Patterns in the Periodic Table

Patterns in the Periodic Table

Chemistry • Tuesday 1/31/23

Agenda

Materials

1.

Learning Objective

2.

Practice

3.

Patterns of the Periodic Table

1.Periodic Table

2.Notes #2: Patterns in PToE

3.Pen/pencil

4.5 Different Colored Pencils

Learning Objectives

Learning Target

2

Success Criteria:

Students can describe the organization and patterns of the
Periodic Table of Elements (PToE).

❏

I can identify patterns in properties of elements on the PToE.
❏

Nuclear Charge, Electron Shielding, Ionization Energy,
Atomic Size, Electronegativity

Chemistry Name GameAtomic Structure and the PToE

Patterns

7
Chemistry Name Game

Atomic Structure and the PToE

Groups - Columns

●There are 18 groups

●Elements in a group have similar
properties.

Period - Row

●There are 7 periods

●Each period adds a new energy level

Patterns - Nuclear Charge

Atomic Structure and the PToE

Increases

Open Ended

How do you determine if one atom has more nuclear charge than another?

Multiple Choice

What is the Nuclear charge of yttrium? 

• 40

• 41

• 38

• 39

Multiple Choice

Which of the following elements has a greater nuclear charge?

• Magnesium

• Beryllium

• Calcium

Multiple Choice

Which of the following elements has a greater nuclear charge?

• Radium

• Francium

• copernicium

• actinium

Patterns - Electron Shielding

9
Chemistry Name Game

Atomic Structure and the PToE

What do you think electron shielding might mean?
The shielding inner electrons provide the valence
(outer) electrons from the attraction of the nucleus.

More energy levels = more shielding

Increases

Patterns - Electron Shielding

9
Chemistry Name Game

Atomic Structure and the PToE

What do you think electron shielding might mean?
The shielding inner electrons provide the valence
(outer) electrons from the attraction of the nucleus.

More energy levels = more shielding

Increases

Patterns - Electron Shielding

9
Chemistry Name Game

Atomic Structure and the PToE

What do you think electron shielding might mean?
The shielding inner electrons provide the valence
(outer) electrons from the attraction of the nucleus.

More energy levels = more shielding

How does electron shielding change…

across a period?
Remains the same

down a group?

Increases

Multiple Choice

Shielding electrons are: 

• Electrons in the highest energy level

• Electrons in the lower energy levels

• Electrons that just come and go - they don't stay with the atom

• Electrons that are excited

Multiple Choice

The concept of shielding happens because of

• attraction between nucleus and valence electrons

• attraction between nucleus and core electrons

• repulsion between valence electrons and other valence electrons

• repulsion between core electrons and valence electrons

Multiple Choice

Which of the following elements has the most "shielding" electrons?

• Nitrogen

• Phosphorus

• Arsenic

• Bismuth

Multiple Choice

Which of the following elements has the lowest amount of shielding electrons?

• Argon

• Neon

• Helium

• Radon

Patterns - Reactivity

10
Chemistry Name Game

Atomic Structure and the PToE

Most reactive metals:

- Group 1 (alkali metals)

Second most reactive metals:

- Group 2 (Alkaline earth metals)

Most reactive nonmetals:

- Group 17 (Halogens)

Least reactive elements:

- Group 18 (Noble Gases)

Patterns - Reactivity

11
Chemistry Name Game

Atomic Structure and the PToE

The unreactivity of noble gases is attributed to the octet rule.

Octet Rule = atoms are stable when they have 8 valence electrons

Patterns - Reactivity

11
Chemistry Name Game

Atomic Structure and the PToE

The unreactivity of noble gases is attributed to the octet rule.

Octet Rule = atoms are stable when they have 8 valence electrons

Sodium, a Group 1 element, has one | two | seven | eight valence electron(s). It can easily

react with chlorine, a Group 17 element, which has one | two | seven | eight valence

electron(s). During bonding, each sodium atom gains one | gains seven | loses one | loses
seven electron(s) to become stable, and each chlorine atom gains one | gains seven | loses

one | loses seven electron(s) to become stable.

Other elements need to gain, lose, or share electrons to meet the octet rule.

Multiple Choice

Sodium, a Group 1 element, has one | two | seven | eight valence electron(s). It can easily react with chlorine, a Group 17 element, which has one | two | seven | eight valence electron(s). During bonding, each sodium atom gains one | gains seven | loses one | loses seven electron(s) to become stable, and each chlorine atom gains one | gains seven | loses one | loses seven electron(s) to become stable.

• One

• Two

• Seven

• Eight

Multiple Choice

Sodium, a Group 1 element, has one valence electron(s). It can easily react with chlorine, a Group 17 element, which has one | two | seven | eight valence electron(s). During bonding, each sodium atom gains one | gains seven | loses one | loses seven electron(s) to become stable, and each chlorine atom gains one | gains seven | loses one | loses seven electron(s) to become stable.

• One

• Two

• Seven

• Eight

Multiple Choice

Sodium, a Group 1 element, has one valence electron(s). It can easily react with chlorine, a Group 17 element, which has seven valence electron(s). During bonding, each sodium atom gains one | gains seven | loses one | loses seven electron(s) to become stable, and each chlorine atom gains one | gains seven | loses one | loses seven electron(s) to become stable.

