Electronic Structure & Periodic Properties

These flashcards contain key terms and definitions related to electronic structure and periodic properties, designed to aid in understanding and memorization for the exam.

Waves

Oscillation of periodic movement that can transport energy from one point in space to another.

Wavelength

Distance between two peaks or troughs.

Frequency

Number of wavelengths that pass a given point in one second.

Amplitude

Half the distance between a peak and trough (vertically).

Electromagnetic Wave

A wave with an electric field oscillating in step with a magnetic field, both perpendicular to the direction of travel.

Interference Pattern

The pattern formed by two or more overlapping waves.

Constructive Interference

When waves overlap and enhance each other, resulting in light regions.

Destructive Interference

When waves overlap and cancel each other out, resulting in dark regions.

Photoelectric Effect

Phenomenon where electrons are ejected from a metal surface when light of a sufficient frequency shines on it.

Energy of a photon (E)

The energy carried by a single photon, calculated using the equation E = hν.

Planck's Constant (h)

A constant used to calculate the energy of photons, approximately 6.626x10^-34 J·s.

Line Spectrum

The spectrum produced by an element that shows discrete wavelengths of light, indicating specific energy levels.

Bohr Model

A model of the atom where electrons move in fixed orbits around the nucleus.

Bound Electron

An electron with energy less than zero, indicating it is associated with an atom. E < 0

Free Electron

An electron that has sufficient energy to be free from the attraction of the nucleus. E > 0 

Pauli Exclusion Principle

No two electrons in the same atom can have the same set of four quantum numbers.

Valence Electrons

Electrons in the highest energy level of an atom that participate in chemical bonding.

Core Electrons

Electrons that are not involved in bonding and are located in inner shells.

Cation

A positively charged ion, smaller than the neutral atom from which it is derived.

Anion

A negatively charged ion, larger than the neutral atom from which it is derived.

Charge = 18 - Group

Isoelectronic

Atoms and ions that have the same electron configuration.

Ionization Energy (IE)

The energy required to remove an electron from a gaseous atom.

always positive and endothermic

AR increase IE decreases

Effective Nuclear Charge (Z_eff)

The net positive charge experienced by an electron in a multi-electron atom.

Electron Affinity

The change in energy when an electron is added to a neutral atom to form a negative ion.

Atomic Radii

The size of an atom, usually measured from the nucleus to the boundary of the surrounding cloud of electrons.

Electron Configuration

The distribution of electrons in an atom's orbitals.

Transition Metals

Elements in the d-block of the periodic table with unique properties and electron configurations.

remove ns first than (n-1)d

Quantum State

The state of an electron as described by its quantum numbers.

de broglie wavelength

The wavelength associated with a moving particle, calculated using the momentum and Planck's constant, representing wave-particle duality.

IE exceptions

Be-B, O-N, Al-Mg, S-P

Polar covalent bonds to memorize

0.4 < EN < 1.8 non metal - non metal

Cl, N, O, F

H, C, Si

non polar covalent bonds to memorize

EN < 0.4, typically between nonmetals, resulting in equal sharing of electrons.

H-H, Cl-Cl, and O-O

C-H, C-S, C-P, Si-H

Ionic bonds

metal - non metal >1.8