PRACTICE PROBLEMS FOR EXAM TWO
CHEM 1311
CHAPTER 4
1. Match the following group or period number with the correct common name?
2
COMMON NAME
a) Alkaline earth elements
b) Alkali metals elements
c) Lanthanides
d) Halogens
e) Noble gases
CORRESPONDING NUMBER
II
VII
VIII
I
VI
3
2. Given the following elements, answer these questions.
Zr
Sn
Ca
Li
Th
Ag
Sb
a) Which is (are) an alkaline earth metal(s)?
b) Which is (are) a representative element(s)?
c) Which is (are) a transition element(s)?
d) Which is (are) metal? nonmetal? metalloid?
3. What type of compound (ionic compound, covalent compound, acid or base) are the following?
a) Ag2SO4
b) Ca(OH)2
c) KCl
d) HNO3
e) NaCH3COO
f) C2H5O
4. What type of electrolytes (strong, weak or non) are the following?
a) KBr
b) H2SO4
c) H2CO3
e) NH4ClO3
f) Ca(OH)2
g) CH4
d) BaSO4
h) NH3
5. Write the total ionic and net ionic equation for this formula unit equation? What are the spectator ions?
2 HF (aq) + Ca(OH)2 (aq) —> CaF2 (aq) + 2 H2O (l)
6. Will a precipitate form when 0.1 M aqueous solutions of AgNO3 (silver (I) nitrate) and NaCl are mixed?
Write the net ionic equation for the reaction. If a precipitate does form, identify the precipitate.
7. Write the balanced equation for the complete reaction of hydrobromic acid (HBr) with calcium hydroxide,
Ca(OH)2.
8. What particular ion would the following elements form? Write the correct symbol and charge of the ion.
a) Al
b) Br
c) Mg
d) Li
e) He
f) Se
9. What type of reaction (displacement ; decomposition ; precipitation ; acid-base ; combination) are the
following:
a)
MgSO3 (s) —> MgO (s) + SO2 (g)
b)
2 H2O2 (l) —> 2 H2O (l) + O2 (g)
c)
2 K (s) + H2 (g) —> 2 KH (s)
d)
Mg (s) + 2 HBr (aq) —> MgBr2 (aq) + H2 (g)
e)
KOH (aq) + HClO3 (aq) —> H2O (l) + KClO3 (aq)
10 Write the correct formula for:
a) chromium (II) hydroxide
b) ammonium phosphate
c) magnesium nitrate
d) aluminum chlorate
e) platinum (IV) iodide
f) calcium sulfate
11. Are the following matched pairs of name and formula CORRECT or INCORRECT. If incorrect, write is
the correct name?
Formula
Name
a)
b)
c)
d)
e)
f)
CaF2
HI
KBr
Na2S
PCl5
Ba(NO3)2
calcium difluoride
iodic acid
potassium bromide
sodium sulfate
phosphorus chloride
barium nitrate
12. Given that H2CO3 is the acid where C has the most common oxidation state, name the following acids:
4
a) H2CO2
b) H2CO4
13. Use the following list of elements in answering the following:
Bromine
Antimony (Sb)
Sulfur
Sodium
a) Which one or ones would likely be able to conduct electricity?
b) Which one or ones would NOT conduct heat well (ignore Sb)?
c) Which one or ones would most likely be hard, shiny solids (ignore Sb)?
d) Which one or ones would most likely be able to form an anion?
