Chemistry
description
Transcript of Chemistry
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The origin of chemistry can be traced to alchemy, or the art of converting metals like copper to
gold.
Chemistry
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Ionic Bonding
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Bonds
What is a chemical bond? Electrostatic forces of attractions (between 2 atoms)
between the nuclei of one atom and the electrons of the other atom.
Why do atoms bond?Three kinds of bonding:
Ionic Covalent Metallic
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Noble Gas
Also called the inert gases or rare gases: He, Ne, Ar, Kr, Xe and Rn.
Noble gases are unreactive.Exist as individual atoms, monatomic.Is there a need to bond?Are there noble gas compounds?
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Noble gas compounds
Examples: Xenon tetrafluoride (XeF4) Xenon tetroxide (XeO4) Krypton difluoride (KrF2) Radon difluoride (RnF2) Xenon trioxide (XeO2)
Notice what these compounds contain?
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Noble Gas Structure
Duplet or octet configurations are most stable.
Also known as a noble gas configuration.Common feature – fully filled valence
electron shell
He Ne
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Why atoms combine
Atoms WANT to achieve the noble gas configuration.
How do atoms achieve the noble gas structure? Transferring or sharing electrons.
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Recap – ions
Normally, an atom is electrically neutral number of protons = number of electrons
An ion is formed when an atom loses or gains electrons.
An ion is a charged particle formed from an atom or a group of atoms by the loss or gain of electrons.
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Cations
Positive ions (cations) are formed by removing/ losing electrons from atoms.
Loss of electrons tends to occur in atoms with few valence electrons (e.g. 1, 2 & 3)
Notice that these are METALS.
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Cations
Electronic configuration: 1s22s22p63s1 1s22s22p6
Na Na++ e-
Na atom Na+ ionNumber of protons
11 11
Number of electrons
11 10
Na Na + + e-
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Anions
Negative ions (cations) are formed by gaining electrons from atoms.
Gain of electrons tends to occur in atoms with larger number of valence electrons (e.g. 5, 6 & 7)
Notice that these are NON-METALS.
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Anions
Electronic configuration: 1s22s22p63s23p5 1s22s22p63s23p6
Cl + e- Cl-
Cl + e-
Cl atom Cl- ionNumber of protons
17 17
Number of electrons
17 18
Cl-
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Discuss
Consider sodium atom and sodium ion. Which do you think is bigger and why?
Na Na+
106 pm186 pm
Consider chlorine atom and chloride ion. Which do you think is bigger and why?
Cl-Cl
100 pm 181 pm
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Trends in radii
Atoms are always larger than any of their cations.
Atoms are always smaller than any of their anions.
http://chewtychem.wiki.hci.edu.sg/Ionic+Bonding
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Quickcheck
Is Mg+ or Mg2+ bigger?Is O- or O2- bigger?
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Ionic Bond
An ionic bond is a chemical bond formed by the electrostatic attraction between the positive and negative ions.
Formation of an ionic bond can be viewed as a transfer of electrons from a metallic atom to a non-metallic atom.
Both will gain a duplet or octet configuration.
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Video
Link to video
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Ionic bond
Na Na + + e-
Cl + e- Cl-
Two processes occuring:
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Na
Na1s22s22p63s1
Cl1s22s22p63s23p5
Cl
+
Na+
1s22s22p6
-
Cl-
1s22s22p63s23p6
Dot and Cross Diagram
Neon:1s22s22p6
Argon:1s22s22p63s23p6
Isoelectronic with
Isoelectronic with
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Dot and Cross Diagram
Cl-
Cl-
Mg2+
Al3+
O2-
2 3
Magnesium Chloride
Aluminium Oxide
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Is this possible?
Na + 7e- Na7-
Cl + 7e-Cl7+
1s22s22p63s1 1s22s22p63s23p6 (Ar)
1s22s22p63s23p5 1s22s22p6 (Ne)
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Chemical formulae
Take for example the following: An ionic compound made of Magnesium and
Fluorine.
Mg2+
F-
Mg2+
F-F-
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Chemical formulae
For Magnesium fluoride, the ions present are Mg2+ and F-.
Mg2+ has 2 positive chargesF- has 1 negative charge. To make the overall compound electrically
neutral there must be two F- to balance one Mg2+.
The formula is MgF2.
