3.4 Periodic Table and Periodic Trends

Slides:



Advertisements
Similar presentations
Periodic Trends.
Advertisements

Periodic Trends Periodic law states that elements are arranged by their atomic numbers with similar properties occuring at regular intervals.
Periodic Trends Compiled by R. Erwin Rockwall ISD.
The Periodic Table When Dimitri Mendeleev developed the Periodic Table, he grouped elements according to their physical properties. As it turns out, there.
Periodic Table Trends. Atomic Radius As you move down a group, atomic radius increases The number of energy levels increases as you move down a group.
Periodic Law History of the Periodic Table Periodic Trends.
Section 5-3 Periodic Trends. Atomic Radius Distance from the center of the atom’s nucleus to the outermost electrons. 1. Atoms get larger going down a.
The Periodic Table Textbook Pages: The Development of The Periodic Table Dmitri Mendeleev ( ) Russian Chemist Developed table according.
Periodic Properties Chemical and physical properties of the elements change with their position in the periodic table.
The Periodic Table Chapter 5. Dmitri Mendeleev Dmitri Mendeleev developed the periodic table in 1869 Dmitri Mendeleev developed the periodic table in.
Dmitri Mendeleev (1834 – 1907) listed elements in vertical columns in order of increasing atomic mass noticed recurrence of their physical and chemical.
Periodic Properties Chapter 12 Notes. Valence Electrons Valence electrons – Electrons in the outer energy level that can be lost, gained, or shared (connected.
Let’s Play Sit in teams of 4. Periodic Table- History and Organization.
Periodic Trends Atomic Radius Ionic Radius Ionization Energy Electronegativity.
History of the Periodic Table
Electron Configuration and Periodic Properties
Periodic Trends The physical and chemical properties of the elements are periodic functions of their atomic numbers.
The Periodic Table Sec 1 How are Elements Organized
Atomic Radius Definition: The distance from the center of an atoms nucleus to it’s outermost electron Radius decreases across a period Measure of atomic.
Periodic Trends.
The Periodicities of the Periodic Table
Suggested Reading Pages Section 5-3
Periodic Trends.
Periodic Table & Trends
The Periodic Table trends.
Write the Complete Electron Configuration for:
Periodic Trends Chemistry.
Periodic trends.
Periodic Trends.
AP CHEMISTRY Ms. Paskowski
Periodic Table Trends.
History of Periodic Table and Periodicity
Periodicity: Looking at the below diagram you will see a red stair- step line. This is the periodic table’s dividing line. On the left side of the line.
Periodic Trends Chemistry 2.
Periodic Properties Chemical and physical properties of the elements change with their position in the periodic table.
The Periodic Table and Periodic Law
Periodic Properties.
Periodic Trends.
PERIODIC TABLE TRENDS & REACTIVITY
Unit 8: The Periodic Table Trends
PERIODIC TABLE.
Part IV: Periodic Trends
Periodic Table Properties and trends.
Trends in the Periodic Table
Unit 4: The Periodic Table
Periodic Trends.
The Periodic Table TRENDS.
Unit 2: Electrons & Periodic Behavior
3.1 Periodic Table and Periodic Trends
How are elements organized?
Development of The Periodic Table and Trends
Periodic Trends Chp 6.
Periodic Trends.
Atomic Radii Ionic Radii Ionization Energies Electronegativity
Periodic Trends.
Periodic Trends The physical and chemical properties of the elements are periodic functions of their atomic numbers.
The Periodic Law (Periodic Table)
III. Periodic Trends (p )
Atomic Radius: size of atom
Chapter14: Periodic Trends
Periodic Trends.
Periodic Trends.
The Periodic Table Chapter 5.
Periodic Trends.
3.1 Periodic Table and Periodic Trends
Periodic Trends.
Periodic Table Chapter 6.
Electron Configuration and Periodic Properties
Atomic Radii Ionic Radii Ionization Energies Electronegativity
Periodic Trends.
Presentation transcript:

3.4 Periodic Table and Periodic Trends Chemistry Objectives 5:a-b, d-e

Essential Questions Why do we use the periodic table? How did the periodic table come into being? How is the periodic table arranged? Why do groups share properties? What are the different periodic trends and how do they change going across and down the periodic table?

Periodic Table Why do we have a periodic table? The periodic table provides a way for organizing elements Why does this matter? The periodic table tells us what properties an element will have

History of the Periodic Table The first periodic table was based off of the work of Mendeleev Mendeleev arranged the elements in his periodic table in order of increasing atomic mass and grouped them according to properties.

History of the Periodic Table (cont) The elements were grouped in columns He even left places for undiscovered elements. Look at Ar, Ca, and K what do you notice?

History of the Periodic Table (cont) How is the current periodic table arranged? Atomic number Moseley arranged the periodic table by atomic number so that elements with the same properties fall into the same column

Arrangement of the Periodic Table The vertical columns of the periodic table are called groups The horizontal rows of the periodic table are called periods The properties of the elements change as you move across a period from left to right. The elements in the same group share properties

Group Properties The common properties of elements in the same group come from having the same valence electrons Valence electrons are “outer shell” or outer energy level electrons. Valence electrons determine an element’s chemical properties

Periodic Trends: Radius Atomic radius is the distance from the center of the nucleus to the outermost electron Atomic radii decreases going across the periodic table and increases as you go down the periodic table

Periodic Trends: Radius (cont) Increases because of adding e- shells Decreases because of increased attractions between nucleus and e- Changes going across rows are smaller than changes going down columns

Periodic Trends: IE Ionization energy (IE) is the energy required to remove an e- Ionization energy increases as you move from left to right across the periodic table and decreases as you go down the periodic table

Periodic Trends: IE (cont) The IE increases going across because as radius decreases the attraction between the nucleus and the electrons increases The IE decreases going down because the as radius increases the attraction between the electron and the nucleus decreases

Periodic Trends: IE (cont) First ionization is lower in energy then the second The second electron is harder to remove because it is closer to the nucleus Valence electrons have a much lower IE then inner shell electrons because inner shell electrons are entire energy level closer to the nucleus

Periodic Trends: e- affinity The energy change that occurs when an electron is acquired by a neutral atom is called the atom’s electron affinity. Electron affinity generally increases across periods. Smaller radius makes it easier to attract electrons Electron affinity generally decreases down groups. The larger radius makes it more difficult to attract/gain electrons Exception is column 18

Periodic Trends: Electroneg Electronegativity is a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound. Electronegativities tend to increase across periods, and decrease or remain about the same down a group. Exception is column 18 equals 0

Essential Questions Why do we use the periodic table? How did the periodic table come into being? How is the periodic table arranged? Why do groups share properties? What are the different periodic trends and how do they change going across and down the periodic table?

3.4 Tracked Assignment p 160 # 2-3, 5, 7 p 178 # 16, 18, 20, 22, 23