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Chemistry
Year 11 ATAR Chemistry definitions and valencies
| Question | Answer |
|---|---|
| Solution | are homogenous mixtures, consisting of a solvent and a solute in a fixed composition |
| Homogenous | a mixture with uniform properties and composition throughout |
| Solute | the substance that is dissolved |
| Solvent | the substance that does the dissolving |
| Saturated Solution | where no more of the solute can dissolve under the existing conditions of temperature and pressure |
| Unsaturated Solution | where more solute can dissolve in the solution at the existing conditions of temperature and pressure |
| Super Saturated Solution | contains more solute than a saturated solution can normally hold for the existing conditions. |
| Concentrated Solution | contains a large proportion of solute and particles are relatively close together. |
| Dilute Solution | contains a small proportion of solute, where particles are relatively far apart. |
| Solubility | is a measure of how much solute can dissolve in a particular amount of solvent |
| Miscible | two liquids that can mic together in any ratio to form a solution |
| Electrolyte | when a substance produces ions when dissolved in a solution |
| Strong electrolyte | Where 100% of the substance dissolved forms ions in the solution |
| Examples of Strong Electrolytes | All ionic compounds, and strong acids (sulfuric, nitric, hydrochloric, HBr, HCl) |
| Weak Electrolytes | where are partial amount of the substance ionises in a solution, and most of it remains in its molecular form |
| Examples of Weak Electrolytes | ethanoic acid, ammonia |
| Non-Electrolytes | Substances that remain fully as molecules when dissolved in a solution |
| Examples of Non-Electrolytes | Most covalent molecular substances (e.g glucose) |
| Dissociation | The process by which an ionic compound is dissolved in water, breaks apart from the ionic lattice, and separates into ions. |
| Ionisation | the process by which covalent molecular compounds are dissolved in water to produce ions through the reaction of the neutral molecules with water. |
| Spectator Ion | Ions that are present in solutions that do not take part in reaction |
| Precipitate | Insoluble solid formed when 2 solutions of ionic compounds are mixed |
| acid + reactive metal = | salt + Hydrogen |
| acid + oxide/hydroxide = | salt + water |
| acid + metal carbonate/ hydrogen-carbonate = | salt + water + carbon dioxide |
| Matter | is anything with mass that takes up space |
| Pure Substance | is a substance that is fixed and definite in its composition. |
| Example of a pure substance? | Elements and compounds |
| Element | is a pure substance made up of only 1 type of atom. cannot be separated into smaller particles |
| Compounds | is a pure substance made up of 2 or more elements chemically combined in a fixed ratio. cannot be separated using physical separation methods |
| Mixtures | contains 2 or more substances. can be physically separated and can be homogenous or heterogenous |
| Heterogenous | is a mixture that has a variable composition throughout. |
| Physical Change | do not change the composition of a substance. |
| what are examples of physical changes? | changes of state, dissolving, changing in size. |
| Chemical Change | involve a change of the substance into a substance |
| Atomic Number | the number of protons in the nucleus of an electron |
| Mass Number | the number of protons and neutrons in the nucleus of an atom |
| Isotopes | are the same type of atom (same number of protons), but have a different number of neutrons. |
| Relative Formula Mass (RFM) | is the atomic mass of a whole compound compared to 1/12 carbon-12 atom |
| Relative Atomic Mass (RAM) | is the mass of 1 atom of an element compared to 1/12 of the carboon-12 isotope |
| Mass Spectrometry | is the process used to find the natural abundance of isotopes of an element |
| Core Charge | measure of the attractive force felt by the valence electrons |
| How do you find out the core charge of an atom? | shielding electrons - protons in nucleus |
| Atomic Radius | is the distance between the nucleus and the valence electrons |
| What happens to atomic radius across a period? | it decreases (stronger force of attraction) |
| What happens to atomic radius down a group? | it increases |
| What happens to core charge across a period? | it increases (more valence electrons, same amount of shielding electrons) |
| What happens to core charge down a group? | it decreases |
| Ionisation Energy | is the energy required to remove the outermost electron from a gaseous atom/ion |
| What happens to ionisation energy across a period? | it increases (stronger force of attraction) |
| What happens to ionisation energy down a group? | it decreases |
| Ammonium | NH4 (+) |
| Cyanide | CN (-) |
| Dihydrogen phosphate | H2PO4 (-) |
| Ethanoate | CH3COO (-) |
| Hydrogen Carbonate | HCO3 (-) |
| Hydrogen Sulfate | HSO4 (-) |
| Hydroxide | OH (-) |
| Nitrate | NO3 (-) |
| Nitrite | NO2 (-) |
| Permangenate | MnO4 (-) |
| Carbonate | CO3 (2-) |
| Chromate | CrO4 (2-) |
| Dichromate | Cr2O7 (2-) |
| Hydrogen Phosphate | HPO4 (2-) |
| Oxalate | C2O4 (2-) |
| Sulfate | SO4 (2-) |
| Sulfite | SO3 (2-) |
| Phosphate | PO4 (3-) |
| Ammonia | NH3 |
| Hydrochloric acid | HCl |
| Hydrogen Peroxide | H2O2 |
| Nitric Acid | HNO3 |
| Carbonic Acid | H2CO3 |
| Sulfuric Acid | H2SO4 |
| Sulfurous Acid | H2SO3 |
| Parts Per Million (PPM) | Mass of solute (mg) / Mass of solution (kg) |
| Grams per litre (concentration) | mass of solute (g) / volume of solution (l) |
Created by:
AC!!
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