chapter 15
Download
Skip this Video
Download Presentation
Chapter 15

Loading in 2 Seconds...

play fullscreen
1 / 13

Chapter 15 - PowerPoint PPT Presentation


  • 100 Views
  • Uploaded on

Chapter 15. Ionic Bonding. Valence Electrons. Do the electron configuration for the following elements Li Be B O F Ne. Valence Electrons. Now look at the outermost electrons by looking at the last s and p orbital Circle and count these electrons These are the valence electrons.

loader
I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
capcha
Download Presentation

PowerPoint Slideshow about ' Chapter 15' - nerita


An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript
chapter 15

Chapter 15

Ionic Bonding

valence electrons
Valence Electrons
  • Do the electron configuration for the following elements
  • Li
  • Be
  • B
  • O
  • F
  • Ne
valence electrons1
Valence Electrons
  • Now look at the outermost electrons by looking at the last s and p orbital
  • Circle and count these electrons
  • These are the valence electrons
valence electrons2
Valence electrons
  • Valence electrons are in the highest energy level of an element’s atom
  • Valence electrons are the same as group # (roman numeral) for the group A representative elements
  • Valence electrons are usually the only electrons used in chemical bonds
  • We use valence e- to write Lewis Dot Structures
valence electrons cont
Valence electrons (cont.)

A. Lewis Dot Structure

Ex: bromine

Br

electron configurations for cations anions
Electron configurations for cations & anions

A. Octet Rule: when forming compounds atoms want to have 8 electrons (s2p6) like the noble gases (except He)

slide7

Cations(metals)tend to lose electrons,positively charged ion

+

lose 1 e-

Na

(atom)

Na

(cation)

1s22s22p63s1

1s22s22p6

octet

Using the Dot Structure

+

lose 1 e-

Na

(cation)

Na

(neutral atom)

2+

Mg

(cation)

lose 2 e-

Mg

(neutral atom)

slide8

Anions(Nonmetals) have negative charges because they gain electrons

-

gain 1 e-

Cl

(atom)

Cl

(chloride ion)

1s22s22p63s23p5

1s22s22p63s23p6

valence

octet

Using the Dot Structure

-

gain 1 e-

Cl

(chloride ion)

Cl

(neutral atom)

2-

gain 2e-

O

(oxide ion)

O

(neutral atom)

practice
Practice

N

3-

gain 3e-

N

(nitride ion)

+

Lose 1 e-

Li

Li

-

I

(iodide ion)

gain 1 e-

I

+2

Ca

Lose 2e-

Ca

ionic compound
Ionic Compound

1. ionic compounds form crystals

2. high melting and boiling points

3. hard and brittle

4. conduct electricity when dissolved in water or melted

  • Composed of a metal (cation) and nonmetal (anion)
  • Ionic bond – oppositely charged ions attract
  • Electrically neutral (+) = (-)

A. Properties

ionic bonds
Ionic Bonds

Na

+1

-1

1. Sodium and Chlorine

-

donates e-

Na+

Cl

Cl

+

NaCl

+1

-2

2. Potassium and Oxygen

donates e-

K

K+

-2

O

+

O

donates e-

K+

K

K2O

slide12

AlBr3

+3

-1

3. Aluminum and Bromine

-

Br

Br

Al

-

Al+3

Br

Br

+

-

Br

Br

+2

-3

4. Magnesium and Nitrogen

Mg+2

-3

Mg

N

N

Mg+2

-3

+

N

Mg

Mg+2

N

Mg

Mg3N2

output example
OUTPUT EXAMPLE:

1. Potassium & Fluorine

+1

-1

-

+

F

K

F

+

K

KF

ad