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Chemical Bonding: The force that holds two atoms
together is called a chemical bond. This bond may be
formed many different ways but for now we will only
discuss two types of bonds, ionic and covalent. An
element’s properties and behavior depends on their
valence electrons. These outer electrons are also
responsible for how atoms bond to another.
Formation of Positive Ions: Groups 1, 2, and 13
will lose electrons to achieve stable octets. This
process is favourable because it requires far less
energy than gaining multiple electrons.
Formation of Negative Ions: Group 15, 16, and
17 have greater attraction to electrons and thus try
to gain more electrons to get a stable octet.
Polyatomic Ions: A group of atoms that
have a charge. For example, OH(hydroxide).
Naming with Only One Type of Atom:
To name anything with only one type of atom just
use the name that appears on the periodic table of
elements. However, there are some exceptions to
this rule.
1. There are 7 diatomic elements which include H2,
N2, O2, F2, Cl2, Br2, and I2. These elements are
found in nature bonded to each other. These still
use the names given in the periodic table.
2. Monatomic cations use the element name followed by
the word ion.
Ex. Cs+ is named cesium ion.
3. Monatomic Anions take their name from the root of
the element plus the “ide” suffix. Can also be found on
your reference sheet.
Ex. Br- is named bromide ion.
4. Phosphorous is found in nature in a group of 4 (P4)
but is still named phosphorous.
Practice- Name the following Atoms:
Li
Br2
Tc
Ca 2+
P4
Rn
S2Titanium
Sodium ion
Phosphide ion
When we name elements we name them
based on the type of bond they form.
Ionic Bonding-ionic bonds are formed
between ions with opposite charges.
Chemical bonds between metals and nonmetals.
Covalent Bonding- chemical bonds between
non-metals and non-metals. Atoms share
electrons.
Ionic Bonds: These bonds are formed when ions are
joined due to electrostatic attraction. Typically a
metal and a non-metal form ionic bonds. For
example, sodium transfers an electron to chlorine gas
and forms sodium chloride. If an ionic bond occurs
between a metal and oxygen it is an oxide (Fe2O3).
Most other ionic bonds are salts.
Naming Binary Ionic Compounds (Nonmetal and metal):
FORMULA
1. Write the symbol of the metal or positive
ion first.
2. Write the symbol of the negative ion.
Common negative ions and nonmentals
are listed on your reference sheet.
3. Overall charge must equal 0. Aluminum
chloride is written as AlCl3 not AlCl.
Al3+
ClO2IN3-
Mn4+ Co3+
Cu2+
Pb4+
FORMULA TO NAME
1. Write the name of the positive ion followed by the
name of the negative ion.
Ex. MgO is named magnesium oxide, Na2S is named
sodium sulfide.
NaOH is named sodium hydroxide
2. Common negative ions and nonmentals are listed
on your reference sheet. Take these names as they
are! DO NOT change them.
Ex. Fluorine becomes fluoride and bromine becomes
bromide.
3. Many transition metals on the periodic table have
more than one possible charge, and therefore when we
look at an ionic compound that contains a multivalent
metal, we need to be able to identify the charge of the
metal ion. If the metal forms more than one type of
cation, the charge has to be indicated using roman
numerals.
Roman Numerals
One (I)
Five (V)
Two (II)
Six (VI)
Three (III)
Seven (VII)
Four (IV)
Eight (VIII)
Ex. Fe2+ becomes Fe (II) and Fe3+ becomes
Fe (III).
If we have a formula of FeCl2 which of the
following would be the correct name?
iron (II) chloride
OR iron (III) chloride
Practice – Name the
following ionic compounds:
NaCl:
AlBr3:
NiO:
PdI4:
PbCl2:
Name to Formula
1. Write the name of the cation. Use the roman
numerals to predict the charge of each atom.
Remember, the Roman numeral is used to help
identify the charge of the atoms.
2. Write the name of the anion as shown on your
reference sheet.
Practice – Write the formula of the following ionic
compounds:
Sodium oxide:
Potassium chloride:
Scandium nitride:
Cobalt (III) sulfide:
Naming Ionic Bonds with a
Polyatomic Ion:
Formula to Name:
1. If the polyatomic compound is the cation then use
the name found on your reference sheet
Ex. Ammonium (NH4+)
2. If the polyatomic compound is the anion find the
name on your reference sheet. Use that name and
do not change the ending. When using an ion there
must be brackets around the entire ion if there is
more than one of that ion.
Ex. Magnesium cyanate is written as Mg(OCN)2
NOT as MgOCN2
Ex. ClO3- (chlorate)
3. Again, the charges must equal 0. If they do not
you must balance them. Remember, the
polyatomic ion is a compound hooked together
which means you must use brackets around the
term to balance it.
