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CHEMISTRY THE CENTRAL SCIENCE Chapter 7 Periodic Properties of the Elements 7.1 Development of the Periodic Table (pg 256 ﹣ 257) 9 elements have been discovered in ancient times. What are they? How do they different than the elements discovered in the last 100 years? Mendeleev predicted the properties of Ge before it was discovered. How was he able to do this? In Moseley’s day, elements were arranged in order of increasing atomic weight. This is not how we arrange elements in the current periodic table. Why? Fe, Cu, Ag, Au, Hg,C, S nature in elemental form Observing patterns in the periodic table, identifying gaps and using the properties of neighboring elements to make predictions Because the atomic number is the fundamental property of an element and represents the number of protons and groups similar chemical properties together
Chapter 7 Periodic Properties of the Elements 7.2 Effective Nuclear Charge (pg 257 ﹣ 260) Coulomb’s Law tells us that the strength of the interaction between two electrical charges depends on: The attractive force between an electron and the nucleus depends on: Define effective nuclear charge and express it as an equation. 1 2 1 2 CHEMISTRY THE CENTRAL SCIENCE The distance between them The magnitudes of the charge The average distance between the nucleus and the electron The magnitude of the nucleus charge The net positive charge experienced by an electron in a many-electron atom; this charge is not the full nuclear charge because there is some shielding of the nucleus by the other electrons in the atom. Ze ff =Z-S
Chapter 7 Periodic Properties of the Elements Figure 7.3 illustrates effective nuclear charge for a sodium atom. Sketch this figure and describe what is being screened, what it is being screened from, and what is doing the screening. If we use a simple model to describe screening in a sodium atom, we would expect Z to equal +1. The actual value is +2.5. How can you explain this? CHEMISTRY THE CENTRAL SCIENCE I hope you are able to recognize that the force of attraction between the nucleus and the electrons surrounding the nucleus are based on electrostatic potential energy. If you are able to relate the periodic trends to electrostatic interactions instead of simply trying to memorize them you will be able to understand the ‘why’ behind the periodic trends. Valence electron (3s) Ten core electrons (1s^2, 2s^2, 2p^6) screen the nucleus from the valence electrons (10-) Sodium nucleus contains 11 protons (11+) because there is a small probability that the 3s electron is close to the nucleus
Chapter 7 Periodic Properties of the Elements What is the trend for Z eff as we progress from left to right in the periodic table? What is the trend for Z eff as we progress down a column in the periodic table? Why do we observe these trends? CHEMISTRY THE CENTRAL SCIENCE The e ff ective nuclear charge increases from left to right across a period of the periodic table. the e ff ective nuclear charge experienced by valence electrons changes far less than it does across a period There instructive
CHEMISTRY THE CENTRAL SCIENCE Effective Nuclear Charge and Ionization Energy
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