• Gains One

• Gains Seven

• Loses Seven

• Loses one

Multiple Choice

Sodium, a Group 1 element, has one valence electron(s). It can easily react with chlorine, a Group 17 element, which has seven valence electron(s). During bonding, each sodium atom loses one electron(s) to become stable, and each chlorine atom gains one | gains seven | loses one | loses seven electron(s) to become stable.

• Gains One

• Gains Seven

• Loses Seven

• Loses one

Patterns - Ionization Energy

12
Chemistry Name Game

Atomic Structure and the PToE

What do you think ionization energy might mean?

Energy required to remove a valence electron from an atom.

Affected by nuclear charge and electron shielding.

More nuclear charge = higher ionization energy

Higher electron shielding = lower ionization energy

How does ionization energy change…

across a period?

Increases

down a group?

Decreases

Multiple Choice

Magnesium and aluminum | Phosphorus and sulfur have a greater ionization energy because their atoms have more protons than silicon has. The additional electrons do not increase shielding because their valence shells are the same as | different from those of the outer electrons of silicon.

 

Magnesium and aluminum | Phosphorus and sulfur have a smaller ionization energy because their atoms have fewer protons than silicon. Germanium has a smaller | larger ionization energy because the shielding effect on its outermost electron is greater than that of silicon.

• Magnesium and aluminum

• Phosphorus and sulfur

Multiple Choice

Phosphorus and sulfur have a greater ionization energy because their atoms have more protons than silicon has. The additional electrons do not increase shielding because their valence shells are the same as | different from those of the outer electrons of silicon.

 

Magnesium and aluminum | Phosphorus and sulfur have a smaller ionization energy because their atoms have fewer protons than silicon. Germanium has a smaller | larger ionization energy because the shielding effect on its outermost electron is greater than that of silicon.

• the same as

• different from

Multiple Choice

Phosphorus and sulfur have a greater ionization energy because their atoms have more protons than silicon has. The additional electrons do not increase shielding because their valence shells are the same as those of the outer electrons of silicon.

 

Magnesium and aluminum | Phosphorus and sulfur have a smaller ionization energy because their atoms have fewer protons than silicon. Germanium has a smaller | larger ionization energy because the shielding effect on its outermost electron is greater than that of silicon.

• Magnesium and aluminum

• Phosphorus and sulfur

Multiple Choice

Phosphorus and sulfur have a greater ionization energy because their atoms have more protons than silicon has. The additional electrons do not increase shielding because their valence shells are the same as those of the outer electrons of silicon.

 

Magnesium and aluminum have a smaller ionization energy because their atoms have fewer protons than silicon. Germanium has a smaller | larger ionization energy because the shielding effect on its outermost electron is greater than that of silicon.

• smaller

• larger

Open Ended

How does ionization energy change with atomic number? Use evidence from the graph to support your claim.

Open Ended

How does ionization energy change across periods and down groups on the periodic table? Use evidence from the graph to support your claim.

Open Ended

Why do noble gases have high ionization energy? What does this suggest about their chemical stability?

Patterns - Ionization Energy

12
Chemistry Name Game

Atomic Structure and the PToE

What do you think ionization energy might mean?

Energy required to remove a valence electron from an atom.

Affected by nuclear charge and electron shielding.

More nuclear charge = higher ionization energy

Higher electron shielding = lower ionization energy

How does ionization energy change…

across a period?

Increases

down a group?

Decreases

Multiple Choice

Which of the following sequences corresponds to a correct trend in ionization energy?

• Cl > S > P > Al

• Sr > Ca > Mg > Be

• Rb > K > Na > Li

• Rb > Sr > I > Xe

Multiple Choice

Which element has the greater ionization energy?

• Strontium

• Boron

Multiple Choice

Which element has the greater ionization energy?

• Lead
• Silicon

Multiple Choice

Put the following in order of increasing ionization energy:Neon, Lithium, Carbon

• Lithium, Carbon, Neon

• Carbon, Lithium, Neon

• Neon, Carbon, Lithium

• Lithium, Neon, Carbon

Multiple Choice

Put the following in order of increasing ionization energy:Strontium, Aluminum, Indium

• Strontium, Indium, Aluminum

• Strontium, Aluminum, Indium

• Indium, Aluminum, Strontium

• Aluminum, Indium, Strontium

Multiple Choice

Which has a higher nuclear charge?

• Hydrogen

• Helium

• Lithium

Multiple Choice

Which has less electron shielding?

• Hydrogen

• Rubidium

• Lithium

Patterns - Atomic Size

13
Chemistry Name Game

Atomic Structure and the PToE

What do you think atomic size might mean?

Size of the atom.

Affected by nuclear charge and electron shielding.

More nuclear charge = smaller atom

Higher electron shielding = bigger atom

How does atomic size change…

across a period?

decreases

down a group?

increases

Patterns - Electronegativity

14
Chemistry Name Game

Atomic Structure and the PToE

What do you think electronegativity might mean?

An atoms attraction to shared electrons.

Affected by nuclear charge and electron shielding.

More nuclear charge = higher electronegativity

Higher electron shielding = lower electronegativity

How does electronegativity change…

across a period?

Increases

down a group?

Decreases