Science 10 - Chemistry - Part 1

First half of chemistry content of science 10 (AB). Organized based on what made sense to my brain at 2:30AM on the fifth of january. Common sense stuff and naming omitted

Atomic Theory - Aristotle

All matter is composed of combinations of fire, water, air, and earth (400 BC)

Atomic Theory - Democritus

All matter is composed of tiny particles that could not be divided (400 BC, less popular theory)

Atomic Theory - John Dalton

Everything was made up of atoms which looked like tiny spheres (Billiard Model) which varied in properties. Proposed particle theory

Atomic Theory - JJ Thomson

Discovered the electron. Developed Plum Pudding model of the atom which involved the electron.

Atomic Theory - Ernest Rutherford

Discovered nucleus of an atom, discovered via the gold foil experiment. Concluded majority of the atom was empty space. Developed the Nuclear Model.

Atomic Theory - Neils Bohr

Proposed electrons surround the nucleus at various energy levels (shells). Developed the Planetary/Bohr Model.

Atomic Theory - Erwin Schrodinger

Proposed electrons exist in electron clouds (orbitals), not specific energy levels, using quantum mechanics. Developed Electron Cloud Model

Atomic Model - Dalton’s Billiard Model

Solid sphere to represent atoms

Atomic Model - JJ Thomson’s Plum Pudding Model

Positive sphere dotted with negatively charged areas (electrons)

Atomic Model - Ernest Rutherford’s Nuclear Model

Distinguished nucleus in the center, surrounded by electrons

Atomic Model - Neils Bohr’s Bohr/Planetary Model

Distinguished nucleus in the center, surrounded by energy levels of electrons that followed 2, 8, 8 rule

Atomic Model - Erwin Schrodinger’s Electron Cloud Model

Distinguished nucleus in the center with areas of electrons surrounding it

Particle Theory

1. Matter is made up of tiny particles

2. Particles are in constant motion

3. Held together by forces (Bonds)

4. Particles have empty space between them

Classification of Matter

1. Pure Substances (Elements, Compounds)

2. Mixtures (Homogeneous, Heterogeneous)

Elements

Can exist as atoms or molecules (singular atoms vs multiple atoms). Basic unit, cannot be broken down further

Ion

A change in the number of electrons in an atom (Can be positive or negative through loss or gain of an electron)

Isotope

A change in the number of neutrons in an atom’s nucleus. Changed notation displays atomic mass

Compound

2 or more elements (ions/atoms) bonded together. Can be molecular or ionic (2 non-metals vs 1 non-metal and 1 metal)

Ionic Compound

1 negative non-metal (anion) and 1 positive metal (cation) bonded together through transfer of electrons. Include bonded polyatomics. (Properties: High melting points, high conductivity, solid at room temperature, most water soluble, can form precipitates)

Precipitate

Solid substance in a solution

Molecular Compound (Covalent Compound)

2 non-metals bonded together through the sharing of electrons. (Properties: Low melting points, low conductivity, can be any state at room temp, low water solubility)

H₂O

Water

C₆H₁₂O₆

Glucose

O₃

Ozone

H₂O₂

Hydrogen Peroxide

NH₃

Ammonia

C₁₂H₂₂O₁₁

Sucrose

CH₄

Methane

C₃H₈

Propane

CH₃OH

Methanol

C₂H₅OH

Ethanol

H₂S

Hydrogen Sulfide or Hydrosulfurous Acid

Diatomics

Elements that are naturally found as molecules (multiple). Include I, Br, Cl, F, O, N, H + P4, S8

Periodic Table

Developed by Mendeleev to organize various discovered elements. Composed of 16 groups (vertical) and 7 periods/families (horizontal)

Transition Metals

Found on left/middle of periodic table. Elements that conduct heat/electricity, are malleable, ductile, and lustrous

Metalloids

Found in area around staircase. Share properties of metals and non-metals

Non-metals

Found on right side of periodic table, above staircase. Elements are non-conductive and brittle as solids

Periodic Table - Periods/Families

Horizontal organization of elements, based on increasing atomic number from left to right.

Periodic Table - Groups

Vertical organization of elements, elements in the same group have the same number of valence electrons and thus similar reactivity

Alkali Metals

Group 1 on the periodic table. Very reactive with water/water soluble. Have 1 valence electron, more reactive going down the group.

Alkaline Earth Metals

Group 2 on the periodic table. Have 2 valence electrons, tend to for 2+ ions.

Halogens

Group 17 on the periodic table. Readily reacts with Alkali Metals ti form salts. Has 7 valence electrons, more reactive going up the group

Noble Gases

Group 18 on the periodic table. Very unreactive with other elements due to full valence shells.

Lewis Dot Diagrams/Lewis Structures

Diagrams that show only the valence electrons around the element symbol

Solubility

Refers to the ability of a substance (solute) to form a solution

Aqueous

Soluble in water

pH

Measurement of how acidic or basic a substance is

Acid

A substance with a pH lower than 7. Involve H⁺ ions, H at beginning (or at end if COO). Molecular substances, water soluble, conductive, corrodes metals

Base

A substance with a pH greater than 7. Involves OH^- ions or ammonium. Molecular or ionic substances, water soluble, conductive

Neutral Substance

Substances with pH’s exactly at 7.

Indicators

Tests used to identify if a substance is an acid or base. (ie litmus paper)

Neutralization

Reaction between acids and bases that results in a pH of 7. H⁺ ions must react with OH^- ions to create water, ionic salts are also produced