General Chemistry 1: Finals

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What are the 6 Parts of a Lab Report?

1.) Theoretical Framework (Hypothesis & Objectives)
2.) Materials & Procedures
3.) Data & Results
4.) Analysis & Discussion
5.) Conclusion
6.) References

How do you handle chemicals and equipment?

• Corrosive Flames = Flame Hood

• Pour acid into water

• Never bring reagent bottles to desk

What are the 9 Safety Labels?

IG FACE OHH (😟)

What is Chemistry?

The study of the structure, function, properties of matter, and its changes.

What are the 5 Classifications of Matter?

1.) Solid

2.) Liquid

3.) Gas

3.) Plasma

4.) Bose-Einstein Condensate

What is a Liquid?

2.) Liquid

• slide past

• assume shape of container

• slow diffusion

• high density

• low heat expansion

What is a Gas?

3.) Gas

• free and straight-line motion

• compressible

• fill container

• rapid diffusion

• high heat expansion

What is Plasma?

3.) Plasma

• ionized gas & free electrons

• exists

What is Bose-Einstein Condensate?

4.) Bose-Einstein Condensate

• low-temp near zero

• hypothetical superfluid

What are the Physical Properties of Matter?

• 5 Senses

  • Texture, luster, odor, sound

• Phase at room temperature

• Numerical description

  • Density

  • Freezing/Boiling Point

• Change in phase

What are the Chemical Properties of Matter?

• Atmospheric Oxygen

  • Flammable/Non-Flammable

  • Flash point

• Water

  • Dissolve, Rust, React

• Acids

  • Corrosive

• Change in composition

  • Burning

What is an Intensive Property?

• identifier/independent of amount

• color, temperature, density, melting/freezing/boiling point

• tell difference between oil, water, alcohol

What is an Extensive Property?

• depends on amount

• description

• vol, mass, energy, enthalpy, entropy, length

What is Heterogenous Matter?

• Non uniform mixture

• No constant properties/composition

What is Homogenous Matter?

• Uniform mixture

• No constant properties/composition

What is an element?

A pure substance that cannot be chemically simplified.

• Constant properties and composition

What is a compound?

Pure substance that CAN be chemically simplified

• Constant properties and composition

• Law of definite composition

What are the 9 Separation Techniques?

(PC FMMEDDD) 😟

1.) Paper Chromatography
2.) Centrifugation
3.) Filtration
4.) Mechanical
5.) Magnetic
6.) Evaporation
7.) Distillation
8.) Decanting
9.) Density

What is Paper Chromatography?

• Molecular attraction (Polarity)

  • Separate plant pigment & dyes

What is Centrifugation?

• Circular motion to sink denser objects

  • DNA from blood

What is the difference between Filtration & Mechanical?

Filter: Trap solid to seep liquid/solid

Mechanical: By hand, color & shape

What is the difference between Evaporation and Distillation?

Evaporation: vaporize liquid to leave solid

Distillation: boiling point separates both liquids

What is the difference between Decanting and Density?

Decant: Pour off liquid based on density

Density: Components cant be soluble with each other

What is the Kinetic Molecular Theory of Gases?

A model that explains gases under normal temperature & pressure ideal in our environment

• Heavier particles decrease velocity to maintain equal KE

• Lighter and heavier particles transfer the same pressure

• PVT is negligible to mass

What are the 5 properties of gases?

1.) Have mass
2.) Are compressible
3.) Take the shape of the container
4.) Move through each other (Diffuse)
5.) Pressure (collisions) dependent on Temp

What are the 5 Postulates?

1.) Gases are small & widely separated (↓Volume ↓ Density ↑ Compress)
2.) Particles are independent

• Unless colliding

• No attractive/repulsive forces

3.) Rapid straight motion until collision

• Perfectly elastic (no net loss of energy in transfer)

4.) Pressure of gas = ∑ collisions

• pressure proportional to no. of gas particles & smaller volume

5.) Average KE depends only on absolute temp

• KE = mv²/2

• Ar, CO2, H2 → Same KE, H₂ lightest = greatest velocity

What is amu?

Amount of gas (n) where,

n = given mass / molar mass

List all Pressure Conversions for 1 atm

1 atm = 760 torr

760 mmHg

101,325 Pa

101.325 kPA

1.01325 bar

14.7 psi

Volume conversions

1 L = 1000 mL
1 m³ = 1000 L

Celcius to Kelvin Conversion

C + 273 = K

What is Boyle’s Law?

PV = k
Pressure inverse to Volume at constant Temp

• Isothermal
  → Breathing

What is Charles’ Law?

V/T = V/T volume and temperature direct

• Isobaric
  → Hot air balloon

What is Gay-Lussac’s Law?

P/T = P/T pressure and temperature direct

• Isochoric

What is Avogradro’s Law?

V/n = V/n isothermal and isobaric

Molar volume = 22.4L

What is the Ideal Gas Law/Combined Gas Law?

Combined: PV/T = k

Ideal: PV = nRT

T = 273K
P = 1 atm
n = 1 mol (m/mm)
V = 22.414 L
R = 0.0821 Latm/molK

What is Dalton’s Partial Pressure?

