BTEC Certificate Applied
Science
Summer Independent Learning Activity.
Btec Applied Science introduction.
• Within the Certificate Applied Science course students
must
complete 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 to
complete.
• This work will contribute towards the first pass tasks (P1)
for Unit 1.
• For a pass criteria students must explain and describe
what 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/educatio
n/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 3
BBC Bitesize - National 5 Chemistry - Structure of an
atom
Subatomic Particles – Can you remember
their charges?
Particle
Protons
Location
Nucleus
Charge
Positive +
Neutron Nucleus
Neutral
Electron Orbiting
the
nucleus
Negative -
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.
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.
How many protons,
neutrons and electrons
does a sodium atom have?
Atomic number (the smaller
number) tells us the number of
protons in the nucleus (this is
always the same as the
number of electrons)
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.
Use the link below to help you
answer the questions in task 3
.
BBC Bitesize - National 5
Chemistry - Ionic compounds
and the periodic table
Ionic Bonds
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 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 negatively
charged 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?
Li
F
How will these atoms form a
compound?
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
Use the link below to help you
BBC Bitesize - National
answer the questions in task 3
5 Chemistry - Covalent
bonding and the
periodic table
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.