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

Unit 1: Chemistry

• Matter - has mass, takes up space.
  • fundamental unit -> ATOMS
• One formula unit - repeating strucure in an ionic compound taht has the simplest ratio of ions in the compound
• Ions are particles with charges

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
• Most metals are considered to be multi-metals
  • can form ions of differing charges
  • add roman numerals to the ions name to indicate its charge, for example, iron(\(`III`\)) oxide.

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

Chemical Nomenclature

• Naming and writing chemical formuals
• According to IUPAC
• Direct relationship beween chemical name and chemical structure

Formula	Name
\(`NaCl`\)	Sodium chloride
\(`K_3P`\)	Potassium phosphide
\(`Mg_3P_2`\)	Magnesium phosphide

Polyatomic Ions

• Ions that are made of \(`\ge 2`\) atoms.
• Molecules with a charge
• eg. \(`CaCo_3`\)
  • \(`Ca \rightarrow`\) Calcium ion \(`Ca^{2+}`\) (Cation)
  • \(`CO_3 \rightarrow`\) Carbonate ion \(`CO_3^{2-}`\) (Anion)
  • Calcium carbonate
• The ones that are not multi-valent are:
  • The first 20 elements
  • alkali metals
  • alkaline earth metals
  • non-metals (the ones hugging the staircase are also non-metals (some of the metalloids))
  • halogens
  • noble gases
• 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)
• If there is more than one polyatomic ion in a formula unit, then surround the ion with brackets
• Oxyanion are negative ions with oxygen in them

Polyatomic Ion Name	Formula (Always Remember The Charge!)
Ammonium	\(`NH_4^+`\)
Acetate	\(`CH_3COO^-`\)
Borate	\(`BO_3^{3-}`\)
Chlorate	\(`ClO_3^-`\)
Cyanide	\(`CN^-`\)
Hydroxide	\(`OH^-`\)
Nitrate	\(`NO_3^-`\)
Permanganate	\(`MnO_4^-`\)
Carbonate	\(`CO_3^{2-}`\)
Chromate	\(`CrO_4^{2-}`\)
Dichromate	\(`Cr_2O_7^{2-}`\)
Sulfate	\(`SO_4^{2-}`\)
Phosphate	\(`PO_4^{3-}`\)

Deriving Ions From Parent

Polyatomic Ion Name	Operation	Chemical Formula
Perchlorate	(add one extra oxygen to the parent)	\(`ClO_4^-`\)
Chlorate	(parent)	\(`ClO_3^-`\)
Chlorite	(has one less oxygen than the parent)	\(`ClO_2^-`\)
Hypochlorite	(has two less oxygens than the parent)	\(`ClO^-`\)

• Note that the charge remains the same
• Polyatomic ions in the same group on the periodic table from similar polyatomic ions

Chlorate	\(`ClO_3^-`\)
Bromate	\(`BrO_3^-`\)

Acidic Oxyanions

• Each hydrogen added to a polyatomic ion increases the charge by one, and c hanges the name:

Name	Chemical Formula
Hydrogen carbonate ion	\(`HCO_3`\)
Dihydrogen phosphate ion	\(`H2PO_4^-`\)
Monohydrogen phosphate ion	\(`HPO_4^{2-}`\)