Aim: What are some trends in the periodic table?

Slides:



Advertisements
Similar presentations
Periodic Trends OBJECTIVES:
Advertisements

Periodic Trends (SL) OBJECTIVES:
1/8/09 Warm Up: The observed regularities in the properties of the elements are periodic functions of their Atomic numbers Mass numbers Oxidation states.
Ch 5.3 Electron Configuration and Periodic Properties
Periodic Trends Chapter 6 Section 3.
Ch 5.3 Electron Configuration and Periodic Properties
The Periodic Law says: PERIODIC LAW states that when elements are arranged in order of increasing atomic number, there is a periodic repetition of their.
Chapter 12 The Periodic Table
The Periodic Table The how and why.
1 Chapter 7 Atomic Structure. 2 Periodic Trends n Ionization energy the energy required to remove an electron form a gaseous atom n Highest energy electron.
Section 14.2 Periodic Trends
Periodic Table Trends & Definitions. How to read the Periodic Table 6 C Carbon Atomic Number Elemental Symbol Elemental Name Atomic Mass.
Periodic Properties and Trends Atomic Radii Size Increases going down a group.Size Increases going down a group. Because electrons are added further.
The Periodic Table. History u Russian scientist Dmitri Mendeleev taught chemistry u Mid molar masses of elements were known. u Wrote down the elements.
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:
4 Periodic Trends: 1) Atomic Radius 2) Ionic Radius 3) Ionization Energy 4) ElectroNegativity ibchem.com/IB/ibfiles/periodicity/per_ppt/pt_trends.ppt.
3:00 2:59 2:58 2:57 2:56 2:55 2:54 2:53 2:52 2:51 2:50 2:49 2:48 2:47 2:46 2:45 2:44 2:43 2:42 2:41 2:40 2:39 2:38 2:37 2:36 2:35 2:34 2:33 2:32 2:31 2:30.
TRENDS IN THE PERIODIC TABLE. Important Definitions  Trend : predictable change in a particular direction  Electron Shielding : inner electrons shield.
Periodicity  Atomic Radius = half the distance between two nuclei of a diatomic molecule. } Radius.
Periodic Trends. Atomic Size The electron cloud doesn’t have a definite edge. Scientists get around this by measuring more than 1 atom at a time. Summary:
Periodic Trends. Atomic Size u First problem where do you start measuring. u The electron cloud doesn’t have a definite edge. u They get around this by.
Atomic Size u Atomic Radius = half the distance between two nuclei of a diatomic molecule. } Radius.
Periodic Trends. Atomic Size Every atom has a nucleus and electrons zooming around it How far the outermost electron is from the nucleus determines the.
Periodic Trends. Types of Periodic Trends How elements differ as you move through the periodic table? Atomic Radius Ionic Radius Ionization Energy Electronegativity.
Chemical Periodicity Trends in the periodic table.
ALL Periodic Table Trends Influenced by three factors: 1. Energy Level –Higher energy levels are further away from the nucleus. 2. Charge on nucleus (#
Chapter 6 The Periodic Table
The Periodic Table The how and why.
Lecture 29 Periodic trends Ozgur Unal
The Periodic Table Periodic Trends.
Suggested Reading Pages Section 5-3
Periodic Table & Trends
Periodic Trends Chemistry.
Chemical Periodicity? What?
Ions, Electron Affinity and Metallic Character
Chapter 6 Section 3: Periodic Trends
Periodic Table & Trends
The Periodic Table Periodic Trends.
Trends In The Periodic Table
5.3 Electron Configuration & Periodic Properties
The periodic table.
Periodic Trends OBJECTIVES:
Periodic Groups and Trends
Identifying the patterns
Periodic Table Trends.
Atomic Size First problem where do you start measuring.
Periodic Trends.
Graph #1: Atomic Radius vs. Atomic Number
Unit 2: Electrons & Periodic Behavior
III. Periodic Trends, Part 2 (p )
Periodicity Periodic Table Trends.
Periodicity Periodic Table Trends.
SWBAT Identify trends on the periodic table
Aim: How do we perfect our knowledge of the periodic table?
Chem 332 – O’Dette Periodic trends.
TRENDS IN THE PERIODIC TABLE.
Periodic Table & Trends
Periodic Trends.
Adapted from Stephen L. Cotton
Section 3 Trends and the Periodic Table
Periodic Trends.
Periodic Trends.
5.3 Electron Configuration & Periodic Properties
Chemical Periodicity.
Periodic Trends.
New topic The Periodic Table
Chapter 5 Notes Crash Course Chemistry - Periodic Table.
Periodic Trends.
Presentation transcript:

Aim: What are some trends in the periodic table? Do now: What is the difference between metals and non metals? Announcement: Exam Friday! Hold on to your quizes, half the questions are going to be on the exam.

#1. Atomic Size - Period Trends Going from left to right across a period, the size gets smaller. Electrons are in the same energy level. But, there is more nuclear charge. Outermost electrons are pulled closer. Na Mg Al Si P S Cl Ar

Trends in Ionic Size: Cations Cations form by losing electrons. Cations are smaller than the atom they came from – not only do they lose electrons, they lose an entire energy level. Metals form cations. Cations of representative elements have the noble gas configuration before them.

Ionic size: Anions Anions form by gaining electrons. Anions are bigger than the atom they came from – have the same energy level, but a greater area the nuclear charge needs to cover Nonmetals form anions. Anions of representative elements have the noble gas configuration after them.

#2. Trends in Ionization Energy Ionization energy is the amount of energy required to completely remove an electron (from a gaseous atom). Removing one electron makes a 1+ ion. The energy required to remove only the first electron is called the first ionization energy.

Ionization Energy The second ionization energy is the energy required to remove the second electron. Always greater than first IE. The third IE is the energy required to remove a third electron. Greater than 1st or 2nd IE.

Symbol First Second Third 11810 14840 3569 4619 4577 5301 6045 6276 HHeLiBeBCNO F Ne 1312 2731 520 900 800 1086 1402 1314 1681 2080 5247 7297 1757 2430 2352 2857 3391 3375 3963 Why did these values increase so much?

#3. Trends in Electronegativity Electronegativity is the tendency for an atom to attract electrons to itself when it is chemically combined with another element. They share the electron, but how equally do they share it? An element with a big electronegativity means it pulls the electron towards itself strongly!

Electronegativity Period Trend Metals are at the left of the table. They let their electrons go easily Thus, low electronegativity At the right end are the nonmetals. They want more electrons. Try to take them away from others High electronegativity.

Summary of the Trends

Individual Work Grab the textbook and open to page 170 Read pgs. 170 - 178 Answer question on pg. 178 # 16 - 23