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Chemical formulae
Mg2+ F-
Mg1 F2 MgF2
Na+ OH-
Na1 OH1 NaOH
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Charge on ion Name of ion Formula+1 Sodium Na+
Potassium K+
Silver Ag+
Ammonium NH4+
Hydrogen H+
+2 Magnesium Mg2+
Calcium Ca2+
Iron(II) Fe2+
Zinc Zn2+
+3 Aluminium Al3+
Iron (III) Fe3+
-1 Chloride Cl-
Fluoride F-
Hydroxide OH-
Nitrate NO3-
-2 Carbonate CO32-
Oxide O2-
Sulfate SO42-
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Find the chemical formula
1. Magnesium oxide2. Zinc chloride3. Calcium hydroxide4. Iron(II) fluoride5. Iron(III) sulfate6. Ammonium nitrate7. Silver chloride8. Potassium iodide9. Manganese(IV) oxide
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General knowledge
General knowledge正离子 = cation负离子 = anion离子键 = ionic bonding共价键 = covalent bonding金属键 = metallic bondingNow you can hao4 lian4 to your friends!
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Ionic lattices
In ionic compounds, ions are held in fixed positions in an orderly arrangement by strong electrostatic forces (or ionic bonds) between the cations and anions.
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Attractions are maximised in this structure while repulsions are minimised.
How many Cl- surround one Na+ and vice versa?The coordination number is the number of nearest
neighbours (atoms, ions or molecules). What are the coordination numbers of Na+ and Cl-?
Ionic lattices
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Ionic Lattices
Different ionic lattice structures exist.http://www.avogadro.co.uk/structure/
chemstruc/ionic/g-ionic.htm
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Properties
High Melting and Boiling PointsHard and brittleConducts electricity when dissolved in water
or when moltenMany ionic compounds are soluble in water
or polar solvents like alcohol, but insoluble in most non-polar solvents like hexane
WHY?
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High Boiling and Melting Point
due to breaking of strong ionic
bonds
Conductor of electricity in liquid state and when in
solution due to presence of free moving charges.
Is brittle due to repulsion between similarly charged ions
Properties - NaCl
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Linus Pauling
Only person to have won two unshared Nobel Prizes (Chemistry and Peace)
The Nature of the Chemical Bond and the Structure of Molecules and Crystals
Pauling Electronegativity Scale
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Electronegativity
Every atom has an attraction for the electrons shared in a bond. Why?
Click this link for the electronegativity table.http://chemwiki.ucdavis.edu/@api/deki/files/4756/=electronegativity_chart.png
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Degree of attraction can be related to the electronegativity of the atom.
The higher the electronegativity, the more the electrons in a chemical bond are attracted to the atom.
Electronegativity
What patterns/ trends do you see?Metals generally have low electronegativity values, while non-metals have higher electronegativity values.Electronegativity values generally decrease down the group.Electronegativity generally increases across a period.
The high affinity for electrons of fluorine leads it to direct reactions with all other elements in which the reaction has been attempted, except for helium and neon.
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Predicting Ionic compounds
What do you notice about ionic compounds?What are they made up of?
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METALLIC BONDS
Metallic Bonding
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Metallic names
Ever wondered why some metals have weird symbols in the Periodic table?
E.g. Au (aurum) and Hg (hydrargyrum)Aurum actually means ‘shining dawn’.Hydragyrum means watery silver.
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Comparing Ionic and Metallic Bonding
Li Cl Li Li?+ -
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Metallic bonding (I)
Metals exist as giant structures too.In metals, atoms are packed closely together
in regular three-dimensional patterns to form a giant lattice.
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Metallic bonding (II)
Image originally created by IBM Corporation.
Platinum atoms
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Metallic bonding (III)
Li+
e
Li+ Li+
Li+ Li+ Li+
Li+ Li+ Li+
Li+
Li+
Li+
e e e
e e e e
e e e e
Mobile/ delocalised electrons.
‘Sea of electrons’ surrounding the positively charged metal cations.
Opposites attract i.e. every positive ion is attracted to the ‘sea of electrons’.
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Metallic bonding (III)
Forces of attraction between positively charged ions and negatively charged electrons – metallic bonding.
Only found in metals! Not ionic or covalent bonding!
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PROPERTIES OF METALS
Metallic Bonding
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Malleability and Ductility (I)
A malleable substance is one which can be bent or hammered out of shape without breaking.
