Upload
hoangcong
View
221
Download
0
Embed Size (px)
Citation preview
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
2
Nomen:_________________________________________ Dies:__________________IB Chemistry Year 1 HL Unit 2: Periodicity (Topics 3 and 13) Classwork_________________________________________________________________________________________________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_________________________________________________________________________________________________
9
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
Which ion would have a larger ionic radius, Na+ or Mg2+?
11
Nomen:_________________________________________ Dies:__________________IB Chemistry Year 1 HL Unit 2: Periodicity (Topics 3 and 13) Classwork_________________________________________________________________________________________________
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
12
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 WaterLithium
Sodium
Potassium
14
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:
15
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?
16
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
17
Nomen:_________________________________________ Dies:__________________IB Chemistry Year 1 HL Unit 2: Periodicity (Topics 3 and 13) Classwork_________________________________________________________________________________________________
18
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) à Ca(OH)2(aq) Non-metallic oxides are acidic: they react with water to form acidic solutions
CO2(g) + H2O(l) à 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) à 2NaAl(OH)4 (acts as an acid)
Al2O3(s) + 6HCl(aq) à 2AlCl3(aq) + 3H2O(l) (acts as a base)
19
Nomen:_________________________________________ Dies:__________________IB Chemistry Year 1 HL Unit 2: Periodicity (Topics 3 and 13) Classwork_________________________________________________________________________________________________
Metal Oxides
Metalloid Oxides
Non-Metal Oxides
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) à 2NaOH (aq)o MgO (s) + H2O (l) à Mg(OH)2 (aq)
Basic oxides react with an acid to form a salt and water:o MgO (s) + HCl (aq) à MgCl2 (aq) + H2O (l)o Li2O (s) + HCl (aq) à LiCl (aq) + H2O(l)
Acidic Character Non-metallic oxides react with water to produce acidic solutions:
o P4O10(s) + 6H2O à 4H3PO4(aq)o P4O6(s) + 6H2O à 4H3PO3 (aq)
Sulfur trioxide reacts with water to produce sulfuric acid:o SO3 (l) + H2O (l) à 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.
21
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:
D-block cont…
23
Nomen:_________________________________________ Dies:__________________IB Chemistry Year 1 HL Unit 2: Periodicity (Topics 3 and 13) Classwork_________________________________________________________________________________________________
REVIEW: Electron Configuration Exceptions! Why?
Effective Nuclear Charge in D-block
Why is this?
Why is this amazing?
24
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?
25
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.
27
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
29
Nomen:_________________________________________ Dies:__________________IB Chemistry Year 1 HL Unit 2: Periodicity (Topics 3 and 13) Classwork_________________________________________________________________________________________________Coordination Number Oxidation Number of
Central IonShape
Let’s Practice: Try to figure out the oxidation number of the following ions:
Oxidation Number of Central Ions1.
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?
LigandsMonodentate
Polydentate
31
Nomen:_________________________________________ Dies:__________________IB Chemistry Year 1 HL Unit 2: Periodicity (Topics 3 and 13) Classwork_________________________________________________________________________________________________
EDTA Usage:1.
2.
3.
4.
5.
6.
Chelating Agents
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:
38
Nomen:_________________________________________ Dies:__________________IB Chemistry Year 1 HL Unit 2: Periodicity (Topics 3 and 13) Classwork_________________________________________________________________________________________________Light:
D Sublevel Splits:
Energy Level Splits1.Nuclear Charge and Identity of Central Ion
2.Charge
39
Nomen:_________________________________________ Dies:__________________IB Chemistry Year 1 HL Unit 2: Periodicity (Topics 3 and 13) Classwork_________________________________________________________________________________________________Density
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
Nomen:_________________________________________ Dies:__________________IB Chemistry Year 1 HL Unit 2: Periodicity (Topics 3 and 13) Classwork_________________________________________________________________________________________________
42