alkali metals has the greatest atomic radius?

• Rubidium

• Lithium

• Hydrogen

• Sodium

Rubidium

It is the lowest in the group.

Remember: Atomic radius DECREASES across a period and INCREASES down a group.

Multiple Choice

Which of the following elements has the greatest atomic radius?

• B

• N

• O

• C

• F

Boron

It is the furthest left out of the element choices.

Remember: Atomic radius DECREASES across the period and INCREASES down a group.

Multiple Choice

Which of the given atoms has the smallest atomic radius?

• Bi

• P

• N

• As

Nitrogen

It is the highest up in the group.

Remember: Atomic radius DECREASES across a period and INCREASES down a group.

An our next trend...

is ionic radius. Please open to that page in your chemistry notebook. You will now be taking notes.

Practice

On the next few slides will be practice problems dealing with ionic radius.

YOU WILL NEED YOUR PERIODIC TABLE FROM YOUR NOTEBOOK.

Fill in the Blanks

Put the following ions in order from largest to smallest: S^2-, Cl^–, Si^4-, P^3-

USE THE FORM:

X, X, X, X

AND DO NOT INCLUDE THE CHARGE.

Si^4-, P^3-, S^2-, Cl^-

The more negative the ion, the larger the size.

Remember: Ionic radius INCREASES the more negative the ion and DECREASES the more positive the ion.

Fill in the Blanks

Put the following ions in order from largest to smallest: Be²⁺, B³⁺, Li⁺, C⁴⁺

USE THE FORM:

X, X, X, X

AND DO NOT INCLUDE THE CHARGE.

Li⁺, Be²⁺, B³⁺, C⁴⁺

The more positive the ion, the larger the size.

Remember: Ionic radius INCREASES the more negative the ion and DECREASES the more positive the ion.

An final next trend...

is electronegativity. Please open to that page in your chemistry notebook. You will now be taking notes.

Practice

On the next few slides will be practice problems dealing with electronegativity.

YOU WILL NEED YOUR PERIODIC TABLE FROM YOUR NOTEBOOK.

Multiple Choice

Which member of the alkaline earth metals has the highest electronegativity?

• Be

• Mg

• Ca

• Sr

• Ba

Beryllium

It is at the top of the alkaline earth metals group and therefore has the highest electronegativity.

Remember: Electronegativity INCREASES across a period and DECREASES down a group.

Fill in the Blanks

Order the following elements from highest to lowest electronegativity: K, Sc, Ca, Zn, Br

USE THE FORM:

X, X, X, X, X

Br > Zn > Sc > Ca > K

Bromine is the furthest to the right and therefore the most electronegative.

Zinc is the second furthest to the right.

Scandium is third closest.

Calcium is second furthest left.

Potassium is the furthest left and therefore the least electronegative.

Remember: Electronegativity INCREASES across a period and DECREASES down a group.

Multiple Choice

Which element is the most electronegative on the periodic table?

• Iodine

• Fluorine

• Lithium

• Francium

Fluorine

It is the furthest to the right and the highest on the periodic table.

Remember: Electronegativity INCREASES across a period and DECREASES down a group.

Great Job!!!

You've finished all the notes and practice for the periodic trends.

Please get in touch with any questions.