Ionic Radius Ionization Energy Electron Affinity

Slides:



Advertisements
Similar presentations
Drill – 11/19 What is meant by “periodic trend”?.
Advertisements

Modern Chemistry Chapter 5 The Periodic Law
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.
Matter Trends and Chemical Bonding Expectations: B2.2, B Periodic Trends and Atomic Properties.
PERIODIC TRENDS What are they? Properties we can predict from the periodic table Why are they? A few reasons explain them.
Periodic Trends Atomic Radius Ionic Radius Ionization Energy Electronegativity.
Agenda Block 4 Attendance Make Groups for element assignment
Electron Configuration and Periodic Properties
Periodic Trends.
The Periodicities of the Periodic Table
Effective Nuclear Charge (Zeff)
Periodic Trends.
Shielding Effect The shielding effect is the reduction of attractive force between the nucleus (+) and its outer electrons (-) due to the blocking affect.
Suggested Reading Pages Section 5-3
Periodic table trends Answers
Periodic Trends.
Periodic Trends: Atomic & Ionic Radii
NOTES ON PERIODIC TRENDS 6.1 Effective Nuclear Charge (Zeff)
SCH3U Mr. Krstovic Agenda: 1) Atomic and Ionic Trends
Periodic Trends.
Trends in the Periodic Table
Examination of properties reveals why
Ions, Electron Affinity and Metallic Character
NOTES ON PERIODIC TRENDS 6.1 Effective Nuclear Charge (Zeff)
Periodic Trends.
Chapter 6 Section 3: Periodic Trends
Periodic Trends.
Atomic Radius.
Periodic Table Trends.
Explaining 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 5(C)
Trends In The Periodic Table
Periodic Trends.
Unit 3 – Lesson 3 Periodic Table.
Periodic table trends Answers
Chem Take out your periodic table Work on Do Now questions
Exploring Periodic Trends
Periodic Trends.
Periodic Trends.
Periodic Groups and Trends
Identifying the patterns
Periodic Table Trends.
Section 4.5—Periodicity – Notable trends of the table
Atomic Size First problem where do you start measuring.
Decoding the Periodic Table
Periodic Trends.
Trends in the Periodic Table
Trends in the Periodic Table
Section 4.5—Periodicity – Notable trends of the table
Periodic Trends Glencoe: Section 6.3.
PERIODIC TRENDS Unit 4.
Periodic Trends.
Atomic Radii Ionic Radii Ionization Energies Electronegativity
Elemental Properties and Patterns
Periodic Trends Chapter 14.2.
Periodic Trends.
Atomic Radius: size of atom
Chem Get packet from yesterday stamped. Take out your periodic table
Section 3 Trends and the Periodic Table
Section 4.5—Periodicity.
PERIODIC TRENDS.
Trends in the Periodic Table
Periodic Trends, Cont. Shielding Ion Size Ionization Energy Electronegativity.
Electron Configuration and Periodic Properties
Atomic Radii Ionic Radii Ionization Energies Electronegativity
Periodic Trends.
Chem Turn in lab if you did not do so last class
Periodic Trends.
Presentation transcript:

Ionic Radius Ionization Energy Electron Affinity Periodic Trends

Ionic Radius The average distance from the centre of the nucleus to the outer edge where electrons may be found for an ION (charged atom) Cation – a positive charged ion formed by the loss of one or more electrons Anion – a negative charged ion formed by the addition of one or more electrons

Trend In general all cations become smaller than their corresponding atom In general all anions become larger than their corresponding atom. Explain WHY using what we talked about yesterday.

Cation When an atom forms a positive ion, electrons are lost so that the atom has the same number of electrons as the closest Noble Gas. In doing so, an entire energy level is lost. The force of attraction of the nucleus is now shared among fewer electrons and therefore stronger, resulting in a smaller radius.

Anion When an atom forms a negative ion, electrons are gained so that the atom has the same number of electrons as the closest Noble Gas. The force of attraction of the nucleus is now shared among more electrons and therefore weaker, resulting in a larger radius.

Ionization Energy The quantity of energy required to remove an electron from an atom or ion in the gaseous state. (form a cation). There may be more than one electron that can be removed so it is usually specified which electron is being removed. 1st IE is the energy required to remove the most loosely held electron. Etc.

Trend in Ionization Energy Using the graph, determine the trend for IE across a period as well as in a group. Explain why.

IE Trend Explained As you move down a group, first ionization energy decreases. WHY? Electrons are further from the nucleus and thus easier to remove the outermost one. "SHIELDING" - Inner electrons at lower energy levels essentially block the protons' force of attraction toward the nucleus.  It therefore becomes easier to remove the outer electron

IE Trend Explained As you move across a period, first ionization energy increases. WHY? - As you move across a period, the atomic radius decreases, that is, the atom is smaller.  The outer electrons are closer to the nucleus and more strongly attracted to the center.  Therefore, it becomes more difficult to remove the outermost electron.

Second and Higher Ionization Energies Definition:  Second Ionization Energy is the energy required to remove a second outermost electron from a ground state atom.  Subsequent ionization energies increase and become a maximum once an ion has reached the state like that of a noble gas.  It becomes extremely difficult to remove an electron from an atom once it loses enough electrons to lose an entire energy level so that its valence shell is filled.

Electron Affinity The energy change (energy released) that occurs when an electron is ADDED to a neutral atom in the gaseous state to form an anion.

EA Trend Across a period the EA generally increases up to the Halogens and drops off significantly with the Noble Gases. Down a group the EA generally decreases.

Summary of Increasing Trends

Homework Read pages 36-41 Questions: page 41 #1-6,8