A ductile substance is one which can be stretched or drawn into thin wires without breaking.
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Malleability and Ductility (II)
The following video shows the malleability of metals.
Metals can be forged into different shapes and sizes by beating and hammering
Especially useful in making tools and machines.
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Malleability and Ductility (III)
The following video shows the ductility of metals.
Notice that an iron strip can be twisted many times before it finally breaks.
Useful in making wires and cables.Why are metals malleable and ductile?
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Malleability and Ductility (IV)
Metal atoms are arranged in orderly layers.Application of a force causes metal atoms to
slide over each other easily. Why does the metal not break easily?Look at the following animation to
understand better.
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Malleability and Ductility (V)
What is this property useful for?
Malleability Ductility
Sculpting
Architecture Machinery
Tubing
Aircraft
Wire
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Melting and Boiling Points (I)
Metals generally have high melting and boiling points.
Most metals are packed closely together and the strong forces of attraction between the positively charged metal ions and the ‘sea of electrons’ result in strong metallic bonding.
A lot of energy is required to separate the metal atoms.
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Melting and Boiling Points (II)
Can you name some exceptions?Just for fun: The following metals might melt
at Singapore’s room temperature! Francium (27oC), Caesium (28oC) and Gallium (30oC).
Mercury
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Melting and Boiling Points (III)
What is this property useful for?
High melting point
Lights
Electrical appliances
Aircraft
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Electrical Conductivity (I)
‘Sea of electrons’ surround metal cations.Mobile or delocalised electrons in the metal
structure allows conduction of electricity.
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Electrical Conductivity (II)
Metals conduct electricity due to mobile delocalised electrons.
Can they conduct electricity in the molten state?
Can ionic compounds conduct electricity in the solid state?
Using electrical conductivity, how can we determine whether a substance is an ionic compound or metal?
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Electrical Conductivity (IV)
Sodium chloride
Iron
Solid Does not conduct electricity
Conducts electricity
Molten Conducts electricity
Conducts electricity
Aqueous Conducts electricity
-(Insoluble)
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Electrical Conductivity (V)
What is this property useful for?
Good conductor
of electricity
WiresElectrical appliances
Lightningrod
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Heat Conductivity (I)
Metals conduct heat well due to mobile delocalised electrons as well.
When you heat one end of a metal, delocalised electrons gain energy, move faster, and collide with neighbouring electrons, thus transferring heat from one end to the other.
Look at the following animation to observe what happens when metal is heated.
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Heat Conductivity (II)
Compare the movement of free electrons when a metal conducts heat and electricity. What are the differences?
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Heat Conductivity (III)
What is this property useful for?
Good conductor
of heatAircon
Heating coil
Refrigerator
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Metals as a whole
In general, metals… Reason(s)
Have high melting and boiling points.
Strong metallic bonding.
Are good conductors of electricity. Mobile/ delocalised electron that can carry electric charges.
Are good conductors of heat. Mobile/ delocalised electrons that collide and transfer heat.
Are malleable and ductile. Atoms arranged in orderly layers that can slide past one another.
Have high densities. For you to find out.
Are shiny in appearance. For those who are interested.
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Covalent Bonding
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Covalent Bonding
Consider the following (chlorine):We know that chlorine is often written as Cl2.Is this possible?
Cl-
Cl-
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Covalent Bonding
Covalent Bonding is the mutual electrostatic attraction between the nuclei of atoms and their shared electrons.
Normally occurs between 2 non-metals only.For example, when two Hydrogen atoms meet, they
will each share one electron to get a duplet configuration.
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Covalent Bonding
Let’s take a look at Hydrogen.As two H atoms approach, the electron on each
atom is attracted to the nucleus of the other, i.e. there are forces of attraction (between what?).
What happens if they are too close?Because of repulsion between nuclei and
attractions between electrons and nuclei, there is a distance between the two atoms where the molecule is most stable. This distance is called the bond length.
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Lennard-Jones Potential
H H
Distance between two atoms
H H
Bond lengt
h
http://upload.wikimedia.org/wikipedia/commons/5/5a/12-6-Lennard-Jones-Potential.png
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Covalent Bonding
Bond length or bond distance is the average distance between nuclei of two bonded atoms in a molecule.
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Covalent Bonding
Now take a look at two chlorine atoms. How do they share electrons?
Cl Cl
How many electrons are there around each chlorine atom now?
