Download The Structure of the Atom

CHEMISTRY 11
UNIT VIII TEST
The Atom, Periodic Table and Bonding
Part A: Matching Questions
From the list of terms on the right, choose the one that BEST fits the description on the left.
1.
Discovered the atomic nucleus.
A.
ALCHEMISTS
2.
Atoms of the same element that contain different numbers of neutrons.
B.
ALKALI METALS
3.
Devised an equation to predict the energy pattern produced by hydrogen.
C.
ALKALINE EARTH METALS
4.
A great deal of practical chemical knowledge was accumulated from their D.
search for methods of separating metals from ores.
E.
Raison bun or plum pudding model.
F.
Earliest suggestion that matter was composed of atoms.
G.
Particles that have the same electronic configuration.
H.
Subatomic particle not found in the nucleus of the atom.
I.
The number of protons found in the nucleus of the atom.
J.
The total number of protons and neutrons in the nucleus of the atom.
K.
Vertical columns in the periodic table.
L.
Sodium, lithium, and potassium are examples.
M.
The elements in groups 1, 2, and 13 to 18.
N.
A nonmetal having electrical conductivity that increases with
O.
temperature.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
ARISTOTLE
ATOMIC NUMBER
BOHR
COVALENT BOND
DALTON
DEMOCRITUS
ELECTRON
ELECTRONEGATIVITY
GROUPS
IONIZATION ENERGY
ISOELECTRONIC
ISOTOPES
15. Magnesium, Calcium, and Barium are examples.
P.
LONDON FORCES
16. The number of unpaired electrons on the atom.
Q.
MASS NUMBER
17. Results from the equal sharing of electrons.
R.
NEUTRON
18. The tendency for an atom to attract electrons from a neighbouring atom.
S.
NOBLE GASES
19. Horizontal rows in the periodic table.
T.
PERIOD
20. The energy required to remove an electron from a neutral atom.
U.
PROTON
21. Weak attractive forces resulting from momentary dipoles.
V.
REPRESENTATIVE ELEMENTS
22. Helium, neon, and krypton are examples.
W.
RUTHERFORD
23. Iron, zinc, cobalt are examples.
X.
SEMICONDUCTOR
24. Collectively, all the weak intermolecular forces between molecules.
Y.
THOMSON
25. Electrons in the outer shell of an atom.
Z.
TRANSITION METALS
26. A subatomic particle with no charge.
AA.
VALENCE
BB.
VALENCE ELECTRONS
CC.
VAN DER WAALS FORCES
THE ATOM, PERIODIC TABLE AND BONDING
1
CHEMISTRY 11
UNIT VIII TEST
Part B: Multiple-Choice Questions (50 marks)
Select the answer that best completes each statement. Fill in the letter of your choice on the SCANTRON sheet
provided.
1.
Which model described the atom as being composed of randomly distributed positively
and negatively charge particles?
A.
Bohr’s model
B.
Rutherford’s model
C.
Thomson’s model
D.
Dalton’s model
2.
Who performed that “gold foil” experiment?
A.
Dalton
B.
Thomson
C.
Rutherford
D.
Bohr
3.
What did the “gold foil” experiment show?
A.
Atoms have a dense positively-charged nucleus.
B.
Atoms are composed of protons, neutrons, and electrons.
C.
Electrons orbit the nucleus like planets around the Sun.
D.
Electrons exist in quantized energy levels.
4.
The subatomic particle that identifies the element is the _____.
A.
neutron
B.
electron
C.
proton
D.
quark
5.
The ion 92 U contains _____.
A.
92 protons, 235 neutrons, 4 electrons
B.
92 protons, 143 neutrons, 88 electrons
C.
92 protons, 143 neutrons, 96 electrons
D.
143 protons, 92 electrons, 88 electrons
6.
The ion 93 Np contains _____.
A.
5 electrons
B.
88 electrons
C.
93 electrons
D.
244 electrons
235
244
4+
5+
THE ATOM, PERIODIC TABLE AND BONDING
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CHEMISTRY 11
7.
The symbol for an ion that has 47 protons, 46 electrons, and 61 neutrons is _____.
A.
B.
C.
D.
8.
B.
C.
D.
115
4+
46 Pd
96
4+
69 Tm
119
4+
50 Sn
119
4+
69 Tm
How many electrons does the following ion
A.
B.
C.
D.
10.
61
+
47 Ag
108
47 Ag
107
+
46 Pd
108
+
47 Ag
The symbol for an ion that has 50 protons, 46 electrons, and 69 neutrons is _____.
A.
9.
UNIT VIII TEST
7+
18 4
W possess?
