IB Chemistry Quiz 1.

• Pure substance composed of identical atoms.

• Atoms of the same element are identical.

Smallest particle of an element, exhibiting its characteristic properties.

Imparts unique properties to each element.

Some exist naturally in pure, uncombined forms.

• Combination of different elements with fixed ratios.

• Held together by chemical bonds, altering properties.

• Blend of substances with distinct properties.

• Variable composition.

Uniform throughout, consistent properties.

Non-uniform, varying properties.

1. Filtration: Solids separated from liquids.

2. Recrystallization: Substance crystallized from a solution.

3. Distillation: Separation by boiling and condensation.

4. Paper Chromatography: Separation based on adsorption.

Solids removed from liquids using a filter.

Substance isolated from a solution via a solvent and crystallization.

Separation through selective boiling and condensation.

Components separated based on adsorption to a solid phase.

• Matter exists in different states due to temperature and pressure.

• States depend on particle energy.

• Temperature relates to average kinetic energy.

• State determined by inter-particle forces.

• Measures average particle kinetic energy.

• E_k

Dense, fixed shape and volume, no atom compression.

Less dense, takes container shape, fixed volume.

Spreads to fill space, no fixed shape or volume, compressible.

Liquids and gases due to flow ability.

Particles evenly disperse via random movement.

• Energy linked to motion.

• Inverse mass-velocity relationship.

• Increases with temperature.

• State changes occur at fixed temperature and pressure.

• Include sublimation, deposition, vaporization, condensation, melting, freezing.

Liquid to gas via evaporation or boiling.

Gas to solid (e.g., frosting).

Solid to gas without liquid phase (e.g., dry ice).

Surface liquid to gas below boiling point.

Liquid becomes gas throughout.

All molecules become gas.

• Liquid's pressure on container walls.

• Boiling when equals atmospheric pressure.

Energy shifts inter-particle forces, not temperature.

• a-b: Solid heats, temperature rises.

• b-c: Melting point, temperature constant.

• c-d: Liquid heats, temperature rises.

• d-e: Boiling point, temperature constant.

• e-f: Gas heats, temperature rises.

• Absolute temperature scale.

• Absolute zero at 0 K (-273.15°C).

Temperature (K) = Temperature (°C) + 273.15.

• Nucleus with protons and neutrons.

• Electrons orbit outside nucleus.

• Mass Number (A) = Protons + Neutrons.

• Atomic Number (Z) = Protons.

• Formed by gaining or losing electrons.

• Cations: Lose electrons, positive charge.

• Anions: Gain electrons, negative charge.

• Same protons, different neutrons.

• Similar chemistry, distinct physical properties.

• Calculated from isotope abundance and mass.

• Measures individual atom mass.

• Presents percent abundance vs. mass/charge ratio.

Varies in energy forms.

Travel at constant speed, different wavelengths.

Waves passing a point per second.

c = λv (c: speed of light, λ: wavelength, v: frequency)

Energy increases with frequency.

• Absorption: Radiation absorbed by atoms.

• Emission: Atoms emit light when electrons return to lower energy levels.

• Unique line spectra for different elements.

• Used for element identification.