Aim: : Can you explain the trends in atomic radius across and down the periodic table? *Puzzle:

Do Now: Record and Answer the following questions in your notebook

1.What is the reactivity trend within group 1?

2. Which element has chemical properties that are most similar to those of calcium?

(1) Co (2) K (3) N (4) Sr

3. What is the reactivity trend within group 17? .

Aim: : Can you explain the trends in atomic radius across and down the periodic table?

*Puzzle: Use the name of an element to solve the puzzle.

“A fur Seller”

Discussion

1. What do you notice about the group number and the number of valence electrons?

2. Explain how the period number correlates to the structure of an atom?

3. Analyze the patterns you notice about the size of the atom and the electrons in the atoms as you go down a group.

4. Analyze the patterns you notice about the size of the atom and the electrons in the atoms as you go across the period?

5. Can you give explanations for the patterns you

describe in Q 3 and 4?

Periodicity

What trend did we look at yesterday?

• REACTIVITY

• Metallic / Non-metallic Character

• Atomic Radius

• Ionization Energy

• Electronegativity

Trends that exist across and down on the Periodic Table

Reel Big Fish- Trendy

Atomic Radius

• Definition-

• The distance between the center of two atoms connected divided by 2.

• Good measure of the size of an

atom

Why does this trend occur?

-Increases down a

group

Why do these trends occur?

• Decreases across a period

Student Explanation: because there are more protons so

the electrostatic attraction between the protons in the

nucleus and the electrons is stronger making our atom

smaller.

Atomic Radii Trends

LEFT RIGHT Atomic Radius DECREASES

TOP BOTTOM Atomic Radius Increases

Atomic Radius Trend

Largest elements on lower left

Smallest elements upper right

Reflection

• Look at your notes and think about the lesson.

Write a two to three sentence summary of the

lesson in your notes

Exit Slip

Explain the trends in atomic

radius across and down the

PT

Do Now: Record and Answer the following questions in your notebook

1.Which metal atom on the periodic table loses electrons most easily?

2.Which non metal atom on the periodic table gains electrons most easily?

3.Why does an elements atomic radius decrease across a period?

4.Why does an elements atomic radius increase going down a group?

Aim: : Can you explain the trend in ionization energy across and down the periodic table?

*Puzzle: Use the name of an element to solve the puzzle.

“A fur Seller”

Review Ionization Energy Practice

Ionization Energy

• Definition-

• The amount of energy needed to remove the outermost electron from a neutral atom.

X + energy X ⁺ + 1 electron

1 ^st Ionization Energy Trend

Highest ionization energy elements are on the upper right

Lowest ionization energy elements are on the lower left

High Ionization Energy

(fill in the blank)

• High ionization energy values indicate a _________ hold on electrons.

• A really High ionization energy means the

element would rather __________electrons?

Low Ionization Energy

(fill in the blank)

• Low ionization energy values indicate a ___________hold on electrons.

• A very low ionization energy means the

element will easily _________ electrons.

Learning Check:

High ionization energy values indicate a strong hold on electrons Low ionization energy values indicate a weak hold on electrons

If an atom has a high ionization energy, what do we know about its ability to lose or gain

electrons?

If an atom has a low ionization energy, what do we know about its ability to lose or gain

electrons?

Learning Check

1.Which has the smallest ionization energy He, N, Na? Why?

Explain in terms of hold on electrons

and atomic size.

Reflection

• Look at your notes and think about the lesson.

Write a two to three sentence summary of the

lesson in your notes

Practice – Handout on

Ionization Energy

Refelction

Answer the aim in two

sentences in your notes

Exit Slip

Explain the trend in

ionization energy across and down the periodic

table.

PT CLASSWORK : green workbook p. 50: Q 17 – 21, 24, 25 (14mins)

p. 44: Q 8-11p. (8mins) p. 48: 12-20 (9mins)

p. 49/50: Q 1-5, 9-11,15,16 (20mins) Please follow these Directions:

Complete the following question on a loose leaf. Be sure to write the correct heading.

Read the question. Identify key words by writing the key words down then annotate the key words.

Finally answer the question by writing out the correct answer choice for MC Q’s or

writing a response for the Short Answer Q’s.

Review Quiz

Do Now: Record and Answer the following questions in your notebook

Aim: : Can you explain the trend in

electronegativity across and down the periodic table?

