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chemistry (my deck) > Chapter 4 - Arrangement of Electrons in Atoms Notes > Flashcards

Chapter 4 - Arrangement of Electrons in Atoms Notes Flashcards

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AP® Chemistry flashcards Periodic Table flashcards
1
Q

How did Mendeleev organize the periodic table?

A

in order of atomic mass

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2
Q

How did Mosley organize the periodic table?

A

in order of atomic number

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3
Q

As the shells for electron arrangement become larger, the energy level also _________.

A

increases

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4
Q

List the number of electrons each shell can hold.

A 
2
8
18
32
18
2
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5
Q

Atomic number equals the number of _______.

A

protons

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6
Q

When electrically neutral, the number of protons equals the number of what?

A

electrons

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7
Q

What is the atomic mass?

A

protons + neutrons

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8
Q

The column numbers on the periodic table show tell the number of what?

A

valence electrons (electrons in the last shell)

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9
Q

The ___ numbers of the periodic table show the number of shells in the atom.

A

row

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10
Q

What is a region of space holding a mass of two electrons?

A

an orbital

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11
Q

List the order of orbitals from lowest energy to highest.

A

s, p, d, f

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12
Q

What shape is the s orbital?

A

sphere

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13
Q

How many boxes are there for the s orbital?

A

1 box

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14
Q

What is the max number of electrons that the s orbital can hold?

A

2 e-

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15
Q

How many boxes are there for the p orbital?

A

3 boxes

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16
Q

What is the max number of electrons that the p orbital can hold?

A

6 e-

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17
Q

How many boxes are there for the d orbital?

A

5 boxes

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18
Q

What is the max number of electrons that the d orbital can hold?

A

10 e-

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19
Q

How many boxes are there for the f orbital?

A

7 boxes

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20
Q

What is the max number of electrons that the f orbital can hold?

A

14 e-

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21
Q

The ______ _________ states that electrons fill regions of lowest energy first.

A

Aufbau Principle

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22
Q

“1s2 2s2 2p6 3s2…” is an example of what?

A

electron configuration

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23
Q

Electron configuration shows the _____ and the ______ of every electron placed.

A

Electron configuration shows the shell and the orbital of every electron placed.

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24
Q

Atom diagrams show what?

A

the electrons in the shell, and the protons and neutrons in the nucleus

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25
Q

Noble gas notation is also called what?

A

shorthand notation

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26
Q

Noble gas notation begins with what?

A

the previous noble gas of the element

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27
Q

What is the shape of the p orbital?

A

an infinity shape

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28
Q

What is the shape of the d orbital?

A

four-lobed structure

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29
Q

What is the shape of f orbital?

A

eight-lobed structure

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30
Q

From s orbital to f orbital, the energy ________.

A

increases

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31
Q

Orbital Box Notation uses the _______ ___________ to denote the diagram.

A

Orbital Box Notation uses the ending configuration to denote the diagram.

32
Q

For orbital box notation, the number of boxes are based on what?

A

the orbital (s-1, p-3, d-5, f-7)

33
Q

In orbital box notation, if one box is full, what is it called?

A

paired

34
Q

In orbital box notation, if one box is half full, what is it called?

A

unpaired

35
Q

_____ ____ states that each equal orbital receives one electron before any receive two.

A

Hund’s Rule states that each equal orbital receives one electron before any receive two.

36
Q

The _____ _______ _________ states that electrons in the same orbital will have an opposite spin, and that no two electrons can have the same four quantum numbers.

A

Pauli Exclusion Principle

37
Q

Quantum Mechanics uses a set of four quantum numbers to describe the exact location of electrons based on what?

A

wave theory

38
Q

The Shrodinger Equation is a mathematical description of electrons as waves. It is a basis for what?

A

quantum numbers

39
Q

What is the first part of quantum numbers, and what does it stand for?

A

Principal (n) - number of shells in the atom [row number]

40
Q

What is the second part of quantum numbers, and what does it stand for?

