Atom Electron Configuration + Phisiologically Important Isotopes Flashcards
Dalton Atomic Theory 1
Elements are composed of small particles called atoms
Dalton Atomic Theory 2
Atoms of given element are identical in size, mass and chemical properties. Atoms of different elements differ from each other
Dalton Atomic Theory 3
Compounds are composed of atoms of more then 1 element. The ratio of different atoms of any 2 elements can be presented as an integer or a simple fraction
Dalton Atomic Theory 4
Chemical reactions involve separation, combination or rearrangement of atoms. Atoms aren’t created or destroyed
Who 1st identified and discovered the electron
Thomson
What instrument was used to determine the electric charge to mass ration of an electron
Cathode Ray Tube
Matter Charge
Neutral. Equal amounts positive and negative particles
Plum Pudding Model Reasoning
Plum Pudding Model Description
Positive sphere, electrons embedded randomly throughout
Who Designed Plum Pudding Model
Thomson
Rutherford Discoveries + Experiment
Nucleus, proton. Gold foil
Rutherford’s Conclusion on Nucleus
Small, dense, positive at center of atom
Bohr Experiement
Study of Hydrogen Emission Line Spectra
Bohr Conclusions
Electrons move in circular orbits around nucleus + orits have specific energy levels
Einstein Discovery
Photoelectric Effect - Light has particle properties
deBroglie’s Theory (building off Einstein)
Wave-particle duality
Heisenberg’s Principle
IT’s impossible to know the position and velocity of an electron
Schrodinger’s Equation Purpose
Calculates the probability of finding an electron in a particular position of an atom
Atomic Orbitals Definition
Region in space with a high probability of finding an electron
Characteristics Differentiating Atomic Orbitals
Size, energy, shape and orientation
s-orbital dimensions + shape
3 dimensions + Spherical
What does a higher orbital number mean
Higer energy + increased distance from nucleus
p-orbital shape + dimensions
dumbbell, 3 dimensions
How px, py and pz orbitals differ from eachother (same energy, same shape)
Different orientation
D orbital shape
Undefined
How many different configurations can a d- orbital have
5 (x^2-y^2, z^2, xy, xz, yz)
Energy Sublevel Def.
Group of atomic orbitals of equal energy in an atom
2p no. of orbitals + max. electron no.
3, 6
Afbau Principle
Electrons fill lowest available energy levels 1st
Hund’s Rule
Orbitals of equal energy are filled singly before filling in pairs
Pauli Exclusion Principle
No more then 2 electrons can fill an orbital and they must have opposite spin
Valence Electron Def.
The outermost electron in an atom
Ion def.
a positively/negatively charged atom
Cation def.
positive ion
Main negative ion in blood
Cl-
Anion def.
Negatively Charged Ion
Main Cation in Cell Fluid
K+
