Bohr Model and Lewis Dot Diagrams - Day 3

You Will Need:1. Pencil, Text Book- Periodic Table,

Colored Pencils2. CALCULATOR2. Get out your 7 page packet3. Textbook open to Periodic Table (196-

197)YOU SHOULD HAVE 4 pages 7 sides to

your packet.4. Test #3 Corrections and Parent

Signature - Due NOW

Please SCHEDULE:

1. To take Part 2 for the 1st time OR to

2. Retake Test #3

• Part 2 – 101/145 or lower

3. Parent Signature and Corrections – due TODAY.

Element Bohr Model Lewis Dot (Symbol + Valence)

Lithium

Atomic #

Atomic Mass – Atomic #

Neon

Atomic #

Atomic Mass – Atomic #

Row =

Electrons= Protons =

Neutrons =

2

3-3+

7-3=

4

P = 3N = 4

21

Li

Row =

Electrons= Protons =

Neutrons =

P =10N =10 Ne

10

10-10+

20-10

10

28

Turn to the blank page #4 behind the Bohr Model and Lewis Dot Diagrams

P=8N=8

P=1N=0

P=1N=0

How to determine the type of bond in a compound?

Calculate the electronegativity factor

What is ELECTRONEGATIVITY? A measure of how much an element wants an electron

How do you know the electronegativity factor of an element?

Look it up (see next slide)

What are the determining values for each type of bond?

0Non-polar covalent

.5Polar covalent

1.7Ionic

http://www.tutor-homework.com/Chemistry_Help/electronegativity_table/electronegativity.html

ELECTRONEGATIVITY VALUES

Let’s try a couple:

P=8N=8

P=1N=0

P=1N=0

H2OCalculate the electronegativity factor

H = 2.1O = 3.5

3.5 – 2.1 = 1.4

NaCl

0Non-polar covalent

.5Polar covalent

1.7Ionic

Polar Covalent

Ionic

Na = .9Cl = 3.0

3.0 - .0 = 2.1

Let’s try a couple:

P=8N=8

P=1N=0

P=1N=0

KCl Calculate the electronegativity factor

K = CL =

CH4C = H=

What are the determining values for each type of bond?

0Non-polar covalent

.5Polar covalent

1.7Ionic

Ionic

.83.0

3.0 - .8 = 2.2

2.52.1

2.5 – 2.1 = .4 Non-polar covalent

Let’s try a couple:

P=8N=8

P=1N=0

P=1N=0

KCl Calculate the electronegativity factor

K = CL =

CH4C = H=

CCl4

CO2

C16H34 (diesel fuel)

Ionic

.83.0

3.0 - .8 = 2.2

2.52.1

2.5 – 2.1 = .4 Non-polar covalent

1. Materials Manager Log in to Learning Point – in charge of PPT

2. Complete Bonding Type Identification

3. Complete Notes and Diagrams – should be done up to page 6 for homework

4. We will be working in class tomorrow – Due at the end of the period

Let’s try a couple:

P=8N=8

P=1N=0

P=1N=0

KCl Calculate the electronegativity factor

K = CL =

CH4C = H=

CCl4

CO2

C16H34 (diesel fuel)

Ionic

.83.0

3.0 - .8 = 2.2

2.52.1

2.5 – 2.1 = .4 Non-polar covalent

Question Answer

What are the characteristics of Ionic Bonds?

• Usually between Metals and Nonmetals• Transfer of electrons – atoms become

IONS• Form Crystal Lattices• Brittle• High melting and boiling points• Dissolve easigly in water• Form compounds• Specific shape

Bismut

h

Crystal Lattice

Question Answer

What are the characteristics of Ionic Bonds?

• Usually between Metals and Nonmetals• Transfer of electrons – atoms become

IONS• Form Crystal Lattices• Brittle• High melting and boiling points• Dissolve easily in water• Form compounds• Specific shape

Illustrate a neutrally charged Bohr Model of an aluminum atom.

P=13N=14

2 83

Question Answer

Illustrate a positively charged Bohr Model of an aluminum atom. (3+)

Why is Al3+ considered an ion? (Look at all the subatomic particles before you answer this question.)

P=13N=14

28

Forming Sodium Chloridehttp://www.youtube.com/watch?v=upg-FUHp6yshttp://www.youtube.com/watch?v=7DjsD7Hcd9U

Before (pg. 233) After

Questions:1)Why does Sodium become an Ion? 2)Is it Positive or Negative? Why?3)Why does Chlorine become an Ion? 4)Is it Positive or Negative? Why?

Questions:1)Why do Sodium and Chlorine bond?2)What is the overall charge of the compound?3)Does NaCl have the same characteristics as Na and Cl?4)What are some unique characteristics of NaCl?

P=11 N = 12

P=11 N = 12

P=17 N = 19

P=17 N = 192

8

1

2

8

2

87

2

8

8

Question Answer

What is a covalent bond? • Valance electrons are shared• More often between nonmetal• Low melting and boiling point• Free flowing but can be brittle• Form molecules• Do not have a specific shape - flexible

C6H10O5

C12H22O11

Polar Covalent

C1

6 H3

4 die

sel fu

el

Non

pola

r covale

nt

Molecule Illustration

Explanation Electron Dot (Color Code each element)

1. What kind of bond does Hydrogen & Oxygen make? How do you know?

2. Why does one Oxygen bond with two Hydrogen atoms?

http://www.youtube.com/watch?v=ulyopnxjAZ8&feature=relmfu Drawing Lewis Dot Diagram Bonds

P=8N=8

P=1N=0

P=1N=0

1. Schedule Test #3 retake

2. Bohr Model vs. Wave Model & Lewis Dot + Electrons and

Chemical Bonding– Pgs. 1-7 – due Thursday