chapter 7 “ionic and metallic bonding” chemistry january 14, 2011
TRANSCRIPT
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Chapter 7
“Ionic and Metallic Bonding”
Chemistry
January 14, 2011
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Bellringer #55 (Jan 14th, 2011) Based on what you read for your
homework:
– What is the rule that atoms tend to follow when forming ions?
– How can you determine the number of valence electrons in an atom of a representative element?
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Agenda (Jan 14th, 2011) Answer Bellringer #55 Check Cornell notes 7.1 Write OBJECTIVES for section 7.1 Notes/Lecture 7.1 Answer “Pair to Pair” questions Hmwk: Section 7.1 assessment and 7.1
Wkst
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Section 7.1 - Ions
OBJECTIVES:
–Determine the number of valence electrons in an atom of a representative element.
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Section 7.1 - Ions
OBJECTIVES:
–Explain how the octet rule applies to atoms of metallic and nonmetallic elements.
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Section 7.1 - Ions
OBJECTIVES:
–Describe how cations form.
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Section 7.1 - Ions
OBJECTIVES:
–Explain how anions form.
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Valence Electrons are…? The electrons responsible for the
chemical properties of atoms, and are those in the outer energy level.
Valence electrons - The s and p electrons in the outer energy level
–the highest occupied energy level Core electrons – are those in the
energy levels below.
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Keeping Track of Electrons Atoms in the same column...
1) Have the same outer electron configuration.
2) Have the same valence electrons. The number of valence electrons are
easily determined. It is the group number for a representative element
Group 2A: Be, Mg, Ca, etc.
– have 2 valence electrons
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Pair to Pair Question #1 Determine how many valence electrons are in
the following atoms:– Rubidium (Rb)– Barium (Ba)– Aluminum (Al)– Fluorine (F)– Argon (Ar)– Helium (He)– Nitrogen (N)– Sulfur (S)
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Electron Dot diagrams are… A way of showing & keeping
track of valence electrons. How to write them? Write the symbol - it
represents the nucleus and inner (core) electrons
Put one dot for each valence electron (8 maximum)
They don’t pair up until they have to…..what rule does this sound like?
Hund’s Rule
X
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The Electron Dot diagram for Nitrogen
Nitrogen has 5 valence electrons to show.
First we write the symbol. NThen add 1 electron at a time to each side.Now they are forced to pair up.
We have now written the electron dot diagram for Nitrogen.
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The Octet Rule In Chapter 6, we learned that noble gases
are unreactive in chemical reactions The Octet Rule: in forming compounds,
atoms tend to achieve a noble gas configuration; 8 in the outer level is stable
Each noble gas has 8 electrons, except for one…..which one is it???????
Helium is an exception in Group 8A because it only has 2 electrons
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Pair to Pair Question #2 Draw the ELECTRON DOT DIAGRAM for the
following atoms:– Aluminum– Silicon– Nitrogen– Sulfur– Fluorine– Argon– Barium– Rubidium
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Formation of Cations Metals lose electrons to attain a noble
gas configuration. They make positive ions (cations) If we look at the electron configuration,
it makes sense to lose electrons: Na 1s22s22p63s1 1 valence electron Na1+ 1s22s22p6 This is a noble gas
configuration with 8 electrons in the outer level.
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Electron Dots For Cations Metals will have few valence electrons
(usually 3 or less); calcium has only 2 valence electrons
Ca
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Electron Dots For Cations Metals will have few valence electrons Metals will lose the valence electrons
Ca
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Electron Dots For Cations Metals will have few valence electrons Metals will lose the valence electrons Forming positive ions
Ca2+NO DOTS are now shown for the cation.
This is named the “calcium ion”.
