Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Lesson 1:Review of Periodic Table Structure
Thursday, October 2, 2014
IB Understandings
 The periodic table is arranged into four blocks associated with the four
sublevels – s, p, d and f
 The periodic table consists of groups (vertical columns) and periods
(horizontal columns)
 The period number (n) is the outer energy level that is occupied by electrons
 The number of the principal energy level and the number of the valence
electrons in an atom can be deduced from its position on the periodic table
 The periodic table shows the positions of metals, non-metals and metalloids
Applications and skills:
 Deduction of the electron configuration of an atom from the element’s
position on the periodic table, and vice versa.
Guidance:
 The terms alkali metals, halogens, noble gases, transition metals, lanthanoids
and actinoids should be known.
 The group numbering scheme from group 1 to group 18, as recommended by
IUPAC, should be used.
Periodic Table Development:
Dobreiner’s
Triads
Newlands
Octaves
Mendeleev
1
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Elements show gradual changes in certain physical properties as one moves across
a period or down a group in the periodic table. These properties repeat after certain
intervals. In other words they are ____________________________.
Periodic properties include:
1.
2.
3.
4.
5.
Elements are arranged by increasing __________________________________________________.
Groups
Periods
Group Number
Name
Characteristics
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
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Metals
Metalloids
Non-Metals
3
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Lesson 2: Periodic Trends
Friday, October 3, 2014
IB Understandings
 Vertical and horizontal trends in the Periodic Table exist for atomic radius,
ionic radius, ionization energy, electron affinity, and electronegativity.
Guidance
 Only examples of general trends across periods and down groups are
required. For ionization energy the discontinuities in the increase across a
period should be covered.
o Trends in metallic and non-metallic behaviour are due to the trends
above.
o Oxides change from basic through amphoteric to acidic across a
period.
Applications and skills:
 Prediction and explanation of the metallic and non-metallic behaviour of an
element based on its position in the Periodic Table.
4
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
 Discussion of the similarities and differences in the properties of elements in
the same group, with reference to alkali metals (Group 1) and halogens
(Group 17).
Guidance
 Group trends should include the treatment of the reactions of alkali metals
with water, alkali metals with halogens and halogens with halide ions.
 Construction of equations to explain the pH changes for reactions of Na2O,
MgO, P4O10, and the oxides of nitrogen and sulfur with water.
Periodicity:
Effective Nuclear
Charge
Atomic Radius
5
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Ionic Radius
Describe and explain the trend in radii of the following atoms
and ions: O2–, F–, Ne, Na+, and Mg2+.
Ionization
Energy
Electron Affinity
6
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Electronegativity
Melting Points
Metals vs. Non-Metals:
7
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Let’s Practice
1 (a) Explain what is meant by the atomic radius of an element.
(b) The atomic radii of the elements are found in Table 9 of the IB data booklet.
(i) Explain why no values for ionic radii are given for the noble gases.
(ii) Describe and explain the trend in atomic radii across the Period 3
elements.
2 Si4+ has an ionic radius of 4.2 × 10–11 m and Si4– has an ionic radius of 2.71 × 10–10
m. Explain the large difference in size between the Si4+ and Si4– ions.
8
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
10
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Lesson 3: Practice!
Remember when studying that the group of an element on the Periodic Table also
tells you the number of valence electrons for that element!
Electron Shielding Effect:
Atomic Radius:


We typically measure atomic radius at ____________________________________________
where we look at atoms in chemical bonds with other atoms of the same
element and take ½ the diameter between the two nuclei
There is also ________________________________________________________________________
or _____________________________________________________________ radius for things like
Noble Gases that do not bond; take a look at these atoms in the solid phase
and measure the distance between two nuclei
11
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Which ion would have a larger ionic radius, Na+ or Mg2+?
Melting Points