Ex. Magnesium nitrate is written as Mg(NO3)2
Al3+
H30+
SCN- Al(SCN)3 H3OSCN
NH4+
Co3+
Cu2+
Pb4+
NH4SCN
Co(SCN)3 Cu(SCN)2 Pb(SCN)4
SO42- Al2(SO4)3 (H3O)2SO4 (NH4)2SCN Co2(SO4)3 CuSO4
Pb(SO4)2
PO42- Al2(PO4)3 (H3O)2PO4 (NH4)2PO4 Co2(PO4)3 CuPO4
Pb(PO4)2
S2O32- Al2(S2O3)3 (H3O)2S2O3 (NH4)2S2O3 Co2(S2O3)3 CuS2O3
Pb(S2O3)2
Practice – Name the following ionic bonds
with polyatomic ions:
NaC2H3O2: sodium acetate
H2O2: hydrogen peroxide
K2HPO4: potassium hydrogen phosphate
Pt(CrO4)2: platinum (IV) chromate
Ca(BrO2)2: calcium bromite
NaOH: sodium hydroxide
H3OBr: hydronium bromide
Name to Formula:
1. Write the name of the cation. Use the roman numerals
to predict the charge of each atom. Remember, the
Roman numeral is used to help identify the charge of the
atoms.
2. Write the name of the anion as shown on your
reference sheet. Remember to include bracket when
balancing charges.
Practice – Write the formula of the following ionic compounds:
Sodium dihydrogen phosphate:
Cesium permanganate:
Ammonium sulfide:
Zinc thiocynate:
Covalent Bonds:
The second type of bond is a covalent bond. These
bonds occur when both atoms need electrons to get to a
stable octet. Instead of transferring electrons they share
them. These usually occur with a non-metal and a nonmetal. For example, F has an electron configuration of
1s22s22p5 which means it has 7 valence electrons and
must gain one more to achieve a full octet. It achieves
this by sharing with another fluorine atom to form F2.
It is important to note that some compounds require
more than one covalent bond to achieve an octet, like N2
or O2. Because these compounds share electrons NO
CHARGES are associated with each atom in the
compound.
Naming Covalent Compounds (Non-metal and Nonmetal):
Formula to Name:
1. The element farthest to the left of the periodic table is
named first. If they are in the same column then the one
with the most protons is named first.
2. Add the appropriate prefix to the front name (unless
the prefix is mono-). This is used to indicate the number
of atoms in each compound. Mono- is not used if there is
only one atom of the first element.
Ex. CO2 is named carbon dioxide NOT monocarbon
dioxide (mono is not used on the first element)
B3Br is name triboron monobromide (mono is used on
the second one)
**Prefixes found on reference sheet.
3. The second uses a prefix and add an “ide” to the
ending of the name.
Ex. Tetrachloride
Practice – Name the following covalent compounds:
CO3:
SF6:
CO:
As2O3:
IF5:
N2O4:
Name to Formula:
Use the rules above in order to predict
the formula:
Dichlorine monoxide:
Silicon dioxide:
Dicarbon trioxide:
Carbon monofluoride:
Pentanitrogen trioxide:
Heptacarbon trinitride:
Octaoxygen dinitride:
Formulas with a ●H2O
These are compounds that have water molecules
bonded to them to create a more stable structure.
The stable structure may be required to ship the
compound from place to place safely.
1. Use the previous rules to name the compound.
2. Attach ●H2O (named hydrate) to the end of the
compound with the appropriate prefix to indicate the
number of water molecules.
Ex. NaNO3●3H2O is named sodium nitrate trihydrate
Pb(NO3)2 ●5H2O is named lead(II) nitrate
pentahydrate
Practice – Name the following compounds
containing hydrates:
CaCl2●6H2O:
Co(NO3)2●6H2O:
Cu(NO3)2●3H2O:
Practice – Use the same rules to predict the
formula:
Ammonium sulfide heptahydrate:
Iron (II) silicate pentahydrate:
Lead (IV) nitrate octahydrate:
Copper (II) chloride trihydrate:
Gold (III) hydride pentahydrate:
Naming Binary Acids (Hydrogen and 1 Other
Element):
To name the compound first determine the
ending of the root element:
Rule #1 –If the anion’s name ends with “-ide”:
•Add the prefix “hydro –.”
•Replace the “-ide” ending with “-ic”.
•Follow the name with the word acid.
Rule #2 –If the anion’s name ends with “-ite”:
•Replace the “-ite” ending with “-ous”.
•Follow the name with the word acid.
Rule #3 –If the anion’s name ends with “-ate”:
•Replace the “-ate” ending with “-ic”.
•Follow the name with the word acid.
Ex. HBr is named
HIO3 is named
HCrO3 is named
HCl is named
HCN is name
Practice – Name the following binary acids:
HIO3:
HF:
H3PO3:
H2CO3:
H2Cr2O7:
H2Se:
Give the formula of the following acids:
Nitrous acid:
Hyrdoselenic acid:
hydrosulfuric acid:
Chromic acid:
Selenous acid:
Hydrocarbons
Naming Hydrocarbons:
Hydrocarbons are compounds which are composed of
hydrogen and carbon units. The majority of hydrocarbons
are found in crude oils in which organic matter has
decomposed to form these compounds.
1. Alkanes
•All alkanes have a formula of CnH2n+2
•All alkanes end with 'ane‘
•See the prefixes listed on your reference sheet.