NAMING AND WRITING CHEMICAL
COMPOUNDS
IUPAC BOHR DIAGRAMS FOR ATOMS TYPES OF CHEMICAL BONDS MOLECULAR COMPOUNDS
◦ TYPES SIMPLE COVALENT COMMON NAME
IONIC COMPOUNDS◦ SIMPLE IONIC◦ MULTIVALENT◦ POLYATOMIC/COMPLEX◦ HYDRATED IONIC
ACIDS
OUTLINE
International Union of Pure and Applied Chemists
This is a global organization that sets the standards in chemistry.
One job of the IUPAC is to give compounds SYSTEMIC NAMES.
IUPAC
Bohr diagrams, also called ENERGY LEVEL DIAGRAMS, are a means of drawing atoms in a 2-D manner.
Keep in mind that atoms are actually 3-D, and there are more complex representations of atoms.
Bohr models always include the NUCLEUS and the ELECTRON ENERGY LEVELS of an atom.
LINK
BOHR DIAGRAMS FOR ATOMS
There are 3 types of SUBATOMIC PARTICLES found in the atom:
PROTONS (p+)◦ Positively charged particles with a significant mass◦ Atomic Number = Number of Protons
ELECTRONS (e-)◦ Negatively charged particles with an insignificant mass◦ Number of Electrons = Number of Protons
NEUTRONS (no)◦ Neutral particles with a significant mass◦ Number of neutrons = Atomic Mass – Atomic Number
BOHR DIAGRAMS . . .
NUCLEUS◦Center of the atom, contains protons and
neutrons◦The atomic mass is concentrated here
ELECTRON ENERGY LEVELS◦Particular areas around the nucleus where
electrons are likely to be found◦Electrons DO NOT exist BETWEEN energy
levels◦ 3 LEVELS:
FIRST LEVEL (Closest to Nucleus) 2 e- SECOND LEVEL 8 e- THIRD LEVEL (Outermost) 8 e-
BOHR DIAGRAMS . . .
VALENCE LEVEL◦DEFINITION: Outermost energy level of an atom
◦Electrons in this level are called VALENCE ELECTRONS
◦Atoms with FULL valence shells are STABLE, meaning they will not bond with other atoms in normal conditions.
◦The atoms of Group 18, the Noble Gases, have full valence levels.
◦Atoms that do not have full electron energy levels are unstable and must GAIN, LOSE, or SHARE electrons to become stable.
BOHR DIAGRAMS . . .
ATOMIC NUMBER◦ Located in the top of each element box
on the periodic table.◦ ATOMIC NUMBER = # OF PROTONS
ATOMIC MASS (MOLAR MASS)◦ Located in the bottom of each element box on the
periodic table.◦ Round it off for calculations.◦ ATOMIC MASS = # OF PROTONS + # OF
NEUTRONS
BOHR DIAGRAMS . . .
EXAMPLE: DRAW BOHR DIAGRAMS FOR:
Li – lithium atom
◦ ATOMIC # = _____________◦ ATOMIC MASS = _____________◦ # p+ = ________________________◦ # e- = ________________________◦ # no = ________________________
BOHR DIAGRAMS . . .
EXAMPLE: DRAW BOHR DIAGRAMS FOR:
Ne – neon atom
◦ ATOMIC # = _____________◦ ATOMIC MASS = _____________◦ # p+ = ________________________◦ # e- = ________________________◦ # no = ________________________
BOHR DIAGRAMS . . .
EXAMPLE: DRAW BOHR DIAGRAMS FOR:
S – sulfur atom
◦ ATOMIC # = _____________◦ ATOMIC MASS = _____________◦ # p+ = ________________________◦ # e- = ________________________◦ # no = ________________________
BOHR DIAGRAMS . . .
Do worksheet in booklet on following page!!!
For complete answers be sure to do the following:◦ Write in the atomic number
and mass number.◦ Write the name of the atom in
the bottom of the square.◦ Include protons and neutrons
in the nucleus of the atom.◦ Write electrons in the energy
levels outside the nucleus.
HOMEWORK!!!
CHEMICAL BONDS◦DEFINITION: A force of attraction between atoms.
◦There are 2 TYPES of Chemical bonds Covalent Ionic
TYPES OF CHEMICAL BONDS
COVALENT BONDS◦AKA: molecular bonds◦“co” – together/sharing , “valent” – outer shell
◦DEFINITION: A SHARING of ELECTRONS between 2 atoms BETWEEN a two or more NONMETALS
◦Solutions of covalently bonded substances are NON-ELECTROLYTIC.
