Transcript III. Quantum Model of the Atom

QUANTUM MODEL
OF THE ATOM
Electrons in Atoms
BOHR MODEL

Auf Bau –
Electrons are
placed in the
lowest
energetically
available
subshell.
AUF BAU
ELECTRON CONFIGURATION
WHAT IS THE MAXIMUM NUMBER OF
ELECTRONS THAT CAN OCCUPY THE F ORBITAL?
1.
2.
3.
4.
A. 10
B. 14
C. 18
D. 22
0%
1
0%
2
0%
3
0%
4
A NEUTRAL ATOM HAS ELECTRON
CONFIGURATION 1S22S22P63S23P2. WHAT
ELEMENT IS THIS?
1.
2.
3.
4.
A. carbon
B. nitrogen
C. silicon
D. germanium
0%
1
0%
2
0%
3
0%
4
A NEUTRAL ATOM HAS AN ELECTRON
CONFIGURATION OF 1S22S22P63S1.
WHAT IS ITS ATOMIC NUMBER?
1.
2.
3.
4.
A. 5
B. 11
C. 14
D. 20
0%
1
0%
2
0%
3
0%
4
How many electrons completely fill the 3rd energy
level?
1.
2.
3.
4.
A. 8
B. 14
C. 18
D. 32
0%
1
0%
2
0%
3
0%
4
WHAT IS THE ELECTRON CONFIGURATION FOR
LITHIUM?
1.
2.
3.
4.
A. 1s3
B. 1s12s2
C. 1s22s1
D. 1s21p1
0%
1
0%
2
0%
3
0%
4
The letter designations for the first four orbital
quantum numbers with the number of electrons
per orbital at each sublevel are:
A.
B.
C.
D.
s:2, p:8, d: 18, f: 32
s:1, p:3, d: 5, f: 7
s:2, p:6, d: 10, f: 14
s:1, d:6, p:10, f: 14
0%
A.
0%
B.
0%
C.
0%
D.
A NEUTRAL ATOM HAS AN ELECTRON CONFIGURATION
OF 1S22S22P6. WHAT IS THE GROUND STATE
CONFIGURATION OF AN ELEMENT THAT POSSESSES
ONE MORE ELECTRON?
1.
2.
3.
4.
A. 1s22s22p63s1
B. 1s22s22p7
C. 1s22s32p6
D. none of the
given answers
0%
1
0%
2
0%
3
0%
4
NOTATION

Longhand Configuration
S 16e- 1s2 2s2 2p6 3s2 3p4
Core Electrons
Valence Electrons
Shorthand Configuration
S
16e
2
4
[Ne] 3s 3p
STABILITY
Full energy level
Full sublevel (s, p, d, f)

Half-full sublevel
1
2
3
4
5
6
7
STABILITY

Electron Configuration Exceptions
Copper
EXPECT:
[Ar] 4s2 3d9
ACTUALLY:
[Ar] 4s1 3d10
Copper gains stability with a full
d-sublevel.
STABILITY

Electron Configuration Exceptions
Chromium
EXPECT:
[Ar] 4s2 3d4
ACTUALLY:
[Ar] 4s1 3d5
Chromium gains stability with a half-full
d-sublevel.
STABILITY

Ion Formation
 Atoms
gain or lose electrons to become more
stable.
 Isoelectronic with the Noble Gases.
1
2
3
4
5
6
7
STABILITY

Ion Electron Configuration
 Write
 EX:
the e- config for the closest Noble Gas
Oxygen ion  O2-  Ne
2O
10e
[He]
2
2s
6
2p
THE ELECTRON CONFIGURATION OF CL IS :
1.
2.
3.
4.
a. [Ne] 2s22p6
b. [Ne] 3s23p5
c. [Ne] 2s23p6
d. [Ne] 3s23p6
0%
1
0%
2
0%
3
0%
4
THE ELECTRON CONFIGURATION OF SILVER IS :
1.
2.
3.
4.
a. [Kr] 5s25d9
b. [Kr] 5s24d10
c. [Kr] 5s14d10
d. [Kr] 5s24d9
0%
1
0%
2
0%
3
0%
4
THE ELECTRON CONFIGURATION OF THE ION THAT
POTASSIUM FORMS IS:
1.
2.
3.
4.
a. [Ne] 3s23p6
b. [Ar] 4s2
c. [Ar] 4s1
d. [Ar] 4s24p6
0%
1
0%
2
0%
3
0%
4
THE ELECTRON CONFIGURATION OF THE ION
FORMED WHEN TE GAINS STABILITY IS:
100%
1.
2.
3.
4.
a. [Kr] 5s24d105p4
b. [Xe] 5s24d105p6
c. [Kr] 5s25d105p6
d. [Kr] 5s24d105p6
0%
1
0%
2
0%
3
4
ORBITS VS.
ORBITALS
QUANTUM MECHANICS

