Chemistry Unit 2 Part 4 - Development and Organization of the Periodic Table

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Information about Chemistry Unit 2 Part 4 - Development and Organization of the Periodic...

Published on October 5, 2007

Author: shawnschlueter

Source: slideshare.net

Matter and Change Part 4: Development and Organization of the Periodic Table

TAKS Student Expectation Integrated Physics and Chemistry (7) Science Concepts. The Student knows the relationship between properties and its components. The Student is expected to: (D) relate the chemical behavior of an element including bonding, to its placement on the periodic table.

Integrated Physics and Chemistry (7) Science Concepts. The Student knows the relationship between properties and its components. The Student is expected to:

(D) relate the chemical behavior of an element including bonding, to its placement on the periodic table.

Elements element is a substance made up of similar atoms. All atoms of the same element have the same number of protons very few elements are found in their pure form in nature. Ex: diamond- pure carbon, oxygen in the air, and nitrogen in the air.

element is a substance made up of similar atoms.

All atoms of the same element have the same number of protons

very few elements are found in their pure form in nature.

Ex: diamond- pure carbon, oxygen in the air, and nitrogen in the air.

Introduction to the Periodic Table

The Development of the Periodic Table 1790 – Antonie Lavoisier (France) compiled a list of all known elements at the time – 23. Discovery of new elements progressed rapidly during the industrial revolution.

1790 – Antonie Lavoisier (France) compiled a list of all known elements at the time – 23.

Discovery of new elements progressed rapidly during the industrial revolution.

1864 – John Newlands (England) noticed when elements were arranged in increasing atomic mass, similar properties occurred every eight elements, which he called octaves. 1869- Demetri Medeleev (Russia) and Lothar Meyer (Germany) listed elements by increasing atomic mass, noticing a regular (periodic) recurrence of physical and chemical properties.

1864 – John Newlands (England) noticed when elements were arranged in increasing atomic mass, similar properties occurred every eight elements, which he called octaves.

1869- Demetri Medeleev (Russia) and Lothar Meyer (Germany) listed elements by increasing atomic mass, noticing a regular (periodic) recurrence of physical and chemical properties.

1. Mendeleev’s chart lists those elements with similar properties side by side. Increasing in atomic mass top to bottom. 2. Several of the elements we know today, were still undiscovered. Using the chart Medeleev predicted the properties of Gallium 15 years before it would be discovered.

1. Mendeleev’s chart lists those elements with similar properties side by side. Increasing in atomic mass top to bottom.

2. Several of the elements we know today, were still undiscovered. Using the chart Medeleev predicted the properties of Gallium 15 years before it would be discovered.

However, with the discovery of newer elements, scientists proved that atomic mass was not the proper order.

However, with the discovery of newer elements, scientists proved that atomic mass was not the proper order.

1913- Henry Mosely- proved that atomic number, instead of atomic mass should be used. Like Mendeleev, he also predicted several elements which were to be discovered later.

1913- Henry Mosely- proved that atomic number, instead of atomic mass should be used. Like Mendeleev, he also predicted several elements which were to be discovered later.

Today’s known elements Of the 110(or more) known elements around 30 are most commonly used. around 20 are man made (synthetic elements).

Of the 110(or more) known elements

around 30 are most commonly used.

around 20 are man made (synthetic elements).

Elements can be represented by their chemical “symbol”, not abbreviation, as such, they must be written properly. The first letter of the symbol is always capitalized The second letter of the symbol (if needed), is always lower-case.

Elements can be represented by their chemical “symbol”, not abbreviation, as such, they must be written properly.

The first letter of the symbol is always capitalized

The second letter of the symbol (if needed), is always lower-case.

Improperly written symbols lead to mistakes Cu vs. CU Co vs. CO MgNO 3 vs MnGO 3 . All known elements have been placed on the Periodic Table of the Elements.

Improperly written symbols lead to mistakes

Cu vs. CU

Co vs. CO

MgNO 3 vs MnGO 3 .

All known elements have been placed on the Periodic Table of the Elements.

Periods and Groups The periodic table organizes chemical elements according to their properties Periods- the horizontal rows of the periodic table Groups- the vertical columns of the periodic chart. Elements in the same group have similar chemical and physical properties.

The periodic table organizes chemical elements according to their properties

Periods- the horizontal rows of the periodic table

Groups- the vertical columns of the periodic chart. Elements in the same group have similar chemical and physical properties.

Group Period

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