Chemistry: 1st Achievement Test

Organic Chemistry

: studies the structure, properties, and composition of carbon-containing compounds / form basis of life and many industrial products.

Inorganic Chemistry

: investigates properties, structures, and reactions of compounds without carbon.

Physical Chemistry

: merges principles of physics and chemistry to understand the physical properties of matter using concepts like thermodynamics, quantum mechanics, and kinetics.

Analytical Chemistry

: develop methods identify and quantify the components of substances, determining their composition and concentration.

Biochemistry

: focuses on the chemical processes and substances occurring within living organisms.

Environmental Chemistry

: examines chemical processes occurring in the environment and studies methods to mitigate environmental damage.

Research Scientist

: conducts experiments, analyzes data, and discovers new application for compounds (e.g. pharmaceuticals, material science, biotechnology).

Chemical Engineer

: applies chemical principles to improve processes and products (e.g. manufacturing, energy production, environmental remediation).

Analytical Chemist

: develops techniques to analyze substances (e.g. quality control in manufacturing, forensic analysis).

Pharmaceutical Scientist

: develops new drugs and improve medications by understanding their chemical properties and reactions to the body.

Chemical Physics

: examines the fundamental physical principles underlying chemical phenomena.

Material Sciences

: explores the properties and applications of materials in chemistry by understanding their composition and behavior.

Kinetic Molecular Theory

: explains the microscopic properties of atoms which lead to macroscopic properties (pressure, volume, temperature) / explains why matter exists in different phases and how matter changes from one phase to the next.

Matter

: made up of particles that are constantly moving.

Energy

: varies depending on temperature / determines whether the substance exists in solid, liquid, or gaseous state.

Solid Phase

: states with least amount of energy.

Gaseous State

: state with greatest amount of energy.

Temperature

: measure of average kinetic energy of particles.

Change in Phase

: occur when the energy of particles are changed.

Intermolecular Forces

: attractive forces between atoms that become stronger as they move closer together.

Van der Waals Forces

: “LDF” / attraction and repulsions between atoms, molecules, and surfaces.

Dipole Interactions

: when partial charges in a molecule are attracted to an opposite partial charge in another molecule / polar molecules align so that the positive end interacts with the negative end.

London Dispersion Force

: temporary attractive force / electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles / “induced dipole reaction” / cause nonpolar substances to condense to liquids and freeze into solids when temperature is lowered.

Polar Molecules

: occur when there is an electronegativity difference between bonded atoms.

Nonpolar Molecules

: occur when electrons are shared equally between atoms of a diatomic molecule or when polar bonds in a larger molecule cancels each other out.

Hydrogen Bond

: attractive force in the hydrogen attached to an electronegative atom of two different molecules which are usually oxygen, nitrogen, or flouride.

Liquid State

: an intermediate phase between solid and gas / subject to intermolecular attraction / volume is constant / have limited compressibility.

Evaporation

: changing from a liquid or solid state into vapor (e.g. fog, mist, steam).

Boiling Point

: temperature at which the vapor pressure of a liquid equals the surrounding pressure, wherein liquid changes into vapor / liquid in a partial vacuum has a lower boiling point than a liquid at atmospheric pressure.

Vapor Pressure

: tendency of a material to change into the gaseous state / increases with temperature / the higher the vapor pressure, the higher the tendency for a material to vaporize.

Surface Tension

: property of a surface of a liquid that allows it to resist an external force due to the cohesive nature of water molecules.

Solids

: extended 3-dimensional arrangement of atoms, ions, & molecules locked into position.

Crystal Lattice

: regular repeating 3-dimensional array.

Crystalline Solids

: regular pattern, well-defined edges and faces, diffract x-rays, and sharp melting points / distinctive internal & flat structures / produce distinctive patterns.

Amorphous Solids

: irregular or curved surfaces / do not give well-resolved x-rays / melt over a wide range of temperatures / almost any substance can solidify in amorphous form if the liquid is cooled rapidly enough.

Crystalline Faces

: faces of crystals can intersect at right angles (e.g. galena, pyrite, quartz).

Cleavage Surfaces

: curved, irregular surfaces when cleaved (e.g. obsidian).

Obsidian

: volcanic glass with same chemical composition as granite.

Crystalline

Amorphous

Glass

: an amorphous, translucent solid.

Lattice of Quartz

: atoms of this crystalline form a regular arrangement consisting of linked tetrahedra.

Solution

: homogenous mixture of 2 or more substances.

Solvent

: dissolves the solute / greater in quantity / determines state of matter of the solution.

Solute

: dissolved by the solvent / lesser in quantity.

Concentration

: refers to amount of solute in a solution or solvent.

Water

: “universal solvent” / polar arrangement of oxygen and hydrogen atoms allows its molecules to be attracted to various molecules.