*Puzzle: Use the name of an element to solve the puzzle.

“Not an exciting person”

Do Now: Record and answer the following in your notebook.

Which group of circles, when

considered in order from the top to the bottom, best represents the

relative size of atoms of Li, Na, K,

and Rb, respectively?

What did we learn yesterday?:

1.Which has the smallest ionization energy Kr, Li, Be? Why? Explain in

terms of hold on electrons and atomic

size.

Recap:

Each element in a group has similar chemical properties because of the same number of valence electrons.

Metal elements lose electrons and we can tell how metallic/active an element is by looking at its ability to LOSE electrons.

(amount of electrons and electrostatic attrition)

Non-metals elements gain electrons and we can tell how active they are by looking at their ability to GAIN electrons.

(amount of electrons and electrostatic attrition)

Electronegativity

• Definition-

• measure of an element’s attraction for electrons when bonded to another atom.

• Scale created by Linus Pauling Scale is from 0.7 - 4.0

4.0 is the highest attraction for electrons 0.7 is the lowest attraction for electrons

• Values can be used to predict the type of bond that will

form between elements

Electronegativity Trend

Most electronegative elements are on upper right

Least electronegative elements are on lower left

Electronegativity Trends

Lower Left Upper Right Electronegativity Increases

Regents Questions Practice

1. Which three groups of the Periodic Table contain the most elements classified as metalloids

(semimetals)?

(1) 2, 13 & 14 (2) 14, 15 & 16 (3) 16, 17 & 18

2. Which element in Group 15 has the strongest metallic character? Why?

Bi, As, P, N

3. Order the following elements according to metallic

character (most to least) and explain why with reference

to energy levels and hold on electrons. Li, I, K, F

Essential Questions:

Start of Classwork (CW8)

1. Which element in Group 2 has the strongest metallic character? Why? Use at least two examples to explain.

2. What happens to the atomic radius of the

following elements as you go across the periodic table and why? Be, B, F

Green work book Page 49 Q 1-8 and 14-16

Classwork 8 Cont.

• Green work book Page 49 Q 1-8 and 14-16

• On a lose leaf write the Question number with correct answer choice and answer choice

number with a short reason.

• * Super Stars Q 21 - 25

Practice 14 – Handout on Electronegativity

and PROJECTS!

Do Now: Record and Answer the following questions in your notebook

1. Write down your definition of an ion.

2. What is the difference between an atom, an ion and an excited state atom. Use Calcium as an

example and draw pictures.

Aim: : How do we explain the trend in ionic

radius verses atomic radius?

• Atoms gain or lose electrons to become charged Ions

particles called: ions.

• Metals lose valence electrons to become positive ions (cations)

• Nonmetals tend to gain valence electrons to become negative ions (anions)

• As these atoms gain or lose electrons, they complete

an octet of valence electrons or a full shell

1. What ions will the following atoms form? Explain why.

Li, S, Br, F

How can we tell what ions will

form from a specific atom?

Ionic Radius

Definition- Distance from the nucleus to the outer energy level of the ion.

• When an atom loses its valence electrons, it loses the outer energy level and its radius decreases.

• When an atom gains valence electrons its radius increases.

• Be able to compare the ion size to the neutral atom size.

(eg. Na atom compared to Na

ion)

1. Metallic ion is always ____________than the metal atom it is formed from.

2. Nonmetallic ion is always ___________than the nonmetal

atom it is formed from.

Ionic Radius

LearningCheck

1. Which is bigger an atom of sodium or an atom of Francium and why?

2. Which is bigger an ion of chlorine or an atom of Cl?

3. Which is smaller an ion of Mg or

and atom of Mg?

Summary

Aim: What is the trend in metallic character on the periodic table?

Do Now: record and answer the following in your notes.

1. What happens to the atomic radius of the

following elements as you go across the

periodic table and why? Be, B, F

Lets take 3 metals in Group 1 to use as examples to explain

metallic character….

Lets take 3 non-metals in Group 17 to use as examples to explain

non-metallic character….

Learning Check

1. Which element in period 2 of the periodic table is the most reactive non-metal?

(1) C (2) O (3) N (4) F

Metallic / Non-metallic Character

Most metallic elements are on the lower left

Least metallic elements are in the upper right

Summary

What

are these

pictures

trying to

show us?