Structure and Properties of Matter Pt1 Flashcards
1
Q
Describe the characteristics and limitations of the
Nuclear Model of the Atom
2 points, 2 limitations
A
- mostly empty space
- e- are outside of a small positively charged nucleus
- limitations:
- nucleus cannot be only pos or it would break
- couldn’t acount for mass of the atom
- scientists thought e- countinuously gave off radiation and would eventually crash into the nucleus, but this doesn’t happen
2
Q
Describe the characteristics and limitations of the
Revised Nuclear Model
A
- discovered positive proton and neutral neutron
3
Q
Describe the characteristics and limitations of the
Bohr Model
2 poins, 3 limitations
A
- energy of e- is quantized (can only have specific values, can move within its energy lvl without losing energy)
- to move from one energy lvl to another, e- needs to gain or lose energy
- limitations:
- could only explain the line spectra for atoms with only one e-
- couldn’t explain why there are only “allowed” orbits/energy lvls
- couldn’t explain many physical or chemical properties
4
Q
Describe the characteristics and limitations of the
Quantum Mechanical Model
A
- ## e- cloud, density is proportional to the probability of finding an e- there
5
Q
How does this work
Emission Spectrum
A
- white light passes through hot gas and gets separated by a prism
- light is emitted when an e- goes to a lower energy lvl and releases energy
emission spectrum and absorption spectrum
6
Q
How does this work
Absorption Spectrum
A
- wihte light passes through cool gas, some wavelengths gets absorbed by the atoms, causing black lines in the absorption spectrum
7
Q
What is an
Orbital
A
- a 3D description of where an e- could be
8
Q
What are the
4 Quantum numbers and their symbols
A
- principle quantum number (n)
- secondary quantum number (l)
- magnetic quantum number (ml)
- spin quantum number (ms)
9
Q
Principle Quantum Number
3 points
A
- the main energy lvl occupied by the e-
- can be any pos integer from 1 to infinity
- max # of e- in an orbital is 2n squared
- e.g. if n=3; max # is 18
10
Q
Secondary Quantum Number
4 points
A
- describes shape of an orbital
- any integer from 0 to n-1 (e.g. if n=2, l=0, 1)
- l = 0, s (sphere)
- l = 1, p (dumbbell)
- l = 2, d
- l = 3, f
- each orbital holds max 2e-
11
Q
Magnetic Quantum Number
2 points
A
- describes orientation of orbitals around nucleus
- any integer from -l to +l (if l = 2, ml = -2, -1, 0, 1, 2)
12
Q
Spin Quantum Number
3 points
A
- specifies direction of the axis of the e-
- must have opposite spins or e- will repel e/o
- +1/2 or -1/2
13
Q
Pauli Exclusion Principle
A
- no 2 e- can have the same quantum numbers
14
Q
Aufbau Principle
A
- e- always fill lower energy orbitals before moving onto higher energy orbitals
- fill diagonally
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
15
Q
Hund’s Rule
A
- when there are orbitals with the same energy in the same energy lvl, e- will half fill before pairing up
- up spin