14. Will a displacement reaction occur? If yes, complete and balance the equation. If no, explain why.
Mg (s) + ZnCl2 (aq) 
ANSWERS FOR CHAPTER 4 QUESTIONS:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
a) II
b) I
c) VI
d) VII
e) VIII
a) Ca
b) Sn ; Ca ; Li ; Sb
c) Zr ; Ag
d) metals = Zr ; Sn ; Ca ; Li ; Th ; Ag nonmetals = none metalloid = Sb
a) ionic compd
b) base
c) ionic compd
d) acid
e) ionic compd
f) covalent (molecular) compound
a) strong
b) strong
c) weak
d) non
e) strong
f) weak
g) non
h) weak
total ionic:
2[H+ + F- ](aq) + [Ca2+ + 2 OH- ](aq) —> [Ca2+ + 2 F-](aq) + 2 H2O(l)
net ionic:
H+(aq) + OH-(aq) —> H2O(l)
spectator ions: Ca2+ and F1Ag+ (aq) + Cl- (aq) —> AgCl (s) ; yes, AgCl precipitates
2 HBr (aq) + Ca(OH)2 (aq) —> 2 H2O(l) + CaBr2 (aq)
a) Al3+
b) Brc) Mg2+
d) Li+
e) none
f) Se2a) decomposition
b) decomposition
c) combination
d) displacement
e) acid-base
neutralization
a) Cr(OH)2
b) (NH4)3PO4
c) Mg(NO3)2
d) Al(ClO3)3
e) PtI4
f) CaSO4
a) incorrect; calcium fluoride
b) incorrect; hydroiodic acid
c) correct
d) incorrect; sodium sulfide
e) incorrect; phosphorus pentachloride
f) correct
a) carbonous acid
b) percarbonic acid
a) Sb and Na
b) S and Br
c) Na
d) Br and S
yes, Mg (s) + ZnCl2 (aq)  Zn (s) + MgCl2 (aq)
CHAPTER 5
1. The number of electrons in a neutral atom of an element is always equal to the __? __ of the element.
2. The mass number of an atom is the number of __?__ in the atom.
3. The atomic number of a certain element is 19 and its atomic weight is 39. How many protons, neutrons and
electrons does the atom have? Write chemical symbol for the element. Also, write the isotopic symbolism for
this atom.
4. Give the number of protons, neutrons, and electrons in an atom of the 87Rb isotope.
5
5. What is the symbol for a species composed of 35 protons, 44 neutrons, and 36 electrons? Write the isotopic
symbol.
6. Are the following statements TRUE or FALSE?
a) Isotopes of an element differ only in the number of protons.
b) The number of protons in an atom is its atomic number.
c) The mass number of an atom is the sum of the number of protons plus electrons in the atom.
d) The volume occupied by the nucleus of an atom represents a large percent of the total volume of the atom.
7. What are the allowed quantum numbers of an electrons for:
n
:
l
:
ml
:
ms
8. a) The maximum number of electrons that can occupy an energy level (n = principal quantum number) is
__?__.
b) The maximum number of electrons that can occupy a 4d orbital (n = 4 ; l = 2 ; ml = -1 ) is __?__.
c) The maximum number of electrons that can occupy a set of orbitals with the subsidiary quantum number,
l = 2 is __?__.
9. Are the following statements TRUE or FALSE?
a) The third major energy level (n = 3) has no f orbitals.
b) There are 10 d orbitals in a set of d orbitals.
c) A set of p orbitals can accommodate a maximum of 6 electrons.
d) A 5d orbital can contain up to 10 electrons.
e) l = 3 corresponds to an electron in a set of f orbitals.
10. Which element has this electronic configuration?
1s22s22p63s23p64s23d104p3
11. What is the electron configuration of tin, Sn? Use the full configuration and the noble gas configuration.
12. Are the following statements TRUE or FALSE?
a) If an electron has the quantum number, n = 3, the electron could be in a d set of orbitals.
b) If an electron has the quantum number, l = 2, the only possible values of ml are 0 and 1.
c) If an electron has ml = -1, it might be in a p, d or f subshell, but not in an s subshell.
d) An electron that has n = 5 cannot be in an f set of orbitals.
e) An electron that has n = 5 could be in an s, p, d or f subshell.
13. An element has the valence configuration of ns2np5 . The element could be _?_.
a) Si
b) P
c) Br
d) Ar
e) Mn
14. Given that an atom has 17 protons and 18 neutrons:
a) What is the name of this element?
b) What is its mass number?
c) What is its atomic number?
d) How many electrons does this atom have?
e) What ion is usually formed by this atom (write symbol and charge)?
f) What is the number of electrons (lost or gained) in ion formation?
g) How many valence electrons does this atom have?
h) What is the electron configuration of this atom?
i) Is this atom a metal, nonmetal or metalloid?
j) What is the common name of the group that this atom belongs?
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15. Given the following:
X has 23 protons, 28 neutrons and 20 electrons.
a) Is X an atom, compound or ion?
b) Write the symbol for X.
16. How many protons, neutrons and electrons do the following contain:
a) Na atom with mass number of 23.
b) Ca2+ with mass number of 41
c) 56 26 X. Identify X?
