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Property of Matter

- Chemistry: science concerned with the properties, composition, and behavior ofmatters.

- Matter: Anything that has mass and occupies space.- Mass: Amount of matter contained in a thing.- Properties: Qualities common to a thing or group of things.

Extensive (depend on the amount) Intensive

Physical (physical changes, state or form) Chemical (chemical changes)

- Kinetic energy: Any form of energy that cannot be stored.- Thermal energy(total) Temperature (average) Heat (transferred)- Operational definition (Observable characteristics) Conceptual definitions:

(Explain operational definition)

- Pure substance: same proportion, one set of properties. (element, compound)- Mixture: may be different proportion, several sets of properties.- Allotropes: different arrangement of same atoms.- Organic compound: compound with C and H

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- Binary compound: compound with two elements.- Acid (compound with H+) + Base (compound with OH-) = Salt- Homogenous mixture (appear same throughout, individual particles smaller than 1

micrometer) heterogenous mixture (appear different through out, larger than 1

micrometer)

Type Tyndall Effect Sediments Centrifugation Conceptual

Solution No No Not separated

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Formula (drawing)

- Molarity: # of moles of chemical per liter of solution.

Chemical Change

- Law of conservation of mass: mass of reactant = mass of product- Exothermic: releases heat (Synthesis A+B=C, Combustion Organic + O2 = CO2 + H2O)- Endothermic absorbs heat (Decomposition A=B+C)- Non-metal Oxide + water = Acid, Metal Oxide + water = Base- Single replacement (more reactive element will kick off less reactive one), Double

replacement (changes places)

- Neutralization: Acid + Base = Salt, exothermic- H = enthalpy change = change in energy. (endothermic positive due to absorbed

energy, exothermic negative due to released energy

- Thermochemical Equation: includes enthalpy change. If negative, then writepositive at reactant side.

- Limiting reactant (reagent) Excess reactant (reagent)- =

100%

- =

100%- Product expected = theoretical yield.

A Closer Look At Matter

- Daltons Atomic Theory: all matter are made up of atoms, they are identical toeach other, they combine in specific ratio, they separate and recombine to form

new compounds.

- J.J.Thompson discovers electron, Ernest Rutherford discovers protons are in nucleus,James Chadwick discovers neutron.

- Negative ion = anion, positive ion = cation.- Isotopes: same number of proton but different number of neutron.

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- Electrons can only be in orbits. To define electrons, we use quantum number- Quantum number: Principal (n, siza of atomic orbita), Angular Momentum (l,

shape of atomic orbital), Magnetic (, orientation in space), Spin (+0.5 or o.5)

- Total number of orbitals: n^2- Pauli exclusion principal (no 2 electrons can have same 4 quantum #s), Aufbau

principal (lowest energy orbitals gets filled first), Hunds rule (most stable is with

maximum number of unpaired electrons)

Relationship and Patterns in Chemistry

- Dimitri Ivanovich Mendeleevs periodic table god accepted due to earliness,focusing on chemical properties, leaving several blanks.

- Period: horizontal row/ Family: vertical row- Metals (shiny, solid except mercury, good conductor, malleable, ductile, flexible),

Non-metals (gases except bromine, dull, translucent, poor conductors), Metalloid

(semi-conductors)

- Alkali metals (soft, silvery solids, most reactive of metals), Alkaline metals (silver-coloured reactive metals), Halogens (most reactive elements, all three states

present), Noble gases (most non-reactive)

- Transition elements: metals, hard solids, high melting & boiling points.- Periodic trends: Trend that is shown when going across or down the periodic table.- Covalent Radius (one half of diatomic particles) Metallic radius (one half of crystal)- Atomic radius increases as go down, as go left. (more electrons = more repulsion tho)- Ionization Energy (minimum energy required to remove an electron) increases as

go up, go right.

- Electronegativity (relative ability of a bonded atom to attract shared electronscloser to their nuclei) increases as go up, go right.

- EN (0= non-polar covalent, 0

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x>1.7 = ionic)

- Lewis structure diagram: fills in electron from right, top, then clockwise. Find out ionby counting electrons & protons.

- Intramolecular forces (chemical bond within molecules), intermolecular forces(forces between molecules)

- Dipole-dipole force: attraction force between polar molecules- Hydrogen Bonds: dipole-dipole including H-N,O,F- Dispersion Force: attraction due to sudden movement of electrons. Everywhere- Ion-dipole force: attraction between ion and polar- Hydration shell: ions covered by water.

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Solution Chemistry

- Solution: Homogenous mixture in one phase. (Solute = dissolved, solvent = dissolving)- Miscible (can be mixed in any proportion) Immiscible.- Solubility: Maximum amount of solute that will dissolve in a given amount of

solvent at a particular temperature.

- Soluble: More than 0.1mol of solute can be dissolved in 1.0L of solution at 25C- Insoluble: Less than 0.1mol of solute can be dissolved in 1.0L of solution at 25C- All alkali ions, hydrogen, ammonium, nitrate are soluble.- Unsaturated (solute completely dissolved), Saturated (no more solid will dissolve),

Supersaturated (more solute is dissolved than maximum)

- Like dissolves like: Polar-> Ionic, Polar / Non-polar-> non-polar- Methanol, Ethanol, Propanol are soluble in polar, Butanol, Pentanol are partly

soluble. Longer chains are almost insoluble.

- Soap (non-polar tail with polar head) acts as emulsifying agent, making immiscibleliquids become a ball and float around. This clump is called micelle.

- Solvation: Process of solvent molecules surrounding solute particles. (If solvent =water, hydration)

- Ionization Equation: Complete Ionic Equation (Everything), Net Ionic Equation(Complete spectator ions)

- Spectator Ions: Ion that stays the same (not forming solid)- Electrolyte (Good = good conductor, bad = bad conductor)- Strong acid/Strong base->dissociate 100%, Weak acid/Weak base->dissociate little.- Titration: Method used to determine the concentration of an unknown solution by

reacting with another substance of known concentration.

- Standardized Solution: Known concentration. Put in burette and poured untilreaction stops.

- Equivalence point (moles of H+ = moles of OH-) Endpoint (indicator changes color)

Organic Chemistry

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- Alkanes: Saturated.- Substituent groups: Branches of carbon atoms.- Meth (1), Eth(2), Prop(3), But(4), Pent(5), Hex(6), Hept(7), Oct(8), Non(9), Dec(10)- Naming branch: -yl (ex: 3-methylbutane)- Structural isomers: Same formula but different structure.- Cycloalkanes: Cyclic structure. (ex: 1,4-dimethylcycloheptane, 2-cyclobutylpentane)- Alkenes: Unsaturated(reactive, other atoms could attach to carbon)- Geometric isomers: Same structure but different orientation (ex: cis-, trans-) Only

comes before the main structure, not before branch groups.

- Aromatic: Includes Benzene. In branch group, called Phenyl-

Gas Law

- = (R=8.31kPa L / mol k) (1 atm = 101.3kPa = 760.0 torr=760.0mmHg)- Boyles Law: = - Charles Law: = - Avogadros Law:

=

- Daltons law of partial pressure: Total V depends on # of moles. = + +,

=

- Absolute Zero: -273.15C, 0K, nothing moves.- =

- Standard molar volume: 22.4L at STP- STP = 0C -> 1 atm.

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Memorize: Alkane, Alkene, Alkyne, Aromatic, Alkyl Halide, Alcohol, Ether, Aldehyde,

Ketone, Carboxylic Acid, Ester, Amine, Amide