Chemie 1 Samenvatting BML medisch diagnostiek jaar 1
Week 1
● Atom
○ Nucleus: composed of protons and neutrons
○ Electrons
Mass number
● Atomic numberAtomic number
○ Mass number: protons + neutrons
○ Atomic number: amount of protons
●
Name Charge Mass (amu) Mass (g)
Electron -1 5,486 * 10-4 9,1094 * 10-28
Proton +1 1,007 1,6726 * 10-24
Neutron 0 1,009 1,6750 * 10 -24
● Isotopes: same atom, but contain difeeent numbee of neuteons→ difeeent mass
numbee
● 1 amu= 1,6605 * 10-24 grams
● Natural abundance= percentage of each isotope, as found in nature
● Dalton’s Theory
○ all matters consists of tiny particles, atoms
○ atoms cannot be destroyed, changed, divided, etc.
○ atoms of particular element have identical properties
○ atoms of different elements have different properties
○ atoms of different elements combine in simple whole- number ratios to produce
compounds
○ chemical change involves joining, separating, or rearranging atoms
● Nuclear fission= splitting
● Crookes→ atoms had + oe - chaege
○ expeeiment: connected two metal electeodes at opposite side of a vacuum
glass tube→ electeicity tuened on and eays of light teaveled between metal
electeodes→ coming feom cathode (cathode eays, negative) to anode
(positive)
● Thomson → demonsteated electeical and magnetical peopeeties of cathode eays
○ Rays were deflected to an positive pole in an external electrical field
○ Cathode rays consists of negative particles
● Goldstein→ same expeeiments as Thomson discoveeed the peotons
● 1932→ James Chadwick demonstrated existence of neutrons
● Rutherford→ nucleus (positive) and negative electeons outside of the nucleus
○ Geigee→ natueal eadioactivity→ some atoms decay (peoduce alpha, betá oe
gamma eadiation)
■ He used radium to shoot alpha particles at gold foil, some went through and
other deflected back and some back into the source
■ Rutheefoed concluded that most of the atom is empty space, as
most of the alpha paeticles went theough→ so theee must be a small
dense eegion (nucleus) → fundamental discoveey
-9
● 10 = atomic level
● Speed of light→ 3,0 * 108 m/s
● Photon→ Max planck did expeeimental studies, which weee inteepeet by Albeet
Einstein→ which let to the conclusion that light consists of photons
, ● Emission spectrum= not all wavelengths are emitted, only some which characteristic for a gas
● Bohr studied the emission specteum of hydeogen→ hypothesized that theee weee
eneegy levels aeound nucleus, quantization (eneegy has ceetain values, but cannot
have an amount between those values)
○ Electrons are found in allowed energy levels
○ Allowed energy levels are quantized
○ Atoms absorb energy and electron goes to higher level (excitation)
○ Atoms loses energy and electron travels back to his original energy level (relaxation)
○ This emitted energy is viewed as light of the same wavelength
○ Energy differences can be calculated from the wavelength of emitted light
○ Spectral lines are result from electron promotion and relaxation
● Atomic orbital= you can find an electron within its energy level in a region of space
● Electron density= probability of finding the electron at any point in time
Week 2
● 1869→ Mendeleev aeeanged elements and ceeated the peeiodic table
● Periodic table
○ Group 1: alkali metals
○ Group 2: alkaline earth metals
○ Group 17: halogens
○ Group 18: noble gases
● Elements between boundary metals and nonmetals are metalloids: they have metal and
nonmetal properties
● Electron configuration= arrangement of electrons in atoms
● Disadvantages of Bohr’s model:
○ Could not explain emission spectrum of more electrons
○ Evidence of electrons with wave properties was problematic
● Scheöedingee→ eefned oher’s model and desceibed electeons in atoms in
peobability teems, developing equitations to explain the wave peopeeties of
electeons
● Principal energy level= regions where electron may be found
● Orbital= section which contains a maximum of 2 electrons
● Energy levels
○ n= 1 → has one sublevel (1s) (2(1)2)= 2e (maximum)
○ n=2→ has two sublevels (2s en 2p) (2(2) )= 8e (maximum)
2
○ n=3→ has theee sublevels (3s, 3p en 3d) (2(3)2)= 18e (maximum)
● Sublevels
○ s→ maximum 2 e
○ p→ maximum 6 e
○ d→ maximum 10 e
● 4s has less energy than 3d, that’s why the order of orbitals mentions s before d
● S orbital has 1 region, p orbital has 3 regions and d orbital has 5 regions
Week 1
● Atom
○ Nucleus: composed of protons and neutrons
○ Electrons
Mass number
● Atomic numberAtomic number
○ Mass number: protons + neutrons
○ Atomic number: amount of protons
●
Name Charge Mass (amu) Mass (g)
Electron -1 5,486 * 10-4 9,1094 * 10-28
Proton +1 1,007 1,6726 * 10-24
Neutron 0 1,009 1,6750 * 10 -24
● Isotopes: same atom, but contain difeeent numbee of neuteons→ difeeent mass
numbee
● 1 amu= 1,6605 * 10-24 grams
● Natural abundance= percentage of each isotope, as found in nature
● Dalton’s Theory
○ all matters consists of tiny particles, atoms
○ atoms cannot be destroyed, changed, divided, etc.