74
67
81
177
191
The formula of an ion that contains 51 protons, 71 neutrons, and 46 electrons is _____.
A.
5+
71
Sb
51
B.
5+
12 2
Lu
71
C.
5+
12 2
Sb
51
D.
5+
97
Sb
51
11.
How many electrons are there in Al3+?
A.
27
B.
24
C.
13
D.
10
12.
What is the charge on the nucleus of S2-?
A.
16
B.
32
C.
18
D.
14
THE ATOM, PERIODIC TABLE AND BONDING
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CHEMISTRY 11
13.
UNIT VIII TEST
How many neutrons are contained in the ion
A.
B.
C.
D.
3+
17 5
Lu ?
71
68
71
104
175
14.
When an electron in a higher energy level drops down to a lower level a/n _____ is
released.
A.
quantum of energy
B.
alpha particle
C.
beta particle
D.
gamma particle
15.
Isotopes are atoms of the same element with different numbers of _____.
A.
protons
B.
neutrons
C.
electrons
D.
quantums
16.
The actual region of space occupied by an electron in a particular energy level is called
a/n _____.
A.
quantum
B.
orbital
C.
shell
D.
subshell
17.
A d-type subshell can contain a maximum of _____ electrons.
A.
two
B.
six
C.
ten
D.
fourteen
18.
An s-type subshell can contain a maximum of _____ electrons..
A.
two
B.
six
C.
ten
D.
fourteen
19.
Which of the following atoms does NOT have an electron configuration in its lowest
energy state?
A.
1s22s22p63s1
B.
1s22s22p53s2
C.
1s22s22p63s2
D.
1s22s22p63s23p1
THE ATOM, PERIODIC TABLE AND BONDING
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CHEMISTRY 11
UNIT VIII TEST
20.
What is the electron configuration for Sn2+?
A.
[Kr]5s24d105p2
B.
[Kr]5s24d10
C.
[Kr]4d105p2
D.
[Kr]5s24d85p2
21.
What is the electron configuration of Cu?
A.
[Ar]4s23d9
B.
[Ar]4s13d10
C.
[Ar]4s24d9
D.
[Ar]4s14d10
22.
What is the electron configuration of Pb?
A.
[Xe]6s25d106p2
B.
[Xe]6s26d106p2
C.
[Xe]6s26f146d106p2
D.
[Xe]6s24f145d106p2
23.
What is the electron configuration of Sb5+?
A.
[Kr]5s24d105p3
B.
[Kr]5s24d8
C.
[Kr]5s24d35p3
D.
[Kr]4d10
24.
What is the electron configuration for P3-?
A.
[Ne]3s2
B.
[Ne]3s23p3
C.
[P]3p3
D.
[Ne]3s23p6
25.
The ion P is isoelectronic with _____.
A.
He
B.
Ne
C.
Ar
D.
Kr
26.
The ion Co is isoelectronic with _____.
A.
Mn
B.
Zn2+
C.
Ca2+
D.
Ni3+
3-
2+
THE ATOM, PERIODIC TABLE AND BONDING
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CHEMISTRY 11
UNIT VIII TEST
3+
27.
The ion Fe is isoelectronic with _____.
A.
Ti2+
B.
Mn2+
C.
Br–
D.
Cr3+
28.
An atom with the electron configuration 1s 2s 2p 3s 3p 4s 3d 4p should show chemical
behaviour similar to that of an atom with the electron configuration _____.
2
2
5
A.
1s 2s 2p
2
2
6
2
6
2
10
6
B.
1s 2s 2p 3s 3p 4s 3d 4p
2
2
6
2
6
2
9
4
C.
1s 2s 2p 3s 3p 4s 3d 4p
2
2
6
2
6
2
10
6
2
D.
1s 2s 2p 3s 3p 4s 3d 4p 5s
29.
Which of the following electron configurations is not a noble gas?
2
2
6
2
6
A.
1s 2s 2p 3s 3p
2
2
6
2
6
2
10
B.
1s 2s 2p 3s 3p 4s 3d
2
2
6
2
6
2
10
6
C.
1s 2s 2p 3s 3p 4s 3d 4p
2
D.
1s
30.
How many valence electrons does As3- have?
A.
0
B.
2
C.
5
D.
8
31.
How many valence electrons does Ga have?
A.
1
B.
2
C.
3
D.
13
32.
How many valence electrons does Sn4+ have?
A.
0
B.
4
C.
10
D.
46
33.
How many valence electrons does Cr3+ have?
A.
0
B.
1
C.
2
D.
3
34.
The organization of the elements today is based upon the law that the properties of the
elements recur periodically when they are arranged in increasing order by their _____.