Comparing melting points is complex because it depends on bonding as well
as nuclear charge
 Trends down Groups 1 through 17 can be explained as elements in each
group bond in the same way!
 Melting points ___________________________________down Group 1 as these metallic
bonds have delocalized electrons and as you move down the group the
attraction decreases
 Melting points _________________________________ down Group 17 because these
diatomic elements are held together by London Dispersion forces which get
stronger as the electron cloud gets bigger
 Melting points generally rise from left to right until Group 14 and then fall
from Group 14 to Group 18
Lesson 4: More Trends
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Warm-Up:
Why does I2 have a higher melting point than F2?
Why does aluminum have a higher melting point than sodium?
Metals:
 Metallic properties are related to ionization energy; the lower the ionization
energy, the more metallic an element is
 A metallic structure consists of a regular lattice of positive ions in a
_______________________________________________________________________________________
 Metallic character ___________________________ from left to right and
________________________________ from top to bottom
1.
2.
3.
4.
5.
Mercury:
Non-Metals:
1.
2.
Metalloids:
1.
Alkali Metals
13
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Physical Properties
Chemical Properties
Reactions
Group 1 Reactions with Water
Lithium
Sodium
Potassium
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Francium
Cesium
Group 17 – Halogens
Physical Properties
Chemical Properties
Reactions
Salts:
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Displacement Reactions with Water
Silver + Halides
Group 18 – Noble Gases
1.
2.
3.
1. Why are alkali metals called alkali?
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
2. How are halides formed?
3. Why does Cl- displace Br- in a displacement reaction?
4. How do the reactivities of the alkali metals and the halogens vary down a
group?
5. Which property of the halogens increases from fluorine to iodine?
A.
ionic charge
B.
electronegativity
C.
melting point of the element
D.
chemical reactivity with metals
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Lesson 5: Oxides and pH Trends
Warm-Up: Explain why each trend occurs below in terms of effective nuclear
charge.
Oxides:
pH of Oxides:
 Metal oxides are basic; they react with water to form metal hydroxides
CaO(s) + H2O(l)  Ca(OH)2(aq)
 Non-metallic oxides are acidic: they react with water to form acidic solutions
CO2(g) + H2O(l)  H2CO3(aq) Carbonic Acid
 If an oxide can act both as an acid and a base, it is classified as
amphoteric!
Al2O3(s) + 2NaOH(aq) + 3H2O(l)  2NaAl(OH)4 (acts as an acid)
Al2O3(s) + 6HCl(aq)  2AlCl3(aq) + 3H2O(l) (acts as a base)
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Formula Na2O
MgO
Al2O3
SiO2
P4O10
SO3 and
of Oxide
SO2
Metal/
NonMetal
Metal
Metal
Metal
Nonmetal
Nature of
Oxide
Basic
Basic
Amphoter Acidic
ic
Nonmetal
Nonmetal
Acidic
Acidic
Metal Oxides
Metalloid
Oxides
Non-Metal
Oxides
Oxide
Formula
Na2O
(s)
MgO (s) Al2O3
(s)
SiO2 (s)
P4O10(s) SO3(l)/
/P4O6 (s) SO2(g)
Cl2O7(l)
/Cl2O
(g)
Oxidation
number
+1
+2
+3
+4
+5/+3
+6/+4
+7/+1
Electrical
conductivity
in molten
state
high
high
high
very low
none
none
none
Structure
giant ionic
giant
covalent
molecular covalent


As you go across period 3, the ionic character _________________________________.
As you go down a group of oxides, the ionic character _________________________.
20
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Basic Character
 Sodium and magnesium oxides will dissolve in water to form alkaline
solutions:
o Na2O (s) + H2O (l)  2NaOH (aq)
o MgO (s) + H2O (l)  Mg(OH)2 (aq)

Basic oxides react with an acid to form a salt and water:
o MgO (s) + HCl (aq)  MgCl2 (aq) + H2O (l)
o Li2O (s) + HCl (aq)  LiCl (aq) + H2O(l)
Acidic Character
 Non-metallic oxides react with water to produce acidic solutions:
o P4O10(s) + 6H2O  4H3PO4(aq)
o P4O6(s) + 6H2O  4H3PO3 (aq)





Sulfur trioxide reacts with water to produce sulfuric acid:
o SO3 (l) + H2O (l)  H2SO4 (aq)
Sulfur dioxide reacts with water to produce sulfic acid
Dichlorine heptoxide reacts with water to produce chloric acid
Dichlorine monoxide reacts with water to produce chlorous acid
Silicon dioxide does not react with water, but will react with alkalis to form
silicates.
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
22
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Lesson 7: Introduction to Transition Metals (HL material)
IB Understandings
 Transition elements have variable oxidation numbers, form complex ions
with ligands, have coloured compounds, and display catalytic and magnetic
properties.
Guidance
 Common oxidation numbers of the transition metal ions are listed in the IB
Data booklet in sections 9 and 14.
 Zn is not considered to be a transition element as it does not form ions with
incomplete d orbitals.
 Transition elements show an oxidation number of +2 when the s electrons
are removed.
IB Applications and Skills
 Explanation of the ability of transition metals to form variable oxidation
states from successive ionization energies.
 Explanation of the nature of the coordinate bond within a complex ion.
 Deduction of the total charge given the formula of the ion and ligands
present.
 Explanation of the magnetic properties in transition metals in terms of
unpaired electrons.
d-Block metals:
23
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
D-block cont…
REVIEW: Electron Configuration Exceptions! Why?
Effective Nuclear Charge in D-block
Why is this?
Why is this amazing?
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Physical Propterties
1.
2.
3.
4.
5.
Chemical Properties
1.
2.
3.
Why is zinc not considered a transition metal?
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Scandium
Oxidation States:
26
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Important Points For IB!
 All the transition metals show both the +2 and +3 oxidation states. The M3+
ion is the stable state for the elements from scandium to chromium, but the
M2+ state is more common for the later elements. The increased nuclear
charge of the later elements makes it more difficult to remove a third
electron.
 The maximum oxidation state of the elements increases in steps of +1 and
reaches a maximum at manganese. These states correspond to the use of
both the 4s and 3d electrons in bonding. Thereafter, the maximum oxidation
state decreases in steps of –1.
 Oxidation states above +3 generally show covalent character. Ions of higher
charge have such a large charge density that they polarize negative ions and
increase the covalent character of the compound (see Figure 3.13).
 Compounds with higher oxidation states tend to be oxidizing agents. The use
of potassium dichromate(VI) (K2Cr2O7), for example, in the oxidation of
alcohols.
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
28
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Lesson 8: Complex Ions and Coordinate Complexes
Complex Ions:
 Transition metal ions in solution have a high charge density
 These ions attract polar water molecules which form
________________________________________________________________________________________
 REMBEMBER: A coordinate bond is a
_________________________________________________________________________________________
_________________________________________________________________________________________
Ligands
 When a complex is formed where a central ion is surrounded by molecules or
ions which possess a lone pair of electrons that can enter into a coordinate
bond, the surrounding species are called _____________________________________
 Ligands have to have a _________________________________________________ to donate!
 The number of coordinate bonds from the ligands to the central atom is
called the ____________________________________________________________________________
Shapes of Complex Ions
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Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Coordination Number
Oxidation Number of
Shape
Central Ion
Let’s Practice: Try to figure out the oxidation number of the following ions:
Oxidation Number of Central Ions
1.
2.
3.
Hints!
1.
2.
30
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
What is the charge for the complex ion in compound? [Cr(H2O)6]Cl3?
What is the charge for the complex ion in the following compounds?
[CrCl(H2O)5]Cl2.H2O and [CrCl2(H2O)4]Cl.2H2O
Platinum (II) can form a complex ion with 1 ammonia and 3 chloride ligands. What
is the overall charge and formula for this complex ion?
Ligands
Monodentate
Polydentate
31
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Chelating Agents
EDTA Usage:
1.
2.
3.
4.
5.
6.
32
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Let’s Practice
33
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Lesson 9 – d-Block Elements as Catalysts and Magnets





