1. 2. 3. what are the trends for atomic radii? why do these trends exist? 4
TRANSCRIPT
1. 2.3. What are the trends for atomic radii? Why do these trends exist?4.
Catalyst
Down in Front!
1.9 – I can define and calculate the effective nuclear charge for an atom and explain how this impacts observed periodic trends.
1.10 – I can define atomic/ionic radius and explain how it relates to the effective nuclear charge. Furthermore, I can explain how this trend changes as you move throughout the Periodic Table and relate it to the elements quantum electron configuration.
Today’s Learning Targets
The force felt by two charged objects is directly related to the size of the charge and inversely related to the distance between the charges.
The force on the electron increases as the nuclear charge increases
The force on the electron decreases as the nuclear charge decreases
Coulomb’s Law
Periodic trends depend on how well electrons “feel” the nucleus
The effective nuclear charge (Zef) is the force felt between the nucleus and the electron of interest
Effective Nuclear Charge
In elements with many electrons, inner electrons shield the valence electrons.
This occurs because the core electrons act to shield the valence electrons from the full positive charge of the nucleus.
Electron Shielding
Do you think the Zef increases or decreases as we go down a group the Periodic Table?
What about as we go across a period? Justify your answer with evidence and the
idea of electron shielding.
Predict the Trend
The further away from the nucleus, the less the nuclear charge is “felt”, so Zef decreases down a group.
As you continue across a period, there are no more core electrons, but there is a stronger positive charge
Therefore, as you go across a period Zef increases.
Trends in Zef
Zef decreases
Zef increases
What is the trend for atomic radii as you go throughout the Periodic Table? Justify your response
Quick Write
Atomic radii increase down a group and decrease across a period.
They increase down a group because more orbitals are being added, making the element “bulkier”
The decrease across a period because Zef is increasing, thus causing the electron to be more attracted to the nucleus.
Trends for Atomic Radii
Removing electrons causes the radius to decrease
Removing electrons causes orbitals to be removed and electron-electron repulsions to decrease
Both of these lead to an increase in Zef and a decrease in the ionic radius
Radii of Cations
Adding electrons causes the radius to increase
Adding electrons causes an increase in electron – electron repulsions, so Zef decreases.
A decrease is Zef causes the radius to be larger
Radii of Anions
Arrange Na+, K+, and K in order of increasing atomic radius
Class Example
Arrange the ions K+, Cl-, Ca2+, and S2- in order of decreasing size.
Table Talk
Arrange the following atoms from smallest to largest: Rb+, Sr2+, Y3+
Table Talk
Summarize
Pick a SideI am going to project up numerous
statementsYou must decide whether you agree or
disagree.Be prepared to defend your response!
Pick a Side Questions1. Coulombs Law says that as you pull charges
away from one another, the force increases.2. The effective nuclear describes the
attraction between the nucleus and the electron of interest.
3. Effective nuclear charge decreases down a group because there are more electrons.
4. Effective nuclear charge increases across a period because of the more positive nucleus.
5. The ionic radius is always larger than the atomic radius for a given atom.
Pick a Side Questions (cont.)5. Order the following from smallest to largest radius: Se2-, Te2-, Se
- Answer: Se, Se2-, Te2
6. Order the following from largest to smallest radius: Co3+, Fe2+, Fe3+
- Answer: Co3+, Fe2+, Fe3+
7. The effective nuclear charge has littler overall impact on the atomic and ionic radius of an element
Closing TimePre – Lab for Lab 3 due at the start of lab on
Thursday/FridayFinal lab right up (results and conclusions) due
Monday/Tuesday for Lab 2.To be on track, read sections 7.1 – 7.3 and
answer the corresponding problems