53 Elements Flashcards
Hydrogen
H
Helium
He
Lithium
Li
Beryllium
Be
Boron
B
Carbon
C
Nitrogen
N
Oxygen
O
Fluorine
F
Neon
Ne
Sodium
Na
Magnesium
Mg
Aluminium
Al
Silicon
Si
Phosphorus
P
Sulfur
S
Chlorine
Cl
Argon
Argon
Ar
Potassium
K
Calcium
Ca
Titanium
Ti
Chromium
Cr
Manganese
Mn
Iron
Fe
Cobalt
Co
Nickel
Ni
Copper
Cu
Zinc
Zn
Gallium
Ga
Arsenic
As
Selenium
Se
Bromine
Br
Krypton
Kr
Rubidium
Rb
Strontium
Sr
Palladium
Pd
Silver
Ag
Cadmium
Cd
Tin
Sn
Antimony
Sb
Tellurium
Te
Iodine
I
Xenon
Xe
Caesium
Cs
Barium
Ba
Platinum
Pt
Gold
Au
Mercury
Hg
Lead
Pb
Bismuth
Bi
Radon
Rn
Francium
Fr
Radium
Ra
First Theory and is it true or false
All matter is made of tiny particles called
atoms; indivisible and indestructible units
False because atoms ARE destructable (Dalton believed that atoms were solid spheres)
2nd theory, true or false?
All atoms of a given element are identical.
False because number neutrons and electrons can vary
Third theory, true or false
Atoms of a given element are different from
those of any other element.
True, the number of protons always differs
4th Theory, true or false
Atoms of one element can combine with
atoms of other elements to form compounds.
True, a given compound always has the same
relative number and type of atoms
5th theory, true or false
Atoms are neither created nor destroyed in
chemical reactions
True. They are only created or destroyed in nuclear fusion or fission
Nuclear Symbol Notation
A on top, Z on bottom, X
A=mass number
Z=atomic number
X=element symbol
Periodic Table Notation
Z above X
Z=Atomic number
Hyphen Notation
X-A
A= Mass number
Properties of metals
Lustrous, malleable, ductile, conductive, tend to form cations by losing electrons in reactions with nonmetals
Properties of nonmetals
Tend to form anions by gaining electrons in reactions with metals, generally lack defining properties as they all vary property-wise but they are bad conductors
Law of Conservation of Mass
Mass is neither created nor destroyed in chemical reactions (for example: the carbon atom in coal becomes carbon dioxide when it is burned)
Group 1
Alkali Metals
Group 2
Alkaline Earth Metals
Group 17
The Halogens
Group 18
The Noble Gasses
Elements left of the staircase
Metals (except for Hydrogen)
Elements right of the staircase
Nonmetals
Elements that border the staircase
Metalloids
Elements located in groups 3-12
Transition metals
Elements below the main section fo the periodic table
Lanthanides (1st row) and Actinides (2nd row)
Down a group, ionization energy
Decreases
Down a group, atomic radius
Increases
Across a period, ionization energy
Increases
Across a period, atomic radius
Decreases
Ionization energy defintion
The amount of energy needed to remove an electron
Tallest point of wave
Crest
Lowest point of wave
Trough
Height of wave
Amplitude
Distance from highest point to highest point on wave
Wavelength
Thomson
Plum pudding model (electrons floating in positive cloud) and cathode ray tube (proved that electrons were negatve bc they were attracted to the positively charged end of the tube)
Rutherford
Discovered positive nucleus through gold foil experiment
Isotopes
Atoms with the same number of protons but different numbers of neutrons
Bohr Model of the Atom
Circular orbits (quantized energy levels), electrons moved between the orbits by absorbing or emitting particular photons.
Schrodinger’s Wave Mechanical Model
Probablity map: 95% chance electron is within shaded region, more electrons in darker regions vs. lighter regions.
Principle Energy level
Distance between electrons and nucleus
Quantized energy levels
Variation of energy levels, electrons can only possess certain discrete energy levels
Aufbau Principle
Electrons fill orbitals in order of increasing energy subshells
Pauli exclusion principle
No two electrons can have the same spin or be in the same location at the same time; this limits repulsion
Hund’s Rule
Each orbital must contain one electron before a second electron is paired; limits repulsion
number of electrons per energy level formula
2(n)^2
