Ch. 1: Atomic Structure Flashcards
Proton
Positive charge and mass around 1 amu; charge of fundamental unit of charge (e= 1.6*10^-19 C)
Neutron
No charge and mass around 1 amu, mass only slightly larger than proton
Electron
Negative charge (equal magnitude of proton) and negligible mass
Nucleus
Contains the protons and neutrons, while the electrons move around the nucleus
Atomic Number
Number of protons in a given element, unique identifier for each element
Mass Number
Sum of an element’s protons and neutrons
Cation
Positively charged atom
Anion
negatively charged atom
Atomic mass
Essentially equal to the mass number, the sum of an element’s protons and neutrons
Isotopes
Atoms of a given element (same atomic number) that have different mass numbers. Differ in the number of neutrons
Isotope Identification
The element followed by the mass number (ex: carbon-12, carbon-13)
3 Isotopes of Hydrogen
Protium, deuterium, and tritium
Atomic Weight
Weighted average of the naturally occurring isotopes of an element. The periodic table lists atomic weights, not atomic masses
Rutherford
Postulated that the atom had a dense, positively charged nucleus that made up only a small fraction of the volume of the atom with gold foil experiment
Bohr Model of the Atom
Dense, positively charged nucleus surrounded by electrons revolving around the nucleus in orbits with distinct energy levels
Quantum
Energy diff between energy levels, first described by Planck
Quantization
There is not an infinite range of energy levels available to an electron; electrons can exist only at certain energy levels. The energy of an electron increases the farther it is from the nucleus
Planck relation
E=hf; E is the energy of a quantum, h is planck’s constant, and f is frequency of radiation
Atomic Absorption Spectrum
Unique; for an electron to jump from a lower energy level to a higher one, it must absorb an amount of energy precisely equal to the energy difference between the two levels
Atomic Emission Spectrum
When electrons return from the excited state to the ground state, they emit an amound of energy that is exactly equal to the energy diff between the two levels; every element has a characteristic atomic emission spectrum and sometimes the electromagnetic energy emitted corresponds to a frequency in the visible light range
Quantum Mechanical Model
Posits that electrons do not travel in defined orbits but rather are localized in orbitals
Orbital
Region of space around the nucleus defined by the probability of finding an electron in that region of space
Heisenberg Uncertainty Principle
States that it is impossible to know both an electron’s position and its momentum exactly at the same time
Quantum numbers:
4, completely describe any electron in an atom; according to pauli exclusion principle no 2 electrons in a given atom can possess the same set of 4 quantum numbers