Chapter 7 Definitions Flashcards
Quantum Mechanics
The theory that explains the behavior of the absolutely small
Waves out of phase means destructive Interference. True/False
True
Waves in phase means constructive Interference. True/False
True
Waves out of phase make bright spot. True/False
Dark Spot
Waves in phase makes bright spot. True/False
True
What are photons?
Discrete packets of light
What do prisms do?
They separate component wavelengths.
Light is emitted as electron falls back to a lower energy lever. True/False
True
Quantum-Mechanical Model
Explains how electrons exist in atoms and how the electrons determine the chemical and physical properties of elements
Electric Field
A region of space where an electrically charged particle experiences a force
Magnetic Field
A region of space where a magnetic particle experiences a force.
Amplitude
Vertical height. The amplitude determines the light’s intensity or brightness. Greater the amplitude, the greater the brightness
Wavelength
Distance between waves. Greater the wavelength, less frequency. Different wavelengths means different colors. Longer wavelengths means red (low energy). Shorter wavelengths means violet (high energy).
List the electromagnetic spectrum from low energy to high energy?
Radia, Microwaves, Infrared, Visible Light. Ultraviolet, X-ray, Gamma ray
Our eyes can only see reflected light. True/False
True
What is on the right side of the electromagnetic spectrum
High energy, short wavelength, and high frequency
What is on the left side of the electromagnetic radiation?
Low energy, Long wavelength, and low frequency
Interference
How waves interact with each other
The photoelectric effect
Observation that metals can emit electrons when light shines upon them
Atomic spectroscopy
The study of the electromagnetic radiation and emitted by atoms
Emission Spectrum
A series of bright lines at specific wavelengths
The white light spectrum is continuous? True/False
True. It consists of light of all wavelength
De Broglie Relation
The wavelength of an electron mass moving at velocity
Probability distribution map
Shows where an electron is likely to be found
Indeterminacy (vague)
Position of an electron is not possible
The solution to the Schrodinger equation for an atom results in three quantum numbers. True/False
True. These numbers describe the size, energy, shape, and orientation of orbitals or energy levels. These are for hydrogen atoms.
What is the Principal Quantum Number (n)
An integer that determines the overall size of the orbital and indicates the energy level of an electron in an orbital
Angular Momentum Quantum Number (azimuthal quantum number)(l)
An integer that relates with the shape of the orbital
Magnetic Quantum Number(ML)
An integer that specifies the orientation of the orbital
What is orbital with same principal level
This means that orbitals have the same value of n
What is orbital with same sublevel(subshell)
This means the orbitals have the same value of n and l
Probability Density
The probability(per unit volume) of finding the electron at a point in space. As you move away from the nucleus the probability density decreases.
Radial Distribution Function
Total probability of finding the electron within a thin spherical shell at a distance r from the nucleus. It has a value of zero at the nucleus.
Node
Point where the wave function and the probability density and radial distribution all go through zero. The probability of finding an electron at a node is zero. It separates the phases of an orbital
Two types of nodes
Angular and radial
Radial Nodes (spherical node)
Spherical surface region where the probability of finding an electron is zero
Angular Nodes
Always equal to the angular momentum Quantum Number. For an s orbital there are no angular nodes. These are planes or surfaces where there is a zero probability of finding an electron
Phase
The sign of the amplitude of a wave(positive or negative). Important in bonding
Electron Configuration
Indicates what orbitals are occupied by electron
Ground State
Lowest energy electron configuration
Electron Spin (Stern-Gerlach Experiment)
The direction of the arrow in an orbital diagram (pointing up or down)
Spin Quantum Number (Ms)
The spin of an electron is specified by a fourth quantum number
Pauli Exclusion Principle
No two electron in an atom can have the same four quantum numbers. Implies that each orbital can have a maximum of only two electrons, with opposing spins
Coulombs Law
The interactions between charged particles
Shielding
How one electron can shield another electron from the full charge of the nucleus
Penetration
how one atomic orbital can overlap spatially with another, thus penetrating into a region close to the nucleus.
Aufbau Principle (build up)
An electron occupies orbitals in order form lowest energy to highest
Hund’s Rule
every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
Paramagnetic
An atom or ion that contains unpaired electrons is attracted to an external magnetic field
Diamagnetic
