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Name_______________________________
Date:______________
Period:______
REVIEW Unit 1 Test (Chp 6,7): Atoms, Electrons, & Periodic Properties
1.
The frequency of electromagnetic radiation is ___________ proportional to the wavelength and
__________ proportional to the energy of the waves.
2.
Of the following, __________ radiation has the longest wavelength and __________ radiation has the
most energy.
X-ray
infrared
microwave
3.
What color of visible light has the shortest wavelength?
4.
In which orbital does an electron in a bromine atom experience the least shielding?
(A) 3s
5.
(B) 3p
(C) 3d
(D) 4s
(E) 4p
[Kr] 5s2 4d10 5p2 is the electron configuration of a(n) ____ atom.
(A) Ge
(B) Sr
(C) I
(D) Sn
(E) Te
6.
List all of the elements in the 4th period that are paramagnetic.
7.
The principle quantum number for the outermost electron in a scandium atom is _____.
8.
Write the electron configuration for the Fe+3 ion.
9.
Electrons in the 2p subshell are much further from the nucleus in C than in Sn due to
_________________ in C.
10.
List one element that could replace calcium in a chemical reaction.
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11.
In general, as you go down a group and across a period in the periodic table:
(1) the atomic radius gets __________ and __________.
(2) the electronegativity gets___________ and __________.
(3) the first ionization energy gets __________ and __________.
12.
Electronegativity gets ________________ across a period toward the noble gases which all have
_______ electronegativities.
13.
Name the group with the lowest first ionization energy and the group with the highest.
Lowest: ________________________
14.
Highest: ________________________
Write an equation for the 1st ionization of magnesium and an equation for the 2nd ionization of Mg.
Ionization Energies for Element X
Ionization Energy
(kJ mol-1)
1st
2nd
3rd
4th
5th
6th
7th
787
1,580
3,200
4,400
16,000
20,000
24,000
___15. The first seven ionization energies of element X are shown in the above. On the basis of these data,
element X is most likely a member of which of the following groups (families) of elements?
(A)
(B)
(C)
(D)
(E)
Alkaline earth metals
Boron group
Carbon group
Nitrogen group
Halogen group
___16. If a metal M forms an ionic chloride with the formula MCl3, then which of the following formulas is
most likely to be that of a stable sulfide of M?
(A) MS2
17.
(B) M2S3
(C) MS6
(D) M(SO3)3
(E) M2(SO3)3
1s2 2s2 2p6 3s1
Atoms of an element, J, have the electronic configuration shown above. The compound element J
will most likely form with oxygen, O, is…
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18.
List 5 characteristics of metals:
19.
Which group has the most reactive metals? Explain.
Which group has the most reactive nonmetals? Explain.
___20. In which of the following groups are the three species isoelectronic?
(i.e. have the same number of electrons?)
(A)
(B)
(C)
(D)
(E)
21.
S2– ,
Sc ,
O2– ,
Mg2+ ,
Cs ,
K+ ,
Ti ,
S2– ,
Ca2+ ,
Ba2+ ,
Ca2+
V2+
Cl–
Sr2+
La3+
Place the answer chosen in #20 above in order of increasing radius.
_____ < _____ < _____
Questions 22-23
Consider atoms of the following elements. Assume that the atoms are in the ground state.
(A) S
(B) Ca
(C) Ga
(D) Sb
(E) Br
___22. The atom that contains exactly two unpaired electrons
___23. The atom that contains only one electron in the highest occupied energy sublevel
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Questions 24-27 refer to neutral atoms for which the atomic orbitals are represented below.
(A) ↑↓
1s
(B) ↑↓ ↑
1s 2s
↑ ↑ ↑.
2p
(C) ↑↓ ↑↓
1s 2s
↑ ↑ ↑
2p
(D) ↑↓ ↑↓
1s 2s
↑↓ ↑↓ ↑↓
2p
(E) [Ar] ↑↓
4s
↑↓ ↑↓ ↑↓ ↑ ↑
3d
___24. Is in an excited state
___25. Has exactly five valence electrons
___26. Has the highest first ionization energy
___27. Forms an aqueous cation that is colored
Use these answers for questions 28-31.
(A) 1s2 2s2 2p6 3s2 3p5
(B) 1s2 2s2 2p6 3s2 3p6
(C) 1s2 2s2 2p6 2d10 3s2 3p6
(D) 1s2 2s2 2p6 3s2 3p6 3d5
(E) 1s2 2s2 2p6 3s2 3p6 3d3 4s2
___28. An impossible electronic configuration
___29. The ground-state configuration for the atoms of a transition element
___30. The ground-state configuration of a negative ion of a halogen
___31. The ground-state configuration of a common ion of an alkaline earth element
Use these answers for questions 32-33.
(A) O
(B) La
(C) Rb
(D) Mg
(E) N
___32. What is the most electronegative element of the above?
___33. Which of the elements above has the smallest ionic radius for its most commonly found ion?
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___34. The elements in which of the following have most nearly the same atomic radius?
(A) Be, B, C, N
(B) Ne, Ar, Kr, Xe
(C) Mg, Ca, Sr, Ba
(D) C, P, Se, I
(E) Cr, Mn, Fe, Co
___35. Which of the following properties generally decreases across the periodic table from sodium to
chlorine?
