Ionic Bonding Notes Day 1 COMPLETE.notebook1
Feb 65:46 PM
1. To be stable, fluoride will gain an electron to
have the same configuration as
____________(a noble gas)
2. To be stable, calcium will lose two electrons
to have the same configuration as
____________(a noble gas)
Graded Opener: February 13th Write
Answers on a separate sheet and turn into the
bin up front
Feb 65:46 PM
Opener: February 13th
1. To be stable, fluoride will gain an electron to
have the same configuration as
____________(a noble gas)
2. To be stable, calcium will lose two electrons
to have the same configuration as
____________(a noble gas)
Neon
Argon
Unit 8 Calendar
Jan 199:52 PM
Objectives and Indicators 1.
Use a model to show how ions and ionic bonds are formed.
2.
Write electron configurations for ions in an ionic compound.
3.
Name and write formulas for ionic compounds.
•
H.C.3A.1: Construct explanations for the formation of molecular compounds via sharing of electrons
and for the formation of ionic compounds via transfer of electrons.
•
H.C.3A.2: Use the periodic table to write and interpret formulas and names of chemical compounds—
binary ionic compounds, binary covalent compounds, and straightchain alkanes up to six carbons).
•
IV.3.b: Explain ionic stability, recognize typical ionic configurations, and predict ionic configurations for
elements (e.g., electron configurations, Lewis dot models)
•
IV.3.c: Describe the nature of the chemical bond with respect to valence electrons in bonding atoms
•
IV.4.a: Use Lewis dot diagrams to represent bonding in ionic and covalent compounds
Jan 912:24 AM
Ion: Example = Ag+ and SO4
2 and S2
A charged atom or group of atoms charge is caused by a loss or
gain of valence electron(s)
Formula Unit: Example = MgCl2 and Na2CO3
The simplest unit of an ionic compound must contain a METAL and
a nonmetal or a metal and a polyatomic ion
Molecule: Example = CO2 and N2 and NH3 and PCl3
The simplest unit of a covalent compound contains ONLY
NONMETALS!
Jan 811:58 PM
CO2
molecule
2
NO2 1
MgCl2 formula unit
O2
Ag atom
Ag+1
PO4 3
3
Mg3(PO4)2
PCl3 molecule
Cl2 molecule
(diatomic molecule)
CP Chemistry 20142015
Unit 8: Chemical Bonding
CP Chemistry 20192020
Feb 65:52 PM
What are the two types of ions?
Why are they attracted to each other?
Jan 1910:25 PM
•
A chemical bond is a mutual electrical
attraction between the nuclei and
valence electrons (outer most) of different
atoms that binds the atoms together.
opposite charges will
attract just like a magnet
Ionic Bonding Notes Day 1 COMPLETE.notebook
4
H C C H
TED Ed Video Ionic vs Covalent
Jan 1910:31 PM
FLASHBACK... This will happen in the "s" and "p" sublevels with the
highest energy level (principal quantum number)
4s 4p
4s 4p
Bromine will gain an electron to satisfy the octet rule
ion
Feb 79:13 AM
Jan 1910:34 PM
Exceptions to the Octet Rule
1) Hydrogen has only one energy level only needs 2 electrons to
fill the 1s1 and look like Helium in noble gas configuration
(1s2)
2) Boron has only three valence electrons and can form hybrid
orbitals to share those electrons to form covalent bonds
3) Some elements with high electronegativity values can form with
an expanded valence using s, p, and d sublevels
B F
Jan 1910:42 PM
•
Ionic Bonding the chemical bond that results from the
electrical attraction between large numbers of cations (+),
anions (), and/or polyatomic ions.
Ca2+
(SO4)2- (NH4)+N3-
polyatomic ions are group of covalently bonded nonmetals that
usually gain (sometimes lose) electrons to fulfill the octet rule.
They have a charge and are treated as if it were a single
ion.
cations anions polyatomics
5
Jan 19:17 PM
Ionic Bonding •
Electrical attraction between cations with a positive charge and anions with a negative
charge •
Involves a metal and nonmetal ions or oppositely charged polyatomic ions
•
Metals form cations (lose valence electrons to form ions with a positive charge)
•
Nonmetals form anions (gain valence electrons to form ions with a negative charge)
•
Polyatomic ions are a group of bonded atoms that have either lost or gained electrons
to have an overall charge
Octet Rule: 8 is great for stability
•
Noble gases (Group 18) tend to be unreactive because they their outer s and p orbitals
are full (ns2p6 = 8 ve) •
Helium (He) is stable with 2 valence electrons (1s2)
•
Exceptions to the octet rule: hydrogen (H), lithium (Li), and beryllium (Be) à all stable
with 2 valence electrons •
Boron (B) is stable with 6 valence electrons
Jan 1911:04 PM
Lewis Dot structures show valence electrons only.
Jan 19:31 PM
Jan 19:20 PM
Jan 1911:06 PM
Example: Using Lewis Structures to show the formation of an ionic
bond
Mg and Br
magnesium bromide (MgBr2)
6
Ionic Bonding Notes Day 1 COMPLETE.notebook
7
Terms to Know
Molecule: a group of covalently bonded atoms (nonmetals)
Formula unit: simplest unit of an ionic compound (metal + nonmetal)
Ion: a charged particle
Polyatomic ion: a group of covalently bonded atoms that has an
overall charge.
