highschool/Grade 10/Science/SNC2DZ/Unit 1: Chemistry.md

Unit 1: Chemistry

• Matter - has mass, takes up space.
  • fundamental unit -> ATOMS

Atoms

• Atoms are the smallest unit of an element that still retains its properties
• Atoms are made of subatomic particles
• Relative Charge: compared to something.
• AMU = atomic mass units
• models allow people to make accurate preictions about the behaviour of matter
• atmoic notation \(`_{19}K`\)
• an isotope is an atom (or atoms) of an element with a unique # of neutrons

Name	Symbol	Relative mass (amu)	Location	Relative Charge
Protons	\(`p^+`\)	\(`1`\)	nucleus	\(`+1`\)
Neutrons	\(`n^0`\)	\(`1`\)	nucleus	\(`0`\)
Electrons	\(`e^-`\)	\(`~\dfrac{1}{2000}`\)	in orbit around nucleus (shell, energy level)	\(`-1`\)

IUPAC

Letter	Definition
I	International
U	Union
P	Pure and
A	Applied
C	Chemistry

• Involved in studying, varifying information (eg the periodic table -> Describes the elements -> pure susbtances made of only one kind of atom),and publishing.

Trends on the Periodic Table

Rows

• Same energy level in each period
• Same number of valence electrons in each group
• Across a row/period \(`\rightarrow`\) more \(`p^+`\) in nucleus \(`\rightarrow`\) greater attraction to \(`e^-`\)
• Atomic radius decreases as you move acroos a row/period, due to more protons in the nucleus that attract the negatives.
• Atomic radius is the from the center of the atom (nucleus) to the outer most shell (valence shell)

Columns

• down a column, increase of energy level, as you move down
• every atom has only one valence shell (cause its the most outer shell)
• if valence shell is further away from the nucleus, less attractive force between nucleus and valence \(`e^-`\)
• more energy levels where \(`e-`\) can be
• Negative electrons are repeling the valence shell electrons (shielding)
• Shielding “inner electrons” repel valence electrons and “block” attraction force between valence electrons and nucleus
• Atomic radius increases as you move down a column/group

Metals

• They tend to lose electrons
• They are shiny, ductile, malleable, conductive
• They have a weak/loose hold on electrons

Non-Metals

• They are dull, bad conductors - insulators
• Tend to gain electrons
• The have a strong hold on electrons

Bonds

• An ionic bond is a bond between a negative ion and a positive ion (so a anion and a cation)
• An convalent bond is a bond between 2 non-metals
• An ion is a charged particle
• An anion is formed when an particle gains electrons
• An cation is formed when an particle loses electrons
• We can use modesl(e.g Lewis dot diagrams) to show bonding
• 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 \(`Ar`\))
• 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 \(`+1`\))

Non Metal Ionic Names

Name	Name
Hydride	Boride
Carbide	Nitride
Oxide	Fluoride
Silicide	Phosphide
Sulphide/Sulfide	Chloride
Arsenide	Selenide
Bromide	Telluride
Iodide	Astitide