Download Naming Covalently Bonded Molecules

Gifted Chemistry – Week 13
Monday
Chrome Book Activity
Tuesday
Student Presentations: Covalent Bonds;
Notes & Guided Practice: Covalent Nomenclature
Wednesday Lab: Naming Covalent Molecules
Thursday
Quiz: Ionic & Covalent Formulas & Nomenclature;
Notes: Lewis Dot Structures for Covalent
Molecules
Friday
Begin Test Review (Test on Tuesday)
Two Quia due on Sunday at 11:59 pm
Week 13: 8-1 and 8-2 & Week 13: Mixed Review
Most Missed Quia – Week 12
Write the formula for the ionic compound
created from
aluminum and carbonate
Al2(CO3)3
Most Missed Quia – Week 12
Write the formula for the ionic compound
created from
calcium and chlorate
Ca(ClO3)2
Most Missed Quia – Week 12
Name this compound: Be(ClO2)2
Beryllium Dichlorite
Beryllium(II) Chloride
beryllium(II) chlorite
beryllium chlorite
Ionic Bonds
• Transferring electrons from one atom
to another in order to complete an octet
of valence electrons
• Groups 1 and 2 lose electrons…become
positive cations
• Chalogens and Halogens gain
electrons…become negative anions
• Metal + nonmetal  salt
• Metal + oxygen  oxide
Ionic Bonds
• Formula Writing
– Balance charges
– Use parentheses, when necessary
Calcium hydroxide
Ca(OH)2
Lithium iodate
LiIO3
Ionic Bonds
• Formula Writing
– Balance charges
– Use parentheses, when necessary
Ammonium sulfate
potassium carbonate
(NH4)2SO4
K2CO3
Ionic Bonds –
Which one is correct?
(Ca) OH2
Ca (OH)2
(NH4)3PO4
NH12PO4
(Fe+2)2(PO3)3
(Fe+2)3(PO3)2
Ionic Bonds
• Compound Naming
– Cations first; anions second
– Use roman numerals for transition metals
Fe(NO2)3
iron (III) nitrite
Sn(CO3)2
tin (IV) carbonate
Properties of Ionic Compounds
• Ionic bonds produce unique physical
structures
• Atoms are highly organized with consistent
spacing and a uniform pattern
• Crystal lattice – a 3D arrangement of particles
Properties of Ionic Compounds
1. Conductivity
Ionic solids do not conduct electricity.
Melted ionic solids or ionic solids dissolved in
a solution will conduct electricity
(electrolytes).
Properties of Ionic Compounds
2. High melting points and high boiling points.
Ionic bonds are very strong and require a lot
of energy to break apart.
Ionic Bonds and Energy
Formation of ionic bonds is always exothermic.
Lattice energy – energy required to separate the
ions in an ionic compound
Smaller ions have greater lattice energies.
Larger charges also have greater lattice energies.
1
Naming Covalently Bonded
Molecules
A binary covalent compound is composed of two
different nonmetal elements. There are four rules
on naming these molecules.
Rule 1. The element with the lower group number
is written first in the name; the element with the
higher group number is written second in the name.
Exception: when the compound contains oxygen
and a halogen, the name of the halogen is the
first word in the name.
Naming Covalently Bonded
Molecules
Rule 2. If both elements are in the same group, the
element with the higher period number is written
first in the name.
Rule 3. The second element in the name is named as
if it were an anion, i.e., by adding the suffix -ide to
the name of the element.
Naming Covalently Bonded
Molecules
Rule 4. Greek prefixes are used to indicate the
number of atoms of each nonmetal element in the
chemical formula for the compound.
Prefix
Meaning
Prefix
Meaning
Mono-
1
Hexa-
6
di-
2
Hepta-
7
tri-
3
Octa-
8
Tetra-
4
Nona-
9
Penta-
5
Deca-
10
Naming Covalently Bonded
Molecules
Practice:
1)
2)
3)
4)
5)
SbCl3
S2Cl2
BF3
P4O6
Se4S10
6)
7)
8)
9)
10)
phosphorus trichloride
selenium tetrafluoride
carbon tetrabromide
sulfur trioxide
tetraphosphorus
hexaoxide
Covalent Bond Review
Covalent bond – chemical bond that occurs
when valence electrons are shared, not
transferred
Molecule – product of a covalent bond
Usually occurs between nonmetals and
elements that are close to each other on the
periodic table
Covalent Bond Nomenclature
Lab
Use your
device to
download a
free dice
rolling app
11 Undeca
12 Dodeca
Lewis Dot Structure
CH4
Lewis Dot Structure
NH3
1) chlorine monoxide
2) oxygen difluoride
3) boron monophosphide
4) dinitrogen monoxide
5) nitrogen trifluoride
6) sulfur tetrachloride
7) xenon trioxide
8) carbon dioxide
9) diphosphorous pentoxide
Diatomic Molecules
Two atoms of the same element share electrons
in order to form a stable molecule
Seven naturally occurring diatomic molecules
H2 O2 F2 Br2 I2 N2 Cl2
“Hof Brincl”
Diatomic Molecules
Diatomic Molecules
More stable
than single H
atoms due to
full shell
Diatomic Molecules
• When only one pair of electrons is shared, it is
a single covalent bond.
Single Bonds
• Draw the Lewis Dot Structure for Water
H2O
Single Bonds
• Draw the Lewis Dot Structure for Ammonia
NH3
Single Bonds
• Draw the Lewis Dot Structure for Methane
CH4
Single Bonds
• Draw the Lewis Dot Structure for Methane
CH4
Double Bonds
Double Bonds
• Draw the Lewis Dot Structure for
carbon dioxide
CO2
Triple Bonds
Triple Bonds
• Draw the Lewis Dot Structure for
acetylene
C2H2
Dot and Mixed Nomenclature
Quiz Review:
Dot and Mixed Nomenclature
Quiz Review:
Dot and Mixed Nomenclature
Quiz Review:
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