Unit F321 Module 1.2.1 Electron Structure. Atomic Structure Protons, neutrons, electrons How to make ions Relative atomic mass.

Slides:

Advertisements

Similar presentations

Atomic Models Bohr Model Cloud Model.

Advertisements

A guide for A level students KNOCKHARDY PUBLISHING

Parts of an Atom FlipChart 1st Flap – Write Parts of an Atom 2 nd Flap – Atom –write the definition for atom 3 rd Flap – Neutron –What charge does a neutron.

Learning Objectives: Define first ionisation energy and successive ionisation energy. Explain the factors that influence ionisation energies. Predict the.

Higher Chemistry Unit 1(c) Ionisation energy. After today’s lesson you should be able to: explain the meaning of the term ‘first ionisation energy’. write.

Atomic Structure Ionisation Energies. Ionisation Energy The first ionisation energy of an element is the energy required to remove completely one mole.

Physical Properties. Syllabus statements Define the terms first ionization energy, and electronegativity Describe and explain the trends.

Why Does Sodium Have a Much Higher Second Ionization Energy? 1 st 0.5 kj/mol 2 nd 4.6 kj/mol.

Homework Private study work (bring notes to show me next lesson); Read pages 40 – 41 in your text book and complete the practice questions on each double.

Periodic Table Trends. Metallic character Metallic Character Depends on how readily the element gives up their valence e-’s.

Ionisation Energy. Definition of the first ionisation energy The energy required to remove one mole of electrons from one mole of gaseous atoms to form.

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.

AS Chemistry Unit 1 Module 3 –The Periodic Table

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

Periodic Trends: 3. Ionization Energy 4. Electronegativity

HIGHER CHEMISTRY REVISION. Unit 1:- Patterns in the Periodic Table 1. The three statements below are taken from a note made by a student studying trends.

IB Chemistry ATOMIC THEORY

The Trends in Elements in 1-20 Atomic Size Ionisation Energies.

Trends in the Periodic Table (Chpt. 7). 1. Atomic radius (size) 2. Ionization energy 3. Electronegativity The three properties of elements whose changes.

HIGHER CHEMISTRY REVISION. Unit 1:- Patterns in the Periodic Table 1. The three statements below are taken from a note made by a student studying trends.

Port Hedland and Mt Lawley Senior High Schools Chem 12 Revision Week 1.

Unit 5: Chemical Bonding Q: How do atoms interact with each other? Ionization Energy Ions: Cations & Anions.

Ionization Energies and Group Numbers

Periodic Trends.

Periodic Table Basics. Finding the number of Atomic Particles # of protons = to the atomic # # of electrons = to the atomic # To determine the # of neutrons.

IONISATION ENERGY OBJECTIVES: To define the term ‘ionisation energy’ To describe and explain the trends in ionisation energy across period 3 and down group.

Born-Haber cycles L.O.:  Define and apply the terms enthalpy of formation, ionisation enthalpy, enthalpy of atomisation of an element and of a compound,

Trends in the Periodic Table (Chpt. 7). 1. Atomic radius (size) 2. Ionization energy 3. Electronegativity The three properties of elements whose changes.

Ionisation energy. Definitions The first ionisation energy is the energy required to remove the first (or outermost) electron from each atom in a mole.

Atomic Structure Composition of an atom Atoms are made up of 3 fundamental subatomic particles: Relative mass Relative electric charge Position in atom.

Lesson objectives Define first ionisation energy and successive ionisation energy. Explain the factors that influence ionisation energies. Predict the.

4 Periodic Trends: 1) Atomic Radius 2) Ionic Radius 3) Ionization Energy 4) ElectroNegativity ibchem.com/IB/ibfiles/periodicity/per_ppt/pt_trends.ppt.

After today, you will be able to… Explain what ionization energy is Describe the ionization energy trend from the Periodic Table Explain why it requires.

 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.

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. Atomic radius Atomic radii trends and explanations Atomic radius decreases across a period because each successive element.

LENSES TO PERIODIC TRENDS. There are 3 major lenses through which advanced Chemistry explains the periodic trends in the groups and periods of the Periodic.

Learning Outcomes Atomic radii (covalent radii only). Explanations for general trends in values: (i) down a group (ii) across a period (covalent radii.

There are 6 patterns or trends we discuss when looking at the periodic table… 1. Reactivity 2. Atomic radius or size 3. Ionic radius 4. Ionization energy.

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.

Periodic Trends Chemistry 5(C). Learning objectives Use the periodic table to identify and explain trends in – Atomic and ionic radii – Electronegativity.

Chem 11. Ionization Energy The amount of energy required to completely remove an electron from a gaseous atom. Removing one electron makes a +1 ion.

I II III Periodic Trends. Valence Electrons  Electrons available to be lost, gained, or shared in the formation of chemical compounds  Outer energy.