ANSWERS FOR CHAPTER 5 QUESTIONS:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
atomic number or number of protons
protons plus neutrons
39
19 p
20 n
19 e
K
K
37 p
50 n
37 e
79
Br 1a) false
b) true
c) false
d) false
n: 1, 2, 3, ..., ∞
l: 0, 1, 2, ... , n-1
ml : -l ... , 0 , ... , +l
ms : + ½ and - ½
2
a) 2(n )
b) 2
c) 10
a) true
b) false
c) true
d) false
e) true
As
1s22s22p63s23p64s23d104p65s24d105p2 ;
[Kr]5s24d105p2
a) true
b) false
c) true
d) false
e) true
c) bromine
a) Cl
b) 35
c) 17
d) 17
e) Clf) 1 gained
2 2 6 2 5
g) 7
h) 1s 2s 2p 3s 3p
i) nonmetal j) halogens
a) ion
b) V3+
a) 11p ; 12n ; 11e
b) 20p ; 21n ; 18e
c) 26p ; 26e ; 30n
X = Fe
CHAPTER 6
1. Name the different general types of elements by region and show their location on the periodic table. What is
the outermost orbital (or subshell) being filled?
2. What would be the general valence electron configuration of the following (use nsxnpy notation).
a)
group VI
b)
group VIII
c)
group I
3. Given the following atoms, answer these questions
Sr
Cr
Be
Si
N
a) Which element has the largest atomic radius?
b) Which element has the highest first ionization energy?
c) Which of the following elements has the most negative electron affinity?
d) Which element would form the largest cation?
4. Which of the following species is not isoelectronic with neon?
a) Mg2+
b) Na+
c) O2d) Cle) Al3+
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5. Given the following atoms, answer these questions
Rb
As
S
V
Sb
a) Which element is the smallest atom?
b) Which element is less likely to form a cation?
c) Which element would have the greatest tendency to gain electrons?
d) Which element is the least electronegative?
6. Arrange these elements from lowest to highest electronegativity?
Ga
Mo
P
Ca
N
7. Answer the following questions.
a) Which is smaller?
C
C4+
C4b) Which atom has the ability to pulls electrons in a bond to itself more than the other atoms?
Al
P
Co
Cs
c) Which is larger in size?
Na
Na+
8. Which element has the smallest ionic radius?
a) Cs+
b) Ba2+
c) Tl3+
d) Bi3+
9. Which of the following atoms is least likely to gain electrons to form an anion?
S
P
As
ANSWERS FOR CHAPTER 6 QUESTIONS:
1.
2.
3.
4.
5.
6.
7.
8.
9.
1) representative elements: s or p
a) ns2np4
b) ns2np6
a) Sr
b) N
d) Cl
a) S
b) S
Ca
Mo
Ga
P
N
4+
a) C
b) P
d) Bi3+
As
2) transition elements: d
c) ns1
c) N
d) Sr
c) S
3) lanthanides and actinides: f
d) Rb
c) Na
CHAPTER 7 (part)
1. List any two different properties of an ionic bond.
2. Are the following statements TRUE or FALSE concerning ionic compounds? Why?
a) The ions in the compound share electrons to form bonds.
b) The compounds tend to be gases at room temperature.
c) The compounds have high melting points.
d) Many are water soluble.
e) Aqueous solutions of these compounds are poor conductors of electricity.
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3. Draw the Lewis Dot structure of:
a)
Al
b)
S2-
c)
K+
4. What is the correct Lewis Dot notation for the formation of a Na and F bond?
5. How many valence electrons do the following contain:
a) K
b) P
c) Se
d) Ne
f) P3-
e) Y
6. Predict the number of electrons that will be LOST or GAINED by the following as they become ions?
a) Ca
b) Al
c) F
d) element Z = 34
e) oxygen
7. Explain the octet rule.
ANSWERS FOR CHAPTER 7 QUESTIONS (part):
1.
2.
see notes
a) false
3.
•
a) •Al •
4.
••
Na+ : F : ••
5.
6.
7.
a) 1
a) lose 2
see notes
b) false
c) true
••
b) : S : 2••
c) K+
b) 5
b) lose 3
c) 6
c) gain l
d) true
e) false
d) 8
d) gain 2
e) 2
e) gain 2
f) 8