vault backup: 2026-09-22 01:37:31
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@@ -333,7 +376,6 @@
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"physics/Oscillations",
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"physics/Oscillations",
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"physics/Fluids",
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"physics/Fluids",
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@@ -0,0 +1,22 @@
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[[Organic Chemistry]]
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Simplest organic compounds are hydrocarbons, composed solely of carbon and hydrogen.
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Non-polar, as they contain only hydrogen and carbon.
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They are classified as aromatic or aliphatic. Aliphatic hydrocarbons have carbon atoms bonded in chains or rings, including straight chains and cyclic alkenes, alkanes and alkynes. Aromatic hydrocarbons are hydrocarbons based on aromatic benzene group.
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Alkanes are hydrocarbons that only contain single bonds, alkenes contain double bonds and alkynes contain triple bonds.
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Alkanes in the shape of a ring are called cycloalkanes. Alkanes not in the shape of rings have formula $C_nH_{2n+2}$. Cycloalkanes are in the shape of rings and have the formula $C_nH_{2n}$. Straight chain alkenes with one double bond have the same formula as cycloalkanes. Straight chain alkynes with one triple bond have the formula $C_nH_{2n-2}$.
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Functional groups are groups of reactive bonded atoms that appear in all members of a family. Reactive double bonds are the functional group of alkenes.
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# Naming Organic Compounds
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Naming organic compounds usually follows the pattern of prefix + root + suffix.
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Root names:
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| Number of Carbon atoms | 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 |
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| ---------------------- | ---- | --- | ---- | --- | ---- | --- | ---- | --- | --- | --- |
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| Root | meth | eth | prop | but | pent | hex | hept | oct | non | dec |
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@@ -1,4 +1,4 @@
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[[G11 Pre-AP Biology]]
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c[[G11 Pre-AP Biology]]
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||||||
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* Non-living
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* Non-living
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* Not capable of surviving on its own
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* Not capable of surviving on its own
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@@ -1 +0,0 @@
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[[Chemistry]]
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@@ -0,0 +1,7 @@
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[[Organic Chemistry]]
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Organic compounds are compounds that contain carbon. It was originally classified as compounds originating from living beings, but a scientist made an organic compound inorganically using ammonium cyanate.
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Carbon usually forms 4 covalent bonds. If a compound contains only single bonds, then it's saturated, unsaturated otherwise.
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Carbons unique bonding allows it to form many shapes, including rings and chains.
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@@ -0,0 +1 @@
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[[chemistry]]
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@@ -1,11 +0,0 @@
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[[Chemistry]]
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**"calculation of relative quantities of reactants and products in chemical reactions"**
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avogardos numbers = $6.02*10^{23}$
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n=mole=conversion factor=$6.02*10^{23}$ things (atoms/ions/molecules/formulaunits/etc)
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1 pair = 2 things
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1 dozen = 12 things
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one atomic unit ~= 1 gram / avogardos number
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avogardos number x atomic unit ~= 1 gram
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[[Matter and Chemical Bonding]]
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covalents are sharing
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ionics are giving
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@@ -1,27 +0,0 @@
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[[Chemistry]]
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**main types**
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synthesis
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decomposition
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single displacement
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double displacement
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combustion
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# synthesis
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just two substances coming together to form a compound,
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reactant + reactant ->
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# single displacement
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requires the replacee to havea a lower activity series than the replacer
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# Double Displacement
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double displacement is a reaction of 2 compounds
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pos and negs switch places to form new stuff
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only works with ionics
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only occurs if one of 3 propduces is formed
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- percipitate (s)
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- gas (g)
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- covalent compound such as water (l)
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# Combustion
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is hydrocarbon react with oxygen to create co2 and h2o
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@@ -1 +1 @@
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[[ROOT]]
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[[root]]
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[[Matter and Chemical Bonding]]
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how much attraction an element has to electrons
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when bonded things different in electronegativity is too high, one basically steals the electron from the other forming an ionic bond, and if it's in the middle then it's polar, and if the difference isnt large than the 2 play nice and share it with a covalent
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[[Stoichiometry]]
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empirical formulas are the simplest whole number ratio of atom in a substance
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eg acetic acid and glucose share an empherical of ch_2o
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@@ -1,5 +0,0 @@
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[[Stoichiometry]]
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law of definite proportions states: the elements in a chemical compound are always present in the same proportion by mass
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$percentcomposition=\frac{massofelement}{totalmassofcompound}*100%$
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[[Matter and Chemical Bonding]]
