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Update Unit 1: Chemistry.md
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# Unit 1: Chemistry
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- Matter - has mass, takes up space.
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- `Matter`: has mass, takes up space.
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- fundamental unit -> ATOMS
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- One `formula unit` - repeating strucure in an ionic compound taht has the simplest ratio of ions in the compound
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- One `formula unit` - repeating strucure in an ionic compound that has the simplest ratio of ions in the compound
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- Can be represented in **Chemical Formula** (e.g $`Li_3P`$)
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- Ions are particles with charges
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- `Models`: Allows people to make accurate `predictions` about `behavior` of MATTER.
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- `Atom`: **Smallest** unit of element that still retains its properties. Made of **subatomic** particles
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- `Atomic mass unit:` $`1.67 \times 10^{-27}kg`$
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## Atoms
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- Atoms are the smallest unit of an element that still retains its properties
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@ -30,8 +35,31 @@
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|C|Chemistry|
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- Involved in studying, varifying information (eg the periodic table -> Describes the elements -> pure susbtances made of only one kind of atom),and publishing.
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- Standarize the information for the public
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## Bohr Rutherford
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- Electrons in **uncharged** atom, # protons $`=`$ # electrons
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- Mass of an atom is the weighted average if akk usitioes if element
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- `Atomic Notation`, Top number is the mass, bottom number is the atomic number.
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<img src="https://d2jmvrsizmvf4x.cloudfront.net/LHJtmeuTDVQ4l2uelrkw_imgres.png" width="300">
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## Lewis Structures (dot diagrams)
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- shows valence $`e^-`$; centre is atomic symbol
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- Use family groups to figure out valence $`e^-`$
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<img src="https://upload.wikimedia.org/wikipedia/commons/6/6b/Lewis_dot_K.svg" width="100">
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<img src="http://www.chemistrylearner.com/wp-content/uploads/2018/08/Neon-Lewis-Dot-Structure.png" width="100">
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<img src="https://qph.fs.quoracdn.net/main-qimg-9a09a4e3ae1808d51ada5405916408e9.webp" width="100">
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## Trends on the Periodic Table
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- `Periodic Table:` Describes **elements** pure susbatances made of only **1** type of Atom.
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- The further away the electron is from the nucleus, the more energy it has.
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- `Periods:` repeating pattern.
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- Metals on **bottom left**, non-metals on **top right**
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### Measuring Atomic Radius
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- Stack a bunch of them, measure, divide by number of atoms, easy clap :p.
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<table>
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<tr>
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@ -49,7 +77,7 @@
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<tr>
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<th><b>Atomic Radius</b> <br> (size of an atom)</th>
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<td>Decrease due to more protons in the nucleus that attract the electrons, while having the same atomic radius</td>
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<td>Increases due to sheilding and more energy levles, which actually cancels out and is greater than the force of increasing protons in the nucleus</td>
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<td>Increases due to shielding and more energy levels, which actually cancels out and is greater than the force of increasing protons in the nucleus</td>
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</tr>
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<tr>
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@ -87,9 +115,10 @@
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- They tend to lose electrons
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- They are shiny, ductile, malleable, conductive
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- They have a weak/loose hold on electrons
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- Most metals are considered to be multi-metals
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- Most metals are considered to be multi-metals (`multi-valent`)
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- can form ions of differing charges
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- add roman numerals to the ions name to indicate its charge, for example, iron($`III`$) oxide.
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- `Metalloids`: non-metals with same metallic or metals with non-metalic properies`
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## Non-Metals
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- They are dull, bad conductors - insulators
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@ -106,6 +135,9 @@
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- We can use modesl(e.g Lewis dot diagrams) to show bonding
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- Atoms will lose or gain electrons to achieve noble gas $`e^-`$ configuration $`\rightarrow`$ The most common stable ion. (eg, if $`Na`$ loses electrons, it becomes like $`Ne`$, if $`Cl`$ gains an electron, it becomes like $`Ar`$)
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- To show that atoms are different than ions, we put square brackets around it $`[Na]`$, then we put superscript on the top right to show its charge, $`[Na]^+`$ (if the charge is only a $`\pm 1`$, we just put a $`+`$ instead of $`1+`$)
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- Example of ionic bond:
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- <img src="https://cdn.kastatic.org/ka-perseus-images/5ea8232d69862ad00d65c8d625907b7e1b04172e.jpg" width="200">
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## Non-Metal Ionic Names
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|Element|Name|
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@ -131,6 +163,8 @@
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- Naming and writing chemical formuals
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- According to IUPAC
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- Direct relationship beween chemical name and chemical structure
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- - Going down diagonally from `aluminium`, we get a pattern of $`3+`$, $`2+`$, $`1+`$ of charge. `Aluminium` has a charge of $`3+`$, `Zinc` has a charge of $`2+`$, and `silver` has a charge of $`1+`$, and they are all mono-valent. (not multi-valent)
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- `Galvanize` (rust $`\rightarrow`$ white shield $`\rightarrow`$ cover iron $`\rightarrow`$ prevnet rusting, but I don't think it will be in this unit)
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|Formula|Name|
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|:------|:---|
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@ -152,10 +186,7 @@
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- non-metals (the ones hugging the staircase are also non-metals (some of the `metalloids`))
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- `halogens`
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- `noble gases`
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- Going down diagonally from aluminium, we get a pattern of $`3+`$, $`2+`$, $`1+`$ of charge. Aluminium has a charge of $`3+`$, Zinc has a charge of $`2+`$, and silver has a charge of $`1+`$, and they
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are all mono-valent. (not multi-valent)
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- If there is more than one polyatomic ion in a formula unit, then surround the ion with brackets
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- If there is more than one polyatomic ion in a formula unit, then surround the ion with brackets/parentheses
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- Oxyanion are negative ions with oxygen in them
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|Polyatomic Ion Name|Formula (Always Remember The Charge!)|
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@ -174,6 +205,15 @@ are all mono-valent. (not multi-valent)
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|Sulfate|$`SO_4^{2-}`$|
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|Phosphate|$`PO_4^{3-}`$|
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### Oxyanions
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- Nitrate
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- Borate
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- Carbonate
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- Chlorate
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- Sulfate
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- Phosphate
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- And their family members :p.
