Periodic Trends 6.3 Section 6.3-2 Periodic Trends II.

Slides:

Advertisements

Similar presentations

Periodic Trends.

Advertisements

Periodic Trends 6.3.

6.3 Periodic Trends Sodium chloride (table salt) produced the geometric pattern in the photograph. Such a pattern can be used to calculate the position.

Good Morning! To begin today, you will need: 1.3 different colors of writing utensils o colored pencils are up front for your use 2.One blank periodic.

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.

AIM: DETERMINING IONIZATION ENERGY AND ELECTRONEGATIVITY OF ELEMENTS DO NOW: 1. LIST IN ORDER OF INCREASING ATOMIC RADII: MAGNESIUM, SILICON, BARIUM, BROMINE.

Slide 1 of 31 Periodic Trends 6.3. © Copyright Pearson Prentice Hall Slide 2 of 31 Periodic Trends Sodium chloride (table salt) produced the geometric.

Organizing the Elements 6.1

Periodic Trends Trends in Atomic Size

Summary: periodic trends

Slide 1 of 31 © Copyright Pearson Prentice Hall Periodic Trends > Trends in Atomic Size The ___________ ________________ is _________ _________ of the.

Are all atoms the same size? NaMgAlSiPSCl. So then... NaMgAlSiPSCl.

Section 5.3 – Electron Configuration and Periodic Properties

Drill Determine the group and period of the following: Determine the group and period of the following: a. Mg b. Ar c. N.

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.

Chemical Periodicity Ch. 14.

Types of Periodic Trends

Even More About the Periodic Table

Periodic Properties. Atomic Size Atomic size: the radius of an atom (distance from nucleus to electron cloud) is considered. Measured in angstroms (A)

Academic Chemistry Class Notes April 9, 2015 Periodic Trends of the Elements.

Ch-6 sec-3. Atomic Size Atomic Size is measured as half the distance between two nuclei Size generally decreases with atomic number within a period Size.

Periodic Trends.

Periodic Trends. Nuclear Charge Shielding Atomic Radius.

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 Section 6.3.

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.

 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.

Summary of Periodic Trends Topic #12 continued…..

Slide 1 of 31 © Copyright Pearson Prentice Hall Periodic Trends > Trends in Atomic Size The atomic radius is one half of the distance between the nuclei.

End Show Slide 1 of 31 Periodic Trends 6.3. End Show © Copyright Pearson Prentice Hall Periodic Trends > Slide 2 of 31 Trends in Atomic Size What are.

III. Periodic Trends. Types of Periodic Trends Atomic size (atomic radius) Ionic size (ionic radius) Ionization energy electronegativity.

Atomic Size The atomic radius is one half of the distance between the nuclei of two atoms of the same element when the atoms are joined.

Aim: Determining ionization energy and electronegativity of elements

The Diatomics They are elements that are found as two atoms bonded to themselves. They are H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2 There are 7 of them and.

© Copyright Pearson Prentice Hall Slide 1 of 31 Periodic Trends > Types of Periodic Trends 4 Periodic Trends 1.Atomic Radii (AR) 2.Ionization Energy (IE)

Periodic Trends We will explain observed trends in  Atomic (and Ionic) Radius  Ionization Eenergy  Electronegativity size lose e – attract e – nuclear.

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.

Aim: What trends can be observed by studying the periodic table? Homework Reminder:Homework Reminder: Due Wed., Nov. 19, 2014 Read pages Answer.

UNIT 5: THE PERIODIC TABLE. Organizing the Elements How would you organize the people in this room? How did chemists begin to organize the known elements?

1 st Ionization Energy The amount of energy required to remove an electron from an atom. Trend: Increases left to right across a row. Increases bottom.

Chemistry Periodic Trends. Section 5 Definitions Atomic Radius Ion Cation Anion Ionization Energy Electronegativity.

Chemistry Chapter 5 Section 3.  Atomic Radius  Definition: ½ distance between center of adjacent nuclei of bonded atoms  Trends: p141  Within group,

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.

Slide 1 of 31 Periodic Trends 6.3. © Copyright Pearson Prentice Hall Slide 2 of 31 Periodic Trends Sodium chloride (table salt) produced the geometric.

For any representative element its group number equals the number of valance electrons (electrons in the highest occupied energy level)

Ionic Bonds Chapter 14.

