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Samenvatting Moleculen en Reactiviteit Termen RUG R88,67
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Samenvatting Moleculen en Reactiviteit Termen RUG

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Alle termen voor de hoofdstukken die je moet leren voor Moleculen en Reactiviteit mede hierdoor heb ik een 9 gehaald voor dit vak

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  • March 7, 2017
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1. Remembering general chemistry: electronic structure and bonding.
● Organic compounds​ are compounds that contain carbon.
● The​ atomic number ​of an atom is the number of protons in its nucleus (or the
number of electrons that surrounds the neutral atom).
● The​ mass number ​of an atom is the sum of its protons and neutrons.
● Isotopes​ have the same atomic number, but different mass numbers.
● Atomic weight​ is the average mass of the atoms in the element.
● Molecular weight​ is the sum of the atomic weights of all the atoms in the
molecule.An atomic orbital tells us the volume of space around the nucleus
where an electron is most llikely to be found.
● The closer the ​atomic orbital ​is to the nucleus, the lower is its energy.
● Minimum energy​ corresponds to maximum stability.
● Degenerate orbitals ​have the same energy.
● Electrons are assigned to orbitals (atomic or molecular) following the ​aufbau
principle​, the ​Pauli exclusion principle​, and ​Hund’s rule​.
● An atom is most stable if its outer shell is either filled or contains eight electrons,
and if it has no electrons of higher energy.
● The ​octet rule​ states that an atom will give up, accept, or share electrons in
order to fill its outer shell or attain an outer shell with eight electrons.
● Electronegative​ elements readily acquire electrons.
● The ​electronic configuration​ of an atom describes the atomic orbitals occupied
by the atom’s electrons.
● A ​proton​ is a positively charged hydrogen ion; a ​hydride ion​ is a negatively
charged hydrogen ion.
● Attractive forces between opposite charges are called ​electrostatic attractions​.
● An ​ionic bond​ results from the electrostatic attraction between ions with
opposite charges.
● A ​covalent bond​ is formed when two atoms share a pair of electrons.
● A ​polar covalent bond ​is a covalent bond between atoms with different
electronegativities​.
● The greater the difference in electronegativity between the atoms forming the
bond, the closer the bond is to the ionic end of the continuum.
● A polar covalent bond has a ​dipole ​(a positive end and a negative end),
measured by a ​dipole moment​.
● The ​dipole moment ​of a bond is equal to the​ size of the charge x the distance
between the charges​.
● The ​dipole moment ​of a molecule depends on the magnitude and direction of all
the bond dipole moments.

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