Study Guide for Regular Chemistry
The exam will cover all the new work done in Quarters 3 and 4 – the nature of
the subject means that some concepts covered earlier in the year will also be
needed to answer the questions and solve the problems but they are being used
at present anyway.
Periodic trends – atomic/ionic radii, ionisation energy, electronegativity
Ionic and Covalent bonding – theory
Shapes of molecules - VSEPRT
Bond and molecular polarity
Intermolecular bonding – vdw, dipole/dipole, H-bonds - theory
Bronsted/Lowry theory of acid/base
pH calculations using weak/strong acid/base and Ka
Indicators – what they are and how they work
Titrations – theory, calculations
Oxidation numbers/state
Balancing redox equations
Calculating cell potentials
Writing cell equations and labelled cell diagrams
Predicting e flow
Electrolytic cells and prediction of products
Labelled cell diagrams
Periodic Trends Worksheet
1)
Rank the following elements by increasing atomic radius: carbon,
aluminum, oxygen, potassium.
2)
Rank the following elements by increasing electronegativity: sulfur,
oxygen, neon, aluminum.
3)
What is the difference between electron affinity and ionization energy?
4)
Why does fluorine have a higher ionization energy than iodine?
5)
Why do elements in the same family generally have similar properties?
Periodic Trends Worksheet - Solutions
1)
Rank the following elements by increasing atomic radius: carbon,
aluminum, oxygen, potassium.
From smallest to largest:
oxygen < carbon < aluminum < potassium
2)
Rank the following elements by increasing electronegativity: sulfur,
oxygen, neon, aluminum.
From smallest to largest:
neon < aluminum < sulfur < oxygen
3)
What is the difference between electronegativity and ionization energy?
Electronegativity is the ability of an atoms to pull electrons towards
itself in a covalent bond. Ionization energy is a measure of how
much energy it takes to pull electrons off of an element. Both values
are for atoms in the gas phase.
4)
Why does fluorine have a higher ionization energy than iodine?
It is harder to pull electrons off of fluorine because fluorine has a
higher electronegativity than iodine. Iodine has a much lower
electronegativity than fluorine because of the shielding effect, which
states that the electrons in inner energy levels tend to push
electrons in outer energy levels away from the nucleus. This
pushing makes it harder for iodine to grab electrons.
5)
Why do elements in the same family generally have similar properties?
Because they have similar electron configurations and the same
number of valence electrons. Because valence electrons are
responsible for most of the chemistry we observe, this similarity
causes the properties of the elements to also be similar.
Ionic bonding
1. What is an Ionic Bond?
2. How does an ionic bond form?
3.What are the physical properties of ionic bonds:
4. Describe the arrangement of the crystal lattice
Covalent bonding
1)
2)
3)
4)
5)
6)
7)
8)
9)
For compounds in number 1 – use N2H2
Draw the Lewis structure for the compound in #1
Draw the Lewis structure for each ion in (NH4)2CO3
The molecule in #1 has two atoms that can be considered central. What is
the shape about each central atom.
What is the electronegativity difference between Nitrogen and hydrogen?
Draw the orbital diagrams for N and H (electron configuration)
Does the molecule in #1 have polar bonds?
Is the molecule in #1 polar over all? How do you know?
What properties do you think the molecule in #1 will have? How will they
differ from the properties of (NH4)2CO3?
Acid and Base questions – Try this website – there are lots and
lots for you to do
http://www.nclark.net/AcidsBases
Ionic bonding
1. What is an Ionic Bond?
- the electrostatic attraction between oppositely charged ions
(attraction between positive and negative ion
2. How does an ionic bond form?
- Ions form from electron transfer. Positive ions form when
atoms lose electrons, giving them to atoms that want to gain
electrons. Negative ions form by taking electrons
- The positive and negative ions attract
3.What are the physical properties of ionic bonds:
- crystals,
- high melting points,
- brittle,
- conduct when dissolved in water or when melted.
4. Describe the arrangement of the crystal lattice
- each ion is surrounded by oppositely charged ions
+
-
+
-
+
-
-
+
+
Covalent bonding
Other review activities
Richard thornly – You tube
Watch any of the following topics.
Periodicity: 3.1.1 – 3.2.4
Bonding: 4.1.1 – 4.4.2
Acid/Base – 8.1.1; 8.2.1- 8.4.4; 18.1.1 – 18.5.1
Redox & votaic cells – 9.1.1 – 9.5.2
Mr wisemans – tests, tutuorials etc
http://www.mwiseman.com/courses/chem_ib/
topic 7,8,9,10 and some stoichiometry