Periodic Trends Elemental Properties and Patterns.

Slides:



Advertisements
Similar presentations
Periodic Trends.
Advertisements

The Periodic Table Dmitri Mendeleev –designed periodic table in which the elements were arranged in order of increasing atomic mass Henry Moseley –designed.
PERIODIC TRENDS Elemental Properties and Patterns.
Trends and the Periodic Properties
Electron Configuration and Periodic Properties
Aim: What are the Properties of Groups and how does the atomic radius change across a period and down a group ? DO Now: 1. Write down the electron configuration.
5-3 Electron Configurations and Periodic Properties
Ch 5.3 Electron Configuration and Periodic Properties
Ch 5.3 Electron Configuration and Periodic Properties
Atomic Radius A measure of the size of an atom – how close it lies to its neighbor. Half the distance between 2 adjacent, identical atoms (crystal or molecule).
For Test #7: The Periodic Table The Periodic Table 1)Dimitri Mendeleev – 1st to publish a periodic table. 2) The Periodic Law: When arranged by increasing.
Summary: periodic trends
Elemental Properties and Patterns  The Periodic Law  Dimitri Mendeleev (1869/1871) was the first scientist to publish an organized periodic table of.
Chemical Periodicity Chart
Chapter 6.
Are all atoms the same size? NaMgAlSiPSCl. So then... NaMgAlSiPSCl.
Section 5.3 – Electron Configuration and Periodic Properties
Chapter 6 The Periodic Table 6.3 Periodic Trends
Mendeleev Made periodic table based on atomic mass and other properties. (especially chemical) Had blank spots for undiscovered elements Called periodic.
CH 6.3 Periodic Trends.
Chapter 9 Chemical Periodicity Chemistry
Periodic Trends 6.3.
Chapter 6 The Periodic Table 6.3 Periodic Trends
The Periodic Table and Periodic Trends
Section 6.3 Periodic Trends
Periodic Table Trends & Definitions. How to read the Periodic Table 6 C Carbon Atomic Number Elemental Symbol Elemental Name Atomic Mass.
What are the periodic trends?
 Russian chemist Dmitri Mendeleev placed the known elements in order of increasing atomic mass.  When he did this he noticed that the elements’ properties.
Periodic Trends Section 6.3
Chapter14: Periodic Trends Modern Chemistry; Holt, Rinehart, & Winston.
Periodic Trends.
Periodic Table Alkali Metals Group 1A Alkaline Metals Group 2A Transition Metals Group B Metalloids (7) Purple elements Halogens Group 7A Noble Gases Group.
Periodic Trends OBJECTIVES:
Periodic Relationships Among the Elements
Periodic Trends Section 6.3.
Periodic Trends. Trends in Atomic Size Atomic Radius –Half of the distance between the nuclei of two atoms of the same element when the atoms are bonded.
4 Periodic Trends: 1) Atomic Radius 2) Ionic Radius 3) Ionization Energy 4) ElectroNegativity ibchem.com/IB/ibfiles/periodicity/per_ppt/pt_trends.ppt.
Atoms. Periodic Table and Electron Configurations Build-up order given by position on periodic table; row by row. Elements in same column will have the.
The Periodic Table The Modern Periodic Table u The modern periodic table is based on the atomic numbers of the elements.
Lesson Starter Define trend. Describe some trends you can observe, such as in fashion, behavior, color, design, and foods. How are trends used to classify?
 Size is expressed in terms of atomic radius.  Atomic radius is ½ the distance between the nuclei of two atoms of the same element when the atoms are.
Periodic Table Trends. (1) Atomic Radius As one goes from left to right across a period, the atomic radii decreases. Reason: All the elements in a period.
Module 3.03 Periodic Trends.
Periodic Trends Periodic Table is arranged by: Atomic number Groups
Periodic Trends Chapter 6 Section 3. Atomic radius Electron clouds do not have clearly defined edges. Electron clouds do not have clearly defined edges.
Periodic Trends Trends in Properties on the Periodic Table.
Periodicity: The arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column, or group.
Periodic Trends Notable trends of the table. What are periodic trends on the periodic table? The predictable pattern by which properties of elements change.
Periodic Trends.
The Periodic Table. ( very ) Brief History 1869 Mendeleev* & Meyer published similar tables * First to be recognized at international convention – Elements.
Periodic Trends Chemistry 5(C). Learning objectives Use the periodic table to identify and explain trends in – Atomic and ionic radii – Electronegativity.
Aim: What are the Properties of Groups and how does the atomic radius change across a period and down a group ? Do Now: 1. Take out your periodic tables.
Section 3: Periodic Trends. Nuclear Charge Nuclear charge is the pull that an electron “feels” from the nucleus. The closer an electron is to the nucleus,
What are the period and group trends of different properties?
Periodic Trends Objectives: AHSGE Reading 4.3 Discern organizational patterns. Other AOD C.3.2 Recognize periodic trends of elements, including the number.
Christopher G. Hamaker, Illinois State University, Normal IL © 2008, Prentice Hall Chapter 10b Periodic Trends INTRODUCTORY CHEMISTRY INTRODUCTORY CHEMISTRY.
PERIODIC TRENDS. Periodic Law When elements are arranged in order of increasing atomic number, elements with similar properties appear at regular intervals.
Chemical Periodicity Trends in the periodic table.
Periodic Trends Section 6.3. Periodic Law The pattern of properties within a period repeats as you move across a period from left to right… When elements.
Periodic Trends 4th block Chemistry.
Atomic and Ionic Radius
Chemistry Chapter 6 The Periodic Law.
Write the Complete Electron Configuration for:
Periodic trends.
The Periodic Table Periodic Trends.
Periodic Trends Section 6.3.
Periodic Trends Section 6.3.
Periodic Trends Section 6.3.
III. Periodic Trends (p )
Chapter 5 Periodic Trends.
Presentation transcript:

