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AP Chemistry > Ch. 8 Quantum Mechanics And Periodic Trends > Flashcards

Ch. 8 Quantum Mechanics And Periodic Trends Flashcards

0
Q

The theory which allows us to determine the probability of finding an electron at a particular place in the Atom

A

Quantum mechanics

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1
Q

Modern atomic theory is referred to as

A

Quantum mechanics

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2
Q

It is impossible to know both the speed and location of an electron at the same time

A

Heisenberg uncertainty principle

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3
Q

Particles that are involved in light

A

Photons

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4
Q

What is the principal quantum number

A

Describes the main energy level of the electron in its distance from the nucleus

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5
Q

How do you calculate the principal quantum number

A

2n^2

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6
Q

What levels to the electrons occupy

A

The lowest energy levels which are the closest to the nucleus

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7
Q

Azimuthal quantum number

A

Describes the sub level the electron is in

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8
Q

List the sub levels in order from least energetic to most energetic

A

S
p
D
F

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9
Q

Azimuthal quantum number

A

Also describes the shape of the electron cloud

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10
Q

Region of space in which an electron of a particular energy might be found

A

Electron cloud

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11
Q

What does the S as azimuthal quantum number look like

A

Sphere

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12
Q

What does the P look like

A

Propeller

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13
Q

What does the d look like

A

Daisy

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14
Q

What does the f look like

A

Too funky to draw

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15
Q

The shape of the space where there is a high probability of finding electrons

A

Orbital

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16
Q

Magnetic quantum number (m)

A

Describes the orbitals orientation in space

Represents the number of ways in which you can position an electron cloud

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17
Q

The space occupied by a pair of electrons

A

Orbital

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18
Q

When placing electrons into orbitals within a sub level place them in orbitals one at a time before doubling up

A

Hund’s role of maximum multiplicity

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19
Q

Spin quantum number (s)

A

Represents the direction of the electron spin

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20
Q

Where does an electron spin and how

A

Electron spins on its axis clockwise and counterclockwise

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21
Q

No two electrons in the same atom can have the same set of four quantum numbers

A

Pauli exclusion principle

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22
Q

Having the same energy

A

Degenerate

23
Q

Electrons will remain unpaired in a given orbital until orbitals of the same sublet will have at least one electron

A

Hund’s rule

24
Q

What sublevels overlap

A

The 4s and 3d

25
Q

Went to the overlaps become more frequent

A

As electrons are placed in n=5 and beyond

26
Q

How are energy levels spaced

A

They are not equally spaced as you get further from the nucleus energy levels get closer together and overlap

27
Q

A property that can be predicted based on an elements location on the periodic table

A

Periodic trend

28
Q

The distance from the center of the nucleus to the edge of the electron cloud

A

Atomic radius

29
Q

Why do scientists use a covalent radius or half the distance between the nuclei of two bonded Atoms

A

Because an electron clouds edge is difficult to define

30
Q

What is an Angstrom

A

1×10 to the -10 m

31
Q

What is the trend for atomic radius

A

Larger as you go down the column and smaller as you go to the right in the row

32
Q

What is the atomic radius get larger as you go down the column

A

Because each step down adds an entirely new main energy level making the Atoms larger

33
Q

What is the atomic radius get smaller as you go to the right in the row

A

Because each step right adds a proton and an electron yet the Atoms do not get larger because they are added to existing main energy levels the added electrons are not farther from the nucleus and the effective nuclear charge is greater

34
Q

Attraction that pulls the electron cloud in

A

Effective nuclear charge

35
Q

Pull that an electron feels from the nucleus

A

Effective nuclear charge

36
Q

The larger the effective nuclear charge

A

The tighter the electron cloud gets pulled in

37
Q

Why don’t we see the effective nuclear charge occur when going down the column

A

As more main energy levels are added to the Atoms the inner layers of electrons shield the outer electrons from the nucleus

38
Q

The energy required to remove an electron from an Atom

A

Ionization energy

39
Q

What is the relationship between ionization energy and atomic radius

A

Inversely proportional

40
Q

Ionization energy is always

A

Endothermic

Energy is added to the atom to remove the electron

41
Q

A measure of an atom’s desire for electrons in a chemical bond

A

Electronegativity

42
Q

What element has the highest electronegativity in what is the value

A

Fluorine the value is 4

43
Q

Which elements or electron dinners and have low electronegativities

A

Metals

44
Q

Which elements are electronic accepter’s and have high electronegativities

A

Nonmetals

45
Q

Best electron dinners and the largest

A

Metals

46
Q

Best electron takers and are the smallest

A

Nonmetals

47
Q

No electronegativities

A

Noble gases

48
Q

All of the ions with the same electron configuration

A

Isoelectronic series

49
Q

Goes from regular element to negative ion

A

Ion is bigger less effective nuclear charge

50
Q

Goes from regular element to Positive ion

A

Ion is smaller

51
Q

Why don’t elements change in an isoelectronic series

A

Because protons determine the element

52
Q

Equations needed to calculate the energy involved in an electron transition

A

Delta E equals RH times the quantity one over ni squared -1 over nf squared

E equals HV

C equals V upside down y

53
Q

Number of cycles that pass in a certain amount of time

A

Frequency

54
Q

V

A

Frequency

55
Q

Upside down y

A

Wavelength

AP Chemistry (5 decks)

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