chapter 1 n.
Download
Skip this Video
Loading SlideShow in 5 Seconds..
Chapter 1 PowerPoint Presentation
Download Presentation
Chapter 1

Loading in 2 Seconds...

play fullscreen
1 / 12

Chapter 1 - PowerPoint PPT Presentation


  • 71 Views
  • Uploaded on

Chapter 1 . Activity 6: Atoms with More than one Electron. PERIODICITY. There are general trends in the properties of atoms and their ions. These trends can be explained using the periodic table. PERIODICITY. Can you name a trend that we have talked about this year?

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 1' - vian


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 1

Chapter 1

Activity 6:

Atoms with More than one Electron

periodicity
PERIODICITY

There are general trends in the properties of atoms and their ions.

These trends can be explained using the periodic table.

periodicity1
PERIODICITY

Can you name a trend that we have talked about this year?

Think about what you graphed

  • Atomic Mass vs Atomic #
  • As Atomic # increases, Atomic Mass increases
  • Atomic Radius vs Atomic #
  • As Atomic # increases, Atomic Radius increases down a group, but decreases across a period.
background
Background

Electrons can move between energy levels (Bohr’s model supported by line spectra)

The nucleus and electrons are attracted to each other (opposites attract)

Electrons that are far away from the nucleus can escape the attraction of the nucleus

(atoms can lose electrons)

Losing an electron is called ionization

ionization energy
Ionization Energy

Ionization energy is the energy required to remove a valence electron from an atom.

Valence electron= outermost electron that is farthest from the nucleus.

period

group

ionization energy1
Ionization Energy
  • Energy needed to remove a loosely held electron from an atom
  • Decreases as you move down a group
    • Atom gets bigger, more energy levels
    • Nucleus is further from the outer most electron (valence electrons)
    • Nucleus & electron attraction decreases, so it is easier to take an electron away.

D

ionization energy2
Ionization Energy
  • Energy needed to remove a loosely held electron from an atom
  • Increases as you move across a period
    • Nonmetals hold onto their electrons tighter
    • Atom is smaller, so nucleus is closer to valence electron making it harder to remove.

I

D

ionization energy3
Ionization Energy

Practice

He or Xe? (kJ/mol)

Which has more ionization energy?

He Xe2372 kJ/mol 1170 kJ/mol

ionization energy4
Ionization Energy

Practice

Li or Ne? (kJ/mol)

Which has more ionization energy?

Li Ne520 kJ/mol 2081 kJ/mol