2
THE ATOM, PERIODIC TABLE AND BONDING
2
6
2
6
2
10
5
6
CHEMISTRY 11
A.
B.
C.
D.
UNIT VIII TEST
molar masses
reactivity with oxygen
mass numbers
atomic numbers
35.
Which of the following is a nonmetallic group of elements?
A.
Li, Na, K, Rb
B.
H, He, Li, Be
C.
F, Cl, Br, I
D.
B, Al, Sc, Y
36.
A period of the periodic table is the same as a _____.
A.
row
B.
column
C.
group
D.
family
37.
The elements in group 1 are called _____.
A.
noble gases
B.
halogens
C.
transition metals
D.
alkali metals
38.
The element _____ is a member of the noble gases.
A.
Bromine
B.
Sodium
C.
Oxygen
D.
Krypton
39.
The element _____ is a member of the halogens.
A.
Xenon
B.
Boron
C.
Astatine
D.
Nitrogen
40.
The elements gold, silver, and platinum are members of the _____.
A.
Lanthanides
B.
Actinides
C.
Transition metals
D.
Precious metals
41.
Which of the following is NOT a property of nonmetals?
A.
ductile
B.
brittle
C.
nonconductor
D.
dull
42.
Which of the following is NOT a property of metals?
THE ATOM, PERIODIC TABLE AND BONDING
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CHEMISTRY 11
A.
B.
C.
D.
UNIT VIII TEST
malleable
good conductors
shiny
translucent
The following information will be used to answer questions 43 to 47
(i)
brittle; steel-grey; partially reflective; fair
conductor
(ii)
soft; silvery-white; reflective; good conductor
(iii)
waxy yellow solid; translucent; poor conductor
(iv)
brittle; bluish-white; reflective; fair conductor
(v)
colourless gas; extremely poor conductor
43.
From the descriptions above, item (i) describes the element _____.
A.
P
B.
Ba
C.
Sb
D.
Ar
E.
As
44.
From the descriptions above, item (ii) describes the element _____.
A.
P
B.
Ba
C.
Sb
D.
Ar
E.
As
45.
From the descriptions above, item (iii) describes the element _____.
A.
P
B.
Ba
C.
Sb
D.
Ar
E.
As
46.
From the descriptions above, item (iv) describes the element _____.
A.
P
B.
Ba
C.
Sb
D.
Ar
E.
As
47.
From the descriptions above, item (v) describes the element _____.
A.
P
THE ATOM, PERIODIC TABLE AND BONDING
8
CHEMISTRY 11
B.
C.
D.
E.
UNIT VIII TEST
Ba
Sb
Ar
As
48.
Elements in the same chemical family tend to have similar _____.
A.
atomic numbers
B.
atomic masses
C.
number of electrons
D.
electron configurations
49.
Which of the following statements is true?
A.
Ionization energy increases from right to left along period in the periodic table.
B.
Ionization energy increases from top to bottom within a group in the periodic
table.
C.
Atomic radius increases from left to right along a period in the periodic table.
D.
Atomic radius increases from top to bottom within a group in the periodic table.
50.
An unlikely chemical combination is _____.
A.
NaH
B.
NeF
C.
MgH2
D.
ScF3
51.
Which of the following atoms has the largest atomic radius?
A.
Zn
B.
V
C.
Fe
D.
Cu
52.
Which of the following elements is the least metallic?
A.
Francium
B.
Potassium
C.
Cesium
D.
Rubiudium
53.
Which of the following elements has the highest ionization energy?
A.
Lead
B.
Osmium
C.
Tungsten
D.
Cesium
54.
Which of the following has a closed shell.
A.
Ne
B.
Ba
C.
Sb
D.
Cl
THE ATOM, PERIODIC TABLE AND BONDING
9
CHEMISTRY 11
UNIT VIII TEST
55.
Which of the following has a closed shell.
A.
O–
B.
Al+
C.
Fe3+
D.
N3-
56.
The valence of an atom of Se is _____.
A.
2
B.
4
C.
6
D.
16
57.
Between atoms in a covalent bond, _____.
A.
the attractions are weaker than the repulsions
B.
electrons are shared
C.
no electrons are located
D.
the electronegativity difference is 1.7 or greater
58.
Which ion pair has the greatest electrostatic attraction between ions?
A.
Li+ and FB.
Na+ and ClC.
Li+ and ClD.
Na+ and F-
59.
Which of the following pairs of atoms would you expect to form covalent bonds when
they join?
A.
H and C
B.
Na and Cl
C.
Zn and S
D.
Fe and O
60.
Which of the following compounds would you expect to have the highest melting point?
A.
CaO
B.