Jan 2012:18 AM
1. Chlorate [ClO3] 1
•
Account for the charge on the ion
•
Divide the total # of valence electrons by 2. This is how many pairs needed.
• Draw the Lewis structure.
Jan 2011:09 PM
Carbonate [CO3] 2
Carbonate [CO3] 2
Jan 2011:12 PM
Find the Lewis Structure for Carbonate CO3
2 that you drew.
Does it matter where the double bond is drawn?
Ionic Bonding Notes Day 1 COMPLETE.notebook
8
Jan 2011:13 PM
Resonance
Sometime, there are molecules and ions whose structure is not
adequately described by one Lewis structure. Consider ozone:
We expect the = bond to be shorter than the bond
Where should the double bond go?
Equivalent Lewis structures are called resonant structures
The real molecule is a hybrid of the two resonance structures
Jan 2011:13 PM
Resonance
Analogy: Green paint
is made of both blue and yellow paint
green paint doesn't oscillate between blue and yellow it is an equal
blend of the two colors.
The electrons are not "locked" into place. The arrangement of
electrons is a blend of each resonant structure
Jan 2011:13 PM
Resonance
Resonance is a term used to describe Lewis structures that have a
double or triple bond that is not "locked" into place.
The electrons in those double and triple bonds are delocalized.
That means than can move throughout the molecule.
The double bonds in this molecule of benzene are NOT locked in place.
The electrons in the double bonds are delocalized.
Where else could the double bonds be drawn?
Jan 2011:15 PM
These are the RESONANCE STRUCTURES for CO3
2.
The MOST accurate diagram is the bottom one that shows the
delocalized electrons.
The double bond is NOT "locked" into 1 location in the molecule
Jan 2011:17 PM
Draw ALL possible resonance structures
for the nitrate ion (NO3
1).
Jan 2011:18 PM
Draw ALL possible resonance structures
for the nitrate ion (NO3
1).
Ionic Bonding Notes Day 1 COMPLETE.notebook
9
Tuesday, January 3rd: Opening Directions
•
Get a periodic table and one index card.
•
On the index card, write the following information on the LINED SIDE!
•
I am working on the online quiz for this week. We are going to use Quia
instead of Edmodo. I will give a you an individual password for Quia. If I
were you, I would take a picture of the password.
•
The online quiz will close FRIDAY at 11:59 p.m.
Jan 31:56 AM
What is the charge of an ion of A? +1
What is the charge of an ion of B? 2
What is the formula of A + B? A2B
What is the charge of the cation in CrO? Cr+2
What is the name of Mg(C2H3O2)2? magnesium acetate
What is the name of Fe3(PO4)2?
iron(II) phosphate
M is a metal that can form the following compounds:
MBr2, MO, and M(NO3)2
What is the charge of metal M? M+2
Jan 199:52 PM
Objectives and Indicators 1.
Use a model to show how ions and ionic bonds are formed.
2.
Write electron configurations for ions in an ionic compound.
3.
Name and write formulas for ionic compounds.
•
H.C.3A.1: Construct explanations for the formation of molecular compounds via sharing of electrons
and for the formation of ionic compounds via transfer of electrons.
•
H.C.3A.2: Use the periodic table to write and interpret formulas and names of chemical compounds—
binary ionic compounds, binary covalent compounds, and straightchain alkanes up to six carbons).
•
IV.3.b: Explain ionic stability, recognize typical ionic configurations, and predict ionic configurations for
elements (e.g., electron configurations, Lewis dot models)
•
IV.3.c: Describe the nature of the chemical bond with respect to valence electrons in bonding atoms
•
IV.4.a: Use Lewis dot diagrams to represent bonding in ionic and covalent compounds
Dec 149:44 AM
Chemistry Speed dating • 1 partner will get a set of flashcards •
There are 6 stations • If you don't have flashcards, you will
rotate around
the six stations (3-4 minutes at each) • Flashcards:
> Hold up the un-lined side of the card > If your partner
answers correctly, put that card
aside. If incorrect, show your partner the answer. > Write down
how many your partner gets correct,
and initial. (You may repeat for a better grade, if time)
Jan 32:05 AM
What is the formula of the
compound?
What is the electron configuration for a
sulfide ion?
Jan 1911:09 PM
A B+ A B+
10
A B+ A B+
A B+ A B+
What is the formula the bonding of A and E?
What is the formula the bonding of A and F?
What is the formula the bonding of A and G?
Jan 1911:15 PM
What is the formula the bonding of B and E?
What is the formula the bonding of C and G?
What is the formula the bonding of A and H?
Jan 1911:17 PM
Closing Questions: Exit Slip
1.
What is the general formula for an ionic compound formed
between an alkaline earth metal (X) and a halogen (Z)?
Show this using Lewis dot diagrams
2.
If X is a metal in group 2 and Z is a nonmetal in group 15,
what would the formula for the ionic compound formed
between them be?
Show this using Lewis dot diagrams
Jan 1911:18 PM
11