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chemistry
im going insane !!!! (finished 3/3)
| Term | Definition |
|---|---|
| Electro configuration | number of electrons found in each shell |
| Outer shell | max=8 |
| Second shell | max =8 |
| First shell | max =2 |
| Atomic number | Total amount of electrons and protons |
| Valence^- | amount of electrons on the most outer shell |
| Atomic mass | neutrons + protons |
| neutrons (equation) | atomic mass - protons |
| Periods | 1-5 (elements in the same period have the same number of electron shells) |
| Groups | 1-18 (elements in the same group have the same number og electrons in their outer shell (not relevant to groups 10-12) - 13-18 groups have electrons 3-8 |
| Ionic Substances/ Ionic Bonding | Ions are formed when atoms gain or lose electrons - occurs between METALS and NON METALS only - Metals lose electrons, becoming positively charged, whereas non metals gain electrons to have a full outer shell, becoming negatively charged |
| Covalent Molecular Substances/ Covalent Bonding | - Occurs between NON METAL ELEMENTS ONLY - Full outer shell achieved by sharing valence electrons - Electrons create a bond between atoms - CO2 (two oxygen atoms share valence electrons to create a full outer shell of carbon |
| Metallic Substances/Metallic Bonding | - METAL ONLY - Delocalised electrons are free to move around atoms - Enables positive metallic ions to be held in place by electrostatic forces of attraction - Allows metals to conduct electricity |
| Metal and Acid Reactions | Metal + Hydrochloric Acid -> Metal Chloride + Hydrogen Metal + Sulfuric Acid -> Metal Sulfate + Hydrogen Metal + Nitric Acid -> Metal Nitrate + Hydrogen |
| Alkanes | Single Covalent Bonds - Cn H2n+2 |
| Alkenes | Double Covalent Bodns - Cn H2n - Write placements of double bonds RIGHT to LEFT and before the 'ene' |
| Alkynes | - Triple Covalent Bonds - Cn H2n-2 - undergo some of the same reactions as alkenes but react twice |
| Substitution Reactions | - Alkanes - Halogen atoms replace a hydrogen on the hydrocarbon molecule - Alkane + X2 -> AlkaneX + HX |
| Addition Reactions | - Alkenes and Alkynes - Double bond is converted to a single bond and 2 extra atoms are added - Just add them together |
| Stem Names | Methane/ene (1) Methyl (1) Hydrocarbons Ethane/ene (2) Ethyl (2) Hydrocarbons Propane/ene (3) Propyl (3) Hydrocarbons Butane/ene (4) Butyl (4) Hydrocarbons Pentane/ene (5) Hexane/ene (6) Heptane/ene (7) Octane/ene(8) Nonane/ene(9) Dec (10 |
| Atomic Weight | = mass of one mole |
| Molar Mass | = mass of one mole of a molecule |
| Finding number of atoms/molecule (N) | = number of moles (n) x (6x10^23) (Na) |
| number of moles (n) when given number of particles | = number of particles (N) / (6x10^23) (Na) |
| Number of moles (n) when given the mass of a substance | = mass of susbatnce given (m) / Molar mass (M) |
| Mass of sample (m) | = number of moles given (n) x Molar mass (M) |
| 1 moles of a compound | consists of different amounts of moles for each element, based on the number next to it |
| Moles to Mass | - Write out equations and balance - Determine mole ratio - Utilise mole ratio to determine (n) for each substance - Calculate molar mass - Multiply molar mass by mole ratio |
| Mass to Moles | - write out equation and balance - determine mole ratio - work out moles based on ratio -mass = n x M |
| Mass to Mass | - write out equation and balance - find mole ratio by finding molar mass and n=m/M - Utilise mole ratio for other molecules - m= n x M |
| Percentage Composition | - % mass of each substance - find total molar mass - divide each elements molar mass by total molar mass and x by 100 |
| Law of conservation of mass | In a chemical reaction, mass is neither created nor destroyed, but stays the same even if the form changes. |
| Metal + Acid | makes Salt + Hydrogen |
| Properties of Covalent Molecular Substances | - Low melting/ boiling points - Many are insoluble in water - Non conductors of electricity in solid/liquid states - Solids are generally soft with a waxy appearance - Many solids are malleable |
| Properties of Metallic Substances | - Good conductors of electricity in liquid/ solid states - Delocalised electrons are responsible for rapid transmission of heat - Malleable - Usually hard and tough at room temp - The stronger the metallic bonds, the higher the melting point |
| Properties of Ionic Compounds | - High melting/boiling points - All solids at room temp - Non-conductors of electricity in their solid state but good conductors in liquid state - Made up of hard crystals (Brittle texture) |
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