BIOLOGY [5090] SYLLABUS
CHEMISTRY A - REVISION GUIDE for Final Examination
INTRODUCTION:
This revision guide is designed to help you prepare for the final examinations. It is based on Indiana’s Academic Standards for Science – Chemistry.
HOW TO USE THIS REVISION GUIDE:
1. This guide contains the list of the topics in your syllabus.
2. Do an assessment and rate yourself in terms of your present mastery of the
subject matter on a scale of 1 to 3 as follows:
|1 |very good; you are comfortable with the topic & you feel you can manage questions on this topic even if you did little|
| |or no further revision; you may just need to have a final read through of the topic in your class notes; writing a|
| |topic summary is a task you can easily do |
|2 |good; you feel you can manage questions on this topic although some revision prior to the exam may help or is |
| |necessary; you need to have a read through of the topic in your class notes and course work and write summary notes to|
| |increase your confidence on the topic; you may then need to go over your summary notes at least twice or thrice before|
| |the examination |
|3 |poor; you feel you are not comfortable with this topic and you therefore need to work on it; this means you need to |
| |go over your class notes and coursework and find time to revise some more |
3. How to do a topic summary: After you have read through the topic [use a highlighter pen
to mark topic highlights]
✓ write down the principles / theories
✓ outline key terms and definitions
✓ note important examples / illustrations / diagrams
✓ label important diagrams
NOTE: REMEMBER THAT YOUR TEACHER IS LOOKING FOR OPPORTUNITIES TO GIVE YOU MARKS – NOT TAKE THEM AWAY!
| | |MASTERY |
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|TOPIC / CONTENT |LEARNING OBJECTIVES |1 |
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|Standard 3: | | |
|BONDING AND MOLECULAR STRUCTURE |Describe, compare and contrast the characteristics of the interactions between atoms in| |
| |ionic and covalent compounds. | |
|Core Standards: | | |
| |Compare and contrast how ionic and covalent compounds form. | |
|Describe how the configuration of | | |
|electrons within an atom |Draw structural formulas for and name simple molecules. | |
|determines its interactions with | | |
|other atoms. |Write chemical formulas for ionic compounds given their names and vice versa. | |
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|Describe the attractive forces |e.g. | |
|among molecules and their effect |1. Define the following terms: | |
|on chemical and physical |(a) cation | |
|properties. |(b) anion | |
| |(c) ionic compound | |
| |(d) covalent compound | |
| |(e) polyatomic ion | |
| |(f) molecules | |
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| |Complete the following table by writing the formula and naming each compound formed: | |
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| |NH4+ | |
| |Na+ | |
| |Ca2+ | |
| |Al3+ | |
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| |OH- | |
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| |SO42- | |
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| |Cl- | |
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| |O2- | |
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| |NO3- | |
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| |What is the Octet Rule? | |
| |Show by way of a diagram the formation of magnesium chloride. | |
| |Show by way of a diagram the formation of methane. | |
| |Name the following compounds: | |
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| |Formula | |
| |Name | |
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| |NH3 | |
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| |CH4 | |
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| |H2O | |
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| |HCl | |
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| |H2SO4 | |
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| |HNO3 | |
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| | |MASTERY |
| | |OF TOPIC |
|TOPIC / CONTENT |LEARNING OBJECTIVES |1 |
| | |2 |
| | |3 |
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|Standard 3: | | |
|BONDING AND MOLECULAR STRUCTURE |RULES FOR NAMING IONIC COMPOUNDS | |
| |1. Binary Compounds | |
|Core Standards: |A compound that contains only two elements is called a binary compound.. | |
| |The name of a binary compound usually ends with IDE. | |
|Describe how the configuration of |If the compound contains a metal and a non-metal, the metal is always named first | |
|electrons within an atom |followed by the name of the non-metal with the ending changed to IDE e.g. CaO is | |
|determines its interactions with |calcium oxide and Na2O is sodium oxide, MgS is magnesium sulfide, KCl is potassium | |
|other atoms. |chloride. | |
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|Describe the attractive forces |2. Compounds of Transition Metals | |
|among molecules and their effect |For a compound of an element that can form two or more ions with different charges, a | |
|on chemical and physical |roman numeral is written after the name of the element to indicate the charge of the | |
|properties. |ion in the compound e.g. FeCl2 is named iron (II) chloride while FeCl3 is named iron | |
| |(III) chloride. | |
|. | | |
| |3. Bases and Alkalis | |
| |A compound that contains a metal and the hydroxide ion, (OH-), has a name ending with| |
| |hydroxide e.g. NaOH is sodium hydroxide, Al(OH)3 is aluminium hydroxide. | |
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| |RULES FOR NAMING COVALENT COMPOUNDS | |
| |1. Binary Compounds | |
| |If the compound contains 2 non-metals which belong to the same group of the Periodic | |
| |Table, the one which is lower down the group is named first, followed by the name of | |
| |the second non-metal with the ending changed to IDE e.g. for a compound of sulphur and | |
| |oxygen, the name is sulphur oxide because sulphur is lower in Group VI of the Periodic | |
| |Table than oxygen and so is named first. | |
| |If the compound contains two non-metals which belong to different groups of the | |
| |Periodic Table, the one with the smaller group number is named first, followed by the | |
| |name of the second non-metal with the ending chaged to IDE e.g. for a compound of | |
| |carbon and sulphur, the name is carbon sulphide because carbon is in Group IV while | |
| |sulphur is in Group VI. | |
| |Water (H2O) and ammonia (NH3) are two exceptions. They are always known by their | |
| |common names. Dihydrogen oxide and trihydrogen nitride are never used. | |
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| |2. Use of prefixes | |
| |If two or more compounds can be formed between two particular elements, a prefix (e.g. | |
| |mono – 1; di – 2; tri – 3; tetra – 4; etc ) is written in front of the name of one | |
| |of the elements to show the number of atoms that is present in the compound e.g. CO is | |
| |carbon monoxide while CO2 is carbon dioxide; SO2 is sulphur dioxide while SO3 is | |
| |sulphur trioxide; CS2 is carbon disulphide. | |
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