Periodicity of Melting Points…

Slides:

Advertisements

Similar presentations

CHEMICAL BONDING.

Advertisements

Boiling Points Andrew, Annie, Paulina, Claudia. What Is Boiling Point? The temperature at which the vapor pressure of the liquid equals the environmental.

Periodic Table Trends. Ionization Energy Increasing or Decreasing?

Ionic & Molecular Compounds Electronegativity Susan Baird Dori Delaney Cindy Rothwell.

Building Blocks 1d Int

Chapter 14 Liquids and Solids. Three types of bonding between atoms Covalent – electrons shared between nonmetal atoms, forms molecules or covalent crystal.

Covalent network lattices and covalent layer lattice

 Water molecule dipole moment.  The polarity of water affects its properties –Causes water to remain liquid at higher temperature –Permits ionic compounds.

Introduction to ATOMS. Electrons are always on the move.

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

Table of Contents Atoms, Bonding, and the Periodic Table Ionic Bonds Covalent Bonds Bonding in Metals Atoms and Bonding.

General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake 5.9 Attractive Forces in Compounds Chapter 5 Compounds and Their Bonds © 2013.

Metallic bonding and structure L.O.:  Describe metallic bonding as the attraction of positive ions to delocalised electrons.  Describe giant metallic.

Periodicity Physical Properties Ionisation energies Li Rb Kr K Ar Na Ne He.

12.2 – Structures Heolddu Comprehensive School 27/05/2016.

Section 12.1 Characteristics of Chemical Bonds 1.To learn about ionic and covalent bonds and explain how they are formed 2.To learn about the polar covalent.

The atomic radius decreases across Period 3 because the force of attraction between the nucleus and the electrons increases.

Based on their structures, explain why sodium oxide, silicon dioxide and carbon dioxide have different melting points. Here are 6 real student answers.

Why do atoms bond? They want to have a full outer electron shell. This is why oxygen that we breathe in is O 2, chlorine gas is Cl 2 etc… METALNON-METAL.

Chemical Bonding Ionic Bonding

Periodic Trends State and explain the following trends: the answers.

Table of Contents Atoms, Bonding, and the Periodic Table Ionic Bonds Covalent Bonds Bonding in Metals Atoms and Bonding.

Type of sub-atomic particleRelative chargeMass Proton Neutron Electron.

Leaving Out the d-block Size Matters Which is the bigger out of the following pairs of atoms: 1.N or P 2.Se or Br 3.Na or Cl.

Foundation Chemistry Semester 1 Dr Joanne Nicholson

Section 12.1 Characteristics of Chemical Bonds 1.To understand why atoms form bonds 2.To learn about ionic and covalent bonds and explain how they are.

What are Intermolecular forces? Intermolecular forces are weak forces of attraction between some covalent molecules. These attractions are responsible.

C2 – Chemistry The Atom, Particles and Bonding. C2 – Chemistry - AIMS to represent the electronic structure of the first twenty elements of the periodic.

Covalent Compounds Covalent compounds share electrons to make bonds. These compounds DO NOT involve ions The smallest component of a covalent compound.

An ionic lattice: a giant regular repeating pattern of alternating positive and negative ions in 3D. The packing structure of the ions depends on the relative.

Apply electronegativity values and the position of two elements on the periodic table to determine the type of dominant bonding that occurs; ionic, polar.

(B) Periodicity. After completing this topic you should be able to : ATOMIC STRUCTURE Bonding in the first 20 elements Learners should be familiar with.

Period 3 Melting/Boiling Points in Period 3. ElementDescription Na They are metals. They have giant structures. They lose their outer electrons to form.

3.2.1 Periodicity. The periodic table The periodic table is a list of all the elements in order of increasing atomic number. You can predict the properties.

Polarity and Physical Properties Review

Macromolecular / giant covalent Molecular / simple covalent

From Standard Grade If we exclude the metal elements

Intermolecular forces

What are intermolecular forces?

Chapter 4.4: Intermolecular forces

Example diagram and detailed description of bonding in substance

Atoms and Bonding Table of Contents

CfE Higher Supported Study

Intermolecular Forces

Macromolecular / giant covalent Molecular / simple covalent

Practice: True or False

Intermolecular Forces

Bonding Knowledge Organiser

For a simple molecular substance to boil, energy is needed to overcome the

Bonding Structures Nat 5

Intermolecular Attractions

Intermolecular Forces

Chemistry – Jan 9, 2018 P3 Challenge- Objective –

[ ] [ ] + - EDEXCEL KEY CONCEPTS 2 Types of substances Ionic bonding

Intramolecular forces vs. Intermolecular forces

Aim: What attracts molecules to each other?

Chapter 8 Liquids and Solids.

Bonding Bonding.

Chemicals of the Natural Environment.

Types of Bonding Objectives: 1. Identify the 3 main types of bonds

Intramolecular Forces

Why does aluminium conduct electricity well?

Simple Molecular Covalent

Intermolecular Forces

Quiz What is an electrostatic dipole.

Which type of bonding is it?

All you need to know about Additional Science

CfE Higher Chemistry Unit 1 Chemical Changes and Structure

Presentation transcript:

Periodicity of Melting Points… Assign the bonding and structure across period 3

Giant Metallic Lattice Periodicity of Melting Points… Metallic Bonding Giant Metallic Lattice

Giant Covalent Lattice Periodicity of Melting Points… Covalent Bonding Giant Covalent Lattice

Periodicity of Melting Points… Covalent Bonding Simple Molecular

Periodicity of Melting Points… Based on the type of structure predict (and justify) which element has the: Highest melting point Lowest melting point

Periodicity of Melting Points… Highest = Silicon Strongest bonds therefore requires the most energy to break them Lowest = Argon Single atoms mean no bonds that can have a dipole induced. Lowest IM forces, so least energy required.

Periodicity of Melting Points… We are going to look at the trend in the melting points of period 2. From the data, produce a relevant graph (this is going to be assessed) Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Melting Point /oC 180 1280 2027 3700 -210 -219 -187 -248.6

Periodicity of Melting Points… Why is there a steep decrease in melting point between carbon and nitrogen? (4) Why do Group two metals have a higher melting point than Group one? (3)

Periodicity of Melting Points… Why is there a steep decrease in melting point between carbon and nitrogen? (4) Both compounds have covalent bonds Carbon is a giant covalent lattice Nitrogen is a simple molecule with INTERMOLECULAR forces Covalent bonds require more thermal energy to break than intermolecular forces

Periodicity of Melting Points… Why do Group two metals have a higher melting point than Group one? (3) Metallic bonding is the electrostatic attraction between the positive ions and the delocalised electrons Group 2 metals have a 2+ charge AND group 1 metals have a 1+ charge The stronger electrostatic attraction between 2+ and an electron requires more energy to overcome

Periodicity of Melting Points… Using a mark scheme correctly is a skill. It allows you to gauge the level you are currently working at. Unfortunately most students don’t use them properly. Mark the example question using the mark scheme.