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 beforethe 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

OF TOPIC

TOPIC / CONTENT

/ LEARNING OBJECTIVES / 1 / 2 / 3
Standard 3:
BONDING AND MOLECULAR STRUCTURE
Core Standards:
Describe howthe configurationof electrons within an atomdetermines its interactions with otheratoms.
Describe the attractive forcesamongmolecules and theireffecton chemical and physical properties. / C.3.1Describe, compare and contrastthe characteristics oftheinteractions betweenatoms in ionic and covalentcompounds.
C.3.2Compare and contrast howionic andcovalentcompoundsform.
C.3.3Drawstructural formulasforandname simple molecules.
C.3.4Writechemicalformulasfor ioniccompounds given theirnames and vice versa.
e.g.
1. Define the following terms:
(a) cation
(b) anion
(c) ionic compound
(d) covalent compound
(e) polyatomic ion
(f) molecules
  1. Complete the following table by writing the formula and naming each compound formed:
NH4+ / Na+ / Ca2+ / Al3+
OH-
SO42-
Cl-
O2-
NO3-
  1. What is the Octet Rule?
  2. Show by way of a diagram the formation of magnesium chloride.
  3. Show by way of a diagram the formation of methane.
  4. Name the following compounds:
Formula / Name
NH3
CH4
H2O
HCl
H2SO4
HNO3
/

MASTERY

OF TOPIC

TOPIC / CONTENT

/ LEARNING OBJECTIVES / 1 / 2 / 3
Standard 3:
BONDING AND MOLECULAR STRUCTURE
Core Standards:
Describe howthe configurationof electrons within an atomdetermines its interactions with otheratoms.
Describe the attractive forcesamongmolecules and theireffecton chemical and physical properties.
. / RULES FOR NAMING IONIC COMPOUNDS
1. Binary Compounds
  • A compound that contains only two elements is called a binary compound..
  • The name of a binary compound usually ends with IDE.
  • If the compound contains a metal and a non-metal, the metal is always named first followed by the name of the non-metal with the ending changed to IDE e.g. CaO is calcium oxide and Na2O is sodium oxide, MgS is magnesium sulfide, KCl is potassium chloride.
2. Compounds of Transition Metals
  • For a compound of an element that can form two or more ions with different charges, a roman numeral is written after the name of the element to indicate the charge of the 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.
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.
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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