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Electron Dots For CationsLet’s do Beryllium, #4The electron configuration is:
1s22s2
Thus, it can lose 2e- (making it 2+), to be like Helium
Be = Be2+ Beryllium ion
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Pair to Pair Question #3 Draw the ELECTRON DOT
STRUCTURES for the following CATIONS:
– Calcium (Ca)
– Sodium (Na)
– Gallium (Ga)
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Electron Configurations: Anions Nonmetals gain electrons to attain
noble gas configuration. They make negative ions (anions) S = 1s22s22p63s23p4 = 6 valence
electrons S2- = 1s22s22p63s23p6 = noble gas
configuration. Halide ions are ions from chlorine or
other halogens that gain electrons
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Electron Dots For Anions Nonmetals will have many valence
electrons (usually 5 or more) They will gain electrons to fill outer shell.
P 3-(This is called the “phosphide ion”, and should show dots)
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Electron Dots For AnionsLet’s do Chlorine, #17The electron configuration is:
1s22s22p63s23p5
Thus, it can gain 1e- (making it 1-), to be like Argon
Cl = Cl 1-
Chloride ion
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Pair to Pair Question #4 Draw ELECTRON DOT STRUCTURES
for the following ANIONS:
– Phosphorous (P)
– Bromine (Br)
– Sulfur (S)
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Stable Electron Configurations All atoms react to try and achieve a
noble gas configuration. Noble gases have 2 s and 6 p electrons. 8 valence electrons = already stable! This is the octet rule (8 in the outer level
is particularly stable).
Ar
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Bellringer #56 (Jan 18th, 2011) Write the ELECTRON DOT DIAGRAMS
of the NEUTRAL atom AND ION for the following elements:
– Bromine
– Boron
– Strontium
****each element should have TWO electron dot diagrams
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Agenda Objective: Review for Semester Exam Bellringer #56 Homework Check Results of Semester Exam: 1st attempt Semester Exam Study Guide Science Fair Make-Up Update Homework: Cornell Notes 7.2 Semester Exam 2nd Attempt: Tomorrow
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Bellringer #57 (Jan 20th, 2011) According to Section 7.2
– What is an IONIC COMPOUND?
– What are three properties of ionic compounds?
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Agenda (Jan 20th, 2011) Bellringer #57 Homework Check: 7.2 Cornell Notes Write Section 7.2 Objectives 7.2 Notes/Lecture Peer-to-Peer Questions (turn in at end
of class) Homework: 7.2 Section Assessment
(#14-22)
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Section 7.2 Ionic Bonds and Ionic Compounds
OBJECTIVES:
–Explain the electrical charge of an ionic compound.
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Section 7.2 Ionic Bonds and Ionic Compounds
OBJECTIVES:
–Describe three properties of ionic compounds.
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Ionic Compounds
1) Also called SALTS
2) Made from: a CATION with an ANION (or literally from a metal combining with a nonmetal)
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Ionic Bonding Anions and cations are held together
by opposite charges (+ and -) Ionic compounds are called salts. Simplest ratio of elements in an ionic
compound is called the formula unit. The bond is formed through the
transfer of electrons (lose and gain) Electrons are transferred to achieve
noble gas configuration.
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Ionic Bonding Example
Na ClThe metal (sodium) tends to lose its one electron from the outer level.
The nonmetal (chlorine) needs to gain one more to fill its outer level, and will accept the one electron that sodium is going to lose.
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Ionic Bonding Example
Na+ Cl -
Note: Remember that NO DOTS are now shown for the cation!
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Ionic Bonding Example
All the electrons must be accounted for, and each atom will have a noble gas configuration (which is stable).
Ca P
Lets do an example by combining calcium and phosphorus:
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Ionic Bonding
Ca P
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Ionic Bonding
Ca2+ P
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Ionic Bonding
Ca2+ P
Ca
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Ionic Bonding
Ca2+ P 3-
Ca
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Ionic Bonding
Ca2+ P 3-
Ca P
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Ionic Bonding
Ca2+ P 3-
Ca2+ P
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Ionic Bonding
Ca2+ P 3-
Ca2+ P
Ca
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Ionic Bonding
Ca2+ P 3-
Ca2+ P
Ca
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Ionic Bonding
Ca2+ P 3-
Ca2+P
3-
Ca2+
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Ionic Bonding
P3-Ca2+
Ca3P2
If you want to predict ionic bonding quickly…
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Ionic Bonding
= Ca3P2Formula Unit
This is a chemical formula, which shows the kinds and numbers of atoms in the smallest representative particle of the substance.