• Gases in a mixture behave independently & exert the same pressure if alone

Density (g/L) = mass/volume
Molar Mass (g/mol)= mRT/VP or DRT/P

Partial pressure: get mols → use PV=nRT
Mole fraction: ∑ mols → X = nA/nT → P = Xa * Pt

Who made the early models of the Atoms?

• Leucippus & Democritus

  • Indivisible atomos

  • 1 Makeup

What is Conservation of Mass?

• Antoine Lavoisier

• Mass remains the same before and after a reaction

What is the Law of Definite Proportions?

• Chemical composition of substances in fixed, whole number rations

Who made the Billiard Ball Model?

Dalton (Electrolysis)

• Indivisible atoms

• Mass & Properties

• Atomic Ratios

• Reactions

Who discovered the electron?

JJ Thompson (Corpuscle)

• Plum Pudding

• Cathode Ray Tubes

• electron is the lightest!

Who discovered the Proton?

Eugen Goldstein

Who discovered the Nucleus & Neutron?

Rutherford

• Nuclear model

James Chadwick

• Nuetron

Who made the Planetary model?

Bohr

• electrons orbit

• quantized energy

• E PN

Who made the Electron Cloud Model?

Schrodinger

• no fixed orbit, just probabilities

What is an isotope?

• same element (p+ as fingerprint), different neutrons

A → mass number (p+ + n)

Z → atomic number (p+, if no charge, = e-)

Calculating Percent Abundance

• Multiply amu * decimal %

  • amu(x) + amu(1-x) = total amu

Cation & Anion electron relationship

• C+ lessen electrons

• A- add electrons

  • from Atomic No.

Quantum Numbers

n → principle energy level

• transition: -1

• f block: -2

l → azimuthal/angular momentum:

• s = 0

• p = 1

• d = 2

• f = 3

• 0 to l-1

ml → magnetic

• +- l

ms → spin

• +- 1/2

Aufbau Principle

Electrons occupy lowest first

Pauli’s exclusion

No more than 2 electrons occupy

Hunds Rule

Electrons occupy the same sublevel before opposing spin

What electrons are in the noble gas config?

Core electrons

Period Trends

• Rows 1 to 7

• No common trends

  • 1st element active & solid, last is inactive gas

Group IA

• Alkali/Alkaline Metal

• Silvery & soft enough to cut

• Found in nature

Group IIA

• Alkali/Alkaline Earth

• harder, denser, stronger

• higher melting point

• less reactive

Transition (B Families)

• good conductors of heat & electricity

• bright color in paint (1 to 2 valence)

Boron Group

• 3 valence

• metalloids stairstep

• aluminum as most abundant element

Carbon group

• 4 bonding sights

• carbon as basis of life

Nitrogen Group

• 78% in atmosphere

• 5 shared electrons

Metal Properties

• Solid at room temp

• Lose electrons

• malleable, ductile, metallic luster, conductor of heat & electricity (except Hg)

Non metal properties

• NOT malleable, ductile, etc

• gas at room temp (mostly)

• gain e-

Mettaloid

• high electrical conductivity

4 Periodic Trends

• Atomic Radii (right down)

  • The greater the attraction, the smaller

  • Pauling scale

• Ionic Size & Radii (down)

  • Most negative biggest, most positive smallest

• Ionization Energy (up left)

  • small IE → cation

  • to remove an electron

  • Big increase = noble gas octet

• Electrogenativity (up left)

  • attract electron

What are the properties of an ionic compound?

• crystalline lattice solid

• high melting point/boiling

• hard brittle solid

• non conductors in solid

• electrolytes in aqueous

• good insulators

• exothermic

• metal & nonmetal

What are the EN differences?

Non-Polar Equal: 0 - 0.4
Polar Unequal: 0.5 - 1.7
Ionic: 1.8 and above

What is VSEPR?

Valence Shell Electron Pair Repulsion

EDG: Domains alone
MG: With Lone Pairs

Relationship of Light Wavelength to Energy

Indirect

What do atoms do when they receive energy?

Ground state → Excited State

Carbohydrates

• Hydroxyl (-OH) and Carbonyl (C-O)

• adlehyde →aldose→hemiacetal→acetal

• ketone→ketose→hemiketal→ketal

• glycogen, cellulose, pectin, starch

• glycosidic bonds

Lipids

• Glycerol, ester carboxylate (OH), ester phosphate, alcohol group

• ester bond

Protein

• amino acid, hydrogen, amino group, carboxyl group, r group

• peptide bond

Biomolecule Reactions

• Addition

  • 2+2 = 1

• Condensation

  • Dehydration

• Esterfication (carbs)

  • acid = alcohol

• Combustion

  • complete

  • incomplete

• Saponification (Lipid)

• Ubiquitination (Protein)

Covalent Bond Properties

• 2 non metals sharing

• dipole

  • magnitude of charge & bond length

• periods 3 above are expanded

What are the properties of non-polar bonds?

• monoatomic, diatomic, etc

• noble gas

• hydrocarbon (C and H)

• symmetry

• no dipole

Whar are the properties of polar bonds?

• H + NOF

• Lack Symmetry