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82 lines
3.3 KiB
Markdown
82 lines
3.3 KiB
Markdown
# Unit 1: Chemistry
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- Matter - has mass, takes up space.
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- fundamental unit -> ATOMS
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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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- Atoms are made of subatomic particles
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- Relative Charge: compared to something.
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- AMU = atomic mass units
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- models allow people to make accurate preictions about the behaviour of matter
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- atmoic notation $`_{19}K`$
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- an isotope is an atom (or atoms) of an element with a unique # of neutrons
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|Name |Symbol|Relative mass (amu)|Location|Relative Charge|
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|:--------|:-----|:------------------|:-------|:--------------|
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|Protons |$`p^+`$| $`1`$ |nucleus | $`+1`$ |
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|Neutrons |$`n^0`$| $`1`$ |nucleus | $`0`$ |
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|Electrons|$`e^-`$|$`~\dfrac{1}{2000}`$|in orbit around nucleus (shell, energy level)|$`-1`$|
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## IUPAC
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|Letter|Definition|
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|:-----|:---------|
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|I|International|
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|U|Union|
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|P|Pure and|
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|A|Applied|
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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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## Trends on the Periodic Table
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## Rows
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- Same energy level in each period
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- Same number of valence electrons in each group
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- Across a row/period $`\rightarrow`$ more $`p^+`$ in nucleus $`\rightarrow`$ greater attraction to $`e^-`$
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- Atomic radius decreases as you move acroos a row/period, due to more protons in the nucleus that attract the negatives.
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- Atomic radius is the from the center of the atom (nucleus) to the outer most shell (valence shell)
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## Columns
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- down a column, increase of energy level, as you move down
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- every atom has only one valence shell (cause its the most outer shell)
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- if valence shell is further away from the nucleus, less attractive force between nucleus and valence $`e^-`$
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- more energy levels where $`e-`$ can be
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- Negative electrons are repeling the valence shell electrons `(shielding)`
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- `Shielding` "inner electrons" repel valence electrons and "block" attraction force between valence electrons and nucleus
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- Atomic radius increases as you move down a column/group
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## Metals
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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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## Non-Metals
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- They are dull, bad conductors - insulators
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- Tend to gain electrons
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- The have a strong hold on electrons
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## Bonds
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- An ionic bond is a bond between a negative ion and a positive ion (so a anion and a cation)
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- An convalent bond is a bond between 2 non-metals
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- An ion is a charged particle
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- An anion is formed when an particle gains electrons
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- An cation is formed when an particle loses electrons
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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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## Non Metal Ionic Names
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|Name|Name|
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|:---|:---|
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|Hydride|Boride|
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|Carbide|Nitride|
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|Oxide|Fluoride|
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|Silicide|Phosphide|
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|Sulphide/Sulfide|Chloride|
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|Arsenide|Selenide|
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|Bromide|Telluride|
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|Iodide|Astitide|
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