1 / 11

Coulomb’s Law

Coulomb’s Law. A more thorough understanding of periodic trends. Coulomb’s Law. E = k Where F = force k = konstant (Germans…) Q = charge r = radius. Ionization Energy.

miracle
Download Presentation

Coulomb’s Law

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. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Coulomb’s Law A more thorough understanding of periodic trends

  2. Coulomb’s Law E = k Where F = force k = konstant (Germans…) Q = charge r = radius

  3. Ionization Energy • Ionization energy – the energy needed to remove the outermost electron. The greater the ionization energy, the stronger the attraction and the more energy needed to remove that electron.

  4. Ionization Energy • So E = ionization energy • = charge of an electron (-1) • = effective nuclear charge of protons in nucleus • Attraction for a valence electron is partially shielded by the inner shell electrons. • The simple way to estimate effective nuclear charge is to start with the atomic number (total protons) and subtract the number of inner shell electrons.

  5. Ionization Energy • For example: • Hydrogen has an effective nuclear charge of 1 • 1 proton – 0 electrons = 1 • Helium is 2 • Lithium is 1 • And so on… • All transition metals are 2 • All halogens are 7…

  6. Ionization Energy • r = radius, as in the radius from the center of one atom to the center of another atom • the distance between charged particles which can be approximated by the Period – two atoms in the same period have approximatelythe same atomic radius. • Na (Period 3) is smaller than K (Period 4) • But similar in size to Al (Period 3)

  7. Lattice Energy • Lattice energy – the energy needed to separate oppositely charged ions. • The higher the lattice energy, the stronger the ionic bond. • The stronger the ionic bond the less soluble in water at a given temperature, since the ions must separate/dissociate from one another and attach to water in order to dissolve.

  8. Lattice Energy • E = lattice energy • = charge of positive ion • = charge of negative ion • r = bond length, the distance between the nuclei of the 2 ions – can also be approximated by the Period.

  9. REMEMBER! • Remember to use the Period of the element that is isoelectronic with the ion! • Na is in Period 3 and has 3 occupied energy levels. • has lost an electron and thus has 10 electrons. • Ergo, it is isoelectronic with Ne in Period 2. • has only 2 occupied energy levels

  10. Practice! • Complete the following handout using complete sentences for explanations. • Also, be prepared to present arguments defending your position. • 10 random volunteers will be chosen on Monday.

  11. Chapter 7 Quiz! Here’s the quiz. Take it home. Completeit. Bring it back. Use your book. Use your notes. Use a friend. Due on Monday.

More Related