Chemistry Chapter 7 Flashcards

1
Q

Name the four quantum numbers

A

n, l, ml, ms

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2
Q

Explain n quantum number

A
  • the shell

- determines the energy and size of the orbital

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3
Q

Explain l quantum number

A

Azimuthal q#

  • sublevel or subshell
  • = to n-1
  • determines energy and shape of the orbital
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4
Q

Explain ml

A
  • magnetic Q#
  • determines the orientation of the orbital
  • rule: l, 0, +l
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5
Q

Explain ms

A
  • spin Q#
  • determines spin of an electron and the orientation of the magnetic field produced by this spin
  • either +1/2 or -1/2
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6
Q

How do electrons spin when they are in the same and different orbitals

A
  • same: spin opposite

- different: same spin

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7
Q

Name the different subshells or l

A

-0, 1, 2, 3, 4, 5

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8
Q

Define the 0 subshell

A
  • (s): sharp
  • has 1 orbital
  • 2 electrons
  • starting shell= s=1
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9
Q

Define the 1 subshell

A
  • p(principle)
  • has 3 orbitals
  • has 6 electrons
  • starting shells is sp=2
  • dumbbell shape
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10
Q

Define the 2 subshell

A
  • diffuse (d)
  • has 5 orbitals
  • has 10 electrons
  • spd=3
  • has butterfly shape
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11
Q

Define the 3 subshell

A
  • fundamental (f)
  • has 7 orbitals
  • has 14 electrons
  • starting shell is spdf=4
  • shape is complex
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12
Q

How do you write the electron configuration for ions that are transition metals

A
  • transition metals lose valence s electrons first then d
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13
Q

How do you write electron configuration for metals in lower p block ions?

A
  • lose valence p electrons then s electrons
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14
Q

What is important about d orbitals

A

completely filled and half filled d orbitals ate stable and prefer to stay that way so they will transfer electrons to get to this stability

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15
Q

State the equation for speed

A

c= frequency(new) times (wavelength) lambda

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16
Q

State the equation for energy

A

E= planks constant times frequency

E= planks constant times speed divided by wavelength

17
Q

What are the units for equation c= frequency times wavelength

A
  • c= m/s
  • wavelength= m
  • frequency= s-1 or Hz
18
Q

What are the units for the equations E= hv and E= hc/ wavelength

A
  • E= J
  • h: 6.626*10^-34 Js
  • c= 2.998*10^8 m/s
19
Q

How to you find the wavelength of light when electrons change states

A

1/wavelength= 1.097*10^7 (1/n2^2- 1/n1^2)

20
Q

What area of the electromagnetic spectrum can humans see

A

350-800

21
Q

What state are atoms usually in

A
  • ground state
22
Q

What happens when electrons absorb energy

A
  • go to excited state
23
Q

Why do atoms have line spectrum and not continuum spectra

A
  • b/c they have discreet energy levels
24
Q

What is effective nuclear charge

A
  • the amount of positive charge experienced by an electron in a polyelectronic atom
25
Q

Explain want happens with effective nuclear charge according to the periodic table

A
  • trend: Zeff, Z sigma, Z eff < z
  • along period: it increases because adding electrons to same shell
  • down a group: it decreases because further away from nucleus
  • Exceptions: none
26
Q

What is atomic radius?

A

the size of the atom determined by the electron cloud