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Samara Don
Ms Macpherson
Chemistry
Year 11 Chemistry Research Task
Introduction to the report
The aim of this report is to explore the fundamental properties of elements in the periodic table,
including atomic radius, electron configuration, first ionisation energy and electronegativity. Using
the periodic table we are able to collect data which allows us to identify and investigate the trends.
This data can be represented through graphs and diagrams which help us to draw conclusions on the
element's properties. These properties are important for understanding the behaviour of elements in
chemical reactions and the formation of chemical bonds.
Definitions of key terms -
(1) Electron configuration - Electron configuration is the arrangement of the electrons
around the nucleus of an atom. The representation of the configuration is shown
through many different models such as the Bohr and Schrödinger model which
feature electron orbital shells and subshells.
(2) Atomic radius - Atomic radius is a measure of an atom's size which is calculated
by the distance from its nucleus to the outer electron shell. It is measured to help
chemists understand why some molecules fit together and supports the conclusions
formed when investigating other properties.
(3) First Ionisation energy - First ionisation energy is the energy needed to remove
the outermost electron from an atom. This changes an atom to an ion. It is important
in understanding the behaviour of atoms in regards to covalent and ionic bonds.
(4) Electronegativity - Electronegativity measures an atom's ability to attract electrons
to itself. Understanding electronegativity is crucial for comprehending chemical
bonding.
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(5) Bohr model - This model is a way of visualising an atom's electrons and the
number of electrons in various shells. This model illustrates the atom as a central
nucleus which contains protons and neutrons with electrons surrounding the nucleus
in circular orbits.
(6) Schrödinger model/Spdf notation - It is an advanced way of describing electron
configuration. It is based on there being four types of orbitals, S, P, D and F in which
each orbital can hold two electrons. The s sublevel has one orbital, the p sublevel has
three orbitals which allows it to hold 6 electrons, the d sublevel has 5 orbitals which
allows it to hold 10 electrons and the f sublevel has 7 orbitals which allows it to hold
14 electrons. This model is very useful in understanding the behaviour of electrons.
(7) Electron affinity - Electron affinity is the amount of energy that is released when a
neutral atom attracts an electron to become an anion. A high electron affinity means
the atom more easily accepts electrons.
(8) Electron shielding effect - Electron shielding refers to the interrupted attraction
between the nucleus and valence electrons due to the presence of inner-shell
electrons.
Body of the report
Relationship between atomic radius and the element’s place on the periodic table
Samara Don
Ms Macpherson
Chemistry
Year 11 Chemistry Research Task
Introduction to the report
The aim of this report is to explore the fundamental properties of elements in the periodic table,
including atomic radius, electron configuration, first ionisation energy and electronegativity. Using
the periodic table we are able to collect data which allows us to identify and investigate the trends.
This data can be represented through graphs and diagrams which help us to draw conclusions on the
element's properties. These properties are important for understanding the behaviour of elements in
chemical reactions and the formation of chemical bonds.
Definitions of key terms -
(1) Electron configuration - Electron configuration is the arrangement of the electrons
around the nucleus of an atom. The representation of the configuration is shown
through many different models such as the Bohr and Schrödinger model which
feature electron orbital shells and subshells.
(2) Atomic radius - Atomic radius is a measure of an atom's size which is calculated
by the distance from its nucleus to the outer electron shell. It is measured to help
chemists understand why some molecules fit together and supports the conclusions
formed when investigating other properties.
(3) First Ionisation energy - First ionisation energy is the energy needed to remove
the outermost electron from an atom. This changes an atom to an ion. It is important
in understanding the behaviour of atoms in regards to covalent and ionic bonds.
(4) Electronegativity - Electronegativity measures an atom's ability to attract electrons
to itself. Understanding electronegativity is crucial for comprehending chemical
bonding.
, 2
(5) Bohr model - This model is a way of visualising an atom's electrons and the
number of electrons in various shells. This model illustrates the atom as a central
nucleus which contains protons and neutrons with electrons surrounding the nucleus
in circular orbits.
(6) Schrödinger model/Spdf notation - It is an advanced way of describing electron
configuration. It is based on there being four types of orbitals, S, P, D and F in which
each orbital can hold two electrons. The s sublevel has one orbital, the p sublevel has
three orbitals which allows it to hold 6 electrons, the d sublevel has 5 orbitals which
allows it to hold 10 electrons and the f sublevel has 7 orbitals which allows it to hold
14 electrons. This model is very useful in understanding the behaviour of electrons.
(7) Electron affinity - Electron affinity is the amount of energy that is released when a
neutral atom attracts an electron to become an anion. A high electron affinity means
the atom more easily accepts electrons.
(8) Electron shielding effect - Electron shielding refers to the interrupted attraction
between the nucleus and valence electrons due to the presence of inner-shell
electrons.
Body of the report
Relationship between atomic radius and the element’s place on the periodic table