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## Deriving Ions From Parent
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|Polyatomic Ion Name|Operation|Chemical Formula|
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@ -191,6 +231,8 @@ are all mono-valent. (not multi-valent)
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|Bromate|$`BrO_3^-`$|
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## Acidic Oxyanions
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- Acids generall have hydrogen ions $`(H^+)`$
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- Acidic Oxyanions $`\rightarrow`$ Negatively charged ion with $`O`$ and $`H`$
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- Each hydrogen added to a polyatomic ion increases the charge by one, and changes the name:
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|Name|Chemical Formula|
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@ -199,15 +241,14 @@ are all mono-valent. (not multi-valent)
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|Dihydrogen phosphate ion|$`H2PO_4^-`$|
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|Monohydrogen phosphate ion|$`HPO_4^{2-}`$|
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- For above, we use mono for phosphate to avoid ambigious cases, where $`H_2PO_4^{-}`$ and $`H_2PO_4^{2-}`$ are the same if we don't put `mono` infront. As for the Hyrogen carbonate ion
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we don't put a mono due to no ambigious cases.
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- For above, we use mono for phosphate to avoid ambigious cases, where $`H_2PO_4^{-}`$ and $`H_2PO_4^{2-}`$ are the same if we don't put `mono` infront. As for the Hyrogen carbonate ion we don't put a mono due to no ambigious cases.
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## Molecular Compounds
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- Are not made of ions, instead molecules
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- Shared pair of electrons -> `covalent bonds`
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- Lone pair of electrons are electrons that are not shared
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- Radicals are unpaired electrons, vefy reactive
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- Molecules have no charge
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- `Lone pair` of electrons are electrons that are not shared
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- Radicals are atoms with unpaired electrons, very reactive
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- Molecules have **no charge**
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- Atoms fill their valence shells to form molecules
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- Double bond between oxygen atoms in an oxygen molecule
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@ -233,6 +274,29 @@ we don't put a mono due to no ambigious cases.
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|Molecualr|liquid, gas, or solid|non-soluble|Has distinct colour?|Not really conductive|
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## Binary Molecular Compounds
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- 2 different kinds of atom in molecule
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- Eg. $`CO_2 \rightarrow`$ Carbon Diox**ide** $`\rightarrow`$ 2nd atom has `ide`.
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- $`CO \rightarrow`$ Carbon Monox**ide** $`\rightarrow`$ If 1st atom is mono, drop `mono`
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### Greek Prefix For Number Of Atom
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|Prefix|Name|Preifx|Name|
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|:-----|:---|:-----|:---|
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|1|mono|6|hexa|
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|2|di|7|hepta|
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|3|tri|8|octa|
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|4|tetra|9|nona|
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|5|penta|10|deca|
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- `Diatomic Molecules` The **gens**, Hydrogen, Nitrogen, Oxygen, Halogen
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### Common Names
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- $`NH_3 \rightarrow`$ Ammonia
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- $`H_2O \rightarrow`$ Water
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- $`CH_4 \rightarrow`$ Methane
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### Elements found As Molecules In Nature
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- $`H_{2(g)}, Cl_{2(g)}, Br_{2(g)}, I_2, N_2, O_2, F_2`$
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|Chemical Formula|Lewis Structure|What does the molecular model look like?|Name|
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|:---------------|:-------------:|:--------------------------------------:|:---|
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|$`H_2`$|<img src="http://www.chemspider.com/ImagesHandler.ashx?id=762&w=250&h=250" width="100">|<img src="https://cdn3.vectorstock.com/i/1000x1000/95/02/a-hydrogen-molecule-vector-20279502.jpg" width="100">|Hydrogen|
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