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Covalent bonding
Covalent bonds exist for compounds too.What about the water molecule?
O H
H
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Covalent bonding
How many electrons does an oxygen atom require?
O O
In this case, oxygen requires 2 electrons each. They can achieve the noble gas configuration by sharing 2 electrons each. The resulting bond is a double bond.
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Nitrogen
Try drawing the covalent molecule, nitrogen.
N N
In this case, nitrogen requires 3 electrons each. They can achieve the noble gas configuration by sharing 3 electrons each. The resulting bond is a triple bond.
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Try these!
NH3
CO2
SiCl4
CH3I
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Structural Formula
Molecule Chemical Formula Structural Formula
Hydrogen H2 H – H
Oxygen O2 O = O
Nitrogen N2 N N
Water H2O H – O – H
Methane CH4
H – C – H H
H
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Polyatomic ions
O- N+O
O-
Nitrate (NO3-)
O- CO
O-
Carbonate (CO32-)
SO
O-
Sulfate (SO42-)
O
O-
O- H
Hydroxide (OH-)
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Sigma Bonds
Head-on overlap of orbitals (s, p or d-orbitals)The resultant electron cloud is called a sigma
bondStrongest kind of covalent bond
1s 1s
H atom H atomH2
molecule
pp
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Pi bond
Side-on overlap of orbitals (p or d orbitals)Weaker than sigma bond because of less
overlap.
Can a molecule with only single bonds have pi bonds? E.g. Cl2?
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Sigma bond vs Pi bond
Pi bonds can only form after a sigma bond is formed.
Sigma bonds can be found in all covalent compounds.
Pi bonds are only found in double bonds or triple bonds.
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Identify the bonds in the given molecules
C C
H
HH
H
F F
O O
N N
C CH H
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Hydrogen
Let’s take a look at the hydrogen molecule.
H H = 2.1 =
2.1
Each H atom has the same attraction for the shared electrons .
Thus the electron density is evenly distributed over the whole molecule.
The molecule is said to be non-polar.
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Hydrogen chloride
Now consider the hydrogen chloride molecule.
H Cl = 2.1 =
3.0
Chlorine is much more electronegative than hydrogen, hence, it attracts the bonding pair of electrons more strongly.
Thus the electron density of the bond in HCl is pulled towards the Cl end of the molecule.
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Hydrogen chloride
Now consider the hydrogen chloride molecule.
H Cl = 2.1 =
3.0
This results in a separation of charge.The molecule is said to be polar and the
bond is a polar covalent bond.The molecule is said to have a permanent
dipole moment.
+ -
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Polar bonds
What happens if one atom is very much more electronegative than the other?
+ -
+ -
If one atom is very much more electronegative than the other, it pulls away the bonding electrons such that it becomes an ionic compound.
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Fluorine
Fluorine is so electronegative that it can bond to almost all atoms, even some noble gas atoms.
It does so because it has very strong attractions for electrons, such that even the electrons of noble gas compounds can be attracted by fluorine, thus forming a bond!
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Electronegativity and bond polarity
As a rule of thumb: If difference in electronegativity ranges from 0 to 0.5,
it is considered a non-polar covalent bond. If difference in electronegativity ranges from 0.6 to
1.6, it is considered a polar covalent bond. If difference in electronegativity is above 2.0, it is
considered an ionic bond. For 1.7 to 1.9, if a metal and non-metal is present, it is
considered ionic; if two non-metals are involved, it is considered polar covalent.
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Try these!
Predict whether the following are covalent or ionic. sodium bromide hydrogen fluoride aluminium oxide aluminium chloride beryllium chloride caesium fluoride
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Overall dipole
Vector sum of all dipole moments on the molecule
OHH
-
+ +
Individual dipoleOverall dipole
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Polar or non-polar?
Not all molecules with a polar bond has a dipole!
For example, carbon dioxide.
O=C=O+ -
Cancel each other
-
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Try these!
Predict whether the following are polar molecules. NH3
H2S CO CH4
CH3Cl
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Bond strength
The strength of the covalent bond between atoms is known as the bond strength.
The higher the bond strength, the more energy is required to break the bond.
Which molecule has the highest bond strength, nitrogen, oxygen or hydrogen?
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Bond strength
一根竹竿容易弯,一把筷子难折断Strengthtriple bond>Strengthdouble bond>Strength
single bond
What is the relationship between bond length and bond strength?
