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
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2
Q

Describe the characteristics and limitations of the

Revised Nuclear Model

A
  • discovered positive proton and neutral neutron
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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
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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
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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

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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
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7
Q

What is an

Orbital

A
  • a 3D description of where an e- could be
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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)
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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
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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-
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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)
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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
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13
Q

Pauli Exclusion Principle

A
  • no 2 e- can have the same quantum numbers
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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
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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
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