Download genchem study guide test_4a

Study Guide
Chemistry Test #4
Learning Goals for Unit #3:
 To understand why the electron cloud model of the atom is more appropriate than
the orbital model of the atom.
 To understand and apply Heisenberg’s Uncertainty Principle, Aufbau Principle, Pauli
Exclusion Principle and Hund’s Rule to electron configurations.
 To write the longhand and shorthand electronic configurations for a given atom.
 To identify the period number, block and group number for a given atom from its
electron configuration.
 To write the orbital diagram for a given atom or ion.
 To identify the number of valence electrons from an atom’s electron configuration.
 To write a Lewis Dot Diagram for a given atom.
 To explain Planck’s Theory and how the existence of quantized energy levels relate
to atomic emission spectra.
1) Name the four different sublevels/atomic orbitals and include the number of orbitals
and electrons contained in each.
Sublevel/atomic orbital
total number of orbitals
Total number of electrons
s
1
2
p
3
6
d
5
10
f
7
14
2) Identify each of the shapes below as one type of orbital.
f p d s 3) What is the maximum number of energy levels an atom can have? 7 (7 periods in
periodic table)
Study Guide
Chemistry Test #4
4) Describe the electron cloud model of the atom. How is it different from the orbital
model?
Electron cloud shows where electrons are MOST LIKELY to be found (Heisenberg’s
Uncertainty Principle). Orbital model showed electrons in neat, tidy, predictable orbits.
5) What is the name of the outermost/highest energy level called? valence
6) What is the most stable number of valence electrons for all but H and He? 8
7) What is the maximum number of electrons in the 2nd energy level? 3rd energy level?
2nd energy level = 2s2 2p6 = 8 electrons; 3rd energy level = 3s2 3p6 3d10 = 18
8) What types of sublevels/orbitals are in the 2nd energy level? 3rd energy level? 4th
energy level?
2nd energy level = 2s 2p; 3rd energy level = 3s 3p 3d; 4th energy level = 4s 4p 4d 4f
9) How many valence electrons does a phosphorus atom have? Which energy level?
Phosphorus 1s22s2p63s23p3
5 valence electrons in the 3rd energy level
10) What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p, 4s, 3d… 4p
11) Using the picture below, identify the correctly filled diagram for carbon.
12) Draw the Lewis Dot Structure for carbon. Study Guide
Chemistry Test #4
13) Which of the following elements has the most stable number of valence electrons?
a) Mg
b) Al
c) O
d) Ar
quantum
14) When a ground state electron absorbs a ___________________ of energy, it jumps to
an excited state.
photon
15) When an excited electron returns to the ground state, a ____________________ of
energy is released.
visible
16) Atomic emission spectrum is the set of __________________ light spectral lines that an
element can emit when its electrons return to their ground state positions.
emission
17) Examples of ____________________ spectra include: fireworks, neon lights, stars,
identifying metals by burning them in a flame test.
d
s
18) Zirconium is found in the _______ block. Strontium is found in the _______ block.
f
p
19) Plutonium is found in the ________ block. Silicon is found in the ________ block.
Study Guide
Chemistry Test #4
20) Write the aufbau/orbital diagram and electron configuration for aluminum (Al).
1s2 2s2 2p6 3s2 3p1
21) Write the noble gas configuration for bohrium (Bh)
[Ar] 4s2 3d10
22) Write the noble gas configuration for zinc (Zn). [Rn] 7s2 5f14 6d5
23) Write the longhand configuration for arsenic (As).
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
24) Identify the element with the configuration [Kr] 5s2 4d7
Rhodium (Rh)
25) Identify the element with the configuration [Xe] 6s2 4f14 5d10
Mercury (Hg)
26) What is the highest energy level that contains electrons in a chlorine atom?
27) Identify the element with 5 valence electrons in the 3rd energy level.
28) Identify the element with 2 electrons in the 4d sublevel.
3
P
Zr
29) Identify the element with 14 electrons in the 5f sublevel and 5 in the 6d sublevel.
Bh
4
30) An element that has a configuration of [Ar] 4s2 3d4 is found in period ______.
14
31) An element that has a configuration of [Kr] 5s2 4d7 5p2 is found in group # ______.
32) In which sublevel, 3p or 5s, is the probability of identifying an electron’s location,
higher? Why?
The probability is higher in the 3p because it has less energy, so it moves more slowly.
33) What does an aubau/orbital diagram tell us about an atom and its configuration?
The orbital diagram shows total number of electrons, the sublevels and orbitals that
contain the electrons including how many in each, and the relative spin of electrons. It
demonstrates the Pauli Exclusion Principle, Hund’s Rule and the aufbau principle.
Study Guide
Chemistry Test #4
Matching
M
Atomic emission spectra O
Aufbau Principle R
Electron cloud I
Electron Configuration J
Lewis Dot Formula P
Energy level C
Energy sublevel F
D
Heisenberg’s Uncertainty Principle Hund’s Rule G
Orbital B
Pauli Exclusion Principle N
Photon A
Planck’s Theory E
Quantum Leap K
Quantum Numbers H
Shorthand Configuration L
Valence Electrons Q
Visible Spectrum A Energy absorbed, electron leaps from ground state to excited state, electron falls and emits energy B Only a max of 2 electrons in each orbital and they must have opposite spins C Subdivision of energy level; the numeric value of energy level is equal to the total number of these in that energy level D Empty Bus Seat Rule; electrons occupy equal‐
energy orbitals so that a maximum number of unpaired electrons results E when an electron jumps from one energy level position to another F You cannot know the location and momentum of an electron at the same time G Hold a maximum of 2 electrons; H Configuration using noble gases as a “landmark” in order to shorten representation I This shows the number of electrons in each sublevel in each energy level of ground‐state atom J Shorthand way of showing number of valence electrons in an atom K These describe certain aspects of the locations of electrons; n, l, m, s L Located in the outermost energy level of an atom M A spectrum that originates from a material (usually a gas) and contains patterns that are characteristic of the elements present in the material. N The light energy released of a very specific energy and frequency; may relate to color if it is visible light O Lazy Tennant Rule; electrons fill lowest energy orbitals first P 3 dimensional regions of space around nucleus where electrons are most likely to be found; aka shell Q If the photon of energy emitted has a wavelength in this region, you will see color R The area around the nucleus comprised of all the energy levels; probability of location of electrons is greatest near the nucleus