Orbital (“electron cloud”)
 Region
in space where there is 90% probability
of finding an e-
Orbital
Radial Distribution Curve
HEISENBERG UNCERTAINTY PRINCIPLE
 Impossible
to know both the velocity and
position of an electron at the same time
S AND P ORBITALS
SCHRODINGHER’S CLOUD MODELS
D ORBITALS
IF THE ACCURACY IN MEASURING THE POSITION
OF A PARTICLE INCREASES, THE ACCURACY IN
MEASURING ITS VELOCITY WILL:
1.
2.
3.
4.
A. increase
B. decrease
C. remain the same
D. be uncertain
0%
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3
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THE REASON THE POSITION OF A PARTICLE
CANNOT BE SPECIFIED WITH INFINITE
PRECISION IS THE:
1.
2.
3.
4.
A. exclusion principle.
B. uncertainty principle.
C. photoelectric effect.
D. principle of relativity.
0%
1
0%
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QUANTUM NUMBERS

Four Quantum Numbers:
 Specify
the “address” of each electron in an atom
UPPER LEVEL
QUANTUM NUMBERS
1. Principal Quantum Number ( n )
 Main
 Size
Energy level
of the orbital
QUANTUM NUMBERS
2. Angular Momentum
Quantum # ( l )
s
 Energy
sublevel
 Shape
of the orbital
p
d
f
QUANTUM NUMBERS
3. Magnetic Quantum Number ( ml )
 Orientation
 Specifies
of orbital (x,y,z)
the exact orbital
within each sublevel
QUANTUM NUMBERS
px
py
pz
A spherical electron cloud surrounding an atomic
nucleus would best represent:
1.
2.
3.
4.
A. an s orbital
B. a px orbital
C. a px and py orbital
D. a d orbital
0%
1
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2
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4
Which orbitals are dumbbell shaped along the x, y
and z axis?
1.
2.
3.
4.
A. s
B. p
C. d
D. f
0%
1
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2
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3
0%
4
QUANTUM NUMBERS

Orbitals combine to form a spherical shape.
2px
2py
2s
2pz
QUANTUM NUMBERS
n = # of sublevels per level
n2 = # of orbitals per level
Sublevel sets: 1 s, 3 p, 5 d, 7 f
QUANTUM NUMBERS
4. Spin Quantum Number ( ms )
 Electron
 An
spin  +½ or -½
orbital can hold 2 electrons that spin in
opposite directions.
How many quantum numbers are used to describe
87%
the energy state of an atom?
1.
2.
3.
4.
A. 1
B. 2
C. 3
D. 4
13%
0%
1
2
0%
3
4
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)
The quantum number that indicates the position of
an orbital about the three axes in space96%
is:
1.
2.
3.
4.
A. principal
B. angular momentum
C. magnetic
D. spin
0%
1
4%
2
0%
3
4
How many different orbital shapes can an f
sublevel have?
1.
2.
3.
4.
100%
A. 3
B. 6
C. 5
D. 7
0%
1
0%
2
0%
3
4
The spin quantum number indicates that
maximum capacity for electrons100%
within an orbital
is:
1.
2.
3.
4.
A. 1
B. 2
C. 6
D. 8
0%
1
0%
2
3
0%
4
THE PRINCIPAL QUANTUM NUMBER, N,
DETERMINES THE ____________
OF THE
100%
ORBITAL
1.
2.
3.
4.
A. Orientation
B. Energy
C. Shape
D. Capacity
0%
1
0%
2
3
0%
4
HOW MANY POSSIBLE ELECTRON
ORIENTATIONS ARE THERE
IN THE 4D ORBITAL?
100%
1.
2.
3.
4.
A. 5
B. 8
C. 10
D. 14
0%
1
2
0%
3
0%
4
 Each
orbital can hold TWO electrons with
opposite spins.
HUND’S RULE

Orbitals of equal energy must each possess
one electron before any can possess a
second.
 “Empty
Bus Seat Rule”
WRONG
RIGHT
Electron Configuration
2
1s
2
2s
1s
2s
ORBITAL DIAGRAM
4
2p
O
8e-
2p
DOT STRUCTURE

Longhand Configuration
S 16e- 1s2 2s2 2p6 3s2 3p4
Core Electrons
Valence Electrons
DOT STRUCTURE
Cl
P
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Chapter 10