Section 5.3 Electron Configuration
• Apply the Pauli exclusion principle, the aufbau principle, and Hund's rule to write electron configurations using orbital diagrams and electron configuration notation.
• Define valence electrons, and draw electron-dot structures representing an atom's valence electrons.
electron: a negatively charged, fast-moving particle with an extremely small mass that is found in all forms of matter and moves through the empty space surrounding an atom's nucleus
Section 5-3

Section 5.3 Electron Configuration
(cont.) electron configuration aufbau principle
Pauli exclusion principle
Hund's rule valence electrons electron-dot structure
A set of three rules determines the arrangement in an atom.
Section 5-3

Ground-State Electron Configuration
• The arrangement of electrons in the atom is called the electron configuration .
• The aufbau principle states that each electron occupies the lowest energy orbital available.
Section 5-3

Ground-State Electron Configuration
(cont.)
• The Pauli exclusion principle states that a maximum of two electrons can occupy a single orbital, but only if the electrons have opposite spins.
• Hund’s rule states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same energy level orbitals.
Section 5-3

Ground-State Electron Configuration
(cont.)
Section 5-3

Ground-State Electron Configuration
(cont.)
• Noble gas notation uses noble gas symbols in brackets to shorten inner electron configurations of other elements.
Section 5-3

Ground-State Electron Configuration
(cont.)
• The electron configurations (for chromium, copper, and several other elements) reflect the increased stability of half-filled and filled sets of s and d orbitals.
Section 5-3

Valence Electrons
• Valence electrons are defined as electrons in the atom’s outermost orbitals— those associated with the atom’s highest principal energy level. (found in s & p orbitals only)
• Electron-dot structure consists of the element’s symbol representing the nucleus, surrounded by dots representing the element’s valence electrons.
Section 5-3

Valence Electrons
(cont.)
Section 5-3

Section 5.3 Assessment
In the ground state, which orbital does an atom’s electrons occupy?
A.
the highest available
B.
the lowest available
C.
the n = 0 orbital
D.
the d suborbital
A. A
B. B
C. C
D. D
Section 5-3

Section 5.3 Assessment
The outermost electrons of an atom are called what?
A.
suborbitals
B.
orbitals
C.
ground state electrons
D.
valence electrons
A. A
B. B
C. C
D. D
Section 5-3

STOP

Chemistry Online
Study Guide
Chapter Assessment
Standardized Test Practice
Image Bank
Concepts in Motion
Resources Menu

Section 5.1 Light and Quantized
Energy
Key Concepts
• All waves are defined by their wavelengths, frequencies, amplitudes, and speeds. c = λν
• In a vacuum, all electromagnetic waves travel at the speed of light.
• All electromagnetic waves have both wave and particle properties.
• Matter emits and absorbs energy in quanta.
E quantum
= h ν
Study Guide 1

Section 5.1 Light and Quantized
Energy
(cont.)
Key Concepts
• White light produces a continuous spectrum. An element’s emission spectrum consists of a series of lines of individual colors.
Study Guide 1

Section 5.2 Quantum Theory and the Atom
Key Concepts
• Bohr’s atomic model attributes hydrogen’s emission spectrum to electrons dropping from higher-energy to lower-energy orbits.
∆ E = E higher-energy orbit
E lower-energy orbit
= E photon
= h ν
• The de Broglie equation relates a particle’s wavelength to its mass, its velocity, and Planck’s constant.
λ = h / m ν
• The quantum mechanical model of the atom assumes that electrons have wave properties.
• Electrons occupy three-dimensional regions of space called atomic orbitals.
Study Guide 2

Section 5.3 Electron Configuration
Key Concepts
• The arrangement of electrons in an atom is called the atom’s electron configuration.
• Electron configurations are defined by the aufbau principle, the Pauli exclusion principle, and Hund’s rule.
• An element’s valence electrons determine the chemical properties of the element.
• Electron configurations can be represented using orbital diagrams, electron configuration notation, and electron-dot structures.
Study Guide 3

The shortest distance from equivalent points on a continuous wave is the:
A.
frequency
B.
wavelength
C.
amplitude
D.
crest
A
0%
A. A
B. B
B
0%
C. C
0%
D. D
C
0%
D
Chapter Assessment 1

The energy of a wave increases as ____.
A.
frequency decreases
B.
wavelength decreases
C.
wavelength increases
D.
distance increases
A
0%
A. A
B. B
B
0%
C. C
0%
D. D
C
0%
D
Chapter Assessment 2

Atom’s move in circular orbits in which atomic model?
A.
quantum mechanical model
B.
Rutherford’s model
C.
Bohr’s model
D.
plum-pudding model
A. A
B. B
B
0%
C. C
0%
D. D
C
0%
D A
0%
Chapter Assessment 3

It is impossible to know precisely both the location and velocity of an electron at the same time because:
A.
the Pauli exclusion principle
B.
the dual nature of light
C.
electrons travel in waves
D.
the Heisenberg uncertainty principle
A
0%
B
A. A
B. B
0%
C. C
0%
D. D
C
0%
D
Chapter Assessment 4

How many valence electrons does neon have?
A.
0
B.
1
C.
2
D.
3
A
0%
A. A
B. B
B
0%
C. C
0%
D. D
C
0%
D
Chapter Assessment 5

Spherical orbitals belong to which sublevel?
A.
s
B.
p
C.
d
D.
f
A
0%
A. A
B. B
B
0%
C. C
0%
D. D
C
0%
D
STP 1

What is the maximum number of electrons the 1s orbital can hold?
A.
10
B.
2
C.
8
D.
1
A
0%
A. A
B. B
B
0%
C. C
0%
D. D
C
0%
D
STP 2

In order for two electrons to occupy the same orbital, they must:
A.
have opposite charges
B.
have opposite spins
C.
have the same spin
D.
have the same spin and charge
A
0%
A. A
B. B
B
0%
C. C
0%
D. D
C
0%
D
STP 3

How many valence electrons does boron contain?
A.
1
B.
2
C.
3
D.
5
A
0%
A. A
B. B
B
0%
C. C
0%
D. D
C
0%
D
STP 4

What is a quantum?
A.
another name for an atom
B.
the smallest amount of energy that can be gained or lost by an atom
C.
the ground state of an atom
D.
the excited state of an atom
A
0%
A. A
B. B
B
0%
C. C
0%
D. D
C
0%
D
STP 5

Click on an image to enlarge.
IB Menu

IB 1

IB 2

IB 3

IB 4

IB 5

IB 6

IB 7

IB 8

IB 9

IB 10

IB 11

IB 12

IB 13

IB 14

IB 15

IB 16

IB 17

IB 18

IB 19

IB 20

IB 21

IB 22

Figure 5.11 Balmer Series
Figure 5.12 Electron Transitions
Table 5.4 Electron Configurations and Orbital
Diagrams for Elements 1 –10
Table 5.6 Electron Configurations and
Dot Structures
CIM

Click any of the background top tabs to display the respective folder.
Within the Chapter Outline, clicking a section tab on the right side of the screen will bring you to the first slide in each respective section.
Simple navigation buttons will allow you to progress to the next slide or the previous slide.
The Chapter Resources Menu will allow you to access chapter specific resources from the Chapter
Menu or any Chapter Outline slide. From within any feature, click the Resources tab to return to this slide.
The “Return” button will allow you to return to the slide that you were viewing when you clicked either the Resources or Help tab.
To exit the presentation, click the Exit button on the Chapter Menu slide or hit
Escape [Esc] on your keyboards while viewing any Chapter Outline slide.
Help

This slide is intentionally blank.
End of Custom Shows