RbI
C.
KBr
D.
SrS
61.
Which of the following is best described as a “formula unit”?
A.
CaO
B.
H2O
C.
CH4
D.
NH3
THE ATOM, PERIODIC TABLE AND BONDING
10
CHEMISTRY 11
62.
In ionic bonding, _____.
A.
the electronegativity difference between atoms is 1.7 or greater
B.
electrons are shared equally
C.
protons are transferred
D.
there are no more than two atoms
63.
Which of the following molecules would NOT be polar?
A.
HCl
B.
H2O
C.
BeH2
D.
NH3
64.
The CCl4 molecule does not behave as a polar molecule because _____.
A.
the C-Cl bonds are nonpolar
B.
the C-Cl bonds are ionic
C.
the bond dipoles cancel
D.
the shape of the molecule is linear
65.
Van der Waals forces do NOT include _____.
A.
dipole-dipole forces
B.
London forces
C.
Hydrogen bonds
D.
polar covalent bonds
66.
In which of the following are van der Waals forces most important?
A.
NH3
B.
Ne
C.
H2O
D.
HCl
67.
What is the shape of the molecule BF3?
A.
trigonal pyramidal
B.
t-shaped
C.
trigonal planar
D.
tetrahedral
68.
What is the shape of the molecule SF6?
A.
trigonal bipyramidal
B.
octahedral
C.
trigonal planar
D.
tetrahedral
69.
What is the shape of the ion NH4+?
A.
trigonal planar
B.
tetrahedral
C.
trigonal pyramidal
D.
trigonal bipyramidal
THE ATOM, PERIODIC TABLE AND BONDING
UNIT VIII TEST
11
CHEMISTRY 11
UNIT VIII TEST
70.
What is the shape of the molecule BeH2?
A.
linear
B.
angular
C.
trigonal planar
D.
tetrahedral
71.
Which of the following molecules is non-polar?
A.
PCl3
B.
BF3
C.
NH3
D.
SbI3
72.
Which of the following molecules is polar?
A.
SF6
B.
PCl5
C.
BrF5
D.
XeF4
Use this table to answer the following questions 73 to 75.
ELECTRONEGATIVITIES OF THE ELEMENTS
2.1
H
1.0
Li
1.5
Be
2.0
B
2.5
C
3.0
N
3.5
O
4.0
F
0.9
Na
1.2
Mg
1.5
Al
1.8
Si
2.1
P
2.5
S
3.0
Cl
0.8
K
1.0
Ca
1.3
Sc
1.5
Ti
1.6
V
1.6
Cr
1.5
Mn
1.8
Fe
1.8
Co
1.8
Ni
1.9
Cu
1.6
Zn
1.6
Ga
1.8
Ge
2.0
As
2.4
Se
2.8
Br
0.8
Rb
1.0
Sr
1.2
Y
1.4
Zr
1.6
Nb
1.8
Mo
1.9
Tc
2.2
Ru
2.2
Rh
2.2
Pd
1.9
Ag
1.7
Cd
1.7
In
1.8
Sn
1.9
Sb
2.1
Te
2.5
I
0.7
Cs
0.9
Ba
1.1
La
1.3
Hf
1.5
Ta
1.7
W
1.9
Re
2.2
Os
2.2
Ir
2.2
Pt
2.4
Au
1.9
Hg
1.8
Tl
1.8
Pb
1.9
Bi
2.0
Po
2.2
At
0.7
Fr
0.9
Ra
1.1
Ac
73.
The bond in a molecule of Br2 is best described as a _____ bond.
A.
covalent
B.
polar covalent
C.
ionic
D.
hydrogen
74.
The bond in a molecule of HBr is best described as a _____ bond.
A.
covalent
THE ATOM, PERIODIC TABLE AND BONDING
12
CHEMISTRY 11
B.
C.
D.
75.
UNIT VIII TEST
polar covalent
ionic
hydrogen
The bond in a molecule of B2H6 is best described as a _____ bond.
A.
covalent
B.
polar covalent
C.
ionic
D.
hydrogen
THE ATOM, PERIODIC TABLE AND BONDING
13
CHEMISTRY 11
UNIT VIII TEST
Part C: Written-Response Questions
Answer each of the following question on the answer sheet provided.
1.
Fill in the following table. Show both the atomic number and mass number of the
“particle”. Where applicable indicate the charge of the “particle”.
Symbol for Particle
Atomic
Mass
# Protons
84
36
35
127
2.
? 3+
X
?
=
36
54
32
24
112
38
=
45
36
66
Zn
30
? 2X
?
# Electrons
36
53
27
11 2
Cd2+
48
# Neutrons
50
36
75
54
103
42
Calculate the expected molar mass of a sample of each mixture.
