Honors Chemistry: Chapter Four. Flashcards
(42 cards)
Wavelength (Lambda)
The distance between corresponding points on adjacent waves
Frequency (V)
The number of waves that pass a given point in a specific time, usually one second
Quantum (Energy)
The minimum quantity of energy that can be lost or gained by an atom
Excited State
State in which an atom has a higher potential energy than it has in its ground state
Ground State
Lowest energy state of an atom
Emission
The act or process of emitting, something coming as an effect
Absorption
Absorbing, or taking in
Photoelectric Effect
The emission of electrons/light from a metal when light shines on the metal. Light of a certain frequency must hit.
Photon
A particle of electromagnetic radiation having zero mass and carrying a quantum of energy (a bundle of energy)
Line Emission Spectrum
The colors that are emitted when energy is given out at several different wavelengths/elements
Continuous Spectrum
A continuous range of frequencies of electromagnetic radiation/visible light
Heisenberg Uncertainty Principle
It is impossible to determine both the exact velocity and location of an electron or any other principle
Aufbau Principle (The Diagonal Rule)
An electron occupies the lowest energy orbital that can receive it. Within each principal energy level, s orbitals are always the lowest
Hund’s Rule (Orbital Notation)
Orbitals of equal energy are each occupied by 1 electron before any is occupied by 2 electrons. All electrons in a singly occupied orbitals must have the same spin.
Pauli Exclusion Principle
No two electrons in the same atom can have the same 4 quantum numbers. (Two electrons must have an opposite spin)
Principal Quantum Number Represented by: Energy Level: Numbers: As n increases: Maximum number of electrons in an energy level is represented by:
Represented by: “n”
Energy Level: Main
Numbers: 1-7
As n increases: Energy and average distance for the nucleus increases
Maximum number of electrons in an energy level is represented by: 2n^2
Orbital Quantum Number (Angular Momentum Quantum Number)
Represented by:
Shapes of s, p, d, and f:
Represented by: "l"/cursive "l" Shape of s: sphere p: peanut/dumbbell d: double peanut/double dumbbell f: complex
Magnetic Quantum Number Represented by: The orientation of an orbital around the nucleus s: p: d: f:
Represented by: “m”
s: 1
p: 3
d: 5
f: 7
Spin Quantum Number
Represented by:
Definition:
Values
Represented by: “s”
Definition: The two spin states of an electron in an orbit
A single orbital can hold a maximum of 2 electrons, but the two electrons must have opposite spin
Values: -1/2 and 1/2
Energy Levels:
1-7
Sub-levels:
s, p, d, and f
Orbitals:
s: 1
p: 3
d: 5
f: 7
Electrons:
s: 2
p: 6
d: 10
f: 14
What is the principal quantum number is 2p?
2.