Bond Bond Length Bond EnergyC – C 154 pm 348 kJ/molC = C 134 pm 614 kJ/molC C 120 pm 839 kJ/mol
266 kJ/mol225 kJ/mol
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Bond strength
In general, the shorter the bond length, the greater the bond strength.
A number of factors affect bond strength. These include, number of bonds, size of atoms, electronegativity of atoms etc.
Bond Bond Length
Bond Energy
C – F 135 pm
488 kJ/mol
C – O 143 pm
360 kJ/mol
C – N 147 pm
308 kJ/mol
Across a period: Down a group:Bond Bond
Length
Bond Energy
C – F 135 pm
488 kJ/mol
C – Cl 177 pm
330 kJ/mol
C – Br 194 pm
288 kJ/mol
C – I 214 pm
216 kJ/mol
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Intermolecular Forces
So far the attractive forces we have covered hold atoms or ions together (intramolecular). What holds MOLECULES together (intermolecular)? van der Waals’ Forces hydrogen-bonding
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van der Waals’ forces
3 kinds Permanent dipole-permanent dipole Permanent dipole-induced dipole Instantaneous dipole-induced dipole
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Permanent dipole-permanent dipole
Consider the hydrochloride molecule
H Cl H Cl
+ - + -
If two HCl molecules approach each other, they will tend to arrange themselves such that the positive end of one molecule is close to the negative end of the other.
dipole-dipole attractions
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Permanent dipole-permanent dipole
Found in molecules with a permanent dipole moment i.e. a polar molecule.
Stronger the dipole moment, stronger the intermolecular force. Why?
Much weaker than a covalent bond.
H Cl H Cl
+ - + -
Weak dipole-dipole attractions(intermolecular)
Strong covalent bond
(intramolecular)
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Polar molecules
When exposed to an electric field, polar molecules align themselves to the positive and negative terminals
http://witcombe.sbc.edu/water/chemistrystructure.html
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Instantaneous dipole-induced dipole
What then holds non-polar molecules together?
Instantaneous dipole-induced dipole, also known as London dispersion forces.
Exists between ALL molecules and atoms.Only kind of intermolecular attraction
possible between non-polar molecules.
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Instantaneous dipole-induced dipole
Electron cloud distribution is symmetrical
Electron cloud distribution
becomes unsymmetrical for
an instant
Neighbouring electron cloud experiences an induced dipole
+- +- +-
NOTE: This kind of attraction is very short-lived because electrons are always moving and the dipoles will disappear very quickly!
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Instantaneous dipole-induced dipole
What does this London dispersion forces depend on? Number of electrons/ Electron cloud size Shape/ Surface area
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B.P. vs Number of electrons
0 10 20 30 40 50 60 70 80 90 100
-300
-250
-200
-150
-100
-50
0
Boiling point/ oC vs Number of electrons
Number of electrons
Boi
ling
poin
t/ o
C
He
Ne
Ar
Kr
Xe
Rn
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Helium
Has a boiling point of -268.93oC. Lowest among all elements!
Remains at a liquid even at -273.15oC (absolute zero)
Can only become a solid at 25 bar pressure at -272.2oC
Because of the weak van der Waals’ forces!
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Recap
3 kinds Permanent dipole-permanent dipole Permanent dipole-induced dipole Instantaneous dipole-induced dipole
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Recap
How does pd-pd and id-id work?Under what conditions does pd-pd happen?Does id-id work on only non-polar molecules?
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Instantaneous dipole-induced dipole
Instantaneous dipole-induced dipole becomes more important than permanent dipole-permanent dipole in determining the boiling point as the molecule or atom’s electron cloud increases.
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Topics
van der Waals’ in actionHydrogen-bondingProperties of Hydrogen-bonded moleculesHydrogen-bonding in real lifeProperties of simple covalent molecules(Properties of giant covalent structures)
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Geckos and Spiders
How do they stay on walls and even ceilings?Let’s take a look at this video.Then look at this website.
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Geckos
Geckos - Geckos have millions of setae--microscopic hairs on the bottom of their feet. These tiny setae are only as long as two diameters of a human hair. That's 100 millionth of a meter long. Each seta ends with 1,000 even tinier pads at the tip. These tips, called spatulae, are only 200 billionths of a meter wide-below the wavelength of visible light.