Aim: What are the Properties of Groups and how does the atomic radius change across a period and down a group? Do Now: Answer in your notebook If an atom.

Chapter 6 The Periodic Table 6.3 Periodic Trends

Aim: Determining ionization energy and electronegativity of elements

Periodic Trends 6.3.

Periodic Trends 6.3.

Chapter 6 Section 3: Periodic Trends

nuclear charge & shielding

Periodic Trends The Periodic Law Classification of Elements

The Periodic Table Periodic Trends.

Periodic Trends 6.3.

Chapter 6 The Periodic Table 6.3 Periodic Trends

The Periodic Table 6.3 Periodic Trends.

Periodic Trends 6.3.

6.3 Trends in Atomic Size Trends in Atomic Size

Periodic Trends 6.3.

Periodic Trends 6.3.

III. Periodic Trends (p )

Electronegativity.

6.3 Periodic Trends Sodium chloride (table salt) produced the geometric pattern in the photograph. Such a pattern can be used to calculate the position.

Periodic Trends 6.3.

6.3 Trends in Atomic Size The atomic radius is one half of the distance between the nuclei of two atoms of the same element when the atoms are joined.

Periodic Trends 6.3.

Periodic Trends 6.3.

Presentation transcript:

Periodic Trends 6.3 Section 6.3-2 Periodic Trends II

Some compounds are composed of particles called ions. 6.3-2 Ions Some compounds are composed of particles called ions. An ion is an atom or group of atoms that has a positive or negative charge. A cation is an ion with a positive charge. An anion is an ion with a negative charge.

Trends in Ionization Energy 6.3-2 Trends in Ionization Energy Trends in Ionization Energy What are the trends among the elements for first ionization energy, ionic size, and electronegativity?

Trends in Ionization Energy 6.3-2 Trends in Ionization Energy The energy required to remove an electron from an atom is called ionization energy. The energy required to remove the first electron from an atom is called the first ionization energy. The energy required to remove an electron from an ion with a 1+ charge is called the second ionization energy.

Trends in Ionization Energy 6.3-2 Trends in Ionization Energy Group and Periodic Trends in Ionization Energy First ionization energy tends to decrease from top to bottom within a group and increase from left to right across a period.

Trends in Ionization Energy 6.3-2 Trends in Ionization Energy

Trends in Ionization Energy 6.3-2 Trends in Ionization Energy Largest Smallest

Trends in Ionization Energy 6.3-2 Trends in Ionization Energy largest First ionization energy tends to increase from left to right across a period and decrease from top to bottom within a group. Predicting Which element would have the larger first ionization energy—an alkali metal in period 2 or an alkali metal in period 4? smallest

Trends in Electronegativity 6.3-2 Trends in Electronegativity Trends in Electronegativity Electronegativity is the ability of an atom of an element to attract electrons when the atom is in a compound. In general, electronegativity values decrease from top to bottom within a group. For representative elements, the values tend to increase from left to right across a period.

Trends in Electronegativity 6.3-2 Trends in Electronegativity Representative Elements in Groups 1A through 7A Largest Smallest

Summary of Trends What is the underlying cause of periodic trends? 6.3-2 Summary of Trends Summary of Trends What is the underlying cause of periodic trends?

6.3-2 Summary of Trends The trends that exist among these properties can be explained by variations in atomic structure.

Nuclear Charge Electronegativity Size of anions Ionic size 6.3-2 Summary of Trends Nuclear Charge Electronegativity Size of anions Ionic size Ionization energy Shielding Size of cations Atomic Size Decreases Constant Increases Decreases Increases Properties that vary within groups and across periods include atomic size, ionic size, ionization energy, electronegativity, nuclear charge, and shielding effect. Interpreting Diagrams Which properties tend to decrease across a period?

1. Which of the following sequences is correct for atomic size? 6.3 Section Quiz 1. Which of the following sequences is correct for atomic size? Mg > Al > S Li > Na > K F > N > B F > Cl > Br

gain electrons to form cations. gain electrons to form anions. 6.3 Section Quiz 2. Metals tend to gain electrons to form cations. gain electrons to form anions. lose electrons to form anions. lose electrons to form cations.

3. Which of the following is the most electronegative? 6.3 Section Quiz 3. Which of the following is the most electronegative? Cl Se Na I

The End ! !