10. Periodic Properties of the Elements

Periodic Trend: Electron Affinity

Electron Affinity - Chemistry Tutorial

Choose the element with the more negative (more exothermic)
electron affinity in each pair.
a. Mg or S 
b. K or Cs 
c. Si or P 
d. Ga or Br

Which of the following processes will release the most energy? (LO 6.9)
(a) 
(b) 
(c) 
(d)

The electron affinity of sodium is lower than that of lithium, 
while the electron affinity of chlorine is higher than that of 
fluorine. Suggest an explanation for this observation.

 These elements follow the general trend in electron affinity in a row of the periodic table. 

 Correct, of the elements listed Cl is furthest to the right in period 3. These elements follow the general trend in electron affinity in a row of the periodic table. 

 In general, electron affinities become more negative moving left to right along a row of the periodic table.  Keep in mind that this is only a general trend. 

 Based on general trends in electron affinity, which of the elements listed is most likely to have the most negative electron affinity? 

What is Electron Affinity?

Choose the element with the more negative (more exothermic) 
electron affinity from each pair. 
a. Na or Rb

Which of the following, I or I-, will have a negative electron
affinity?

Determine which atom in the following set has the most exothermic electron affinity:N, O, C, B, Ne

Periodic Trend: Electron Affinity Example 1

Hydrogen is an unusual element because it behaves in some 
ways like the alkali metal elements and in other ways like 
nonmetals. Its properties can be explained in part by its electron 
configuration and by the values for its ionization energy 
and electron affinity. (a) Explain why the electron affinity of 
hydrogen is much closer to the values for the alkali elements 
than for the halogens.

Trends - Electron Affinity and Metallic Character

7.5 Electron Affinity

Why does ionization energy increase regularly across the periodic table from group 1A to group 8A, whereas electron affinity increases irregularly from group 1A to group 7A and then falls dramatically for group 8A?

Choose the element with the more negative (more exothermic)
electron affinity from each pair.
c. C or N

Periodic Trends: Electronegativity, Ionization Energy, Atomic Radius - TUTOR HOTLINE

Which of the following represents the third electron affinity of Si?

The electron affinities, in kJ>mol, for the group 11 and group 
12 metals are as follows: 
Cu -119 
Zn 7 0 
Ag -126 
Cd 7 0 
Au -223 
Hg 7 0 
(b) Why do the electron affinities of the 
group 11 elements become more negative as we move down 
the group? [Hint: Examine the trends in the electron affinities 
of other groups as we proceed down the periodic table.]<img src="https://lightcat-files.s3.amazonaws.com/problem_images/7269e12339629346-1660915832163.jpg" alt="" />

Rank the following elements in order of increasing electron affinity:Cs, Hg, F, S

If the electron affinity for an element is a negative number,
does it mean that the anion of the element is more stable
than the neutral atom? Explain.

What is electron affinity? | Chemistry | Extraclass.com

Choose the element with the more negative (more exothermic) 
electron affinity from each pair. 
b. B or S

Periodic Trends: Electronegativity and Electron Affinity

The Periodic Table: Atomic Radius, Ionization Energy, and Electronegativity

Write an equation for the first electron affinity of helium.
Would you predict a positive or a negative energy value for
this process? Is it possible to directly measure the first electron
affinity of helium?

Electron Affinity Equations

Electron Affinity

Generally, electron affinity increases moving from left to right across a period and going up a group.

Learn the toughest concepts covered in Chemistry with step-by-step video tutorials and practice problems by world-class tutors

Jules

General Chemistry

https://static.studychannel.pearsonprd.tech/courses/general-chemistry/thumbnails/general-chemistry

#FFFFFF

Mark Clemente

Melissa Maribel

Najam Academy

Pearson

TheChemistrySolution

chemistNATE

Extraclass Official

The Science Classroom

Jules Bruno

Professor Dave Explains

FusChemistryVideos

1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Periodic Trend: Cumulative

Periodic Trends are patterns present in the periodic table based on an element's size and electron distribution.&nbsp;

Periodic Trend: Ionic Radius

Ionic Radius is the distance between an ion's nucleus and its most outer occupied electron shell.&nbsp;

The Electron Configuration

The electron configuration of an element is the distribution of its electrons within atomic orbitals.&nbsp;

The Electron Configuration: Ions

The Electron Configuration of Ions involves either adding or removing electrons from a given orbital of an element.

Periodic Trend: Successive Ionization Energies

Successive Ionization Energies deals with the removal of multiple electrons from a gaseous atom or ion through multiple steps.

Periodic Trend: Atomic Radius

The atomic radius of an element is the distance from its nucleus to its outer electron shell.

Valence Electrons of Elements

The Valence Electrons represent the outer shell electrons of an element or ion.&nbsp;

Periodic Trend: Effective Nuclear Charge

Effective Nuclear Charge (Zeff) measures the force exerted onto an electron by the nucleus.&nbsp;

Periodic Trend: Ionization Energy

Ionization Energy is the energy absorbed&nbsp;in order to remove an electron from a gaseous atom or ion.&nbsp;

Periodic Trend: Metallic Character

Metallic Character&nbsp;deals with how easily an electron can be removed from an element.&nbsp;

Paramagnetism and Diamagnetism

Paramagnetism&nbsp;and&nbsp;Diamagnetism deal with the presence of electrons that are either unpaired or paired in an orbital.

Electron Affinity is the energy released from the addition of an electron to a gaseous atom or ion.&nbsp;

The Electron Configuration: Quantum Numbers

The Quantum Numbers ultimately can be used to determine the precise location of an electron.&nbsp;

Periodic Trend: Electronegativity

Electronegativity is an element's ability to attract electrons.

The Electron Configurations: Exceptions

Most Electron Configuration Exceptions are the result of elements drive to obtain half filled or totally filled d orbitals.&nbsp;

The Electron Configuration: Condensed

Condensed Electron Configurations are a faster method in determining the configuration of elements and ions.&nbsp;