Day 4 2-181. Which metal would you expect to

be more reactive - Fr OR Cu? WHY?

2. Which nonmetal would you expect to be more reactive - F OR Ne? WHY?

How is the periodic table arranged?

Periodic TrendsAtomic radius:- Measure of size – radius of an atom- Atoms with more electrons do NOT necessarily have a larger atomic radius

Periodic Trends- Atoms with more electrons do NOT necessarily have a larger atomic radius

Periodic Trends- Atoms with more electrons do NOT necessarily have a larger atomic radius

1. Atoms get larger going down a group.

2. Atoms get smaller going across a period

So why?...

Periodic Trends- Atoms with more electrons do NOT necessarily have a larger atomic radius

As you move down a group you increase the number of energy levels in the atom and so the atom gets larger as expected.

Periodic Trends- Atoms with more electrons do NOT necessarily have a larger atomic radius

As you move across a period, # of protons increases and outermost energy level stays the same, the attractive force between elecs. and pros. pulls the atom tighter (closer to nucleus)

Periodic TrendsWhat’s bigger:

B or Al

B or N

N or Zn

C or Cl

Red = ?Green = ?Blue = ?

Good Conductors = ?

Inert elements = ?

Review1. What element is in Group 2,

Period 3?

2. Name an element in Group 3

3. How many valence electrons in Xe?

4. Give me an element with 1 valence electron.

Alkali metals

7 valence

Nonmetals

Magnesium

Ductile

Halogens

1 valence

Noble gases

Atomic radius

Period 3

metalloids

inert

fluorine

malleable

Helium

Halogens

1 valence

Noble gases

Atomic radius

Period 3

Day 5 2-191. Why does the size of an atom

decrease moving across a period?

2. What is more reactive Cl or Ar – Explain!!!

Red = ?Green = ?Blue = ?

Good Conductors = ?

Inert elements = ?

Review1. What element is in Group 2,

Period 3?

2. Name an element in Group 3

3. How many valence electrons in Xe?

4. Give me an element with 1 valence electron.

Partner Review1. What element is in Group 17,

Period 3?

2. What family of elements is the element above in?

3. How many valence electrons does it have?

Periodic TrendsWhat are ions?

- atoms that are charged due to the loss or gain of

electrons- If an atom loses elecs. it becomes smaller and positive

- If an atom gains elecs. it becomes larger and negative

Notes page 4

Periodic TrendsWhat are ions?- If an atom loses elecs. it becomes smaller

- If an atom gains elecs. it becomes larger

PAGE 176-179Which elements gain elecs.? Which elements lose elecs.? Pattern?

Periodic TrendsElements on the right side of the periodic table form _________ ions

Elements in the same group form ___________ ions

negative

The same

Periodic TrendsWhat’s bigger:

F or F-

Na or Na+

Na or Rb

Na of Al

F or Cl-

Read / review Section 6.2 and

complete #s 11-17 on page 173

Day 2 3-21. Which halogen is found in period 2?

2. How many valence electrons does calcium have?

3. Why does the size of an atom increase moving down a group?

Octet rule – Atoms tend to gain, lose, or share electrons in order to acquire a full set of valence electrons (8)

- 2 for H, He, Li, Be, + B

notes page 6

As of today, you should have the following:

Families colored in (page 168)

Valence electrons marked

+1, +2, -1,-2, and -3 ions marked

Day 2 3-2

Valence electrons =

2

1

3 4 5 6 7

8

Ions = +1

+2 -3 -2 -1

Add today:

Reactivity trend (front / back)

Atomic size (front / back)

Positive and negative ion trend on back

Day 2 3-2

Valence electrons =

2

1

3 4 5 6 7

8

Ions = +1

+2 -3 -2 -1

Atom size decreases

Atom

size increases

Reactivity increases away from the middle

Positive and Negative ion trendElements on the right side form negative ions.

Elements on the left form positive ions.

Read / review Section 6.2 and

complete #s 11-17 on page 173