Periodic Trends Elemental Properties and Patterns

The Periodic Law Mendeleev understood the ‘Periodic Law’ which states: When arranged by increasing atomic number, the chemical elements display a regular and repeating pattern of chemical and physical properties.

Atomic and Ionic Radius Periodic Trends – chapter 6.3

Objectives Compare period and group trends of several properties Relate period and group trends in atomic radii to electron configuration

Atomic Radius The electron cloud surrounding the nucleus is based on probability and does not have a defined edge Atomic size is determined by how closely an atom lies to a neighboring atom.

Trends within periods In general, there is a decrease in atomic radii as you move left to right across a period This is caused by the increasing positive charge in the nucleus and the fact that the principal energy level stays the same. Because the electrons are in the same energy level, there is no “sheild” from the increased pull of the nucleus. (Shielding effect remains constant) The result is that the increased nuclear charge pulls the outermost electrons closer to the nucleus.

Look at the trend within the periods.

Trends within groups Atomic radii generally increase as you move down a group. Moving down a group the outermost orbital increases in size along with the increasing principal energy level. The nuclear charge increases, but the electrons are in a larger energy level with more other levels “shielding” in between.

Look at the trend within groups.

Summarize this trend with arrows and descriptive words.

Practice Problems For each of the following pairs, predict which atom is larger? – Mg, Sr – Sr, Sn – Ge, Sn – Ge, Br – Cr, W

Ionic Radius When an atom gains or loses electrons, it becomes an ion. Because an electron is negatively charged, atoms that lose or gain acquire a net charge – If an atom loses electrons it becomes _________ – If an atom gains electrons it becomes _________

Ionic Radius Continued When an atom loses electrons, they always become smaller. When atoms gain electrons, they always become larger.

Trends within periods In general as you move left to right across a period, the size of the positive ions gradually decreases. Then, beginning in groups 5A or 6A, the size of the much larger negative ions also gradually decreases.

Look at the trends for ionic size as you move across a period.

Trends within groups As you move down a group, an ion’s outer electrons are in higher principal energy levels, resulting in increased size.

Look at the trends in ionic size as you move down a group

Practice Problems For each of the following pairs, predict which atom or ion is larger – Mg, Mg 2+ – S, S 2- – Ca 2+, Ba 2+ – Cl -1, I -1 – Na +1, Al 3+