How many spherical objects can you think of? Starter

If an electron was enlarged to the size of our Solar System it would be perfectly round: to within the width of a human hair. perfectly-round-scientists-discover.html

1.1 Structures and bonding

By the end of today: –You will all be able to name the parts of an atom. –State the charges of each particle. –Define atomic (proton) number. –Describe how the elements are ordered in the periodic table. 1.1 Atomic Structure

Homework Homework Homework Go to mrmathesonsphysics.wikispaces.com and complete ‘Homework 1’ on the C2 page Buy/steal/acquire a compass for drawing circles.

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By the end of today: –You will be able to draw the ‘electronic structure’ of the first 20 elements. –State the relationship between the electrons in the highest energy level and the group. –Some will be able to explain how the electronic configuration relates to its properties. 1.2 Arrangement of Electrons in Atoms

Electrons occupy particular energy levels. Each electron in an atom is at a particular energy level (in a particular shell). The electrons in an atom occupy the lowest available energy levels (innermost available shells). 1st shell - up to 2 electrons 2nd shell - up to 8 electrons 3rd shell - up to 8 electrons Electronic Structure

Draw a clear diagram showing all the particles in a Hydrogen atom. Then a clear diagram showing all the particles in a Sodium atom. And finally a clear diagram showing all the particles in a Uranium-235 atom.

The easier way Sodium Na 2,8,1

The easier way Sodium ion Na + 2,8

Tasks Copy and complete this table for the first 20 elements: Element Symbol Electron Arrangement Hydrogen H 1 Page Complete Summary Questions 1, 2 and 3 Remember to draw the electron arrangement with a pencil and compass. Make the diagrams large and clear. This should take no more than 15 minutes.

1.Nucleus, shells (energy levels), energy levels (shells), energy, period, electron, group. 2.a)b) c)d) 3.They both have full outer shells which are stable. Answers

By the end of today: –You will be able to name the two types of bonding present in compounds. –Explain why atoms bond. –Explain and work out the charge on an ion. –Explain the formation of ions when elements react together. 1.3 Chemical Bonding

What are sodium's properties? What are chlorine’s properties? What are sodium chlorides properties? Elements have very different properties compared to the compounds they make.

Learning Tasks Use page 119 and a periodic table to assist you. Draw a Magnesium Atom showing the arrangement of electrons. – How many electrons are in the outer shell? – What Group is Mg in? – How many electrons must it lose to have a full outer shell? Draw a Magnesium Ion showing the arrangement of electrons if it has a full outer shell. Draw an Oxygen Atom showing the arrangement of electrons. – How many electrons are in the outer shell? – What Group is O in? – How many electrons must it gain to have a full outer shell? Draw an Oxygen Ion showing the arrangement of electrons if it has a full outer shell. Why does magnesium want to bond with oxygen? What kind of bonding is this? Complete the following equation – Write in the correct words and symbols – Extension: Is it a balanced equation (page 148)? Magnesium + → Magnesium Oxide + O 2 → Complete summary questions 1 and 2 on page 119

What is the difference… Between Covalent and Ionic Bonding? CVALENT BONDINGBONDING INC

What is the difference… Between Covalent and Ionic Bonding? CVALENT BONDINGBONDING INC

Burning Mg Practical CAUTION: Do not look at the bright light! 1.Set up and light a bunsen burner safely. 2.Use the blue flame to ignite the Mg. 3.Carefully observe the reaction and the products. 4.Pack equipment away neatly. 5.Decide how best to record your observations. Any unsafe practice will result in remedial work at lunchtime

Homework Homework Homework Homework 2 Sodium chloride is an important compound in our diet. Research why humans need salt and what the damaging effects are if too much is consumed. (One paragraph in your own words)

Match up the keywords to the sentences. 1) A charged particle formed by an atom A) Element losing or gaining electrons. 2) All the atoms are the same.B) Ion 3) More than one type of atom chemically bonded together.C) Ionic bond 4) A chemical bond is formed as electrons are transferred. D) Compound Starter

Think back to yesterdays lesson Well done on the way that practical work was carried out. Why did you do the practical? What did you learn? What could you do different next time to make practical work more useful to you?

By the end of today: –You can describe ionic bonding as electrostatic forces of attraction. –Draw dot and cross diagrams (e.g. for MgO and CaCO 2 ). –You will be able to describe an ionic lattice. 1.4 Ionic Bonding

Ionic Bonding 1)Occurs between non metals and metals. 2)Involves the transferring of electrons. 3)The bond arises from the electrostatic attraction between the oppositely charged ions formed as a result from the electron transfer. 4)Elements in group 1 usually react with group 7 to form full outer shells. Copy this page

Ionic Bonding Using page 120 and 121 answer the following questions in full sentences. 1)What is a definition of an ionic bond? 2)What type of structure do ionic compound make? 3)Why do ionic compounds have high melting points?( think about forces of attraction) 4)Why do ionic compounds have a regular arrangement? 5)What other groups apart from 1 and 7 can form ionic compounds? 6)Draw an 3D ionic lattice of sodium chloride. 7)Draw a dot cross diagram for CaCl 2 and MgO.

By the end of today: –You can state a simple definition for a covalent bond. –Draw dot and cross diagrams for covalent bonds. –Explain their formation. –Explain the bonding in giant covalent structures and give named examples. 1.5 Covalent Bonding

Molymod This is a good way to visualise the structure of compounds. The number of holes is equivalent to the number of bonds that element makes. Work in a group of about 6. For the following write the molecular formula, structural formula and also draw a picture of the model you make. O 2, H 2 0, CH 4, NaCl, CO 2 and H 2 Once you have completed that try making some of the organic compounds on the other side of the sheet. C H O N S Cl Na

Each kit contains: C H O N S Cl Na x 12 x 20 x 6 x 4 x 2 x 4 x medium links and 12 long links

By the end of today: –You will be able to describe the bonding in metals. –List examples of giant metallic structures. –Some will be able to explain the structure and the delocalised electrons. 1.6 Bonding in Metals

Practical Work 1.Safety glasses on. 2.Collect a boiling tube, rack, copper wire and emery cloth. 3.Add silver nitrate to the tube (about half way up). 4.Clean the surface oxidation off the Cu with the emery cloth. 5.Add Cu to the solution and carefully record your observations with a few notes. 6.Explain your observation.

Metallic Bonding Ca