Test #1 Periodic Table Flashcards
Atomic number
The protons in the nucleus and electrons for natural atoms
Mass number
The sum of protons in neutrons
Cation
Positive charge, if a neutral atom loses, one or more electrons, it became a cation
Anion
Negative charge, atom gains, one or more electron then it becomes an anion
Periodic table group 1
Alkali metals
Periodic table group 2
Alkaline earth metals
Periodic table group 17
Halogens
Periodic table group 18
Noble gases
Transition metals
All the others
Metalloid
Elements that are around the staircase
Alpha particle
Composite particles consisting of two protons, and two neutrons tightly bonded together
Beta particle 
High energy high speed, electron aura positron emitted by the radioactive decay of an atom nucleus
Gamma ray
Cause ionizations that damaged tissue and DNA
What is a mass spectrometer used for?
To identify unknown compounds via molecular weight determination 
What is nuclear decay?
The news, July release energy in the form of ionization radiation
What is a radioisotope? 
Radioactive isotope of an element
Modern atomic theory
Bohrs model of the atom
Electron transitions
When an atom is given energy electrons absorb the energy and can jump from their ground state to a higher energy level “excited state”
Flaws to bohr  model
Each energy level is actually made up of energy sublevels
Who discovered the uncertainty principle theory
Werner Heisenberg 
What was the purpose of the uncertainty principle?
Electrons are now described as being in probabilities electron clouds around the nucleus, called orbitals
How much does an orbital hold?
2 e-
What does each sublevel hold?
S - 2
P - 6
D - 10
F - 14
Aufbau principal
Electrons occupy orbitals of lower energy first
Pauli principle
An orbital can hold only two electrons, and they must have opposite
Hunds rule
The same sublevel will not pair up until all of the orbitals in that sublevel have at least 1 e
Ion review
Adams can gain or lose electrons to become more stable
Cat ions have lost electrons to become positive
And ions have gained electrons to become negative
Valence electrons are the most electrons in an atom
Adam lose or gain electrons to get a stable “octet”
Atomic radius trend
Across a period - decreases from L to R
Down a family - increases moving down 
Ionization energy trend
Across a period - increases L To R
Moving down a family - decreases
Electron affinity trend
Across a period - increases from l to r
Moving down a family - decreases
Electronegativity trend
Increasing moving left to right across a period
Decreasing moving down a family
Ionic compound
Made up of metals and nonmetals
Properties of ionic compounds
Electrolytes, our hard, but brittle, have a high melting point
Ionic bonds
Form went to oppositely, charged ions, are attracted to each other.
John Dalton
Dalton proposed a modern atomic model based on experimental not on pure reason. His model can be compared to a billiard ball.
Democritus
Site matter could not be divided indefinitely
Aristotle
Modified an early theory that matter was made up before elements, earth, water, air, and fire
Isotope
Adams with the same number of protons, but different number of neutrons
Avogadros constant
The number of entities in one mole
