CHEM1002 â Structure and Reactivity
CHEM1002 – Structure and Reactivity Notes taken from lectures and labs throughout the CHEM1002 course and compiled against the unit outcomes. At the end of the typed notes are hand drawn notes to allow better understandings of visual representations and mechanisms.
Table of Contents •
Electronic structure and periodic trends
1-3
•
Chemical Bonding
3-5
•
Molecular Geometry and Stereochemistry
5-7
•
Organic Chemistry
•
Biological Chemistry
•
The Chemistry of Transition Metals
7-14 14-16 16
CHEM1002 Learning Outcomes 1.
Electronic structure of atoms and the periodic properties of the elements •
Atomic Number = number of protons (z)
•
Periodic Table o
Elements with similar properties can be found in the same group (up and down). Periods go left to right
o
More metallic elements can be found closer to the bottom left of the table, the more metallic an element is, the more ionic it’s compounds are with non-metals and the more basic it’s oxides are.
o
The most powerful reducing agents can be found closer to the bottom left of the table. The most powerful oxidising agents can be found closer to the top right of the table
•
Atomic Radius: the covalent radius, when atoms are bonded together in a molecule. It is half the distance between the two nuclei o
In metals, the metallic radius is half the distance between adjacent nuclei in a crystal
o
Atomic size: larger atoms (less protons, more electrons) can be found closer to the bottom left of the table
o
Ionic Radius: the estimate based on the distance between cations and anions in a crystalline compound. Cations are smaller than their parent and anions are larger than their parent
•
•
Charge on monoatomic ions Group 1 2 13 14 15 16 17 Charge +1 +2 +3 +4/-4 -3 -2 -1 Ionization Energy: IE, is the minimum amount of energy required to eject an outer electron. Larger ionization energies can be found closer to the top right of the table (more protons to attract the neutrons)
•
Electronegativity: is the ability to attract the electrons from another atom, forming a molecule. The more electronegative elements can be found closest to fluorine (highest !)
•
Electron affinity: the enthalpy change associated with the removal of one electron to form an anion
•
Waves o
"
Wavelength, is the distance between each crest. $ = 2×( #
1
Table of Contents •
Electronic structure and periodic trends
1-3
•
Chemical Bonding
3-5
•
Molecular Geometry and Stereochemistry
5-7
•
Organic Chemistry
•
Biological Chemistry
•
The Chemistry of Transition Metals
7-14 14-16 16
CHEM1002 Learning Outcomes 1.
Electronic structure of atoms and the periodic properties of the elements •
Atomic Number = number of protons (z)
•
Periodic Table o
Elements with similar properties can be found in the same group (up and down). Periods go left to right
o
More metallic elements can be found closer to the bottom left of the table, the more metallic an element is, the more ionic it’s compounds are with non-metals and the more basic it’s oxides are.
o
The most powerful reducing agents can be found closer to the bottom left of the table. The most powerful oxidising agents can be found closer to the top right of the table
•
Atomic Radius: the covalent radius, when atoms are bonded together in a molecule. It is half the distance between the two nuclei o
In metals, the metallic radius is half the distance between adjacent nuclei in a crystal
o
Atomic size: larger atoms (less protons, more electrons) can be found closer to the bottom left of the table
o
Ionic Radius: the estimate based on the distance between cations and anions in a crystalline compound. Cations are smaller than their parent and anions are larger than their parent
•
•
Charge on monoatomic ions Group 1 2 13 14 15 16 17 Charge +1 +2 +3 +4/-4 -3 -2 -1 Ionization Energy: IE, is the minimum amount of energy required to eject an outer electron. Larger ionization energies can be found closer to the top right of the table (more protons to attract the neutrons)
•
Electronegativity: is the ability to attract the electrons from another atom, forming a molecule. The more electronegative elements can be found closest to fluorine (highest !)
•
Electron affinity: the enthalpy change associated with the removal of one electron to form an anion
•
Waves o
"
Wavelength, is the distance between each crest. $ = 2×( #
1