A

Angular momentum ( ) - identifying the orbital shape

41
Q

What can angular momentum also be called?

A

the Azimuthal quantum number

42
Q

What is each orbitals angular momentum number?

A

S - 0
P - 1
D - 2
F - 3

43
Q

What is the third part of quantum numbers, and what does it stand for?

A

Magnetic number (m) - orientation of the orbital in space (think of how the box is situated on the the axis)

i.e. “m=-1 to 1”
m= - to

*you must label the boxes:
_ _ _
-1 0 1

44
Q

What will always be in the middle of the labeled boxes for magnetic numbers?

A

zero 0

45
Q

What is the fourth part of quantum numbers, and what does it stand for?

A

spin (M or M ) - rotation of electron [commonly the last]

i.e. “spin = +1/2, -1/2”

46
Q

If the orbital box is full __, then the spin is what?

A

+1/2

47
Q

If the orbital box is half-full, then the spin is what?

A

-1/2

48
Q

According to the Wave Nature of Light, ___ forms of energy traveling through space is a wave.

A

According to the Wave Nature of Light, all forms of energy traveling through space is a wave.

**remember EMR

49
Q

A _________ is the distance from crest to crest (in meters).

A

wavelength ( )

50
Q

Frequency is the number of waves to what?

A

Pass a point per second

51
Q

What is frequency measured in?

A

Hertz or 1/sec

52
Q

Wavelength and frequency have an ______ relationship.

A

Wavelength and frequency have an inverse relationship.

53
Q

As wavelength _________, frequency ________.

A

As wavelength increases, frequency decreases.

54
Q

List the electromagnetic spectrum from lowest wavelength to highest wavelength.

A 
Gamma
X-rays
UV
Visible (VIBGYOR)
Infrared
Microwave
Radio
55
Q

What is the speed of light (c)?

A

3.00 x 10^8 m/s

56
Q

c= ?

A

c = (λ)(f)

speed of light = (wavelength)(frequency)

57
Q

What is the SI unit prefix conversion line?

A

(T)era - - (G)gia - - (M)ega - - (K)ilo (H)ecto (Da) deka BASE UNIT
(D)eci (C)enti (m)illi - - (μ) micro - - (N)ano - - (P)ico

58
Q

Who founded the Particle Theory of Light?

A

Max Plank

59
Q

What did Plank theorize?

A

Plank theorized that energy travels as particles.

60
Q

Quanta/Quantum means what?

A
  • particles of energy

- carry a defined amount of energy

61
Q

What is the main support behind the Particle Theory of Light?

A

photoelectric effect

62
Q

The Photoelectric effect refers to the ________ of electrons from a metal when light shines on the particle.

A

emission

63
Q

Energy =

A

(h)(f)

plank’s constant)(frequency

64
Q

The spectroscope separates light into different what?

A

wavelengths (and, therefore, colors)

65
Q

1 Angstrom =

A

1 x10 ^-10 meters

66
Q

The emission/absorption spectrum is a part of what?

A

Particle theory

67
Q

The emission spectrum is also called the ______ ____ spectrum.

A

bright line

68
Q

The emission spectrum goes from a ____-______ state to a ___-_____ state.

A

The emission spectrum goes from a high-energy state to a low-energy state.

excited to ground

69
Q

A ______ is released as energy.

A

photon

70
Q

The high-energy state is what?

A

excited state

71
Q

The low-energy state is what?

A

ground state

72
Q

The absorption spectrum is also called the what?

A

Dark line spectrum

73
Q

The absorption spectrum goes from a ___-______ state to a ____-______ state.

A

The absorption spectrum goes from a low-energy state to a high-energy state.

ground to excited

74
Q

Who combined the Wave Nature of Light and the Particle Theory of Light?

A

Einstein

75
Q

Einstein said that light behaves as a ____ and a _______.

A

wave and a particle

76
Q

What states that you can not determine the position and velocity of an electron at the same time?

A

Heisenberg Uncertainty Principle

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