Chemistry: Matter and Change

1
Section 5-3
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
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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.
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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.

4
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.

• Hunds 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.

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

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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.

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Section 5-3
Valence Electrons

• Valence electrons are defined as electrons in the
  atoms outermost orbitalsthose associated with
  the atoms highest principal energy level. (found
  in s p orbitals only)

• Electron-dot structure consists of the elements
  symbol representing the nucleus, surrounded by
  dots representing the elements valence electrons.

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Section 5-3
Valence Electrons (cont.)
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Section 5-3
Section 5.3 Assessment
In the ground state, which orbital does an atoms
electrons occupy? A. the highest
available B. the lowest available C. the n 0
orbital D. the d suborbital

1. A
2. B
3. C
4. D

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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

1. A
2. B
3. C
4. D

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• STOP

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Resources Menu
Chemistry Online Study Guide Chapter
Assessment Standardized Test Practice Image
Bank Concepts in Motion
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Study Guide 1
Section 5.1 Light and Quantized Energy
Key Concepts

• All waves are defined by their wavelengths,
  frequencies, amplitudes, and speeds. c ??

• 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.Equantum h?

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Study Guide 1
Section 5.1 Light and Quantized Energy (cont.)
Key Concepts

• White light produces a continuous spectrum. An
  elements emission spectrum consists of a series
  of lines of individual colors.

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Study Guide 2
Section 5.2 Quantum Theory and the Atom
Key Concepts

• Bohrs atomic model attributes hydrogens
  emission spectrum to electrons dropping from
  higher-energy to lower-energy orbits. ?E E
  higher-energy orbit - E lower-energy orbit E
  photon h?

• The de Broglie equation relates a particles
  wavelength to its mass, its velocity, and
  Plancks constant. ? h / m?
• The quantum mechanical model of the atom assumes
  that electrons have wave properties.
• Electrons occupy three-dimensional regions of
  space called atomic orbitals.

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Study Guide 3
Section 5.3 Electron Configuration
Key Concepts

• The arrangement of electrons in an atom is called
  the atoms electron configuration.

• Electron configurations are defined by the aufbau
  principle, the Pauli exclusion principle, and
  Hunds rule.
• An elements valence electrons determine the
  chemical properties of the element.
• Electron configurations can be represented using
  orbital diagrams, electron configuration
  notation, and electron-dot structures.

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

1. A
2. B
3. C
4. D

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

1. A
2. B
3. C
4. D

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Chapter Assessment 3
Atoms move in circular orbits in which atomic
model? A. quantum mechanical model
B. Rutherfords model C. Bohrs model
D. plum-pudding model

1. A
2. B
3. C
4. D

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Chapter Assessment 4
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

1. A
2. B
3. C
4. D

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

1. A
2. B
3. C
4. D

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

1. A
2. B
3. C
4. D

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

1. A
2. B
3. C
4. D

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STP 3
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

1. A
2. B
3. C
4. D

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

1. A
2. B
3. C
4. D

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STP 5
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

1. A
2. B
3. C
4. D

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CIM
Figure 5.11 Balmer Series Figure 5.12 Electron
Transitions Table 5.4 Electron Configurations
and Orbital Diagrams for Elements 110 Table 5.6
Electron Configurations and Dot Structures
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