BTEC applied science UNIT 1 exam revision- PRINCIPLES AND APPLICATIONS OF SCIENCE I
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Course
Unit 1 - Principles and Applications of Science I
Institution
PEARSON (PEARSON)
This document is a revision pack full of notes, questions and answers from the unit 1 exam. I received a distinction grade in this exam last year so these notes and hard work and revision will guarantee you a distinction in the exam, GOOD LUCK!
BTEC APPLIED SCIENCE - Unit 1 EXAM NOTES - Pearson
BTEC SCIENCE UNIT 1 REVISION: CHEMISTRY:
Define electron configuration:
It can be defined as the distrubution of electrons in an atom or molecule.
Ionic Bonding:
This occurs when an atom of an element loses one or more electrons and donates it to another atom
of a different element. The atom that loses electrons become postively charged and the atoms that
gains electrons becomes negatively charged due to the imbalance of protons and electrons.
To make a more simplified defintion, it is an electrostatic attraction between two oppositely charged
ions.
Define electrostatic attraction:
It is the force that has been experienced by oppositely charged particles which holds the particles
strongly.
Define giant ionic lattice:
It is shown as the regular arrangement of positive ions and negative ions.
Covalent Bonding:
This occurs between atoms of two non - metals where it forms when an electron is shared between
the atoms. These electrons come from the top energy level of the atoms.
To make a more simplified defintion it is called a molecular bond, is a chemical bond that involves
the sharing of electron pairs between atoms.
, Define lone pair:
It is defined as a non - binding pair of electrons.
Define organic compound:
It is shown as a compound that contains one or more carbons in a carbon chain.
Metal Properties:
- High melting points
- Malleable: It can be hammered into shape without breaking.
- Ductile: It can be hammered thin or stretched into wires without breaking.
- Electrical/Thermal conductors
- Solids at room temperature
Metallic Bonding:
Metallic bonding is caused because electrons in the highest energy level of the metal atom has the
ability in order to become delocalised and this demonstrates that they free to move around through
the metal under a 'sea' of electrons which gives the metal nuclei a postive charge which is attracted
to the negative charge on the delocalised electrons allowing it to have a strong force of attraction.
Metallic bonding is not as strong in covalent or ionic bonding.
Define delocalised:
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