S1.2 Flashcards
The Nuclear Atom
What are some differences between Dalton’s Atomic Theory and the Modern Atomic Theory?
Dalton :
- elements = indivisible + indestructible particles (atoms)
- Same element atoms = exactly alike + have some masses
- Different element atoms–> have different masses
- Atoms come together to form compounds in small whole number ratios
Modern :
- atoms = divisible (composed of subatomic particles)
= Atoms of the same element do NOT always have same mass (ex. isotopes)
- Nuclear transformations may -> atoms getting alter/destroy atoms
Similarities :
- matter = composed of atoms
- All atoms of one element differ n their properties
What are examples of 3 elements and what element did they discuss?
- Thomson’s model
- Rutherford Model
- Bohr’s Model
- electron
- proton
3.?
What are atoms?
Atoms are what is made up by + charged nucleus which has protons and neutrons + electrons which are outside the nucleus
What are key factors of a nucleus?
- small compared to atom
- structure = highly dense with most (BLANK?) in the nucleus
- charged
What is important to know about the charge and rel. charge of a neutron?
Both 0
Explain Ions, Cations, and Anions.
Ions = atoms that have either gained an electron or lost an electron
Cation = + charged ion with loss of of 1 or more electrons
Anion = - charged with gain of 1 or more electrons
How to calculate neutrons?
Know how to draw nuclear symbol notation.
What of neutrons in a neutral atom?
- Atomic # (or number of protons) from atomic mass) an-am
- ^3 He (lower subscript 1)
means , (3 = mass number, 1 = # of protons or atomic #) - = same as protons
What are isotopes and their properties?
- element with diff number of protons or atomic number?
- Properties - ?
?
?
What is rel. atomic mass and how do you calculate it?
- The weighted mean of isotopes that naturally occur to 1/12 of a carbon-12 atom (mass spectometry y used)
- Atomic Mass * abundance expressed as decimal
