10. Periodic Properties of the Elements

Periodic Trend: Electronegativity

Electronegativity and Ionization Energy

Trends in the Periodic Table

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

Electronegativity

What general trends in electronegativity occur in the periodic table?

How to calculate Electronegativity?  Easy Trick

The Periodic Table EXPLAINED | Chemical Families and Periodic Trends

Between which two elements is the difference in electronegativity the greatest?

Periodic Trends: Electronegativity and Electron Affinity

Using only the periodic table as your guide, select the most
electronegative atom in each of the following sets: (d) O, P, Ge, In.

Moving towards the top right corner of the Periodic Table causes electronegativity to increase.

Periodic Trend: Electronegativity Example 1

One scale for electronegativity is based on the concept that
the electronegativity of any atom is proportional to the
ionization energy of the atom minus its electron affinity:
electronegativity = k1I - EA2, where k is a proportionality
constant. (b) Why are both ionization
energy and electron affinity relevant to the notion of
electronegativity?

What is electronegativity | Chemistry | Electronegativity IIT JEE | Electronegativity NEET

A major challenge in implementing the “hydrogen economy”
is finding a safe, lightweight, and compact way of storing
hydrogen for use as a fuel. The hydrides of light metals
are attractive for hydrogen storage because they can store a
high weight percentage of hydrogen in a small volume. For
example, NaAlH4 can release 5.6% of its mass as H2 upon
decomposing to NaH1s2, Al1s2, and H21g2. NaAlH4 possesses
both covalent bonds, which hold polyatomic anions
together, and ionic bonds. (b) Which element in
NaAlH4 is the most electronegative? Which one is the least
electronegative? 

Which element in NaAlH4 is the least electronegative?

One scale for electronegativity is based on the concept that 
the electronegativity of any atom is proportional to the 
ionization energy of the atom minus its electron affinity: 
electronegativity = k1I - EA2, where k is a proportionality 
constant. (c) By using data in Chapter 7, determine 
the value of k that would lead to an electronegativity of 4.0 
for F under this definition.

One scale for electronegativity is based on the concept that
the electronegativity of any atom is proportional to the
ionization energy of the atom minus its electron affinity:
electronegativity = k1I - EA2, where k is a proportionality
constant. (d) Use your result from part (c)
to determine the electronegativities of Cl and O using this
scale. 

Use your result to determine the electronegativity of Cl using this scale.

Predict the electronegativity of the undiscovered element with Z = 119.

Which of the following statements about electronegativity is
false? (a) Electronegativity is the ability of an atom in a molecule
to attract electron density toward itself. (b) Electronegativity is
the same thing as electron affinity. (c) The numerical values
for electronegativity have no units. (d) Fluorine is the most
electronegative element. (e) Cesium is the least electronegative
element.

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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

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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.

Periodic Trend: Electron Affinity

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;

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;

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