Cape Chemistry Reminders

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36 Terms

1
Relative Atomic Mass
This is the average mass of an atom of an element according to 1/12 of the mass of carbon-12
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2
Ionic Bonding
This is the electrostatic attraction between two oppositely charged atoms forming a lattice. This usually involves the attraction between a metal and non-metal
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3
Covalent bonding
This is force of attraction between the nuclei of two neighboring atoms and a pair of electrons between them.
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4
Metallic Bonding
This is the sharing of free electrons among the lattice of positively charged metal ions.
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5
Law of Conservation of Mass
states that masses cannot be created or destroyed. This means that the combined masses of the product of the reaction is equal amounts to the combined masses of the starting reactants.
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6
Law of Definite Proportions
states that different samples of a pure substance will contain the same proportions of the same element by mass.
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7
Mole
This is the amount of substance which has the same number of particles as there atom in exactly 12g of carbon-12 isotope.
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8
Empirical Formula
This is the simplest formula showing the relative amount of atoms in a compound. It is the simplest of a mole ratio of elements in a compound
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9
Molecular formula
It tells the actual number of atoms of element a molecule present in a compound. This only for molecular substances. It is a simple whole number multiple of the empirical formula
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10
Avagadro’s Law
states that at the same volume all gases of the same pressure and temperature has equal number of molecules.
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11
R.T.P.
1 mole= 24
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12
S.T.P.
1 mole = 22.4
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13
Concentration of a solution
refers to the amount of solute dissolved in a specific solvent to create a solution.
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14
An electron is stable when…..
its wavelength or multiple of it, is exactly fit around a nucleus at a particular distance
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15
Titration
This is a method of analysis that allows you to determine the precise endpoint of a reaction and therefore the precise quantity of reactants in the titration flask.
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16
A burette is used for…..
deliver the second reactant to the flask
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17
An indicator or pH meter is used to…
detect the endpoint of a reaction.
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18
The standard solution of a titrant
is a solution of known concentration that is required to react quantitatively with another solution of unknown concentration.
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19
Primary standard
this is a substance of high purity used to prepare the concentration of the standard solution in the volumetric analysis.
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20
Properties of primary standard
high purity, stable towards air, absence of water of crystallization, high formula weight, soluble in titration medium
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21
Why cant sodium hydroxide be a primary standard?
This is because it is impure, hydroscopic, absorbs oxygen in air. It also absorbs moisture in air
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22
Preparing a Standard Solution by Dilution
Fill clean dry burette with more concentrated solution.

Run calculated volume of the more concentrated solution in the volumetric flask

Make solution up to the mark with distilled water. Invert several times
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23
Equivalence Point
This is when both solutions are the same number of moles.
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24
Endpoint
This is when there is a color change and it signals that the reaction is complete.
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25
Use of Titration
to determine the amount of substance in an unknown solution
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26
Determining concentration of solution of alkali
  1. Fill the burette with the acid known concentration (after washing with acid).

  2. Record initial reading

  3. Put a known volume of the alkali into a flask using a pipette

  4. Add an acid-base indicator into the flask with the alkali

  5. Add slowly the acid from the burette until the indicator color change (endpoint)

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27
Heat of fusion
This is the amount of energy required to change one gram of a solid to a liquid without changing its temperature.
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28
Vapor pressure is called Saturated vapor pressure when
the molecules reach a dynamic equilibrium for this is when the rate of evaporation is equal to the rate of condensation
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29
When does a liquid boils
This is when the saturate vapor pressure is equal to external pressure hence called vaporization.
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30
Boyle’s Law
The volume of a fixed mass of gas is inversely proportional to pressure at constant temperature. P= k/V
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31
Charles Law
The volume of fixed mass of gas is directly proportional to the absolute temperature at constant pressure.
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32
Absolute Zero
This is the temperature at which the volume of the gas becomes zero if it did not condense.
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33
Constant Volume Law
The the pressure of a fixed mass of gas is directly proportional to temperature at constant volume
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34
Ideal Gas
This is a gas which obeys the general gas equation of PV=nRT and other gas laws at all temperature and pressure
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35
When do real gases approach ideal gas behaviour
In high temperatures and low pressure
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36
When do real gases
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