10. Periodic Properties of the Elements

Periodic Trend: Metallic Character

What Are Metallic Bonds | Properties of Matter | Chemistry | FuseSchool

Neither strontium (Sr) nor antimony (Sb) is shown in the activity series of Table 4.5. Based on their positions in the periodic table, which would you expect to be the better reducing agent? Will the following reaction occur? Explain.

Metallic Character and Non metallic Character in Periodic Table | Chemistry

Periodic Trend: Metallic Character Example 1

Moving towards the top right corner of the Periodic Table causes metallic character to decrease.

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

⚗️ Determining Metallic Character based on Periodic Table Trends

3.2 Trends in metallic character (SL)

Periodic Trends: Metallic Character

Consider the elements: Na, Mg, Al, Si, P. 
c. Which element is least metallic?

Trends - Electron Affinity and Metallic Character

Arrange these elements in order of decreasing metallic character:
Sr, N, Si, P, Ga, Al.

Arrange these elements in order of increasing metallic character: 
Fr, Sb, In, S, Ba, Se.

Choose the more metallic element from each pair. 
c. Cl or O

The most metallic elements are located in the lower left hand corner of the periodic table.

 Metallic character generally increases right left along a row of the periodic table and from the top to the bottom of a column. 

Of the elements listed in the choices, which would be expected to have the most metallic character?

Choose the more metallic element from each pair. 
a. Sb or Pb 
b. K or Ge 
c. Ge or Sb 
d. As or Sn

Little is known about the properties of astatine, At, because
of its rarity and high radioactivity. Nevertheless, it is possible
for us to make many predictions about its properties. (b) Would you expect At to be a metal,
nonmetal, or metalloid? Explain.

Metallic Character

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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;

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;

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;

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