BTEC Certificate Applied Science

Summer Independent Learning Activity.

Btec Applied Science introduction.

• Within the Certificate Applied Science course students mustcomplete 3 units of work over a year.

• The summer introductory assignment will focus on Unit 1: Fundamentals of Science.

What criteria are we looking at?

• For the summer assessment there are three tasks you need tocomplete.

• This work will contribute towards the first pass tasks (P1) for Unit 1.

• For a pass criteria students must explain and describewhat is being asked.

Scenario

• You are working as a scientist for ‘Edvisprog’ – a company producing visual aids for education. You need to assemble a portfolio of scientific information to be passed to the graphic designer for preparation of a web-based programme to help the teaching and understanding of the use of titrations and the periodic table.

• For your first Pass task, you must outline the periodic table, the electronic structure of atoms and the bonding of atoms.

• This will take the form of an essay to include pictures and diagrams.

Task 1

• Include in your essay:

• A labeled diagram of the periodic table showing the following areas:

• The alkali metals.

• The earth metals.

• The transition metals.

• The Halogens.

• The noble gases.

Task 2:

• Describe how the following changes as you move across a period and down a group.

• Covalent radius

• Electronegativity

• Ionization energy

• Using this information describe how reactivity changes as you move down groups 1 and 2 and explain why.

Task 3:

• What is the atomic number of Carbon? Explain why Carbon has the atomic number.

• What is the relative atomic mass of Carbon? Explain why Carbon has this relative atomic mass.

• Explain how the number of Protons & Neutrons gives Carbon an Isotopic mass of 14.

• Explain what happens to the electrons in ionic bonding and show this as a diagram for sodium chloride and magnesium oxide. You must include the number of electrons lost and gained by each ion.

• Explain what happens to the electrons in covalent bonding. Show this as a diagram for methane and carbon dioxide. You must show the electron pairs and describe the molecular shape of both molecules.

• Draw Bohr atom diagrams for two different atoms of your choice. You must label the Protons, Neutrons & Electrons.

Btec Certificate Applied Science Resource. Summer Independent Learning Activity.

The periodic table contains information about the elements which make up all matter.

What are elements?

Pure substances which contain only 1 type of atom.The position of an element in the periodic table gives scientists information about the element and its reactivity.

The elements are arranged in PERIODS (rows) and GROUPS (columns).

The elements in each GROUP (column) have similar properties.

Use pages 5, 6 & 7 in link below to help you with task 2.

http://www.bbc.co.uk/education/guides/zxc99j6/revision/5

Atomic Structure

This a Bohr atomic model of an atom. It shows the position of the proton, neutrons in the nucleolus and the orbit of the electron in their shells

Use the link below to help you answer the questions in task 3BBC Bitesize - National 5 Chemistry - Structure of an atom

Subatomic Particles – Can you remember their charges?

Particle Location Charge

Protons Nucleus

Neutron Nucleus

Electron Orbiting the nucleus

Rubbish Chemistry Joke - A neutron walked into a bar and asked how much is a pint of lager? The bar man replied, for you, there will be no charge.

Positive +

Neutral

Negative -

Using the periodic table to find Atomic Number and Mass Number.Mass Number (the larger

number) tells us the combined number of protons and neutrons in the nucleus of an element.

Atomic number (the smaller number) tells us the number of protons in the nucleus (this is always the same as the number of electrons)

How many protons, neutrons and electrons does a sodium atom have? Isotopes – The number of protons and electrons making up the atoms of

an element are always the same (their charges must be balanced).

Sometimes the number of neutrons present in the atoms of an element can vary e.g. Carbon usually has 6 protons, 6 electrons & 6 neutrons but sometimes it can have 8 neutrons producing C14 a carbon isotope.

Use the link below to help you answer the questions in task 3.BBC Bitesize - National 5 Chemistry - The arrangement of electrons in the periodic table

Electron Shells

Electrons orbit the nucleus in shells.

Shell 1 can hold 2 electrons

Shell 2 can hold 8 electrons

Shell 3 can hold 8 electrons

When the third shell is full, the fourth shell starts to fill up.

e.g. Magnesium Atoms

The atomic number of Magnesium (Mg) is 12

Mg has 12 electrons so it’s electron arrangement is 2, 8, 2

Usually we use small crosses or dots to represent the arrangement of electrons in the electron shells of an atom.

Sodium (Na) has an atomic number of 11

On a whiteboard draw a diagram to show the arrangement of electrons in a Sodium atom.

Challenge

Which feature do the structures of atoms in each group of the periodic table have in common?

They all have the same number of electrons in their outer electron shell.

Forming Bonds

Every atom ‘wants’ to have a full outer

shell of electrons.

So atoms either lose electrons, gain

electrons or share them with other

atoms.

This is what causes all chemical

reactions.

BBC Bitesize - National 5 Chemistry - Ionic compounds and the periodic table

Use the link below to help you answer the questions in task 3.

Ionic BondsWhen metals bond with non-metals the metal atom gives one or more electrons to the non-metal.

Both atoms become charged particles called Ions.

Metal atoms lose electrons and form positively charged ions.

Non-metals gain electrons and become negatively charged ions.

When metals bond with non-metals the metal atom gives one or more electrons to the non-metal.

Both atoms become charged particles called Ions.

Metal atoms lose electrons and form positively charged ions.

Non-metals gain electrons and become negativelycharged ions.

He oppositely charged ions attract each other and the overall charge is cancelled out.

http://www.bbc.co.uk/education/clips/zx2r87h

1. How many electrons are there in the outer shell of Sodium atoms?

2. How many electrons are there in the outer shell of elements in group 7?

3. What charge will an atom have if it loses 1 electron?

4. What charge will an atom have if it gains 1 electron?

5. Which compound is formed when sodium and chlorine react?

6. Which types of elements can react to form ionic compounds?

How will these atoms form a

compound?

Li F

Li F

LI+

F-

How will the following ions form compounds?

1. Na+ and Cl- (NaCl) – Sodium Chloride

2. Mg2+ and O2- (MgO) – Magnesium Oxide

BBC Bitesize - National 5 Chemistry - Covalent bonding and the periodic table

Use the link below to help you

answer the questions in task 3

Covalent Bonds

Non-metal atoms bond with each other by COVALENT BONDS.

The atoms gain full outer electron shells by sharing electrons.

No Ions are formed.

One carbon atom can form bonds with 4 hydrogen atoms to produce 1 molecule of METHANE a simple HYDROCARBON which has a square or TETRAHEDRAL shape. Tetrahedral hydrocarbons form the basis of many organic compounds.

Covalent Bonding in Carbon Dioxide

One carbon atom can form bonds with 2 oxygen atoms to produce 1 molecule of Carbon dioxide (CO2) with a LINEAR shape.