Chapter 4 - Arrangement of Electrons in Atoms Notes

Question 1

How did Mendeleev organize the periodic table?

Answer 1

in order of atomic mass

Question 2

How did Mosley organize the periodic table?

Answer 2

in order of atomic number

Question 3

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

Answer 3

increases

Question 4

List the number of electrons each shell can hold.

Answer 4

2
8
18
32
18
2

Question 5

Atomic number equals the number of _______.

Answer 5

protons

Question 6

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

Answer 6

electrons

Question 7

What is the atomic mass?

Answer 7

protons + neutrons

Question 8

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

Answer 8

valence electrons (electrons in the last shell)

Question 9

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

Answer 9

row

Question 10

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

Answer 10

an orbital

Question 11

List the order of orbitals from lowest energy to highest.

Answer 11

s, p, d, f

Question 12

What shape is the s orbital?

Answer 12

sphere

Question 13

How many boxes are there for the s orbital?

Answer 13

1 box

Question 14

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

Answer 14

2 e-

Question 15

How many boxes are there for the p orbital?

Answer 15

3 boxes

Question 16

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

Answer 16

6 e-

Question 17

How many boxes are there for the d orbital?

Answer 17

5 boxes

Question 18

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

Answer 18

10 e-

Question 19

How many boxes are there for the f orbital?

Answer 19

7 boxes

Question 20

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

Answer 20

14 e-

Question 21

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

Answer 21

Aufbau Principle

Question 22

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

Answer 22

electron configuration

Question 23

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

Answer 23

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

Question 24

Atom diagrams show what?

Answer 24

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

Question 25

Noble gas notation is also called what?

Answer 25

shorthand notation

Question 26

Noble gas notation begins with what?

Answer 26

the previous noble gas of the element

Question 27

What is the shape of the p orbital?

Answer 27

an infinity shape

Question 28

What is the shape of the d orbital?

Answer 28

four-lobed structure

Question 29

What is the shape of f orbital?

Answer 29

eight-lobed structure

Question 30

From s orbital to f orbital, the energy ________.

Answer 30

increases

Question 31

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

Answer 31

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

Question 32

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

Answer 32

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

Question 33

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

Answer 33

paired

Question 34

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

Answer 34

unpaired

Question 35

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

Answer 35

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

Question 36

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.

Answer 36

Pauli Exclusion Principle

Question 37

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

Answer 37

wave theory

Question 38

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

Answer 38

quantum numbers

Question 39

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

Answer 39

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

Question 40

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

Answer 40

Angular momentum ( ) - identifying the orbital shape

Question 41

What can angular momentum also be called?

Answer 41

the Azimuthal quantum number

Question 42

What is each orbitals angular momentum number?

Answer 42

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

Question 43

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

Answer 43

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

Question 44

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

Answer 44

zero 0

Question 45

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

Answer 45

spin (M or M ) - rotation of electron [commonly the last] i.e. "spin = +1/2, -1/2"

Question 46

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

Answer 46

+1/2

Question 47

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

Answer 47

-1/2

Question 48

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

Answer 48

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

Question 49

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

Answer 49

wavelength ( )

Question 50

Frequency is the number of waves to what?

Answer 50

Pass a point per second

Question 51

What is frequency measured in?

Answer 51

Hertz or 1/sec

Question 52

Wavelength and frequency have an ______ relationship.

Answer 52

Wavelength and frequency have an inverse relationship.

Question 53

As wavelength _________, frequency ________.

Answer 53

As wavelength increases, frequency decreases.

Question 54

List the electromagnetic spectrum from lowest wavelength to highest wavelength.

Answer 54

``` Gamma X-rays UV Visible (VIBGYOR) Infrared Microwave Radio ```

Question 55

What is the speed of light (c)?

Answer 55

3.00 x 10^8 m/s

Question 56

c= ?

Answer 56

c = (λ)(f) | speed of light = (wavelength)(frequency)

Question 57

What is the SI unit prefix conversion line?

Answer 57

(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

Question 58

Who founded the Particle Theory of Light?

Answer 58

Max Plank

Question 59

What did Plank theorize?

Answer 59

Plank theorized that energy travels as particles.

Question 60

Quanta/Quantum means what?

Answer 60

- particles of energy | - carry a defined amount of energy

Question 61

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

Answer 61

photoelectric effect

Question 62

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

Answer 62

emission

Question 63

Energy =

Answer 63

(h)(f) | plank's constant)(frequency

Question 64

The spectroscope separates light into different what?

Answer 64

wavelengths (and, therefore, colors)

Question 65

1 Angstrom =

Answer 65

1 x10 ^-10 meters

Question 66

The emission/absorption spectrum is a part of what?

Answer 66

Particle theory

Question 67

The emission spectrum is also called the ______ ____ spectrum.

Answer 67

bright line

Question 68

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

Answer 68

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

Question 69

A ______ is released as energy.

Answer 69

photon

Question 70

The high-energy state is what?

Answer 70

excited state

Question 71

The low-energy state is what?

Answer 71

ground state

Question 72

The absorption spectrum is also called the what?

Answer 72

Dark line spectrum

Question 73

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

Answer 73

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

Question 74

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

Answer 74

Einstein

Question 75

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

Answer 75

wave and a particle

Question 76

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

Answer 76

Heisenberg Uncertainty Principle