For an ionic compound, the smallest representative particle is called a: Formula Unit
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Ionic Bonding
Cl-Na+
NaCl
Another example… both have single charges
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Ionic Bonding
F-Mg2+
Mg F2
REMEMBERIf you want to predict ionic bonding quickly…
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Ionic Bonding
O2-Ti4+
Ti O2
But be careful! It can be like balancing a fraction!TiO2, not Ti2O4
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Peer-to-Peer Question #1 Draw the FORMULA UNIT for the
following atoms when they create an ionic bond:
– Mg and Cl
– Al and O
– K and Br
– Li and O
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Properties of Ionic Compounds1. Crystalline solids - a regular repeating
arrangement of ions in the solid: Fig. 7.9, page 197
– Ions are strongly bonded together.– Structure is rigid.
2. High melting points Coordination number- number of ions
of opposite charge surrounding it
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- Page 198
Coordination Numbers:
Both the sodium and chlorine have 6
Both the cesium and chlorine have 8
Each titanium has 6, and each oxygen has 3
NaCl
CsCl
TiO2
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Do they Conduct? Conducting electricity means allowing charges
to move. In a solid, the ions are locked in place. Ionic solids are insulators. When melted, the ions can move around.3. Melted ionic compounds conduct.
– NaCl: must get to about 800 ºC.– Dissolved in water, they also conduct (free
to move in aqueous solutions)– Ex: Salt water conducts electricity but
WATER alone does NOT
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- Page 198
The ions are free to move when they are molten (or in aqueous solution), and thus they are able to conduct the electric current.
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Bellringer #58 (Jan 21st, 2011) Determine the formula and name for
when the following atoms combine to create IONIC COMPOUNDS:
– Ca and O
– Al and S
– K and N
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Agenda (Jan 21st, 2011) Bellringer #58 Homework Check 2nd attempt distribution and discussion Review for Semester Exam Homework: Study Guide for EXTRA
CREDIT IF YOU PASS!!!!!!
– Extra study guide available on homework website…..VERY helpful!
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Bellringer #59 (Jan 24th, 2011) Determine the electron configuration for
the following atoms:
– Phosphorous
– Fluorine
– Calcium
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Bellringer #1 (Jan 31st, 2011) Name three things you know about ionic
compounds.
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Agenda (Jan 31st, 2011) Bellringer #1 Discuss new semester Objective: Learn how to name ionic
compounds from transition metal ions Work on Chapter 7 Section
Assessment: pg. 207 #30-47 Hmwk: Cornell Notes 7.3 Mini Quiz Tomorrow
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New Semester…..New Beginnings New Semester: Everyone starts all over again Starting at BR #1: Collecting BR #1-59
TOMORROW Late Work Policy: accept homework 1 DAY
LATE. Work MUST have a note on it as to WHY it is late and personally hand to Ms. Ingham.
Don’t wait too late to ask for help. This semester WILL BE harder than last.
Homework Board in back of room WILL BE updated.
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Cornell Notes Cornell Notes MUST include the following for
COMPLETE credit:– Answer KEY CONCEPT questions.– Define ALL vocabulary in the section AND
give a picture and/or example.– Write notes for EVERY RED heading in the
section.– All notes MUST end with a brief summary
discussing the main points of the section. (If you take good notes, this should not be hard to do.)
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Ionic Compounds With Transition Metals
The charges for transition metals are not as easy to predict as the metals from representative elements.– Ex: Copper can have a charge of 1+ or 2+
(Cu1+ or Cu2+) For this reason you MUST be given the
charge of the ion from a transition metal if you are going to create a ionic compound– Ex: Ti4+ and O
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Ion ExamplesSymbol Name
Cu+ Copper (I) ion
Cu2+ Copper (II) ion
Fe2+ Iron (II) ion
Fe3+ Iron (III) ion
Pb2+ Lead (II) ion
Pb4+ Lead (IV) ion
Sn2+ Tin (II) ion
Sn4+ Tin (IV) ion
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#1:Complete the table below (turn in at end of class).