A single seta can lift the weight of an ant. A million setae, which could easily fit onto the area of a dime, could lift a 45-pound child. If a gecko used all of its setae at the same time, it could support 280 pounds.
Geckos cannot stick to teflon (non-stick coating on cooking pans). Go and find out why!
http://www.sciencedaily.com/releases/2002/08/020828063412.htm
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Spiders
On each of the spider's feet there are hair-like tufts, called scopulae, … it was discovered that a single scopula is itself composed of many, many, much smaller, single hairs… The number of setules per foot is estimated to be 78,000 each, and since spiders have eight feet, they have upwards of 600,000 individual points of contact with any given surface.
The total adhesive force is extremely powerful, up to 170 times the weight of the spider, if all eight legs are in contact.
http://www.istl.org/05-summer/article3.html
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Hmmm…
If scientists manage to come up with materials that are like a gecko’s legs…,
What uses can they be used for?What issues will crop up?
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Intermolecular
Are the only intermolecular forces van der Waals’?
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Group IV hydrogen compounds
CH4
SiH4
GeH4
SnH4
0 20 40 60 80 100 120 140
-190
-140
-90
-40
10
60
110
Group IV
Group IV
Molecular mass
Boi
ling
Poin
t/ o
C
CH4 has the lowest boiling point as it is the smallest molecule.
Larger molecules have greater number of electrons and thus, greater intermolecular forces. As a result, they have higher boiling points.
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Group V hydrogen compounds
NH3
PH3
AsH3
SbH3
0 20 40 60 80 100 120 140
-140
-90
-40
10
60
110
Group V
Group V
Molecular Mass
Boi
ling
poin
t/ o
C
NH3 is the smallest molecule and is expected to have the lowest boiling point. Some additional force must be present!
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Group VI hydrogen compounds
0 20 40 60 80 100 120 140
-70
-50
-30
-10
10
30
50
70
90
110
Group VI
Group VI
Molecular Mass
Boi
ling
poin
t/ o
C
H2O
H2S
H2Se
H2Te
H2O is the smallest molecule and is expected to have the lowest boiling point. Some additional force must be present!
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Group VII hydrogen compounds
HF
HCl
HBr
HI
0 20 40 60 80 100 120 140
-140
-90
-40
10
60
110
Group VII
Group VII
Molecular Mass
Boi
ling
poin
t/ o
C
HF is the smallest molecule and is expected to have the lowest boiling point. Some additional force must be present!
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Hydrogen compounds
0 20 40 60 80 100 120 140
-190
-140
-90
-40
10
60
110
Hydrogen compounds
Group IVGroup VGroup VIGroup VII
Molecular mass
Boi
ling
Poin
t/ o
C
CH4
SiH4
GeH4
SnH4
NH3
PH3
AsH3
SbH3
H2O
H2SH2Se
H2TeHF
HCl HBr
HI
The additional forces existing between NH3, H2O and HF molecules are called hydrogen bonds.
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Hydrogen bonding
Hydrogen bonding occurs only when molecules contain an H atom covalently bonded to a very small, highly electronegative atom with lone pairs of electrons, i.e. F, O and H.
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How H-bonding works
When H is covalently bonded to an extremely electronegative atom, F, O or N, the electronegative atom will attract the electron cloud strongly, leaving the H nucleus almost bare.
Thus when another molecule containing an F, O or N with lone pair of electrons approaches, it can get very close to the H atom, thus the intermolecular force is much stronger.
This accounts for the high boiling points of water, ammonia and hydrogen fluoride.
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Conditions for H-bonding
The H-atom must be covalently bonded to either N, O or F, the 3 most electronegative elements.
There must be a lone pair on N, O or F of the neighbouring molecule which can attract the partial positive charge on the H-atom.
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Hydrogen bonding
HO
H
HO
H
HO
H
HO
HH
O H
HO
H
Strong (intramolecular
) covalent bonds
Weaker (intermolecular
) Hydrogen bonds
Why must it be hydrogen???
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Strength of H-bonds
Strength of H bonds: H – F > H – O > H – N Why does water have a much higher boiling
point than HF when HF forms stronger H-bonds?
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Hydrogen Bonding in water
Why does ice float on water?When most substances freeze, the particles
are closer to one another as they are in the solid state as compared to the liquid state.
