2. Overview of Types of Bonds
• Metal and Nonmetals = ionic bond= transfer of electrons
• Nonmetal and Nonmetal= covalent bond=sharing electrons
• Metal and Metal = metallic bond
3. ION BONDS LEQ’S & OBJECTIVES:
• What is an ionic bond and
how does it form?
• What are the properties of
ionic compounds?
• How are ionic formula units
written?
• How are ionic compounds
named?
• Use know and use the
identified vocabulary.
• Determine the number of
valance electron for an element
in the representative families
and the transition metal
identified.
• Apply the octet rule to an
element.
• Explain how ions form.
• Write the chemical formula
• Name binary compounds.
• Describe the properties of an
ionic compound.
4. Ionic Bonds
http://www.pbslearningmedia.org/asset/lsps07_int_ionicbonding/
Ionic bonds are formed from the electrostatic force between ________
with opposite _______________ that makes them “stick” together.
The ions are formed when one or more ______________ from one atom
are ___________ to another. The atom that loses an electron is a
____________ and has a ________________ charge. The atom that gains
an electron is a _______________ and has a ______________ charge.
5. How do you know what ions are
formed?
• Metals form _____________; Nonmetals
form_____________.
• The octet rule states: (p188)
_________________________________________
_________________________________________
______________
• Look at the diagrams of electron configuration change in
sodium (p 189) and oxygen (p192).
• For each representative group find the charge of the ion produced
6. Charges
• You must MEMORIZE the charges of the representative groups.
Group 1 = +1
Group 2 = +2
Group 13 = +3
Group 15 = -3
Group 16 = -2
Group 17 = -1
7. Polyvalant Metals
Most Transition Metals can have more than one
charge, polyvalent.
A few have only one cation, so MEMORIZE:
Zn +2
Ag +1
Cd +2
Otherwise you will be told the charge in the
name!
8. Why are they called formula units?
The ions are attracted to each other by
the electrostatic charges and form 3-D
shape called a ________________
The simplest ratio that ions combine in
is _____________________.
Give two examples:
9. Writing Formula Units
• Compounds have NO charge, so
Total Positive Charge = Total Negative Charge
Example: K+1 and S-2
Ca+2 and Cl-1
Cr+3 and Br-1
Fe+2 and O-2
Fe+3 and O-2
10. Names of Ions
(We will only learn the modern Stock names)
For metals in the group 1, 2 and the metals that only
have one cation, just say the name.
Al +3 = aluminum cation
For metals with more than one cation, the name is
followed by a Roman number giving the charge.
Fe+2 = Iron (II)= “iron two cation”
For nonmetals keep the stem of the element name and
add –ide.
Cl-1 = chloride anion
To Name a Compound: name the cation and the anion.
CuCl2 = Copper(II) Chloride
*Notice: the 2 in the name is NOT the number of ions
in the compound!
12. Practice Writing and Naming
Ba+2 and O-2
K+1 and S-2
Ca+2 and Cl-1
Fe+3 and Br-1
Cr+3 and O-2
13. And in Reverse
• Iron(II) Bromide
• Silver Chloride
• Potassium Oxide
• Copper (II) Telleride
14.
15. Polyatomic Ion
• A covalently bonded group of atoms that
has a charge and behaves as a unit.
• List on the back cover.
• Writing the formula unit is the same
process, but use ( ) around the group if you
have more than one.
16. Master List
• You have a list of ions that you will be able to use
on practice and tests but it is helpful to recognize
a few things:
Most polyatomic ions are anions; ammonium is the
exception.
Most do end in –ate or ite; the exception are
cyanide, peroxide, and hydroxide.
A family has the same charge; oxides of sulfur are -
2, oxides of nitrogen are -1.
25. What are covalent bonds
• A covalent bond is formed by _________
pairs of _____________. It is the stable
balance force of __________ between the
nucleus and the electrons and the force of
repulsion between the two _________.
• The __________ occurs at the point where
the potential energy is the lowest.
26. What are single, double and triple
bonds?
• A single bond results from _____________ 1
pair (2 electrons).
• A double bond results from sharing
_____________ pairs (4 electrons).
• A triple bond results from sharing 3 pair (
______ electrons).
27. What are the characteristics of
covalent compounds?
• Gases, liquids or solids made of
molecules.
•Low melting and boiling points
• Poor conductors in all phases
28. Naming
• The first element is given using its name
• The second element is name likes its anion
(with –ide)
• Prefixes are added to tell the number of
atoms present for each.
• Mono- is not used to name the first
element.
31. DoNow
• What naming system do you think will give
you the most problems? Why?
32. Polar Bonds and Molecules
• Nonpolar share the electrons equally
• Polar bond is a covalent bond where
the electrons are shared unequally
resulting in regions of charge.
• The difference in electronegativity
determines the bond type.
34. Naming Acids
• If hydrogen is with a strong nonmental : hydro______ic acid
• ex HCl: hydrochloric acid
• If hydrogen with polyatomic ending in -ate: _____ic acid
• Ex H2SO4 Sufuric acid
• If hydrogen with polyatomic ending in -ite: _____ous acid
• Ex H2SO3 Sufurous acid