Name: _____________________________
Date: ___________________________
Ground vs. Excited States
Homework Unit 7 - Topic 2
1. When electrons in an atom in the excited
6. Which principal energy level change by the
state fall back to lower energy levels, energy
electron of a hydrogen atom will cause the
Assignment:
Practice with Ground
& Excited
is
the greatest
amount of energy to be
absorbed?
1) absorbed, only
2) released,
1. When
electrons only
in an atom in the excited state fall
3) neither
nor absorbed
back
to lowerreleased
energy levels,
energy is
4) both released and absorbed
1. absorbed, only
2. 2.What
is theonly
total number of valence electrons
released,
3.in neither
released
absorbed
a fluorine atomnor
in the
ground state?
4.1)both
released
and
absorbed
5
2) 2
2. What is the total number of valence electrons in a
3) 7 atom in the ground state?
fluorine
4) 9
1. 5
3. 2.When
2 the electrons of an excited atom return
to
3. 7a lower energy state, the energy emitted
4.can9 result in the production of
1) lightening
3. When
the electrons of an excited atom return to a
2) isotopes
lower energy state, the energy emitted can result
3) protons
in the production of
4) spectra
1. lightening
4. The diagram shows the characteristic spectral
2. isotopes
patterns of four elements. Also shown are
3.line
protons
spectral lines produced by an unknown
4.the
spectra
substance. Which pair of elements is present
4. in the unknown?
1) lithium and sodium
The diagram
shows
thehydrogen
characteristic spectral line
2) sodium
and
patterns
of
four
elements.
Also shown are spectral
3) lithium and helium
lines produced
by
an
unknown
4) helium and hydrogensubstance. Which pair
of elements is present in the unknown?
5. Compared to a sodium atom in the ground
1.state,
lithium
and sodium
a sodium
atom in the excited state
2.must
sodium
and
hydrogen
have
3. lithium and helium
a greater
number of electrons
4.1)helium
and hydrogen
2) a smaller number of electrons
3) an electron with greater energy
4) an electron with less energy
Regents & IB Chemistry 11
n = 2 to to
n=
4
5. 1)Compared
a sodium
atom in the ground state, a
sodium
atom
in
the
excited
state must have
2) n = 2 to n = 5
3) n = 4 to n = 2
1. a greater number of electrons
4) n = 5 to n = 2
2. a smaller number of electrons
3. an electron
with greater
7. Spectral
lines produced
fromenergy
the radiant
4. an electron with less energy
energy emitted from excited atoms are
to be due
to thelevel
movements
ofthe
6. thought
Which principal
energy
change by
electrons
electron of a hydrogen atom will cause the
amount
energy
to be absorbed?
1)greatest
from lower
toof
higher
energy
levels
2) form higher to lower energy levels
1. n = 2 to n = 4
3) within their orbitals
2. n = 2 to n = 5
4)3. out
n =of4 the
to n nucleus
=2
4. n = 5 to n = 2
8. What is the electron configuration of a sulfur
in the
excited
state?
7. atom
Spectral
lines
produced
from the radiant energy
emitted
from excited atoms are thought to be due to
1) 2-4
the movements of electrons
2) 2-6
3) 2-8-6
1. from lower to higher energy levels
4)2. 2-8-5-1
from higher to lower energy levels
3. within their orbitals
9. Electron X can change to a higher energy
4. out of the nucleus
level or lower energy level. Which statement
true of
electron
X? configuration of a sulfur atom
8. isWhat
is the
electron
the excited
state? energy when it changes
1)in Electron
X emits
to a higher energy level.
1. 2–4
2) Electron X absorbs energy when it
2. 2–6
3. changes
2–8–6 to a higher energy level.
3)4. Electron
2–8–5-1X absorbs energy when it
changes to a lower energy level.
9. 4)Electron
X can
changeemits
to a higher
energy level or
Electron
X neither
nor absorbs
a lower
energy
level.
Which
statement
is true of
energy when it changes energy level.
electron X?
1. Electron X emits energy when it changes to a
higher energy level.
2. Electron X absorbs energy when it changes to
a higher energy level.
3. Electron X absorbs energy when it changes to
a lower energy level.
4. Electron X neither emits nor absorbs energy
when it changes energy level.
Unit 7, Topic 2: Ground vs. Excited State
Name: _____________________________
Date: ___________________________
Choose from the following set of answers for
questions 10-12:
1.
2.
3.
4.
2-7
2-8
2-8-1
2-7-1-1
11. _____ Represents the electron configuration
of the Na+1 ion.
12. _____ Represents an excited state electron
configuration for an atom of sodium.
13. The characteristic bright-line spectrum of an
element is produced when its electrons
10. _____ Represents the electron configuration
of an atom of sodium in the ground state.
1)
2)
3)
4)
form a covalent bond
form an ionic bond
move to a higher energy state
return to a lower energy state.
Draw Bohr diagram of
atom in ground state
Draw Bohr diagram of
atom in excited state
Draw Bohr diagram of ION
Electron Configuration:
_________________________
Electron Configuration:
_________________________
Electron Configuration:
_________________________
Electron Configuration:
_________________________
Electron Configuration:
_________________________
Electron Configuration:
_________________________
Sodium
Fluorine
Regents & IB Chemistry 11
Unit 7, Topic 2: Ground vs. Excited State
Name: _____________________________
Date: ___________________________
Emission Spectrum Identification
Enter the name of the
element fromSpectrum
the list on the Identification
left beside its spectrum of
Assignment:
Emission
absorption on the right.
Regents & IB Chemistry 11
Unit 7, Topic 2: Ground vs. Excited State