Symbol Name
Cr2+
Chromium (III) ion
Mn2+
Manganese (III) ion
Cobalt (II) ion
Co3+
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Predicting Ionic Compounds and Charges of Transition Metals
What Copper ion would create CuO?
What Copper ion would create Cu2O?
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#2: Predict the ion that would create the compound below, then name the compound.
SnF2
SnS2
Fe2O3
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What Next? Turn in questions #1 and #2 Begin work on pg.207 (unfinished work
is homework along with Cornell notes) Mini Quiz Tomorrow Bellringers #1-59 due TOMORROW
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Bellringer #2 Write THREE things you know about
metals.
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Agenda (Feb 1st, 2011) Bellringer #2 Homework Check 1st Semester BR Collection Write 7.3 Objectives 7.3 Overview Mini Quiz Hmwk: 7.3 Section Assessment #23-29
and Writing Activity
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Section 7.3Bonding in Metals
OBJECTIVES:
–Model the valence electrons of metal atoms.
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Section 7.3Bonding in Metals
OBJECTIVES:
–Describe the arrangement of atoms in a metal.
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Section 7.3Bonding in Metals
OBJECTIVES:
–Explain the importance of alloys.
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Metallic Bonds are…How metal atoms are held
together in the solid.Metals hold on to their valence
electrons very weakly.Think of them as positive ions
(cations) floating in a sea of electrons: Fig. 7.12, p.201
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Sea of Electrons
+ + + ++ + + +
+ + + +
Electrons are free to move through the solid.
Metals conduct electricity.
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Metals are MalleableHammered into shape (bend).Also ductile - drawn into wires.Both malleability and ductility
explained in terms of the mobility of the valence electrons
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- Page 201
1) Ductility 2) Malleability
Due to the mobility of the valence electrons, metals have:
and
Notice that the ionic crystal breaks due to ion repulsion!
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Malleable
+ + + ++ + + +
+ + + +
Force
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Malleable
+ + + +
+ + + ++ + + +
Mobile electrons allow atoms to slide by, sort of like ball bearings in oil.
Force
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Ionic solids are brittle
+ - + -+- +-
+ - + -+- +-
Force
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Ionic solids are brittle
+ - + -
+- +-+ - + -
+- +-
Strong Repulsion breaks a crystal apart, due to similar ions being next to each other.
Force
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Crystalline structure of metal (pg. 202)
If made of one kind of atom, metals are among the simplest crystals; very compact & orderly
Note Fig. 7.14, p.202 for types:1. Body-centered cubic:
–every atom (except those on the surface) has 8 neighbors
–Na, K, Fe, Cr, W
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Crystalline structure of metal (pg.202)
2. Face-centered cubic:
–every atom has 12 neighbors
–Cu, Ag, Au, Al, Pb
3. Hexagonal close-packed
–every atom also has 12 neighbors
–different pattern due to hexagonal
–Mg, Zn, Cd
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Alloys We use lots of metals every day,
but few are pure metals Alloys are mixtures of 2 or more
elements, at least 1 is a metal made by melting a mixture of the
ingredients, then cooling Brass: an alloy of Cu and Zn Bronze: Cu and Sn
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Why use alloys? Properties are often superior to the pure
element Sterling silver (92.5% Ag, 7.5% Cu) is
harder and more durable than pure Ag, but still soft enough to make jewelry and tableware
Steels are very important alloys
– corrosion resistant, ductility, hardness, toughness, cost
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More about Alloys… Table 7.3, p.203 – lists a few alloys Types? a) substitutional alloy- the
atoms in the components are about the same size
b) interstitial alloy- the atomic sizes quite different; smaller atoms fit into the spaces between larger
“Amalgam”- dental use, contains Hg
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