Chemistry - formulae and equations

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24 Terms

1
Element
An element is a substance made up of only one type of atom.
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2
Compound
A compound is made up of at least two different elements chemically bonded together. This means compounds are made up of more than one type of atom.
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3
Nitrate Ion
Nitrate: NO3-
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4
Carbonate Ion
Carbonate: CO3 2-
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5
Oxide Ion
Oxide: O2-
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6
Hydroxide Ion
Hydroxide: OH-
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7
Ammonium Ion
Ammonium: NH4+
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8
Sulfate Ion
Sulfate: SO4 2-
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9
Ionic Compound
Ionic compounds are made up of positive and negative ions, held together by electrostatic attraction.
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10
Sodium Chloride Formula
Sodium chloride has the formula NaCl as the charges on the ions must cancel to give a compound with no overall charge.
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11
Aluminium Oxide Formula
For the ionic compound to have no overall charge, two aluminium ions must bond with three oxygen ions, giving the formula Al2O3.
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12
Zinc Nitrate Formula
For the ionic compound to have no overall charge, two nitrate ions must bond with the zinc ion. This gives the formula Zn(NO3)2.
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13
Oxidation Number
A number assigned to an atom or an ion which represents how many electrons have been lost or gained by the atom.
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14
Oxidation Number of an Element
Zero.
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15
Overall Oxidation Number of CaCO3
Zero. The oxidation numbers of a neutral compound add up to zero.
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16
Overall Oxidation Number of HCO3-
-1. The overall oxidation number of a charged compound is simple as it is the charge shown on the molecule.
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17
Oxidation States of Hydrogen and Oxygen
Hydrogen: +1 (except in metal hydrides where it is -1). Oxygen: -2 (except in peroxides and F2O where it is -1).
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18
Common Oxidation States of Halogens and Group One Metals
Halogens: -1. Group one metals: +1.
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19
Oxidation Number of Sulfur in Na2SO4
Sulfur must have an oxidation number of +6 to balance the charges.
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20
Oxidation Number of Chromium in K2Cr2O7
Chromium must have an oxidation number of +6 to balance the charges.
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21
State Symbols in Chemical Equations
(g) - gas; (aq) - aqueous; (l) - liquid; (s) - solid.
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22
Ionic Equation
Ionic equations only show the reacting ions and can be written for any reaction involving ions in solution.
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23
Ionic Equation for HNO3 and NaOH
H+(aq) + OH-(aq) → H2O(l)
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24
Ionic Equation for AgNO3 and NaCl
Ag+(aq) + Cl-(aq) → AgCl(s)
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