TYPES OF CHEMICAL BONDS
IONIC BOND◦DEFINITION: A TRANSFER of ELECTRONS between two atoms
BETWEEN a METAL and a NONMETAL◦Solutions of ionic bonded substances are ELECTROLYTIC.
COMPOUNDS consist of atoms or ions of two or more elements bonded together.
TYPES OF CHEMICAL BONDS
Forms when 2 or more NONMETALS share electrons in COVALENT BONDS.
2 TYPES:◦BINARY Molecular Compounds◦TRIVIAL NAME Molecular Compounds
MOLECULAR COMPOUNDS
Also called SIMPLE molecular compounds.
Binary Molecular Compounds use IUPAC prefixes:◦We will write these prefixes in the following
table.
BINARY MOLECULAR COMPOUNDS
Number Prefix1 mono2 di3 tri4 tetra5 penta6 hexa7 hepta8 octa9 nona
10 deca
RULES:
1. Write NAMES of elements, with the 2nd element ending in “-ide”.
2. Add PREFIXES to indicate HOW MANY ATOMS of each element.
3. Do NOT use the prefix “mono” for the 1st element, only with the 2nd element.
Given Molecular Formula, Write Name
N2O4________________________
P2O5 ________________________
CCl4 ________________________
Given Formula, Write Name EXAMPLE
RULES:
1. Write ELEMENT SYMBOLS for each element in the compound.
2. Use the PREFIX in the name to determine NUMBER OF ATOMS, and write that number as a SUBSCRIPT next to the symbol (no subscript for 1 atom).
GIVEN MOLECULAR NAME, WRITE FORMULA
carbon monoxide ____________
triphosphorus pentabromide ____________
sulfur hexafluoride ____________
Given Name, Write Formula EXAMPLE
Also called COMMON NAME molecular compounds.
There are SOME molecular compounds that go by their COMMON NAMES, and we must memorize these names.
TRIVIAL NAME Molecular Compounds
FORMULA TRIVIAL/COMMON NAMEO3 ozone
H2O waterH2O2 hydrogen peroxideNH3 ammoniaCH4 methane
CH3OH methanolC2H5OH ethanolC6H12O6 glucose
C12H22O11 sucrose
Complete the NEXT THREE SHEETS in your handout for HOMEWORK.
Refer to the following notes for help:
◦FIRST SHEET Given Name, Write Formula Notes
◦SECOND SHEET Given Formula, Write Name Notes
◦THIRD SHEET Everything! Watch out for those common name molecular compounds!!!
HOMEWORK ALERT!!!
IONS◦RECALL: AS mentioned earlier, atoms other than the
NOBLE GASES are unstable, and need to GAIN, LOSE, or SHARE ELECTRONS to become more stable.
If they SHARE electrons, this forms a COVALENT BOND to another atom.
If they LOSE or GAIN electrons, atoms become IONS and form IONIC BONDS with other atoms.
OCTET RULE◦Atoms that have an octet of valence electrons are STABLE and UNREACTIVE.
Ions are charged atoms that have lost or gained electrons to achieve the valence configurations of a noble gas.
TWO TYPES:◦CATIONS: POSITIVE ions that are formed from a LOSS of
electrons. It has more PROTONS than ELECTRONS and
therefore has a net POSITIVE charge. METALS form cations. MEMORY TOOL: t in “cation” resembles a “+” sign
EXAMPLE: lithium ion Li+ 1+ charge
WHAT IS AN ION?
◦ANIONS: NEGATIVE ions that are formed from a GAIN
of electrons. It has more ELECTRONS than PROTONS and
therefore has a net NEGATIVE charge. change the ending of the name of anions to -ide
NONMETALS form anions. MEMORY TOOL: A Negative ION EXAMPLE: fluoride ion F- 1- charge LINK
METALS◦ ATOMS of METALS will LOSE electrons to become CATIONS.◦ ATOMS with 1, 2, or 3 VALENCE electrons will LOSE these electrons to
form 1+, 2+, or 3+ ions respectively.
