S1-L2 The structure of the Atom Flashcards
Outline the basic structure of an atom
- Electrons (-)
- Protons (+)
- Neutrons (uncharged)
How big is the atom compared to the nucleus?
-atom diameter 10, 000x larger than that of its nucleus
What is the charge of an atom?
- neutral
- -> e- loss gives charged ion
Briefly outline the nucleus of an atom
- centre of atom- almost all mass there
- atom’s protons & neutrons compose it
Define the following terms:
1-Nucleons
2-Atomic number (Z)
3-Mass number (A)
1- protons and neutrons
2- n. of protons in nucleus of atom
-sum of protons and neutrons in nucleus
–>AKA nucleon number
Describe the electrons of an atom
- surround nucleus–> occupy specific region in space-orbitals
- orbitals grouped in to shells
- ->identified by principle quantum number, n= 1, 2, 3…each shells contains unique set of orbitals
- completely filled shell v. stable–> noble gas
- e-s determine atom properties like reactivity AND bond forming ability
Define an isotope
- atoms with same atomic number BUT different mass number
- ->or same n. of protons BUT different n. of neutrons
- different atoms of same element
- same n. of protons as e-‘s
- mass varies due to varying neutron number
Outline the following properties of isotopes:
1-chemical
2-physical
1- isotopes outer e- same AND same chemical identity so chemical properties identical
2-such as density can differ due to different mass of isotope
What is the “kinetic isotope effect”?
-heavier isotopes react slightly slower
What are the 3 main isotopes of hydrogen?
- 1H- most abundant isotope
- 2H- use in isotopic labelling experiments/ v. useful in NMR spectroscopy
- 3H- radioactive–>used in labelling experiments
Outline the main isotopes of carbon
- carbon-12 (6,6) stable
- carbon-13 (6, 7) stable
- carbon-14 (6, 8) radioactive
What are the isotopes of chlorine AND bromine?
- chlorine: 35 Cl/ 37 Cl
- bromine: 79 Br. 81 Br AND 23+ more unstable isotopes
Define Relative atomic mass (Ar)
-of an element is weighted average of individual isotopes
Example: 35 Cl and 37 Cl
What are their mass number?
- 35 Cl: P=17/ E= 17/ N=18
- -> mass number is 35
- 37 Cl: P= 17/ E=17/ N=20
- ->mass number is 37
Outline the composition of an ordinary chlorine atom and it’s measured atomic weight
- ordinary composition is 3 35 Cl atoms and 1 37 Cl atoms
- ->so measured atomic weight is (3 x 35) + (1 x 37)/ 4 = 35.5
What are “stable” and “unstable” isotopes?
- Stable: remain unchanged indefinitely
- Unstable: undergo spontaneous disintegration- to become stable nucleus
- -> disintegration results in emission of small particles AND or radiation
- also named as radioactive isotopes
Outline the use of the two types of isotopes mentioned above
-Can use both forms as diagnostic AND tracer tools in research
What is “mass spectrometry”?
- measures molecular weight of atoms/ compounds via observation of m/z ratio of ions
- works for both stable and unstable isotopes
What are the applications of mass spectrometry and how does this occur?
-determining isotopic abundance AND identity of small molecules + proteins and more
-atoms + molecules converted in to ions which can separate into ions which can separate on basis of their masses AND motions in
magnetic/electrical field
Example: Outline the features of the mass spectrum of neon-3 isotopes present
- 20 Ne/ 21 Ne/ 22 Ne
- peak position gives atomic mass
- peak intensity–> gives relative abundance
- normally highest abundance scaled up to 100%
- -> other values adjusted accordingly
Outline some of the uses of the following stable isotopes:
1- Ca-42, -44, -46, -48
2- C-13
3- Fe-54, -57, -58
4- O- 18
1-calcium metabolism/ bioavailability/ nutritional Ca role in pregnancy, growth AND development & lactation
2- molecular structure AND chemical reaction mechanism study
-molecular fingerprinting-dope testing athletes
3- metabolism/ energy expenditure studies
-metabolic tracer studies to identify genetic iron control mechanisms
4- studies of metabolism & energy expenditure
-lean body mass measurements
-obesity research
Define the term “radioactive decay”
- nucleus of unstable radioisotope seeks energetic stability by emitting particles/ radiation
- -> alpha/ beta AND gamma particles
What is “half life”?
- t 1/2 (time to half) of radioactive isotopes
- -> time taken for activity set amount of radioactive substance to decay to half its original value
Outline and briefly explain the following mechanisms of radioactive decay
1- Alpha (a) radiation
1- Alpha particle emission
- helium nuclei
- (+) charged