A _____________________________ alters the rate of reaction by providing an
alternate pathway with a lower activation energy
Catalysts are extremely important as they allow reactions to proceed
__________________________________
In a__________________________________ catalyst, the catalyst is in the same state as
the reactants
In a __________________________________ catalyst, the catalyst is in a different state
as the reactants
Transition metals are super effective __________________________________
____________________since they can use their s and d electrons to weakly interact
with reactant molecules and arrange them in the correct orientation
(remember that in order for a reaction to occur, the reactants must combine
with enough energy in the correct orientation!)
Heterogeneous Catalyst:
Iron
Nickel
Pt and PD
MnO2
V2O5
Nickel
(with oils)
Hydrogenation of Oils:
34
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Homogeneous Catalysts:
Iron
Cobalt
Catalytic Converters:
Magnetism
Diamagnetism
Paramagnetism
Ferromagnetism


Iron, nickel, and cobalt are ______________________________________________; the
unpaired d electrons in large numbers of atoms line up with parallel spins in
regions called domains.
Paramagnetism increases with the number of unpaired electrons so
generally _____________________________________________________________________across
the Periodic Table, reaches a maximum at chromium, and decreases. Zinc has
no unpaired electrons and so is diamagnetic.
35
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
36
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Lesson 10 – D-Sublevel Splits and Colored Ions
Understandings:
 The d sub-level splits into two sets of orbitals of different energy in a
complex ion.
 Complexes of d-block elements are coloured, as light is absorbed when an
electron is excited between the d orbitals.
 The colour absorbed is complementary to the colour observed.
Guidance
 The relation between the colour observed and absorbed is illustrated by the
colour wheel in the IB Data booklet in section 17.
Applications and Skills
 Explanation of the effect of the identity of the metal ion, the oxidation
number of the metal, and the identity of the ligand on the colour of transition
metal ion complexes.
Guidance
 Students are not expected to recall the colour of specific complex ions.
 Explanation of the effect of different ligands on the splitting of the d orbitals
in transition metal complexes and colour observed using the
spectrochemical series.
 The spectrochemical series is given in the IB data booklet in section 15. A list
of polydentate ligands is given in the data booklet in section 16. Students are
not expected to know the different splitting patterns and their relation to the
coordination number. Only the splitting of the 3-d orbitals in an octahedral
crystal field is required.
Colored Ions:
37
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Visible Spectrum:
Light:
D Sublevel Splits:
38
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Energy Level Splits
1.Nuclear
Charge and
Identity of
Central Ion
2.Charge
Density
39
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
3.Geometry
4.Number of d
electrons and
oxidation
number
Spectrochemical series:
40
Nomen:_________________________________________
Dies:__________________
IB Chemistry Year 1 HL
Unit 2: Periodicity (Topics 3 and 13) Classwork
_________________________________________________________________________________________________
Let’s Practice
State the formula and the shape of the complex ion formed in the following
reactions.
(a) Some iron metal is dissolved in sulfuric acid and then left exposed to air until a
yellow solution is formed.
(b) Concentrated hydrochloric acid is added to aqueous copper sulfate solution to
form a yellow solution.
(c) A small volume of sodium chloride is added to aqueous silver nitrate solution.
The white precipitate dissolves to form a colourless solution when ammonia
solution is added.
41