Study Guide: Bonding Unit
Valence Electrons – Electrons that are
in the outer most shell of an atom. The
number of Valence Electrons is the
same as the column it is in on the
Periodic table, not exceeding eight.
Magnesium is in column 2, it has two
valence electrons. The Octet rule says
that all elements want to have eight
Valence Electrons.
Lewis Dot Diagrams – The element
with only its Valence Electrons drawn.
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∙O∙ Oxygen has six Valence Electrons
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Electron Configuration – How the
electrons are distributed around the
nucleus. There are four levels S, P, D
and F (table below). All of the
superscripts add up to the atomic
number.
Ca – 1s², 2s², 3s², 3p⁶, 4s². (Long
version)
Ca – [Ar] 4s². (Take the last Noble gas
and fill in the rest).
Polarity – When some atoms are
stronger than others, when they take
electrons. They would have that charge.
Take the electro negativity and subtract
the bigger form the smaller
0- 0.4covalent non polar
0.5 – 1.6 covalent polar
1.7 → ionic polar
Quantum Numbers – show you what the
atom would look like in all dimensions
of it. N represents the level, L is the
sublevel, M is the magnetic number and
S is the spin of the electrons (table
below). Every element has only ONE
set of quantum numbers.
N L M S
Li – 2 0 0 +½
Quantum Boxes - How to draw the
Electron Configuration. Each box holds
two electrons represented as arrows that
go up and down. It has to be drawn up,
up …of as many boxes and then you go
down, down….to fill them in.
Covalent Non-Polar Bonding –When two
identical non-metals EQUALLY SHARE
electrons to make the Octet rule.
Covalent Polar Bonding – When two
different non-metals UNEQUALLY
SHARE electrons, to make the Octet rule.
Ionic Bonds- The transfer of electrons
between a metal and a non-metal, a giveand-take effect, to give both the Octet
rules.
Hydrogen Bonds - When Hydrogen bonds
with a highly electronegative element;
mainly fluorine, oxygen and nitrogen.
Metallic Bonds – The bonding between
the electrons and the positive ions within
the atom.
Stephanie Edwards
Mr. Therrien Chem. 11ADV
Pauli Exclusion Principle – States that “no two
electrons in the same atom can have identical
value for all four of their quantum numbers”.
Aufbau Principle – A set of rules enabling the
construction of an electron structure of an atom
from its atomic number. Aufbau means
“building up”.
Hund’s Rule – States that when electrons are
placed in a set of orbital’s o equal energy they
are spread out as much as possible to give as
few paired electrons as possible
Intermolecular Forces – Forces of attraction
between neighboring molecules.
Intermolecular Forces – Forces of attracting
within molecules.
Van der Waals Forces – Attraction forces
including dipole-dipole, ion-dipole and
induced dipole forces.
London Forces – Weak attraction forces
caused by instantaneous dipole – induces
dipole attractions
VSPER (Valence Shell Electron Pair
Repulsion) says that electron pairs repel each
other; thus molecules must change their shape
so the pairs are as far away as possible. The
pairs repel each other around the central atom
in different ways because they repel all
electrons pairs; both shared and lone pairs.
They repel in this order:
Lone Pair – Lone Pair
Lone Pair – Shared Pair
Shared Pair – Shared Pairs