A.
69
Ga = 60.0%, 71Ga = 40.0%
B.
70
Ge = 20.5%, 72Ge = 27.4%, 73Ge = 7.8%, 74Ge = 36.5%, 76Ge = 7.8%
THE ATOM, PERIODIC TABLE AND BONDING
14
CHEMISTRY 11
UNIT VIII TEST
3.
Using core notation, write the electron configurations for the following.
A.
Fe
B.
Bi
C.
Np
4.
Using core notation, write the electron configurations for the following.
A.
Ti2+
B.
Ge4+
C.
Sb3+
5.
How many valence electrons do each of the following contain?
A.
Tc4+
B.
O–
C.
I5+
6.
What happens to atomic radius as you:
A.
go from left to right across a period. (1 mark)
Explain ______________________________________________________________
B.
go top to bottom down a group. (1 mark)
Explain: ______________________________________________________________
7.
8.
A.
Consider the compounds NaCl and KBr. Which compound will have a higher
melting point? Explain. (2 marks)
B.
Consider the compounds MgO and NaF. Which compound will have a higher
melting point? Explain. (2 marks)
Draw the Lewis structure for each of the following ionic compounds. (3 marks)
A.
9.
MgO
B.
CaCl2
C.
K3P
Draw the Lewis structures to the following molecules. (6 marks)
A.
F2
D.
CN–
B.
H2O
E.
SCl6
C.
NH3
F.
BrF3
THE ATOM, PERIODIC TABLE AND BONDING
15
NAME _____________________________________
DATE _________________________ BLOCK _____
The Structure of the Atom
Part A: Matching Questions
From the list of terms on the right, choose the one that BEST fits the description on the left.
1.
____
8.
____
15.
____
22.
____
2.
____
9.
____
16.
____
23.
____
3.
____
10.
____
17.
____
24.
____
4.
____
11.
____
18.
____
25.
____
5.
____
12.
____
19.
____
26.
____
6.
____
13.
____
20.
____
7.
____
14.
____
21.
____
Part C: Written-Response Questions
Answer each of the following question on the answer sheet provided.
1.
Fill in the following table. Show both the atomic number and mass number of the
“particle”. Where applicable indicate the charge of the “particle”. (11 marks)
Symbol for Particle
Atomic Mass
# Protons
84
36
35
127
? 3+
?X
=
VERSION: May 22, 2003
36
54
32
24
112
38
=
45
36
66
Zn
30
? 2X
?
# Electrons
36
53
27
11 2
2+
48 Cd
# Neutrons
103
50
36
75
54
42
1
CHEMISTRY 11
2.
UNIT VIII TEST
Calculate the expected molar mass of a sample of each mixture. (2 marks)
A.
69
Ga = 60.0%, 71Ga = 40.0%
__________________________________________________________________
B.
70
Ge = 20.5%, 72Ge = 27.4%, 73Ge = 7.8%, 74Ge = 36.5%, 76Ge = 7.8%
__________________________________________________________________
3.
4.
5.
6.
Using core notation, write the electron configurations for the following. (3 marks)
A.
Fe
__________________________________________
B.
Bi
__________________________________________
C.
Np
__________________________________________
Using core notation, write the electron configurations for the following. (3 marks)
A.
Ti2+
__________________________________________
B.
Ge4+
__________________________________________
C.
Sb3+
__________________________________________
How many valence electrons do each of the following contain? (3 marks)
A.
Tc4+
__________________________________________
B.
O–
__________________________________________
C.
I5+
__________________________________________
What happens to atomic radius as you:
A.
go from left to right across a period. (1.5 mark)
Explain ______________________________________________________________
_____________________________________________________________________
B.
go top to bottom down a group. (1.5 mark)
Explain: ______________________________________________________________
_____________________________________________________________________
7.
A.
Consider the compounds NaCl and KBr. Which compound will have a higher
melting point? Explain. (1.5 marks)
THE ATOM, PERIODIC TABLE AND BONDING
2
CHEMISTRY 11
UNIT VIII TEST
_____________________________________________________________________
_____________________________________________________________________
B.
Consider the compounds MgO and NaF. Which compound will have a higher
melting point? Explain. (1.5 marks)
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8.
Draw the Lewis structure for each of the following ionic compounds. (3 marks)
A.
9.
MgO
B.
CaCl2
C.
K3P
Draw the Lewis structures to the following molecules. (6 marks)
A.
F2
D.
CN–
B.
H2O
E.
SCl6
C.
NH3
F.
BrF3
THE ATOM, PERIODIC TABLE AND BONDING
3