Water, however, has maximum density at 4oC. Recall that density = mass/volume. When water cools down from 4oC to 0oC, the formation of solid ice actually forces the water molecules to be fixed in a tetrahedral shape.
Click here for animation.
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Hydrogen Bonding in water
Similarly when ice melts, the solid structure actually collapses, so that the water molecules are closer together. They are closest at the temperature of 4oC. Why is this important for freshwater fish in winter?
Ice (00C)Water (10C)Water (20C)
Water (30C)Water (40C)
http://v.ku6.com/show/SXoq6mSJK2Ysgaga.html
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Solubility in water
Polar molecules are able to dissolve in water, which is a highly polar molecule, due to H-bonding.
C C
H
H
H
H
H
O H
Ethanol
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Solubility in water
Sugar (sucrose) is highly polar and can dissolve very well in water.
Carboxylic acids like ethanoic acid (vinegar) are able to form H-bonds as well in water.
C C
H
H
HO
OH
Sucrose Ethanoic acid
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Solubility in water
Some ionic compounds dissolve in water as well.
See animation.
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H-bonds in life
DNA (deoxyribonucleic acid) consists of two strands of polymers (very long molecules).
The 2 strands are held together by H-bonds.H-bonds can be broken by heating to high
temperatures.
http://en.wikipedia.org/wiki/File:DNA_chemical_structure.svghttp://en.wikipedia.org/wiki/File:DNA_orbit_animated_static_thumb.png
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H-bonds in Life
Proteins are made up of amino acids. Primary, secondary, tertiary and quaternary
structure. Secondary – alpha helix and beta-pleated
sheet.
Alpha Helix Beta-pleated Sheet
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Properties of covalent molecules
We have learnt that van der waals’ forces and hydrogen bonds hold molecules together. These forces are relatively weak as compared to covalent bonds.
What are the properties of such compounds?
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Melting point/boiling point
Simple covalent molecules have high volatility, i.e. they have low boiling point.
Note: No breaking of covalent bonds required!
Reasons for low melting/boiling point:- Strong covalent bonds within the molecules
but weak van der Waals’ forces between the molecules
- Little energy is required to overcome the weak intermolecular forces.
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Melting point/boiling point
In an iodine molecule, the two atoms are held by a strong covalent bond.
Weak van der Waals’ forces hold the iodine molecules together.
When heat is supplied, the weak intermolecular forces break and iodine sublimes.
Iodine molecule,
I2
Strong covalent bond
Weak van der Waals’ forces between molecules of iodine
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Solubility
Simple covalent molecules are generally insoluble in water or polar solvents UNLESS they are able to form hydrogen bonds or can dissociate (later).
Rule: “Like dissolves like.”For instance if you try to dissolve a non-polar
molecule like oil in water, water molecules will prefer to bond to water molecules (they have H-bonds) whereas the oil molecules will prefer clump together because energy is needed to break the H-bonds. Hence oil does not dissolve in water.
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Electrical conductivity
Simple covalent molecules do not conduct electricity.
Absence of free moving electrons/ ions.
N N
What about water?
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Electrical conductivity
Some simple covalent molecules (often acids or bases) when dissolved in water produce free moving ions in the solution which can conduct electricity. H Cl
H ClH+ Cl-
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Checklist – Covalent or not?
Iodine? Sand?Are they covalent?
Do they have similar physical properties?
Commonly formed between non-metals Form bonds by sharing electrons After bonding, each atom achieves noble
gas configuration
Note: Sand is made up mostly of silicon dioxide, SiO2 and is a main component of glass.
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Iodine vs GlassWhat do you think happens to glass (75% SiO2)?What about iodine?
Watch the Youtube Video on heating iodine in glass: http://www.youtube.com/watch?v=E-fs9OwE9Y0&NR=1
After gentle heating,- Physical form of glass remains intact.- Iodine sublimed (Solid → Gas)
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Classification of covalent substances
Covalent substances
Simple molecular structure
Giant covalent structure
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Structure of SiO2
SiO2 has a giant covalent structure.All the atoms are held
together by strong covalent bonds that extend throughout the structure.
No separate molecules (covalent bonds hold the atoms together, not van der Waals’ forces)
Si
O
Note: This structure is not really accurate. The O atoms are supposed to form a ‘V’ shape with the silicon instead of a straight line.
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Structure of SiO2
Each silicon atom is bonded to 4 oxygen atoms in a tetrahedral shape.