◦GROUP 1 ATOMS – ALKALI 1 valence electrons(s) (will lose 1 to become stable) 1 + ion
◦GROUP 2 ATOMS – ALKALINE EARTH 2 valence electrons(s) (will lose 2 to become stable) 2 + ion
◦GROUP 13 ATOMS 3 valence electrons(s) (will lose 3 to become stable) 3 + ion
BOHR DIAGRAMS FOR IONS
NONMETALS◦ ATOMS of NONMETALS will GAIN electrons to become ANIONS.◦ ATOMS with 5,6, or 7 VALENCE electrons will GAIN these electrons to form 3-, 2-, or 1- ions
respectively.
◦ GROUP 15 ATOMS 5 valence electrons(s) (will gain 3 to become stable) 3 - ion
◦ GROUP 16 ATOMS 6 valence electrons(s) (will gain 2 to become stable) 2 - ion
◦ GROUP 17 ATOMS - HALOGENS 7 valence electrons(s) (will gain 1 to become stable) 1 - ion
◦ GROUP 18 ATOMS - NOBLE GASES FULL outer valence levels
BOHR DIAGRAMS FOR IONS
Note that in BOHR DIAGRAMS for IONS, electron numbers have changed.
Here is a quick equation for calculating the number of electrons:
# e- = #p+ - charge
TO DRAW:
A sodium ATOM and a sodium ION
DRAW A BOHR DIAGRAM FOR:
A chlorine ATOM and a chloride ION
DRAW A BOHR DIAGRAM FOR:
Complete the next two worksheets in your booklet for homework!
Do a few examples of each page in class so that when you go home, you know what you are doing!!!
HOMEWORK!!!
Form when at least 1 METAL AND 1 NONMETAL transfer electrons in an IONIC BOND.
Metals will become CATIONS and LOSE electrons and nonmetals will become ANIONS and GAIN electrons.
These ions, with opposite charges, attract and form IONIC BONDS.
Unlike covalent bonds, these bonds are not “ACTUAL BONDS,” but forces of attraction between oppositely charged ions.
They stay together in a CRYSTAL LATTICE.
IONIC COMPOUNDS
Example: NaCl (Draw on your sheet)IONIC COMPOUNDS
Cl- Cl-
Cl-Cl-
Cl-Cl-
Cl-
Na+
Na+Na+Na+ Na+
Na+Na+
Cations are surrounded by anions and vice versaAlso refer to Figure 4, p. 189
Example: NaClIONIC COMPOUNDS
3 TYPES:◦Binary Ionic Compounds SIMPLE MULTIVALENT
◦Polyatomic Ionic Compounds
◦Hydrated Ionic Compounds
IONIC COMPOUNDS
“Binary” Only 2 types of ions involved.
SIMPLE IONIC COMPOUNDS◦ Simple ionic compounds are composed of a metal ion (+)
and a nonmetal ion(-).
GIVEN FORMULA, WRITE NAME◦ RULES:
1. Write the name of the CATION before the ANION (Be positive before being negative )
2. Change the ending of the ANION name to “-ide”3. Do not use CAPITALS, Do not use PREFIXES!
BINARY IONIC COMPOUNDS
EXAMPLE:◦MgBr2 _________________________________◦KCl _________________________________◦Na2S _________________________________◦Mg3P2 _________________________________◦Ba3N2 _________________________________
WHAT’S WRONG WITH THE FOLLOWING NAMES FOR BaS?◦barium sulfur ____________________________◦Barium Sulfide ____________________________◦barium sulfuride
____________________________
SIMPLE IONIC COMPOUNDS
Do the following sheet in the booklet for homework:
Follow rules for:◦“GIVEN FORMULA, WRITE NAME” for Ionic
Compounds.
HOMEWORK!
GIVEN NAME, WRITE FORMULA◦RULES:1. Write element symbols.2. Look up the ION CHARGE on the
periodic table.3. Use the “crossover” method to
determine the numbers of each ion in the compound.
4. Ion ratios are always in the lowest common multiple.
5. Ion charges must add up to “zero” overall.
SIMPLE IONIC COMPOUNDS
EXAMPLE: sodium bromide _____________________
barium iodide ___________________
SIMPLE IONIC COMPOUNDS
EXAMPLE: magnesium oxide _____________________
aluminum oxide ___________________
SIMPLE IONIC COMPOUNDS
Do the next two sheets for homework!
FIRST PAGE:◦Given NAME, Write FORMULA
SECOND PAGE:◦TOP HALF – Molecular
Compound Naming◦BOTTOM HALF – Ionic
Compound Naming
HOMEWORK!!!