IONISATION ENERGY CONTENTS What is Ionisation Energy?

The atomic radius increases down Group 2. There are more filled energy levels between the nucleus and the outer electrons, which are more shielded.

 The arrangement of electrons in an atom helps determine the properties and behavior of that atom.

Factors Affecting Periodicity Periodic Trends: Atomic Radius: the distance from the center of the nucleus to the outermost electron (how big an atom is)

AS Chemistry Lesson 4 (24/09/2013) Ionisation Energy Trends across periods & down groups.

AP Chemistry Big Idea 1 Coulomb’s Law & Ionization Energy.

Periodic Trends. Predicting Periodic Trends A number of physical and chemical properties of elements can be predicted from their position in the periodic.

Chemical Periodicity Trends in the periodic table.

Atomic Trends: Atomic Size n = 1 n = 2 n = 3 n = 4 n = 5 n = 6 n = 7 Increasing “n” Larger orbitals Small Large n is constant... Additional electrons.

IONISATION ENERGY. WHAT IS IONISATION ENERGY? Ionisation Energy is a measure of the amount of energy needed to remove electrons from atoms. As electrons.

There is a decrease in ionisation energy as you go down the group. Beryllium to Magnesium.

Unit F321 Module Electron Structure. Atomic Structure Protons, neutrons, electrons How to make ions Relative atomic mass.

12.1 Electrons in Atoms HL.

IONISATION ENERGY OBJECTIVES: To define the term ‘ionisation energy’ To describe and explain the trends in ionisation energy across period 3 and down.

1.6 IONISATION ENERGY OBJECTIVES: To define the term ‘ionisation energy’ To describe and explain the trends in ionisation energy across period 3 and.

Periodic Trends.

IONISATION ENERGY OBJECTIVES: To define the term ‘ionisation energy’ To describe and explain trends in ionisation energy KEY WORDS: IONISATION ENERGY.

4 The Atom & Electronic Configuration

Do Now: Write the electron configurations of the following atoms and ions Na Mg2+ Al3+ Ne.

Orbitals Electron Configurations Orbitals.

1.6 IONISATION ENERGY OBJECTIVES: To define the term ‘ionisation energy’ To describe and explain the trends in ionisation energy across period 3 and.

Presentation transcript:

Unit F321 Module Electron Structure

Atomic Structure Protons, neutrons, electrons How to make ions Relative atomic mass

Mass / kgCharge / C Relative mass Relative charge PROTON NEUTRON ELECTRON x x x x x Inside an atom Atomic number = no. protons in nucleus Mass number = no. protons + no. neutrons Ion: a positively or negatively charged atom or group of atoms

Ionisation Energy What is ionisation energy? Definitions –First ionisation energy –Successive ionisation energies What affects ionisation energy?

WHAT IS IONISATION ENERGY? Ionisation Energy is a measure of the amount of energy needed to remove electrons from atoms. As electrons are negatively charged and protons in the nucleus are positively charged, there will be an attraction between them. The greater the pull of the nucleus, the harder it will be to pull an electron away from an atom. - Attraction between the nucleus and an electron FIRST IONISATION ENERGY - Definition The energy required to remove ONE MOLE of electrons from each atom in ONE MOLE of gaseous atoms to form ONE MOLE of gaseous positive ions. e.g.Na(g) Na + (g) + e - Al(g) Al + (g) + e - Make sure you write in the (g)

WHAT AFFECTS IONISATION ENERGY? The value of the 1st Ionisation Energy depends on the electronic structure HydrogenHeliumLithium The value for helium is higher than that for hydrogen because there are now two protons in the nucleus. The nuclear charge is greater so the pull on the outer electrons is larger. More energy will be needed to pull an electron out of the atom. 519 kJ mol kJ mol kJ mol -1

Ionisation Energy is affected by 3 things: 1.Atomic Radius 2.Nuclear Attraction 3.Electron Shielding

Successive Ionisation Energies A measure of the energy required to remove each electron in turn. Mg(g)  Mg + (g) + e - 1 st I.E. =+738 kJ.mol -1 Mg + (g)  Mg 2+ (g) + e- 2 nd I.E.= kJ.mol -1 Mg 2+ (g)  Mg 3+ (g) + e- 3 rd I.E.= kJ.mol -1 Mg 3+ (g)  Mg 4+ (g) + e- 4 th I.E.= kJ.mol -1

Which electron is removed first? (First Ionisation Energy)

Which electron is removed first? (First Ionisation Energy)

Successive Ionisation Energies of Calcium Draw a graph to show the successive ionisation energies of calcium, using the log 10 values (press log, then the number, then = ) Explain all the main points about the graph that you can see (use Pg 41 of OCR AS Chemistry to help you)

1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 2,8,8,2

Put these words in order of importance: Ionisation energy Atom Successive ionisation energy Ion Energy level Most Important Least Important