(A)
(B)
(C)
(D)
(E)
First ionization energy
Atomic mass
Electronegativity
Maximum value of oxidation number
Atomic radius
___36. Define the following terms:
(A) nuclear charge –
(B) effective nuclear charge –
(C) shielding effect –
(D) ionization energy –
(E) electronegativity –
___37. The photoelectron spectra below show the energy required to remove a 1s electron from a nitrogen
atom and from an oxygen atom. Which of the following statements best accounts for the peak in the
upper spectrum being to the right of the peak in the lower spectrum?
(A) Nitrogen atoms have a half-filled p subshell.
(B) There are more electron-electron repulsions
in oxygen atoms than in nitrogen atoms.
(C) Electrons in the p subshell of oxygen atoms
provide more shielding than electrons in the
p subshell of nitrogen atoms.
(D) Nitrogen atoms have a smaller nuclear
charge than oxygen atoms.
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Section II Free Response
Calculator Allowed
CLEARLY SHOW THE METHODS USED AND STEPS INVOLVED IN YOUR ANSWERS.
It is to your advantage to do this, because you may earn partial credit if you do and little or no credit if you
do not. Attention should be paid to significant figures.
1. Answer the following questions regarding light and its interactions with molecules, atoms, and ions.
(a) A certain line in the spectrum of atomic hydrogen is associated with the electronic transition in
the H atom from the second energy level (n=2) to the fifth energy level (n=5).
(i) Indicate whether the H atom emits energy or whether it absorbs energy during the transition.
Justify your answer.
(ii) Calculate the wavelength, in nanometers, of light that corresponds to this line with an
energy of 4.63 x 10–19 J.
O3(g) UV
 O2(g) + O(g)
(b) In the upper atmosphere, ozone molecules decompose as they absorb ultraviolet (UV) radiation,
as shown by the equation above. Ozone serves to block harmful ultraviolet radiation that comes
from the Sun. A molecule of O3(g) absorbs a photon with a frequency of 1.00  1015 s–1.
(i) How much energy, in joules, does the O3(g) molecule absorb per photon?
(ii) The minimum energy needed to break an oxygen-oxygen bond in ozone is 387 kJ mol–1.
Does a photon with a frequency of 1.00  1015 s–1 have enough energy to break this bond?
Support your answer with a calculation.
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Your responses to these questions will be graded on the basis of the accuracy and relevance of the
information cited. Explanations should be clear and well organized. Examples and equations may be
included in your responses where appropriate. Specific answers are preferable to broad, diffuse responses.
2. Use principles of atomic structure and/or chemical bonding to answer each of the following.
K
Ca
Ionization Energy
(kJ/mol)
First
Second
419
3,050
590
1,140
(a) Explain the difference between Ca and K in regard to
(i) their first ionization energies,
(ii) their second ionization energies
(b) The first ionization energy of aluminum is lower than the first ionization energy of magnesium.
(First ionization energies: 12Mg = 7.6 eV; 13Al = 6.0 eV)
(c) For magnesium, the difference between the second and third ionization energies is much larger
than the difference between the first and second ionization energies.
(Ionization energies for Mg: 1st = 7.6 eV; 2nd = 14 eV; 3rd = 80 eV)
(d) A neutral atom of which of these four elements has the largest radius? K, Ca, Mg, Al
(e) Which of these four elements (K, Ca, Mg, Al) is the least metallic?
(f) Write the complete electron configuration for calcium.
(g) What is the most common charge for calcium ions? Explain.
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3. Consider an unknown element J that has the electron configuration [Rn]7s25f146d107p1.
(a) What is the number of the group to which J belongs in the periodic table?
(b) Would J be a metal or a nonmetal? Explain in terms of electron configuration.
(c) On the basis of periodic trends, would J have the largest atomic radius in its group or would it
have the smallest? Explain in terms of electronic structure.
(d) What would be the most likely charge of the J ion in stable ionic compounds?
(e) Assume that J reacts to form a nitrate compound.
–
Write the formula for the compound formed between J and the nitrate ion, NO3 .
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4. Using principles of atomic and molecular structure and the information in the table below, answer the
following questions about atomic fluorine, oxygen, and xenon, as well as some of their compounds.
Atom
First Ionization
Energy (kJ mol–1)
F
1,681.0
O
1,313.9
Xe
?
(a) Write the equation for the ionization of atomic fluorine that requires 1,681.0 kJ mol–1.
(b) Account for the fact that the first ionization energy of atomic fluorine is greater than that of
atomic oxygen. (You must discuss both atoms in your response.)
(c) Predict whether the first ionization energy of atomic xenon is greater than, less than, or equal to
the first ionization energy of atomic fluorine. Justify your prediction.
(d) The radius of the fluorine atom is smaller than the radius of the fluoride ion, F–.
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Answer Key
1.
2007B #2(b)(c) (modified)
2.
1994D (c)(d) 1987D (c)(d)
3.
2006 #8
4.
2008 #5(a)(b)(c)
(ATOMIC THEORY) (modified)
(modified)
(d) added
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