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.
● 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.