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naming chemical compounds
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[[Chemistry]]
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periods are rows
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groups are columns
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[[Matter and Chemical Bonding]]
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[[electronegativity]]
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when 2 bonding atoms have an $\Delta$ EN greater than 0.5 and less than 1.7, it's a polar covalent bond
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polar covalents have an imbalance of electrons, causing partial positive charges and partial negative charges, the atom with the stronger EN pulls the electron more but not enough to completely take it, making the electron closer and giving it a partial negative charge
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[[Chemistry]]
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**"a charged chemical species composed of two or more atoms covalently bonded or of a metal complex, that can be considered to be acting as a single unit"
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H stable at a duet 2d
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Be stable at a tetrad 4e
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B stable at a sextet 6e
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| **Name** | **Formula** |
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| ---------------------------------------------- | ---------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------- |
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| **Polyatomic ions (carrying negative charge)** | |
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| Hydroxide | OH [Matter and Chemical Bonding]]<br><br>add or remove valence e according to charge<br><br>H stable at a duet 2d<br>Be stable at a tetrad 4e<br>B stable at a sextet 6e<br>all other elements in pe 1 and 2 require octets 8e (common ball)<br>per 3 and below can go above an octet (common ball)<br><br><br><br>– |
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| Acetate | CH3COO – |
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| Cyanide | CN – |
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| Chlorate | ClO3 – |
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| Chlorite | ClO2 – |
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| Nitrate | NO3 – |
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| Nitrite | NO2 – |
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| Hypochlorite | OCl – |
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| Hypobromite | OBr – |
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| Iodate | IO3 – |
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| Bisulphite | HSO3 – |
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| Bisulphate | HSO4 – |
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| Permanganate | MnO4 – |
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| Thiocyanate | SCN – |
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| Hydrogen carbonate | HCO 3– |
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| Carbonate | CO3 2- |
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| Sulphate | SO4 2- |
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| Sulphite | SO3 2- |
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| Oxalate | C2O4 2- |
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| Silicate | SiO3 2- |
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| Manganate | MnO4 2- |
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| Thiosulphate | S2O3 2- |
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| Chromate | CrO4 2- |
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| Dichromate | Cr2O7 2- |
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| Phosphate | PO4 3- |
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| Phosphite | PO3 3- |
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| Aluminate | AlO3 3- |
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| Arsenite | AsO3 3- |
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| Arsenate | AsO4 3- |
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| Borate | BO3 3- |
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| Pyrophosphate | P2O7 4- |
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| **Polyatomic ions (carrying positive charge)** | |
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| Ammonium | NH 4+ |
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## List of monatomic ions
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- The ions made of a single atom are called **simple ions or monatomic ions**.
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| **Name** | **Formula** |
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| --------------------------------------------- | ----------- |
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| **Monatomic ions (carrying positive charge)** | |
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| Hydrogen | H+ |
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| Potassium | K+ |
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| Sodium | Na+ |
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| Silver | Ag+ |
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| Cuprous | Cu+ |
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| Aurous | Au+ |
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| Barium | Ba2+ |
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| Calcium | Ca2+ |
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| Magnesium | Mg2+ |
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| Cupric | Cu2+ |
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| Ferrous | Fe2+ |
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| Stannous | Sn2+ |
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| Mercuric | Hg2+ |
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| Zinc | Zn2+ |
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||||||
| Plumbous | Pb2+ |
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| Aluminum | Al3+ |
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| Ferric | Fe3+ |
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||||||
| Auric | Au3+ |
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||||||
| Arseneous | As3+ |
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||||||
| Plumbic | Pb4+ |
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||||||
| Stannic | Sn4+ |
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| **Monatomic ions (carrying negative charge)** | |
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||||||
| Chloride | Cl– |
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| Bromide | Br – |
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||||||
| Iodide | I– |
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||||||
| Oxide | O2- |
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| Sulphide | S2- |
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| Nitride | N3- |
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| Phosphide | P3- |
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@@ -1,6 +0,0 @@
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[[chemical reactions]]
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||||||
shrimple little table to check how stuff reacts with other stuff,
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- sol for soluble which means aqueous
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- ppt for precipitate
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@@ -1,2 +0,0 @@
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[[chemical reactions]]
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[[Matter and Chemical Bonding]]
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@@ -1,6 +0,0 @@
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[[Matter and Chemical Bonding]]
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each lone pair is E
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A is central atom
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X for each binded stuff
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eg $H_2O$ is $AX_2E_2$
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Reference in New Issue
Block a user