Quantum Model of the Atom

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Quantum Model of the Atom

• Electrons in Atoms

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Bohr Model

• Auf Bau Electrons are placed in the lowest
  energetically available subshell.

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Auf bau
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Electron Configuration
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What is the maximum number of electrons that can
occupy the f orbital?

1. A. 10
2. B. 14
3. C. 18
4. D. 22

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A neutral atom has electron configuration
1s22s22p63s23p2. What element is this?

1. A. carbon
2. B. nitrogen
3. C. silicon
4. D. germanium

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A neutral atom has an electronconfiguration of
1s22s22p63s1.What is its atomic number?

1. A. 5
2. B. 11
3. C. 14
4. D. 20

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How many electrons completely fill the 3rd
energy level?

1. A. 8
2. B. 14
3. C. 18
4. D. 32

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What is the electron configuration for Lithium?

1. A. 1s3
2. B. 1s12s2
3. C. 1s22s1
4. D. 1s21p1

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The letter designations for the first four
orbital quantum numbers with the number of
electrons per orbital at each sublevel are

1. s2, p8, d 18, f 32
2. s1, p3, d 5, f 7
3. s2, p6, d 10, f 14
4. s1, d6, p10, f 14

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A neutral atom has an electron configuration of
1s22s22p6. what is the ground state configuration
of an element that possesses one more electron?

1. A. 1s22s22p63s1
2. B. 1s22s22p7
3. C. 1s22s32p6
4. D. none of the given answers

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Notation

• Longhand Configuration

S 16e-
2s2
2p6
1s2
3s2
3p4

• Shorthand Configuration

S 16e- Ne 3s2 3p4
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Stability

• Full energy level

• Full sublevel (s, p, d, f)

• Half-full sublevel

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Stability

• Electron Configuration Exceptions

• Copper

EXPECT Ar 4s2 3d9
ACTUALLY Ar 4s1 3d10

• Copper gains stability with a full d-sublevel.

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Stability

• Electron Configuration Exceptions

• Chromium

EXPECT Ar 4s2 3d4
ACTUALLY Ar 4s1 3d5

• Chromium gains stability with a half-full
  d-sublevel.

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Stability

• Ion Formation
• Atoms gain or lose electrons to become more
  stable.
• Isoelectronic with the Noble Gases.

3
1
2
NA
3-
2-
1-
0
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Stability

• Ion Electron Configuration
• Write the e- config for the closest Noble Gas
• EX Oxygen ion ? O2- ? Ne

O2- 10e- He 2s2 2p6
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The electron configuration of CL- is

1. a. Ne 2s22p6
2. b. Ne 3s23p5
3. c. Ne 2s23p6
4. d. Ne 3s23p6

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The electron configuration of sILVER is

1. a. Kr 5s25d9
2. b. Kr 5s24d10
3. c. Kr 5s14d10
4. d. Kr 5s24d9

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The electron configuration of the ion that
Potassium forms is

1. a. Ne 3s23p6
2. b. Ar 4s2
3. c. Ar 4s1
4. d. Ar 4s24p6

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The electron configuration of the ion formed when
te gains stability is

1. a. Kr 5s24d105p4
2. b. Xe 5s24d105p6
3. c. Kr 5s25d105p6
4. d. Kr 5s24d105p6

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Orbits vs. orbitals
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Quantum Mechanics

• Orbital (electron cloud)
• Region in space where there is 90 probability of
  finding an e-

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Heisenberg Uncertainty Principle

• Impossible to know both the velocity and position
  of an electron at the same time

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S and p orbitals
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Schrodinghers cloud models
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D orbitals
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If the accuracy in measuring the position of a
particle increases, the accuracy in measuring its
velocity will

1. A. increase
2. B. decrease
3. C. remain the same
4. D. be uncertain

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The reason the position of a particle cannot be
specified with infinite precision is the

1. A. exclusion principle.
2. B. uncertainty principle.
3. C. photoelectric effect.
4. D. principle of relativity.

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Quantum Numbers

• Four Quantum Numbers
• Specify the address of each electron in an atom

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Quantum Numbers

• 1. Principal Quantum Number ( n )
• Main Energy level
• Size of the orbital

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Quantum Numbers

• 2. Angular Momentum Quantum ( l )
• Energy sublevel
• Shape of the orbital

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Quantum Numbers

• 3. Magnetic Quantum Number ( ml )
• Orientation of orbital (x,y,z)
• Specifies the exact orbitalwithin each sublevel

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Quantum Numbers
px
py
pz
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A spherical electron cloud surrounding an atomic
nucleus would best represent

1. A. an s orbital
2. B. a px orbital
3. C. a px and py orbital
4. D. a d orbital

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Which orbitals are dumbbell shaped along the x, y
and z axis?

1. A. s
2. B. p
3. C. d
4. D. f

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Quantum Numbers

• Orbitals combine to form a spherical shape.

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Quantum Numbers

• n of sublevels per level
• n2 of orbitals per level
• Sublevel sets 1 s, 3 p, 5 d, 7 f

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Quantum Numbers

• 4. Spin Quantum Number ( ms )
• Electron spin ? ½ or -½
• An orbital can hold 2 electrons that spin in
  opposite directions.

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How many quantum numbers are used to describe the
energy state of an atom?

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

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Quantum Numbers

• Pauli Exclusion Principle
• No two electrons in an atom can have the same 4
  quantum numbers.
• Each e- has a unique address

1. Principal ? 2. Ang. Mom. ? 3. Magnetic
? 4. Spin ?
energy level sublevel (s,p,d,f) Orbital
(X,Y,Z) Electron (1/2, -1/2)
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The quantum number that indicates the position of
an orbital about the three axes in space is

1. A. principal
2. B. angular momentum
3. C. magnetic
4. D. spin

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How many different orbital shapes can an f
sublevel have?

1. A. 3
2. B. 6
3. C. 5
4. D. 7

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The spin quantum number indicates that maximum
capacity for electrons within an orbital is

1. A. 1
2. B. 2
3. C. 6
4. D. 8

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The principal quantum number, n,determines the
____________ of the orbital

1. A. Orientation
2. B. Energy
3. C. Shape
4. D. Capacity

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How many possible electron orientations are there
in the 4d orbital?

1. A. 5
2. B. 8
3. C. 10
4. D. 14

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• Each orbital can hold TWO electrons with opposite
  spins.

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Hunds Rule

• Orbitals of equal energy must each possess one
  electron before any can possess a second.
• Empty Bus Seat Rule

RIGHT
WRONG
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Orbital Diagram

• Electron Configuration

1s2 2s2 2p4
O 8e-
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Dot structure

• Longhand Configuration

S 16e-
2s2
2p6
1s2
3s2
3p4
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Dot structure
Cl
P
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Feeling overwhelmed?
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