Each oxygen atom is in turn bonded to 2 silicon atoms.
Each tetrahedral is arranged in a repeating pattern extending in three dimensions.
Si
O
O
O
O
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Structure of SiO2
To melt this solid, a great deal of heat is required to break the covalent bonds
High melting point
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Discuss
What other physical properties does sand have, besides high melting point, and why?
- Electrical conductivity?- Brittleness?- Solubility? In water? In organic solvent?
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Carbon
Eight forms of elemental carbon: a) Diamond, b) Graphite, c) Lonsdaleite, d) C60 (Buckminsterfullerene or buckyball), e) C540, f) C70, g) Amorphous carbon, and h) single-walled carbon nanotube or buckytube.
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Diamond (from the ancient Greek αδάμας – adámas "unbreakable")
Allotrope of carbonGiant covalent
structureTetrahedral
arrangement: Each carbon atom is bonded tetrahedrally to four other carbon atoms
Strong covalent bonding in all directions
CC
C
C
C CC
C
C
C
CC
C
C
C
CC
C
C
C
Strong covalent bonds
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Diamond
CC
C
C
C CC
C
C
C
CC
C
C
C
CC
C
C
C
C C
C
C
C
See Simulation of Diamond: http://www.worldofmolecules.com/3D/graphite.htm
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Predict the properties of diamond
Melting point Extremely high melting point due to strong covalent bonds,
Carbon in all its allotropes has the highest melting point of all elements.
Hardness Hardest natural material due to strong covalent bonds, 10 on
the Mohs Scale of hardnessElectrical conductivity
Does not conduct electricity because all valence electrons are used up for bonding i.e. no delocalised electrons
Solubility Not soluble in polar or non-polar solvents due to very strong
covalent bonds.
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Some uses of diamond
Rock drillJewelryMemory??? Watch this video.http://www.lifegem.com/
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The carat
You have often heard about the carat in advertisements or movies. How much exactly is a carat?
1 carat = 200 mg
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carat vs carat
Is this the same as the carat used for gold?此 carat 非彼 caratFor gold, 24 carat is 100% carat.So for instance, 18 carat gold means it is
18/24 × 100% = 75% gold.
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Graphite
Another allotrope of carbon
Trigonal planar arrangement with respect to each carbon atom
Layers of carbon atoms
Each carbon covalently bonded to 3 other carbon atoms
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Graphite
Draw the dot-and-cross diagram of each carbon atom. What do you notice?
C CC
C
One extra valence electron!
CC
C C
One extra valence electron!
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Graphite
Layers of
carbon atoms
Side view
Weak van der Waals’
forces
The layers are held together by weak van der Waals’ forces.Within the layers, atoms are covalently bonded in repeating
pattern of hexagons (6-membered rings).See Simulation of Graphite: http://www.worldofmolecules.com/3D/graphite.htm
Pictures taken from: http://en.wikipedia.org/wiki/Graphite
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Properties
Hard or soft?Within the layers, bonded strongly by
covalent bonds.But between layers, weak van der Waals’
forces can be easily overcome upon stress.
Weak van der Waals’ forces
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Properties
Does it conduct electricity?YES! Remember the extra electron from the
dot-and-cross diagram? Presence of delocalised electrons which can
move along the layers in the presence of an electric current
Delocalised valence electrons
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Properties
Solubility?Melting/boiling point?Same as diamond.
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Uses of Graphite
As a lubricant for hot machinesPencil leadSome batteries
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Find out the uses of the following (Enrichment)
Carbon nanotubesGrapheneCarbon fibre
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Covalent SubstancesSimple molecular structure Giant covalent structure
Arrangement- Strong covalent bonds between the atoms within each molecule- Weak van der Waals’ forces/ H-bonds acting between the molecules
- Strong covalent bonds between the atoms- Consist of three-dimensional repeating patterns but no separate units.Examples: sand, diamond, graphite
Physical properties-Volatile, low melting & boiling point-Usually liquids or gases at room temperature-Insoluble in water (There are exceptions); Most are soluble in organic solvents.- Non-conductors of electricity
-Non-volatile, high melting & boiling point-Solids at room temperature-Insoluble in all solvents-Non-conductors of electricity (except graphite)
Examples: iodine, carbon dioxide, methane
Examples: sand, diamond, graphite