○ atoms of particular element have identical properties
○ atoms of different elements have different properties
○ atoms of different elements combine in simple whole- number ratios to produce
compounds
○ chemical change involves joining, separating, or rearranging atoms
● Nuclear fission= splitting
● Crookes→ atoms had + oe - chaege
○ expeeiment: connected two metal electeodes at opposite side of a vacuum
glass tube→ electeicity tuened on and eays of light teaveled between metal
electeodes→ coming feom cathode (cathode eays, negative) to anode
(positive)
● Thomson → demonsteated electeical and magnetical peopeeties of cathode eays
○ Rays were deflected to an positive pole in an external electrical field
○ Cathode rays consists of negative particles
● Goldstein→ same expeeiments as Thomson discoveeed the peotons
● 1932→ James Chadwick demonstrated existence of neutrons
● Rutherford→ nucleus (positive) and negative electeons outside of the nucleus
○ Geigee→ natueal eadioactivity→ some atoms decay (peoduce alpha, betá oe
gamma eadiation)
■ He used radium to shoot alpha particles at gold foil, some went through and
other deflected back and some back into the source
■ Rutheefoed concluded that most of the atom is empty space, as
most of the alpha paeticles went theough→ so theee must be a small
dense eegion (nucleus) → fundamental discoveey
-9
● 10 = atomic level
● Speed of light→ 3,0 * 108 m/s
● Photon→ Max planck did expeeimental studies, which weee inteepeet by Albeet
Einstein→ which let to the conclusion that light consists of photons
, ● Emission spectrum= not all wavelengths are emitted, only some which characteristic for a gas
● Bohr studied the emission specteum of hydeogen→ hypothesized that theee weee
eneegy levels aeound nucleus, quantization (eneegy has ceetain values, but cannot
have an amount between those values)
○ Electrons are found in allowed energy levels
○ Allowed energy levels are quantized
○ Atoms absorb energy and electron goes to higher level (excitation)
○ Atoms loses energy and electron travels back to his original energy level (relaxation)
○ This emitted energy is viewed as light of the same wavelength
○ Energy differences can be calculated from the wavelength of emitted light
○ Spectral lines are result from electron promotion and relaxation
● Atomic orbital= you can find an electron within its energy level in a region of space
● Electron density= probability of finding the electron at any point in time
Week 2
● 1869→ Mendeleev aeeanged elements and ceeated the peeiodic table
● Periodic table
○ Group 1: alkali metals
○ Group 2: alkaline earth metals
○ Group 17: halogens
○ Group 18: noble gases
● Elements between boundary metals and nonmetals are metalloids: they have metal and
nonmetal properties
● Electron configuration= arrangement of electrons in atoms
● Disadvantages of Bohr’s model:
○ Could not explain emission spectrum of more electrons
○ Evidence of electrons with wave properties was problematic
● Scheöedingee→ eefned oher’s model and desceibed electeons in atoms in
peobability teems, developing equitations to explain the wave peopeeties of
electeons
● Principal energy level= regions where electron may be found
● Orbital= section which contains a maximum of 2 electrons
● Energy levels
○ n= 1 → has one sublevel (1s) (2(1)2)= 2e (maximum)
○ n=2→ has two sublevels (2s en 2p) (2(2) )= 8e (maximum)
2
○ n=3→ has theee sublevels (3s, 3p en 3d) (2(3)2)= 18e (maximum)
● Sublevels
○ s→ maximum 2 e
○ p→ maximum 6 e
○ d→ maximum 10 e
● 4s has less energy than 3d, that’s why the order of orbitals mentions s before d
● S orbital has 1 region, p orbital has 3 regions and d orbital has 5 regions
