Unit 1: Atomic Structure, Periodicity, Trends on the Periodic Table Flashcards
Allotropes
2 versions of the same element
Protons
Charge: +1
Mass: 1
Location: Nucleus
Neutrons
Charge: 0
Mass: 1
Location: Nucleus
Electrons
Charge: -1
Mass: 0
Location: Valence shells
Atomic mass =
fractional abundance x mass number
Mass spectrometer
seperates atoms by mass
n is the?
principle energy level
Number of electrons in each level
2n^2
sublevel: S
holds 2 electrons, 1 orbital, sphere
sublevel: P
holds 6 electrons, 3 orbitals, teardrops
sublevel: D
holds 10 electrons, 5 orbitals
sublevel: F
holds 14 electrons, 7 orbitals
electrons in orbitals…..
have different spins ↑↓
ground state
as close to the nucleus as an electron can get
Aufbau principle
another way to put the electron configuration in order
electron configuration shortcut
go to the nearest noble gas
e.g. [Ar] 4s2 3d10 4p3
what type of sublevels are more stable?
half-filled sublevels and full sublevels
isoelectronic
‘same configuration’
c=λv
c: speed of light
λ: wavelength
v: frequency
E=hv
Equation for the incoming energy of electromagnetic radiation
E: energy
h: planck’s constant
v: frequency
Longer wavelengths have….
lower frequency
Shorter wavlengths have….
higher frequency
Periodicity
repeating patterns of physical and chemical properties
Metals tend to….
lose electrons
Non-metals tend to….
gain electrons
Atomic radius trend
increases down and to the left, focuses on electrons
Shielding
increases down and to the right, focuses on protons
1st ionization energy
energy to remove an electron, increases up and to the right
Electronegativity
attraction an atom has for the electrons in a bond, closest to Fluorine in the most electronegative, increases up and to the right, covalent < 1.7 < ionic
Electron affinity
energy released when one electron is added to a neutral atom in the gas state (exothermic), adding second electron is endothermic, increases up and to the right
Melting point
transition metals have a high melting point, metaks have a low melting point, carbon’s family has a high melting point, diamond has the highest melting point.
The more metals in the valence, the harder the metals, the higher the metling point.
Basic oxides
Metals: tend to lose electrons, tend to be ionic oxides
Acidic oxides
Non-metals: tend to gain electrons, tend to be covalent oxides
Amphoteric
it acts as a base in some situations and an acid in others - e.g. Al2O3
Transition metals
incomplete ‘d’ sublevel, Zn is an exception
Variable oxidation states
just a broader term for the charge
Ligands
complex ions, ligands are lewis bases, metal ions are lewis bases, lewis acid recieves the lone pair, lewis base provides the lone pair, must use square brackets for complex ions
Coordinate covalent bond
one atom provides both electrons for covalent bonds
Dimagentism
only paired electrons, commonly ‘non-magnetic’, weak repulsion in a magnetic field
Paramagnetism
half-filled orbitals, the more half-filled orbitals the more magnetic, strong repulsion in a magnetic field
Ferromagnetism
lots of half-filled orbitals, everday magnetism, Fe, Co, Ni
Catalyst
something that causes a reaction to go faster, increases reaction rate, the catalyst is unchanged during the reaction
Heterogeneous
transition metals
Homogeneous
enzymes, Iron (II), Cobalt (III)
Colorwheel
transition metals often have bright colors, complimentary colors are opposite, Sc3+ is colorless (there are no electrons in a d sublevel)
Photons of visible light can….
promote (raise) an electron to a slightly higher energy level
4 factors
identity of a ligand, identity of the metal ion, geometry, oxidation state on the metal ion
LEO says GER
LEO: loss of electrons, oxidation - reducing agent, causes reduction
GER: gain of electrons, reduction - oxidizing agent, causes oxidation
