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Atom
The building block of all matter, made up of protons and neutrons in the nucleus and electrons orbiting in shells.
Modern Atomic Theory
Proposed by John Dalton, stating that each element consists of the same type of atom unique to that element.
Plum Pudding Model
A model by JJ Thomson depicting the atom as a positive sphere filled with electrons.
Photon
A quantum of light, showing energy emitted or absorbed by an atom during transitions between allowed energy states.
Bohr Model
A representation by Niels Bohr where electrons orbit the nucleus in defined energy levels.
Heisenberg Uncertainty Principle
States we cannot know both the exact location and the speed of a particle with high accuracy.
Electron Cloud Model
Developed by Erwin Schrödinger, it describes the probabilistic locations of electrons around the nucleus.
Ionization Energy
The amount of energy required to remove an electron from an atom.
Periodic Trends
Patterns observed in the properties of elements across periods and groups in the periodic table.
Electrostatics
The study of electric charges that can be collected and held in one place.
Coulomb's Law
F=kq1q2/r^2, which describes the strength of electrostatic forces between two charges.
Electric Current
The flow of electric charge, calculated as I=q/Δt.
Ohm's Law
The relationship between voltage, current, and resistance in a circuit, expressed as V=IR.
Series Circuit
A circuit configuration where there is a single path for current to flow.
Parallel Circuit
A circuit with multiple paths for current to flow.
Resistance
A measure of the opposition to current flow, typically expressed in ohms.
Noble Gas Configuration
The electron configuration of an atom that matches the configuration of the nearest noble gas.
Basic Properties of Metals
Metals are malleable, ductile, conductors of electricity and heat, and metallic colored.
Valence Electrons
Electrons in the outermost shell of an atom that are involved in chemical reactions.
Octet Rule
The concept that atoms tend to gain, lose, or share electrons to have eight electrons in their valence shell.
Electronegativity
The ability of an atom to attract electrons in a chemical bond; measured on a scale.
Electrolytic Cell
A type of cell that uses electrolysis to drive a non-spontaneous chemical reaction.
Ionization Energy Formula
The amount of energy required to remove an electron from an atom, often expressed in joules or electronvolts.
Electric Field Strength Formula
E = F/q, where E is the electric field strength, F is the force, and q is the charge.
Power Formula in Electrical Circuits
P = IV, where P is power, I is current, and V is voltage.
Rutherford's Gold Foil Experiment
Demonstrated that atoms have a small, dense nucleus and that most of the atom is empty space, providing evidence against the plum pudding model.
Thomson's Cathode Ray Experiment
Discovered electrons as negatively charged particles, leading to the development of the plum pudding model of
Equivalent Resistance
The total resistance of a circuit or combination of resistors that can replace the original resistors without changing the current or voltage in the circuit.
Formula for Equivalent Resistance in Series
R_eq = R_1 + R_2 + ... + R_n, which states that the equivalent resistance is the sum of individual resistances in a series circuit.
Formula for Equivalent Resistance in Parallel
1/R_eq = 1/R_1 + 1/R_2 + ... + 1/R_n, which states that the inverse of the equivalent resistance is the sum of the inverses of individual resistances in a parallel circuit.
Power Formula in Electrical Circuits
P = IV, where P is power, I is current, and V is voltage. Alternatively, P = I²R or P = V²/R, showing power in terms of resistance (R) and current (I) or voltage (V) respectively.
Coulomb's Law
F = k(q1q2)/r^2, which describes the strength of electrostatic forces between two charges.
Sublevel
A subdivision of an electron shell in an atom, represented by the letters s, p, d, and f, which indicate the shape and energy of the orbitals.
Work (W) formula
The formula for work done is W = fd = Eqd, where W is work, f is force, d is distance, E is electric field strength, and q is charge.
Polarization
Separation of charges by induction
Periodic Trends
Patterns observed in the properties of elements across periods and groups in the periodic table.
Atomic Radius Trend
Atomic radius tends to increase down a group and decrease across a period from left to right.
Ionization Energy Trend
Ionization energy tends to decrease down a group and increase across a period from left to right.
Electronegativity Trend
Electronegativity tends to decrease down a group and increase across a period from left to right.
Electron Affinity Trend
Electron affinity tends to become more negative across a period and varies less predictably down a group.
Metals
metallic colored, malleable, ductile, conductors of electricity and heat.Metals are on the left of representatives, all the transition metals (including actinides and lanthanides)
Metalloids:
Brittle, semiconductor, solid, between non-metal and metal, metallic luster
Staircase between metal and non-metal (7 total)
Non-metals
Hydrogen and the right of the table or staircase.
High ionizations, electronegative, poor conductors , brittle solids, no luster, dull.
